stud
bud
Sign up
Log in
Home
Library
Explore
SAT
More
Semester 1 Final Review Flashcards | StudBud
Explore
/
Semester 1 Final Review
Semester 1 Final Review
100 terms
·
StudBud Administration
·
80 plays
Imported from external platform
Flashcards
100 cards
F
Practice quiz
P
Host live
L
Questions
100
Answers
1
The law of conservation of mass states that mass
cannot be transformed.
cannot be created or destroyed.
never changes its appearance.
is multiplied in every reaction.
2
The sun is made of mostly what element?
iron
hydrogen
oxygen
carbon
3
Which type of bond forms when electrons are taken from one atom, and given to another?
Ionic
Covalent
None of these
Metallic
4
The reactants in the following equation are
Na and Cl2
Cl
Na
NaCl
5
Sodium has 11 protons, 12 neutrons and 11 electrons. What is it's mass number?
11
12
23
22
6
How many kg is 1,000 g?
1 kg
100 kg
0.1 kg
10 kg
7
What is the SI base unit for measuring temperature?
degrees Celsius
Kelvin
degrees Fahrenheit
degrees Centigrade
8
Which of the following is an example of a quantitative observation.
It is 3 degrees today.
It is frigid today.
It is cold today.
It is freezing today.
9
This is the study of human behavior.
biology
natural sciences
chemistry
social sciences
10
The following reaction would be classified as
synthesis.
single replacement.
double replacement.
decomposition.
11
Which subatomic particle is largest in size?
neutrons
protons
electrons
12
In an atom, the number of protons equals the number of ____.
electrons
nuclei
neutrons
isotopes
13
Which is the correct name for CaCl2
Calcium Chlorite
Calcium chlorine
Calcium dichloride
Calcium chloride
14
Which of the following is an example of a derived unit?
kilograms
meters/second
Kelvin
meters
15
What is the chemical formula of carbon tetrachloride?
C4Cl
CCl4
CCl2
CCl
16
What type of bond will form between atoms of gold?
None of these
Ionic
Covalent
Metallic
17
The "arrow" in a chemical equation means
equals.
stop.
turn.
yields.
18
Which of the following is not a result of metallic bonding?
Brittleness
Conductivity
Malleability
Ductility
19
Chemistry is an example of a
social science.
fun time.
unnatural science.
natural science.
20
How does bond length relate to the strength of the bond?
Longer bonds are stronger bonds.
Bonds are the same strength regardless of the length.
Bond length does not affect the strength.
Shorter bonds are stronger bonds.
21
Which of the following IS NOT an example of a crystalline solid?
Plastic
All of these
Table Salt
Sugar
22
Temperature is a measure of
chemical energy.
potential energy.
average kinetic energy.
thermal energy.
23
Which group contains the most elements?
metals
metalloids
non-metals
24
Which of the following IS NOT a type of model that can be used in science?
a physical object
an inference
an event
a mathematical expression
25
Fluorine, chlorine, bromine and iodine are part of a family called _____.
noble gases
metalloids
alkali metals
halogens
26
The following reaction would be classified as
single replacement.
decomposition.
synthesis.
double replacement.
27
Which of the following is the SI unit for time?
seconds
days
hours
minutes
28
A bond between a metal and a non-metal is called:
Ionic
Metallic
Molecular
Covalent
29
The following reaction would be classified as
double replacement.
synthesis.
single replacement.
decomposition.
30
50 cm is how many mm?
5 mm
0.5 mm
500 mm
5,000 mm
31
When applied to balancing equations, the law of conservation of mass tells us that the
mass of the reactants will always be more.
mass of the products will never equal mass of the reactants.
# atoms of an element must be = for products & reactants.
mass of the products will always be more than the reactants.
32
Which state of matter will take the shape and volume of its container?
All of these
Liquid
Gas
Solid
33
How many dg is 4.56 dag?
456 dg
0.456 dg
4,560 dg
45.6 dg
34
In the following equation, the subscript of H in the product H
2
O is
2
8
1
4
35
During a change of state, the temperature of a substance will remain the same.
False
True
36
The following reaction would be classified as
decomposition.
single replacement.
double replacement.
synthesis.
37
In an endothermic process
energy is taken in.
energy is given off.
38
This is the attractive force between the surface of a liquid and a surrounding solid.
Capillary Action
Surface Tension
Cohesive forces
Suction
39
This is the state of matter where particles are close together but are able to slide past one another.
liquid
plasma
gas
solid
40
What is a valence electron?
An electron in outermost energy level.
An electron in the nucleus.
An electron in the innermost energy level.
The total number of electrons in an atom.
41
How does the atomic mass of the elements change as you move from top to bottom on the table?
Stays the same
Mass increases
Mass decreases
42
2 reactants, one 65 g & one 15 g, combine to make one product. The mass of the product is
15 g
65 g
50 g
80 g
43
Which state of matter has a definite volume, but will take the shape of its container?
Gas
Liquid
Plasma
Solid
44
How did Moseley change Mendeleev's periodic table?
He used atomic number instead of atomic mass.
He included physical properties like density.
He used atomic mass instead of atomic number.
He included chemical properties like bonding power.
45
A solid turns straight into a gas through the process of
deposition.
sublimation.
vaporization.
condensation.
46
The following reaction would be classified as
double replacement.
synthesis.
single replacement.
decomposition.
47
This is vaporization that occurs only on the surface of a liquid.
evaporation
freezing
condensation
boiling
48
This is the state of matter where particles are only able to vibrate.
Solid
Plasma
Gas
Liquid
49
A block of lead will sink when added to water. This occurs because the lead
beats up the water on the way to the bottom.
is less dense than the water.
is more dense than the water.
has the same density as the water.
50
Which type of bond forms when electrons are shared?
Metallic
Covalent
None of these
Ionic
51
The following reaction would be classified as
single replacement.
double replacement.
synthesis.
decomposition.
52
1 dekaliter is larger than 1 deciliter.
True
False
53
This is the closeness of a measurement to the actual value.
Exactness
Precision
Accuracy
Specificity
54
Mendeleev created the first periodic table by arranging the elements in order of _____.
increasing atomic number
increasing melting points and densities
increasing atomic mass
decreasing atomic mass
55
An anion is formed by when an atom
gains electrons
loses protons
gains protons.
loses electrons
56
If an atom has 15 electrons, how many protons will it have?
15
30
0
20
57
Anything with the ability to flow can be classified as
lava.
a solid.
a fluid.
a gas.
58
Which of the following statements about metals is true?
Metals are found to right of the stair-step line on the periodic table.
Metals typically display a very low luster.
Metals are able to be hammered into thin sheets.
Metals are good insulators
59
The following reaction would be classified as
single replacement.
decomposition.
double replacement.
synthesis.
60
Sodium has 11 protons, 12 neutrons and 11 electrons. What is it's atomic number?
22
11
23
12
61
The "beginning ingredients" in a chemical reaction are known as the
reactants
products
coefficients
subscripts
62
Particles are randomly in arranged in --- solids.
crystalline
amorphous
63
Which of the following statements about transition metals is true?
They are always found combined with another element in nature.
They include metals such as gold, silver and copper
They are the most reactive of all types of metals
They are extremely brittle.
64
The number of valence electrons can be determined by
the last digit of the group number.
the average atomic mass.
the atomic number.
the period number.
65
What type of bond forms when oxygen(O) and bromine(Br) bond?
Molecular
covalent
Metallic
Ionic
66
This is an educated guess.
an observation
a hypothesis
an inference
an experiment
67
This is the study of matter and how it interacts.
Chemistry
Biology
Physics
Botany
68
The following reaction would be classified as
double replacement.
decomposition.
single replacement.
synthesis.
69
Which state of matter CANNOT be classified as a fluid?
plasma
solid
liquid
gas
70
A liquid turns to a solid through the process of
freezing.
vaporization.
sublimation.
melting.
71
The kinetic molecular theory states that the particles in matter are
arranged in patterns.
always stuck in place.
always in motion.
arranged randomly.
72
How many mL is 63.4 L?
0.634 mL
0.0634 mL
6.34 mL
63,400 mL
73
The Greek prefix for the number 4 is
tetra-
tri-
hexa-
penta-
74
What is unique about noble gases?
form salts
exist as solid elements
Glow bright colors when electricity is added
Are very reactive
75
Why would it be difficult to determine the properties of a new synthetic element?
The element would not fit in the periodic table
The element's nuclei would break apart very quickly
The element would combine the properties of the nuclei
The element would lack properties of ordinary elements
76
In the following equation, the coefficient of the reactant O is
2
3
77
A bond between two non-metals is called:
Molecular
Metallic
Ionic
Covalent
78
The conversion factor for relating months to years is 1 month:12 years.
True
False
79
A mixture of 2 or more metals, such as steel, is called
an alloy.
a hybrid.
a crystal.
an emulsion.
80
The elements in a group on the periodic table ____.
are in the same period
have similar chemical symbols
have the same atomic mass
have similar properties
81
A material is ductile if it _____.
can be pulled or drawn into a long wire
is a mixture of metal with at least one other element
can be hammered or rolled into flat sheets
can transfer heat or electricity to another metal
82
The "end result" of a chemical reaction is known as the
coefficients.
products.
subscripts.
reactants.
83
Which group of elements share characteristics with both metals and non-metals?
lanthanides
salts
metalloids
halogens
84
How many valence electrons does oxygen have?
6
7
1
5
85
The small number that tells how many atoms are present is known as the
product.
reactant.
coefficient.
subscript.
86
Which of the following is an example of an exothermic process?
Sublimation
Condensation
Vaporization
Melting
87
A gas turns to a liquid through the process of
melting.
vaporization.
condensation.
freezing.
88
What is the name of NaCl?
monosodium monochloride
monosodium chlorine
sodium chloride
sodium monochloride
89
Which particles in atoms have a negative electric charge?
protons
nucleus
neutrons
electrons
90
What ion does Sulfur form?
-2
-1
+3
+1
91
This type of equation is known as
single replacement.
decomposition.
double replacement.
synthesis.
92
Which of the following is an accurate conversion factor?
1 foot: 12 inches
12 feet: 12 inches
12 feet:1 inch
1 feet: 1 inch
93
This is the 3-dimensional pattern formed by ionic compounds.
crystal lattice
crysallis
molecular substrate
metallic pattern
94
The elements that are not reactive are
elements in the carbon family
metals
noble gases
halogens
95
Which of the following is the correct conversion factor for days and weeks?
1 day: 1 week
7 days: 1 week
1 day: 7 weeks
7 days: 7 weeks
96
Which of the following is in the correct order from smallest unit to largest unit?
milli, kilo, deci
deci, milli, mega
milli, deci, kilo
deci, kilo, milli
97
What is the chemical formula for magnesium fluoride?
MgF
Mg2F2
MgF2
Mg2F
98
How many cg are in 0.033 hg?
3,300 cg
330 cg
3.3 cg
33 cg
99
When the following equation is balanced, the coefficient for KOH is
3
2
4
1
100
Melting is the change from
a liquid to a gas.
a solid to a liquid.
a liquid to a solid.
a gas to a liquid.
