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Chemistry Chapter 3 Review

Total questions: 71

Worksheet time: 36mins

Name
Class
Date
1.

Use each of the terms below just once to complete the passage: amplitude, energy, frequency, hertz, light, wave, wavelength, speed. Electromagnetic radiation is a kind of (1) ________ that behaves like a(n) ________ as it travels through space. Choose the best term for blank (1).

a)

energy

b)

light

c)

wave

d)

speed

2.

Use each of the terms below just once to complete the passage: amplitude, energy, frequency, hertz, light, wave, wavelength, speed. Electromagnetic radiation is a kind of energy that behaves like a(n) (2) ________ as it travels through space. Choose the best term for blank (2).

a)

wave

b)

energy

c)

wavelength

d)

frequency

3.

Use each of the terms below just once to complete the passage: amplitude, energy, frequency, hertz, light, wave, wavelength, speed. (3) ________ is one type of electromagnetic radiation. Choose the best term for blank (3).

a)

light

b)

amplitude

c)

hertz

d)

speed

4.

Use each of the terms below just once to complete the passage: amplitude, energy, frequency, hertz, light, wave, wavelength, speed. All waves can be characterized by their wavelength, amplitude, frequency, and (4) ________. Choose the best term for blank (4).

a)

speed

b)

hertz

c)

energy

d)

wavelength

5.

Use each of the terms below just once to complete the passage: amplitude, energy, frequency, hertz, light, wave, wavelength, speed. The shortest distance between equivalent points on a continuous wave is called a(n) (5) ________. Choose the best term for blank (5).

a)

wavelength

b)

amplitude

c)

frequency

d)

hertz

6.

Use each of the terms below just once to complete the passage: amplitude, energy, frequency, hertz, light, wave, wavelength, speed. The height of a wave from the origin to a crest or from the origin to a trough is the (6) ________. Choose the best term for blank (6).

a)

amplitude

b)

wavelength

c)

speed

d)

light

7.

Use each of the terms below just once to complete the passage: amplitude, energy, frequency, hertz, light, wave, wavelength, speed. (7) ________ is the number of waves that pass a given point in one second. Choose the best term for blank (7).

a)

frequency

b)

speed

c)

amplitude

d)

energy

8.

Use each of the terms below just once to complete the passage: amplitude, energy, frequency, hertz, light, wave, wavelength, speed. The SI unit for frequency is the (8) ________, which is equivalent to one wave per second. Choose the best term for blank (8).

a)

hertz

b)

wavelength

c)

light

d)

energy

9.

Use the figure of a sinusoidal wave labeled A, B, C, and D relative to an origin line to answer: Which letter(s) represent the amplitude?

a)

A

b)

B

c)

C

d)

D

10.

A(n) _____ is the minimum amount of energy that can be lost or gained by an atom.

a)

valence electron

b)

electron

c)

quantum

d)

Planck's constant

11.

According to Planck's theory, for a given frequency, ν\nu , matter can emit or absorb energy only in

a)

units of hertz.

b)

whole-number multiples of hνh\nu .

c)

entire wavelengths.

d)

multiples of 12hν\tfrac12 h\nu , 14hν\tfrac14 h\nu , and so on.

12.

The _____ is the phenomenon in which electrons are emitted from a metal's surface when light of a certain frequency shines on it.

a)

quantum

b)

Planck concept

c)

photon effect

d)

photoelectric effect

13.

Which equation would you use to calculate the energy of a photon?

a)

Ephoton=hν×E_{\text{photon}} = h\nu \times Planck's constant

b)

Ephoton=hνE_{\text{photon}} = h\nu

c)

Ephoton=12hνE_{\text{photon}} = \tfrac12 h\nu

d)

c=λνc = \lambda\nu

14.

Like the visible spectrum, an atomic emission spectrum is a continuous range of colors.

a)

True

b)

False

15.

Each element has a unique atomic emission spectrum.

a)

True

b)

False

16.

A flame test can be used to identify the presence of certain elements in a compound.

a)

True

b)

False

17.

The fact that only certain colors appear in an element's atomic emission spectrum indicates that only certain frequencies of light are emitted.

a)

True

b)

False

18.

Atomic emission spectra can be explained by the wave model of light.

a)

True

b)

False

19.

The neon atoms in a neon sign emit their characteristic color of light as they absorb energy.

a)

True

b)

False

20.

When an atom emits light, photons having certain specific energies are being emitted.

a)

True

b)

False

21.

Use each of the terms below to complete the statement: atomic emission spectrum; electron; frequencies; ground state; higher; energy levels; lower. The lowest allowable energy state of an atom is called its ______.

a)

ground state

b)

higher

c)

lower

d)

electron

22.

Use each of the terms below to complete the statement: atomic emission spectrum; electron; frequencies; ground state; higher; energy levels; lower. Bohr’s model of the atom predicted the ______ of the lines in hydrogen’s atomic emission spectrum.

a)

frequencies

b)

energy levels

c)

ground state

d)

electron

23.

Use each of the terms below to complete the statement: atomic emission spectrum; electron; frequencies; ground state; higher; energy levels; lower. According to Bohr’s atomic model, the smaller an electron’s orbit, the ______ the atom’s energy level.

a)

lower

b)

higher

c)

ground state

d)

electron

24.

Use each of the terms below to complete the statement: atomic emission spectrum; electron; frequencies; ground state; higher; energy levels; lower. According to Bohr’s atomic model, the larger an electron’s orbit, the ______ the atom’s energy level.

a)

higher

b)

lower

c)

ground state

d)

atomic emission spectrum

25.

Use each of the terms below to complete the statement: atomic emission spectrum; electron; frequencies; ground state; higher; energy levels; lower. Bohr proposed that when energy is added to a hydrogen atom, its ______ moves to a higher-energy orbit.

a)

electron

b)

ground state

c)

frequencies

d)

energy levels

26.

Use each of the terms below to complete the statement: atomic emission spectrum; electron; frequencies; ground state; higher; energy levels; lower. According to Bohr’s atomic model, the hydrogen atom emits a photon corresponding to the difference between the ______ associated with the two orbits it transitions between.

a)

energy levels

b)

frequencies

c)

ground state

d)

atomic emission spectrum

27.

Use each of the terms below to complete the statement: atomic emission spectrum; electron; frequencies; ground state; higher; energy levels; lower. Bohr’s atomic model failed to explain the ______ of elements other than hydrogen.

a)

atomic emission spectrum

b)

ground state

c)

electron

d)

energy levels

28.

If you looked closely, could you see the wavelength of a fast-moving car?

a)

No; its de Broglie wavelength is far too small to see.

b)

Yes; macroscopic objects have large wavelengths that are visible.

c)

No; cars do not have wavelengths at all.

29.

Using de Broglie’s equation, λ=hmv\lambda=\frac{h}{mv} , which would have the larger wavelength: a slow-moving proton or a fast-moving golf ball?

a)

A slow-moving proton

b)

A fast-moving golf ball

c)

Both would have the same wavelength

30.

Match each item in Column A with the correct item in Column B. Column A: - The modern model of the atom that treats electrons as waves - States that it is impossible to know both the velocity and the position of a particle at the same time - A three-dimensional region around the nucleus representing the probability of finding an electron - Originally applied to the hydrogen atom, it led to the quantum mechanical model of the atom Column B: - Heisenberg uncertainty principle - Schrödinger wave equation - quantum mechanical model of the atom - atomic orbital

a)

The modern model of the atom that treats electrons as waves

1.

quantum mechanical model of the atom

b)

States that it is impossible to know both the velocity and the position of a particle at the same time

2.

Heisenberg uncertainty principle

c)

A three-dimensional region around the nucleus representing the probability of finding an electron

3.

atomic orbital

d)

Originally applied to the hydrogen atom, it led to the quantum mechanical model of the atom

4.

Schrödinger wave equation

31.

How do the Bohr model and the quantum mechanical model of the atom differ in how they describe electrons?

a)

Bohr: electrons move in fixed circular orbits; quantum mechanical: electrons are described by probability distributions (orbitals) with wave behavior, not fixed paths

b)

Both models place electrons at exact positions and velocities around the nucleus at all times

c)

Bohr: electrons behave as waves in standing-wave orbitals; quantum mechanical: electrons are particles moving in fixed paths

d)

Bohr: electrons are located inside the nucleus; quantum mechanical: electrons orbit within the nucleus

32.

Atomic orbitals (do, do not) have an exactly defined size.

a)

do

b)

do not

33.

Each orbital may contain at most (two, four) electrons.

a)

two

b)

four

34.

All s orbitals are (spherically shaped, dumbbell shaped).

a)

spherically shaped

b)

dumbbell shaped

35.

A principal energy has ( nn , n2n^2 ) energy sublevels.

a)

nn

b)

n2n^2

36.

The maximum number of (electrons, orbitals) related to each principal energy level equals 2n22n^2 .

a)

electrons

b)

orbitals

37.

There are (three, five) equal energy p orbitals.

a)

three

b)

five

38.

Hydrogen’s principal energy level 2 consists of (2s and 3s, 2s and 2p) orbitals.

a)

2s and 3s

b)

2s and 2p

39.

Hydrogen’s principal energy level 3 consists of (nine, three) orbitals.

a)

nine

b)

three

40.

Use the word bank (Aufbau principle; electron configuration; ground-state electron configuration; Hund's rule; lowest; Pauli exclusion principle; spins; stable) to complete the statement: The arrangement of electrons in an atom is called the atom's _____.

a)

electron configuration

b)

spins

c)

ground-state electron configuration

d)

Hund's rule

41.

Use the word bank (Aufbau principle; electron configuration; ground-state electron configuration; Hund's rule; lowest; Pauli exclusion principle; spins; stable) to complete the statement: Electrons in an atom tend to assume the arrangement that gives the atom the _____ possible energy.

a)

lowest

b)

stable

c)

spins

d)

Aufbau principle

42.

Use the word bank (Aufbau principle; electron configuration; ground-state electron configuration; Hund's rule; lowest; Pauli exclusion principle; spins; stable) to complete the statement: This arrangement of electrons is the most _____ arrangement.

a)

stable

b)

lowest

c)

spins

d)

Hund's rule

43.

Use the word bank (Aufbau principle; electron configuration; ground-state electron configuration; Hund's rule; lowest; Pauli exclusion principle; spins; stable) to complete the statement: This arrangement is called the atom's _____.

a)

ground-state electron configuration

b)

electron configuration

c)

Pauli exclusion principle

d)

Aufbau principle

44.

Use the word bank (Aufbau principle; electron configuration; ground-state electron configuration; Hund's rule; lowest; Pauli exclusion principle; spins; stable) to complete the statement: The _____ states that each electron occupies the lowest energy orbital available.

a)

Aufbau principle

b)

Pauli exclusion principle

c)

Hund's rule

d)

electron configuration

45.

Use the word bank (Aufbau principle; electron configuration; ground-state electron configuration; Hund's rule; lowest; Pauli exclusion principle; spins; stable) to complete the statement: The _____ states that a maximum of two electrons may occupy a single atomic orbital, but only if the electrons have opposite _____.

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau principle

d)

ground-state electron configuration

46.

Use the word bank (Aufbau principle; electron configuration; ground-state electron configuration; Hund's rule; lowest; Pauli exclusion principle; spins; stable) to complete the statement: A maximum of two electrons may occupy a single atomic orbital only if they have opposite _____.

a)

spins

b)

lowest

c)

stable

d)

electron configuration

47.

Use the word bank (Aufbau principle; electron configuration; ground-state electron configuration; Hund's rule; lowest; Pauli exclusion principle; spins; stable) to complete the statement: _____ states that single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins occupy the same orbitals.

a)

Hund's rule

b)

Aufbau principle

c)

Pauli exclusion principle

d)

ground-state electron configuration

48.

Complete the table: For Helium, the electron configuration shown is 1s21s^2 . What is the atomic number of Helium?

a)

2

b)

4

c)

6

d)

10

49.

Complete the table: The row with atomic number 7 corresponds to which element?

a)

Nitrogen

b)

Oxygen

c)

Fluorine

d)

Carbon

50.

What is the ground-state electron configuration for an atom with atomic number 7?

a)

1s2 2s2 2p31s^2\ 2s^2\ 2p^3

b)

1s2 2s2 2p41s^2\ 2s^2\ 2p^4

c)

1s2 2s1 2p41s^2\ 2s^1\ 2p^4

d)

1s2 2s2 2p51s^2\ 2s^2\ 2p^5

51.

For Neon, which electron configuration matches the filled 2p orbitals shown in the table's orbital diagram?

a)

1s2 2s2 2p61s^2\ 2s^2\ 2p^6

b)

1s2 2s2 2p51s^2\ 2s^2\ 2p^5

c)

1s2 2s1 2p61s^2\ 2s^1\ 2p^6

d)

1s2 2s2 2p41s^2\ 2s^2\ 2p^4

52.

What is the atomic number of Neon?

a)

8

b)

10

c)

12

d)

18

53.

What is germanium's atomic number? How many electrons does germanium have?

a)

32; 32 electrons

b)

34; 34 electrons

c)

14; 14 electrons

d)

28; 28 electrons

54.

What is noble-gas notation, and why is it used to write electron configurations?

a)

It uses the symbol of the nearest noble gas in brackets to represent inner-shell electrons, simplifying the configuration.

b)

It lists only the valence electrons without any core electrons so the atom appears neutral.

c)

It replaces electron configurations with atomic masses to make trends easier to see.

d)

It names orbitals by color instead of quantum numbers to avoid exponents.

55.

Write the ground-state electron configuration of a germanium atom, using noble-gas notation.

a)

[Ar] 3d10 4s2 4p2

b)

[Kr] 4s2 4p2

c)

[Ne] 3s2 3p2

d)

[Ar] 4s2 4p4

56.

The electrons in an atom's outermost orbitals are called

a)

electron dots

b)

quantum electrons

c)

valence electrons

d)

noble-gas electrons

57.

In an electron-dot structure, the element's symbol represents the

a)

nucleus of the noble gas closest to the atom in the periodic table

b)

atom's nucleus and inner-level electrons

c)

atom's valence electrons

d)

electrons of the noble gas closest to the atom in the periodic table

58.

How many valence electrons does a chlorine atom have if its electron configuration is [Ne]3s2 3p5?

a)

3

b)

21

c)

5

d)

7

59.

Given boron's electron configuration of [He]2s2 2p1, which of the following represents its electron-dot structure?

a)

B with three dots around the symbol

b)

B with two dots around the symbol

c)

B with one dot next to the symbol

d)

B with four dots around the symbol

60.

Given beryllium's electron configuration of 1s2 2s2, which of the following represents its electron-dot structure?

a)

Be with two dots around the symbol

b)

Be with three dots around the symbol

c)

Be with one dot next to the symbol

d)

Be with four dots around the symbol

61.

Which electrons are represented by the dots in an electron-dot structure?

a)

valence electrons

b)

inner-level electrons

c)

only s electrons

d)

both a and c

62.

Match each definition from Column A (items 1–5) with the correct term from Column B.

a)

The set of frequencies of the electromagnetic waves emitted by the atoms of an element

1.

atomic emission spectrum

b)

The minimum amount of energy that can be lost or gained by an atom

2.

quantum

c)

A form of energy that exhibits wavelike behavior as it travels through space

3.

electromagnetic radiation

d)

A three-dimensional region around the nucleus of an atom that describes an electron’s probable location

4.

atomic orbital

e)

The shortest distance between equivalent points on a continuous wave

5.

wavelength

63.

Match each definition from Column A (items 6–9) with the correct term from Column B.

a)

The lowest allowable energy state of an atom

1.

ground state

b)

A particle of electromagnetic radiation with no mass that carries a quantum of energy

2.

photon

c)

The emission of electrons from a metal’s surface when light of a certain frequency shines on it

3.

photoelectric effect

d)

A figure indicating the relative sizes and energies of atomic orbitals

4.

principal quantum number

64.

Describe how the pair is related: frequency, amplitude. Choose the statement that best explains their relationship.

a)

Frequency measures the number of wave cycles per second, while amplitude measures the wave’s height (or maximum displacement).

b)

Frequency and amplitude are the same quantity and always increase together.

c)

Amplitude is the distance between consecutive crests, while frequency is the time for one cycle.

d)

Frequency equals wavelength multiplied by amplitude.

65.

Describe how the pair is related: valence electron, electron-dot structure. Choose the statement that best explains their relationship.

a)

An electron-dot structure represents only core (nonvalence) electrons as dots around an element’s symbol.

b)

An electron-dot structure represents an atom’s valence electrons as dots around the element’s symbol.

c)

Valence electrons are shown as pairs of arrows in an electron-dot structure.

d)

Electron-dot structures list all electrons by principal quantum number.

66.

Describe how the pair is related: principal energy levels, energy sublevels. Choose the statement that best explains their relationship.

a)

Each principal energy level (n) contains one or more energy sublevels (such as s, p, d, f).

b)

Energy sublevels contain several principal energy levels within them.

c)

Principal energy levels and energy sublevels are unrelated concepts.

d)

Energy sublevels determine the number of protons in a nucleus.

67.

Quantum Mechanics says that electrons

a)

can act as both a particle and a wave

b)

can neither act as both a particle and a wave

c)

are a pure form of a wave only

d)

are particles only

68.

When an electron emits light

a)

the electron gets "excited" and "jumps out" away from the nucleus

b)

the electron gets "excited" and "drops back down" closer to the nucleus

c)

the electron "calms down" and "jumps out" away from the nucleus

d)

the electron "calms down" and "drops back down" closer to the nucleus

69.

Which subatomic particle is not found in the nucleus of an atom?

a)

Proton

b)

Neutron

c)

Electron

d)

All of the above are found in the nucleus

70.

What is the charge of a proton?

a)

Negative

b)

Positive

c)

Neutral

d)

Variable

71.

Which of the following is true about isotopes?

a)

They have different atomic numbers but the same mass number

b)

They have the same atomic number but different mass numbers

c)

They have different numbers of electrons but the same number of protons

d)

They are always ions

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