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WorksheetsChemistry Year Review
Total questions: 68
Worksheet time: 1hrs 8mins
Name
Class
Date
1.
Which state of matter has the least kinetic energy?
a)
solid
b)
liquid
c)
gas
d)
plasma
2.
At the melting point of a substance, there is a net balance between which phases?
a)
solid and liquid
b)
solid and gas
c)
gas and liquid
d)
solid, gas, and liquid
3.
Which phase of matter is described as neutral, fast-moving particles that will spread out to fill the volume of their container?
a)
gas
b)
liquid
c)
solid
d)
plasma
4.
What happens to the particles of a substance when it is heated?
a)
the particles move faster
b)
the particles move slower
c)
the particles get closer together
d)
the particles are more attracted to each other
5.
An element is...
a)
made of only one type of atom
b)
2 or more different elements bonded together
c)
2 different mixtures
d)
a solid suspended in a liquid
6.
A compound is...
a)
2 or more different elements bonded together
b)
made of only one type of atom
c)
2 different mixtures
d)
a solid suspended in a liquid
7.
A mixture that has the same proportions (mix) of components throughout is called a...
a)
homogeneous mixture
b)
heterogeneous mixture
c)
suspension
d)
colloid
8.
A mixture is different than a compound because its components are not...
a)
chemically bonded together
b)
near each other
c)
made of atoms
d)
able to be separated
9.
Which substance is an element?
a)
nitrogen (N₂)
b)
water (H₂O)
c)
ammonia (NH₃)
d)
salt (NaCl)
10.
What is an atom?
a)
the smallest unit of an element
b)
smallest living organism
c)
mixture of particles
d)
the center of a cell
11.
The 3 subatomic particles are protons, neutrons, and ____________.
a)
electrons
b)
neurons
c)
photons
d)
gluons
12.
The small, dense center of an atom is called the ...
a)
nucleus
b)
orbital
c)
energy level
d)
mitochondria
13.
Electrons have a _________ charge.
a)
negative
b)
positive
c)
neutral
d)
opposite
14.
Neutrons have a _________ charge.
a)
neutral
b)
negative
c)
positive
d)
opposite
15.
Protons have a _________ charge.
a)
positive
b)
neutral
c)
negative
d)
opposite
16.
What are orbitals?
a)
areas where electrons are most likely to be found
b)
areas where protons are most likely to be found
c)
flat sections of an atom
d)
pathways of planets around a star
17.
Which subatomic particles are in the nucleus of an atom?
a)
protons and neutrons
b)
protons and electrons
c)
electrons and neutrons
d)
protons, neutrons, and electrons
18.
What are valence electrons?
a)
electrons in the outer-most energy level
b)
electrons closest to the nucleus
c)
electrons in the third energy level
d)
electrons in full energy levels
19.
How many electrons can fit in the first energy level (closest to the nucleus)?
a)
2
b)
1
c)
8
d)
10
20.
What is the general rule for placing electrons in orbitals / energy levels?
a)
separate before pairing
b)
pair before separating
c)
only 8 electrons in each orbital
d)
at least 8 electrons in every energy level
21.
do you think we will ever learn anything new about atoms? or do people completely understand them now?
4 lines
22.
Dmitri Mendeleev's design for the periodic table was chosen over other designs because...
a)
it could PREDICT the properties of elements we had not discovered yet
b)
it was the most ORGANIZED
c)
it was the closest SHAPE to a rectangle
d)
it was the FIRST design ever made
23.
The groups of the periodic table are the columns going up and down. What does an element's group number tell us about its structure?
a)
number of valence electrons
b)
number of energy levels
c)
number of protons
d)
atomic mass
24.
The periods of the periodic table are the rows going across left and right. What does an element's period number tell us about its structure?
a)
number of energy levels
b)
number of valence electrons
c)
number of protons
d)
atomic mass
25.
How many valence electrons does an atom of magnesium have?
a)
2
b)
1
c)
3
d)
4
26.
How many valence electrons does an atom of sulfur have?
a)
6
b)
2
c)
3
d)
5
27.
How many energy levels does an atom of lithium (Li) have?
a)
2
b)
1
c)
3
d)
5
28.
How many energy levels does an atom of potassium (K) have?
a)
4
b)
1
c)
2
d)
3
29.
What happens when electrons get near each other?
a)
they repel each other
b)
they attract each other
c)
they bond with each other
d)
they cancel each other
30.
Which periodic trend is an atom's ability to attract electrons away from other atoms?
a)
electronegativity
b)
atomic radius
c)
first ionization energy
d)
ionic radius
31.
Which element on the periodic table has the highest electronegativity?
a)
Fluorine (F)
b)
Helium (He)
c)
Francium (Fr)
d)
Hydrogen (H)
32.
Why do the elements in group 18 have no electronegativity?
a)
they have full valence levels, so it takes too much energy to add more levels for extra electrons
b)
they are gases and they have too much energy for more electrons
c)
they have too many energy levels that are not filled yet
d)
they have very weak attractive forces from having a small number of protons
33.
The octet rule states that atoms are most stable when...
a)
they have a full valence energy level
b)
they have 8 shielding electrons
c)
they have 8 total electrons
d)
they have a full nucleus
34.
An ionic bond is the attraction between...
a)
cations and anions
b)
dogions and anions
c)
cations and onions
d)
north and south magnets
35.
When an atom of fluorine (F) becomes an ion, it will...
a)
gain 1 electron
b)
lose 1 electron
c)
gain 2 electrons
d)
lose 2 electrons
36.
When an atom of aluminum (Al) becomes an ion, it will...
a)
lose 3 electrons
b)
gain 3 electrons
c)
gain 5 electrons
d)
lose 5 electrons
37.
What is the charge of a calcium (Ca) ion?
a)
positive 2
b)
negative 2
c)
positive 1
d)
negative 1
38.
What is the charge of an oxygen (O) ion?
a)
negative 2
b)
positive 2
c)
negative 1
d)
positive 1
39.
During the formation of an ionic bond, nonmetals...
a)
take electrons away from metals
b)
give electrons to metals
c)
lose all of their valence electrons
d)
become positively charged
40.
During the formation of an covalent bond, nonmetals...
a)
share electrons with other nonmetals
b)
share electrons with metals
c)
gain electrons from metals
d)
lose electrons to other nonmetals
41.
What will be the formula of an ionic compound made of Mg and Cl? (draw the Lewis structures with the arrows)
a)
MgCl₂
b)
MgCl
c)
Mg₂Cl
d)
Mg₂Cl₂
42.
What will be the formula of an ionic compound made of Li and P?
a)
Li₃P
b)
LiP₂
c)
LiP
d)
Li₃P₃
43.
What will be the formula of a covalent compound made of N and H? (draw the Lewis structures with the circles)
a)
NH₃
b)
NH
c)
NH₂
d)
N₂H₂
44.
What will be the formula of a covalent compound made of S and Cl?
a)
SCl₂
b)
SCl
c)
S₂Cl
d)
SCl₃
45.
What will be the formula of a covalent compound made of C and O? (draw the Lewis structures with the circles)
a)
CO₂
b)
CO
c)
CO₄
d)
C₂O
46.
Which type of bonding will occur between 2 atoms with very similar electronegativity values?
a)
covalent
b)
ionic
47.
Which type of bonding will occur between 2 atoms with very different electronegativity values?
a)
ionic
b)
covalent
48.
VSEPR Theory helps us predict the ________ of molecules since we know how many electrons pairs will be repelling each other.
a)
shape
b)
size
c)
bond length
d)
bond strength
49.
What is the name of the compound NaCl?
a)
sodium chloride
b)
sodium monochloride
c)
nitrogen chloride
d)
sodium chlorine
50.
What is the name of the compound Al₂S₃?
a)
aluminum sulfide
b)
dialuminum trisulfide
c)
aluminum sulfur
d)
aluminum trisulfur
51.
What is the name of the compound CH₄?
a)
carbon tetrahydride
b)
carbon hydride
c)
carbon hydrogen
d)
carbon tetrahydrogen
52.
What is the name of the compound P₂O₅?
a)
diphosphorus pentoxide
b)
phosphorus dioxide
c)
diphosphide pentoxygen
d)
phosphorus dipentoxide
53.
What do we call the substances that start a reaction?
a)
Reactants
b)
Products
c)
Yield Arrows
d)
Ingredients
54.
What do we call the substances that are formed during a reaction?
a)
Reactants
b)
Products
c)
Yield Arrows
d)
Ingredients
55.
A chemical reaction is different than a physical change because by the end of a chemical reaction...
a)
there is a transfer of heat
b)
there has been a change of phase
c)
reactants have changed their forms
d)
a different substance has been produced
56.
Which type of reaction combines 2 or more reactatnts into one product?
a)
synthesis
b)
decomposition
c)
combustion
d)
single replacement
57.
Which type of reaction is a fuel that burns in the presence of oxygen?
a)
synthesis
b)
decomposition
c)
combustion
d)
single replacement
58.
Which type of reaction is one element taking the place of another element in a compound?
a)
decomposition
b)
combustion
c)
single replacement
d)
double replacement
59.
Which type of reaction includes two different compounds that exchange components?
a)
decomposition
b)
combustion
c)
single replacement
d)
double replacement
60.
Which type of reaction is when one reactant breaks apart into pieces?
a)
decomposition
b)
combustion
c)
single replacement
d)
double replacement
61.
What is the law of conservation of mass?
a)
new atoms can be created during chemical reactions
b)
atoms can not be created or destroyed during a chemical reaction
c)
the mass at the end of the reaction can be different than the mass at the beginning
d)
every atom must be bonded to other atoms by the end of a chemical reaction
62.
Which chemical reaction is balanced?
a)
H₂ + 2 O₂ --> H₂O
b)
3 N₂ + 6 H₂ --> 2 NH₃
c)
Li + CaCl₂ --> LiCl + Ca
d)
CH₄ + 2 O₂ --> CO₂ + 2 H₂O
63.
Which graph represents a reaction that is exothermic?
a)
b)
64.
What does a catalyst do in a chemical reaction?
a)
makes the particles collide more
b)
absorbs heat from the surroundings
c)
lowers the activation energy needed to start
d)
bonds with both reactants to make a different product
65.
Collision Theory explain that we need 3 conditions for a reaction: 1) reactants must collide, 2) they must collide in the correct orientation, and 3)...
a)
the collisions must be between at least three particles
b)
the collisions must have enough energy to start the reaction
c)
the collisions must absorb energy from the surroundings
d)
the collisions must cause other collisions in a chain reaction
66.
What will happen to most chemical reaction if you heat them?
a)
go slower
b)
go faster
c)
nothing
d)
explosions!
67.
What will happen to most chemical reaction if you increase the concentration of reactants?
a)
go slower
b)
go faster
c)
nothing
d)
explosions!
68.
Breaking up a reactant into very small pieces makes a reaction go faster because...
a)
breaking things apart is fun
b)
the small pieces can move more
c)
there will be more reactant than we started with
d)
there will be more surface area for collisions
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