Question 1

Which statement best explains why the sublevels in a hydrogen atom are said to be 'degenerate'?

Accepted Answer

All sublevels within a principal energy level have the same energy because there is only one electron and no electron-electron repulsion.

Question 2

How many orbitals are present in the n = 3 principal energy level of an atom?

Accepted Answer

$$9$$

Question 3

Which quantum number is responsible for describing the orientation of an electron's spin in an orbital?

Accepted Answer

Spin quantum number $$m_s$$

Question 4

What is the maximum number of electrons that can occupy the $$3d$$ sublevel?

Accepted Answer

$$10$$

Question 5

Which of the following best describes the shape of a $$p$$ orbital?

Accepted Answer

Dumbbell-shaped with two lobes on opposite sides of the nucleus

Question 6

What is the value of the spin quantum number $$m_s$$ for an electron with spin 'down'?

Accepted Answer

$$-\frac{1}{2}$$

Question 7

Which of the following elements is expected to have the largest atomic radius?

Accepted Answer

Potassium ($$K)$$

Question 8

Why are cations generally smaller than their parent neutral atoms?

Accepted Answer

Cations have fewer electrons, resulting in less electron-electron repulsion and a greater effective nuclear charge per electron.

Question 9

Which of the following statements about ionization energy is correct?

Accepted Answer

First ionization energy generally increases across a period due to increasing effective nuclear charge.

Question 10

Which element is expected to have the most negative electron affinity?

Accepted Answer

Chlorine ($$Cl)$$

Question 11

A transition metal ion with unpaired electrons will exhibit which magnetic property?

Accepted Answer

Paramagnetism

Question 12

Which of the following ions is expected to be diamagnetic?

Accepted Answer

$$Zn^{2+}$$

Question 13

Which orbital penetrates closest to the nucleus in a multi-electron atom?

Accepted Answer

$$3s$$

Question 14

What is the total number of nodes in a $$2p$$ orbital?

Accepted Answer

$$1$$

Question 15

Which of the following best explains why noble gases have positive electron affinities?

Accepted Answer

Adding an electron would require placing it in a higher energy orbital, which is energetically unfavorable due to their closed sublevels.

Question 16

If an atom has $$n = 4$$, how many sublevels are present?

Accepted Answer

$$4$$

Question 17

Which of the following best describes the trend in ionic radius for anions compared to their parent atoms?

Accepted Answer

Anions are larger than their parent atoms due to increased electron-electron repulsion.

Question 18

Which of the following is the correct electron configuration for a neutral nitrogen atom?

Accepted Answer

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

Question 19

Which of the following best explains the large increase in ionization energy when removing a core electron?

Accepted Answer

Core electrons are much closer to the nucleus and experience a much higher effective nuclear charge.

Question 20

A hospital is using sodium vapor lamps for lighting. Which property of sodium makes it suitable for this application?

Accepted Answer

Sodium has a low first ionization energy, making it easy to excite electrons and produce light.

Atomic Structure, Quantum Numbers, and Periodic Trends: Study Notes

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