wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Unit 3 Review Quizziz

Total questions: 126

Worksheet time: 5hrs 34mins

Name
Class
Date
1.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
2.
Balance the following equation:
146C --> 0-1e + ________
a)
145B
b)
146C
c)
147N
d)
42He
3.
Which type of nuclear radiation is being emitted here?
a)
Alpha
b)
beta
c)
gamma 
d)
none
4.

Solve this equation for beta decay.

614C = ___ + -10e

a)

410Be

b)

714N

c)

210He

d)

613C

5.
Complete the nuclear equation and determine the type of decay that is occurring in this reaction. 
a)
alpha
b)
beta
c)
gamma
d)
none
6.

Uranium 238 emits an alpha particle to become what nucleus?

a)

Thorium-234

b)

Thorium-239

c)

Thorium-236

7.

If the half-life of a radioactive substance is 4 days, how much of a 200-g radioactive sample is left after 16 days?

a)

800g

b)

50g

c)

25g

d)

12.5g

8.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
9.
Solve this equation for beta decay.
614C = ___ + -10e
a)
410Be
b)
714N
c)
210He
d)
613C
10.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
11.

The sum of protons and neutrons

a)

atomic number

b)

atom mass

12.

Gamma radiation is...

a)

An electromagnetic wave

b)

A helium nucleus

c)

An electron

13.

What form of radiation is emitted by nuclei with too many neutrons?

a)

Alpha

b)

Gamma

c)

Beta

14.

Gamma radiation can be significantly reduced by...

a)

Paper

b)

Aluminum

c)

Lead

15.

What causes an atom's nucleus to become unstable?

a)

Too many or too few neutrons in the nucleus

b)

More electrons than protons

c)

Fewer electrons than protons

16.

Uranium 238 emits an alpha particle to become what nucleus?

a)

Thorium-234

b)

Thorium-239

c)

Thorium-236

17.

An alpha particle is...

a)

An electron

b)

A helium nucleus

c)

An electromagnetic wave

18.

Which type of radiation can reach the furthest?

a)

Beta

b)

Gamma

c)

Alpha

19.

What fraction of a radioisotope has decayed after two half-lives?

a)

One quarter

b)

All of it

c)

Three quarters

20.

How long does it take a 180-gram of gold-198 to decay to 22.5 grams if the half -life of gold-198 is 2.68 days?

a)

8.04 days

b)

3 days

c)

4 days

d)

2.68 days

21.

How long will it take for a 28-gram sample of radon-222 to decay to 3.5 grams? the half-life of radon-222 of 3.82 days

a)

15.28 days

b)

11.46 days

c)

3 days

d)

4 days

22.

How long will it take for a 150-gram sample of Nitrogen-16 tp decay to 18.75 grams if the half-life for Nitrogen -16 is 7.2 seconds

a)

7.2 seconds

b)

14.4 seconds

c)

18.75 seconds

d)

21.6 seconds

23.

How long will it for a take for a 40 gram. The half-life of cobalt-60 is 5.26 years sample ofcobalt-60 to decay to 5 grams?

a)

17.75 days

b)

15.78 years

c)

15.15 years

d)

17.17 years

24.

In the equation, 146C --> 147N + 0-1B, the _______ decay of radioactive carbon-14 results in the creation of a new nitrogen-14 atom.

a)

Gamma

b)

Beta

c)

Alpha

25.
Uranium-238  decays into  Thorium-234  by emitting .........
a)
an alpha particle
b)
a beta particle
c)
gamma rays
d)
visible light
26.
If we start off with element 24X50 after an alpha decay we get another element Y that looks like
a)
22Y50
b)
22Y46
c)
20Y48
d)
26Y54
27.
Has the highest penetrating power.  Can penetrate our body.  Even several cm thick of lead or several meters thick of concrete cannot stop all of it.
a)
Alpha
b)
Beta
c)
Gamma
28.

24094Pu —› ____ + 42He

a)

23692U

b)

24796Cm

c)

24493Np

d)

24295Am

29.
How many protons are in this atom?
a)
3
b)
4
c)
6
d)
10
30.
How many neutrons are in this isotope of Uranium?
a)
235
b)
92
c)
327
d)
143
31.

Gamma rays have

a)

no mass

b)

a huge mass

c)

a small mass

d)

an average mass

32.
Electronegativity is...
a)

the ability of an atom to attract electron shared towards itself

b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
33.
What elements have zero electronegativity?
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
34.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

35.

As you move across a period, the outer electrons are ________ to the nucleus, so the nucleus of the atom is ________ to attract electrons in a bond.

a)

closer, more able

b)

closer, less able

c)

further, less able

d)

further, more able

36.

Why does electronegativity decrease as you go down a group?

a)

As you go down a group, the outer electrons are further away from the nucleus

b)

As you go down a group, the nucleus is less able to attract electrons in a bond

c)

Both of these

d)

None of these

37.

Based on the data in the table above, which of the following correctly predicts the decreasing of relative electronegativity of the elements X, Y, and Z, and provides the correct reason?

a)

X > Y > Z because smaller elements have a stronger attraction between the nucleus and valence electrons

b)

X > Y > Z because smaller elements have a weaker attraction between the nucleus and valence electrons

c)

Z > Y > Z because larger elements have a stronger attraction between the nucleus and valence electrons

d)

Z > Y > Z because larger elements have a weaker attraction between the nucleus and valence electrons

38.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
39.

What is the trend for electronegativity as you move left to right across a period and why?

a)

EN increases because the shielding effect increases causing the effective nuclear charge to decrease as you add more protons to the nucleus

b)

EN decreases because the shielding effect decreases causing the effective nuclear charge to increase as you add more protons to the nucleus

c)

EN increases because the effective nuclear charge increases as the size of atom becomes smaller and the attraction between nucleus and electrons getting stronger

d)

EN decreases because the effective nuclear charge decreases as the size of atom becomes bigger and the attraction between nucleus and electrons getting weaker

40.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
41.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
42.
Which of the following is the least electronegative element?
a)
oxygen
b)
potassium
c)
fluorine
d)
nitrogen
43.
Put these in order of increasing electronegativity:
Se, S, and O
a)
Se < S < O
b)
Se < O < S
c)
O < S < Se
d)
S < Se < O
44.

What does electronegativity do as you go across a period?

a)

decrease

b)

no pattern

c)

stay the same

d)

increase

45.

Electronegativity _______ across a period and ______ down a group.

a)

increases, increases

b)

increases, decreases

c)

decreases, increases

d)

decreases, decreases

46.

Which of these atoms is the most electronegative?

a)

Bromine

b)

Fluorine

c)

Hydrogen

d)

Potassium

47.

Which element in the pair of adjacent elements, Mg and Na,has a higher first ionization energy?

a)

Na

b)

Mg

48.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
49.

Which statement correctly and completely identifies a trend?

a)

Atomic radius decreases across a period and increases down a group.

b)

Electronegativity decreases across a period and decreases down a group.

c)

Ionization energy increases across a period and increases down a group.

d)

Ionic radius increases across a period and increases down a group.

50.
Which of the following is true about a sulfur atom and a chlorine atom?
a)
Sulfur is larger and has higher ionization energy.
b)
Sulfur is larger and has lower ionization energy.
c)
Sulfur is smaller and has higher ionization energy.
d)
Sulfur is smaller and has lower ionization energy.
51.

What did Rutherford discover about atoms?

a)

An atom is always negatively charged.

b)

An atom is mostly empty space, but has a dense positively charged center(nucleus).

c)

An atom is always positively charged.

d)

All particles will pass straight through gold foil with no change in path.

52.

What is a positively charged particle?

a)

neutron

b)

electron

c)

proton

d)

atom

53.

What is a negatively charged particle?

a)

neutron

b)

electron

c)

proton

d)

atom

54.

What is a particle with no charge?

a)

neutron

b)

electron

c)

proton

d)

atom

55.

Who discover the electron?

a)

Dalton

b)

Rutherford

c)

Thomson

d)

Bohr

56.

What did Rutherford discover in his experiment?

a)

nucleus

b)

electrons

c)

neutrons

d)

protons

57.

Who proposed a model with electrons moving in specific layers?

a)

Dalton

b)

Rutherford

c)

Bohr

d)

Thomson

58.

What does atom mean?

a)

small

b)

visible

c)

indivisible

d)

particle

59.

Rutherford's "gold-foil" experiment using alpha particle scattering concluded that

a)

the center of the atom is empty

b)

atomic mass is spread over the whole atom

c)

the center of the atom has a negative charge

d)

most of the atom is empty

60.
A tiny but very dense, positively charged portion of the atom that holds most of the atomic mass
a)
Electron Shells
b)
Orbitals
c)
Electron Cloud
d)
Nucleus
61.

Who was considered as one of the founders of the ancient atomist theory?

a)

Aristotle

b)

Parmenides

c)

Empedocles

d)

Democritus

62.

What is the correct order of scientists in order of their work related to the atomic theory from earliest to most recent?

a)

Ernest Rutherford, JJ Thomson, John Dalton, & Democritus

b)

JJ Thomson, John Dalton, Ernest Rutherford, & Democritus

c)

Democritus, John Dalton, JJ Thomson, Ernest Rutherford.

d)

John Dalton, JJ Thomson, Democritus, & Ernest Rutherford

63.

Who discovered the neutron?

a)

JOSEPH JOHN THOMSON

b)

ERNEST RUTHERFORD

c)

NEILS BOHR

d)

JAMES CHADWICK

64.

It is the smallest particle of an element

a)

PROTON

b)

ELECTRON

c)

NEUTRON

d)

ATOM

65.

Where are electrons located in an atom?

a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
66.

What did Thomson's atomic theory model look like?

a)

A ring with gold foil in the middle.

b)

Electrons orbiting the nucleus like the planets around the sun.

c)

A cloud of electrons floating around the nucleus.

d)

A scoop of chocolate chip ice cream. It had electrons scattered within a ball of positive charge.

67.

What did Bohr's atomic theory model look like?

a)

A ring with gold foil in the middle.

b)

Electrons orbiting the nucleus like the planets around the sun.

c)

A cloud of electrons floating around the nucleus.

d)

A scoop of chocolate chip ice cream. It had electrons scattered within a ball of positive charge.

68.

The cloud model is what we use for the atomic theory now. What does the cloud model look like?

a)

A ring with gold foil in the middle.

b)

Electrons orbiting the nucleus like the planets around the sun.

c)

A cloud of electrons floating around the nucleus.

d)

A scoop of chocolate chip ice cream. It had electrons scattered within a ball of positive charge.

69.

What did Rutherford discover about atoms?

a)

An atom is always negatively charged.

b)

An atom is mostly empty space, but has a dense positively charged center(nucleus).

c)

An atom is always positively charged.

d)

All particles will pass straight through gold foil with no change in path.

70.

What is the mass of a proton?

a)

1840 amus

b)

1 amu

c)

1/1840 amus

d)

It has no mass.

71.

What is the mass of a neutron?

a)

1840 amus

b)

1 amu

c)

1/1840 amus

d)

It has no mass.

72.

The mass number is the sum of what two parts of an atom?

a)

proton and neutron

b)

proton and electron

c)

electron and netron

d)

none of the above

73.

If oxygen-16 has 8 protons, then how many neutrons does it have?

a)

9

b)

16

c)

8

d)

7

74.

If oxygen-17 has 8 protons, then how many neutrons does it have?

a)

9

b)

16

c)

8

d)

7

75.

If oxygen-18 has 8 protons, then how many neutrons does it have?

a)

9

b)

16

c)

8

d)

10

76.

Fluorine has a mass number of 19. It has 10 neutrons. How many protons does it have?

a)

10

b)

9

c)

8

d)

7

77.

How do you know how many electrons an atom has if you know how many protons it has?

a)

You add them together to equal the atomic number.

b)

There is no way of knowing

c)

You add as many electrons as you need to get to the mass number.

d)

There must be an equal amount of protons and electrons.

78.

How many electrons can the first energy level (s level) hold?

a)
1
b)
2
c)
8
d)
0
79.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
80.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
81.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
82.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
83.

Which would be the correct electron configuration for the silver ion?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d9

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d9

c)

1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p6 5s1 5d9

d)

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d8

84.

What atom matches this electron configuration? 1s22s22p63s23p64s23d8

a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
85.

The 4 orbitals are

a)

s, p, d, f

b)

a, b, c, d

c)

2, 4, 6, 8

86.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
87.

What do you start all electron configurations with?

a)

1s2

b)

1d10

c)

1f14

d)

1p6

88.

What atom matches this electron configuration? [Xe] 6s2

a)
Mercury
b)

Barium

c)
Platinum
d)
Thallium
89.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
90.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
91.

How many electrons can the f sublevel hold?

a)
8
b)
10
c)
2
d)

14

92.

What atom matches this electron configuration? 1s22s22p63s23p1

a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
93.

Which of the following is the correct abbreviated noble gas electron configuration for chlorine?

a)
[Ne]3s23p5
b)
[He]2s22p63s23p5
c)
[Mg]3p5
d)
[Ne]1s22s22p63s23p5
94.

Which would be the correct electon configuration for the ion of Phosphorus?

a)

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

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s3

d)

1s2 2s2 3s2 3p6

95.

What is the abbreeviate noble gas electron for Sulfur atom?

a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
96.

What is the charge of an atom that has gained one electron?

a)
-1
b)
-2
c)
+1
d)
+2
97.

Which would be the correct electron configuration for the Fe+4 ion?

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d3

c)

1s2 2s2 2p6 3s2 3p6 3d4

d)

1s2 2s2 2p6 3s2 3p6 4s1 3d6

98.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
99.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
100.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
101.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
102.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
103.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

104.

Which of the following will have a lower ionization energy than Scandium (Sc)?

a)

Helium (He)

b)

Titanium (Ti)

c)

Calcium (Ca)

d)

Magnesium (Mg)

105.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

106.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

107.

Which group of elements has the lowest ionization energies?

a)

Alkali Metals (Group 1)

b)

Alkaline Earth Metals (Group 2)

c)

Halogens (Group 17)

d)

Noble Gases (Group 18)

108.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

109.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

110.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

111.

What is a positively-charged ion which forms when an atom loses electrons?

a)

atom

b)

ion

c)

cation

d)

anion

112.

What is a negatively-charged ion which forms when an atom gains electrons?

a)

cation

b)

anion

c)

electron

d)

ion

113.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

114.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
115.

Used the word "atomos" to decsribe the uncuttable (indivisible) atom.

a)

Democritus

b)

Thomson

c)

Bohr

d)

Dalton

116.

Proposed that electrons move around the nucleus in specific layers, or shells.

a)

Bohr

b)

Rutherford

c)

Chadwick

d)

Thomson

117.

This picture best represents ___________________ atomic model.

a)

Thomson's

b)

Dalton's

c)

Bohr's

d)

Chadwick's

118.

Which model was created after the discovery of the nucleus?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical

d)

Plum Pudding

119.

Which model was created after the discovery of the electron cloud?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical

d)

Plum Pudding

120.

Which model was created after the discovery of electrons?

a)

Dalton's

b)

Rutherford's

c)

Quantum Mechanical Model

d)

Plum Pudding

121.

What is the correct order of scientists in order of their work related to the atomic theory from earliest to most recent?

a)

Neils Bohr, Ernest Rutherford, JJ Thomson, John Dalton, & Democritus

b)

JJ Thomson, John Dalton, Neils Bohr, Ernest Rutherford, & Democritus

c)

Democritus, John Dalton, JJ Thomson, Ernest Rutherford, and Neils Bohr

d)

John Dalton, Neils Bohr, JJ Thomson, Democritus, & Ernest Rutherford

122.
Ernest Rutherford discovered that the atom was mostly _________________ and has a _______________ charged nucleus.
a)
empty space, positively
b)
empty space, negatively
c)
full of protons, positively
d)
full of neutrons, negatively
123.

This isotope have how many neutrons?

a)

26

b)

12

c)

14

d)

16

124.

Which of the Chlorine [Cl] is heavier?

a)

Cl-37

b)

Cl-35

125.

For Cl 37, what does the 37 represent?

a)

Number of Protons

b)

Number of Neutrons

c)

Number of Electrons

d)

Atomic Mass Number

126.

Which element is located at period 4 group 6? [click the picture to zoom in]

a)

Cr

b)

Sg

c)

Hf

d)

Ta

Similar Resources on Wayground

Review - Reaction Rates

127 questions

Review - Reaction Rates

quiz

Worksheet

•

9th - 12th Grade

LATIHAN PSAT KIMIA XI MIPA 2023-2024

125 questions

LATIHAN PSAT KIMIA XI MIPA 2023-2024

quiz

Worksheet

•

11th Grade

Microbiology

121 questions

Microbiology

quiz

Worksheet

•

12th Grade - University

Pre-Fall Break Review (AME) (Units 1, 2, 3)

125 questions

Pre-Fall Break Review (AME) (Units 1, 2, 3)

quiz

Worksheet

•

9th - 12th Grade

Billings Unit 1 Test Review

121 questions

Billings Unit 1 Test Review

quiz

Worksheet

•

9th - 12th Grade

Gr. 9 Chemistry Revision 1

128 questions

Gr. 9 Chemistry Revision 1

quiz

Worksheet

•

9th - 12th Grade

Physics 1 Review

125 questions

Physics 1 Review

quiz

Worksheet

•

9th - 12th Grade

Anatomy Second Semester Final Practice Test

126 questions

Anatomy Second Semester Final Practice Test

quiz

Worksheet

•

11th - 12th Grade