Q: Calculate the energy (in J) of a photon emitted when an electron in a hydrogen atom relaxes from $$n=6 to$$ $$n=2. $$Use $$B = -2.18 \times 10$$^{-18}$$\ \text{J}.$$

$$4.85 \times 10$$^{-19}$$\ \text{J}$$

Question 1

Which quantum number determines the overall size and energy of an atomic orbital?

Accepted Answer

The principal quantum number, $$n$$

Question 2

What is the maximum number of electrons that can occupy the 3d subshell?

Accepted Answer

10

Question 3

Which of the following sets of quantum numbers is NOT allowed for an electron in an atom?

Accepted Answer

$$n=2,\ l=2,\ m_l=0,\ m_s=+\frac{1}{2}$$

Question 4

According to the Pauli Exclusion Principle, which statement is correct?

Accepted Answer

No two electrons in an atom can have the same set of four quantum numbers.

Question 5

What is the electron configuration for the element Scandium (Sc, atomic number 21)?

Accepted Answer

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

Question 6

Which of the following best describes the shape of a p orbital?

Accepted Answer

Dumbbell-shaped

Question 7

How many possible values of $$m_l$$ are there for an electron in a 4d orbital?

Accepted Answer

5

Question 8

Which principle explains why electrons fill all orbitals singly before pairing up in a subshell?

Accepted Answer

Hund's Rule

Question 9

Calculate the energy (in J) of a photon emitted when an electron in a hydrogen atom relaxes from $$n=6 to$$ $$n=2. $$Use $$B = -2.18 	imes 10$$^{-18}$$\ 	ext{J}.$$

Accepted Answer

$$4.85 	imes 10$$^{-19}$$\ 	ext{J}$$

Question 10

Which quantum number is responsible for distinguishing between the different orientations of orbitals within a subshell?

Accepted Answer

Magnetic quantum number, $$m_l$$

Question 11

Which of the following statements about the Heisenberg Uncertainty Principle is correct?

Accepted Answer

It states that it is impossible to know both the exact position and momentum of an electron simultaneously.

Question 12

Which of the following electron configurations violates the Aufbau Principle?

Accepted Answer

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

Question 13

Which set of quantum numbers could represent the last electron added to an oxygen atom ($$Z=8$$)?

Accepted Answer

$$n=2,\ l=1,\ m_l=0,\ m_s=-\frac{1}{2}$$

Question 14

Which of the following best describes the difference between the Bohr model and the quantum mechanical model of the atom?

Accepted Answer

The Bohr model describes electrons in fixed orbits, while the quantum mechanical model describes electrons as existing in orbitals defined by probability distributions.

Question 15

How many electrons can be held in all orbitals with $$n=3 in a $$single atom?

Accepted Answer

18

Question 16

Which of the following is the correct order of filling for the first four subshells according to the Aufbau Principle?

Accepted Answer

$$1s \rightarrow 2s \rightarrow 2p \rightarrow 3s$$

Question 17

A certain orbital is described by the quantum numbers $$n=4$$, $$l=2$$, $$m_l=0. $$What type of orbital is this?

Accepted Answer

4d orbital

Question 18

Which of the following statements about atomic orbitals is true?

Accepted Answer

An atomic orbital is a region in space where there is a high probability of finding an electron.

Question 19

If $$n=3$$, what are the possible values for the angular momentum quantum number $$l$$?

Accepted Answer

0, 1, 2

Quantum Mechanics, Electron Configurations, and Periodic Trends: Study Notes

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