Question
f Giving reasons explain how the following periodic trends varies across and down the group (10 marks) i. Electron Affinity ii. Atomic radius iii. Electronegativity iv Effective nuclear charge v. Ionization energy
Solution
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(335 Votos)
Francielle
Profissional · Tutor por 6 anos
Resposta
i. Electron Affinity:Electron affinity generally increases across a period from left to right and decreases down a group in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the incoming electron. As you move down a group, the outermost electron is farther from the nucleus, resulting in a weaker attraction and lower electron affinity.ii. Atomic radius:The atomic radius generally decreases across a period from left to right and increases down a group in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, causing the electrons to be pulled closer to the nucleus, resulting in a smaller atomic radius. As you move down a group, the number of electron shells increases, causing the outermost electron to be farther from the nucleus, resulting in a larger atomic radius.iii. Electronegativity:Electronegativity generally increases across a period from left to right and decreases down a group in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the bonding electrons. As you move down a group, the outermost electron is farther from the nucleus, resulting in a weaker attraction and lower electronegativity.iv. Effective nuclear charge:Effective nuclear charge generally increases across a period from left to right and decreases down a group in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the electrons. As you move down a group, the outermost electron is farther from the nucleus, resulting in a weaker attraction and lower effective nuclear charge.v. Ionization energy:Ionization energy generally increases across a period from left to right and decreases down a group in the periodic table. This is because as you move across a period, the number of protons in the nucleus increases, leading to a stronger attraction between the nucleus and the electrons, making it more difficult to remove an electron. As you move down a group, the outermost electron is farther from the nucleus, resulting in a weaker attraction and lower ionization energy.