Question 1

Which of the following best explains why the first ionization energy of nitrogen is higher than that of oxygen, despite oxygen having a greater nuclear charge?

Accepted Answer

Nitrogen has a half-filled 2p subshell, which is more stable due to minimized electron-electron repulsion, making it harder to remove an electron.

Question 2

Based on Coulomb’s law, which factor most significantly increases the force of attraction between the nucleus and a valence electron?

Accepted Answer

Increasing the magnitude of the nuclear charge (number of protons)

Question 3

Which of the following ions has the largest ionic radius: $$\mathrm{K^+}$$, $$\mathrm{Ca$$^{2+}$$}$$, $$\mathrm{S$$^{2-}$$}$$, or $$\mathrm{Cl^-}$$?

Accepted Answer

$$\mathrm{S$$^{2-}$$}$$

Question 4

Which element has the highest electronegativity value?

Accepted Answer

Fluorine

Question 5

As you move down a group in the periodic table, what happens to the atomic radius and why?

Accepted Answer

Atomic radius increases because electrons are added to higher energy levels, increasing the distance from the nucleus.

Question 6

Which of the following best describes the trend in first ionization energy as you move from left to right across a period?

Accepted Answer

It increases due to increasing nuclear charge with electrons in the same energy level.

Question 7

Given the electron configurations below, which particle has a larger radius: $$\mathrm{Na} or$$ $$\mathrm{Na^+}$$? Justify your answer.

Accepted Answer

$$\mathrm{Na}$$, because it has one more electron, resulting in greater electron-electron repulsion and a larger radius.

Question 8

Which of the following best explains why the second ionization energy of sodium is much higher than that of magnesium?

Accepted Answer

The second electron in sodium is removed from a lower energy level (closer to the nucleus), resulting in a much stronger attraction according to Coulomb’s law.

Question 9

Which of the following pairs of elements will form a binary ionic compound with the formula $$\mathrm{$$MgCl_2$$}$$?

Accepted Answer

Magnesium and chlorine

Question 10

Which of the following statements about electronegativity is correct?

Accepted Answer

Electronegativity increases across a period and decreases down a group.

Question 11

Which of the following best explains why the electron affinity of fluorine is more negative than that of lithium?

Accepted Answer

Fluorine has a higher nuclear charge and a smaller atomic radius, resulting in a stronger attraction for the added electron.

Question 12

Which of the following elements has the greatest tendency to form a $$2+$$ ion?

Accepted Answer

Magnesium

Question 13

Which of the following best describes the trend in atomic radius as you move from left to right across a period?

Accepted Answer

Atomic radius decreases due to increasing nuclear charge pulling electrons closer.

Question 14

Which of the following is the correct ground-state electron configuration for $$\mathrm{Fe$$^{2+}$$}$$?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^6$$\ $$3s^2$$\ $$3p^6$$\ $$3d^6$$

Question 15

Which of the following best explains why the ionic radius of $$\mathrm{Fe$$^{2+}$$} is $$larger than that of $$\mathrm{Fe$$^{3+}$$}$$?

Accepted Answer

$$\mathrm{Fe$$^{2+}$$}$$ has one more electron, resulting in greater electron-electron repulsion and a larger radius.

Question 16

Which of the following best describes the relationship between atomic radius and electronegativity?

Accepted Answer

As atomic radius decreases, electronegativity increases.

Question 17

Which of the following elements is most likely to form an anion with a $$1-$$ charge?

Accepted Answer

Fluorine

Question 18

Which of the following best explains why successive ionization energies increase for a given element?

Accepted Answer

As each electron is removed, the remaining electrons experience a greater effective nuclear charge, increasing the energy required to remove the next electron.

Question 19

Which of the following best describes the direction of the dipole moment in a polar covalent bond between atoms X and Y, where Y is more electronegative?

Accepted Answer

The dipole moment points toward Y, the more electronegative atom.

Study Guide: Periodic Trends, Atomic Structure, and Ionic Compounds

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