Q: A sodium atom emits light with a wavelength of $$589\ \text{nm}$$ when an electron transitions from a higher to a lower energy level. What is the energy of the emitted photon? ($$h = 6.626 \times 10$$^{-34}$$\ \text{J}\cdot\text{s}$$, $$c = 3.00 \times 10^8$\ \text{m/s})$$

$$3.38 \times 10$$^{-19}$$\ \text{J}$$

Q: Which of the following pairs of elements is most likely to form an ionic bond?

Sodium ($$\text{Na}) $$and Chlorine ($$\text{Cl})$$

Question 1

Which of the following best explains why the effective nuclear charge ($$Z_{	ext{eff}}) $$experienced by a 3p electron in sulfur is less than the actual nuclear charge ($$Z) of $$sulfur?

Accepted Answer

Because inner-shell electrons shield outer electrons from the full nuclear charge.

Question 2

Which set of quantum numbers is NOT allowed for an electron in an atom?

Accepted Answer

$$n = 2,\ l = 2,\ m_l = 0,\ m_s = +\frac{1}{2}$$

Question 3

Which of the following electron configurations represents a paramagnetic ion?

Accepted Answer

$$[	ext{Ne}]\ 3s^2$\ 3p^5$

Question 4

A sodium atom emits light with a wavelength of $$589\ 	ext{nm}$$ when an electron transitions from a higher to a lower energy level. What is the energy of the emitted photon? ($$h = 6.626 	imes 10$$^{-34}$$\ 	ext{J}\cdot	ext{s}$$, $$c = 3.00 	imes 10^8$\ 	ext{m/s})$$

Accepted Answer

$$3.38 	imes 10$$^{-19}$$\ 	ext{J}$$

Question 5

Which of the following statements about core and valence electrons is correct?

Accepted Answer

Valence electrons are responsible for chemical bonding.

Question 6

Which element has the highest first ionization energy?

Accepted Answer

Neon ($$	ext{Ne})$$

Question 7

Which of the following ions is isoelectronic with argon ($$	ext{Ar}$$)?

Accepted Answer

$$	ext{K}^+$$

Question 8

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

Accepted Answer

Atomic radius decreases due to increasing effective nuclear charge.

Question 9

Which of the following electron configurations represents the ground state of a chromium atom ($$Z=24$$)?

Accepted Answer

$$[	ext{Ar}]\ 4s^1$\ 3d^5$

Question 10

Which of the following best explains why ionic compounds tend to have high melting points?

Accepted Answer

Because the electrostatic attraction between oppositely charged ions is strong.

Question 11

Which of the following pairs of elements is most likely to form an ionic bond?

Accepted Answer

Sodium ($$	ext{Na}) $$and Chlorine ($$	ext{Cl})$$

Question 12

Which of the following ions is expected to be diamagnetic?

Accepted Answer

$$	ext{Zn}^{2+}$$

Question 13

Which of the following statements about covalent bonds is correct?

Accepted Answer

Covalent bonds involve the sharing of electrons between atoms.

Question 14

Which of the following best describes the emission of light from an atom?

Accepted Answer

An electron falls from a higher to a lower energy level, emitting a photon.

Question 15

Which of the following elements has the greatest number of unpaired electrons in its ground state?

Accepted Answer

Nitrogen ($$	ext{N})$$

Question 16

Which of the following best explains why magnesium forms a $$2+$$ ion?

Accepted Answer

Magnesium has two valence electrons, which it loses to achieve a noble gas configuration.

Question 17

Which of the following is the correct order of increasing electronegativity?

Accepted Answer

$$	ext{Na} \u003c 	ext{Mg} \u003c 	ext{Al} \u003c 	ext{Cl}$$

Question 18

A sample of calcium ions ($$	ext{Ca}^{2+}) is $$placed in a magnetic field. What is the expected magnetic behavior?

Accepted Answer

Diamagnetic, because all electrons are paired.

Question 19

Which of the following best describes the difference between ionic and covalent bonding?

Accepted Answer

Ionic bonding involves the transfer of electrons, while covalent bonding involves the sharing of electrons.

Question 20

Which of the following is the correct electron configuration for the oxide ion ($$	ext{O}^{2-}$$)?

Accepted Answer

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

CH101 EOH Quiz 2 Study Guide: Atomic Structure, Periodic Trends, and Bonding

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