Question 1

Which of the following best explains why $$d$$ subshell orbitals are more stable when they are half-filled or fully-filled?

Accepted Answer

Because half-filled and fully-filled $$d$$ orbitals have lower energy due to symmetrical distribution and exchange energy.

Question 2

What is the condensed electron configuration for silver (Ag), based on the exceptions discussed?

Accepted Answer

$$[Kr] \ 5s^1$ \ 4d$$^{10}$$

Question 3

Which element's electron configuration is an exception to the expected order due to increased stability of a half-filled $$d$$ subshell?

Accepted Answer

Chromium ($$Cr)$$

Question 4

Given the atomic number $$Z = 42$$, what is the correct condensed electron configuration for molybdenum (Mo), considering exceptions?

Accepted Answer

$$[Kr] \ 5s^1$ \ 4d^5$

Question 5

Which of the following is the correct condensed electron configuration for gold (Au)?

Accepted Answer

$$[Xe] \ 4f$$^{14}$$ \ 5d$$^{10}$$ \ 6s^1$

Question 6

Why does copper ($$Cu) $$have the electron configuration $$[Ar] \ 4s^1$ \ 3d$$^{10}$$ instead of $$[Ar] \ $$4s^2$$ \ $$3d^9$$?

Accepted Answer

Because a fully-filled $$3d$$ subshell is more stable than a partially-filled one.

Question 7

Which of the following statements is true regarding the electron configurations of palladium (Pd) and silver (Ag)?

Accepted Answer

Ag has 2 more $$d$$ electrons and 1 less $$s$$ electron than Pd.

Question 8

Which of the following best describes the reason for the observed exceptions in electron configurations for transition metals?

Accepted Answer

The increased stability associated with half-filled or fully-filled $$d$$ subshells.

Question 9

Which of the following is the correct electron configuration for chromium ($$Cr$$)?

Accepted Answer

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

Question 10

A scientist is analyzing the electron configuration of an unknown element and finds it to be $$[Kr] \ 5s^1$ \ 4d$$^{10}$$. Which element is this most likely to be?

Accepted Answer

Silver ($$Ag)$$

Question 11

Which of the following is a real-world consequence of the stability of half-filled and fully-filled $$d$$ subshells in transition metals?

Accepted Answer

Transition metals often exhibit multiple oxidation states.

Question 12

Which of the following electron configurations represents an exception due to the stability of a fully-filled $$d$$ subshell?

Accepted Answer

$$[Ar] \ 4s^1$ \ 3d$$^{10}$$

Question 13

If an atom has the electron configuration $$[Kr] \ 5s^2$ \ 4d^8$, which element is it?

Accepted Answer

Rhodium ($$Rh)$$

Question 14

Which of the following best describes the condensed electron configuration for molybdenum ($$Mo) $$based on the observed exceptions?

Accepted Answer

$$[Kr] \ 5s^1$ \ 4d^5$

Question 15

Which of the following is NOT a reason for the observed exceptions in electron configurations of transition metals?

Accepted Answer

The higher energy of $$s$$ orbitals compared to $$d$$ orbitals.

Electron Configuration Exceptions and Stability

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