Question 1

Which quantum number is directly associated with the 'spin' of an electron, and what are its possible values?

Accepted Answer

The spin quantum number ($$m_s$$), with possible values of $$+\frac{1}{2}$$ and $$-\frac{1}{2}$$

Question 2

According to the Pauli Exclusion Principle, what is the maximum number of electrons that can occupy a single orbital?

Accepted Answer

$$2$$

Question 3

Which of the following electron configurations correctly represents the condensed electron configuration for phosphorus (P)?

Accepted Answer

$$[Ne]\ 3s^2$\ 3p^3$

Question 4

If an atom has the electron configuration $$1s^2$$\ $$2s^2$$\ $$2p^6$$\ $$3s^2$$\ $$3p^1$$, which element is it?

Accepted Answer

Aluminum (Al)

Question 5

How many different $$d-$$type orbitals exist in a given energy level?

Accepted Answer

$$5$$

Question 6

Which statement best explains why the $$2p$$ orbitals are considered 'degenerate'?

Accepted Answer

They have the same energy because they are all part of the same subshell.

Question 7

What is the condensed electron configuration for magnesium (Mg)?

Accepted Answer

$$[Ne]\ 3s^2$

Question 8

Which of the following is a correct electron configuration for nitrogen (N)?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^3$$

Question 9

Why do electrons fill the $$2p$$ orbital after the $$2s$$ orbital?

Accepted Answer

Because the $$2s$$ orbital is lower in energy and must be filled first according to the Aufbau principle.

Question 10

Which rule states that electrons will fill degenerate orbitals singly before pairing up?

Accepted Answer

Hund's Rule

Question 11

What is the electron configuration for sodium (Na)?

Accepted Answer

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

Question 12

Which of the following best describes the condensed electron configuration notation?

Accepted Answer

It uses the symbol of the nearest noble gas to represent filled inner shells.

Question 13

How many electrons can occupy all the $$p$$ orbitals in a given energy level?

Accepted Answer

$$6$$

Question 14

Which element has the electron configuration $$[Ne]\ 3s^2$\ 3p^4$?

Accepted Answer

Sulfur (S)

Question 15

If you add one electron to the $$2p$$ orbital of carbon ($$1s^2$$\ $$2s^2$$\ $$2p^2$$), what element do you get?

Accepted Answer

Nitrogen (N)

Question 16

Which of the following statements about orbital energies is correct?

Accepted Answer

The $$2p$$ orbital is higher in energy than the $$2s$$ orbital.

Question 17

How many electrons can occupy all the $$d$$ orbitals in a given energy level?

Accepted Answer

$$10$$

Question 18

Which principle explains why no two electrons in an atom can have the same set of four quantum numbers?

Accepted Answer

Pauli Exclusion Principle

Question 19

What is the electron configuration for oxygen (O)?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^4$$

Question 20

Which of the following elements has a full $$2p$$ subshell in its ground state electron configuration?

Accepted Answer

Neon (Ne)

Electron Spin, Electron Configurations, and Orbital Energies

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