Q: A photon of light has a frequency of $$6.0 \times 10$$^{14}$$\ \mathrm{Hz}. $$What is its wavelength in meters? (Speed of light $$c = 3.0 \times 10^8$\ \mathrm{m/s})$$

$$2.0 \times 10$$^{-7}$$\ \mathrm{m}$$

Q: A sodium atom emits light at a wavelength of $$589\ \mathrm{nm}. $$What is the energy of one photon of this light? ($$h = 6.63 \times 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 \times 10^8$\ \mathrm{m/s})$$

$$3.37 \times 10$$^{-19}$$\ \mathrm{J}$$

Question 1

Which of the following statements best describes the relationship between the energy and wavelength of electromagnetic radiation?

Accepted Answer

Energy increases as wavelength decreases.

Question 2

A photon of light has a frequency of $$6.0 	imes 10$$^{14}$$\ \mathrm{Hz}. $$What is its wavelength in meters? (Speed of light $$c = 3.0 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$2.0 	imes 10$$^{-7}$$\ \mathrm{m}$$

Question 3

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

Accepted Answer

Gamma rays

Question 4

According to the Bohr model, what happens when an electron in a hydrogen atom absorbs energy?

Accepted Answer

It moves to a higher energy orbit.

Question 5

Which of the following quantum numbers describes the shape of an atomic orbital?

Accepted Answer

Angular momentum quantum number ($$l)$$

Question 6

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

Accepted Answer

6

Question 7

Which electron configuration represents the ground state of oxygen ($$Z=8$$)?

Accepted Answer

$$1s^2$$\ $$2s^2$$\ $$2p^4$$

Question 8

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

Accepted Answer

Fluorine (F)

Question 9

Which of the following is a correct statement about electron affinity?

Accepted Answer

Electron affinity is the energy change when an atom gains an electron.

Question 10

Which of the following electron configurations is an exception to the expected order due to increased stability of half-filled subshells?

Accepted Answer

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

Question 11

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

Accepted Answer

Magnetic quantum number ($$m_l)$$

Question 12

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

Accepted Answer

The nuclear charge increases, pulling electrons closer.

Question 13

Which of the following is the correct order of increasing energy for the electromagnetic spectrum?

Accepted Answer

Radio waves \u003c Infrared \u003c Visible \u003c Ultraviolet \u003c Gamma rays

Question 14

A sodium atom emits light at a wavelength of $$589\ \mathrm{nm}. $$What is the energy of one photon of this light? ($$h = 6.63 	imes 10$$^{-34}$$\ \mathrm{J\cdot s}$$, $$c = 3.00 	imes 10^8$\ \mathrm{m/s})$$

Accepted Answer

$$3.37 	imes 10$$^{-19}$$\ \mathrm{J}$$

Question 15

Which of the following statements about the Pauli Exclusion Principle is correct?

Accepted Answer

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

Question 16

Which of the following elements has the electron configuration $$[Ne]\ 3s^2$\ 3p^5$?

Accepted Answer

Chlorine (Cl)

Question 17

Which of the following best describes Hund's Rule?

Accepted Answer

Electrons occupy degenerate orbitals singly before pairing.

Question 18

Which of the following ions has the same electron configuration as neon ($$Ne$$)?

Accepted Answer

$$Na^+$$

Question 19

Which of the following is the correct electron configuration for $$Cr ($$Chromium, $$Z=24$$), considering the observed exception?

Accepted Answer

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

Question 20

Which of the following best explains why noble gases are chemically unreactive?

Accepted Answer

They have completely filled valence shells.

Electrons in Atoms and the Periodic Table: Study Notes

Study Guide - Practice Questions

Study Guide - Flashcards