WorksheetsChem for Life 1st Semester Review
Total questions: 88
Worksheet time: 44mins
Name
Class
Date
1.
Indicate the dependent variable
a)
reaction pathway
b)
time
c)
catalyst
d)
energy
2.
Indicate the independent variable
a)
reaction pathway
b)
time
c)
catalyst
d)
energy
3.
Barney measured the mass of 12.78 grams of sugar in the density lab. How would you best describe the observation in the prior statement?
a)
qualitative
b)
quantitative
c)
homogeneous
d)
heterogeneous
4.
The Empire State Building is really tall. How would describe the observation in the prior statement?
a)
qualitative
b)
quantitative
c)
homogeneous
d)
heterogeneous
5.
The fundamental chemical substance from which all other substances are made is known as a(n)
a)
mixture
b)
element
c)
compound
d)
solution
6.
A substance composed of two or more elements bonded together in fixed proportions that cannot be broken down into simpler substances by physical means is known as a(n)
a)
mixture
b)
element
c)
compound
d)
ion
7.
Sugar water is an example of
a)
mixture
b)
element
c)
compound
d)
molecule
8.
Alka-Seltzer placed in water and bubbling is an example of a _____?
a)
physical property
b)
physical change
c)
chemical property
d)
chemical change
9.
The flammability of a substance, is a
a)
physical property
b)
physical change
c)
chemical property
d)
chemical change
10.
Chicken noodle soup is what type of mixture?
a)
heterogeneous
b)
homogeneous
c)
colloid
d)
physical
11.
Ice floats in water because…..
a)
Water is more dense than ice
b)
Water is less dense than ice
c)
Ice is more dense than water
d)
Ice actually sinks in water
12.
A particle found in the nucleus of an atom that doesn’t have a charge.
a)
electron
b)
neutron
c)
proton
d)
isotope
13.
A particle with very little mass, a negative charge, and orbits around the nucleus is called a(n)
a)
electron
b)
neutron
c)
proton
d)
isotope
14.
The smallest building block of matter that we studied in chemistry for life (aka: the fundamental unit of matter).
a)
atom
b)
neutron
c)
nucleus
d)
isotope
15.
A particle found in the nucleus of an atom that has a positive charge.
a)
electron
b)
neutron
c)
proton
d)
isotope
16.
All neutral atoms have the same ____
a)
number of protons and electrons
b)
number of protons and neutrons
c)
number of neutrons and electrons
d)
mass number
17.
The result of Rutherford’s Gold Foil Experiment and the current accepted atomic structure, the nucleus of an atom is:
a)
The average mass of one atoms of an element
b)
The number of neutrons
c)
negatively charged and has a high density
d)
positively charged and has a high density
18.
Two atoms of the same element that have different numbers of neutrons are said to be:
a)
isotopes
b)
isomers
c)
ions
d)
molecules
19.
Which of the following shows the correct Lewis Dot Diagram for an Oxygen (O) atom?
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
20.
The electron cloud model of the atom ______.
a)
Defines the exact path of an electron around the nucleus
b)
Was proposed by Niels Bohr
c)
Involves the probability of finding an electron in a certain location around the nucleus
d)
Doesn’t show electrons
21.
All of the following characteristics of most metals EXCEPT:
a)
have luster
b)
malleable
c)
brittle
d)
good conductor of electricity
22.
Where are Noble gases on the periodic table?
a)
Group 1A/1
b)
Group 2A/2
c)
Group 7A/17
d)
Group 8A/18
23.
The chemical properties of an element are determined by its
a)
atomic mass
b)
proton number
c)
electron arrangement
d)
atomic size
24.
Group I (the alkali metals) include lithium (Li), sodium (Na), and potassium (K). These elements have similar chemical properties because they have the same ___
a)
numbers of protons and neutrons
b)
numbers of electrons in their highest energy level
c)
numbers of protons in the nucleus
d)
numbers of neutrons in the nucleus
25.
Which elements are in the same period?
a)
B, Si, As
b)
Na, Mg, Al
c)
F, Cl, Br
d)
Fr, La, Rn
26.
How many protons (p) and neutrons (n) are in an atom of ⁹⁰₃₈Sr ?
a)
38 p, 90 n
b)
38 p, 52 n
c)
90 p, 38 n
d)
52 p, 38 n
27.
What is the correct temperature reading on the Celsius thermometer above (meaning you are reading the thermometer precisely)?
a)
15 °C
b)
15.67 °C
c)
16 °C
d)
15.6 °C
28.
How many protons are found in Manganese?
a)
55
b)
80
c)
25
d)
30
29.
How many electrons are found in an atom of Manganese?
a)
55
b)
80
c)
25
d)
30
30.
How many neutrons are found in an atom of Manganese with a mass number of 55?
a)
55
b)
80
c)
25
d)
30
31.
What is the average atomic mass of Manganese?
a)
55
b)
54.94
c)
25
d)
30
32.
What is the Mass number for a Manganese atom with 28 neutrons?
a)
55
b)
54.94
c)
54
d)
53
33.
How do we determine the mass number of an atom?
a)
electrons + neutrons
b)
protons + electrons
c)
protons + neutrons
d)
atomic mass - protons
34.
What is A pointing to?
a)
electrons
b)
protons
c)
neutrons
d)
orbital
35.
What is B pointing to?
a)
electrons
b)
protons
c)
neutrons
d)
orbital
36.
What is C pointing to?
a)
electrons
b)
protons
c)
neutrons
d)
orbital
37.
What is the name of this element?
a)
Boron
b)
Carbon
c)
Nitrogen
d)
Oxygen
38.
What is the atomic number for the atom in image pictured?
a)
6
b)
5
c)
14
d)
8
39.
What is the overall charge of the atom?
a)
positive
b)
negative
c)
neutral
d)
polar
40.
What is the region of the atom where the protons and neutrons are found?
a)
orbitals
b)
inner energy levels
c)
outer energy levels
d)
nucleus
41.
What is the mass number of the element in the image?
a)
6
b)
7
c)
11
d)
8
42.
Which of the following combination of elements are needed to make an ionic compound?
a)
metal + metal
b)
metal + non metal
c)
non metal + non metal
d)
metalloid + metalloid
43.
Which of the following combination of elements are needed to make an covalent compound?
a)
metal + metal
b)
metal + non metal
c)
non metal + non metal
d)
metalloid + metalloid
44.
In which set do all elements tend to form CATIONS in binary ionic compounds?
a)
O, F, Cl
b)
N, As, Bi
c)
Li, B, O
d)
Mg, Cr, Pb
45.
In which set do all elements tend to form ANIONS in binary ionic compounds?
a)
O, F, Cl
b)
Li, N, Cl
c)
K, Fe, Br
d)
Mg, Cr, Pb
46.
Magnesium Iodide is made up of which of the following pairs of ions?
a)
Mg⁺¹ , I⁻¹
b)
Mg⁺², I⁻²
c)
Mg⁺¹ , I⁻²
d)
Mg⁺² , I⁻¹
47.
Which of the following statements about chemical formulas is FALSE?
a)
The subscripts represent the relative number each type of atom in the compound.
b)
The subscripts represent the relative mass of each type of atom in the compound.
c)
Different compounds made of the same elements have different subscripts.
d)
The subscripts do not change for a given compound.
48.
What is the charge on the Cr in the ionic compound Cr₂O₃?
a)
+2
b)
+1
c)
+3
d)
-2
49.
Li₂S is named
a)
lithium (II) sulfide.
b)
lithium sulfide.
c)
lithium sulfur.
d)
lithium disulfide.
50.
The chemical formula for calcium nitrate is
a)
Ca(NO₂)₂
b)
CaN₂
c)
Ca₂N
d)
Ca(NO₃)₂
51.
The compound, CuCl₂, is named
a)
copper (II) chloride
b)
copper (I) chloride (II)
c)
copper (I) chloride
d)
copper chloride (II)
52.
An unknown liquid has the mass of 15.3 g and the volume of 20 mL. What is the density of the unknown liquid?
a)
1.31 g/mL
b)
306 g/mL
c)
13.07 mL/g
d)
0.765 g/mL
53.
Given the density of an unknown liquid is 0.92 g/mL, what would it do in water? Water has a density of 1.00 g/mL.
a)
Sink
b)
Float
54.
A platinum ring has the density of 21.46 g/mL, if the ring has a mass of 25 g. What will the volume of the ring be?
a)
1.16 mL
b)
1.16 g
c)
0.858 mL
d)
536.5 mL
55.
Magnesium metal reacts with hydrochloric acid solution according to the following equation: ___ Mg + ___ HCl → ___ MgCl₂ + ___ H₂ What coefficients are necessary to balance the equation?
a)
1, 1 → 1, 1
b)
1, 1 → 1, 2
c)
1, 2 → 1, 2
d)
1, 2 → 1, 1
56.
Magnesium metal reacts with hydrochloric acid solution according to the following equation: ___ Mg + ___ HCl → ___ MgCl₂ + ___ H₂ What type of chemical reaction is the reaction above?
a)
synthesis
b)
decomposition
c)
single replacement
d)
double replacement
e)
combustion
57.
Given the general arrangement AB + CD → CB + AD, one can predict that this is a
a)
Synthesis reaction
b)
Decomposition reaction
c)
Single replacement reaction
d)
Double replacement reaction
58.
Given the general arrangement A + D → AD, one can predict that this is a
a)
Synthesis reaction
b)
Decomposition reaction
c)
Single replacement reaction
d)
Double replacement reaction
59.
Given the general arrangement AB → B + A, one can predict that this is a
a)
Synthesis reaction
b)
Decomposition reaction
c)
Single replacement reaction
d)
Double replacement reaction
60.
Given the general arrangement A + CD → AC + D, one can predict that this is a
a)
Synthesis reaction
b)
Decomposition reaction
c)
Single replacement reaction
d)
Double replacement reaction
61.
Balance the following reaction: ___ FeCl₃ + ___ Pb(NO₃)₂ → ___ PbCl₂ + ___ Fe(NO₃)₃
a)
3, 2 → 2, 3
b)
2, 3 → 3, 2
c)
1, 3 → 3, 1
d)
2, 1 → 3, 2
62.
Balance the following reaction: ___Al + ___ O₂ → ___ Al₂O₃
a)
2, 3 → 3
b)
4, 3 → 2
c)
4, 3 → 4
d)
2, 2 → 2
63.
Balance the following reaction: ___ C₂H₄ + ___ O₂ → ___ H₂O + ___ CO₂
a)
1, 3 → 2, 2
b)
2, 6 → 4, 6
c)
1, 2 → 2, 2
d)
2, 8 → 2, 4
64.
Balance the following reaction: ____ HNO₃ → ___ N₂O₅ + ____ H₂O
a)
6 → 2, 3
b)
2 → 1, 1
c)
2 → 2, 1
d)
3 → 2, 1
65.
Balance the following reaction: ___ Mg + ___ Cu₃(PO₄)₂ → ___ Mg₃(PO₄)₂ + ___ Cu
a)
3, 1 → 1, 3
b)
1, 3 → 3, 1
c)
3, 2 → 2, 3
d)
1, 1 → 1, 1
66.
What type of reaction is the following: ___ FeCl₃ + ___ Pb(NO₃)₂ → ___ PbCl₂ + ___ Fe(NO₃)₃
a)
Synthesis
b)
Combustion
c)
Decomposition
d)
Single Replacement
e)
Double Replacement
67.
What type of reaction is the following: ___Al + ___ O₂ → ____ Al₂O₃
a)
Synthesis
b)
Combustion
c)
Decomposition
d)
Single Replacement
e)
Double Replacement
68.
What type of reaction is the following: ___ C₇H₁₆ + ___ O₂ → ___ H₂O + ___ CO₂
a)
Synthesis
b)
Combustion
c)
Decomposition
d)
Single Replacement
e)
Double Replacement
69.
What type of reaction is the following: ____ HNO₃ → ___ N₂O₅ + ____ H₂O
a)
Synthesis
b)
Combustion
c)
Decomposition
d)
Single Replacement
e)
Double Replacement
70.
What type of reaction is the following: ___ Mg + ___ Cu₃(PO₄)₂ → ___ Mg₃(PO₄)₂ + ___ Cu
a)
Synthesis
b)
Combustion
c)
Decomposition
d)
Single Replacement
e)
Double Replacement
71.
What is the name of the part of the equation with the corresponding number 1?
a)
solid
b)
yields
c)
gas
d)
reactants
e)
liquid
72.
What is the name of the part of the equation with the corresponding number 2?
a)
reactants
b)
yields
c)
gas
d)
liquid
e)
aqueous solution
73.
What is the name of the part of the equation with the corresponding number 3?
a)
coefficient
b)
yields
c)
gas
d)
reactants
e)
liquid
74.
What is the name of the part of the equation with the corresponding number 4?
a)
liquid
b)
yields
c)
gas
d)
reactants
e)
aqueous solution
75.
What is the name of the part of the equation with the corresponding number 5?
a)
yields
b)
gas
c)
reactants
d)
liquid
e)
aqueous solution
76.
What is the name of the part of the equation with the corresponding number 6?
a)
products
b)
yields
c)
gas
d)
reactants
e)
liquid
77.
What is the name of the part of the equation with the corresponding number 7?
a)
aqueous solution
b)
yields
c)
gas
d)
reactants
e)
liquid
78.
What is the name of the part of the equation with the corresponding number 8?
a)
gas
b)
yields
c)
reactants
d)
liquid
e)
aqueous solution
79.
Which of the following symbols is NOT a correct indication of the phase of a substance in a reaction?
a)
(s) solid
b)
(l) liquid
c)
(g) grams
d)
(aq) aqueous or dissolved in water
e)
all are correct
80.
Electrons that are equally shared form a(n)
a)
metallic bond
b)
ionic bond
c)
covalent bond
d)
adhesive bond
81.
A chemical reaction is a process in which
a)
reactants change into products
b)
the law of conservation of mass applies
c)
substances can change state
d)
all of these options
82.
During a chemical reaction
a)
new elements are produced
b)
atoms are destroyed
c)
atoms are rearranged
d)
elements are destroyed
83.
An equation is balanced by
a)
changing subscripts
b)
adding coefficients
c)
erasing elements as necessary
d)
adding elements as necessary
84.
What are the reactants in the following equation: Zn + CuSO₄ ⟶ ZnSO₄ + Cu
a)
Zinc and copper
b)
Zinc and copper (II) sulfate
c)
Zinc sulfate and copper
d)
only zinc
85.
What are the products in the following equation: Zn + CuSO₄ ⟶ ZnSO₄ + Cu
a)
Zinc and copper
b)
Zinc and copper (II) sulfate
c)
Zinc sulfate and copper
d)
only zinc
86.
Chemical equations must be balanced in order to maintain
a)
law of conservation of energy
b)
law of definite proportions
c)
law of conservation of mass
d)
Newton's laws of motion
87.
Which of the following is a chemical change?
a)
pouring a glass of milk
b)
adding chocolate syrup to the milk
c)
stirring the chocolate syrup into the milk
d)
letting the milk sit out overnight and waking up to find it soured
88.
Which of the following is NOT a chemical change?
a)
lighting a match
b)
lighting a bunsen burner
c)
ice in a beaker over the bunsen burner
d)
adding pieces of calcium to water in a beaker and forming calcium hydroxide
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