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What is the significance of a big jump between the 2nd and 3rd ionisation energies?

A big jump indicates that the element is in group 2 of the periodic table, as the 3rd electron is removed from an electron shell closer to the nucleus.

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"What is the significance of a big jump between the 2nd and 3rd ionisation energies?"	"A big jump indicates that the element is in group 2 of the periodic table, as the 3rd electron is removed from an electron shell closer to the nucleus."
"What do the arrows in a spin diagram represent?"	"The arrows in a spin diagram represent the different spins of the electrons in an orbital."
"How do you fill up sub levels with several orbitals in the model of atomic structure?"	"When filling up sub levels with several orbitals, each orbital is filled singly before starting to pair up the electrons."
"Describe the structure of the periodic table."	"The periodic table is split into blocks based on the type of subshell that the outer electron of an element is filling."
"What is an S block element?"	"An S block element is one whose outer electron is filling an s-subshell."
"Define a p block element."	"A p block element is one whose outer electron is filling a p-subshell."
"How is a d block element defined?"	"A d block element is one whose outer electron is filling a d-subshell."
"Describe the electronic structure of O2-."	"Oxygen (O) with the electronic structure 1s2 2s2 2p4 becomes O2- with the electronic structure 1s2 2s2 2p6."
"What is the electronic structure of Cu2+?"	"Copper (Cu) with the electronic structure 1s2 2s2 2p6 3s2 3p6 4s1 3d10 becomes Cu2+ with the electronic structure [Ar] 3d9."
"Do d-block elements lose their 4s electrons first when forming ions?"	"Yes, d-block elements lose their 4s electrons first when forming ions."
"Describe the electronic structure of Zn2+."	"Zinc (Zn) with the electronic structure 1s2 2s2 2p6 3s2 3p6 4s2 3d10 becomes Zn2+ with the electronic structure [Ar] 3d10."
"Describe the first ionisation energy."	"The enthalpy change when one mole of gaseous atoms forms one mole of gaseous ions with a single positive charge."
"Define the second ionisation energy."	"The enthalpy change when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a double positive charge."
"What are the three main factors that affect ionisation energy?"	"1. The attraction of the nucleus 2. The distance of the electrons from the nucleus 3. Shielding of the attraction of the nucleus"
"Why are successive ionisation energies always larger?"	"The first electron removal forms a positive ion, increasing the attraction on the remaining electrons, requiring more energy to remove the next electron."
"How are ionisation energies linked to electronic structure?"	"Ionisation energies provide information about the electronic structure of an element. The closer an electron is to the nucleus and the less shielding it has, the higher the ionisation energy."
"Write the electronic structure of oxygen using letters and numbers."	"The electronic structure of oxygen is 1s2 2s2 2p4."
"What is the equation for the first ionisation energy?"	"H(g) -> H+(g) + e-"
"What is the equation for the second ionisation energy?"	"Ti+(g) -> Ti2+(g) + e-"
"Describe the shape of the graph for periods two and three in the first ionisation energy of the elements."	"The shape of the graph for periods two and three in the first ionisation energy of the elements is similar."
"Define periodicity."	"Periodicity refers to a repeating pattern across a period."
"How does the first ionisation energy of helium compare to hydrogen?"	"Helium has a larger first ionisation energy than hydrogen because its first electron is in the first shell closest to the nucleus and has no shielding effects from inner shells. Additionally, helium has one more proton."
"Why do first ionisation energies decrease down a group?"	"First ionisation energies decrease down a group because the outer electrons are found in shells further from the nucleus and are more shielded, resulting in a smaller attraction of the nucleus."
"Why is there a general increase in first ionisation energy across a period?"	"There is a general increase in first ionisation energy across a period because the electrons are being added to the same shell, which has the same distance from the nucleus and same shielding effect. However, the number of protons increases, making the effective attraction of the nucleus greater."
"Why does sodium have a much lower first ionisation energy than neon?"	"Sodium has a much lower first ionisation energy than neon because its outer electron is in a 3s shell further from the nucleus and is more shielded."
"Why is there a small drop in first ionisation energy from magnesium to aluminum?"	"There is a small drop in first ionisation energy from magnesium to aluminum because aluminum is starting to fill a 3p subshell, whereas magnesium has its outer electrons in the 3s subshell. The electrons in the 3p subshell are slightly easier to remove due to their higher energy and slight shielding by the 3s electrons."
"Why is there a small drop in first ionisation energy from phosphorus to sulfur?"	"There is a small drop in first ionisation energy from phosphorus to sulfur because with sulfur, there are 4 electrons in the 3p subshell and the 4th electron is starting to doubly fill the first 3p orbital. When the second electron is added to a 3p orbital, there is a slight repulsion between the two negatively charged electrons, making the second electron easier to remove."
"Define second ionisation energy."	"Second ionisation energy refers to the energy required to remove the second electron from an atom or ion."
"How does the second ionisation energy of lithium compare to helium?"	"The second ionisation energy of lithium is higher than that of helium because lithium has more protons and its second electron is removed from the 1s shell closest to the nucleus, experiencing less shielding from inner shells."
"Define isotopes."	"Isotopes are atoms of the same element that have different numbers of neutrons and therefore different mass numbers."
"Define atomic number and mass number."	"Atomic number (Z) is the number of protons in the nucleus, while mass number (A) is the total number of protons and neutrons in the atom."
"How can a mass spectrometer be used to identify elements and isotopes?"	"A mass spectrometer can determine the isotopes present in a sample of an element and identify elements by analyzing the mass-to-charge ratio of ions."
"Describe the process of electron impact ionization in a mass spectrometer."	"Electron impact ionization involves firing high-energy electrons at a vaporized sample, causing outer electrons to be knocked out and forming positive ions with different charges."
"Explain the process of electrospray ionization in a mass spectrometer."	"Electrospray ionization involves dissolving the sample in a volatile, polar solvent and injecting it through a fine needle. The sample gains a proton from the solvent, forming MH+ ions, which are then analyzed in the mass spectrometer."
"What is the purpose of maintaining a vacuum in a mass spectrometer?"	"A vacuum is necessary in a mass spectrometer to prevent air particles from ionizing and registering on the detector."
"List the essential steps in a mass spectrometer."	"The essential steps in a mass spectrometer are ionization, acceleration, detection, and time measurement."
"Describe acceleration in a mass spectrometer."	"Acceleration in a mass spectrometer refers to the process of increasing the velocity of positive ions using an electric field, while keeping their kinetic energy constant."
"What is the relationship between the velocity and mass of particles in a mass spectrometer?"	"In a mass spectrometer, lighter particles have a faster velocity, while heavier particles have a slower velocity."
"Define kinetic energy in the context of a mass spectrometer."	"Kinetic energy in a mass spectrometer is the energy possessed by a particle due to its motion. It is calculated using the equation KE = 1/2 mv^2, where KE is the kinetic energy, m is the mass of the particle, and v is its velocity."
"How are positive ions distinguished in a mass spectrometer?"	"Positive ions in a mass spectrometer are distinguished by their flight times. The ions with smaller m/z values have the same kinetic energy as those with larger m/z values, but they move faster."
"Describe the detection process in a mass spectrometer."	"In a mass spectrometer, the ions reach the detector and generate a small current. This current is produced by electrons transferring from the detector to the positive ions. The size of the current is proportional to the abundance of the species being analyzed."
"Describe the concept of relative atomic mass."	"The relative atomic mass is a weighted average of all the isotopes of an element, as quoted on the periodic table."
"What is the formula to calculate the relative atomic mass (R.A.M) of an element?"	"R.A.M = (isotopic mass X % abundance) / 100"
"How can you calculate the relative atomic mass using relative abundance data?"	"R.A.M = [(mass1 x abundance1) + (mass2 x abundance2) + ...]"
"Describe the three sub-atomic particles and their positions in an atom."	"Protons are located in the nucleus, neutrons are also located in the nucleus, and electrons are found in orbitals surrounding the nucleus."
"Describe how to calculate the percentage abundances of isotopes."	"Percentage abundance can be calculated using the equation: R.A.M = (y x mass1) + [(1-y) x mass2], where y represents the percentage abundance of the first isotope and (1-y) represents the percentage abundance of the second isotope."
"Describe the composition of the mass spectra for Cl2 and Br2."	"The mass spectra for Cl2 and Br2 show the relative abundance of different isotopes of chlorine and bromine in the diatomic molecules."
"How can mass spectrometers be used in planetary space probes?"	"Mass spectrometers in planetary space probes can identify elements on other planets by analyzing the composition of isotopes."
"Describe the process of measuring the molecular mass (M) of a molecule using a mass spectrometer."	"When a molecule is put through a mass spectrometer with electron impact ionization, it often breaks up into fragments. The peak with the largest m/z corresponds to the complete molecule and is equal to the relative molecular mass (M) of the molecule."
"What is the relative abundance of the isotopes Cl³5 and Cl³7 in chlorine?"	"The relative abundance of Cl³5 is 75%, while the relative abundance of Cl³7 is 25% in chlorine."
"Describe the Bohr model of the atom."	"The Bohr model of the atom proposed that electrons orbit the nucleus in spherical orbits, with 2 electrons in the first shell, 8 in the second, and so on."
"What are the sub energy levels in the model of atomic structure?"	"The sub energy levels in the model are labeled S, p, d, and f."
"Define orbitals in the model of atomic structure."	"Orbitals are regions around the nucleus that hold up to a specific number of electrons. They are split into sub-levels, such as S, p, d, and f."
"Describe the shapes of orbitals in the model of atomic structure."	"Orbitals represent the mathematical probabilities of finding an electron at any point within certain spatial distributions around the nucleus. Each orbital has its own approximate three-dimensional shape."
"How does an atom fill up sub shells in the model of atomic structure?"	"An atom fills up the sub shells in order of increasing energy. For example, the 3d sub shell is higher in energy than the 4s sub shell, so it gets filled after the 4s."

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What is the significance of a big jump between the 2nd and 3rd ionisation energies?

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A big jump indicates that the element is in group 2 of the periodic table, as the 3rd electron is removed from an electron shell closer to the nucleus.

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This jump in ionization energy indicates a change in the electron configuration and can provide information about the element's position in the periodic table.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974191,"front":"What do the arrows in a spin diagram represent?","back":"The arrows in a spin diagram represent the different spins of the electrons in an orbital.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":1,"explanation":"The arrows in a spin diagram represent the orientation of the electron spins in an orbital. Electrons have a property called spin, which can be either \"up\" or \"down\". The arrows indicate the direction of the spin, with one arrow pointing up and the other pointing down. This representation helps to visualize the arrangement of electrons in an orbital and understand their behavior in relation to each other.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974193,"front":"How do you fill up sub levels with several orbitals in the model of atomic structure?","back":"When filling up sub levels with several orbitals, each orbital is filled singly before starting to pair up the electrons.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":2,"explanation":"In the model of atomic structure, sub levels are filled with several orbitals by first filling each orbital singly before pairing up the electrons. This is based on the principle known as Hund's rule, which states that electrons will occupy separate orbitals within a sub level before they start to pair up. This arrangement ensures that the electrons are distributed as evenly as possible, maximizing the stability of the atom.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974195,"front":"Describe the structure of the periodic table.","back":"The periodic table is split into blocks based on the type of subshell that the outer electron of an element is filling.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":3,"explanation":"The periodic table is organized into blocks that represent the different types of subshells being filled by the outer electrons of elements. These blocks include s, p, d, and f. The arrangement of elements in the periodic table is based on their atomic number, which increases from left to right and top to bottom. This arrangement allows for the grouping of elements with similar properties in the same columns, known as groups or families. The periodic table provides a systematic way to understand the relationships between elements and predict their chemical behavior.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974197,"front":"What is an S block element?","back":"An S block element is one whose outer electron is filling an s-subshell.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":4,"explanation":"An S block element refers to an element in the periodic table whose outermost electron is filling an s-subshell. The s-subshell can hold a maximum of 2 electrons. These elements are typically found in the leftmost two columns of the periodic table, including hydrogen and helium in the first column. The filling of the s-subshell determines the chemical properties and reactivity of these elements.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974199,"front":"Define a p block element.","back":"A p block element is one whose outer electron is filling a p-subshell.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":5,"explanation":"A p block element refers to an element in the periodic table whose outermost electrons are filling the p-subshell. The p-subshell can hold a maximum of 6 electrons. These elements exhibit a wide range of properties due to the varying number of valence electrons. They can form covalent bonds and display diverse chemical reactivity. The p block elements are found in groups 13 to 18 on the periodic table.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974200,"front":"How is a d block element defined?","back":"A d block element is one whose outer electron is filling a d-subshell.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":6,"explanation":"A d block element is defined by the filling of its outer electron in a d-subshell. The d-subshell is part of the second innermost electron shell, known as the d-block. These elements exhibit a wide range of properties due to the presence of partially filled d orbitals, which can participate in bonding and form complex compounds. The d-block elements are transition metals and have characteristic metallic properties such as high melting and boiling points, conductivity, and variable oxidation states.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974202,"front":"Describe the electronic structure of O2-.","back":"Oxygen (O) with the electronic structure 1s2 2s2 2p4 becomes O2- with the electronic structure 1s2 2s2 2p6.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":7,"explanation":"The electronic structure of an atom describes the arrangement of its electrons in different energy levels or orbitals. Oxygen (O) has 8 electrons, with 2 in the 1s orbital, 2 in the 2s orbital, and 4 in the 2p orbital. When oxygen gains two electrons to become O2-, it achieves a stable octet configuration by filling up the 2p orbital with 6 electrons. This results in the electronic structure of O2- as 1s2 2s2 2p6.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974203,"front":"What is the electronic structure of Cu2+?","back":"Copper (Cu) with the electronic structure 1s2 2s2 2p6 3s2 3p6 4s1 3d10 becomes Cu2+ with the electronic structure [Ar] 3d9.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":8,"explanation":"The electronic structure of an atom is determined by the arrangement of its electrons in different energy levels or orbitals. Copper (Cu) has 29 electrons, and its electronic structure is 1s2 2s2 2p6 3s2 3p6 4s1 3d10. When copper loses two electrons to form Cu2+, it becomes a cation with a positive charge. The loss of two electrons occurs from the 4s orbital, leaving behind the electronic structure [Ar] 3d9. This configuration reflects the arrangement of the remaining 29-2=27 electrons in the atom.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974204,"front":"Do d-block elements lose their 4s electrons first when forming ions?","back":"Yes, d-block elements lose their 4s electrons first when forming ions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":9,"explanation":"Yes, d-block elements lose their 4s electrons first when forming ions. This is because the 4s orbital has a lower energy level than the 3d orbital. When forming ions, electrons are removed from the outermost energy level first, which in this case is the 4s orbital. This allows the d-block elements to achieve a more stable electron configuration.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974205,"front":"Describe the electronic structure of Zn2+.","back":"Zinc (Zn) with the electronic structure 1s2 2s2 2p6 3s2 3p6 4s2 3d10 becomes Zn2+ with the electronic structure [Ar] 3d10.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":10,"explanation":"Zinc (Zn) has an atomic number of 30, meaning it has 30 electrons. In its neutral state, Zn has the electronic configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10. When Zn loses two electrons to form Zn2+, it becomes a cation with a positive charge. The loss of two electrons leaves behind the electronic configuration [Ar] 3d10, where [Ar] represents the electron configuration of the noble gas argon.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974206,"front":"Describe the first ionisation energy.","back":"The enthalpy change when one mole of gaseous atoms forms one mole of gaseous ions with a single positive charge.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":11,"explanation":"The first ionization energy is a measure of the energy required to remove one electron from a gaseous atom to form a gaseous ion with a single positive charge. It represents the strength of the attraction between the nucleus and the outermost electron. Higher ionization energies indicate stronger attractions and more difficulty in removing an electron.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974207,"front":"Define the second ionisation energy.","back":"The enthalpy change when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a double positive charge.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":12,"explanation":"The second ionization energy is a measure of the energy required to remove a second electron from a gaseous ion. It specifically refers to the enthalpy change when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a double positive charge. This energy is influenced by factors such as the nuclear charge and electron-electron repulsion, which affect the attraction and stability of the electrons in the ion.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974208,"front":"What are the three main factors that affect ionisation energy?","back":"1. The attraction of the nucleus\n2. The distance of the electrons from the nucleus\n3. Shielding of the attraction of the nucleus","front_language":"English","back_language":"English","front_image":"","back_image":"","order":13,"explanation":"The three main factors that affect ionization energy are the attraction of the nucleus, the distance of the electrons from the nucleus, and the shielding of the attraction of the nucleus. These factors determine the amount of energy required to remove an electron from an atom. The stronger the attraction of the nucleus, the higher the ionization energy. The closer the electrons are to the nucleus, the higher the ionization energy. The more shielding there is from other electrons, the lower the ionization energy.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974209,"front":"Why are successive ionisation energies always larger?","back":"The first electron removal forms a positive ion, increasing the attraction on the remaining electrons, requiring more energy to remove the next electron.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":14,"explanation":"Successive ionization energies are always larger because removing the first electron creates a positive ion, which increases the attraction between the remaining electrons and the nucleus. This stronger attraction requires more energy to remove the next electron, making the successive ionization energies larger.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974210,"front":"How are ionisation energies linked to electronic structure?","back":"Ionisation energies provide information about the electronic structure of an element. The closer an electron is to the nucleus and the less shielding it has, the higher the ionisation energy.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":15,"explanation":"Ionisation energies are linked to electronic structure because they measure the energy required to remove an electron from an atom. The higher the ionisation energy, the more tightly the electron is held by the nucleus. This is influenced by factors such as the distance between the electron and nucleus, as well as the shielding effect of other electrons. Therefore, ionisation energies can provide insights into the arrangement and distribution of electrons in an atom's electronic structure.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974190,"front":"Write the electronic structure of oxygen using letters and numbers.","back":"The electronic structure of oxygen is 1s2 2s2 2p4.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":16,"explanation":"The electronic structure of an atom describes the arrangement of its electrons in different energy levels or orbitals. Oxygen has 8 electrons, and its electronic structure is represented by a series of numbers and letters. The numbers indicate the energy levels (1s, 2s, 2p), and the superscript numbers represent the number of electrons in each orbital (2 in 1s, 2 in 2s, and 4 in 2p). This notation helps us understand the distribution of electrons in an atom.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974212,"front":"What is the equation for the first ionisation energy?","back":"H(g) -> H+(g) + e-","front_language":"English","back_language":"English","front_image":"","back_image":"","order":17,"explanation":"The equation provided represents the first ionization energy, which is the energy required to remove one electron from a gaseous atom or ion. In this specific case, it shows the ionization of a hydrogen atom, where a hydrogen atom loses an electron to form a hydrogen ion (H+) and a free electron (e-). This equation is a simplified representation of the ionization process and is commonly used to describe the first ionization energy of hydrogen.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974213,"front":"What is the equation for the second ionisation energy?","back":"Ti+(g) -> Ti2+(g) + e-","front_language":"English","back_language":"English","front_image":"","back_image":"","order":18,"explanation":"The equation provided represents the second ionization energy of titanium (Ti). Ionization energy is the energy required to remove an electron from an atom or ion. In this case, the equation shows the removal of an electron from a singly charged titanium ion (Ti+) to form a doubly charged titanium ion (Ti2+). The process involves the loss of one electron (e-) and the resulting ionization energy is the energy required for this electron removal.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974214,"front":"Describe the shape of the graph for periods two and three in the first ionisation energy of the elements.","back":"The shape of the graph for periods two and three in the first ionisation energy of the elements is similar.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":19,"explanation":"The similarity in the shape of the graph for periods two and three in the first ionisation energy of the elements can be attributed to the trend of increasing ionisation energy across a period. This trend is due to the increasing nuclear charge, which attracts the outermost electrons more strongly, making it harder to remove them. As a result, the ionisation energy generally increases from left to right across a period.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974215,"front":"Define periodicity.","back":"Periodicity refers to a repeating pattern across a period.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":20,"explanation":"Periodicity is a concept that describes the occurrence of a repeating pattern over a specific period of time or space. It is commonly observed in various natural phenomena, such as the periodic table of elements, where elements exhibit similar properties in regular intervals. Periodicity is also seen in other fields, such as mathematics and music, where patterns repeat at regular intervals. This concept helps in understanding and predicting the behavior of systems that exhibit periodic patterns.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974217,"front":"How does the first ionisation energy of helium compare to hydrogen?","back":"Helium has a larger first ionisation energy than hydrogen because its first electron is in the first shell closest to the nucleus and has no shielding effects from inner shells. Additionally, helium has one more proton.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":22,"explanation":"The first ionization energy of helium is larger than that of hydrogen due to two main factors. Firstly, helium's first electron is in the first shell, which is closer to the nucleus and experiences stronger attraction, resulting in a higher ionization energy. Secondly, helium has one more proton than hydrogen, which increases the positive charge in the nucleus and further strengthens the attraction for the electron, contributing to a higher ionization energy.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974218,"front":"Why do first ionisation energies decrease down a group?","back":"First ionisation energies decrease down a group because the outer electrons are found in shells further from the nucleus and are more shielded, resulting in a smaller attraction of the nucleus.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":23,"explanation":"First ionization energies decrease down a group due to the increasing atomic size and electron shielding. As you move down a group, the outer electrons are located in higher energy levels, farther from the nucleus, and experience increased electron shielding from inner electron shells. This results in a weaker attraction to the nucleus, leading to a decrease in the energy required to remove the outermost electron.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974219,"front":"Why is there a general increase in first ionisation energy across a period?","back":"There is a general increase in first ionisation energy across a period because the electrons are being added to the same shell, which has the same distance from the nucleus and same shielding effect. However, the number of protons increases, making the effective attraction of the nucleus greater.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":24,"explanation":"The increase in first ionization energy across a period can be attributed to the increasing number of protons in the nucleus. As the number of protons increases, the positive charge in the nucleus becomes stronger, resulting in a greater attraction for the electrons in the outer shell. This increased attraction requires more energy to remove an electron, leading to a higher ionization energy. Additionally, the electrons in the same shell experience similar shielding effects, so the increase in ionization energy is primarily due to the increased nuclear charge.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974220,"front":"Why does sodium have a much lower first ionisation energy than neon?","back":"Sodium has a much lower first ionisation energy than neon because its outer electron is in a 3s shell further from the nucleus and is more shielded.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":25,"explanation":"Sodium has a lower first ionization energy than neon due to the outer electron being in a 3s shell, which is further from the nucleus and more shielded. This makes it easier to remove the outer electron in sodium compared to neon.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974221,"front":"Why is there a small drop in first ionisation energy from magnesium to aluminum?","back":"There is a small drop in first ionisation energy from magnesium to aluminum because aluminum is starting to fill a 3p subshell, whereas magnesium has its outer electrons in the 3s subshell. The electrons in the 3p subshell are slightly easier to remove due to their higher energy and slight shielding by the 3s electrons.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":26,"explanation":"The drop in first ionization energy from magnesium to aluminum occurs because aluminum is starting to fill a 3p subshell, while magnesium has its outer electrons in the 3s subshell. The 3p electrons are slightly easier to remove due to their higher energy and slight shielding by the 3s electrons. This results in a small decrease in ionization energy.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974222,"front":"Why is there a small drop in first ionisation energy from phosphorus to sulfur?","back":"There is a small drop in first ionisation energy from phosphorus to sulfur because with sulfur, there are 4 electrons in the 3p subshell and the 4th electron is starting to doubly fill the first 3p orbital. When the second electron is added to a 3p orbital, there is a slight repulsion between the two negatively charged electrons, making the second electron easier to remove.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":27,"explanation":"The small drop in first ionization energy from phosphorus to sulfur is due to the electron-electron repulsion in the 3p orbital. In sulfur, the 4th electron starts to doubly fill the first 3p orbital, causing repulsion between the two negatively charged electrons. This repulsion makes it easier to remove the second electron, resulting in a lower ionization energy.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974225,"front":"Define second ionisation energy.","back":"Second ionisation energy refers to the energy required to remove the second electron from an atom or ion.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":30,"explanation":"The second ionization energy is a measure of the energy needed to remove the second electron from an atom or ion. It is typically higher than the first ionization energy because removing a second electron requires overcoming stronger electrostatic forces and reducing the stability of the ion. This energy can be used to determine the electron configuration and stability of an atom or ion.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974226,"front":"How does the second ionisation energy of lithium compare to helium?","back":"The second ionisation energy of lithium is higher than that of helium because lithium has more protons and its second electron is removed from the 1s shell closest to the nucleus, experiencing less shielding from inner shells.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":31,"explanation":"The second ionization energy of lithium is higher than that of helium due to lithium's greater nuclear charge and the removal of the second electron from the 1s orbital, which experiences less shielding. This results in a stronger attraction between the nucleus and the electron being removed.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974169,"front":"Define isotopes.","back":"Isotopes are atoms of the same element that have different numbers of neutrons and therefore different mass numbers.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":32,"explanation":"Isotopes are atoms of an element with varying numbers of neutrons, leading to different mass numbers. This results in distinct physical properties while retaining the same chemical behavior. Isotopes play a crucial role in fields like medicine, energy, and environmental science.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974154,"front":"Define atomic number and mass number.","back":"Atomic number (Z) is the number of protons in the nucleus, while mass number (A) is the total number of protons and neutrons in the atom.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":33,"explanation":"The atomic number is crucial in determining an element's identity, as it represents the number of protons in the nucleus. On the other hand, the mass number accounts for both protons and neutrons, providing insight into an atom's mass. Understanding these numbers is fundamental in chemistry and physics.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974156,"front":"How can a mass spectrometer be used to identify elements and isotopes?","back":"A mass spectrometer can determine the isotopes present in a sample of an element and identify elements by analyzing the mass-to-charge ratio of ions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":35,"explanation":"A mass spectrometer is used to identify elements and isotopes by analyzing the mass-to-charge ratio of ions. It does this by ionizing the sample, separating the ions based on their mass-to-charge ratio, and detecting the ions. By comparing the mass-to-charge ratios of the ions to known values, the elements and isotopes present in the sample can be identified. This technique is based on the principle that different elements and isotopes have different masses, allowing for their differentiation and identification.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974157,"front":"Describe the process of electron impact ionization in a mass spectrometer.","back":"Electron impact ionization involves firing high-energy electrons at a vaporized sample, causing outer electrons to be knocked out and forming positive ions with different charges.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":36,"explanation":"Electron impact ionization is a common method used in mass spectrometry to ionize molecules. High-energy electrons are directed towards a vaporized sample, resulting in the ejection of outer electrons from the molecules. This process forms positive ions with varying charges, allowing for their separation and analysis in the mass spectrometer.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974158,"front":"Explain the process of electrospray ionization in a mass spectrometer.","back":"Electrospray ionization involves dissolving the sample in a volatile, polar solvent and injecting it through a fine needle. The sample gains a proton from the solvent, forming MH+ ions, which are then analyzed in the mass spectrometer.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":37,"explanation":"Electrospray ionization is a technique used in mass spectrometry to analyze samples. It involves dissolving the sample in a volatile, polar solvent and injecting it through a fine needle. The solvent helps the sample gain a proton, forming MH+ ions. These ions are then analyzed in the mass spectrometer to determine their mass-to-charge ratio. This technique is particularly useful for analyzing large and complex molecules, such as proteins and peptides.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974159,"front":"What is the purpose of maintaining a vacuum in a mass spectrometer?","back":"A vacuum is necessary in a mass spectrometer to prevent air particles from ionizing and registering on the detector.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":38,"explanation":"Maintaining a vacuum in a mass spectrometer is crucial because the presence of air particles can interfere with the ionization process and lead to inaccurate readings on the detector. A vacuum ensures that only the sample being analyzed is ionized and detected, improving the accuracy and reliability of the results.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974160,"front":"List the essential steps in a mass spectrometer.","back":"The essential steps in a mass spectrometer are ionization, acceleration, detection, and time measurement.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":39,"explanation":"A mass spectrometer is a scientific instrument used to measure the mass-to-charge ratio of ions. It begins with ionization, where a sample is ionized to create charged particles. These ions are then accelerated through an electric field, allowing them to separate based on their mass-to-charge ratio. The separated ions are then detected, usually by measuring their electrical charge or their impact on a detector. Finally, the time it takes for the ions to reach the detector is measured, providing information about their mass-to-charge ratio.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974161,"front":"Describe acceleration in a mass spectrometer.","back":"Acceleration in a mass spectrometer refers to the process of increasing the velocity of positive ions using an electric field, while keeping their kinetic energy constant.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":40,"explanation":"Acceleration in a mass spectrometer involves applying an electric field to increase the velocity of positive ions. This is done to separate ions based on their mass-to-charge ratio. By keeping the kinetic energy constant, the ions can be focused and directed towards the detector, allowing for accurate analysis of their mass and abundance.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974162,"front":"What is the relationship between the velocity and mass of particles in a mass spectrometer?","back":"In a mass spectrometer, lighter particles have a faster velocity, while heavier particles have a slower velocity.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":41,"explanation":"In a mass spectrometer, the relationship between the velocity and mass of particles is inversely proportional. This means that as the mass of the particles increases, their velocity decreases. Conversely, as the mass of the particles decreases, their velocity increases. This relationship is due to the conservation of energy and momentum principles in the mass spectrometer. Lighter particles require less energy to accelerate, resulting in higher velocities, while heavier particles require more energy and therefore have slower velocities.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974163,"front":"Define kinetic energy in the context of a mass spectrometer.","back":"Kinetic energy in a mass spectrometer is the energy possessed by a particle due to its motion. It is calculated using the equation KE = 1/2 mv^2, where KE is the kinetic energy, m is the mass of the particle, and v is its velocity.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":42,"explanation":"In a mass spectrometer, kinetic energy is crucial for separating particles based on their mass-to-charge ratio. The equation KE = 1/2 mv^2 quantifies this energy, with velocity and mass determining the particle's kinetic energy. This energy is then utilized for particle analysis and identification within the mass spectrometer.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974164,"front":"How are positive ions distinguished in a mass spectrometer?","back":"Positive ions in a mass spectrometer are distinguished by their flight times. The ions with smaller m/z values have the same kinetic energy as those with larger m/z values, but they move faster.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":43,"explanation":"Positive ions in a mass spectrometer are distinguished based on their flight times. This is because ions with smaller m/z values have the same kinetic energy as ions with larger m/z values, but they move faster. By measuring the time it takes for ions to reach the detector, the mass spectrometer can differentiate between ions with different m/z values. This allows for the identification and quantification of different ions in a sample.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974165,"front":"Describe the detection process in a mass spectrometer.","back":"In a mass spectrometer, the ions reach the detector and generate a small current. This current is produced by electrons transferring from the detector to the positive ions. The size of the current is proportional to the abundance of the species being analyzed.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":44,"explanation":"The detection process in a mass spectrometer involves ions reaching the detector and causing electrons to transfer, generating a current. This current's magnitude is directly related to the abundance of the species being analyzed, providing valuable quantitative information.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974166,"front":"Describe the concept of relative atomic mass.","back":"The relative atomic mass is a weighted average of all the isotopes of an element, as quoted on the periodic table.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":45,"explanation":"The relative atomic mass considers the abundance of each isotope of an element. It reflects the average mass of all the isotopes relative to the mass of a carbon-12 atom. This value is crucial for understanding chemical reactions and stoichiometry in chemistry.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974167,"front":"What is the formula to calculate the relative atomic mass (R.A.M) of an element?","back":"R.A.M = (isotopic mass X % abundance) / 100","front_language":"English","back_language":"English","front_image":"","back_image":"","order":46,"explanation":"The relative atomic mass (R.A.M) of an element is calculated by multiplying the isotopic mass of each isotope by its percentage abundance and then dividing the sum by 100. This formula takes into account the different isotopes of an element and their relative abundance in nature. By calculating the weighted average of the isotopic masses, the R.A.M provides a measure of the average mass of the atoms in a sample of the element.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974168,"front":"How can you calculate the relative atomic mass using relative abundance data?","back":"R.A.M = [(mass1 x abundance1) + (mass2 x abundance2) + ...]","front_language":"English","back_language":"English","front_image":"","back_image":"","order":47,"explanation":"The relative atomic mass (R.A.M) can be calculated by multiplying the mass of each isotope by its relative abundance and summing these values. This calculation takes into account the different isotopes of an element and their respective abundances, providing a weighted average of the atomic masses. By considering the relative abundance data, the R.A.M calculation reflects the actual distribution of isotopes in a sample.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974153,"front":"Describe the three sub-atomic particles and their positions in an atom.","back":"Protons are located in the nucleus, neutrons are also located in the nucleus, and electrons are found in orbitals surrounding the nucleus.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":48,"explanation":"Protons and neutrons are tightly packed in the nucleus, contributing to the atom's mass, while electrons move rapidly in specific energy levels around the nucleus. This arrangement maintains the overall charge neutrality of the atom.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974170,"front":"Describe how to calculate the percentage abundances of isotopes.","back":"Percentage abundance can be calculated using the equation: R.A.M = (y x mass1) + [(1-y) x mass2], where y represents the percentage abundance of the first isotope and (1-y) represents the percentage abundance of the second isotope.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":49,"explanation":"To calculate the percentage abundances of isotopes, you need to use the equation R.A.M = (y x mass1) + [(1-y) x mass2]. This equation takes into account the mass of each isotope and their respective percentage abundances. By substituting the values for mass1 and mass2, you can solve for y, which represents the percentage abundance of the first isotope. The (1-y) term represents the percentage abundance of the second isotope. This equation allows you to determine the relative amounts of each isotope in a sample.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974171,"front":"Describe the composition of the mass spectra for Cl2 and Br2.","back":"The mass spectra for Cl2 and Br2 show the relative abundance of different isotopes of chlorine and bromine in the diatomic molecules.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":50,"explanation":"The mass spectra for Cl2 and Br2 provide information about the isotopes present in the molecules. Isotopes are atoms of the same element with different numbers of neutrons. The relative abundance of these isotopes can be determined by analyzing the mass spectra. This information is important for understanding the chemical behavior and properties of these diatomic molecules.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974173,"front":"How can mass spectrometers be used in planetary space probes?","back":"Mass spectrometers in planetary space probes can identify elements on other planets by analyzing the composition of isotopes.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":52,"explanation":"Mass spectrometers are crucial in planetary space probes as they can analyze isotopic composition to identify elements on other planets. This helps scientists understand planetary composition and potential habitability without the need for physical samples.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974174,"front":"Describe the process of measuring the molecular mass (M) of a molecule using a mass spectrometer.","back":"When a molecule is put through a mass spectrometer with electron impact ionization, it often breaks up into fragments. The peak with the largest m/z corresponds to the complete molecule and is equal to the relative molecular mass (M) of the molecule.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":53,"explanation":"Mass spectrometry with electron impact ionization causes a molecule to fragment. The peak with the highest m/z ratio represents the intact molecule's molecular mass (M). This method is widely used for determining the molecular mass of various compounds.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974178,"front":"What is the relative abundance of the isotopes Cl³5 and Cl³7 in chlorine?","back":"The relative abundance of Cl³5 is 75%, while the relative abundance of Cl³7 is 25% in chlorine.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":57,"explanation":"The relative abundance of isotopes in an element is determined by the natural abundance of each isotope in the Earth's crust. Isotopes with higher natural abundance will have a higher relative abundance in the element. In the case of chlorine, Cl³5 has a higher natural abundance than Cl³7, resulting in a higher relative abundance of Cl³5 compared to Cl³7. This is why Cl³5 has a relative abundance of 75% and Cl³7 has a relative abundance of 25% in chlorine.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974180,"front":"Describe the Bohr model of the atom.","back":"The Bohr model of the atom proposed that electrons orbit the nucleus in spherical orbits, with 2 electrons in the first shell, 8 in the second, and so on.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":59,"explanation":"The Bohr model of the atom was a significant advancement in understanding atomic structure. It introduced the concept of quantized electron energy levels, explaining atomic spectra and stability. This model laid the foundation for modern quantum mechanics.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974182,"front":"What are the sub energy levels in the model of atomic structure?","back":"The sub energy levels in the model are labeled S, p, d, and f.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":60,"explanation":"The sub energy levels in the model of atomic structure are labeled S, p, d, and f. These sublevels are associated with different shapes and orientations of the electron orbitals within an atom. They play a crucial role in understanding the organization of electrons within an atom.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974184,"front":"Define orbitals in the model of atomic structure.","back":"Orbitals are regions around the nucleus that hold up to a specific number of electrons. They are split into sub-levels, such as S, p, d, and f.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":61,"explanation":"Orbitals are crucial in understanding atomic structure. They provide a way to visualize where electrons are likely to be found within an atom. The different sub-levels (s, p, d, and f) have distinct shapes and orientations, reflecting the probability of finding electrons in specific regions around the nucleus. This model helps explain the behavior of electrons in atoms and their interactions with each other.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974186,"front":"Describe the shapes of orbitals in the model of atomic structure.","back":"Orbitals represent the mathematical probabilities of finding an electron at any point within certain spatial distributions around the nucleus. Each orbital has its own approximate three-dimensional shape.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":62,"explanation":"Orbitals in the model of atomic structure represent the probability distribution of finding an electron in a specific region around the nucleus. These regions have different shapes, such as spherical (s orbitals), dumbbell-shaped (p orbitals), and more complex shapes (d and f orbitals). Each orbital has its own unique three-dimensional shape, which is determined by the mathematical equations that describe the behavior of electrons in atoms.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":974188,"front":"How does an atom fill up sub shells in the model of atomic structure?","back":"An atom fills up the sub shells in order of increasing energy. For example, the 3d sub shell is higher in energy than the 4s sub shell, so it gets filled after the 4s.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":63,"explanation":"In the model of atomic structure, sub shells are filled in order of increasing energy. This is because electrons occupy the lowest energy levels first before moving to higher energy levels. For example, the 3d sub shell has higher energy than the 4s sub shell, so it gets filled after the 4s. This filling pattern is based on the principle that electrons seek to occupy the most stable and lowest energy states available to them.","deleted_at":null,"flashcard_deck_id":"QuTAl","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}}]

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