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Honors: Final Exam

Total questions: 100

Worksheet time: 2hrs 7mins

Name
Class
Date
1.

What are the products of this reaction?
Cu(+2) + AgNO3--> 

a)
Cu(NO3)2+Ag
b)
CuNO3 + Ag
c)
CuAg+NO3
d)
Cu+ AgNO3
2.
Write a Balanced Equation for this reaction:
C2H4 + 2 O2 -->
a)
C2O2 + H4
b)
CO2 + HOH
c)
CO + H
d)
2 CO2 + 2H2O
3.
Which of the following equations represents the balanced synthesis reaction of iron (III) and oxygen?
a)
Fe + 3 O2 → Fe2O3
b)
3 Fe + 3 O2 → 2 Fe2O3
c)
2 Fe + O2 → Fe2O3
d)
4 Fe + 3 O2 → 2 Fe2O3
4.
If an element is diatomic it should have a subscript of___
a)
2, always
b)
2, only when it is by itself
c)
it shouldn't have a subscript, it should have a coefficent
5.
What kind of reaction is this:
2H2O2 →2 H2O + O2
a)
Synthesis
b)
Decomposition
c)
Single Replacement 
d)
Combustion
6.
Which of the following are PRODUCTS?
H2O + CO2 → HCO + HO
a)
H2O and CO2
b)
HCO and HO
c)
H2O ONLY
d)
HCO ONLY
7.

Predict the products, before balancing.

Co2(SO4)3 + NaOH -->

a)

CoOH + NaSO4

b)

CoNa + OH(SO4)3

c)

Co2OH + Na(SO4)3

d)

Co(OH)3 + Na2SO4

e)

no reaction

8.

Predict the product of the following synthesis reaction.

Ca + N2 -->

a)

CaN2

b)

CaN

c)

Ca3N2

d)

CaNNot

9.
Write a balanced equation for this Double Displacement reaction
NaOH + Fe(NO3)3 -->
a)
NaFe + OH(NO3)3
b)
2NaNO3 + 3Fe(OH)3
c)
NaNO3 + FeOH
d)
3NaNO3 + Fe(OH)3
10.

KI + Pb(NO₃)₂ →

a)

KNO + PbI

b)

KNO₃ + PbI₂

11.

What is the left part of a chemical equation called?

2H2 + O2 ---> 2H2O

a)

Reactants

b)

Yields

c)

Products

d)

Chemical equation

12.

Balance the following equation--> What coefficient would need to be put in front of HCl to balance this equation. CH4 + 4 Cl2 → CCl4 + _____ HCl

a)

2

b)

3

c)

4

d)

5

13.
What is the little number after an element in a chemical equation called.
Example: H2
a)
Coefficient 
b)
Subscript
c)
Atom
d)
Equation
14.
Iron reacts with sulfur to produce iron(II) sulfide powder.
a)
2Fe(s) + S(s) → Fe2S(s)
b)
Fe(s) + S(s) → FeS(s)
c)
Fe(s) + S(g) → FeS(s)
d)
4Fe(s) + S2(g) → 2Fe2S
15.

What state of matter is this substance?

a)

solid

b)

liquid

c)

gas

d)

aqueous

16.
How many significant figures: 216 m
a)
1
b)
2
c)
3
d)
0
17.
How many significant figures: 2016 m
a)
1
b)
2
c)
3
d)
4
18.
How many significant figures: 153.0 mL
a)
1
b)
2
c)
3
d)
4
19.
How many significant figures: 0.012 km
a)
1
b)
2
c)
3
d)
4
20.
How many significant figures: 1000 mL
a)
1
b)
2
c)
3
d)
4
21.
What two types of measurements make up DENSITY? 
a)
Mass and Volume
b)
Temperature and Mass
c)
Grams and Centimeters
d)
Volume and Weight
22.
What units are used to measure mass?
a)
g
b)
cm3
c)
g/cm3
d)
cm3/g
23.
Jack has a rock. The rock has a mass of 14g and a volume of 2cm3. What is the density of the rock?
a)
7 mL
b)
7 g/cm3
c)
28 g/cm3
d)
1/7 g/cm3
24.
Why do some substances float on water?
a)
they are warmer than water
b)
they are cooler than water
c)
they are more dense than water
d)
they are less dense than water
25.
What is the volume of the fish?
a)

18.0 ml

b)

6.0 ml

c)

38.0 ml

26.
A diamond has a mass of 1.2 g.  If diamond has a density of 3.51 g/mL, what is the volume of the diamond.
a)
0.34 mL
b)
2.9 g/mL
c)
2.3 mL
d)
4.2 mL
27.

The positively charged particle in an atom.

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

28.

The smallest part of any element. Made up of protons, neutrons and electrons.

a)

Atom

b)

AMU

c)

Ion

d)

Isotope

29.

Identifies the number of protons in an atoms nucleus.

a)

Electron Cloud

b)

Atomic Theory

c)

Atomic Number

d)

Mass Number

30.

The negatively charged particles in an atom

a)

Proton

b)

Electron

c)

Neutron

d)

Electron Cloud

31.

The region inside an atom where electrons are likely to be found

a)

Proton

b)

Atom

c)

Electron Cloud

d)

Neutron

32.

A charged atom

a)

Ion

b)

Isotope

c)

Proton

d)

Electron

33.

Atoms of the same element that have different numbers of neutrons

a)

Ion

b)

Isotope

c)

Proton

d)

Electron

34.

The total number of protons and neutrons in the nucleus of an atom

a)

Atomic Number

b)

Mass Number

c)

Atomic Theory

d)

Electron Cloud

35.

The particles in the nucleus of an atom that do not have a charge (neutral)

a)

Proton

b)

Electron

c)

Neutron

d)

Ion

36.

The small, dense, positively charged center of an atom

a)

Neutron

b)

Proton

c)

Nucleus

d)

Electron

37.

What is a positive ion called?

a)

anion

b)

cation

c)

isotope

d)

covalent

38.

What is a negative ion called?

a)

anion

b)

cation

c)

covalent

d)

isotope

39.

If an atom loses electrons, the charge will be positive.

a)

true

b)

false

40.

A Bromine ion gains 1 electron, which of the following is the correct symbol for a Bromine ion?

a)

Br-1

b)

Br+1

c)

Br+7

d)

Br-7

41.
What is the charge of an atom that has lost one electron?
a)
-1
b)
-2
c)
+1
d)
+2
42.

An atom with 2 protons, 3 neutrons, and 4 electrons has a charge of ____.

a)

+2

b)

-2

c)

+3

d)

0

43.

If an element has 3 valence electrons, what charge will likely form on its ion ?

a)

+3

b)

+5

c)

-3

d)

-5

44.
Ions are: 
a)
atoms with a positive or negative charge
b)
atoms with no charge
c)
atoms with ONLY a positive charge
d)
atoms with ONLY a negative charge
45.

S has 6 valence electron. It will have a charge of _______

a)

-2

b)

-1

c)

+1

d)

+2

46.

Isotopes of an element have a different number of...

a)

Protons

b)

Neutrons

c)

Electrons

d)

Mass

47.

Potassium-39 has how many neutrons?

a)

19

b)

18

c)

20

d)

21

48.

76 protons and 114 neutrons

a)

Osmium-114

b)

Osmium-76

c)

Osmium-190

d)

Osmium-190.23

49.

How do you calculate mass number?

a)

Mass x percent

b)

Protons + Electrons

c)

Protons + Neutrons

d)

Neutrons + Protons + Electrons

50.
Which answer choice describes the subatomic particles and their respective charges?
a)
p-    e+    n
b)
p+    e     n-
c)
p+    e-    n
d)
p-     e+    n
51.
If an atom gains an electron it is a(n)
a)
Positive ion
b)
Negative ion
c)
Isotope
d)
Neutral Atom
52.
Carbon has an atomic number of 6 and an atomic mass of 12. Which elements are considered isotopes of carbon?
a)
Carbon-12
b)
Carbon-13
c)
Carbon-14
d)
Both Carbon-13 and Carbon-14
53.
What is the name of the pictured isotope?
a)
Copper-29
b)
Copper-63
c)
Copper-34
d)
CopperWopperHopperBopper
54.
An atom is electrically neutral when
a)
protons and neutrons are the same
b)
protons and electrons are the same
c)
neutrons and electrons are the same
d)
neutrons balance the protons and electrons
55.
If X is the symbol for an element, which of the following two symbols represent    isotopes of the same element?     I. 7735X  II. 7733X  III. 8137X  IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
56.
How many neutrons does the isotope below have?     89 36Kr
a)
53
b)
36
c)
89
d)
125
57.

Which scientist first theorized atoms cannot be created destroyed or divided?

a)

Niels Bohr

b)

Richard Feynman

c)

Democritus

d)

Ernest Rutherford

58.

What experiment and scientist discovered the nucleus of an atom?

a)

Cathode Ray Tube - J.J. Thomson

b)

Gold Foil - Rutherford

59.

Who discovered the Neutron?

a)

James Chadwick

b)

Niels Bohr

c)

John Dalton

d)

Ernest Rutherford

60.

Who proposed electrons are found in specific orbits around the nucleus?

a)

Democritus

b)

John Dalton

c)

James Chadwick

d)

NielsBohr

61.

How are elements ordered on the Periodic Table?

a)

Alphabetical Order

b)

By their atomic mass.

c)

By their color.

d)

By their atomic number.

62.

Rows on the period table are called _____ while columns are called _____.

a)

groups, families

b)

periods, groups

c)

groups, periods

d)

families, groups

63.

Atoms with similar properties are most likely located...

a)

in the same period.

b)

in different periods.

c)

in the same group.

d)

to the right and left of each other.

64.

Which of the following determines the identity of an element?

a)

number of protons

b)

number of neutrons

c)

atomic mass

d)

number of shells

65.

What is the atomic number of the atom pictured?

a)

9

b)

8

c)

18

d)

19

66.

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 protons

c)

12 electrons

d)

24 protons and neutrons

67.

What is the atomic number of this atom?

a)

1

b)

3

c)

4

d)

7

68.

Which element is this?

a)

Nickel

b)

Neon

c)

Sodium

d)

Nitrogen

69.

How many valence electrons?

a)

2

b)

3

c)

4

d)

5

70.

What is a valence electron?

a)

Electrons in the first energy shell

b)

Electrons in the second energy shell

c)

Electrons in the outer shell

d)

Total number of electrons

71.

What element is represented in this Bohr Model?

a)

Carbon

b)

Hydrogen

c)

Aluminum

d)

Lithium

72.
Element or compound?
H2O
a)
element
b)
compound
73.
Which of the following is a compound?
a)
Co
b)
O2
c)
C
d)
CO2
74.
The red numbers in the image below represent ________
a)
subscripts
b)
coefficients
c)
I don't know, and don't want to try
d)
None of the answers are correct
75.
The blue numbers in the image below represent ________
a)
I don't know, and don't want to try
b)
coefficients
c)
subscripts
d)
none of the answers are correct
76.
The blue atoms are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
77.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
78.
The substances at the beginning of a chemical equation are called the ____
a)
product
b)
yield
c)
chemical symbol
d)
reactants
79.
All of the following are chemical changes except
a)
iron rusting
b)
water evaporating
c)
wood burning
d)
food rotting
80.
What is the correct formula for the compound, lithium oxide?
a)
LiO
b)
Li2O
c)
LiO2
d)
Li2O2
81.

Which of the following is NOT an ionic compound?

a)

CaO

b)

NaOH

c)

BaCl2

d)

Br2

82.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
83.
When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..
a)
atomic number
b)
mass number
c)
charge
d)
ionization energy
84.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
85.

What type of elements form covalent bonds?

a)

Metals

b)

Non Metals

c)

Metalloids

d)

Nobel Gas

86.

When a covalent bond forms _______________ are shared.

a)

protons

b)

nutrons

c)

valence electrons

d)

quarks

87.
a)

Element

b)

Compound

c)

Mixture

88.
a)

Element

b)

Compound

c)

Mixture

89.

Choose the correct formula for this compound:


Dinitrogen Pentasulfide

a)

N5S2

b)

N2S5

c)

Ni2Se5

d)

NS

90.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
91.
N2, Cl2, and O2 are all 
a)
diatomic molecules.
b)
ionic bonds.
c)
of equal mass.
d)
solids.
92.
Bonds between two nonmetal atoms are 
a)
covalent.
b)
ionic.
c)
incomplete.
d)
complete.
93.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
94.
What is the correct name for C4H6?
a)
Carbon Hexahydride
b)
Pentacarbon Pentahydride
c)
Hexacarbon Tetrahydride
d)
Tetracarbon Hexahydride
95.
What is the molar mass of AuCl3?
a)
96 g
b)
130 g
c)
232.5 g
d)
303.3 g
96.
2Na + 2H2O → 2NaOH+ H2
How many grams of hydrogen are produced if 120 g of Na are available?
a)
5.2 g
b)
2.6 g
c)
690 g
d)
45 g
97.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
98.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of Mg to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
99.

Solve the nuclear decay reaction:

a)

b)

c)

d)

100.

Solve the nuclear decay reaction:

a)

b)

c)

d)

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