Electron Configuration

What does electron configuration describe?

• The arrangement of protons and neutrons in an atom's nucleus.

• The distribution of electrons within an atom or ion.

• The total number of electrons in a given element.

• The energy required to create an ion.

Which factors primarily determine the ionization energy of an electron according to Coulomb's Law?

• The mass of the electron and the speed of light.

• The number of neutrons and the atomic mass.

• The charges of the particles and the distance between them.

• The electron's spin and orbital angular momentum.

Why does Lithium (Li) have a lower first ionization energy than Helium (He), despite having more protons?

• Lithium has a smaller atomic radius, increasing electron-nucleus attraction.

• Lithium's valence electron is in a higher energy shell, experiencing less nuclear attraction due to shielding.

• Helium has a completely filled outer shell, making it less reactive.

• Lithium's nucleus has a weaker positive charge compared to Helium.

What trend is observed in the first ionization energy graph for elements like Helium, Neon, Argon, Krypton, and Xenon?

• They represent the lowest ionization energies within their respective periods.

• They consistently show a decrease in ionization energy as atomic number increases.

• They correspond to the highest ionization energies, indicating stable electron configurations.

• They are transition metals with variable ionization energies.

What is the primary reason for the decrease in first ionization energy when moving from Beryllium to Boron?

• The electron in Boron is in a higher energy 2p orbital, making it easier to remove.

• Boron has more protons, increasing the nuclear attraction.

• Beryllium has a completely filled 2s subshell, which is very stable.

• Boron has a larger atomic radius than Beryllium.

Which factor explains the decrease in first ionization energy from Nitrogen to Oxygen?

• Oxygen has a larger atomic radius, reducing nuclear attraction.

• The added electron in Oxygen pairs up in a 2p orbital, leading to increased electron-electron repulsion.

• Nitrogen has a half-filled 2p subshell, which is more stable.

• Oxygen has a higher effective nuclear charge.

What is the maximum number of electrons that can be accommodated in a d-subshell?

• 2

• 6

• 10

• 14

What is the full electron configuration for Chlorine (Cl), which has 17 electrons?

• 1s2 2s2 2p6 3s2 3p5

• 1s2 2s2 2p6 3s2 3p6

• 1s2 2s2 2p6 3s2 3d5

• 1s2 2s2 2p6 3s2 4s2 3d3