Subshells and Electronic Configuration

Question 1

What is the maximum number of electrons in the S subshell?

Answer 1

2 electrons

Question 2

How many orbitals are present in the P subshell?

Answer 2

3 orbitals

Question 3

What is the total number of electrons that can occupy the D subshell?

Answer 3

10 electrons

Question 4

Fill in the blank: The F subshell can hold a maximum of _______ electrons.

Answer 4

14 electrons

Question 5

How many orbitals does the F subshell contain?

Answer 5

7 orbitals

Question 6

What is the predicted electron configuration for Chromium (Cr)?

Answer 6

1s2, 2s2, 2p6, 3s2, 3p6, 3d4, 4s2

Question 7

What is the actual electron configuration for Chromium (Cr)?

Answer 7

1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1

Question 8

What is the predicted electron configuration for Copper (Cu)?

Answer 8

1s2, 2s2, 2p6, 3s2, 3p6, 3d9, 4s2

Question 9

What is the actual electron configuration for Copper (Cu)?

Answer 9

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1

Question 10

True or False: The stability of an electron configuration increases when the 3d subshell is half-full or completely full.

Answer 10

True

Question 11

Why is having one electron in each orbital more stable?

Answer 11

It maximizes exchange energy and minimizes repulsion.

Question 12

What is the Aufbau principle?

Answer 12

Fill from the lowest energy level first.

Question 13

What does the Pauli exclusion principle state?

Answer 13

Only a maximum of two electrons can occupy an orbital.

Question 14

What is Hund’s rule?

Answer 14

Fill one electron per orbital first before pairing.