WorksheetsFinal Review
Total questions: 67
Worksheet time: 3hrs 1mins
Name
Class
Date
1.
What is the atomic number?
a)
the number of protons in the nucleus
b)
the number of protons and neutrons in the nucleus
c)
the number of neutrons in the nucleus
d)
the number of protons in the energy levels
2.
What is the mass number?
a)
the number of protons in the nucleus
b)
the number of protons and neutrons in the nucleus
c)
the number of neutrons in the nucleus
d)
the number of protons and electrons in the atom
3.
What is the mass number of this atom?
a)
1
b)
3
c)
4
d)
7
4.
In order for an atom to be neutral what has to be true?
a)
The atom has more protons than neutrons
b)
The atom has more neutrons than protons
c)
The atom has the same number of protons and neutrons
d)
The atom has the same number of protons and electrons
5.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of e- and p+ together
b)
Subtract the number of e- from p+
c)
Subtract the number of p+ from the mass number
d)
Add the mass number to the number of e-
6.
Which subatomic particles contribute the most to the mass of an atom?
a)
Protons, Neutrons, Electrons
b)
Protons only
c)
Protons and Electrons
d)
Protons and Neutrons
7.
If an atom has 12 positively charged subatomic particles, which of the following must it also have to be considered a neutral atom?
a)
12 neutrons
b)
12 electrons
c)
12 protons
d)
24 protons and neutrons
8.
An atom has 10 protons, 15 neutrons and 10 electrons what is its mass number.
a)
20
b)
10
c)
35
d)
25
9.
An element with a mass number of 11 and an atomic number of 5 has how many neutrons?
a)
11
b)
5
c)
6
d)
16
10.
Water is an element
a)
true
b)
false
11.
Which subatomic particle determines the identity of an element?
a)
protons
b)
neutrons
c)
electrons
12.
Maximum number of electron that can occupy 3d orbital is
a)
2
b)
6
c)
8
d)
10
13.
What is the molar mass of NaCl?
a)
58.45g/mol
b)
28g/mol
c)
12g/mol
d)
6.02 x 1023
14.
What is the molar mass of C2H4O2?
a)
40g
b)
50g
c)
60g
d)
68g
15.
What would be the mass of 1.5mol H2O
a)
20
b)
27
c)
32
d)
40
16.
How many particles would be in 8.4 moles of Octane (C8H18)?
a)
5.77 x 1023
b)
5.04 x 1024
c)
5.77 x 1026
d)
5.04 x 1023
17.
How many molecules are in 32.4 grams of phosphorous pentoxide?
a)
1.76 x 1023 molecules
b)
0.29 moles
c)
1.76 x 1022 molecules
d)
0.29 molecules
18.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
19.
Find the percent composition of N2S2.
a)
N: 69.6% S: 30.4%
b)
N:36% S: 75.6%
c)
N: 96.6% S: 3.4%
d)
N: 30.4% S: 69.6%
20.
Find the percent composition of Mg in Mg3(PO4)2.
a)
27.75% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
21.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2
d)
MgN
22.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
23.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula
d)
Distance Formula
24.
What is the correct representation of 702.2g in scientific notation?
a)
7.02 x 103g
b)
70.22 x 101 g
c)
7.022 x 102 g
d)
70.22 x 102 g
25.
What is chemistry?
a)
the study of matter
b)
the study of the universe
c)
the study of science
d)
the study of numbers
26.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
27.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
28.
What is the maximum number of electrons that an orbital can have?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
29.
What is this element?
1s22s22p63s23p6
4s23d104p6
1s22s22p63s23p6
4s23d104p6
a)
Argon
b)
Krypton
c)
Selenium
d)
Bromide
30.
What atom matches this electron configuration?
[Xe] 6s2 4f14 5d9
[Xe] 6s2 4f14 5d9
a)
Mercury
b)
Gold
c)
Platinum
d)
Thallium
31.
What is the shorthand electron configuration for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p3
32.
How many valence electrons does Chlorine have?
a)
5
b)
2
c)
7
d)
5
33.
Which element is pictured?
a)
neon
b)
fluorine
c)
magnesium
d)
argon
34.
What noble gas should be used to write the shorthand configuration for Te?
a)
Ar
b)
Kr
c)
Xe
d)
Sb
35.
What element in Period 4 has 5 valence electrons?
a)
Zr
b)
As
c)
V
d)
Sb
36.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
37.
Electron arrangement that uses arrows
a)
Electron configuration
b)
Shorthand configuration
c)
Lewis dot structure
d)
Orbital diagram
38.
What type of bond forms when electrons are transferred from one atom to another?
a)
ionic bond
b)
atomic bond
c)
covalent bond
d)
metallic bond
39.
The bond between Na & F. Ionic or covalent?
a)
Ionic
b)
Covalent
40.
The bond between N & H. Ionic or covalent?
a)
Ionic
b)
Covalent
41.
Which of the following gives the correct chemical formula for the compound Magnesium Phosphide?
a)
Mg2P3
b)
MgP
c)
Mg3P2
d)
MgP2
42.
Which of the following gives the correct chemical formula for the compound Calcium Nitride?
a)
Ca2N3
b)
CaN
c)
Ca3N2
d)
CaN2
43.
Which of the following gives the correct chemical formula for the compound Dinitrogen Monoxide?
a)
NO
b)
N2O
c)
N2O2
d)
O2N2
44.
What is the correct chemical name for the ionic compound: Fe3N2
a)
Iron nitride
b)
Iron (III) nitride
c)
Iron (II) nitride
d)
TriIron dinitride
45.
What is the correct chemical name for the ionic compound: CuS
a)
copper sulfide
b)
copper (I) sulfide
c)
copper (II) sulfide
d)
copper monosulfide
46.
What is the correct chemical name for the molecular compound: CS2
a)
Carbon Sulfide
b)
Carbon diSulfide
c)
diCarbide diSulfide
d)
Carbon (II) Sulfide
47.
What type of atoms make a covalent bond?
a)
only Nonmetals
b)
Metal and a Nonmetal
c)
only Metals
d)
only Noble Gases
48.
Ionic bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
49.
What type of compound is CaF2?
a)
covalent
b)
ionic
c)
polar
d)
metallic
50.
Given the picture, what type of bond is holding the atoms together in this molecule?
a)
polar covalent bond
b)
nonpolar covalent bond
c)
ionic bond
d)
metallic bond
51.
What is the charge on the calcium ion?
a)
1+
b)
2+
c)
2-
d)
1-
52.
What is the name for the NO3- ion?
a)
nitrate ion
b)
nitrite ion
c)
nitrogan ion
d)
nitride ion
53.
Name the compound NH4OH
a)
ammonium hydroxide
b)
ammonia oxyhydride
c)
mononitrogen tetraoxihydride
d)
hydrogen nitrate
54.
Name the compound NH4OH
a)
ammonium hydroxide
b)
ammonia oxyhydride
c)
mononitrogen tetraoxihydride
d)
hydrogen nitrate
55.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?
Which element has the highest electronegativity?
a)
W
b)
X
c)
Y
d)
Z
56.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine
c)
bromine
d)
iodine
57.
The number of valence electrons in an element affects the reactivity of that element. Which element listed has the fewest valence electrons?
a)
beryllium (Be)
b)
sodium (Na)
c)
oxygen (O)
d)
neon (Ne)
58.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium
c)
francium
d)
cesium
59.
Balance this equation
_Al +_HCl --> _H2 +_AlCl3
a)
2,6,3,2
b)
it's already balanced
c)
4,12,3,4
d)
2,1,4,5
60.
What is the left part of a chemical equation called?
2H2 + O2 --> 2H2O
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products
c)
Yields
d)
Chemical Equation
61.
What is the right part of a chemical equation called...
2H2 + O2 --> 2H2O
2H2 + O2 --> 2H2O
a)
Reactants
b)
Products
c)
Yields
d)
Chemical Equation
62.
How many Mn atoms are found in the following compound?
3Cr(MnO4)6
3Cr(MnO4)6
a)
3
b)
4
c)
6
d)
18
63.
Element or compound?
O2
O2
a)
Element
b)
Compound
64.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
What mass of O2 will be needed to burn 36.1 g of B2H6?
What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)
124 g O2
65.
What is the mole ratio of H2O to H3PO4 in the following chemical equation? P4O10 + 6 H2O --> 4 H3PO4
a)
6:4
b)
4:6
c)
1:3
d)
3:1
66.
Balance the following reaction :
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
CaC₂(s) + H₂O(l) --> C₂H₂(g) + Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
67.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
100 %
