Q: A photon of light has a wavelength of $$500\ \mathrm{nm}. $$What is its energy in joules? (Use $$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s}$$ and $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

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

Q: Calculate the wavelength (in meters) of an electron moving at $$2.00 \times 10^6$\ \mathrm{m/s}. ($$Mass of electron $$= 9.11 \times 10$$^{-31}$$\ \mathrm{kg}$$, $$h = 6.626 \times 10$$^{-34}$$\ \mathrm{J\cdot s})$$

$$3.63 \times 10$$^{-10}$$\ \mathrm{m}$$

Question 1

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

Accepted Answer

They are inversely proportional; as wavelength increases, frequency decreases.

Question 2

A photon of light has a wavelength of $$500\ \mathrm{nm}. $$What is its energy in joules? (Use $$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s}$$ and $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

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

Question 3

Which phenomenon provides evidence for the wave nature of light?

Accepted Answer

Diffraction and interference

Question 4

Which transition in a hydrogen atom would release the most energy as a photon?

Accepted Answer

$$n = 2 \rightarrow n = 1$$

Question 5

Which of the following statements about the photoelectric effect is correct?

Accepted Answer

Electrons are ejected only if the light's frequency is above a certain threshold, regardless of intensity.

Question 6

Calculate the wavelength (in meters) of an electron moving at $$2.00 	imes 10^6$\ \mathrm{m/s}. ($$Mass of electron $$= 9.11 	imes 10$$^{-31}$$\ \mathrm{kg}$$, $$h = 6.626 	imes 10$$^{-34}$$\ \mathrm{J\cdot s})$$

Accepted Answer

$$3.63 	imes 10$$^{-10}$$\ \mathrm{m}$$

Question 7

Which quantum number determines the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 8

How many possible values of $$m_l$$ are there for a $$d$$ orbital?

Accepted Answer

5

Question 9

Which set of quantum numbers is NOT allowed?

Accepted Answer

$$n = 4,\ l = 3,\ m_l = 4$$

Question 10

Which element has the ground-state electron configuration $$[Ar]4s^23$d^{10}4p^5$?

Accepted Answer

Bromine

Question 11

Which of the following ions is isoelectronic with argon?

Accepted Answer

Cl$$^-$$

Question 12

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

Accepted Answer

The effective nuclear charge increases, pulling electrons closer.

Question 13

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

Accepted Answer

Sulfur

Question 14

Which of the following best describes Hund's Rule?

Accepted Answer

Electrons occupy degenerate orbitals singly before pairing.

Question 15

Which of the following ions is the smallest in size?

Accepted Answer

Ca$$^{2+}$$

Question 16

Which of the following best describes a paramagnetic atom?

Accepted Answer

An atom with at least one unpaired electron

Question 17

Which of the following is the correct order of increasing first ionization energy?

Accepted Answer

Sr \u003c Mg \u003c Be

Question 18

Which equation correctly relates the energy of a photon to its frequency?

Accepted Answer

$$E = h
u$$

Question 19

Which of the following best describes the Pauli Exclusion Principle?

Accepted Answer

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

Question 20

Which of the following best explains why the second ionization energy of sodium is much higher than the first?

Accepted Answer

The second electron is removed from a noble gas core, which is much more stable.

Quantum Mechanical Model, Electron Configuration, and Periodic Trends: Study Notes for General Chemistry

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