Question 1

Which of the following statements best explains why the atomic radius of transition metals remains nearly constant across a period?

Accepted Answer

Electrons are added to inner d orbitals, which shield the increase in nuclear charge, resulting in little change in atomic radius.

Question 2

Across a period, the atomic radius of main group elements generally:

Accepted Answer

Decreases because the effective nuclear charge increases.

Question 3

Which element from each period would you predict to have the largest atomic size?

Accepted Answer

The element in group 1 (alkali metals).

Question 4

Why do transition metals show a much smaller decrease in atomic radius across a period compared to main group elements?

Accepted Answer

Because electrons are added to inner d orbitals, which partially shield the increase in nuclear charge.

Question 5

Which of the following transition metals is expected to have the highest density?

Accepted Answer

Os

Question 6

What is the primary factor that causes the density of transition metals to increase down a group?

Accepted Answer

Increase in mass of the metal atoms.

Question 7

Which of the following best describes the trend in density across a period for transition metals?

Accepted Answer

Density remains nearly constant across the period.

Question 8

Given the following elements: Fe, Co, Ni, which would you expect to have the smallest atomic radius?

Accepted Answer

Ni

Question 9

Which of the following equations correctly represents the relationship for effective nuclear charge ($$Z_{eff}) in $$transition metals?

Accepted Answer

$$Z_{eff} = Z - S$$

Question 10

A student claims that atomic radius always increases as you move down a group in the periodic table. Which of the following best evaluates this claim for transition metals?

Accepted Answer

The claim is mostly correct; atomic radius increases down a group, but the increase is less pronounced for transition metals due to d-orbital electron shielding.

Question 11

Which of the following best explains why the atomic radius of transition metals does not decrease as much as expected across a period?

Accepted Answer

The addition of electrons to the d subshell increases electron-electron repulsion, offsetting the increased nuclear charge.

Question 12

Which of the following is the most significant factor in determining the density of a transition metal?

Accepted Answer

Atomic mass and how closely atoms are packed.

Question 13

If you compare the atomic radius of Mn and Fe, which would you expect to be smaller and why?

Accepted Answer

Fe, because it has a higher atomic number and greater effective nuclear charge.

Question 14

Which of the following transition metals would you expect to have nearly the same atomic radius as its neighbor in the same period?

Accepted Answer

Fe and Co

Question 15

Which of the following statements about the density of transition metals is correct?

Accepted Answer

Density increases more significantly down a group than across a period.

Question 16

Which of the following is NOT a reason for the nearly constant atomic radius of transition metals across a period?

Accepted Answer

Transition metals have a variable number of protons.

Question 17

Which of the following elements is most likely to have the largest atomic radius in its period?

Accepted Answer

Na

Question 18

A transition metal has a high atomic mass but a relatively small atomic radius. What property does this combination most directly affect?

Accepted Answer

Its density.

Question 19

Which of the following best describes the effect of d-orbital electron addition on atomic radius in transition metals?

Accepted Answer

It causes the atomic radius to remain nearly constant across the period.

Question 20

Which of the following is the correct order of increasing density for the transition metals Zn, Fe, and Os?

Accepted Answer

Zn \u003c Fe \u003c Os

Atomic Radius and Density of Transition Metals

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