WorksheetsChemistry Final
Total questions: 76
Worksheet time: 1hrs 16mins
Name
Class
Date
1.
In a chemical equation, “dissolved in water” is represented by which of the following symbols?
a)
(s)
b)
(l)
c)
(g)
d)
(aq)
2.
How many atoms of oxygen are represented in
a)
2
b)
4
c)
8
d)
16
3.
A solid produced from two aqueous solutions in a chemical reaction is known as a(n)
a)
precipitate
b)
oxide
c)
salt
d)
hydrocarbon
4.
Classify the following reaction:
a)
double replacement
b)
single replacement
c)
combustion
d)
decomposition
5.
To balance a chemical equation, it may be necessary to change the substances’
a)
subscripts
b)
superscripts
c)
coefficients
d)
formulas
6.
Which of the following statements best describes the following reaction?
a)
it is a double replacement reaction
b)
it is a decomposition reaction
c)
it is a synthesis reaction
d)
the reaction will not occur
7.
Which of the following would not be considered evidence of a chemical reaction?
a)
Formation of a precipitate
b)
Production of a gas
c)
State of matter change
d)
Sudden release of light
8.
Which of the following statements best describes the following reaction?
a)
it is a single replacement reaction
b)
it is a decomposition reaction
c)
it is a synthesis reaction
d)
the reaction will not occur
9.
Which of the following best represents the general equation for a synthesis reaction?
a)
AB -> A + B
b)
A + B -> AB
c)
AX + B -> BX + A
d)
AX + BY -> AY + BX
10.
Balance the following reaction.
a)
1 + 1 ->1
b)
2 + 1 -> 2
c)
2 + 2 -> 2
d)
3 + 1 -> 3
11.
Classify the following reaction.
a)
synthesis
b)
single
c)
decomposition
d)
double
12.
Which of the following is the correct name for NiO?
a)
Nickel oxide
b)
Nickel (I) oxide
c)
Nickel (II) oxide
d)
None of these
13.
Micah tells his mom he can’t go to school today to take his chemistry test because he is running a temperature of 310.2 K. What is his temperature in degrees Fahrenheit?
a)
Option 1
b)
Option 2
c)
Option 3
d)
Option 4
14.
Using the graduated cylinder to the right, select the most accurate AND precise measurement.
a)
22 mL
b)
20 mL
c)
22.0 mL
d)
20.0 mL
15.
Balance the following reaction.
a)
1 + 1 -> 1 + 1
b)
2 + 1 -> 1 + 1
c)
2 + 2 -> 2 + 1
d)
3 + 3 -> 3 + 1
16.
Classify the following reaction.
a)
synthesis
b)
single
c)
decomposition
d)
double
17.
Balance the following reaction.
a)
1 -> 1 + 1
b)
1 -> 1 + 2
c)
2 -> 2 + 2
d)
2 -> 2 + 1
18.
Classify the following reaction.
a)
synthesis
b)
single
c)
decomposition
d)
double
19.
Balance the following reaction.
a)
1 + 1 -> 1 + 1
b)
1 + 2 -> 1 + 2
c)
2 + 2 -> 2 + 2
d)
3 + 1 -> 3 + 1
20.
Classify the following reaction.
a)
synthesis
b)
single
c)
decomposition
d)
double
21.
What mass of hydrogen would you expect to be produced from the reaction to the right?
a)
2 g
b)
63 g
c)
70 g
d)
200 g
22.
Complete the following equations. Then balance.
a)
BaS
b)
Option 2
c)
Option 3
d)
8 BaS
23.
Complete the following equations. Then balance.
a)
NaCl + CuS
b)
CuNa + ClS
c)
2 NaCl + CuS
d)
ClNa + SCu
24.
Complete the following equations. Then balance. Single: Mg + HCl ->
a)
MgCl + H
b)
2 MgClH
c)
2 MgCl + 2 H
d)
Option 4
25.
Find the molar mass of acetylene gas (C2H2)
a)
26.038 g
b)
28.63 g
c)
23.86 g
d)
26
26.
Determine the number of moles of water formed if you start with 12.00 moles of acetylene gas
a)
12 mol
b)
10 mol
c)
2 mol
d)
24 mol
27.
Calculate the mass produced, in grams, of carbon dioxide if 1.75 moles of oxygen react completely
a)
61.6 g
b)
66.1 g
c)
6.16 g
d)
6.61 g
28.
Determine the mass of oxygen gas needed to produce 180.0 grams of water
a)
799.3 g
b)
79.93 g
c)
7.993 g
d)
0.7993 g
29.
Consider if C2H2 is an empirical formula. What would be the molecular formula if a sample of the compound was found to have a molar mass of 78.114 g/mol?
a)
CH
b)
C2H2
c)
C3H3
d)
C6H6
30.
A neutral atom may contain 8 protons,
a)
9 neutrons and 10 electrons
b)
9 neutrons and 8 electrons
c)
8 neutrons and 10 electrons
d)
10 neutrons and 9 electrons
31.
You can determine the identity of an element if you know how many _____ it has
a)
protons
b)
neutrons
c)
electrons
d)
energy levels
32.
The nucleus of an atom has all of the following characteristics EXCEPT that it
a)
is positively charged
b)
is very dense
c)
contains nearly all the atom's mass
d)
contains nearly all the atom's volume
33.
The element boron has two naturally occurring isotopes – one with an atomic mass of 10.01 and another with an atomic mass of 11.01. Given the information provided on the periodic table, which do you think is the most abundant isotope?
a)
The one with an atomic mass of 10.01
b)
The one with an atomic mass of 11.01
c)
They are both equally as abundant
d)
Not enough information is provided to answer this
34.
An element with 5 protons, 6 neutrons, and 8 electrons has an atomic number of ____?
a)
5
b)
6
c)
8
d)
11
35.
An element with 5 protons, 6 neutrons, and 8 electrons has a mass number of ____?
a)
5
b)
6
c)
8
d)
11
36.
How many valence electrons does an atom of magnesium typically have?
a)
2
b)
3
c)
12
d)
24
37.
How many valence electrons does an atom of aluminum typically have?
a)
2
b)
3
c)
13
d)
27
38.
The number of energy levels an atom will have is based on the number of ______it has.
a)
protons
b)
neutrons
c)
electrons
d)
quarks
39.
Which of the following would NOT be found in the nucleus of an atom?
a)
protons
b)
neutrons
c)
electrons
d)
quarks
40.
Which statement about the arrangement of the periodic table is not true?
a)
Noble gases are on the right side of the periodic table.
b)
Metals are found on the right side of the periodic table.
c)
Halogens are on the right side of the periodic table.
d)
Transition metals are in the center of the periodic table.
41.
What kind of charge does an ion have?
a)
positive
b)
negative
c)
neutral
d)
can be positive or negative
42.
An atom is electrically neutral when its
a)
neutrons balance the protons and electrons.
b)
nuclear forces stabilize the charges.
c)
numbers of protons and neutrons are equal.
d)
numbers of protons and electrons are equal.
43.
Which statement about the relationship between viscosity and intermolecular forces is true?
a)
The stronger the intermolecular forces, the higher the viscosity.
b)
The stronger the intermolecular forces, the less resistant the fluid is to movement
c)
The stronger the intermolecular forces, the lower the viscosity
44.
Which of the following bonds would not be considered a type of intramolecular bond?
a)
covalent
b)
hydrogen
c)
ionic
d)
metallic
45.
Molecules that are symmetrical tend to be _____. Molecules that are asymmetrical tend to be ______.
a)
nonpolar; polar
b)
polar; nonpolar
c)
nonpolar; nonpolar
d)
polar; polar
46.
Which intermolecular force is responsible for the high surface tension of water?
a)
London dispersion forces
b)
Hydrogen bonds
c)
Covalent bonds
d)
Dipole-dipole forces
47.
Which intermolecular force is the strongest?
a)
London dispersion forces
b)
Hydrogen bonds
c)
Covalent bonds
d)
Dipole-dipole forces
48.
Which intermolecular force is the weakest?
a)
London dispersion forces
b)
Hydrogen bonds
c)
Covalent bonds
d)
Dipole-dipole forces
49.
What is the only type of intermolecular force that would have an impact on noble gases?
a)
London dispersion forces
b)
Hydrogen bonds
c)
Covalent bonds
d)
Dipole-dipole forces
50.
Identify the molecular shape for a diatomic element like
a)
linear
b)
bent
c)
triagonal planar
d)
tetrahedral
51.
Identify the molecular shape for an element with 3 electron domains
a)
linear
b)
bent
c)
triagonal planar
d)
tetrahedral
52.
Identify the molecular shape for a molecule with two bonding pairs and two lone pairs of electrons
a)
linear
b)
bent
c)
triagonal planar
d)
tetrahedral
53.
a)
London dispersion forces
b)
Hydrogen bonds
c)
Covalent bonds
d)
Dipole-dipole forces
54.
The most dominant intermolecular force at work between two HBr molecules would be
a)
London dispersion forces
b)
Hydrogen bonds
c)
Covalent bonds
d)
Dipole-dipole forces
55.
The most dominant intermolecular force at work between two water molecules would be
a)
London dispersion forces
b)
Hydrogen bonds
c)
Covalent bonds
d)
Dipole-dipole forces
56.
Identify the element with the following electron configuration:
a)
Be
b)
Si
c)
C
d)
F
57.
Identify the total amount of electrons in an element with this electron configuration:
a)
3
b)
5
c)
11
d)
15
58.
Identify the number of valence electrons in an element with this electron configuration:
a)
3
b)
5
c)
11
d)
15
59.
Which of the following statements is true about anions?
a)
Typically nonmetals
b)
Typically metals
c)
Tend to share electrons
d)
Tend to have positive charge
60.
Metals will ____ in reactivity as you move down and left in the periodic table. Nonmetals will ____ in reactivity as you move up and right
a)
increase; increase
b)
decrease; increase
c)
increase; decrease
d)
decrease; decrease
61.
Identify the element with the following electron configuration:
a)
K
b)
N
c)
Ge
d)
As
62.
Consider the periodic trend seen for ionic radius. Atoms that lose electrons tend to become _____. Atoms that gain electrons tend to become _____
a)
smaller; smaller
b)
larger; smaller
c)
smaller; larger
d)
larger; larger
63.
Which of the following groups of elements would most likely have the greatest electronegativity?
a)
Halogens
b)
Alkali metals
c)
Alkaline earth metals
d)
Transition metals
64.
Which of the following groups of elements would most likely have the least electronegativity?
a)
Halogens
b)
Alkali metals
c)
Alkaline earth metals
d)
Transition metals
65.
Two atoms have a difference in electronegativity of 2.34. What type of bond will they most likely form?
a)
covalent
b)
polar covalent
c)
ionic
d)
they will not form a bond
66.
Two atoms have a difference in electronegativity of 0. What type of bond will they most likely form?
a)
covalent
b)
polar covalent
c)
ionic
d)
they will not form a bond
67.
The energy required to remove one electron from a neutral atom of an element is known as
a)
electronegativity
b)
reactivity
c)
ionization energy
d)
quantum energy
68.
Which of the following would NOT be considered an electron domain?
a)
Electrons shared in a bond
b)
Lone pairs
c)
Double bond
d)
Central atom
69.
What is the coefficient of oxygen gas?
(a)
70.
What does the (l) in the equation represent?
(a)
71.
List the reactants in this reaction.
(a)
72.
What is the subscript of oxygen gas?
(a)
73.
Use the following clue and the periodic table to determine the identity of the element.
This element is in the same group as Br, but has fewer protons than Mg.
(a)
74.
Use the following clue and the periodic table to determine the identity of the element.
This element has 6 energy levels and 8 valence electrons.
(a)
75.
Use the following clue and the periodic table to determine the identity of the element.
This element is in the alkaline earth metals group and has 3 energy levels.
(a)
76.
Use the following clue and the periodic table to determine the identity of the element.
This element is in the group with the most reactive nonmetals and has 4 energy levels.
(a)
100 %
