Q: A photon of green light has a wavelength of $$520\ \mathrm{nm}. $$What is its frequency? (Speed of light $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$5.77 \times 10$$^{14}$$\ \mathrm{Hz}$$

Question 1

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

Accepted Answer

Wavelength and frequency are inversely proportional; as one increases, the other decreases.

Question 2

A photon of green light has a wavelength of $$520\ \mathrm{nm}. $$What is its frequency? (Speed of light $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$5.77 	imes 10$$^{14}$$\ \mathrm{Hz}$$

Question 3

Which region of the electromagnetic spectrum has the highest energy photons?

Accepted Answer

Gamma rays

Question 4

The energy of a photon is given by $$E = h
u. If $$the frequency of a photon is doubled, what happens to its energy?

Accepted Answer

The energy is doubled.

Question 5

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 6

How many electrons can occupy the $$3d$$ sublevel in an atom?

Accepted Answer

10

Question 7

Which of the following electron configurations represents a noble gas in its ground state?

Accepted Answer

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

Question 8

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 9

A sodium atom ($$Na) $$loses one electron to form $$Na^+. $$What is the electron configuration of $$Na^+$$?

Accepted Answer

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

Question 10

Which of the following is a correct condensed electron configuration for chlorine ($$Cl$$)?

Accepted Answer

$$[Ne]\ 3s^2$\ 3p^5$

Question 11

Which of the following best explains why transition metals often have multiple possible oxidation states?

Accepted Answer

They can lose s and d electrons from similar energy levels.

Question 12

Which of the following ions is isoelectronic with argon ($$Ar$$)?

Accepted Answer

$$S^{2-}$$

Question 13

Which rule states that electrons fill degenerate orbitals singly before pairing up?

Accepted Answer

Hund's Rule

Question 14

Which quantum number describes the orientation of an orbital in space?

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 15

Which of the following best describes the Heisenberg Uncertainty Principle?

Accepted Answer

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

Question 16

Which of the following transitions in a hydrogen atom would emit the highest energy photon?

Accepted Answer

$$n=4 to$$ $$n=1$$

Question 17

Which orbital type is described as having a spherical shape?

Accepted Answer

s orbital

Question 18

Which of the following elements has an electron configuration ending in $$4p^4$$?

Accepted Answer

Selenium (Se)

Question 19

A pulse of $$675\ \mathrm{nm}$$ laser light emits a total of $$55.0\ \mu J of $$energy. How many photons does this pulse contain? ($$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$1.87 	imes 10$$^{14}$$

Question 20

Which of the following best explains why the emission spectrum of hydrogen consists of discrete lines?

Accepted Answer

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

Quantum Mechanics and Electronic Structure: Study Notes for General Chemistry

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