wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

2024 Chem I spring review

Total questions: 93

Worksheet time: 2hrs 20mins

Name
Class
Date
1.
What color has the shortest wavelength, or the highest frequency?
a)
yellow
b)
blue
c)
red
d)
violet
2.
Which of the following types of radiation has the shortest wavelength and the highest frequency?
a)
Radio Waves
b)
Infrared
c)
Visible
d)
X-Rays
3.

The lines in the emission spectrum for hydrogen are formed from ___.

a)

energy given off when the electron moves from higher energy levels to lower energy levels

b)

electrons given off as hydrogen burns

c)

protons given off when protons move from higher energy levels to lower energy levels

d)

electrons given off as hydrogen cools

4.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
5.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
6.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
7.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
8.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
9.
A covalent bond is
a)
a bond that shares electrons metallicaly
b)
A bond that shares electrons with non metals
c)
Metalloids bonding
d)
metals and nonmetals bonding
10.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
11.

a collection of atoms of one type that cannot be broken down into simpler substances by ordinary chemical or physical means

a)

element

b)

subatomic particle

c)

electron

d)

matter

12.

the positively charged subatomic particle contained in the nucleus of an atom

a)

proton

b)

neutron

c)

electron

d)

matter

13.
An element's identity is determined by the number of
a)
electrons.
b)
protons.
c)
neutrons.
d)
valence.
14.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
15.
An element is made up of only one kind of _____.
a)
isotope
b)
plastic
c)
atom
d)
metal
16.
An atom of the element with atomic number 6 always has _____.
a)
six protons in its nucleus
b)
an atomic mass of six
c)
more than six neutrons
d)
six electron clouds
17.
Electronegativity is the...
a)
energy needed to remove the outermost electron.
b)
ability of an atom to attract electrons from another atom.
18.
What elements generally make an ionic bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
19.
What elements generally make a covalent bond?
a)
metal and nonmetal
b)
2 nonmetals
c)
metal
d)
none of the above
20.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
21.
What happens when an atom loses an electron?
a)
It becomes Negatively Charged
b)
It remains neutral because the proton also leaves.
c)
It becomes Positively Charged
d)
It stays the same.
22.
The number of _____ is most important in determining how an atoms will bond. 
a)
Neutrons
b)
Protons
c)
Valence Electrons
d)
Electron sin the innermost shell
23.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
24.
High Melting & Boiling Points
a)
Ionic
b)
Covalent
25.
What type of bond is formed when electrons are transferred (stolen, or given) from one atom to another?
a)
Ionic Bond
b)
Covalent Bond
c)
Metallic Bond
d)
Acidic Bond
26.

What is the number of valence electrons for Neon and the other Noble Gases?

a)

5

b)

6

c)

7

d)

8

27.
What ending is used for the names of negative ions formed when atoms gain (steal) electrons?
a)
ade
b)
ate
c)
ion
d)
ide
28.

When naming COVALENT/MOLECULAR compounds, you use ______ to indicate the amount of each element in the name.

a)

prefixes

b)

coefficients

c)

subscripts

d)

superscripts

29.

Phosphorous trichloride

a)

PCl3

b)

P3Cl

c)

P3Cl3

d)

PCl

30.

The formula for the ionic compound of magnesium and nitrogen would be

a)

MgN2

b)

MgN

c)

Mg3N2

d)

MgN3

31.
What is the correct chemical name for the ionic compound: Fe3N2
a)
Iron nitride
b)
Iron (III) nitride
c)
Iron (II) nitride
d)
TriIron dinitride
32.
What is the correct chemical name for the molecular compound:  CS2
a)
Carbon Sulfide
b)
Carbon diSulfide
c)
diCarbide diSulfide
d)
Carbon (II) Sulfide
33.
If you have an oxyacid and it contains an -ite polyatomic ion, then acid's ending will change to _____. 
a)
-ic 
b)
-ous 
c)
hydro-root-ic acid 
d)
-ate 
34.
What element do all acids contain?
a)
H
b)
O
c)
C
d)
He
35.
bromic acid
a)
HBr
b)
H2Br
c)
HBrO3
d)
HBrO4
36.
chlorous acid
a)
HClO3
b)
HClO2
c)
HClO
d)
HCl
37.
H2SO3
a)
sulfuric acid
b)
hydrosulfuric acid
c)
sulfurous acid
d)
persulfuric acid
38.
HF
a)
flouric acid
b)
hydrofluoric acid
c)
fluorate acid
d)
hydrogen fluoridic acid
39.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
40.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
41.
Select the correct formula for sulfur hexachloride
a)
S2Cl6
b)
S6Cl
c)
SCl6
d)
SF6
42.
Name the compound NH4OH
a)
ammonium hydroxide
b)
ammonia oxyhydride
c)
mononitrogen tetraoxihydride
d)
hydrogen nitrate
43.
Which is the name of the kind of solid substance formed in this figure?  
a)
aqueous 
b)
precipitate
c)
acid
d)
synthesis 
44.
An element plus additional element reacts to form one product is an example of which type of chemical reaction? 
a)
combustion
b)
decomposition 
c)
synthesis 
d)
single replacement
45.
Magnesium reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas this happens because? 
a)
Magnesium is higher on the reactivity series then hydrogen
b)
magnesium is more reactive than hydrogen
c)
magnesium is able to break the bond between HCl and form MgCl2
d)
both b and c are correct
46.
Describes the number of molecules in a compound and is used to balance a chemical reaction. 
a)
coefficient 
b)
subscript
c)
superscript
d)
SI unit
47.
Which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water?
a)
double replacement 
b)
decomposition 
c)
combustion 
d)
single replacement
48.
What is the probable product of a double-replacement reaction?
a)
A new compound and a replaced metal
b)
A new compound and a replaced nonmetal
c)
2 different compounds 1 aqueous and 1 that is a solid, liquid or gas
d)
A single compound
49.
What are the correct coefficients when this equation is balanced?
KClO3  --> KCl  +  O2
a)
2,2,2
b)
2,2,3
c)
1,2,3
d)
3,3,3
50.
a substance that is formed as the result of a chemical reaction
a)
Product 
b)
Reactant
c)
Starters
d)
Enders
51.
type of chemical reaction where an element reacts with a compound and takes the place of another element in that compound
a)
Double Displacement
b)
Single Displacement
c)
Synthesis
d)
Decomposition
52.

According to the law of conservation of mass, how does the amount of each element on the product side compare to each element on the reactant side?

a)

The amount of atoms on each side is equal

b)

The amount of atoms on the product side is greater

c)

The amount of atoms on the reactant side is greater

d)

Depends on the reaction

53.

Which is the correct net ionic equation for the reaction of AgNO3 + CaCl2? if Silver chloride is a solid

a)
Ca2+(aq) +  2Cl- (aq) → CaCl(s)
b)
Ag+(aq)  +  Cl- (aq) → AgCl(s)
c)
Ag +  Cl  →  AgCl
d)
Ag+  +  Ca2+   →Ag2Ca (s)
54.

Identify the type of chemical equation below:

Cu2+ (aq) + 2 OH- (aq) --> Cu(OH)2 (s)

a)

Molecular equation

b)

Complete ionic equation

c)

Net ionic equation

55.

Identify the type of chemical equation below:

Cu2+ (aq) + SO42- (aq) + 2 Na+ (aq) + 2 OH- (aq) --> 2 Na+ (aq) + SO42- (aq) + Cu(OH)2 (s)

a)

Molecular equation

b)

Complete ionic equation

c)

Net ionic equation

56.

Identify ALL substances that CANNOT be broken apart in a net ionic equation.

a)

Solids

b)

Liquids

c)

Aqueous solutions

d)

Gases

57.

The number 6.022 x 1023 is called...

a)

A dozen

b)

Bohr's number

c)

Buckley's number

d)

Avogadro's number

58.

Which has more molecules?

a)

1 mole H2O

b)

1 mole CH4

c)

1 mole Cl2

d)

They're are all the same.

59.

One mole of sulfur (S) is equal to home many atoms?

a)

32 atoms

b)

16 atoms

c)

1.20 x 1023 atoms

d)

6.022 x 1023 atoms

60.

To convert from moles to particles, you should multiply by ....

a)
b)
c)
d)
61.

5.11 x 1023 atoms of lithium (Li) is equal to how many moles?

a)

1.18 moles

b)

0.351 moles

c)

1.34 moles

d)

0.849 moles

62.

36.0 g of beryllium (Be) contains how many moles?

a)

0.25 mol

b)

4.0 mol

c)

45 mol

d)

320 mol

63.

How many atoms would be contained in 454 grams of iron (Fe)?

a)

6.02 x 1023 atoms

b)

8.14 atoms

c)

4.90 x 1024 atoms

d)

55.85 x 1023 atoms

64.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
65.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
66.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
67.

The mole can be used to measure (SELECT ALL CORRECT ANSWERS)

a)

The amount of atoms

b)

The amount of molecules or compounds in a substance

c)

The amount of particles

d)

The amount of fission or fusion decay over time

68.

What is the mass of one mole of potassium (K)?

a)

19 grams

b)

39.10 grams

c)

30.97 grams

d)

38 grams

69.

What part of the electromagnetic spectrum can be seen by humans?

a)

Visible Light

b)

Microwaves

c)

Ultraviolet Waves

d)

Infrared Waves

70.

Which color on the image of the periodic table corresponds with the metalloids.

a)

bright yellow

b)

gold

c)

teal

d)

light blue

71.

The periodic table is mostly comprised of what type of element?

a)

Metals

b)

Nonmetals

c)

Metalloids

72.

Which elements are colored red?

a)

nonmetals

b)

metals

c)

metalloids

73.
All of these properties describe metals except...
a)
malleable
b)
conductors
c)
brittle 
d)
shiny
74.

Which structure consists of a giant lattice of cations and anions held together by strong electrostatic forces of attraction?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

75.

Which structure consists of a giant lattice of regularly arranged cations surrounded by a sea of delocalized electrons.

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

76.

Which of the following types of bonding results in materials which have the highest melting and boiling points?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

77.

Why do covalent compounds have lower melting and boiling points compared to ionic compounds?

a)

Covalent compounds have weak intermolecular forces between the molecules

b)

Covalent compounds do not conduct electricity

c)

Covalent compounds have strong intermolecular forces between the molecules

d)

Covalent compounds have very weak bonds between the atoms

78.

The structure of salt is shown. Salt would be considered...

a)

an ionic compound because it between a metal and nonmetal

b)

an ionic compound because it is between nonmetals

c)

a covalent compound because it is between a metal and nonmetal

d)

a covalent compound because it is between nonmetals

79.
Why does K become positive when it bonds to Cl to form KCl?
a)
Because it loses an electron to have a full valence shell 
b)
Because it gains an electron to have 2 valence electrons
c)
Because it loses an electron to become negatively charged
d)
Because Cl gives away its 7 electrons to Na to form an equal charge 
80.
The octet rule means that all valence shells want to have the number...... 
a)
1
b)
9
c)
8
d)
16
81.
All atoms/elements bond in order to ....
a)
Have a full valence shell
b)
Give away electrons or take electrons
c)
Only share electrons
d)
To create electrical currents for human use 
82.
How many atoms of iodine are in a mole of iodine?
a)
53
b)
63.55g
c)
126.9
d)
6.02 x 1023
83.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
84.
What is the mass of 54.3x1045molecules of BeO?
a)
3.27x1070 g
b)
9.01 x1022g
c)
2.25 x1024 g
d)
1.31 x1069g
85.

How many grams of magnesium nitride is required to produce

25.00 g

of magnesium hydroxide?

Mg3N2+H2O→Mg(OH)2+NH3

1

a)

14.43 grams

b)

43.29 grams

c)

41.42 grams

d)

None of the above

86.

I2 is produced by the reaction of 0.4235 mol of CuCl2 according to the following equation: 2CuCl2+4KI→2CuI+4KCl+I22CuCl2+4KI→2CuI+4KCl+I2 .

  1. How many molecules of I2 are produced?

a)

2.544 x 10 ^23

b)

3.456 x10^22

c)

5.678 x 10^24

d)

1.272 x 10^23

87.

Consider the balanced chemical equation for the synthesis of ammonia (NH3) from its elements:

N2 + 3 H2 → 2 NH3

  1. How many moles of NH3 will be produced by the reaction of 4.0 moles of N2?

a)

4 mol

b)

8 mol

c)

2 mol

d)

1 mol

88.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

89.

Rubidium has two common isotopes, 85Rb and 87Rb. If the abundance of 85Rb is 72.2% and the abundance of 87Rb is 27.8%, what is the average atomic mass of rubidium?

a)

85.468 amu

b)

37 amu

c)

85.6 amu

d)

86.4 amu

90.
The scientist responsible for "discovering" the nucleus is:
a)
Bohr
b)
Rutherford
c)
Schroedinger
d)
Einstein
91.
The nucleus of an atom can be described as:
a)
spacious and negatively charged
b)
dense and positively charged
c)
spacious and positively charged
d)
dense and negatively charged
92.
Electrons are not factored into atomic mass because:
a)
They are so small their mass is negligible
b)
They're not in the nucleus
c)
They're too big
d)
They move so quickly their mass is zero
93.

Who proposed electrons are found in specific orbits around the nucleus?

a)

Democritus

b)

John Dalton

c)

James Chadwick

d)

NielsBohr

Similar Resources on Wayground

Unit 1 Review Chem

96 questions

Unit 1 Review Chem

quiz

Worksheet

•

9th - 12th Grade

25.3 Half Life

91 questions

25.3 Half Life

quiz

Worksheet

•

10th - 12th Grade

Molecular compounds practice

98 questions

Molecular compounds practice

quiz

Worksheet

•

10th Grade - University

Ionic Compounds and Review for Adaptive Question Bank - CP

96 questions

Ionic Compounds and Review for Adaptive Question Bank - CP

quiz

Worksheet

•

8th - 11th Grade

Solubiity Rules Practice

92 questions

Solubiity Rules Practice

quiz

Worksheet

•

9th - 12th Grade

Honors Chemistry Unit 2 Exam Review

92 questions

Honors Chemistry Unit 2 Exam Review

quiz

Worksheet

•

10th Grade

Unit 7 Bonding and Compounds Review Game

89 questions

Unit 7 Bonding and Compounds Review Game

quiz

Worksheet

•

10th - 12th Grade