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Chemistry - Semester 1 Review

Total questions: 100

Worksheet time: 2hrs 18mins

Name
Class
Date
1.

What is the atomic mass of Neon?

a)

10

b)

20.18

c)

10.18

d)

21

2.

How many electrons does an Iodine atom have?

a)

53

b)

126

c)

73

d)

179

3.

What does the topmost number (3) represent?

a)

Mass Number

b)

Atomic Number

c)

Atomic Mass

d)

Number of Neutrons

4.

How many neutrons does an Oxygen atom have?

a)

8

b)

16

c)

24

d)

7.999

5.
Measure mainly of the nuclear particles: protons + neutrons
a)
Subatomic Particles
b)
Atomic Number
c)
Atomic Mass
d)
Gluons
6.
Value representing the number of protons in an element
a)
Atomic Mass
b)
Mass Number
c)
Valence Electrons
d)
Atomic Number
7.

The smallest particle of an element.

a)

Element

b)

Molecule

c)

Atom

8.

The nucleus of an atom contains which subatomic particles?

a)

protons and electrons

b)

protons and neutrons

c)

electrons and neutrons

d)

protons, electrons, and neutrons

9.
An atom with 19 protons, and 19 electrons and a mass of 39 has how many neutrons?
a)
19
b)
39
c)
20
d)
58
10.
Which of the subatomic particles is the heaviest?
a)
electrons 
b)
protons 
c)
neutrons 
d)
protons and neutrons have equal mass
11.

period

a)

Elements that occur in vertical columns on the periodic table.

b)

A horizontal row of elements in the periodic table

c)

Found in group two of the periodic table; highly reactive

d)

A subatomic particle that has a negative charge

12.

found in group one of the periodic table; highly reactive

a)

Non-metals

b)

Transition Metals (Groups 3-12)

c)

alkali metals (group 1)

d)

metalloids (semimetals)

13.

not able to conduct heat or electricity, little to no metallic luster

a)

Non-metals

b)

noble gases

c)

atomic mass

d)

Neutron

14.

Found in group two of the periodic table; highly reactive

a)

period

b)

Alkali Earth Metals (Group 2)

c)

metalloids (semimetals)

d)

alkali metals (group 1)

15.

The electrons in the outermost shell (main energy level) of an atom; these are the electrons involved in forming bonds

a)

alkali metals (group 1)

b)

Halogens (Group 17)

c)

atomic number

d)

valence electrons

16.

Halogens (Group 17)

a)

gas at room temperature, low boiling point.

b)

most reactive nonmetals

c)

The electrons in the outermost shell (main energy level) of an atom; these are the electrons involved in forming bonds

d)

Number of protons and neutrons

17.

Elements that occur in vertical columns on the periodic table.

a)

Neutron

b)

metalloids (semimetals)

c)

groups

d)

Proton

18.

metalloids (semimetals)

a)

Elements that occur in vertical columns on the periodic table.

b)

an element that has both metallic and nonmetallic properties

c)

not able to conduct heat or electricity, little to no metallic luster

d)

found in group one of the periodic table; highly reactive

19.

Noble Gases are in group # ___.

a)

12

b)

18

c)

8

d)

3

20.

These elements are really bad at conducting heat/electricity.

a)

Non-metals

b)

Transition Metals

c)

Metals

d)

Metalloids

21.

These are normally solid at room temperature.

a)

Metals

b)

Halogens

c)

Noble Gases

d)

Non-metals

22.
Which group has the most reactive nonmetals?
a)
alkali metals
b)
noble gases
c)
metalloids
d)
halogens
23.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
24.

Which of the following atoms has the greatest atomic radius?

a)

nitrogen

b)

phosphorus

c)

potassium

d)

cesium

25.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
26.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
27.

What is the amount of energy required to remove an electron from an atom?

a)

atomic energy

b)

ionization energy

c)

ionic energy

d)

electron energy

28.

What is a measure of the tendency of an atom to attract a bonding pair of electrons when the atom is in a compound?

a)

ionization energy

b)

electropositivity

c)

electronegativity

d)

electron energy

29.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
30.

A positively charged ion that has lost electrons

a)

Anion

b)

Cation

c)

Neutral Atom

d)

Isotope

31.

Atoms of the same element that have different mass than expected because they have a different number of neutrons.

a)

Neutral Atom

b)

Ion

c)

Isotope

d)

Cation

32.

If an atom has 9 protons and 10 electrons it has a charge of ____.

a)

0

b)

-1

c)

+1

d)

-2

33.

What do these isotopes have in common?

a)

the number of protons in the nucleus

b)

the number of electrons in the nucleus

c)

the number of protons and neutrons in the nucleus

34.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
35.
A neutral atom of Boron has 5 p+, 6 n, and 5 e-. The Boron atom pictured is a....
a)
Positive ion
b)
Negative ion
c)
Isotope
d)
Neutral atom
36.

Consider all of the isotopes of mercury listed here, whether they are neutral or charged. What is true about this group of isotopes?

a)

Electrons, protons, and neutrons must always be the same.

b)

Protons must always be the same, but electrons and neutrons may change.

c)

Electrons must always be the same, but protons and neutrons may change.

d)

Protons and neutrons must stay the same, but electrons may change.

37.

How many neutrons are in the following isotope?

a)

108

b)

47

c)

61

d)

155

38.
When metals bond with non-metals they form what type of bonds
a)
covalent
b)
ionic
c)
cooperative
d)
lewis
39.
name the following ionic compound: NaF
a)
nitrogen fluorine
b)
sodium fluoride
c)
nitrogen fluoride
d)
sodium fluorine
40.
The chemical formula of carbon tetrachloride is
a)
CCl
b)
C₄Cl
c)
CCl₄
d)
C(IV)Cl
41.

How many Oxygen atoms are in H2O?

a)

1

b)

2

c)

0

d)

4

42.

Classify:

sulfur dioxide, SO2

a)

ionic compound

b)

covalent compound

c)

metallic element

d)

non-metallic element

43.

A compound has a weak bond, low melting point, and can dissolve in water.

a)

Ionic

b)

Covalent

c)

Metalic

d)

No Clue

44.

Alloys are examples of:

a)

ionic compounds

b)

covalent compounds

c)

metal compounds

d)

elements

45.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
46.
How do the following two elements bond together?
K1+  S2- 
a)
KS
b)
K8S
c)
K6S3
d)
K2S
47.
The proper formula for magnesium hydroxide:
a)
MgOH
b)
Mg2OH
c)
Mg(OH)2
d)
Mg2OH2
48.
Name the following ionic compound: LiNO3
a)
lithium nitrate
b)
lithium III nitrate
c)
lithium nitride
d)
lithium oxide
49.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
50.
The chemical formula of lead (IV) nitrate is
a)
PbN₄
b)
PbNO₃₄
c)
Pb(NO₃)₄
d)
Pb₃NO₄
51.
What is the formula for copper(I) sulfate?
a)
CuSO3
b)
CuSO4
c)
Cu2SO3
d)
Cu2SO4
52.

Which of the following best describes covalent compounds?

a)

Transfer electrons

b)

Share electrons

c)

Have electrons floating in a "sea" of electrons

53.

BCl3 can be used in soldering fluxes. What is the chemical name for BCl3?

a)

boron chloride

b)

boride chloride

c)

boron trichloride

d)

boron chlorine

54.
What is the formula for nitric acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
55.
Name HF
a)
hydrofluoric acid
b)
Hypofluoric acid
c)
hydrogen fluorine acid
d)
fluoric acid
56.
HNO2
a)
hydronitrogen
b)
hydrogen nitrogen oxygen
c)
nitrous acid
d)
nitric acid
57.
Name the acid: HC2H3O2
a)
Acetic Acid
b)
Acetous Acid
c)
Hydrogen Acetate
d)
Hydrogen Dicarbon Trihydrogen Dioxygen
58.
bromic acid
a)
HBr
b)
H2Br
c)
HBrO3
d)
HBrO4
59.
Hydroiodic acid
a)
H2I2
b)
H1I1
c)
HI
60.
How many electrons should Oxygen have around its Lewis dot model?
a)
5
b)
6
c)
7
d)
8
61.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
62.
Which of the following is the correct Lewis structure for the compound PBr3?
a)
structure A
b)
structure B
c)
structure C
d)
structure D
63.
This is a correct dot diagram for fluorine (F)
a)
true
b)
false
64.
If electrons are shared unequally then the bond is....
a)
Non-polar covalent
b)
Ionic
c)
Non-polar ionic
d)
Polar covalent
65.
When writing Lewis Structures, only __________ electrons are used.
a)
Inner shell
b)
Core 
c)
Valence
d)
Stable
66.
A molecule of methane has what shape?
a)
Tetrahedral
b)
Triangular
c)
Pyramidal
d)
Octahedral
67.
A molecule of water has what shape?
a)
Linear
b)
Tetrahedral
c)
Bent
d)
Triangular
68.
Atoms of H only form _________ bonds.
a)
Double
b)
Single
c)
Multiple
d)
Triple
69.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
70.
What is the correct structure for BF3?
a)
Option A.
b)
Option B. 
c)
Option C.
d)
Option D.
71.
How many valence electrons are available for bonding in the sulfate ion (SO4-2)?
a)
30 electrons
b)
32 electrons
c)
28 electrons
d)
impossible to tell
72.
Which substance contains bonds that involve a transfer of electrons from one atom to another?
a)
CO2
b)
NH3
c)

NaF

d)
Cl2
73.
Predict the bond that will form between Se and Cl.
a)
Ionic
b)
Covalent
c)
Metallic
d)
Nonpolar
74.
Which of the following is a property of an ionic compound?
a)
high melting point
b)
soft
c)
malleable
d)
liquid at room temperature
75.

Why do ionic compounds have high melting and boiling points?

a)

Their ions are free to move.

b)

Their ions are held in fixed positions.

c)

They have many strong bonds.

d)

They have many weak bonds.

76.
Molten compound does NOT conduct electricity.
a)
ionic compound
b)
covalent compound
77.
Have a low m.p. (< 200°C)
a)
ionic compounds
b)
covalent compounds
78.
When dissolved in water, the solution is a good conductor of electricity.
a)
ionic compounds
b)
covalent compounds
79.

Is the following compound ionic or covalent?

A material that LOSES and GAINS electrons

a)

Ionic

b)

Covalent

80.

Which type of solid has mobile electrons in the crystal (sea of electrons)?

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent Network

81.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

82.
The mass of one mole of substance is called...
a)
molecular mass
b)
mole constant
c)
molar mass
d)
atomic weight
83.
What is the molar mass of sodium?
a)
11
b)
23
c)
45.98
d)
3
84.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
85.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
86.
What is the MOLECULAR geometry of the molecule?
a)
Linear
b)
Bent
c)
Trigonal Planar
d)
Seesaw
87.
What is the best explanation of VSEPR theory?
a)
It explains the shapes that electrons make around atoms when they repel
b)
It explains how many electrons fit into an element's valent shell
c)
It explains why electrons pair up
d)
It explains why electrons repel each other
88.

48.86 g of cobalt is equal to how many moles of cobalt?

a)

2879 moles

b)

8.291 moles

c)

.8291 moles

d)

.829 moles

89.

What is the mass of 4.98 x 1024 atoms of Zn?

a)

541 g

b)

8.27 g

c)

.122 g

d)

4.59 x 1046 g

90.

Convert 86.235 g of diphosphorus pentaoxide to moles.

a)

12240 moles

b)

1.8747 moles

c)

.608 moles

d)

.60755 moles

91.
Which conversion factor should be used for the following question " How many molecules are there in 4.00 moles of glucose, C6H12O6? 
a)
1 mole = 78.12 g
b)
1 mole = 22.4 L 
c)
1 mol = 6.02x 1023 particles 
d)
more than one
92.
The number 6.02 x 1023, which is the number of particles found in a mole. 
a)
molar mass
b)
mole
c)
Avogadro's number
d)
hydrate
93.
How many molecules are in 9.44 moles of AlCl3?
a)
5.68 molec AlCl3
b)
5.68x1024 molec AlCl3
c)
0.705 molec AlCl3
d)
1.25x1023 molec AlCl3
94.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of carbon?

a)

29%

b)

43%

c)

57%

d)

73%

95.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of magnesium?

a)

13%

b)

43%

c)

63%

d)

87%

96.
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
97.
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
98.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
99.

What equipment allows you to measure liquid's volume and measures in milliliters?

a)

test tube

b)

beaker

c)

flask

d)

graduated cylinder

100.

Which equipment heats objects with an open flame?

a)

hot plate

b)

thermometer

c)

bunsen burner

d)

beaker

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