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Chemistry 1st Semester Exam Review

Total questions: 145

Worksheet time: 2hrs 5mins

Name
Class
Date
1.

(a)   is the study of the composition, structure, and properties of matter.

2.

(a)   are the building blocks of all things. They are the smallest unit of an element that retains the identity and properties of that element.

3.

Chemistry is a ____________________ science.

a)

physical

b)

social-behavioral

c)

political

d)

pseudo

4.

(a)   chemistry is the study of most carbon-containing compounds.

5.

(a)   is the study of the processes and substances occurring in living things.

6.

A (a)   is any substance with a definite composition.

7.

(a)   is research performed for the sake of knowledge itself.

8.

(a)   is the use of applied and basic research to produce goods for consumer use.

9.

All matter has ________________ and _____________________.

a)

mass

b)

volume

c)

color

d)

weight

e)

scent

10.

A(n) ______________________ cannot be broken down into smaller, stable parts.

a)

element

b)

compound

c)

molecule

d)

chemical

11.

A (a)   can be broken down into smaller, stable parts.

12.

A (a)   mixture is made when substances are evenly distributed throughout the mixture.

13.

(a)   properties are dependent on the amount of the substance present.

14.

__________________________ properties are related to the ability of a substance to undergo change.

a)

chemical

b)

physical

15.

Ice melting into water is an example of a...

a)

physical change

b)

chemical change

16.

Matter in the (a)   state has definite shape and definite volume.

17.

Matter in the (a)   state is in a high energy state where it has lost its electrons.

18.

Wood burning is an example of a _____________________ change.

a)

chemical

b)

physical

19.

All pure substances are ____________________.

a)

heterogeneous

b)

homogeneous

20.

What is the atomic number of Nitrogen?

(a)  

21.

I hand you a substance which is lustrous and conducts heat very well. What is it?

a)

A metal

b)

A nonmetal

c)

A metalloid

d)

A noble gas

22.

I show you a substance that does not react with other substances. What is it?

a)

A noble gas

b)

a metal

c)

a metalloid

d)

a nonmetal

23.

Group 18 elements are called (a)   gases.

24.

Malleability is a characteristic of (a)   .

25.

Starting substances in a reaction are called...

(a)  

26.

Factors in an experiment that do not change are called ______________________.

a)

controls

b)

variables

c)

experimental

d)

globular

27.

Once enough data is collected to back up a hypothesis, with rigorous testing and repeated confirmation of the hypothesis, the hypothesis becomes a _________________.

a)

theory

b)

law

c)

textbook

d)

discipline

28.

Mass is how much stuff is present. ____________________ is how much gravitational force acts on that matter.

a)

weight

b)

volume

c)

density

d)

terminal velocity

29.

Convert:

81 kg to grams

(a)  

30.

Convert:

22 mg to grams

(a)  

31.

_____________________ refers to the closeness of measures to the accepted value.

a)

accuracy

b)

precision

32.

Write 2.5×1072.5\times10^7 in expanded form.



(a)  

33.

8.2×10n=82 000 000 000 0008.2\times10^n=82\ 000\ 000\ 000\ 000 .
What is n?

(a)  

34.

(3.1×104)×(2.8×106)\left(3.1\times10^4\right)\times\left(2.8\times10^6\right)  

a)

8.68×10108.68\times10^{10}  

b)

8.68×1028.68\times10^2  

c)

5.9×10105.9\times10^{10}  

d)

2.83×1062.83\times10^6  

35.

The SI Unit for temperature is...

(a)  

36.

The first step in the scientific method is to...

a)

ask a question

b)

form a hypothesis

c)

make an observation

d)

perform an experiment

37.

A testable statement is called a...

(a)  

38.

A theory explains why a phenomenon happens, whereas a

__________________ describes the phenomenon.

a)

law

b)

hypothesis

c)

guess

d)

postulate

39.

True or False:

The Imperial System is the system scientists use to communicate measurements.

a)

True

b)

False

40.

(a)   data is descriptive and tells the characteristics of the system we are studying.

41.

(a)   are often used to communicate theories, explaining how a phenomenon works and how data or events are related.

42.

(a)   are the SI unit for the intensity of light.

43.

(a)   is a derived unit of length, width, and height multiplied together.

44.

(a)   is a derived SI unit with mass divided by volume.

45.

(2.8×105)+(1.5×106)\left(2.8\times10^5\right)+\left(1.5\times10^6\right)  

a)

1.78×1061.78\times10^6  

b)

4.4×1054.4\times10^5  

c)

1.78×10−61.78\times10^{-6}  

d)

4.4×10114.4\times10^{11}  

46.

First person to propose the concept of an atom

a)

Rutherford

b)

Democritus

c)

Dalton

d)

Bohr

47.

These particles are found in the nucleus

a)

protons and electrons

b)

nucleus and neutrons

c)

protons and neutrons

d)

electrons and neutrons

48.

Rutherford experimented with ____

a)

Gold foil and alpha particles

b)

Cathode rays and alpha particles

c)

electron and alpha particles

d)

gold foil and cathode rays

49.

Thomson Experimented with ______

a)

Gold Foil

b)

alpha particles

c)

cathode rays

d)

protons

50.
Which scientist developed the atomic theory?
a)
JJ Thomson
b)
Ernest Rutherford
c)
John Dalton
d)
James Chadwick
51.

Subatomic particles with a negative charge

a)

Electrons

b)

Neutrons

c)

Protons

d)

Quarks

52.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
53.
Subatomic particles that are neutral in charge
a)
Neutrons
b)
Protons
c)
Nucleus 
d)
Electrons
54.
Where electrons are likely to be found as they travel around the nucleus
a)
Nucleus
b)
Electron Cloud
c)
Within a Proton
d)
Within a Neutron
55.

John Dalton stated:

a)

Atoms are tiny, invisible particles.

b)

Atoms of one element are all the same.

c)

Atoms of different elements are different.

d)

Compounds form by combining atoms.

e)

All of the statements listed.

56.

What is the smallest unit of matter? It is composed of protons and neutrons, held together in the nucleus, and electrons around the nucleus in different electron orbitals, which form an electron cloud.

a)

cell

b)

nucleus

c)

atom

d)

electron

57.

What is the number of protons in the nucleus of an atom that determines the chemical properties of an atom?

a)

mass number

b)

atomic mass

c)

atomic number

d)

atomic symbol

58.

What is the mass number?

a)

the number of protons in the nucleus

b)

the number of protons and neutrons in the nucleus

c)

the number of neutrons in the nucleus

d)

the number of protons and electrons in the atom

59.

Protium, Deuterium and Tritium are isotopes of the element Hydrogen.


Why does Tritium have a greater mass number than both Protium and Deuterium?

a)

It has more protons

b)

It has more neutrons

c)

It is electrically neutral

d)

It has more electrons

60.

What is the mass number of an atom that contains 9 protons, 10 neutrons, and 9 electrons?

a)

9

b)

10

c)

18

d)

19

61.

What is true about the carbon atom depicted in the image?

a)

This carbon atom has 13 protons

b)

There are 13 subatomic particles in the electron cloud

c)

The mass number of this carbon atom is 13

d)

The atomic number of this carbon atom is 13

62.

All the isotopes of a particular element will always have the same -

a)

Atomic number

b)

Mass number

c)

Number of neutrons

d)

Total number of subatomic particles

63.

These three isotopes of carbon have different -

a)

Atomic numbers

b)

Mass numbers

c)

Numbers of protons

d)

Symbols

64.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
65.
What is the mass of one mole of aluminum?
a)
26.982 g
b)
13 g
c)
53.985 g
d)
14 g
66.
How many moles are in 16.94g of water?
a)
16.94
b)
0.9403
c)
305.2
d)
1.063
67.
What is Avogadro's Number?
a)
6 x 1023
b)
6 x 103
c)
600
d)
6.0
68.
How many moles are in 6 x 1023 molecules of H2O?
a)
1
b)
2
c)
6
d)
600
69.

The mass of one mole of an element is equal to

a)

its atomic number from the periodic table, but in amus.

b)

its atomic mass from the periodic table, but in amus.

c)

its atomic mass from the periodic table, but in grams.

d)

its atomic number from the periodic table, but in grams.

70.

What is the mass of 1.2 x 1024 atoms of C?

a)

2.0 grams

b)

24 grams

c)

0.17 grams

d)

1.4 x 1025 grams

71.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
72.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
73.
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 there should only be 1 orbital in the first 2p box and one in the 2nd 2p box
d)
All the arrows should be pointing up.
74.
The blue section of the wave is measuring _________________.
a)
wavelength
b)
crest
c)
trough
d)
amplitude 
75.

Electrons fill energy levels and sublevels _____ in energy first.

a)

lower

b)

higher

76.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
77.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
78.
Which orbital shows a violation of the Pauli Exclusion Principle?
a)
A
b)
B
c)
C
d)
D
79.

Which shows the correct orbital diagram for Cobalt?

a)
b)
c)
d)
80.

What element's orbital notation is pictured here?

a)

Ar

b)

Br

c)

Cu

d)

Cl

81.
Which letter represents wavelength?
a)
A
b)
B
c)
C
d)
D
82.
Which wave has a greater frequency?
a)
A
b)
B
83.

If a wave has a greater frequency, what happens to the wavelength?

a)

increases

b)

decreases

c)

stays the same

84.

If a wave has a greater frequency, what happens to number of waves per second?

a)

increases

b)

decreases

c)

stays the same

85.

What property does the orange arrow (A) represent?

a)

Crest

b)

Trough

c)

Wavelength

86.

What property does the green arrow (B) represent?

a)

Crest

b)

Trough

c)

Wavelength

87.
In a vacuum, all electromagnetic waves have the same
a)
wavelength
b)
frequency
c)
speed
d)
amplitude
88.
which of the following does NOT belong in the electromagnetic spectrum:
a)
X-ray
b)
sound wave
c)
ultra violet rays
d)
microwaves
89.
The distance from one point to the next corresponding point on a wave is called the ________________.
a)
waveform
b)
peak
c)
amplitude
d)
wavelength
90.
Which kind of wave has the greatest frequency?
a)
gamma rays
b)
infrared
c)
ultraviolet
d)
microwaves
91.

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

92.

Who proposed that electrons are only found in specific, discrete circular orbits around the nucleus?

a)

Albert Einstein

b)

Erwin Schrodinger

c)

Ernest Rutherford

d)

Niels Bohr

93.

Who used theoretical calculations and experimental results to devise and solve a mathematical equation describing the behavior of the electron in a hydrogen atom?

a)

JJ Thomson

b)

Niels Bohr

c)

Erwin Schrodinger

d)

James Chadwick

94.

If n = 3, what is the maximum number of electrons that can fit in this shell?

a)

2

b)

8

c)

18

d)

32

95.

How many d orbitals make up the d subshell?

a)

1

b)

5

c)

3

d)

7

96.

What orbital is shown in the picture?

a)

s orbital

b)

p orbital

c)

d orbital

d)

f orbital

97.

What is the difference in a 1s orbital and a 2s orbital?

a)

The shape of the orbital

b)

The size of the orbital

c)

The number of electrons it can hold

d)

None of the above

98.

Which quantum number represents the shape of the orbital?

a)

principal quantum number

b)

azimuthal (angular momentum) quantum number

c)

magnetic quantum number

d)

spin quantum number

99.

What states that every orbital of a subshell must be singly occupied before any orbital can have a pair?

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau principle

d)

None of the above

100.

This states that no two electrons will have the same 4 quantum numbers in an atom or molecule. The two electrons of the same orbital must have opposite spin states.

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau principle

d)

None of the above

101.

What states that electrons fill the lowest energy orbitals/levels first before occupying higher energy levels?

a)

Pauli exclusion principle

b)

Hund's rule

c)

Aufbau Principle

d)

None of the above

102.

How many electrons can be held in the first energy level?

a)

2

b)

8

c)

6

d)

10

103.

How many energy levels are currently present on the periodic table?

a)

18

b)

7

c)

6

d)

4

104.

How many orbitals are there in a p-sublevel?

a)

1

b)

3

c)

5

d)

7

105.

What sublevels are present in the 5th energy level of an atom?

a)

s

b)

p and d

c)

d and f

d)

s p and d

e)

s p d and f

106.

How many orbitals are there in a d-sublevel?

a)

10

b)

6

c)

3

d)

5

107.

Magnesium is placed in the ____ energy level on the periodic table.

a)

1st

b)

5th

c)

3rd

d)

24th

e)

12th

108.

The area on the far right of the periodic table is known as the ____ block.

a)

s

b)

p

c)

d

d)

f

109.

The f-block on the periodic table can hold ___ elements.

a)

3

b)

6

c)

18

d)

14

e)

10

110.

Which sublevels are present in n=3?

a)

s

b)

s and p

c)

s and d

d)

s p d and f

e)

s p and d

111.

How many total electrons can fit in the d-sublevel?

a)

2

b)

18

c)

10

d)

14

112.

How many atoms are in a single row of the p-block of the periodic table?

a)

1

b)

3

c)

10

d)

5

e)

6

113.

Electrons prefer to be in...

a)

third energy level

b)

highest energy level

c)

2nd energy level

d)

lowest possible energy level

114.

How many electrons could fit in a HALF full d-sublevel?

a)

2

b)

10

c)

5

d)

6

115.

Bohr's model of the atom is sometimes called the planetary model. If the atoms is like a solar system, what is analogous to the sun?

a)

energy levels

b)

electrons

c)

neutrons

d)

the nucleus

116.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

117.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
118.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
119.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
120.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
121.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
122.

I am a metal


I am in group 2


I am in period 6


I am…

a)

Mo

b)

Re

c)

S

d)

Ba

123.

I am a nonmetal


I am in period 2


I am in group 16/6A

a)

Ba

b)

Si

c)

Ba

d)

O

124.

Find an element with similar chemical properties to Barium (Ba).

a)

Ca an Ra, because they are in the same group and have similar chemical properties.

b)

Cs and La, b/c they are in the same period number.

c)

Ca and Y, b/c they are 90 degree angle and have similiar properties.

125.
Why were there blank spaces left in Mendeleev's periodic table?                                              
a)
He didn't know what to put there.
b)
 Undiscovered elements not yet known.
c)
Multiple elements could have fit
d)
He forgot to add the elements in.
126.
_______________ developed the first periodic table and arranged the elements in order of increasing atomic mass.
a)
Stevie Wonder
b)
Sasha Vujacic
c)
Dmitri Mendeleev
d)
James Mosely
127.
Mendeleev classified elements based on not only atomic mass but what else?                                                   
a)
reactivity
b)
boiling points
c)
physical properties only 
d)
 chemical & physical properties
128.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
129.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
130.
What does the C represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
131.

Periodic law states that the elements are arranged according to their atomic ________ so that elements with similar chemical properties are in the same ________ and properties repeat periodically.

a)

numbers, rows

b)

masses, rows

c)

masses, column

d)

numbers, column

132.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

133.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

134.

Which element has similar chemical properties as sodium but has 7 energy levels?

a)

Francium (Fr)

b)

Cesium (Cs)

c)

Rubidium (Rb)

d)

Potassium (K)

135.

Find these groups: Locate Lanthanides and Actinides.

a)
b)
c)
d)
136.
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
137.
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
138.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
139.
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.
140.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
141.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
142.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
143.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
144.
Which particles change the charge in atoms when ions are formed?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Kittens
145.
How many total electrons does Mg+2 (a magnesium ion) have?
a)
10
b)
12
c)
14
d)
22

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