Q: A sodium lamp emits light with a wavelength of $$\lambda = 589 \ \mathrm{nm}. $$What is the frequency $$\nu of $$this light? (Speed of light $$c = 2.998 \times 10^8$ \ \mathrm{m/s})$$

$$5.09 \times 10$$^{14}$$ \ \mathrm{Hz}$$

Q: Calculate the energy of a photon with a frequency of $$\nu = 6.00 \times 10$$^{14}$$ \ \mathrm{Hz}. ($$Planck's constant $$h = 6.626 \times 10$$^{-34}$$ \ \mathrm{J \cdot s})$$

$$3.98 \times 10$$^{-19}$$ \ \mathrm{J}$$

Q: A baseball (mass $$0.145\ \mathrm{kg}) is $$thrown at $$40.0\ \mathrm{m/s}. $$What is the de Broglie wavelength of the baseball? ($$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J \cdot s})$$

$$1.14 \times 10$$^{-34}$$\ \mathrm{m}$$

Question 1

Which region of the electromagnetic spectrum has the highest energy per photon?

Accepted Answer

Gamma rays

Question 2

A sodium lamp emits light with a wavelength of $$\lambda = 589 \ \mathrm{nm}. $$What is the frequency $$
u of $$this light? (Speed of light $$c = 2.998 	imes 10^8$ \ \mathrm{m/s})$$

Accepted Answer

$$5.09 	imes 10$$^{14}$$ \ \mathrm{Hz}$$

Question 3

Which of the following statements best describes the Heisenberg Uncertainty Principle?

Accepted Answer

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

Question 4

Calculate the energy of a photon with a frequency of $$
u = 6.00 	imes 10$$^{14}$$ \ \mathrm{Hz}. ($$Planck's constant $$h = 6.626 	imes 10$$^{-34}$$ \ \mathrm{J \cdot s})$$

Accepted Answer

$$3.98 	imes 10$$^{-19}$$ \ \mathrm{J}$$

Question 5

Which of the following electron configurations represents a violation of the Pauli Exclusion Principle?

Accepted Answer

An orbital diagram with two electrons in the same orbital, both with $$m_s = +\frac{1}{2}$$

Question 6

Which of the following best explains why atomic radius decreases from left to right across a period?

Accepted Answer

Effective nuclear charge increases, pulling electrons closer to the nucleus.

Question 7

A hydrogen atom undergoes a transition from $$n_i = 4 to$$ $$n_f = 2. $$Using the Balmer-Rydberg equation $$\frac{1}{\lambda} = R_\infty \left[ \frac{1}{n_f^2$} - \frac{1}{n_i^2$} ight]$$, what is the wavelength of the emitted photon? ($$R_\infty = 1.097 	imes 10^7$ \ \mathrm{m}^{-1})$$

Accepted Answer

$$486 \ \mathrm{nm}$$

Question 8

Which quantum numbers are possible for the last electron added to a phosphorus atom ($$Z=15) in $$its ground state?

Accepted Answer

$$n=3,\ l=1,\ m_l=0,\ m_s=+\frac{1}{2}$$

Question 9

Which of the following ions is isoelectronic with neon ($$\mathrm{Ne}$$)?

Accepted Answer

$$\mathrm{Na}^+$$

Question 10

Which of the following statements about electron affinity is correct?

Accepted Answer

Electron affinity generally becomes more negative from left to right across a period.

Question 11

A baseball (mass $$0.145\ \mathrm{kg}) is $$thrown at $$40.0\ \mathrm{m/s}. $$What is the de Broglie wavelength of the baseball? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J \cdot s})$$

Accepted Answer

$$1.14 	imes 10$$^{-34}$$\ \mathrm{m}$$

Question 12

Which of the following best describes Hund’s Rule?

Accepted Answer

Electrons occupy degenerate orbitals singly before pairing.

Question 13

Which of the following elements has the highest first ionization energy?

Accepted Answer

$$\mathrm{Ne}$$

Question 14

Which of the following statements about s and p orbitals is correct?

Accepted Answer

An s orbital is spherical, while a p orbital is dumbbell-shaped.

Question 15

Which of the following best explains why the ionization energy of core electrons is much higher than that of valence electrons?

Accepted Answer

Core electrons are closer to the nucleus and experience a stronger attraction.

Question 16

Which of the following is the correct noble gas shorthand electron configuration for $$\mathrm{Ca}^{2+}$$?

Accepted Answer

$$[\mathrm{Ar}]$$

Question 17

Which of the following best describes the trend in effective nuclear charge ($$Z_{\mathrm{eff}}) $$across a period?

Accepted Answer

$$Z_{\mathrm{eff}}$$ increases from left to right across a period.

Question 18

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 19

Which of the following best explains why $$\mathrm{Cl}^-$$ and $$\mathrm{K}^+$$ have similar chemical properties?

Accepted Answer

They are isoelectronic and have the same number of electrons as $$\mathrm{Ar}.$$

Question 20

Which of the following best describes the octet rule as it applies to ion formation?

Accepted Answer

Atoms tend to gain or lose electrons to achieve a noble gas electron configuration.

Quantum-Mechanical Model of the Atom and Periodic Properties: Study Guide

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