Q: A photon of ultraviolet light has a wavelength of $$2.50 \times 10$$^{-7}$$ m. What is the energy of this photon? (Planck's constant h = 6.626$$ \times $$10^{-34} J$$·s, speed of light $$c = 3.00 \times 10^8$ m/s)

$$E = 7.95 \times 10$$^{-19}$$ J$

Q: According to the de Broglie hypothesis, what is the wavelength of an electron (mass $$9.11 \times 10$$^{-31}$$ kg) moving at 2.00$$ \times $$10^6 m/s$$?

$$\lambda = 3.63 \times 10$$^{-10}$$ m$

Question 1

Which equation correctly relates the speed of light ($$c$$), wavelength ($$\lambda$$), and frequency ($$
u) of $$electromagnetic radiation?

Accepted Answer

$$c = \lambda 
u$$

Question 2

A photon of ultraviolet light has a wavelength of $$2.50 	imes 10$$^{-7}$$ m. What is the energy of this photon? (Planck's constant h = 6.626$$ 	imes $$10^{-34} J$$·s, speed of light $$c = 3.00 	imes 10^8$ m/s)

Accepted Answer

$$E = 7.95 	imes 10$$^{-19}$$ J$

Question 3

Which statement best explains why the emission spectrum of hydrogen consists of discrete lines rather than a continuous spectrum?

Accepted Answer

Electrons in hydrogen atoms can only occupy specific energy levels, and transitions between these levels emit photons of specific energies.

Question 4

According to the de Broglie hypothesis, what is the wavelength of an electron (mass $$9.11 	imes 10$$^{-31}$$ kg) moving at 2.00$$ 	imes $$10^6 m/s$$?

Accepted Answer

$$\lambda = 3.63 	imes 10$$^{-10}$$ m$

Question 5

Which principle states that no two electrons in the same atom can have identical sets of quantum numbers?

Accepted Answer

Pauli Exclusion Principle

Question 6

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

Accepted Answer

10

Question 7

Which quantum number determines the shape of an orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 8

If an electron transitions from $$n=4 to$$ $$n=2 in a $$hydrogen atom, which equation gives the energy released? (Rydberg constant $$R_H = 1.097 	imes 10^7$ m$$^{-1}$$, h$ and c$ as usual)

Accepted Answer

$$\Delta E = -hcR_H \left( \frac{1}{2^2$} - \frac{1}{4^2$} \right)$$

Question 9

Which of the following is a correct electron configuration for chromium, considering its anomalous behavior?

Accepted Answer

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

Question 10

Which quantum number(s) are needed to uniquely specify an electron in an atom?

Accepted Answer

All four quantum numbers: $$n$$, $$l$$, $$m_l$$, $$m_s$$

Question 11

What is the shape of a $$p$$ orbital?

Accepted Answer

Two lobes with a node between them

Question 12

According to Hund’s Rule, how are electrons distributed in degenerate orbitals?

Accepted Answer

Electrons fill each orbital singly with parallel spins before pairing

Question 13

Which quantum number describes the three-dimensional orientation of an orbital?

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 14

What is the probability density map ($$\$$psi^2$$) used for in quantum mechanics?

Accepted Answer

To show the likelihood of finding an electron in a particular region of space

Question 15

Which of the following best describes the Heisenberg Uncertainty Principle?

Accepted Answer

The more precisely the momentum of a particle is known, the less precisely its position is known

Question 16

How many nodes does a $$3s$$ orbital possess?

Accepted Answer

2

Question 17

Which block of the periodic table corresponds to elements whose valence electrons occupy $$d$$ orbitals?

Accepted Answer

Transition metals (d-block)

Question 18

What is the electron configuration for neon (Ne)?

Accepted Answer

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

Question 19

Which of the following statements about the energy of orbitals in a hydrogen atom is correct?

Accepted Answer

All orbitals with the same principal quantum number ($$n) $$are degenerate (have the same energy)

Electronic Structure of Atoms and Quantum Mechanics

Study Guide - Practice Questions

Study Guide - Flashcards