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Electrons in Atoms

Total questions: 68

Worksheet time: 54mins

Name
Class
Date
1.

1. What atom matches this electron configuration?

1s2 2s2 2p6 3s23p4

a)

sodium

b)

sulfur

c)

silicon

d)

potassium

2.

What is the correct electron configuration for oxygen?

a)

1s22s22p63s23p64s2

b)

1s22s22p63s23p4

c)

1s12s22p5

d)

1s22s22p4

3.

What is the maximum number of electrons that an orbital can have?

a)

2

b)

6

c)

8

d)

10

4.

How many d orbitals are there?

a)

2

b)

5

c)

7

d)

10

5.

How many electrons can the p sublevel hold?

a)

2

b)

3

c)

6

d)

8

6.

What is this element?

1s2 2s2 2p6 3s2 3p6 4s2 3d5

a)

magnesium

b)

iron

c)

manganese

d)

chromium

7.

What element is depicted in the orbital diagram above?

a)

scandium

b)

chlorine

c)

bismuth

d)

bromine

8.

What is the noble gas configuration for a sulfur atom?

a)

[Ar] 3p4

b)

[Ne] 3p4

c)

[Ne] 3s23p4

d)

[He] 3s23p4

9.

Which element is depicted above?

a)

carbon

b)

neon

c)

oxygen

d)

calcium

10.

Which element below matches this noble gas configuration? [Kr] 5s2 4d2

a)

titanium

b)

calcium

c)

zirconium

d)

hafnium

11.

Which of the following is a correct configuration for aluminum?

a)

1s2 2s2 3s2 3p1

b)

1s2 2s2 2p2 2s2 3p1

c)

[Ne] 3s2 3p1

d)

[Ne] 3p1

12.

Which of the following is the correct notation for osmium (Os)?

a)

[Xe] 6s2 5d6

b)

[Xe] 6s2 4f14 5d6

c)

[Rn] 6d6

d)

[Kr] 5s2 4d6

13.

How many total electrons can an f orbital contain?

a)

2

b)

7

c)

8

d)

14

14.

Which of the following is a noble gas?

a)

hydrogen

b)

argon

c)

potassium

d)

iodine

15.

Which rule says orbitals are filled from lowest energy to highest?

a)

Aufbau's principle

b)

Hund's principle

c)

Pauli exclusion principle

d)

Law of conservation of mass

16.

Which of the following is correct for germanium (Ge)?

a)

[Ar] 4s2 4d10 4p2

b)

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p2

c)

[Ar] 4s2 3d10 4p2

d)

4s2 3d10 4p2

17.

Which element is show above?

a)

lithium

b)

hydrogen

c)

helium

d)

carbon

18.

The emission of electrons from a metal when light shines on the metal → photoelectric effect

a)

true

b)

false

19.

A state in which an atom has a higher potential energy than it has in its ground state → ground state

a)

true

b)

false

20.

when a narrow beam of the emitted light was shined through a prism, it was separated into four specific colors of the visible spectrum →line emission spectrum

a)

true

b)

false

21.

visible light, which is a form of energy that exhibits wavelike behavior as it travels through space

a)

electromagnetic spectrum

b)

photoelectric effect

c)

electromagnetic radiation

d)

line emission spectrum

22.

all the forms of electromagnetic radiation

a)

electromagnetic spectrum

b)

line emission spectrum

c)

electromagnetic radiation

d)

photoelectric effect

23.

The lowest energy state of an atom

a)

excited state

b)

ground state

c)

frequency

d)

wavelength

24.
When an electron moves from a lower to a higher energy level, the electron ________________.
a)
gains a certain amount of energy
b)
gains any amount of energy
c)
loses energy
d)
moves closer to the nucleus
25.
The light given off when electricity is passed through sodium gas is called sodium's _______________
a)
wavelength
b)
emission spectrum
c)
light
d)
continuous spectrum
26.
In Bohr's model of the atom, where are the electrons and protons located?
a)
the electrons orbit the protons, which are at the center of the atom
b)
the electrons and protons move throughout the atom
c)
the electrons and protons are located throughout the atoms, but they are not free to move
d)
the electrons are stationary around the protons, which are at the center of the atom
27.
Emission of light from an atom occurs when the electron ________.
a)
moves within its atomic orbital
b)
jumps from a lower to a higher energy level
c)
falls into the nucleus
d)
drops from a higher to a lower energy level
28.

What atom matches this electron configuration?

1s22s22p63s2

a)

20Ca

b)

12Mg

c)

13Al

d)

19K

29.

Which atom matches this electron configuration?

1s22s22p63s23p64s23d10

a)

30Zn

b)

29Cu

c)

28Ni

d)

32Ge

30.
The shortest wavelength in visible light is______.
a)
violet
b)
red
c)
blue
d)
yellow
31.
_____ have the longest wavelengths and lowest frequencies of all electromagnetic waves.
a)
microwaves
b)
radio waves
c)
gamma rays
d)
ultraviolet
32.
_______ carry the greatest amount of energy. 
a)
x-rays
b)
gamma rays
c)
infrared rays
d)
visible light
33.
The shortest wavelength in visible light is______.
a)
violet
b)
red
c)
blue
d)
yellow
34.

The _____ determines the color of visible light.

a)

wavelength

b)

speed

c)

amplitude

d)

light

35.

Which drawing represents the process by which an emission line is formed? [Emission means that energy is being "emitted" or released by the atom.]

a)

A

b)

B

c)

C

d)

D

36.

Which drawing represents the process by which an absorption line is formed? [Absorption means that energy is being absorbed or taken-in by the atom.]

a)

A

b)

B

c)

C

d)

D

37.

Which electron transition is associated with a higher energy wave?

a)

n = 4 to n = 3

b)

n = 4 to n = 2

c)

n = 4 to n = 1

38.
What is the light that you can see called?
a)
observatory
b)
wavelength
c)
visible light
39.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
40.

Four gas spectra are given. What gases are in the unknown mixture?

a)

Gas B & Gas D

b)

Gas C & Gas B

c)

Gas A & Gas D

d)

Gas D & Gas C

41.
Hund’s rule states…
a)
Atomic orbitals have opposite spins and 2 electrons each
b)
Electrons occupy orbitals of highest energy first and energy level changes as you go up
c)
Electrons occupy orbitals of lowest energy first, starting with 1s
d)
Electrons occupy orbitals of equal energy, one electron enters EACH orbital ONE AT A TIME until orbitals of the entire energy level have one electron with the SAME SPIN.
42.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
43.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

44.

Which element is represented by this orbital notation?

a)

neon

b)

sodium

c)

magnesium

d)

aluminum

45.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
46.
Electrons are paired based on their spin directions, clockwise and counterclockwise, is what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
47.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
48.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
49.
In an orbital diagram,  an arrow represents: 
a)
an electron
b)
an orbital
c)
an element
50.
The maximum number of electrons that can be placed in an f orbital.  
a)
2
b)
6
c)
10
d)
14
51.
The maximum number of electrons that can be placed in an d  orbital.  
a)
2
b)
6
c)
10
d)
14
52.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
53.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
54.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

55.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

56.

All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.


Using the Bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”).

a)

Lithium and cadmium are in the mixture. Strontium is not in the mixture.

b)

Lithium and strontium are in the mixture. Cadmium is not in the mixture

c)

Cadmium and strontium are in the mixture. Lithium is not in the mixture

d)

All of the shown elements are present in the mixture.

57.

Flame tests can be used to identify an element. Each element emits characteristic waves of light when it is heated in a flame. What describes how the light is produced?

a)

Protons in the ground state lose energy and give off light.

b)

Protons in the ground state gain energy and are emitted from the nucleus, giving off light.

c)

Electrons in the ground state lose energy and move to an excited state, giving off light.

d)

Electrons in the ground state gain energy, move to an excited state, and give off light when they return to the ground state.

58.

__________ represents the distance the electrons are from the nucleus

a)

energy level

b)

sublevel

59.
Why are line emission spectra of elements called "atomic fingerprints"?
a)
They are all the same
b)
They are all unique
c)
They are all similar
d)
They all contain colored light
60.

Look carefully at the picture. It shows an electron in the excited state on the left, and the electron returning to its ground state on the right. When the electron return to the ground state it emits a_______________________.

a)

blast of cold air

b)

electrostatic charge

c)

proton

d)

photon (light)

61.

All forms of EM radiation travel at the same speed and have the same energy.

a)

False, they travel at the same speed but have different energies

b)

True

c)

False, they travel at different speeds but have the same energy

62.

Which scientist is credited with the discovery of atomic energy levels?

a)

Bohr

b)

Thomson

c)

Rutherford

d)

Bunsen

63.

Why do we see an apple is red?

a)

Red light is absorbed by apple

b)

All light is absorbed by apple

c)

Red light is reflected by apple

d)

All light is reflected by apple

64.

Where are the electrons in the atom?

a)

The nucleus

b)

The orbitals or clouds

c)

The Golgi Apparatus

d)

Atoms do not have electrons

65.

An electron that jumps multiple orbitals compared to an electron that jumps only one will release

a)

a shorter wavelength of color

b)

a longer wavelength of color

c)

no wavelengths of color

d)

all the wavelengths of color

66.

A shorter wavelength of color would be in what part of the light spectrum

a)

Red

b)

Orange

c)

Yellow

d)

Indigo

67.

Which of the following statement is wrong?

a)

Two electrons must occupy each equal energy orbital before additional electrons can occupy the same orbitals.

b)

A maximum of two electrons may occupy the same orbitals.

c)

In filling up orbitals, electron occupies the lowest energy orbital first before the higher energy orbitals.

d)

None of the choices.

68.

Electrons prefer to be in...

a)

third energy level

b)

highest energy level

c)

2nd energy level

d)

lowest possible energy level

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