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2022-23 Chemistry T1 Final Units 1-4

Total questions: 125

Worksheet time: 3hrs 38mins

Name
Class
Date
1.

The SI unit for temperature is __?__.

a)

degree fahrenheit (° F)

b)

degree celsius (° C)

c)

kelvin (K)

d)

degree centigrade (°C)

2.

The metric prefix "kilo" means __?__.

a)

one tenth (0.1)

b)

one thousandth (0.001)

c)

one hundred (100)

d)

one thousand (1,000)

3.
You know 1000 mg = 1 g.  Convert 2.5 grams into milligrams.
a)
25 mg
b)
25,000 mg
c)
250 mg
d)
2500 mg
4.

How many minutes are in 17 years?

a)

5,256,000min

b)

525,600min

c)

8,935,200min

d)

31,536,000min

5.
What charge does a proton have?
a)
positive
b)
negative
c)
no charge
d)
neutral
6.
Where are protons located in the atom?
a)
orbitals
b)
nucleus
c)
rings
d)
positive
7.
If an atom loses an electron, does the atom become more positive or more negative?
a)
more positive
b)
more negative
c)
both
d)
neither
8.
An extremely unreactive group 18 element.
a)
halogen
b)
alkali metal
c)
noble gas
d)
alkaline earth metal
9.
Elements that are generally gases or dull brittle solids that are poor conductors of heat and electricity.
a)
noble gas
b)
halogen
c)
nonmetal
d)
metalloids
10.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
11.
What is the number of valence electrons for Silicon?
a)
1
b)
2
c)
6
d)
4
12.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
13.
Name CCl4
a)
carbon carbon tetraiodide
b)
carbon tetrachloride
c)
monocarbon tetrachloride
d)
water
14.
a substance formed when two or more elements are chemically bonded together
a)
Element Soup
b)
Pure Element
c)
Ion
d)
Compound
15.
As water begins changing from liquid to solid, it will ____ & _____.
a)
freeze, shrink
b)
freeze, expand
c)
condensate, shrink
d)
condensate, expand
16.

In order to convert to Kelvin, you add ______ to the Celsius measurement.

a)

372

b)

273

c)

237

d)

732

17.
salt water is a 
a)

compound

b)

element

c)

heterogeneous mixture

d)

solution (homogeneous mixture)

18.

What is oxidation number (charge) of Fe in FeO ?

a)

+2

b)

-2

c)

0

d)

+1

19.
Identify the equipment shown here:
a)
graduated cylinder
b)
Erlenmeyer flask
c)
beaker
d)
volumetric flask
20.
Identify the equipment shown here:
a)
beakers
b)
flasks
c)
decanters
d)
graduated cylinders
21.
When in the lab...
a)
long sleeves and loose clothing should be rolled up
b)
closed toe shoes should be worn
c)
long hair should be pulled back
d)
all of the above
22.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
23.

Bond breaking releases energy.

a)

true

b)

false

24.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

25.

LiBr is called

a)

lithium bromine

b)

lithium (I) bromine

c)

lithium bromide

d)

lithuim (I) bromide

26.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

27.

Which of these combinations is an ionic compound made of?

a)

Metal and Metal

b)

Nonmetal and Nonmetal

c)

Metal and Nonmetal

d)

Cation and Cation

28.
What is the chemical formula for Tetrasulfur pentoxide?
a)
SO
b)
S4O
c)
S4O5
d)
S5O4
29.
What is a positivly charge atom called?
a)
cation
b)
anion
30.

What is the little number after an element in a chemical formula called. Example: H2

a)

Coefficient 

b)

Subscript

c)

Atom

d)

Equation

31.

All of the following are physical properties of matter EXCEPT ____.

a)

mass

b)

color

c)

melting point

d)

ability to rust

32.

The chemical symbol for iron is ____.

a)

fe

b)

FE

c)

Fe

d)

Ir

33.

Which of the following is a chemical property?

a)

color

b)

hardness

c)

freezing point

d)

ability to react with oxygen

34.

All of the following changes to a metal are physical changes EXCEPT ____.

a)

bending

b)

melting

c)

rusting

d)

polishing

35.

The smallest particle of an element that retains the properties of that element is a(n) ____.

a)

atom

b)

electron

c)

proton

d)

neutron

36.

Which of the following is true about subatomic particles?

a)

Electrons are negatively charged and are the heaviest subatomic particle.

b)

Protons are positively charged and the lightest subatomic particle.

c)

Neutrons have no charge and are the lightest subatomic particle.

d)

The mass of a neutron nearly equals the mass of a proton.

37.

What is the relative mass of an electron?

a)

1/1840 the mass of a hydrogen atom

b)

1/1840 the mass of a neutron + proton

c)

1/1840 the mass of a C-12 atom

d)

1/1840 the mass of an alpha particle

38.

All atoms are ____.

a)

positively charged, with the number of protons exceeding the number of electrons

b)

negatively charged, with the number of electrons exceeding the number of protons

c)

neutral, with the number of protons equaling the number of electrons

d)

neutral, with the number of protons equaling the number of electrons, which is equal to

the number of neutrons

39.

The nucleus of an atom is ____.

a)

the central core and is composed of protons and neutrons

b)

positively charged and has more protons than neutrons

c)

negatively charged and has a high density

d)

negatively charged and has a low density

40.

The atomic number of an element is the total number of which particles in the nucleus?

a)

neutrons

b)

protons

c)

electrons

d)

protons and electrons

41.

Isotopes of the same element have different ____.

a)

numbers of neutrons

b)

numbers of protons

c)

numbers of electrons

d)

atomic numbers

42.

An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the

element are ____.

a)

152 protons and 76 electrons

b)

76 protons and 0 electrons

c)

38 protons and 38 electrons

d)

76 protons and 76 electrons

43.

The mass number of an element is equal to ____.

a)

the total number of electrons in the nucleus

b)

the total number of protons and neutrons in the nucleus

c)

less than twice the atomic number

d)

constant number for the lighter elements

44.

How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain?

a)

50 protons, 50 electrons, 75 neutrons

b)

75 electrons, 50 protons, 50 neutrons

c)

120 neutrons, 50 protons, 75 electrons

d)

70 neutrons, 75 protons, 50 electrons

45.

What is the number of electrons in the outermost energy level of an oxygen atom?

a)

2

b)

4

c)

6

d)

8

46.

The modern periodic table is arranged in order of increasing atomic ____.

a)

mass

b)

charge

c)

number

d)

radius

47.

Of the elements Pt, V, Li, and Kr, which is a nonmetal?

a)

Pt

b)

V

c)

Li

d)

Kr

48.

Which of the following elements is a transition metal?

a)

cesium

b)

copper

c)

tellurium

d)

tin

49.

The metals in Groups 1A, 2A, and 3A ____.

a)

gain electrons when they form ions

b)

all form ions with a negative charge

c)

all have ions with a 1+ charge

d)

lose electrons when they form ions

50.
How many sig. fig. are in the number below:
106.00
a)
2
b)
3
c)
4
d)
5
51.
How many sig. fig. are in the number below:
705000
a)
2
b)
3
c)
5
d)
6
52.

Convert the following to scientific notation.

0.000480

a)

4.8 x 10-4

b)

4.80 x 10-4

c)

48 x 10-5

d)

4.80 x 104

53.
Round 1047.78 to three sig figs
a)
104
b)
105
c)
1050
d)
1050.00
54.
A bottle of hand sanitizer is 88mL. What is its volume in Liters?
a)
.88 Liters
b)
.088 Liters
c)
8.8 Liters
d)
88 Liters
55.
240 cm = ___________ m
a)
2400
b)
24
c)
2.4
d)
0.24
56.

What step does every scientific experiment begin with?

a)

hypothesis

b)

question/problem

c)

procedures

d)

conclusion

57.
Calculate the answer to the following problem and round the final answer to the correct number of sig figs:
24.567 + 0.04478 =
a)
24.61178
b)
24.612
c)
24.611
d)
24.61
58.
Calculate the answer to the following problem and round the final answer to the correct number of sig figs:
4.627 / 0.00371 = 
a)
1247.169811
b)
1250
c)
1247
d)
1240
59.
Which is NOT a diatomic molecule?
a)
Fluorine
b)
Nitrogen
c)
Boron
d)
Bromine
60.

Convert 72⁰F to Celsius (5/9 x (0F - 32))

a)

2.2⁰C

b)

222⁰C

c)

22.2⁰C

d)

161.6⁰C

61.

Convert 35⁰F to Celsius (5/9 x (0F - 32))

a)

1.6⁰

b)

1.7⁰C

c)

2.0⁰

d)

16.6⁰C

62.
Put the liquids in order from most dense to least dense?
a)
4, 3, 2, 1
b)
1, 2, 3, 4
c)
3, 4, 2, 1, 
d)
4, 3, 1, 2
63.
Jack has a rock. The rock has a mass of 14 g and a volume of 2 cm3. What is the density of the rock?
a)
7 mL
b)
7 g/cm3
c)
28 g/cm3
d)
1/7 g/cm3
64.
What is the density of water?
a)
0 g/ml
b)
1 g/ml
c)
10 g/ml
d)
100 g/ml
65.
What is the volume of the fish?
a)
18.0 cm3
b)
6.0 cm3 
c)
38.0 cm3
d)
32.0 mL
66.
A passenger jet has a speed of 900 km/h.
What is its speed in m/s?
(1 km = 1000 m)
a)
250 m/s
b)
324 m/s
c)
1,500 m/s
d)
2,500 m/s
67.

Convert 70,000 quarts/year to pints/day

a)

383.6 pints/day

b)

767.1 pints/day

c)

1,534.2 pints/day

d)

191.8 pints/day

68.
What is the volume of liquid in this graduated cylinder?
a)
40.0 mL
b)
40.3 mL
c)
43.0 mL
d)
44.0 mL
69.

The branch of science that studies what "Stuff" is made of and how it interacts with other "Stuff".

a)

STEM

b)

Biology

c)

Chemistry

d)

Engineering

70.

We see chemistry in action in our lives when we...

a)

Bake cookies

b)

Take medicine

c)

Wash our clothes

d)

All of the above

71.
The top number in this isotope notation is
a)
the mass number
b)
the atomic number
c)
the atomic mass
d)
the neutron number
72.
The bottom number in this isotope notation is
a)
the mass number
b)
the atomic number
c)
the atomic mass
d)
the neutron number
73.
According to the isotopic notation for copper-63, how many neutrons are present in this type of atom?
a)
29
b)
34
c)
63
d)
92
74.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
75.
Group 1 elements, except for hydrogen, they are reactive and usually exist as compounds with other elements.
a)
alkaline earth metal
b)
halogen
c)
alkali metal
d)
representative element
76.
A highly reactive group 17 element.
a)
halogen
b)
metalloid
c)
noble gas
d)
alkali metal
77.
Elements that are generally gases or dull brittle solids that are poor conductors of heat and electricity.
a)
noble gas
b)
halogen
c)
nonmetal
d)
metalloids
78.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
79.
What is the number of valence electrons for Silicon?
a)
1
b)
2
c)
6
d)
4
80.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
81.
Name CCl4
a)
carbon carbon tetraiodide
b)
carbon tetrachloride
c)
monocarbon tetrachloride
d)
water
82.

The name of FeCl₂ is

a)

iron chloride

b)

iron (II) chloride

c)

iron (I) chloride

d)

iron dichloride

83.

What is the name of the compound Na2(SO4)?

a)

Sodium sulfate

b)

Sodium sulfide

c)

Sodium sulfite

d)

Sodium sulfuroxide

84.
What is a positivly charge atom called?
a)
cation
b)
anion
85.

How many valence electrons do elements in Group 13 have?

a)

13

b)

5

c)

3

86.

What is the charge, or oxidation number, for elements in Group 17?

a)

+ 1

b)

-7

c)

-1

87.
The proper technique for smelling chemicals is ______________
a)
keeping your nose close to the glassware
b)
wafting
c)
to sniff only a small amount
d)
Trick question; you never are allowed to smell chemicals in class
88.

The following footwear is the best in the laboratory

a)

sandals

b)

open-toed shoes

c)

closed-toe shoes

d)

shoes appropriate for the weather

89.

Approved eye protection devices (such as goggles) are worn in the laboratory

a)

to avoid eye strain

b)

to improve your vision

c)

so that you look super cool

d)

any time chemicals, heat or glassware are used

90.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
91.
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
92.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
93.

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

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

94.

Which of the following halogens has the greatest electronegativity?

a)

Chlorine (Cl)

b)

Bromine (Br)

c)

Iodine (I)

d)

Astatine (At)

95.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

96.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

97.

What is one-half the distance between the nuclei of identical atoms that are bonded together?

a)

atomic radius

b)

atomic diameter

c)

atomic width

d)

atomic length

98.

What is a vertical (up and down) column in the periodic table?

a)

group or family

b)

period

c)

periodic law

d)

octet rule

99.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
100.

There are several elements that this could be. One of them is listed below. Pick it!

a)

Mg

b)

O

c)

F

d)

Be

101.

What ion will this form?

a)

1+

b)

1-

c)

7+

d)

7-

102.

What ion will K form?

a)

1+

b)

2+

c)

1-

d)

2-

103.

What ion will a atom with 5 valence electrons form?

a)

3+

b)

3-

c)

5+

d)

5-

104.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
105.

Which is the correct molecular structure for carbon dioxide?

a)
b)
c)
d)
106.

3. Which is a correct Lewis structure for hydrogen cyanide, HCN?

a)
b)
c)
d)
107.

Carbonate (CO32-) has how many double bonds?

a)

0

b)

1

c)

2

d)

3

108.
How many electrons are shared in a double bond?
a)
2
b)
4
c)
6
d)
8
109.

Since covalent compounds do not have free charges, they are

a)

good conductors

b)

poor conductors

c)

ionic

d)

metallic

110.

Which interaction from below needs the most energy to be broken?

a)

Ionic bond

b)

Induced dipole

c)

Permanent dipole

111.

Which of the following are properties of ionic compounds? Choose all correct answers.

a)

high melting and boiling points

b)

can be solids, liquids, or gases at room temperature

c)

tend to be highly flammable

d)

form crystalline structures

e)

can conduct electricity when dissolved or melted

112.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
113.

How many valence electrons does perchlorate (ClO4-) have?

a)

26

b)

28

c)

30

d)

32

114.

Most atoms are most stable when their outer shell is complete with 8 electrons.

a)

true

b)

false

115.
Why do elements bond?
a)
To be friends
b)
To create a new element
c)
To become stable
116.

Breaking a bond is always

a)

Endothermic (requires energy)

b)

Exothermic (releases energy)

117.

Predict the bond that will form between Se and Cl

a)

Ionic-bond

b)

Covalent-bond

c)

Metallic-bond

d)

Hydrogen-bond

118.

Predict the bond formed between Be and F

a)

Covalent-bond

b)

Ionic-bond

c)

Metallic-bond

d)

Hydrogen-bond

119.

Why don't noble gases form bonds?

a)

Noble gases do form bonds

b)

They all have a full octet

c)

They only bond with each other

120.

What type of bond (intramolecular force) is made between to atoms of almost equal electronegativities?

a)

non-polar covalent

b)

polar covalent

c)

ionic

121.

What type of bond (intramolecular force) is made between to atoms of slightly different electronegativities where they differ between .4 and 1.7?

a)

non-polar covalent

b)

polar covalent

c)

ionic

122.

Which of the following not a Diatomic gas/element?

a)

N2

b)

O2

c)

I2

d)

H2

e)

They are all Diatomic gases/elements

123.

Which of the following types of bonding results in materials which are generally insoluble in water?

a)

ionic bonding

b)

metallic bonding

c)

covalent bonding

124.
Does H2O have hydrogen bonding?
a)
yes
b)
no
125.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules

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