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Periodicity

A-Level AQA Chemistry

This pack of flashcards covers the concepts of periodicity, electron configuration, and chemical bonding in elements. It explains atomic radius trends, ionization energy, metallic bonding strength, and variations in bonding types across different elements, including the transition from metallic to covalent and van der Waals forces.

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"Describe periodicity."	"Periodicity is the repeating pattern of physical or chemical properties going across the periods."
"Define s, p, and d blocks."	"Elements are classified as S, p or d block, according to which orbitals the highest energy electrons are in."
"How does atomic radius change across a period?"	"Atomic radii decrease from left to right across a period, because the increased number of protons create more positive charge attraction for electrons which are in the same shell with similar shielding."
"What is the trend in atomic radius in period 2?"	"The atomic radii decrease from left to right in period 2."
"Describe the trend in 1st ionization energy."	"There is a general trend across to increase in 1st ionization energy. This is due to the increasing number of protons as the electrons are being added to the same shell."
"What is the reason for the small drop in ionization energy between phosphorous and sulfur?"	"Sulfur's outer electron is being paired up with another electron in the same 3p orbital."
"Explain why the second electron is easier to remove when added to an orbital."	"When the second electron is added to an orbital, there is a slight repulsion between the two negatively charged electrons, making the second electron easier to remove."
"What is the relationship between the number of electrons in the outer shell and the strength of metallic bonding?"	"The more electrons there are in the outer shell that are released to the sea of electrons, the stronger the metallic bonding."
"Define metallic bonding."	"Metallic bonding is a type of chemical bonding that occurs between metal atoms, where the outer electrons are delocalized and form a 'sea' of electrons that surround the positively charged metal ions."
"Describe the relationship between the size of an ion and its bonding strength."	"A smaller sized ion with a greater positive charge makes the bonding stronger."
"What is the general trend in energy needed to break bonds?"	"Higher energy is needed to break bonds."
"What type of bonding does Na, Mg, Al, Si, P, S, Cl, and Ar exhibit?"	"Na, Mg, Al, and Si exhibit metallic bonding, P and S exhibit macromolecular bonding, Cl2(g), S8(s), and P4(s) exhibit simple molecular bonding, and Ar exhibits monoatomic weak van der Wa bonding."
"Why does S8 have a higher melting point than P4?"	"S8 has more electrons, resulting in stronger van der Waals forces between molecules."

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Describe periodicity.

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Periodicity is the repeating pattern of physical or chemical properties going across the periods.

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[{"id":977909,"front":"Describe periodicity.","back":"Periodicity is the repeating pattern of physical or chemical properties going across the periods.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Periodicity refers to the regular and predictable repetition of certain properties or behaviors in a periodic table. This pattern is observed as elements are arranged in increasing atomic number. The periodicity is a result of the periodic law, which states that the properties of elements are a periodic function of their atomic number. This periodic pattern allows for the classification and prediction of various properties, such as atomic radius, ionization energy, and chemical reactivity, based on an element's position in the periodic table.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977911,"front":"Define s, p, and d blocks.","back":"Elements are classified as S, p or d block, according to which orbitals the highest energy electrons are in.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The classification of elements into s, p, and d blocks is based on the arrangement of electrons in their orbitals. The s block consists of elements whose highest energy electrons are in the s orbital, the p block consists of elements with highest energy electrons in the p orbital, and the d block consists of elements with highest energy electrons in the d orbital. This classification helps in understanding the periodic trends and properties of elements.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977913,"front":"How does atomic radius change across a period?","back":"Atomic radii decrease from left to right across a period, because the increased number of protons create more positive charge attraction for electrons which are in the same shell with similar shielding.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The atomic radius decreases across a period due to the increasing number of protons in the nucleus. This leads to a stronger positive charge attraction for the electrons in the same shell. Additionally, the shielding effect from inner electron shells remains constant, resulting in a stronger pull on the outermost electrons. As a result, the atomic radius decreases across a period.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977915,"front":"What is the trend in atomic radius in period 2?","back":"The atomic radii decrease from left to right in period 2.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The trend in atomic radius in period 2 is due to the increasing nuclear charge as you move from left to right across the period. This results in a stronger pull on the electrons, leading to a decrease in atomic radius.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977917,"front":"Describe the trend in 1st ionization energy.","back":"There is a general trend across to increase in 1st ionization energy. This is due to the increasing number of protons as the electrons are being added to the same shell.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The trend in 1st ionization energy is generally increasing. This is because as the number of protons increases, the positive charge in the nucleus becomes stronger, making it more difficult to remove an electron. Additionally, as electrons are added to the same shell, they experience increased repulsion from each other, making it harder to remove an electron.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977920,"front":"What is the reason for the small drop in ionization energy between phosphorous and sulfur?","back":"Sulfur's outer electron is being paired up with another electron in the same 3p orbital.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The small drop in ionization energy between phosphorus and sulfur can be attributed to the pairing of sulfur's outer electron with another electron in the same 3p orbital. This electron-electron repulsion makes it easier to remove the outermost electron, resulting in a lower ionization energy.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977923,"front":"Explain why the second electron is easier to remove when added to an orbital.","back":"When the second electron is added to an 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":0,"explanation":"The presence of the first electron in an orbital creates a repulsive force that slightly weakens the attraction of the nucleus for the second electron. This makes it easier to remove the second electron compared to adding the first one.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977924,"front":"What is the relationship between the number of electrons in the outer shell and the strength of metallic bonding?","back":"The more electrons there are in the outer shell that are released to the sea of electrons, the stronger the metallic bonding.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The number of electrons in the outer shell directly affects the strength of metallic bonding. When more electrons are released into the sea of electrons, there is a greater attraction between the positive metal ions and the negative electron cloud. This results in stronger metallic bonding.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977926,"front":"Define metallic bonding.","back":"Metallic bonding is a type of chemical bonding that occurs between metal atoms, where the outer electrons are delocalized and form a 'sea' of electrons that surround the positively charged metal ions.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"Metallic bonding is a fundamental concept in chemistry and materials science. It explains the unique properties of metals, such as conductivity and malleability. The delocalized electrons create a strong attractive force between metal ions, leading to the characteristic properties of metals.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977929,"front":"Describe the relationship between the size of an ion and its bonding strength.","back":"A smaller sized ion with a greater positive charge makes the bonding stronger.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The size of an ion is inversely related to its bonding strength. Smaller ions have a stronger bonding strength because they have a higher charge density. This means that the positive charge is concentrated in a smaller space, leading to stronger electrostatic attractions between ions. Additionally, smaller ions can get closer to each other, allowing for stronger bonding interactions.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977931,"front":"What is the general trend in energy needed to break bonds?","back":"Higher energy is needed to break bonds.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The general trend in energy needed to break bonds is that it is higher. This is because breaking bonds requires overcoming the attractive forces between atoms or molecules, which requires energy input. The strength of these forces varies depending on the type of bond, but in general, stronger bonds require more energy to break.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977935,"front":"What type of bonding does Na, Mg, Al, Si, P, S, Cl, and Ar exhibit?","back":"Na, Mg, Al, and Si exhibit metallic bonding, P and S exhibit macromolecular bonding, Cl2(g), S8(s), and P4(s) exhibit simple molecular bonding, and Ar exhibits monoatomic weak van der Wa bonding.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"The elements mentioned exhibit different types of bonding based on their atomic structure and properties. Metallic bonding occurs in metals, macromolecular bonding in nonmetals, simple molecular bonding in diatomic and polyatomic molecules, and monoatomic weak van der Waals bonding in noble gases. These bonding types are determined by the arrangement and behavior of the atoms in each element.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}},{"id":977936,"front":"Why does S8 have a higher melting point than P4?","back":"S8 has more electrons, resulting in stronger van der Waals forces between molecules.","front_language":"English","back_language":"English","front_image":"","back_image":"","order":0,"explanation":"S8 has a higher melting point than P4 due to the presence of more electrons, leading to stronger van der Waals forces between molecules. This results in a greater amount of energy required to overcome these forces, leading to a higher melting point.","deleted_at":null,"flashcard_deck_id":"d3Tav","original_id":null,"examMode":{"text":"","correct":"","incorrect":"","info":""}}]

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