Q: What is the wavelength ($\lambda$) of an electron (mass $9.11 \times 10^{-31}$ kg) moving at $2.00 \times 10^6$ m/s? ($h = 6.626 \times 10^{-34}$ J·s)

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

Q: A transition from $n=4$ to $n=2$ in a hydrogen atom emits a photon. Which formula gives the energy of this photon?

$\Delta E = -2.18 \times 10^{-18} \left( \frac{1}{2^2} - \frac{1}{4^2} \right)$ J

Question 1

Which of the following statements best describes the relationship between wavelength ($\lambda$) and frequency ($
u$) for electromagnetic radiation traveling at the speed of light ($c$)?

Accepted Answer

$c = \lambda 
u$

Question 2

A metal surface requires a minimum energy of $4.0 	imes 10^{-19}$ J to emit electrons via the photoelectric effect. What is the minimum frequency of light ($
u$) that will cause electron emission? ($h = 6.626 	imes 10^{-34}$ J·s)

Accepted Answer

$
u = 6.04 	imes 10^{14}$ Hz

Question 3

Which phenomenon could NOT be explained by the classical wave theory of light, but was explained by the quantum theory?

Accepted Answer

The photoelectric effect

Question 4

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

Question 5

Which equation gives the energy of a photon in terms of Planck's constant ($h$) and frequency ($
u$)?

Accepted Answer

$E = h 
u$

Question 6

What is the principal quantum number ($n$) primarily responsible for in an atom?

Accepted Answer

The energy level and size of the orbital

Question 7

How many possible values of the magnetic quantum number ($m_l$) are there for a $d$ subshell?

Accepted Answer

5

Question 8

Which of the following is a correct set of quantum numbers for an electron in a 4p orbital?

Accepted Answer

$n=4, \ l=1, \ m_l=0$

Question 9

Which statement about the Pauli Exclusion Principle is correct?

Accepted Answer

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

Question 10

Which of the following electron configurations represents the ground state of selenium (Se, atomic number 34)?

Accepted Answer

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

Question 11

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($l$)

Question 12

What is the wavelength ($\lambda$) of an electron (mass $9.11 	imes 10^{-31}$ kg) moving at $2.00 	imes 10^6$ m/s? ($h = 6.626 	imes 10^{-34}$ J·s)

Accepted Answer

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

Question 13

Which of the following best describes Hund’s Rule?

Accepted Answer

Electrons fill degenerate orbitals singly before pairing up.

Question 14

Which of the following is a limitation of the Bohr model?

Accepted Answer

It only accurately describes hydrogen-like atoms.

Question 15

How many orbitals are present in the $n=3$ shell of a hydrogen atom?

Accepted Answer

9

Question 16

Which of the following statements about $s$ orbitals is true?

Accepted Answer

$s$ orbitals are spherical and have $l=0$.

Question 17

A transition from $n=4$ to $n=2$ in a hydrogen atom emits a photon. Which formula gives the energy of this photon?

Accepted Answer

$\Delta E = -2.18 	imes 10^{-18} \left( \frac{1}{2^2} - \frac{1}{4^2} ight)$ J

Question 18

Which quantum number is associated with the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($m_l$)

Question 19

Which of the following best describes the Heisenberg Uncertainty Principle?

Accepted Answer

It is impossible to know both the exact position and momentum of a particle simultaneously.

Chapter 6: Electronic Structure of Atoms – Study Notes

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