Question 1

Which of the following best explains why the first ionization energy ($$IE_1) of $$lithium is much lower than that of neon?

Accepted Answer

Lithium has a larger atomic radius and its valence electron is farther from the nucleus, so it is less tightly held.

Question 2

Which element would you expect to have the largest jump between its second and third ionization energies?

Accepted Answer

Mg

Question 3

Why is the first ionization energy of boron ($$B) $$lower than that of beryllium ($$Be$$), even though $$B is to $$the right of $$Be in $$the periodic table?

Accepted Answer

The $$2p$$ electron in $$B is $$higher in energy and less tightly held than the $$2s$$ electron in $$Be.$$

Question 4

Which of the following elements has the most negative electron affinity?

Accepted Answer

Cl

Question 5

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

Accepted Answer

Metallic character decreases because ionization energy increases.

Question 6

Which of the following elements would you expect to have the highest first ionization energy ($$IE_1$$)?

Accepted Answer

Ne

Question 7

Why does oxygen ($$O) $$have a lower first ionization energy than nitrogen ($$N$$)?

Accepted Answer

Oxygen has electron-electron repulsion due to paired electrons in the $$2p$$ orbital.

Question 8

Which of the following best explains why sodium ($$Na) $$commonly forms a $$1+$$ ion and not a $$2+$$ ion?

Accepted Answer

Sodium has only one valence electron that is easily removed; removing a second electron would be much more difficult because it would be a core electron.

Question 9

Arrange the following elements in order of increasing metallic character: Si, Cl, Na, Rb.

Accepted Answer

Cl \u003c Si \u003c Na \u003c Rb

Question 10

Which of the following statements about electron affinity is correct?

Accepted Answer

Electron affinity generally becomes more negative across a period due to increasing effective nuclear charge.

Question 11

Which element would you expect to have the largest atomic radius?

Accepted Answer

Rb

Question 12

Which of the following best describes the effective nuclear charge ($$Z_{eff}) $$experienced by the valence electron in lithium ($$Li$$)?

Accepted Answer

$$Z_{eff} \approx 3 - 2 = 1$$

Question 13

Which of the following elements would you expect to have the least metallic character?

Accepted Answer

Cl

Question 14

Which of the following best explains why the second ionization energy ($$IE_2) of $$sodium is much higher than its first ionization energy ($$IE_1$$)?

Accepted Answer

The second electron is removed from a core shell, which is much closer to the nucleus and more tightly held.

Question 15

Which of the following elements would you expect to have the lowest first ionization energy?

Accepted Answer

K

Question 16

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

Accepted Answer

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

Question 17

Which of the following best explains why chlorine ($$Cl) $$has a more negative electron affinity than sodium ($$Na$$)?

Accepted Answer

Chlorine achieves a noble gas configuration upon gaining an electron, resulting in greater stability.

Question 18

Which of the following elements would you expect to have the highest metallic character?

Accepted Answer

Rb

Question 19

Which of the following statements about periodic trends is correct?

Accepted Answer

Atomic radius increases down a group and decreases across a period.

Periodic Properties of the Elements: Ionization Energy, Electron Affinity, and Metallic Character

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