Question 1

Which of the following elements has the highest first ionization energy?

$$\mathrm{A)\ K} \qquad \mathrm{B)\ S} \qquad \mathrm{C)\ Cl} \qquad \mathrm{D)\ Na}$$

Accepted Answer

Cl

Question 2

As you move from left to right across a period in the periodic table, which of the following trends is generally observed for atomic radius?

$$\mathrm{A)\ It\ increases}$$

$$\mathrm{B)\ It\ decreases}$$

$$\mathrm{C)\ It\ remains\ constant}$$

$$\mathrm{D)\ It\ first\ increases,\ then\ decreases}$$

Accepted Answer

It decreases

Question 3

Which element below would you expect to have the lowest electron affinity?

$$\mathrm{A)\ Cl} \qquad \mathrm{B)\ Na} \qquad \mathrm{C)\ P} \qquad \mathrm{D)\ O}$$

Accepted Answer

Na

Question 4

Rank the following elements in order of increasing atomic radius: $$\mathrm{S,\ K,\ B,\ Cl}$$.

$$\mathrm{A)\ B \u003c S \u003c Cl \u003c K}$$

$$\mathrm{B)\ K \u003c Cl \u003c S \u003c B}$$

$$\mathrm{C)\ Cl \u003c S \u003c B \u003c K}$$

$$\mathrm{D)\ B \u003c Cl \u003c S \u003c K}$$

Accepted Answer

B \u003c S \u003c Cl \u003c K

Question 5

Which of the following best explains why ionization energy decreases as you move down a group in the periodic table?

$$\mathrm{A)\ The\ atomic\ radius\ increases}$$

$$\mathrm{B)\ The\ number\ of\ protons\ decreases}$$

$$\mathrm{C)\ The\ number\ of\ neutrons\ increases}$$

$$\mathrm{D)\ The\ electron\ affinity\ increases}$$

Accepted Answer

The atomic radius increases

Question 6

Which of the following elements is expected to have the most metallic character?

$$\mathrm{A)\ Na} \qquad \mathrm{B)\ Cl} \qquad \mathrm{C)\ S} \qquad \mathrm{D)\ P}$$

Accepted Answer

Na

Question 7

Which of the following statements is true regarding periodic trends for main group elements?

$$\mathrm{A)\ Electronegativity\ decreases\ across\ a\ period}$$

$$\mathrm{B)\ Atomic\ radius\ increases\ across\ a\ period}$$

$$\mathrm{C)\ Ionization\ energy\ increases\ across\ a\ period}$$

$$\mathrm{D)\ Metallic\ character\ increases\ across\ a\ period}$$

Accepted Answer

Ionization energy increases across a period

Question 8

Which of the following elements would require the most energy to remove its outermost electron?

$$\mathrm{A)\ K} \qquad \mathrm{B)\ Na} \qquad \mathrm{C)\ Cl} \qquad \mathrm{D)\ S}$$

Accepted Answer

Cl

Question 9

Which of the following is the correct order of increasing ionization energy for the elements $$\mathrm{Na,\ K,\ Cl,\ S}$$?

$$\mathrm{A)\ K \u003c Na \u003c S \u003c Cl}$$

$$\mathrm{B)\ Na \u003c K \u003c S \u003c Cl}$$

$$\mathrm{C)\ Cl \u003c S \u003c Na \u003c K}$$

$$\mathrm{D)\ S \u003c Cl \u003c Na \u003c K}$$

Accepted Answer

K \u003c Na \u003c S \u003c Cl

Question 10

Which of the following elements is most likely to gain an electron to form a stable anion?

$$\mathrm{A)\ Na} \qquad \mathrm{B)\ Cl} \qquad \mathrm{C)\ K} \qquad \mathrm{D)\ S}$$

Accepted Answer

Cl

Question 11

Which of the following best describes the trend in metallic character as you move down a group in the periodic table?

$$\mathrm{A)\ It\ increases}$$

$$\mathrm{B)\ It\ decreases}$$

$$\mathrm{C)\ It\ remains\ constant}$$

$$\mathrm{D)\ It\ first\ increases,\ then\ decreases}$$

Accepted Answer

It increases

Question 12

Which of the following elements has the smallest atomic radius?

$$\mathrm{A)\ K} \qquad \mathrm{B)\ S} \qquad \mathrm{C)\ Cl} \qquad \mathrm{D)\ Na}$$

Accepted Answer

Cl

Question 13

Which of the following statements is correct regarding electron affinity?

$$\mathrm{A)\ Electron\ affinity\ becomes\ more\ negative\ across\ a\ period}$$

$$\mathrm{B)\ Electron\ affinity\ becomes\ less\ negative\ across\ a\ period}$$

$$\mathrm{C)\ Electron\ affinity\ does\ not\ change\ across\ a\ period}$$

$$\mathrm{D)\ Electron\ affinity\ increases\ down\ a\ group}$$

Accepted Answer

Electron affinity becomes more negative across a period

Question 14

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

$$\mathrm{A)\ Cl} \qquad \mathrm{B)\ K} \qquad \mathrm{C)\ S} \qquad \mathrm{D)\ B}$$

Accepted Answer

K

Question 15

Which of the following is the best explanation for why chlorine has a higher electron affinity than sodium?

$$\mathrm{A)\ Chlorine\ has\ a\ smaller\ atomic\ radius}$$

$$\mathrm{B)\ Sodium\ has\ more\ protons}$$

$$\mathrm{C)\ Chlorine\ is\ more\ metallic}$$

$$\mathrm{D)\ Sodium\ has\ a\ higher\ ionization\ energy}$$

Accepted Answer

Chlorine has a smaller atomic radius

Main Group Elements: Periodic Trends Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards