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2025 Spring Semester Exam Quizizz Review Part I

Total questions: 110

Worksheet time: 2hrs 4mins

Name
Class
Date
1.
What is the first thing you must do to solve a stoichiometry problem?
a)
Write a Balanced Equation
b)
Panic
c)
Write an Unbalanced Equation
d)
Avogadro's Number
2.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
3.
What is the mole ratio of H2O to H3PO4 in the following chemical equation?   P4O10 + 6 H2O --> 4 H3PO4 
a)
6:4
b)
4:6
c)
1:3
d)
3:1
4.
2H2   +   O2  →  2H2O
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
5.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
6.
Fe + S --> FeS
If 7.62g Fe react with 8.67g S, what is the limiting reactant?
a)
Fe
b)
S
c)
FeS
d)
none 
7.
SO2 + PCl5 --> SOCl2 + POCl3
How much SOCl2 is produced when 16.2g SO2 react with 13.7g PCl5? 
a)
7.87g
b)
30.1g
c)
26.4g
d)
19.8g 
8.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
9.

The reaction:

A + B → C

ΔH = + 25 kJ

is a(n):

a)

Exothermic Reaction

b)

Endothermic Reaction

c)

Neutralization Reaction

d)

Spontaneous Reaction

10.
Which is true for this enthalpy diagram?
a)
Exothermic Reaction
b)
Endothermic Reaction
c)
ΔH > 0 kJ
d)
Δ H = 0 kJ
11.

The quantity of heat needed to raise the temperature of 1 g of water by 1 degree celsius-

a)

enthalpy

b)

specific heat

c)

joule

d)

calorie

12.

What would likely happen if you were to touch the flask in which an endothermic reaction were occurring?

a)

The flask would probably feel cooler than before the reaction started.

b)

The flask would probably feel warmer than before the reaction started.

c)

The flask would feel the same as before the reaction started.

d)

none of the above

13.

How can you describe the specific heat of olive oil if it takes approximately 420 J of heat to raise the temperature of 7.0 g of olive oil by 30 degrees?

a)

greater than the specific heat of water

b)

less than the specific heat of water

c)

equal to the specific heat of water

d)

not enough information given

14.

The specific heat of silver is 0.24 J/goC. ow many joules of energy are needed to warm 4.37 g of silver from 25.0oC to 27.5oC?

a)

2.62 J

b)

0.14 J

c)

45.5 J

d)

0.022 J

15.

The ΔH for the following reaction is -1652 kJ/mol. How much energy is involved in the formation of 5.0 g of Fe2O3?

4 Fe + 3 O2 → 2 Fe2O3 -1652kJ/mol

a)

25.9 kJ

b)

25.9 J

c)

66 kJ

d)

66 J

16.

How much energy is needed to change the temperature of 50.0 g of water by 15.0oC?

a)

3.315 J

b)

3135 J

c)

17765 J

d)

17.765 J

17.

The specific heat of aluminum is 0.900 J/goC. How much energy is needed to raise the temperatur eof a 850 g block of aluminum from 22.8oC to 94.6oC?

a)

10654 J

b)

10.654 kJ

c)

54927 J

d)

54.927 K

18.

A piece of metal weighing 59.047 g was heated to 100.0 o C and then submerged into 100.0 g of water(initially at 23.7 o C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 o C. Assuming no heat lost to the environment, calculate the specific heat of the metal.

a)

.356 J/goC

b)

.307 J/goC

c)

.402 J/goC

d)

..684 J/goC

19.

Is the diagram pictured exothermic or endothermic?

a)

exothermic

b)

endothermic

20.

Would the ΔH for the process in this energy diagram have a positive or negative sign?

a)

positive

b)

negative

21.

An endothermic reaction ________________ heat.

a)

releases

b)

absorbs

22.

An exothermic reaction or process is where heat is ____________.

a)

released

b)

absorbed

23.

In a chemical reaction, according to an energy diagram, if more energy is held in the products compared to the energy held in the reactants, then the reaction is termed __________.

a)

exothermic

b)

endothermic

24.

Enthalpy, or ΔH for a process is a positive value if

a)

the reaction is endothermic

b)

the reaction is exothermic

25.

In the following reaction, the heat is listed on the reactant side. This indicates an _________________ reaction.

a)

endothermic

b)

exothermic

26.

Determine the final temperature when a 25.0 g piece of iron at 85.0 °C is placed into 75.0 grams of water at 20.0 °C.

a)

29.4 oC

b)

22.3 oC

27.

Determine the final temperature when 10.0 g of aluminum at 130.0 °C mixes with 200.0 grams of water at 25.0 °C.

a)

26.1 oC

b)

22.4 oC

28.

Determine the temperature change when 20.0 g of water is heated from 16.8 oC to 39.2 oC.

a)

-22.4 oC

b)

22.4 oC

29.

What electromagnetic wave . has . the shortest wavelengths and the highest frequencies?

a)

Gamma Rays

b)

Ultraviolet Rays

c)

Radio Waves

d)

X Rays

30.

What happens to wavelength as the frequency of a wave increases?

a)

increase

b)

stays the same

c)

decreases

d)

becomes faster

31.

The color blue has more energy than the color red.

a)

True

b)

False

32.

what happens to the frequency of a wave as wavelength increases?

a)

increases

b)

decreases

c)

remains constant

d)

diminishes to zero

33.
The shortest wavelength in visible light is______.
a)
violet
b)
red
c)
blue
d)
yellow
34.

The lower the frequency the ______ the energy.

a)

higher

b)

lower

c)

neither, stays the same

35.
The _______________ determines the color of visible light. 
a)
wavelength
b)
speed
c)
amplitude
d)
light
36.
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.
37.
Which drawing represents the process by which an absorption line is formed?
a)
A
b)
B
c)
C
d)
D
38.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
39.
When talking about energy levels in an atom, what is an "excited state"?
a)
The highest energy state of an atom.
b)
Any level higher than the ground state.
c)
The lowest energy state of an atom.
d)
When an atom loses an electron
40.

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

a)

absorbs energy

b)

releases energy

41.
The parallel lines represents...
a)
energy levels of the atom
b)
energy levels of the electrons
c)
energy levels of the photons
d)
energy levels of the nucleus
42.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
43.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
44.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
45.
 The diagram above represents two electrons with 
a)
a. opposite spins.
b)
 b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
46.
What is the correct noble-gas notation for the electron configuration of an atom of chlorine? 
a)
a. [Ar]3s2 3p5
b)
 b. [Ne]3s2 3p4
c)
 c. [Ar]3s2 3p4
d)
 d. [Ne]3s2 3p5
47.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
48.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
49.
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
50.

How many electrons can the p sublevel hold?

a)

14

b)

10

c)

2

d)

6

51.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
52.

How many electrons does an atom with 8 protons have (assuming the atom is neutral)?

a)

8

b)

16

c)

15.99

d)

24

53.
The blue section of the wave is measuring _________________.
a)
wavelength
b)
crest
c)
trough
d)
amplitude 
54.

What element has this orbital notation?

a)

lithium

b)

beryllium

c)

boron

d)

carbon

55.

What element has this electron configuration?

a)

helium

b)

lithium

c)

beryllium

d)

boron

56.

Which element is represented by this orbital notation?

a)

carbon

b)

nitrogen

c)

oxygen

d)

fluorine

57.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
58.
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
59.

Which orbital has the least amount of energy?

a)

p orbital

b)

d orbital

c)

s orbital

d)

What is an orbital?

60.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
61.

What is the Aufbau principle?

a)

Within an energy level, s orbitals are the lowest energy, followed by p, d and then f. F orbitals are the highest energy for that level.

b)

The lower the principal quantum number (n) the lower the energy.

c)

All three.

d)

The Aufbau Principle states that electrons enter the lowest energy orbitals first.

62.

Which rule is violated in the following orbital diagrams?

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli's Exclusion Principle

63.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
64.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
65.

CO2 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

e)

4

66.

NH3 has how many lone pairs?

a)

0

b)

1

c)

2

d)

3

67.

How many valence electrons does Nitrogen 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 Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

69.

How many valence electrons does Aluminum Have?

a)

1 Valence electron

b)

2 Valence electron

c)

3 Valence electron

d)

4 Valence electron

e)

5 Valence electron

70.
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
71.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
72.

CCl4 has how many double bonds?

a)

0

b)

1

c)

2

d)

3

73.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
74.
Three pairs of electrons are shared in a
a)
Single bond
b)
Double bond
c)
Triple bond
75.

What is the correct structure for BF3?

a)

Option A.

b)

Option B.

c)

Option C.

d)

Option D.

76.

What is ionic bonding?

a)

Bonding that is the result of two elements sharing electrons

b)

Bonding involving only one atom

c)

Bonding that is the result of an exchange of electrons between a metal and a nonmetal

d)

Bonding between two metals

77.

What is Covalent Bonding?

a)

Bonding that is the result of two nonmetals sharing electrons

b)

Bonding between two metals

c)

Bonding that is the result of a nonmetal and a metal exchanging electrons

d)

Bonding between more than two elements

78.

Which particle is responsible for bonding?

a)

Protons

b)

Electrons

c)

Neutrons

d)

Nucleus

79.

This Lewis Dot Structure for water is correct

a)

True

b)

False

80.

Which of the following is true about Ionic Bonds? (select ALL TRUE options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

81.

Which of the following is true about Covalent (non-polar) bonds? (select ALL true options)

a)

High melting point

b)

Low melting point

c)

Can dissolve in water

d)

Cannot dissolve in water

e)

Can conduct electricity

82.

Potassium Chloride is...

a)

Ionic

b)

Covalent

83.

Water (H2O) is...

a)

Ionic

b)

Covalent

84.

Potassium Sulfate (K2SO4) is...

a)

Ionic

b)

Covalent

85.

Ammonium (NH4) is...

a)

Ionic

b)

Covalent

86.

The correct name for CH4 is...

a)

Carbon Hydrogen

b)

Carbon Tetrahydride

c)

Monocarbon hydride

d)

Carbon Hydride

87.

What is the correct formula for Calcium Oxide?

a)

CaO

b)

Ca2O

c)

CaO2

d)

CaO3

88.

What is the correct formula for Carbon Dioxide?

a)

C2O2

b)

CO2

c)

C2O

d)

CO3

89.
Have a high m.p. (1000°C-3000°C)
a)
ionic compounds
b)
covalent compounds
90.
Have a low m.p. (< 200°C)
a)
ionic compounds
b)
covalent compounds
91.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
92.
usually hard but brittle
a)
ionic compounds
b)
covalent compounds
93.
forms ions in solution
a)
ionic compounds
b)
covalent compounds
94.
electrolytes
a)
ionic compounds
b)
covalent compounds
95.

Compounds composed of a ______________ and _____________ like the compound CaCl2 , are ionic compounds.

a)

metal ... metal

b)

nonmetal ... nonmetal

c)

metal ... nonmetal

96.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
97.

Which of the following describes covalent bonds?

a)

Bonds form because of opposite charges

b)

electrons are shared to fill outer electron shells

c)

Electrons are transferred between atoms

d)

Covalent bonds are magical

98.

What set of elements is most likely to form a covalent compound?

a)

Na and O

b)

Na and K

c)

O and C

99.

Which element is most likely to form 4 bonds?

a)

Carbon

b)

Fluorine

c)

Sulfur

d)

Nitrogen

100.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

101.

Is this molecule polar or non-polar?

a)

Polar

b)

Non-polar

102.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

103.

Is this molecule polar or non-polar?

a)

Non-polar

b)

Polar

104.
In covalent bonds, electrons are ___________.
a)
transferred
b)
gained
c)
lost
d)
shared
105.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
106.
In this Lewis structure, the symbol above F means...
a)
electrons are being transferred to Fluorine
b)
electrons are less attracted to F than H
c)
electrons are more attracted to F than H
d)
Fluorine has formed a cation
107.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
108.
What geometry will this molecular structure have?: PH3
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
109.
What geometry will this molecular structure have?: H2S
a)
bent
b)
tetrahedral
c)
linear
d)
trigonal pyramidal
110.
Will this molecule be polar or nonpolar? H2S
a)
polar
b)
nonpolar

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