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Pre-Fall Break Review (AME) (Units 1, 2, 3)

Total questions: 125

Worksheet time: 3hrs 16mins

Name
Class
Date
1.
Convert 8 kilometers to meters
a)
800 m
b)
80,000 m
c)
8,000 m
d)
.008 m
2.
1 Meter = ______cm
a)
100
b)
10
c)
1
d)
1000
3.
Which one is not in the metric system?
a)
Kilometer
b)
Yard
c)
Centimeter
d)
Meter
4.
The base unit for length is the
a)
second
b)
gram
c)
meter
d)
liter
5.
The base unit for length is the
a)
second
b)
gram
c)
meter
d)
liter
6.
The base unit for volume is the
a)
second
b)
gram
c)
meter
d)
liter
7.
The base unit for mass is the
a)
meter
b)
gram
c)
kilogram
d)
liter
8.
What is the abbreviation for centimeter?
a)
c
b)
cm
c)
m
d)
km
9.
The metric system is based on multiples of:
a)
100
b)
20
c)
10
d)
1
10.
What does the abbreviation km stand for?
a)
kilo
b)
kilometer
c)
kilogram
d)
meter
11.
1000 grams = _____ kilograms
a)
0.0001
b)
1,000,000
c)
10
d)
1
12.
What would be the best unit of measurement to measure the length of a toothbrush?
a)
millimeters
b)
meters
c)
centimeters
d)
kilometers
13.

To change kilometers to meters, move the decimal place...

a)

3 to the right.

b)

3 to the left.

c)

2 to the right.

d)

1 to the left.

14.

To change cm to m, move the decimal place...

a)

3 to the right.

b)

3 to the left.

c)

2 to the left.

d)

1 to the right.

15.

Convert 323 m to km.

a)

0.323 km

b)

3.23 km

c)

323,000 km

d)

3,230 km

16.

Convert 0.75 L to mL.

a)

750 mL

b)

75 mL

c)

75,000 mL

d)

0.0075 mL

17.

240 cm = ___________ m

a)

2400

b)

24

c)

2.4

d)

0.24

18.

1000 m = ___________ km

a)

100

b)

10

c)

1

d)

0.1

19.

2,804 mg = ___________ g

a)

0.2804

b)

2.804

c)

28.04

d)

280.4

20.

0.932 g = ___________ mg

a)

9.32

b)

93.2

c)

932

d)

9,320

21.

56 L = ___________ mL

a)

560

b)

5,600

c)

56,000

d)

560,000

22.

Which units are the BASE units in the metric system? Check all that apply.

a)

Meters

b)

Liters

c)

Grams

d)

Inches

e)

Miles

23.

What scientific tool is used to measure volume of liquids, such as water and chemicals?

a)

Meter Stick

b)

Ruler

c)

Graduated Cylinder

d)

Triple Beam Balance

24.

Which units below are NOT part of the metric system? Check all that apply.

a)

Inches

b)

Feet

c)

Meters

d)

Grams

25.

Which unit below is the largest?

a)

Kilogram

b)

Gram

c)

Centigrams

d)

Milligrams

26.

Which unit below is the SMALLEST?

a)

Kilometer

b)

Millimeters

c)

Meters

d)

Centimeters

27.
The atomic number tells you what?
a)
number of electrons
b)
number of protons
c)
number of neutrons
d)
both electrons and protons in an atom.
28.
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
29.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
30.
A proton is....
a)
A negatively charged subatomic particle
b)
A positively charged subatomic particle
c)
A neutrally charged subatomic particle
d)
The only subatomic particle located in the nucleus
31.

The mass of an atom, calculated by adding the number of protons and neutrons in the nucleus of the atom

a)

element name

b)

element symbol

c)

atomic number

d)

atomic mass

32.
These are found on the Periodic Table.
a)
Compounds
b)
Elements
c)
Mixtures
33.

the basic structural unit of matter

a)

atom

b)

matter

c)

element

d)

nucleus

34.

a subatomic particle, contained in the nucleus of an atom, having the same mass as a proton but no electrical charge

a)

proton

b)

neutron

c)

electron

d)

matter

35.

a negatively charged subatomic particle that orbits the nucleus of an atom

a)

proton

b)

neutron

c)

electron

d)

matter

36.

a grouping of elements based on similar properties, arranged by columns in the periodic table; also known as a group

a)

family

b)

period

c)

row

d)

isotope

37.

a row on the Periodic Table of Elements

a)

family

b)

period

c)

row

d)

isotope

38.
Most of the mass of an atom is found it its _____.
a)
electron cloud
b)
nucleus
c)
atomic number
d)
empty space
39.
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
40.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

41.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

42.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

43.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
44.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
45.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

46.

The chemical bond between a metal and a non-metal will be a _____ bond.

a)

metal

b)

ionic

c)

covalent

d)

polar

47.

Carbon and Oxygen will make a ___________ bond.

a)

ionic

b)

covalent

c)

metallic

48.

Nitrogen and Oxygen will make a ____________ bond

a)

ionic

b)

covalent

c)

metallic

49.
Ionic compounds are formed when one or more valence electrons are transferred from _____
a)
a nonmetal atom to a metal atom
b)
a nonmetal atom to a nonmetal atom
c)
a metal atom to a nonmetal atom
d)
a metal atom to a metal atom
50.
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
51.
Large bodies of water do not quickly fluctuate in temperature. Why?
a)
Water is a solvent.
b)
Water has a high heat capacity.
c)
Water acts as a buffer.
d)
Water is non-polar.
52.
Water is a universal solvent because it...
a)
It can be found anywhere
b)
It freezes when it gets cold
c)
floats when frozen
d)
Dissolves most substances
53.
The fact that ice floats on liquid water is due to the fact that water's solid is ___________ than it's liquid form
a)
less polar
b)
more polar
c)
less dense
d)
more dense
54.
Which end of the water molecule has a slightly positive charge?
a)
the oxygen end
b)
the hydrogen end
c)
both ends are slightly positive
d)
neither end is positive
55.

A type of strong chemical bond in which two atoms share one or more pairs of valence electrons.

a)

Covalent bond

b)

Hydrogen bond

c)

Ionic Bond

d)

Water Bond

56.
 Many fish and aquatic plants can survive a cold winter because the layer of ice that forms at the top of the lake insulates the water below and prevents the lake from freezing solid. What unique property of water contributes to this effect? 
a)
Water absorbs heat when it evaporates and forms a gas 
b)
 Water expands and becomes less dense when it freezes.
c)
Water molecules completely separate into ions in solutions.
d)
 Water forms hydrogen bonds with ions and other polar substances. 
57.
A florist places a bouquet of white carnations in water containing blue dye. After a time, the flowers turn blue. What process helped the carnations to change color?
a)
Specific heat 
b)
Surface tension
c)
Cohesion and adhesion of water molecules 
d)
Formation of covalent bonds between hydrogen and oxygen molecules
58.
Ionic or covalent?
Na  Br
a)
Ionic
b)
Covalent
59.
The abbreviation for liter is _________.
a)
liter
b)
l or L
c)
g
d)
m
60.
The abbreviation for kilogram is _______.
a)
KG
b)
Kl
c)
cg
d)
kg
61.
The metric unit of measurement for length is ____________________. 
a)
Liter
b)
Meter
c)
gram
d)
inch
62.
The metric unit of measurement for weight or mass is ________________.
a)
Gram
b)
Liter
c)
Pound
d)
Meter
63.
The metric unit of measurement for capacity or volume is ________________.
a)
Gram
b)
Meter
c)
Liter
d)
Ounce
64.
The abbreviation for centimeter is ________.
a)
CM
b)
cg
c)
cl
d)
cm
65.
The abbreviation for millimeter is ________.
a)
mm
b)
mi
c)
MM
d)
ml
66.
The abbreviation cg stands for ____________.
a)
kilogram
b)
centipede
c)
centigallon
d)
centigram
67.

9 meters = ___________cm

a)

900 cm

b)

90 cm

c)

0.9 cm

d)

0.09 cm

68.

8 kilometers equals how many meters?

a)

800 m

b)

80,000 m

c)

8,000 m

d)

0.008 m

69.
Convert 17 m to cm:
a)
0.17 cm
b)
0.017 cm
c)
1,700 cm
d)
170 cm
70.

The base metric unit of measurement for length is the:

a)

gram

b)

liter

c)

meter

d)

cm

71.

abbreviation

millimeter

a)

m

b)

mm

c)

me

d)

mt

72.

abbreviation

decimeter

a)

dm

b)

dam

c)

d

d)

dcm

73.

abbreviation

dekagram

a)

dag

b)

dg

c)

dkg

d)

dgm

74.

abbreviation

hectoliter

a)

hL

b)

hcL

c)

htL

d)

L

75.

What are the 6 main metric prefixes in order from largest to smallest?

a)

kilo, hecto, deka, deci, centi, milli

b)

milli, centi, deci, deka, hecto, kilo

c)

kilo, deka, deci, milli, centi, hecto

d)

milli, deka, hecto, kilo, deci, centi

76.

Water freezes at

a)

0 degrees Celsius

b)

32 degrees Celsius

c)

100 degrees Celsius

d)

212 degrees Celsius

77.

Which object has a mass of about one gram?

a)

a paper clip

b)

a book

c)

a chair

d)

a car

78.

Water boils at

a)

0 degrees Celsius

b)

32 degrees Celsius

c)

100 degrees Celsius

d)

212 degrees Celsius

79.

The amount of matter in something is its'

a)

mass

b)

volume

c)

length

d)

density

80.

Put these in order from smallest to BIGGEST

a)

millimeter, centimeter, meter, kilometer

b)

centimeter, millimeter, kilometer, meter

c)

meter, millimeter, centimeter, kilometer

d)

kilometer, meter, centimeter, millimeter

81.

Put these in order from smallest to BIGGEST

a)

milliliter, centiliter, liter, kiloliter

b)

centiliter, milliliter, kiloliter, liter

c)

liter, milliliter, centiliter, kiloliter

d)

kiloliter, liter, centiliter, milliliter

82.

Put these in order from BIGGEST to smallest

a)

milligram, centigram, gram, kilogram

b)

centigram, milligram, kilogram, gram

c)

gram, milligram, centigram, kilogram

d)

kilogram, gram, centigram, milligram

83.
Convert 0.25 m to mm
a)
25
b)
2.5
c)
250
d)
0.025
84.
Which is more 4 kg or 3,000 g?
a)
4 kg
b)
3,000 g
85.
Which is bigger 1g or 1kg?  Or are they equal?
a)
1g
b)
1kg
c)
equal
86.
Is 4,000 mg greater than, less than, or equal to 4 g?
a)
greater than
b)
less than
c)
equal to
87.
6,000 millilters = ______ liters
a)
60
b)
600
c)
6
d)
6,000
88.
Convert 17 m to cm:
a)
0.17 cm
b)
0.017 cm
c)
1,700 cm
d)
170 cm
89.
How do covalent bonds form?
a)
Donating & receiving valence e- between atoms.
b)
Opposite slight charges attract each other between compounds.
c)
Scientists are still not sure how they form.
d)
Sharing valence e- between atoms.
90.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
91.
What is the correct name for NO?
a)
Mononitrogen Monoxide
b)
Nitrogen Monoxide
c)
Mononitrogen Dioxide
d)
Nitrogen Oxide
92.
What is the formula for Tricarbon Octahydride?
a)
Ca3O
b)
C2H8
c)
C3H8
d)
Ca3H8
93.
What is Sulfur Trichloride?
a)
SCl3
b)
SiCl3
c)
SCl4
d)
Si3Cl
94.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
95.

An electron located in the outermost shell (valence shell) of the atom, that can be transferred to or shared with another atom.

a)

Ionic bond

b)

Valence electrons

c)

Ion

d)

Anion

96.

Bond formed by the transferring of electrons. Occurs between a metal (loses electrons) and a nonmetal (gains electrons).

a)

Ionic bond

b)

Ion

c)

Product

d)

Molecule

97.

A rule stating that atoms lose, gain, or share electrons in order to have 8 valence electrons.

a)

Reactant

b)

molecule

c)

Oxidation number

d)

Octet rule

98.

Which of the following pair of elements is most likely to form an ionic compound?

a)

Magnesium and fluorine

b)

Nitrogen and sulfur

c)

Oxygen and chlorine

d)

Sodium and aluminum

99.
How do the following two elements bond together?
Al3+  O2-         
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
100.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
101.
When a metal loses electrons, it becomes this type of ion.
a)
anion
b)
cation
102.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
103.
Ag +  and  Br -
a)
AgBr
b)
BrAg
c)
Ag2Br2
d)
Br2Ag2
104.
Ba +3 and  Cl-
a)
Ba3Cl
b)
Ba3Cl3
c)
BaCl3
d)
BaCl
105.
Elements in Group 1 lose one electron to form ions with a _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
106.
What is the charge of Neon?
a)
0
b)
+1
c)
-1
d)
1
107.
How many valence electrons does hydrogen have?
a)
1
b)
2
c)
3
d)
4
108.

Calcium Fluoride has a chemical formula of CaF2. What does the chemical formula tell you?

a)

There are 2 Calcium ions for every 1 Fluoride ion in the crystal

b)

There is 1 Calcium ion for every 2 Fluoride ions in the crystal

109.
What side of the periodic table are metals on?
a)
left
b)
right
c)
top
d)
bottom
110.
What side of the periodic table are nonmetals on?
a)
left
b)
right 
c)
top
d)
bottom
111.

Which of the following gases is not a noble gas?

a)

Helium

b)

Oxygen

c)

Neon

112.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
113.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

114.

The weaker the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

115.

In an endothermic reaction, heat is ...

a)

taken in

b)

given out

116.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
117.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
118.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
119.

O2(g) + 2 H2 (g) → 2 H2O (g) + EnergyO_2\left(g\right)\ +\ 2\ H_2\ \left(g\right)\ \rightarrow\ 2\ H_2O\ \left(g\right)\ +\ Energy  

a)

endothermic

b)

exothermic

120.

6 CO2+ 6 H2O + Energy → C6H12O6 + 6 O26\ CO_2+\ 6\ H_2O\ +\ Energy\ \rightarrow\ C_6H_{12}O_6\ +\ 6\ O_2

a)

endothermic reaction

b)

exothermic reaction

121.

A student mixed two chemicals to allow them to react. The temperature before the reaction was 25 ° C. The temperature after the reaction was 18° C. Which of the following is true?

a)

It is an exothermic reaction

b)

It is an endothermic reaction

122.

When an _____ reaction occurs, the reactants are at a lower energy.

a)

endothermic

b)

exothermic

123.

In a laboratory, a student combines vinegar and baking soda into a beaker. The initial temperature is 28 degrees Celsius and the final temperature reading two minutes later is 20 degrees Celsius. Was energy absorbed from or released to the surroundings?

a)

absorbed from

b)

released to

124.
The rate of a chemical reaction is NOT affected by which of the following:
a)
temperature
b)
concentration
c)
particle size (surface area)
d)
All of these affect reaction rates
125.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.

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