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Semester Review - Chemistry

Total questions: 125

Worksheet time: 10hrs 25mins

Name
Class
Date
1.
a)
Periods
b)
Groups
2.
a)
Periods
b)
Groups
3.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
4.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
5.
a)
Same group
b)
Same period
6.
a)
Group 1
b)
Group 17
c)
Group 2
d)
Group 18
7.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
8.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
9.
a)
Metals
b)
Nonmetals
c)
Metalloids
10.
a)
Metals
b)
Nonmetals
c)
Metalloids
11.
a)
Metals
b)
Nonmetals
c)
Metalloids
12.
a)
Metals
b)
Nonmetals
c)
Metalloids
13.
a)
Metals
b)
Nonmetals
c)
Metalloids
14.
a)
Metals
b)
Nonmetals
c)
Metalloids
15.
a)
Metals
b)
Nonmetals
c)
Metalloids
16.

Who invented the Periodic Table?

a)

Mendeleev

b)

Bohr

c)

Lewis

d)

Democritus

17.

What happens to the number of shells as you move down a group?

a)

They decrease by 1

b)

They increase by 1

c)

Nothing

18.

The first energy shell can hold ______ electrons.

a)

2

b)

8

c)

18

19.

What do all elements in the same period have?

a)

same number of shells

b)

same number of electrons

c)

belong in the same family

20.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
21.
Name group 1A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
noble gases
d)
halogens
22.
Name group 2A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
23.
Name groups 3B - 12B on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
24.
Name group 18 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
noble gases
25.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
26.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
27.
Name group 17 on the periodic table.
a)
transition metals
b)
metalloids
c)
halogens
d)
alkali metals
28.

3 subatomic particles that makeup an atom.

a)

Positive, negative, neutral

b)

Positron, Neutral, Electron

c)

Proton. Neutron, Electron

29.

This subatomic particle has a positive charge.

a)

Proton

b)

Neutron

c)

Electron

30.

The subatomic particle holds the atom together.

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

31.

The subatomic particles found in the nucleus.

a)

Electron, Neutron

b)

Proton, Neutron

c)

Electron, Proton

d)

Proton, Neutron, Electron

32.

The subatomic particle that identifies the element.

a)

Proton

b)

Positron

c)

Neutron

d)

Electron

33.

The subatomic particle that determines reactivity.

a)

Electron

b)

Proton

c)

Shell

d)

Neutron

34.

A neutron has a _____ charge.

a)

Positive

b)

Negative

c)

Neutral

d)

1/2 charge

35.

A electron has a ______ charge.

a)

No charge

b)

Positive

c)

Neutral

d)

Negative

36.

The atomic number tells you the number of

a)

Neutrons

b)

Protons

c)

Neutrons plus Protons

37.

The atom model that we will use in this class is called ________ model.

a)

Rutherford

b)

Thompson

c)

Bohr

d)

Karen

38.

An isotope has different number of ______.

a)

Neutrons

b)

Protons

c)

Electrons

d)

Nucleus

39.

The building block of everything.

a)

Atoms

b)

Elements

c)

Positive

d)

Biology

40.

A piece of paper contains_______ of atoms.

a)

Hundreds

b)

Tens

c)

Millions

41.
a)
Bunsen burner
b)
Ring stand
c)
Graduated cylinder
d)
Test tube holder
42.
a)
beaker
b)
cup-with-lines
c)
wash bottle
d)
graduated cylinder
43.
a)
Erlenmeyer flask
b)
beaker
c)
wash bottle
d)
watch glass
44.
a)
graduated cylinder
b)
beaker
c)
Erlenmyer flask
d)
bunsen burner
45.

The following piece of glassware is used to ...

a)

measure a precise volume of a liquid

b)

prepare solutions to an accurate volume

c)

hold and mix chemicals without spilling

46.

Which piece of glassware would you use to measure a precise volume of a liquid?

a)
b)
c)
d)
47.

Which of these would be best to hold large amounts of liquid?

a)

Beaker

b)

Boiling tube

c)

Conical flask

d)

Test tube

48.

Sandals are permitted during laboratory experiments.

a)

True

b)

False

49.

Using chipped glassware is permitted during the labs.

a)

True

b)

False

50.

If you do not understand a direction or part of a lab procedure, you should

a)

figure it out as you do the lab

b)

try several methods until something works

c)

ask the instructor before proceeding

d)

skip it and go on to the next part

51.

Ionic bonding occurs between a _________ and a __________.

a)

metal, metal

b)

metal, nonmetal

c)

nonmetal, nonmetal

d)

metallic, sea of electrons

52.

In an ionic bonds electrons are ____________.

a)

transferred

b)

shared

c)

transferred and shared

d)

arrange like a sea of electrons

53.

A covalent bond occurs between a __________ and a __________.

a)

nonmetal, nonmetal

b)

metal. metal

c)

metal, nonmetal

d)

sea of electrons, metallic

54.

In a covalent bond electrons are _____________.

a)

transferred

b)

shared

c)

depends on ionization energy

d)

connect through a sea of electrons

55.

Valence electrons are the electrons in ______________.

a)

the inner shell

b)

the outermost shell

c)

includes all electrons

d)

depends on atom

56.

Valence electrons determine___________.

a)

the reactivity of the atom

b)

the identity of the atom/element

c)

the atomic number of the atom

d)

the charge of the atom in a neutral sphere

57.

In an ionic bond metals will have a _______________ charge.

a)

positive

b)

negative

c)

neutral

d)

protonic

58.

According to the octet rule most elements need _______ valence electrons.

a)

2

b)

8

c)

6

d)

18

59.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

60.
 Which of the following is the correct formula for these two ions:
Al+3 +  S-2
a)
AlS3
b)
Al2S3
c)
Al3S2
d)
Al3S
61.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
62.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
63.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
64.
How many valence electrons does nitrogen have?
a)
3
b)

2

c)
5
d)
1
65.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
66.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
67.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
68.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
69.

dinitrogen pentoxide

a)

N2O5

b)

NO5

c)

N5O2

d)

N2O6

70.

What is an ion?

a)

An atom that gains or loses electrons

b)

Pieces of the atom that are atoms of the same element

c)

An atom that is the sum of the number of protons and neutrons in an element.

71.

The isotope is the change in what number of the nucleus?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Protons and Neutrons

72.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 
73.

Water melting, freezing, or evaporating is an example of a

a)

physical change

b)

chemical change

c)

physical property

d)

chemical propery

74.

An -ate or -ite at the end of a compound name usually indicates that the compound contains _____________.

a)

fewer neutrons than protons

b)

a polyatomic ion

c)

electons

d)

a neutral atom

75.

When polyatomic ions bond with other ions the net charge of the ionic compound will be

a)

zero

b)

positive

c)

negative

d)

depends on the bond

76.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
77.

There are 4 different types of subshells(orbitals) s,p,d,f

a)

true

b)

false

78.

What is the maximum number of electrons that an S orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

79.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
80.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

81.
How many electron can be found in a p orbital?
a)
2
b)
3
c)
4
d)
6
82.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
83.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
84.
Which periodic table family could have electrons filling orbitals in the s-block?
a)
Alkaine Earth 
b)
Halogens
c)
Noble Gases
d)
Transition Metals
85.

How many electrons can the f sublevel hold?

a)

14

b)

10

c)

8

d)

2

86.
Combining substances to form a new substance
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
87.
Breaking down a substance into simpler substances
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
88.
What type of reaction is the equation C + O2 → CO2?
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
89.
What type of reaction is the equation 2NaCl →2Na +Cl2?
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
90.
Cu + 2Ag(NO3) → 2Ag + Cu(NO3)
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
91.
Ca3(PO4)2 + 3 H2SO4 + 3 CaSO4 + 2 H3(PO4)
a)
Synthesis Reaction
b)
Decomposition Reaction
c)
Single Displacement Reaction
d)
Double Displacement Reaction
92.
Which generalized equation represents a decomposition reaction?
a)
A + BC → AC+ B
b)
A + B → AB
c)
AB → A + B
93.
Which generalized equation represents a single displacement reaction?
a)
A + BC → AC+ B
b)
A + B → AB
c)
AB → A + B
94.
CxHy +O2 --> H2O + CO2
a)
Decomposition
b)
Double replacement
c)
Combustion
d)
Single Replacement
95.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
96.

3 Pb + 2 H3PO4 ----> 3 H2 + 1 Pb3(PO4)2

a)

Synthesis (or combination)

b)

Decomposition

c)

Single replacement

d)

Double replacement

97.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
98.
How many Oxygen are in H2O?
a)
1
b)
2
c)
0
d)
4
99.
How many Magnesium are in 10MgCl2?
a)
10
b)
5
c)
20
100.
2H2 + O2 ----> 2H2O What is the product?
a)
------>
b)
2H2O
c)
2H2+ O2
101.
2H2 + O2 --------> 2H2O What  are the reactants?
a)
----->
b)
2H2O
c)
2H2 +O2
102.
How many O's are in Al₂(SO₄)₃
a)
4
b)
12
c)
7
d)
24
103.
Number of H in 3(NH₄)₂CrO₄
a)
4
b)
2
c)
8
d)
24
104.
How many atoms are there TOTAL in:
H2SO4
a)
6
b)
5
c)
7
d)
3
105.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
106.
A subscript is the small number below a(n) ________ that tells the number of _______ of that element.
a)
element symbol; atoms
b)
atom; element symbol
c)
subscript; protons
d)
compound; elements
107.

What is the charge/oxidation number in group 1?

a)

+1

b)

-1

c)

varies due to valence electrons

d)

depends on element

108.

What is the oxidation number/charge for transition metals?

a)

varies

b)

3-12

c)

+3

109.

Why is group 18 unreactive?

a)

the outer shell is full

b)

it has 7 valence electrons

c)

the inner shell contains 2 electrons

d)

they are gases

110.

The largest atom on the periodic table is _____

a)

F

b)

Fr

c)

Og

d)

H

111.

The most electronegative atom on the periodic table______

a)

Fr

b)

F

c)

He

d)

Og

112.

Ionization energy is the energy needed to...

a)

remove an electron

b)

remove a proton

c)

gain an electron

d)

gain a proton

113.

Ionization energy down a group will...

a)

increase because you are not adding energy levels

b)

decrease because you are adding energy levels

c)

stays the same

114.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
115.
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
116.

A chemical change occurs when a piece of wood

a)

splits

b)

cut

c)

chopped

d)

burns

117.

Which of the following is a heterogeneous mixture?

a)

milk

b)

gatorade

c)

hot tea

d)

sand

118.

How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain?

a)

50, 50, 125

b)

125, 125, 125

c)

50, 50, 75

119.

An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are ____.

a)

76

b)

undetermined

c)

38 each

d)

152

120.

From left to right across a period of the periodic table, atomic radius tends to -

a)

increase

b)

decrease

c)

stay the same

d)

depends on acetate

121.

Which element do all acids begin with?

a)

H

b)

Cl

c)

Na

d)

Fr

122.

How many atoms of oxygen are in the following?

Ca3(PO4)2

a)

2

b)

4

c)

6

d)

8

123.

The law of conservation of mass states that_______.

a)

matter can be created into a new substance from random stuff.

b)

matter can not be created nor destroyed only rearranged.

c)

matter will become water that evaporates into the atmosphere.

d)

matter smells like acetate.

124.

Who is buried in Grant's tomb?

a)

Grant

b)

Reid

c)

Lincoln

125.

What school do you take Chemistry?

a)

Tascosa

b)

Harvard

c)

Yale

d)

Princeton

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