Free Printable Electrons in the Atom-Practice Quiz

1.

Rutherford’s atomic model could NOT explain which of the following?

a)

Location of the nucleus

b)

Why atoms are mostly empty space

c)

The chemical properties of elements

d)

Presence of protons

2.

Rutherford’s Gold Foil Experiment demonstrated that:

a)

Electrons move in fixed circular paths

b)

The atom has a dense nucleus

c)

Electrons behave like waves

d)

Light is quantized

3.

Bohr’s model proposed that electrons:

a)

Orbit randomly

b)

Occupy fixed energy levels

c)

Are located in a dense nucleus

d)

Are spread uniformly throughout the atom

4.

The fixed energies that electrons may have are called:

a)

Quanta

b)

Orbitals

c)

Waves

d)

Photons

5.

Which analogy best describes Bohr’s energy levels?

a)

A ramp

b)

A bouncing ball

c)

Ladder rungs

d)

A spinning top

6.

Bohr’s model works well for:

a)

Carbon

b)

Hydrogen

c)

Sodium

d)

Neon

7.

The quantum mechanical model is based on:

a)

Direct observation

b)

Newton’s laws

c)

Mathematical probability

d)

Mechanical motion only

8.

The region where an electron is most likely found is called:

a)

Orbit

b)

Quantum line

c)

Atomic orbital

d)

Photon Cloud

9.

In the quantum mechanical model, electrons:

a)

Follow exact paths

b)

Move randomly

c)

Have probable locations

d)

Are stationary

10.

The ground state of an electron is:

a)

The highest possible energy

b)

An unstable condition

c)

The lowest possible energy

d)

When the electron disappears

11.

Which sublevel can hold a maximum of 2 electrons?

a)

p

b)

s

c)

f

d)

d

12.

How many electrons can the p sublevel hold?

a)

2

b)

6

c)

10

d)

14

13.

How many orbitals are in a d sublevel?

a)

1

b)

3

c)

5

d)

7

14.

The Aufbau Principle states that electrons:

a)

Must pair before occupying orbitals

b)

Fill highest energy levels first

c)

Fill lowest energy orbitals first

d)

All spin in the same direction

15.

The Pauli Exclusion Principle states:

a)

Only one electron can be in an orbital

b)

Electrons pair with opposite spins

c)

Electrons avoid each other

d)

Electrons fill singly first

16.

Hund’s Rule states that electrons:

a)

Pair first

b)

Fill in opposite spins immediately

c)

Spin randomly

d)

Fill each orbital singly before pairing

17.

Which of the following is the correct electron capacity for the d sublevel?

a)

2

b)

6

c)

10

d)

14

18.

The most stable electron configurations often have:

a)

Half-filled or fully filled sublevels

b)

All orbitals empty

c)

Only s electrons

d)

No electrons in p orbitals

19.

Copper is an exception to the Aufbau Principle because:

a)

It has no p electrons

b)

It prefers a filled 3d sublevel

c)

It has a negative charge

d)

It contains radioactive isotopes

20.

The noble gas configuration for sulfur is:

a)

$[He]\ 2s^2\ 2p^4$

b)

$[Ne]\ 3s^2\ 3p^4$

c)

$[Ar]\ 4s^2$

d)

$[Kr]\ 5s^2\ 4d^{10}$

21.

Which element has the configuration $1s^2\ 2s^2\ 2p^5$ ?

a)

Oxygen

b)

Fluorine

c)

Neon

d)

Nitrogen

22.

Which element ends in $4s^2\ 3d^6$ ?

a)

Fe

b)

Cr

c)

Mn

d)

Co

23.

The shorthand electron configuration for calcium is:

a)

$[Ne]\ 3s^2$

b)

$[Ar]\ 4s^2$

c)

$[Kr]\ 5s^2$

d)

$[Xe]\ 6s^2$

24.

Which orbital type has the most complex shape?

a)

s

b)

p

c)

d

d)

f

25.

What determines how elements bond and react?

a)

Neutrons

b)

Valence electrons (outermost e-)

c)

Protons

d)

Atomic mass

26.

Section 3 – Waves & Light: A wave’s height from the rest position to the crest is the:

a)

Wavelength

b)

Frequency

c)

Amplitude

d)

Speed

27.

Section 3 – Waves & Light: Wavelength is measured:

a)

From crest to crest

b)

From trough to equilibrium

c)

In seconds

d)

In joules

28.

Section 3 – Waves & Light: Frequency is measured in:

a)

Meters

b)

Hertz

c)

Joules

d)

Newtons

29.

Section 3 – Waves & Light: The relationship between wavelength and frequency is:

a)

Direct

b)

Random

c)

Exponential

d)

Inverse

30.

Section 3 – Waves & Light: The speed of light is:

a)

$3.00 \times 10^{8}\ \text{m/s}$

b)

$6.02 \times 10^{23}\ \text{m/s}$

c)

$9.81\ \text{m/s}^2$

d)

$1.60 \times 10^{-19}\ \text{m/s}$

31.

Section 3 – Waves & Light: Which equation correctly relates light speed, frequency, and wavelength?

a)

$E = mc^2$

b)

$c = \lambda v$

c)

$F = ma$

d)

$\lambda = c + v$

32.

Section 3 – Waves & Light: As wavelength increases, frequency:

a)

Increases

b)

Decreases

c)

Stays the same

d)

Doubles

33.

Section 3 – Waves & Light: The electromagnetic spectrum is arranged based on:

a)

Color

b)

Wavelength

c)

Temperature

d)

Volume

34.

Section 3 – Waves & Light: Visible light is:

a)

The entire electromagnetic spectrum

b)

A small portion of the spectrum

c)

The lowest energy region

d)

Only red and blue light

35.

Section 3 – Waves & Light: Which type of EM radiation has the highest frequency?

a)

Infrared

b)

Ultraviolet

c)

Gamma rays

d)

Microwaves

36.

Section 4 – Atomic Emission Spectra: What causes electrons to move to higher energy levels?

a)

Absorption of energy

b)

Emission of photons

37.

When electrons return to lower energy levels, they emit:

a)

Neutrons

b)

Protons

c)

Light

d)

Electrons

38.

The atomic emission spectrum is:

a)

Continuous

b)

Unique to each element

c)

Always the same colors

d)

Random

39.

The lines in an emission spectrum represent:

a)

Specific frequencies of light

b)

Neutron absorption

c)

Thermal changes

d)

Reflections

40.

A photon is:

a)

A massless particle of light

b)

A neutron

c)

A proton

d)

A wave crest

41.

The ground state of an electron is when it:

a)

Is highest in energy

b)

Emits a photon

c)

Drops to the lowest energy level

d)

Absorbs energy

42.

Firework colors are produced by:

a)

Explosives only

b)

Atoms absorbing energy

c)

Electrons emitting light as they return to ground state

d)

Changes in chemical bonds

43.

The frequency of emitted light is proportional to:

a)

Electron mass

b)

Energy change between levels

c)

Number of protons

d)

Temperature

44.

The quantum number n represents:

a)

Orbital shape

b)

Principal energy level

c)

Spin direction

d)

Electron charge

45.

Orbitals are grouped into:

a)

Levels

b)

Isotopes

c)

Nuclei

d)

Photons

46.

Which sublevel appears first when filling electrons?

a)

3d

b)

4s

c)

4d

d)

5p

47.

Atomic orbitals describe:

a)

Exact electron paths

b)

Probable locations

c)

Definite positions

d)

Fixed circles

48.

Light behaves as both:

a)

A wave and a particle

b)

A solid and gas

c)

A proton and neutron

d)

A chemical and physical change

49.

A wave with high frequency has:

a)

Low energy

b)

High energy

c)

No energy

d)

Constant energy

50.

A longer wavelength means:

a)

Higher energy

b)

Lower frequency

c)

Higher frequency

d)

More visible colors

51.

Which element is pictured?

a)

neon

b)

fluorine

c)

magnesium

d)

argon

52.

What is the mass number of this atom?

a)

1

b)

3

c)

4

d)

7

53.

What electron configuration matches an oxygen atom?

a)

1s²2s²2p⁶3s2, 3p⁶4s²3d¹⁰4p⁵

b)

1s²2s²2p⁴

c)

1s²2s²2p⁶

d)

1s²2s²2p⁶3s²3p⁶4s²3d¹

54.

This orbital diagram represents:

a)

C

b)

B

c)

N

d)

O

55.

How many electrons can the first energy level hold?

a)

1

b)

2

c)

8

d)

0

56.

How many electrons can the p sublevel hold?

a)

14

b)

10

c)

2

d)

6

57.

Which element is depicted from this atomic orbital diagram?

a)

Carbon

b)

Nitrogen

c)

Oxygen

d)

Phosphorus

58.

What atom matches this electron configuration?
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

59.

How many electrons can the d sublevel hold?

a)

14

b)

10

c)

2

d)

6

60.

What is the speed of light in a vacuum?

a)

$3\times10^8$ m/s

b)

$3\times10^{-8}$ m/s

c)

$6.63\times10^{34}$ J s

d)

$6.63\times10^{-34}$ J s

61.

Calculate the wavelength of light with a frequency of 7.66 x 10¹⁴ Hz. (c=3.00x10⁸ m/s)

a)

3.92 x 10^-7 m

b)

4.25 x 10⁷ m

c)

7.60 x 10^-8 m

d)

2.53 x 10²² m

62.

Green light has a frequency of 6.01 x 10¹⁴ Hz. What is the wavelength?

a)

4.7 × 10⁵ m

b)

7.31 × 10¹⁹ Hz

c)

3.91 × 10^-7 m

d)

4.99 × 10^-7 m

63.

Calculate the frequency of a wave of light with a wavelength of 3.91 x 10^-7 m

a)

7.82 x 10^-7 Hz

b)

7.67 x 10¹⁴ Hz

c)

3.00 x 10⁸ Hz

d)

1.30 x 10^-15 Hz

Electrons in the Atom-Practice Quiz

Total questions: 63

Worksheet time: 35mins

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