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Chem 1 Midterm Review

Total questions: 142

Worksheet time: 5hrs 27mins

Name
Class
Date
1.
Which of the following is an ionic compound:
a)

CH4

b)

I2

c)

LiBr2

d)
CO
2.

Name the following ionic compound with the correct polyatomic ion: Mg(SO4)

a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
3.
What is the ionic compound formed between Calcium and Oxygen?
a)
CaO
b)
Ca2O
c)
CaO2
4.
Name the following ionic compound: BeCl2
a)
beryllium chlorine
b)
beryllium II chloride
c)
beryllium chloride
d)
beryllium dichloride
5.

What is the correct name for ionic compound Al2(SO4)3?

a)

aluminum(II) sulfate

b)

dialuminum trisulfate

c)

aluminum sulfide

d)

aluminum sulfate

6.

What is the name of K2S?

a)

potassium sulfur

b)

potassium sulfite

c)

potassium sulfide

d)

potassium sulfate

7.

What is the correct formula for the ionic compound, lithium oxide?

a)

LiO

b)

Li2O

c)

LiO2

d)

Li2O2

8.

Name the following covalent compound.

NO

a)

Mononitrogen Oxide

b)

Nitrogen monoxide

c)

Nitrogen Oxide

9.

Hydrogen needs _____ electrons in its valence shell to be stable.

a)

4

b)

8

c)

2

d)

3

10.
What is the name of C3Cl8 ?
a)
Carbon octachloride
b)
Tricarbon octachloride
c)
Carbon trichloride
d)
Octacarbon trichloride
11.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
12.

The _____ ____ tells us that atoms are generally very stable with 8 valence electrons.

(a)  

13.

How many electrons are shared in each bonding line (-) in a Lewis structure?

a)

1

b)

2

c)

3

d)

4

14.

When drawing Lewis structures, only __________ electrons are used.

a)

inner shell

b)

core

c)

valence

d)

stable

15.

Match each property to the correct bond type.

Categorize the following

Conductive when dissolved

Conductive as a solid

Gas, liquid, or soft solid at room temp

Brittle solid with crystal lattice

Malleable solid

Lowest melting point

Ionic
Metallic
Covalent
16.
After drawing in your bonds, what do you do if you don't have enough electrons to get each atom to its octet?
a)
Place dots until everything has eight
b)
Place dots only around the terminal atoms
c)
Add a multiple bond
d)
Have eight only around the central atom
17.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
18.
Where are the metalloids located on the periodic table?
a)
Blue
b)
Red
c)
Green
19.
Where are metals located on the periodic table?
a)
Blue
b)
Green
c)
Red
20.
Where are the nonmetals located on the periodic table? 
a)
Blue
b)
Red
c)
Green
21.
Which is the charge that results when oxygen becomes an ion?
a)
+3
b)
+2
c)
-2
d)
-3
22.

What group does not react because they already have a full valence shell.

a)

halogens

b)

noble gasses

c)

alkali metals

d)

alkali earth metals

23.

What is the total charge of the Lithium Oxide compound?

a)

0

b)

+2

c)

-2

d)

-1

24.

Properties of metallic compounds include:

a)

brittle, conducts electricity (aqueous state), high melting points

b)

usually gas or liquid, relatively low melting points, does not conduct electricity

c)

shiny, malleable, ductile, conducts electricity, usually a solid

25.

Properties of ionic compounds include:

a)

brittle, conducts electricity (aqueous state), high melting points

b)

usually gas or liquid, relatively low melting points, does not conduct electricity

c)

shiny, malleable, ductile, conducts electricity, usually a solid

26.

Properties of covalent compounds include:

a)

brittle, conducts electricity (aqueous state), high melting points

b)

usually gas or liquid, relatively low melting points, do not conduct electricity

c)

shiny, malleable, ductile, conducts electricity, usually a solid

27.
 A lone pair is defined as
a)
A pair of bonding electrons
b)
One non-bonding electron
c)
A pair of non-bonding electrons
d)
A pair of electrons on the central atom
28.

Match each element with its common ion charge.

a)

Oxygen (O)

1.

-2

b)

Nitrogen (N)

2.

-3

c)

Lithium (Li)

3.

+1

d)

Calcium (Ca)

4.

+2

e)

Aluminum (Al)

5.

+3

29.

Categorize each compound as ionic or covalent.

Categorize the following

H2O

N2O5

MgCl2

Na(OH)

Al2O3

Ionic
Covalent
30.

Chemical names should end in - (a)   unless there is a polyatomic ion.

31.

4. What usually forms the positive ion?

a)

Metal

b)

Nonmetals

c)

None

32.

6. What usually forms the negative ion?

a)

Nonmetals

b)

Metal

c)

None

33.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
34.

Which of these is the correct Lewis structure for NH3?

a)

b)

c)

d)

35.

Looking at your periodic table, how many valence electrons does Bromine have?

a)

5

b)

6

c)

7

d)

8

36.

Ionic bonds are held together by what force?

a)

intermolecular

b)

electrostatic

c)

free moving valence electrons

d)

intramolecular

37.

Choose the correct Lewis dot structure for Nitrogen. It is okay if the lone pair is rotated.

a)

E

b)

F

c)

G

d)

H

38.

Which type of bond is being formed in this diagram?

a)

covalent bond

b)

energy bond

c)

ionic bond

39.

Which of the following is the correct Lewis dot between Rb and O?

a)
b)
c)
d)
40.

How many connection points does carbon have to bond?

a)

2

b)

4

c)

6

d)

8

41.

Which of these is the correct match to form an ionic compound? Hint Recall the sum of the charges must be 0!

a)

b)

c)

d)

42.

Which of these is the correct match to form an ionic compound? Hint Recall the sum of the charges must be 0!

a)

b)

c)

43.

Select the correct Lewis structure for CH4.

A
B
C
D
44.

Select the correct Lewis structure for O2?

A
B
C
D
45.

Select the correct Lewis structure for PH3?

A
B
C
D
46.

When do you need to use the "drop and switch" method?

a)

When making an ionic formula from a name

b)

When making a covalent formula from a name

c)

When writing a name for any compound

47.

When do you need to use prefixes in a name?

a)

When the compound is covalent

b)

When the compound is ionic

c)

When there is a polyatomic ion

48.

Match the type of bond to its state of matter at room temperature.

a)

Malleable solids

1.

Metallic

b)

Brittle solids with crystal lattice

2.

Ionic

c)

Gas, liquids, or soft/powdery solids

3.

Covalent

49.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
50.
What is this element?
[Xe] 6s24f145d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
51.
What is the noble gas shorthand for Sulfur?
a)
[Ar]3p4
b)
[He]3s23p4
c)
[Ne]3s23p4
d)
[Na]3s23p4
52.
How many valence electrons are represented here?
a)
7
b)
5
c)
2
d)
8
53.

Order the following from largest to smallest scale organization of electrons

a)

Atoms

b)

Shell

c)

Subshell

d)

Orbital

1)
2)
3)
4)
54.

Match each subshell to its maximum number of electrons

a)

s

1.

2 e-

b)

p

2.

6e-

c)

d

3.

10e-

d)

f

4.

14e-

55.

Match each subshell to an image of its possible shapes.

a)

1.

s

b)

2.

p

c)

3.

d

d)

4.

f

56.

Match the term with its correct definition.

a)

Atomic Radius

1.

Describes the size of an atom.

b)

Ionization

2.

The energy needed to remove an electron

c)

Electronegativity

3.

How much an atom attracts an electron

57.

Which atom has the largest atomic radius of the entire periodic table?

a)

potassium (K)

b)

rubidium (Rb)

c)

francium (Fr)

d)

cesium (Cs)

58.

As you move down the periodic table atoms get bigger.  This is because the atoms get more ​ (a)   as you move down a group.

Choose from the below words
protons
neutrons
electron shells/levels
59.

As you move across the periodic table atoms tend to get smaller because, the atoms get more (a)   as you move from left to right.

Choose from the below words
neutrons
electron shells
protons
60.

Which periodic group (aka family) has the smallest atomic radius? Click the spot on that group.

A
B
C
D
61.

Which periodic group (aka family) has the highest electronegativity? Click the spot on that group.

A
B
C
D
E
62.

Why do Noble gases have the highest ionization energy but the lowest electronegativity?

4 lines
63.

In just a couple words, what could we say ultimately causes the periodic trends? Remember the "golden answer" we talked about

4 lines
64.

Which element below has the highest ionization energy?

a)

Lead (Pb)

b)

Sulfur (S)

c)

Helium (He)

65.

Order the elements below from lowest electronegativity (1) to highest electronegativity (3).

a)

Calcium (Ca)

b)

Aluminum (Al)

c)

Fluorine (F)

1)
2)
3)
66.

Order the elements below from the smallest atom (1) to the largest atom (4)

a)

Nitrogen (N)

b)

Boron (B)

c)

Magnesium (Mg)

d)

Calcium (Ca)

1)
2)
3)
4)
67.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
68.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
69.
What is this element?
[Xe] 6s24f145d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
70.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
71.
How many valence electrons does phosphorus have?
a)
5
b)
2
c)
8
d)
15
72.

Which of the following electron configurations represents a noble gas?

a)

1s22s22p63s1

b)

1s22s22p4

c)

1s22s22p63s23p5

d)

1s22s22p6

73.

Order the following from largest to smallest scale organization of electrons

a)

Atoms

b)

Shell

c)

Subshell

d)

Orbital

1)
2)
3)
4)
74.

What can be thought of as a specific distance (aka energy amount) away from the nucleus.

a)

Atom

b)

Shell

c)

Subshell

d)

Orbital

75.

Electron shells (aka energy levels) are HIGHER energy the ____________ they are to the nucleus.

a)

closer

b)

further away

c)

more similar

76.

These describe differently shaped areas that electrons occupy within a shell.

a)

Atom

b)

Shell

c)

Subshell

d)

Orbital

77.

This is any area that can hold two electrons with opposite "spin."

a)

Atom

b)

Shell

c)

Subshell

d)

Orbital

78.

Match each subshell to its maximum number of electrons

a)

s

1.

2 e-

b)

p

2.

6e-

c)

d

3.

10e-

d)

f

4.

14e-

79.

Match each subshell to an image of its possible shapes.

a)

1.

s

b)

2.

p

c)

3.

d

d)

4.

f

80.

How many electrons shells does rubidium have?

a)

2

b)

3

c)

4

d)

5

81.

What is the electron configuration for titanium, Ti? You can use the noble gas short cut, if you want. Put a space between each subshell. Example: 1s2 2s2 ...

4 lines
82.

Who is known as the father of the periodic table?

a)

Dmitri Mendeleev

b)

Marie Curie

c)

Isaac Newton

d)

Albert Einstein

83.

Why is it called the periodic table? AKA what does periodicity mean?

4 lines
84.

How are elements organized in the Periodic Table?

a)

Elements are ordered by atomic weight

b)

Elements are ordered by atomic number

c)

Elements are arranged alphabetically

d)

Elements are grouped color

85.
All of these properties describe metals except...
a)
malleable
b)
conductors
c)
brittle 
d)
shiny
86.
One property of a nonmetals is that it is a good conductor of electricity?
a)
true
b)
false
87.
Non-metals are good conductors of heat and electricity. 
a)
TRUE
b)
FALSE
88.
Which of the following properties refers to the ability of metals to be drawn into wires?
a)
A. malleability 
b)
B. compressibility
c)
C. ductility
d)
D. luster
89.
Metals appear to the _______ of the dark ziz-zag line on the periodic table. 
a)
A. right
b)
B. middle
c)
C. left
90.
Anytime you see the word SEMICONDUCTOR - what substance do you have?
a)
Metal
b)
Nonmetal
c)
Metalloid
91.
If a material can easily be drawn into the shape of a wire, it is
a)
Ductile
b)
Magnetic
c)
Malleable
d)
Reactive
92.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
93.

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

a)

groups

b)

towers

c)

periods

d)

atomic numbers

94.

Elements in a .................. have similar chemical properties.

a)

period

b)

group

c)

row

95.

The group number tells you the number of

a)

protons

b)

valence electrons

c)

energy levels

96.

The period number tells you the number of

a)

protons

b)

energy levels

c)

valence electrons

97.

Which two elements have properties in common?

a)

Nitrogen and Phosphorous

b)

Oxygen and Nitrogen

c)

Sulfur and Nitrogen

98.

These elements are in a:

a)

group

b)

period

99.

These elements are in a:

a)

group

b)

period

100.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
101.
How many protons are in this element?
a)
79
b)
196
c)
117
d)
Cannot be determined
102.

How many NEUTRONS does Fluorine have?

a)

19

b)

10

c)

9

d)

28

103.

How many PROTONS does Boron have?

a)

11

b)

5

c)

16

d)

6

104.
What is the name of this element?
a)
Helium
b)
Hydrogen
c)
Argon
d)
Silver
105.

What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

106.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
107.

Organize these options into the right categories based on type of property.

Categorize the following

Observed with senses

Determined without destroying matter

Indicates how a substance reacts with something else

Matter will be changed into a new substance

Color

Density

Solubility (dissolves)

Flammability (burns)

Reacts with acids

Reacts with water

Physical Property
Chemical Property
108.

Organize these examples into the right categories based on type of change that occurs.

Categorize the following

A change in shape or size.

No new substance is formed.

A change in the chemical properties.

A new substance is formed.

Baking soda mixed with Vinegar.

Smashing a Vase.

Cutting an apple.

Iron rusting.

Physical Changes
Chemical Changes
109.
Question Image

Match the following evidence with the observation

a)

1.

Physical Change - because it is melting.

b)

2.

Chemical Change - because it is burned.

c)

3.

Physical Change - because it is bent.

d)

4.

Physical Change - because size changes.

e)

5.

Chemical change - because acids/bases.

110.

Type of mixture that has the same composition in every part.

a)

Homogeneous

b)

Heterogeneous

111.

Type of mixture that DOESN'T HAVE the same composition in every part.

a)

Homogeneous

b)

Heterogeneous

112.

Name the separation technique shown in the diagram.

a)

evaporation

b)

distillation

c)

filtration

113.

During a science class experiment, Genesis and Rosalina are trying to separate sand from iron filings. Which one of the following would they use?

a)

a bar magnet

b)

filter paper

c)

chromatography paper

d)

alum

114.

What mixture could you use this tool to best separate that mixture?

a)

Sugar and Salt

b)

Sand and rocks

c)

Apples and grapes

115.

Fill in the blanks

a)

17

b)

16

c)

Phosphorus

d)

Chlorine

e)

30.97

f)

15

1
2
3
4
1)
2)
3)
4)
116.

What type of decay is shown in this equation?

a)

alpha decay

b)

beta decay

c)

gamma emission

117.

What particle completes this reaction?

a)
b)
c)
d)
118.
Solve this equation for alpha decay.
85209At = ___ + 24He
a)
83205Bi
b)
86209Rn
c)
81207Tl
d)
85208At
119.
Solve this equation for beta decay.
614C = ___ + -10e
a)
410Be
b)
714N
c)
210He
d)
613C
120.

What type of decay type is shown by this generic equation?

a)

alpha decay

b)

beta decay

c)

gamma emission

d)

fission

121.

What type of decay type is shown by this generic equation?

a)

alpha decay

b)

beta decay

c)

gamma emission

d)

fission

122.
What particle completes this reaction?
a)
alpha particle
b)
beta particle
c)
gamma particle
d)
neutron
123.

What particle completes this reaction?

a)

42He

b)

0-1 e

c)

00Y

d)

178O

124.

How many protons does this isotope of titanium have?

a)

48

b)

22

c)

26

d)

70

125.

What is the symbol for a gamma ray?

a)
b)
c)
d)
126.
What is the symbol for an alpha particle?
a)
42He
b)
0-1e
c)
0+1 e
d)
10n
127.
What does the symbol -10e represent
a)
alpha
b)
beta
c)
gamma
d)
the zero element
128.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
129.
?
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
130.

How close a measurement is to the accepted value is called..

a)

Accuracy

b)

Precision

c)

Significant

d)

Estimate

131.
A set of data are all close to each other, but they are not close to the actual value.  This set of data can be described as...
a)
accurate
b)
precise
c)
both precise and accurate
132.

Identfy the graduated Cylinder, which is a volumetric (accurate) piece of glassware.

A
B
C
D
133.
Which of the following is considered safety equipment in our classroom?
a)
eyewash station
b)
emergency shower
c)
fire extinguisher
d)
all of the above
134.
Which of the following is a safety rule in the science lab?
a)
Bring your lunch to the lab.
b)
Always have a bottle of water in case you are thirsty.
c)
Snacks are permitted during a long experiment.
d)
Never eat or drink during a lab.
135.

Match the atomic model to its name.

a)

1.

Bohr (Planetary) Model

b)

2.

Plum Pudding Model

c)

3.

Quantum Mechanical (Cloud) Model

d)

4.

Sphere Model (Dalton)

e)

5.

Nuclear Model (Rutherford)

136.

This is an example of...

a)

Fission chain reaction

b)

Fusion reaction

c)

Decomposition reaction

d)

Decay

137.

Which phrase describes a risk associated with producing energy in a nuclear power plant?

a)

depletion of atmospheric hydrogen

b)

depletion of atmospheric carbon dioxide

c)

production of wastes needing long-term storage

d)

production of wastes that cool surrounding water supplies

138.

Organize these options into the right categories

Categorize the following

Atom is divided

Two atoms join

Nuclear waste is an issue

Uses uranium and other radioactive elements

1000 x stronger

Typically uses hydrogen and produces helium

Naturally occuring on the sun

Produces energy in stars

Used in nuclear power plants

Chain reaction can occur

Nuclear Fission (5)
Nuclear Fusion (5)
139.

The nucleus is held together by the ___________________________force.

a)

The Strong Nuclear Force

b)

The Weak Nuclear Force

c)

Electromagnetism

d)

Gravity

140.
How many protons are in this atom?
a)
3
b)
4
c)
6
d)
10
141.
How many neutrons are in this isotope of Uranium?
a)
235
b)
92
c)
327
d)
143
142.
In order of most to least penetrating radiation we have
a)
Alpha , Beta,  Gamma
b)
Beta , Gamma , Alpha
c)
Gamma, Beta, Alpha
d)
Gamma, Alpha, Beta

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