Question 1

Which of the following statements best explains why each element has a unique line spectrum?

Accepted Answer

Each element has a unique arrangement of electrons, resulting in specific allowed energy transitions.

Question 2

According to the Bohr model, what happens when an electron in a hydrogen atom transitions from $$n=3 to$$ $$n=2$$?

Accepted Answer

A photon is emitted and the atom moves to a lower energy state.

Question 3

Which quantum number determines the shape of an orbital?

Accepted Answer

Angular momentum quantum number, $$l$$

Question 4

How many possible values of $$m_l$$ are there for a $$d$$ orbital?

Accepted Answer

5

Question 5

Which of the following electron configurations represents a transition metal in its ground state?

Accepted Answer

$$1s^2$$ $$2s^2$$ $$2p^6$$ $$3s^2$$ $$3p^6$$ $$4s^2$$ $$3d^5$$

Question 6

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

Accepted Answer

Pauli Exclusion Principle

Question 7

What is the maximum number of electrons that can occupy the $$n=3$$ shell?

Accepted Answer

18

Question 8

Which of the following best describes the difference between core and valence electrons?

Accepted Answer

Valence electrons are involved in chemical bonding, while core electrons are not.

Question 9

Which of the following electron configurations is correct for the ground state of sodium ($$Na$$)?

Accepted Answer

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

Question 10

A hospital uses sodium vapor lamps for lighting. The yellow color observed is due to:

Accepted Answer

Electrons in sodium atoms transitioning between specific energy levels, emitting photons of characteristic energy.

Question 11

Which quantum number(s) must be different for two electrons in the same orbital?

Accepted Answer

Only $$m_s$$

Question 12

Which of the following is the correct condensed electron configuration for bromine ($$Br$$, atomic number 35)?

Accepted Answer

$$[Ar] 4s^2$ 3d$$^{10}$$ 4p^5$

Question 13

Which of the following best describes Hund’s Rule?

Accepted Answer

Electrons occupy degenerate orbitals singly before pairing.

Question 14

Which of the following elements is filling the $$4f$$ sublevel in its ground state electron configuration?

Accepted Answer

Cerium ($$Ce)$$

Question 15

A certain atom has the following set of quantum numbers for one of its electrons: $$n=3$$, $$l=2$$, $$m_l=0$$, $$m_s=+\frac{1}{2}. $$Which type of orbital does this electron occupy?

Accepted Answer

$$3d$$

Question 16

Which of the following explains why the $$4s$$ orbital fills before the $$3d$$ orbital in potassium?

Accepted Answer

The $$4s$$ orbital is lower in energy than the $$3d$$ orbital.

Question 17

Which of the following is a possible set of quantum numbers for the last electron added to a phosphorus atom ($$Z=15$$)?

Accepted Answer

$$n=3$$, $$l=1$$, $$m_l=1$$, $$m_s=+\frac{1}{2}$$

Question 18

Which of the following best describes the difference between a shell and a subshell?

Accepted Answer

A shell is defined by $$n$$ and contains all orbitals with that $$n$$, while a subshell is defined by $$l$$ and contains orbitals of a specific shape within a shell.

Electronic Structure of Atoms: Quantum Numbers, Orbitals, and Electron Configurations

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