Question 1

Which of the following best explains why the atomic radius increases as you move down a group in the periodic table?

Accepted Answer

Electrons are added to higher principal energy levels, increasing the distance from the nucleus.

Question 2

Which of the following elements is expected to have the highest first ionization energy?

Accepted Answer

S

Question 3

A main-group element has the outer electron configuration $$ns^2np^5$. What charge is likely for an ion of this element?

Accepted Answer

$$1-$$

Question 4

Which of the following statements about the periodic law is correct?

Accepted Answer

When elements are arranged in order of increasing atomic number, certain sets of properties recur periodically.

Question 5

Which of the following ions is expected to be paramagnetic?

Accepted Answer

$$\mathrm{Fe$$^{3+}$$}$$

Question 6

Which of the following best describes the trend in electron affinity across a period (left to right) for main-group elements?

Accepted Answer

Electron affinity becomes more negative.

Question 7

Which of the following elements is a transition metal?

Accepted Answer

Cr

Question 8

Which of the following statements about the Pauli exclusion principle is correct?

Accepted Answer

No two electrons in an atom can have the same set of four quantum numbers.

Question 9

Which of the following best explains why sodium 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 more difficult because it would be a core electron.

Question 10

Which of the following pairs of elements is arranged in order of increasing atomic radius?

Accepted Answer

N \u003c F

Question 11

Which of the following statements about metallic character is correct?

Accepted Answer

Metallic character increases down a group and decreases across a period.

Question 12

Which of the following electron configurations represents a noble gas?

Accepted Answer

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

Question 13

Which of the following best describes the effect of penetration on sublevel energy in multi-electron atoms?

Accepted Answer

An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.

Question 14

Which of the following best explains why valence electrons are more important than core electrons in determining the reactivity and bonding in atoms?

Accepted Answer

Since bonding involves the transfer or sharing of electrons, valence electrons are most important because they are held most loosely.

Question 15

Which of the following statements about the electron configuration of transition metals is correct?

Accepted Answer

Some transition metals have irregular electron configurations due to the stability of half-filled or fully filled d sublevels.

Question 16

Which of the following best describes the trend in first ionization energy as you move down a group in the periodic table?

Accepted Answer

First ionization energy decreases.

Question 17

Which of the following is the correct electron configuration for phosphorus (P)?

Accepted Answer

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

Question 18

Which of the following pairs is isoelectronic?

Accepted Answer

$$\mathrm{Na^+}$$ \, \& \, \mathrm{Ne}$

Question 19

Which of the following statements about the effective nuclear charge ($$Z_{\mathrm{eff}}) is $$correct?

Accepted Answer

$$Z_{\mathrm{eff}}$$ increases as you go across a period and decreases as you go down a group.

Periodic Properties of the Elements: Structure, Electron Configuration, and Trends

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