wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Super Review Chem Semester 1

Total questions: 129

Worksheet time: 43mins

Name
Class
Date
1.

What is the nucleus of an atom made of?

a)

Protons & electrons

b)

Protons & neutrons

2.

The nucleus of an atom makes up _____ of its mass.

a)

50%

b)

99.9%

3.

What is the relationship between the size of the nucleus and the size of the atom?

a)

The nucleus is about 100,000 times smaller than the atom.

b)

The nucleus is twice as big as the atom.

4.

Neutrons have __________ charge.

a)

positive

b)

no

5.

Protons have __________ charge.

a)

no

b)

positive

6.

Electrons have __________ charge.

a)

negative

b)

no

7.

Which particle has almost no mass?

a)

Electrons

b)

Protons

8.

What does amu stand for?

a)

Atomic mass unit

b)

Atom matter unit

9.

Which best describes the movement of electrons?

a)

They move slowly.

b)

They are constantly moving.

10.

Most of the atom is empty space.

a)

True.

b)

False.

11.

Thompson was the first to discover a subatomic particle - the electron. What are the others?

a)

protons & neutrons

b)

protons & positrons

12.

Rutherford concluded that the amount of positive charge varies

a)

with different elements.

b)

with the amount of neutrons in the nucleus.

13.

A positively charged particle found in the nucleus is called a

a)

neutron.

b)

proton.

14.

The word "proton" comes from an ancient Greek word meaning

a)

to change or become flexible.

b)

proteus.

15.

The word "electron" comes from the ancient Greek word meaning

a)

electricity.

b)

amber.

16.

Electrons can best be described as having a

a)

large size, negative charge.

b)

very small size, negative charge.

17.

Electrons are subatomic particles that exist

a)

in simultaneous dimensions.

b)

outside the nucleus.

18.

Neutrons (discovered by James Chadwick in 1932) are neutral subatomic particles that are located

a)

in the nucleus.

b)

in alternate universes.

19.

Neutrons have almost exactly the same mass as

a)

protons.

b)

quarks.

20.

Only protons & neutrons can be distinguished by mass, charge and position in an atom.

a)

True

b)

False

21.

James Dalton proved that the true nature of the atom could best be described as resembling "plum pudding."

a)

True

b)

False

22.

Rutherford proved the existence of protons located in a very small nucleus by using a crude particle accelerator in 1911.

a)

True

b)

False

23.

The atomic number (#) of an element is equal to the

a)

# of protons in a single atom of that element.

b)

weight of an electron.

24.

Atoms of different elements have

a)

the same # of protons.

b)

a different # of protons.

25.

Because atoms are neutral, each positive charge is

a)

the same as no charge.

b)

balanced by a negative charge.

26.

Which statement best describes the mass number (#) of an atom?

a)

the difference in mass between protons & neutrons

b)

the sum of protons & neutrons in the nucleus

27.

If you know the atomic number (or # of protons) and mass number of an atom, you can find the

a)

number of electrons by adding to the mass number.

b)

number of neutrons by subtracting from the mass number.

28.

If the atomic mass of an element is 32 and the atomic # is 16, then

a)

the number of neutrons is also 16.

b)

the element most likely has isotopes.

c)

the number of electrons is also 16.

d)

the number of protons is also 32.

29.

Every neutral atom has the same number of protons and electrons, however

a)

they may also have the same atomic mass.

b)

they may not have the same # of neutrons.

30.

Which statement best describes an isotope of an element?

a)

they share an equal amount of neutrons

b)

they have the same atomic #'s but with different mass #'s

31.

What is the subatomic particle that has a negative charge?

a)

Neutrons

b)

Electrons

32.

What is the image a picture of?

a)

Pierre Model

b)

Bohr Model

33.

What subatomic particles are located in the nucelus?

a)

Electrons

b)

Protons

34.

_________ has a positive charge.

a)

Neutrons

b)

Protons

35.

What subatomic particle has a 0 charge?

a)

Neutrons

b)

Electrons

36.

What is the basic unit of matter?

a)

Subatomic Particles

b)

Atom

37.

The center of an atom is called the (a)   .

38.

True or False: Protons and Neutrons are always the same number

a)

True

b)

False

39.

True or False: Protons and Electrons are equal to the atomic number.

a)

True

b)

False

40.

The scientist(s) that is repsonsible for the Solid Sphere Model is

a)

JJ Thompson

b)

John Dalton

41.

The scientist(s) that is repsonsible for the Plum Pudding Model is

a)

JJ Thompson

b)

Schordinger & Heisenberg

42.

The scientist(s) that is repsonsible for the Electron Cloud Model is

a)

Schordinger & Heisenberg

b)

JJ Thompson

43.

The scientist(s) that is repsonsible for the Planetary Model is

a)

Niels Bohr

b)

Ernest Rutherford

44.

The results of the Gold Foil Experiment led Rutherford to discover

a)

that the nucleus is positively charged

b)

that the atom is a solid sphere

c)

that the atom is mostly empty space

d)

that electrons exist

45.

During the gold foil experiment, postively charged particles (alpha particles) were shot at an atoms thick piece of gold. What was observed?

a)

Most of the alpha particles went straight through but a few bounced back

b)

All of the alpha particles bounced back

46.

The results of the Cathode Ray Tube experiment led Thompson to believe

a)

The atom is an electron cloud

b)

The atom is a positively charged particle with negative electrons distributed through out

47.

During the Cathode Ray Tube experiment the beam bent towards the magnet's positive side. This meant that the beam was

a)

Positively charged

b)

Negatively charged

c)

Neutrally charged

d)

No Charge was observed.

48.

The Electron Cloud Model of an atom

a)

is a mathematical representation of the possible location of electrons around the nucleus.

b)

tells us the exact location of an electron and its speed at the same time.

49.

The solid sphere model was developed

a)

because no one could come up with a better idea.

b)

by Dalton experimenting with different substances and gasses and noticing patterns

50.

The image shows the

a)

Solid Sphere Model

b)

Plum Pudding Model

c)

Planetary Model

d)

Bohr Model

e)

Electron Cloud Model

51.

The image shows the

a)

Solid Sphere Model

b)

Plum Pudding Model

c)

Planetary Model

d)

Bohr Model

e)

Electron Cloud Model

52.

The image shows the

a)

Solid Sphere Model

b)

Plum Pudding Model

c)

Planetary Model

d)

Bohr Model

e)

Electron Cloud Model

53.

The image shows the

a)

Solid Sphere Model

b)

Plum Pudding Model

c)

Planetary Model

d)

Bohr Model

e)

Electron Cloud Model

54.

The image shows the

a)

Solid Sphere Model

b)

Plum Pudding Model

c)

Planetary Model

d)

Bohr Model

e)

Electron Cloud Model

55.

Electrons that have not been excited are said to be at:

a)

high level

b)

base line

c)

set state

d)

ground state

56.

This shape is that of a...

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

57.

This is a ____ orbital

a)

s

b)

d

c)

p

d)

d

58.

The principle quantum number, n, represents the:

a)

spin value

b)

suborbital value

c)

energy level

d)

magnetic value

59.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

60.

With each higher energy level, the electrons are

a)

lower in energy

b)

more stable

c)

weaker

d)

farther from the nucleus

61.

How many electrons total are found in the f orbital?

a)

2

b)

6

c)

10

d)

14

62.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

63.

How many electrons are in 1s2 2s2 2p4?

a)

5

b)

6

c)

8

d)

13

64.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
65.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
66.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
67.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
68.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
69.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
70.
What is incorrect about this orbital diagram?
a)
Both arrows in the 2p box should be pointing up
b)
There is nothing incorrect with this diagram
c)
In the 2p box there should only be 1 electron in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
71.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
72.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
73.

Identify the rule that is being violated

a)

Aufbau's Principle

b)

Hund's Rule

c)

Pauli's Exclusion Principle

d)

Heisenberg uncertainty principle

74.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
75.

Which is the electron configuration of Ar (Argon)

a)

1s2 2s2 2p6 3s2 3p6

b)

1s2 2s2 2p6 3s2 3p0

c)

1s2 2s2 3s2 4s2 4p6

d)

3s2 4f14 4s2

76.

1s22s22p63s23p64s23d6

a)

cobalt

b)

iron

c)

copper

d)

zinc

e)

manganese

77.

In 1s2, the 1 means

a)

there is 1 electron

b)

the electrons are in the 1st energy level

c)

the shape is circular

d)

there is a -1 charge

78.

In 1s2, the s means

a)

the shape of the orbital is circular

b)

the shape of the orbital is figure 8

c)

there are six electrons

d)

it is neutral

79.

In 1s2, the 2 means

a)

there are 2 electrons in this level

b)

it is the 2nd energy level

c)

there is a +2 charge

d)

there is a -2 charge

80.

Cr (Z=24) shows anomalous electronic configuration.

The actual electronic configuration is

1s2 2s2 2p6 3s2 3p6 4s1 3d5.

This is because ...

a)

the half-filled d-orbital (3d5) is more stable

b)

the completely filled d-orbital (3d10) is more stable

c)

the partially filled d-orbital (3d4) is more stable

81.
This is the correct dot diagram for sodium (Na)
a)
true
b)
false
82.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
83.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
84.

What are valence electrons?

a)

The innermost electrons

b)

The outermost electrons

85.

What is the octet rule?

a)

Elements can only have 8 electrons in its outermost shell

b)

The elements must form an octopus like structure

86.

How many valence electrons does Carbon have

a)

1

b)

4

87.

How many valence electrons does Argon have

a)

8

b)

11

88.

Electron dot notation is . . . .

a)

A representation of an element in which only valence electrons of an atom are shown

b)

A representation of how compounds are formed.

89.
How many electrons should Helium have around its Lewis dot model?
a)
1
b)
2
c)
7
d)
8
90.

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

a)

1

b)

2

c)

3

d)

4

91.
Electronegativity is...
a)
how good an atom is at attracting electrons
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. 
92.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
93.

Which statement correctly and completely identifies a trend?

a)

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

b)

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

94.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
95.
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.
96.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
97.

As you move down a group, atomic radius increases because - 

a)

you add more and more neutrons

b)

you add more and more shells (energy levels)

98.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
99.

Francium (Fr) has the lowest ionization energy in Group 1 because - 

a)

it has the smallest number of valence electrons

b)

its 1 valence electron is very far from the nucleus, so little energy is needed to remove it

100.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
101.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

102.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

103.

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)

104.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

105.

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)

106.
Iron
a)
Ir
b)
I
c)
Fe
d)
Fn
107.
Argon
a)
A
b)
Ag
c)
An
d)
Ar
108.
Iodine
a)
Id
b)
Io
c)
I
d)
Ii
109.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

110.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
111.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
112.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
113.

What element is in period 3 group 18, 8A?

a)

Aluminum

b)

Potassium

c)

Argon

d)

Neon

114.

How many valence electrons does this element have?

a)

20

b)

2

c)

4

d)

1

115.

The horizontal (left to right) rows on the periodic table are known as

a)

periods.

b)

atoms.

c)

groups or families.

d)

valence electrons.

116.

Using the element picture, what is the atomic number?

a)

1

b)

H

c)

Hydrogen

d)

1.00794

117.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
118.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
119.

Which of the following elements has the best physical properties to be a good conductor of energy?

a)

Carbon (C)

b)

Chlorine (Cl)

c)

Iron (Fe)

d)

Neon (Ne)

120.

Sodium (Na) is found in period

a)

3

b)

2

c)

4

d)

1

121.

The Alkali Metals are group _____ on the periodic table.

a)

2

b)

6

c)

3

d)

1

122.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
123.
How many significant figures does the following number have: 100.3
a)
4
b)
3
c)
5
d)
2
124.
Round 1009 to three sig figs
a)
100
b)
101
c)
1010
d)
1000
125.

What is 20,300,000 in scientific notation?

a)

2.03×1072.03\times10^7

b)

20.3×10720.3\times10^7

c)

2.03×1062.03\times10^6

d)

20.3×10620.3\times10^6

126.

What is 0.00051 in scientific notation?

a)

5.1×10−45.1\times10^{-4}

b)

5.1×1045.1\times10^4

c)

5.1×10−35.1\times10^{-3}

d)

5.1×1035.1\times10^3

127.

What is 99,010,000,000 in scientific notation?

a)

9.901×10109.901\times10^{10}

b)

9.901×10−109.901\times10^{-10}

c)

9901×1079901\times10^7

d)

9.901×1099.901\times10^9

128.

What does kilo mean?

a)

10310^3

b)

10−310^{-3}

c)

10−610^{-6}

d)

10−210^{-2}

129.

How many grams is 400 kilograms?

a)

4×1054\times10^5  

b)

4×1034\times10^3  

c)

4×10−34\times10^{-3}  

d)

4×10−54\times10^{-5}  

Similar Resources on Wayground

Periodic Table Skills Review

125 questions

Periodic Table Skills Review

quiz

Worksheet

•

10th - 11th Grade

UNIT 1: Chemistry FUNdamentals

130 questions

UNIT 1: Chemistry FUNdamentals

quiz

Worksheet

•

10th Grade

Stoichiometry Quiz

126 questions

Stoichiometry Quiz

quiz

Worksheet

•

9th - 12th Grade

Q2 H. Chem Final Review 23-24

125 questions

Q2 H. Chem Final Review 23-24

quiz

Worksheet

•

9th - 12th Grade

PSci Unit 4: Compounds

125 questions

PSci Unit 4: Compounds

quiz

Worksheet

•

11th Grade

Chemistry Matter Check for Understanding

131 questions

Chemistry Matter Check for Understanding

quiz

Worksheet

•

9th - 12th Grade

Chemistry Unit 1 GSE

124 questions

Chemistry Unit 1 GSE

quiz

Worksheet

•

10th - 12th Grade

Repaso Actividades 1,2,3,4,5,6,7,8,9 y 10 AD19 Química

125 questions

Repaso Actividades 1,2,3,4,5,6,7,8,9 y 10 AD19 Química

quiz

Worksheet

•

12th Grade