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Chapter 4 Review

Total questions: 78

Worksheet time: 56mins

Name
Class
Date
1.

Whose model suggested that negative particles were mixed in with positively charged material - like seeds in a watermelon? (plum pudding model)

a)

J.J. Thomson

b)

Ernest Rutherford

c)

Niels Bohr

d)

Albert Einstein

2.

Who discovered that the atom had an small, dense, positively charged center?

a)

Ernest Rutherford

b)

J.J Thomson

c)

Robert Millikan

d)

John Dalton

3.

Place the following atomic models in order, from earliest to latest:


A) Rutherford B) Thomson C) Dalton

a)

B, C, A

b)

C, A, B

c)

A, C, B

d)

C, B, A

4.

Who named the positive center of the atom the "nucleus?"

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

5.
Where are electrons of an atom found?
a)
Nucleus
b)
Electron Cloud
c)
Some are in the nucleus and some in the electron cloud.
d)
They are moving everywhere.
6.

Which of the following is a positively charged particle found in the nucleus of an atom?

a)

Electron

b)

Proton

c)

Neutron

d)

Quark

7.

Which particle carries no charge?

a)

Neutrons

b)

Electrons

c)

Protons

8.
Which is the smallest?
a)
electron
b)
proton
c)
atom
d)
neutron 
9.
What is in the nucleus of an atom?
a)
Neutrons and protons 
b)
Protons
c)
Protons and Electrons
d)
Electrons and Nuetrons
10.
True or False? Neutrons have a negative charge
a)
True
b)
False
11.
A particle that moves around the nucleus is a(n)...
a)
Proton
b)
Neutron
c)
Electron
d)
Quark
12.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
13.

The first modern atomic theory was proposed by

a)

Ariostotle

b)

Dalton

c)

Rutherford

d)

Thompson

14.

Joke: A neutron walks into the cafeteria and buys a soda. When he is checking out, the clerk says:

a)

"For you, no charge."

b)

"That will be $1.99."

c)

"I am going to give you money for being so positive."

d)

MR. SEEBODE- your jokes are NOT funny :/

15.

Rutherford realized that the atomic nucleus was positively charged because

a)

it attracted alpha particles.

b)

it deflected alpha particles.

c)

it had no effect on alpha particles.

d)

it produced alpha particles.

16.

Niels Bohr added _______________ to the model of the atom.

a)

electrons.

b)

a nucleus.

c)

neutrons.

d)

energy levels.

17.

How many energy levels would be in the Bohr model for magnesium?

a)

1

b)

2

c)

3

d)

4

18.

If an atom were enlarged so that the nucleus were the size of a marble, then the entire atom would occupy the volume of a(n)

a)

tennis ball.

b)

basketball.

c)

large beach ball.

d)

football field.

19.

A line emission spectrum is produced when electrons

a)

become excited and move from ground state to higher levels in an atom.

b)

leave the atom completely.

c)

fall from higher, excited states back to lower or ground state.

d)

move from a cathode to an anode.

20.

What is the name of this element? Look at the number of protons - the atomic number.

a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
21.

What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

22.
What is the name of this element?
a)
Lithium
b)
Boron
c)
Carbon
d)
Neon
23.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
24.

Isotopes are elements with the same atomic number but different amounts of...

a)
protons
b)
neutrons
c)
electrons
d)
atoms
25.
an element will always have the same number of 
a)
neutrons
b)
protons
c)
isotopes
d)
atoms
26.
How are electrons arranged in an atom?
a)
In groups of five
b)
In energy levels
c)
By color
d)
By shape
27.

What is the atomic number of this element?

a)

17

b)

18

c)

35

d)

35.453

28.

Which element does this Bohr model represent?

a)

Aluminum

b)

Silicon

c)

Magnesium

d)

Cobalt

29.
What is the atomic number of Chlorine (Cl)?
a)
17
b)
Cl
c)
35.453
d)
Chlorine
30.

If the first and second energy levels of an atom are full, then what would be the total number of electrons in the atom?

a)

6

b)

8

c)

10

d)

18

31.

How many orbitals are present in the 4p sub level?

a)

7

b)

5

c)

4

d)

3

32.

According to Pauli Exclusion Principle, how many electrons may occupy a single orbital?

a)

1

b)

2

c)

4

d)

8

33.

“An electron should occupy the lowest energy level first before the higher energy level” is stated in what rule?

a)

Hund's rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

All of the above.

34.

What rule states that single electrons must occupy each orbital in a sublevel before they can pair up?

a)

Hund's rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

None of the choices.

35.

What is the electron configuration of Argon?

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s1

c)

1s2 2s2 2p6 3s2

d)

1s2 2s2 2p6 3s2 3p6

36.

Which atom has an electron configuration of 1s2 2s2 2p6?

a)

He

b)

Ne

c)

Ar

d)

Xe

37.

What is the electron configuration of Gallium, 31Ga?

a)

1s2 2s2 2p6 3s2 3p5 4s2 3d10 4p1

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d9 4p2

d)

1s2 2s2 2p6 3s2 3p5 4s2 3d10 4p2

38.

Which one of the following electron configurations is INCORRECT?

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p5

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d9 4p2

39.

Which of the following electron configurations is CORRECT?

a)

1s2 2s3

b)

1s2 2s2 2p6

c)

1s2 2s2 3s2

d)

1s2 2s2 2p6 3s2 4s2

40.

Who is the Greek philosopher that developed the idea about atoms in 500 BC?

a)

Dalton

b)

Plato

c)

Aristotle

d)

Democritus

41.

What model of the atom replaced Bohr's model?

a)

Heisenberg's model

b)

Thomson's model

c)

Rutherford's model

d)

Quantum Mechanical model

42.

Regions in which electrons are likely to be found is called... also known as probability clouds.

a)

atomic orbitals

b)

principal energy level

c)

energy sublevel

d)

spin

43.

A region around the nucleus of an atom where an electron is likely to be moving is called

a)

atomic orbital

b)

principal energy level

c)

energy sublevel

d)

spin

44.
What is the shape of p orbitals? 
a)
Peanut shaped
b)
Spherical shaped
45.
What is the shape of s orbitals?
a)
Dumbbell shaped
b)
Peanut shaped
c)
Spherical shaped
d)
Hybrid structure
46.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
47.
What is the maximum number of electrons that can be on the p sublevel?
a)
6
b)
3
c)
2
d)
4
48.
How many orbitals are there in the "d" sublevel?
a)
1
b)
3
c)
5
d)
7
49.
How many orbitals are there in the "s" sublevel?
a)
1
b)
3
c)
5
d)
7
50.
How many orbitals are there in the "p" sublevel?
a)
1
b)
3
c)
5
d)
7
51.
How many orbitals are there in the "f" sublevel?
a)
1
b)
3
c)
5
d)
7
52.
How many electrons can the f sublevel hold?
a)
14
b)
10
c)
6
d)
4
53.
Which main energy level is furthest from the nucleus ?
a)
1
b)
2
c)
3
54.
The quantum number "n" represents:
a)
electron spin
b)
orbital
c)
sublevel
d)
main energy level
55.

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 returns to the ground state it emits a_______________________.

a)

blast of cold air

b)

electrostatic charge

c)

proton

d)

photon (light)

56.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

57.

Line emission spectra is produced from atoms when

a)

electrons release energy as they move to their excited state.

b)

electrons absorb energy as they move to their excited state.

c)

electrons release energy as they return to the ground state.

d)

electrons absorb energy as they return to the ground state.

58.

Region of high probability of finding an electron

a)

atomic orbital

b)

ground state

c)

Heisenberg uncertainty principle

d)

electron configuration

59.

How many neutrons would Fe-56 have? Iron has an atomic number of 26.

a)

56

b)

26

c)

30

d)

33

60.

If an atom of nickel (atomic number 27) has a charge of +3, how many electrons does the atom have?

a)

28

b)

24

c)

26

d)

31

61.

If an atom of oxygen (atomic number 8) has a charge of -2, how many electrons does the atom have?

a)

18

b)

6

c)

8

d)

10

62.

How many neutrons would V-49 have? Vanadium has an atomic number of 23.

a)

26

b)

49

c)

23

d)

50.94

63.

What is the mass number of an atom of gold (Au - atomic number 79) with 117 neutrons?

a)

117

b)

196

c)

196.97

d)

197

64.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
65.

What is a cation's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element

66.

What is an anion's charge?

a)

positive

b)

negative

c)

neutral

d)

depends on the element's charge

67.

How many valence electrons does Nitrogen (N) Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

68.

How many valence electrons does Magnesium (Mg) have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

69.
What's a valence electron?
a)
electrons in the second energy level
b)
electrons in the outermost energy level
c)
the atomic number
d)
electrons in the first level
70.

Which of the elements in the picture has the most correct electron dot notation?

a)

1

b)

2

c)

3

d)

4

71.

Which of the elements in the picture has correct electron dot notation? Remember - likes repel!

a)

1

b)

2

c)

3

d)

4

72.
Question Image

Match the following

a)

Rutherford's model

1.

Gold foil experiment - positive nucleus added

b)

Chadwick

2.

added neutrons to nucleus

c)

Bohr model

3.

planetary model with energy levels

d)

energy levels

4.

discovered because of emission spectrum

e)

Quantum model

5.

orbitals, not orbits

73.
Question Image

Match the following

a)

what is the charge of an up quark?

1.

+2/3

b)

What is the charge of a down quark?

2.

-1/3

c)

What quarks are in protons?

3.

2 up and 1 down

d)

What quarks are in neutrons?

4.

2 down and 1 up

e)

An alpha particle

5.

2 protons and 2 neutrons or nucleus of helium atom

74.

Which spectrum results from taking in energy causing excited electrons?

a)

absorption

b)

emission

c)

continuous

75.
Question Image

Match the following

a)

Believed in what became the Continuous Theory of Matter

1.

Aristotle

b)

Believed in what became the Particle Theory of Matter

2.

Democritus

c)

Particles cannot be divided infinitely without changing its properties

3.

Particle Theory of Matter

d)

Particles can be divided without end without changing its properties.

4.

Continuous Theory of Matter

e)

Every compound is formed of elements combined in specific ratios

5.

Law of Definite Composition

76.
Question Image

Match the following

a)

Rutherford sent these through gold foil and discovered the nucleus

1.

alpha particles

b)

Thompson discovered electrons because these bent towards + charged plates

2.

cathode rays

c)

Chadwick discovered

3.

neutrons

d)

Most massive particle in the nucleus

4.

neutron

e)

He developed the idea of principle energy levels

5.

Niels Bohr

77.

De Broglie said electrons act like...

a)

particles

b)

waves

c)

particles and waves

78.

According to the Heisenberg Uncertainty Principle it is impossible to know both the energy and the position of an electron at the same time.

a)

True

b)

False

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