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final review

Total questions: 111

Worksheet time: 2hrs 55mins

Name
Class
Date
1.
The right of the arrow is called?
a)
Reactant 
b)
Product
c)
Yields
2.
H
H2
NaCl
Cl
O2
List the correct answers in order.
a)
molecule, compound, molecule, element,molecule
b)
element, molecule, compound, compound, molecule
c)
element, molecule, compound, element, molecule
d)
Compound, element, ,molecule, vector, roger
3.
List the coeffecieints in order.
a)
4,3,2
b)
2,2,3
c)
4,2,3
d)
1,2,3
4.
Type of reaction?
a)
Decomposition
b)
Single replacement
c)
Double replacement
d)
Combustion
5.
Type of reaction?
a)
Sythesis
b)
Decomposition
c)
Combustion
d)
Single Replacement
6.
Type of reaction?
a)
Sythesis
b)
Decomposition
c)
Single Replacement
d)
Double replacement
7.
Type of reaction?
a)
Sythesis
b)
Decomposition
c)
Single replacement
d)
Double replacement
8.

The molar volume of a gas at STP occupies _____________.

a)

22.4 L

b)

0˚C

c)

1 kiloPascal

d)

12 grams

9.

In a double replacement, ____________________

a)

The reactants are usually a metal and a nonmetal

b)

One of the reactants is often water

c)

The reactants are generally 2 ionic compounds in aqueous solutions

d)

Energy in the form of light or heat is often produced

10.

If 2.00 L of a gas in a container at room temperature exerts a pressure of 4.00 atm. If the pressure doubles and the temperature remains the same, the volume would become ________.

a)

16.0 L

b)

2.00 L

c)

4.00 L

d)

1.00 L

11.

If 7.00 grams of nitrogen gas are contained in a 5.00 L flask at 4.62 kPa. What is the temperature of the gas?

a)

11.1 K

b)

1.00 K

c)

4.12 K

d)

9.07 K

12.

Chemical equations must be balanced to satisfy ____.

a)

The law of definite proportions

b)

The law of multiple proportions

c)

The law of conservation of mass

d)

Avogadro's principle

13.

What is the name of H2SO4?

a)

hyposulfuric acid

b)

hydrosulfuric acid

c)

sulfuric acid

d)

sulfurous acid

14.

Which of the following shows both the correct formula and correct name of an acid?

a)

HClO2, chloric acid

b)

HNO2, hydronitrous acid

c)

H3PO4, phosphoric acid

d)

HI, iodic acid

15.

When an equation is used to calculate the amount of product that could form during a reaction, then the value obtained is called the ____.

a)

Actual yield

b)

Percent yield

c)

Minimum yield

d)

Theoretical yield

16.

The equation 2C3H7OH + 9O2 → 6CO2 + 8H2O is an example of which type of reaction?

a)

Combustion reaction

b)

Single replacement reaction

c)

Double replacement reaction

d)

Decomposition reaction

17.

A process that absorbs heat is a(n) _________.

a)

Exothermic process

b)

Polythermic process

c)

Endothermic process

d)

Ectothermic process

18.

In which state of matter will the atoms of an element be tightly packed?

a)

solids

b)

liquid

c)

gas

d)

plasma

19.

Which of the following is an example of a mixture?

a)

aluminum

b)

carbon dioxide

c)

water

d)

fruit punch

20.

Which of the following is an example of a compound?

a)

salt (sodium chloride)

b)

fruit punch

c)

aluminum

d)

salad dressing

21.

Iron filings are spilled into a bag of sand.  What is the best way to separate this mixture?

a)

Use a magnet to pick up the sand

b)

Use a magnet to pick up the iron filings

c)

Sift through the sand for all the iron

d)

Use filtration to remove the iron from the sand

22.

If an element has a full outer shell and does not tend to react with other elements, what family is it a part of?

a)

alkali metals

b)

transition metals

c)

halogens

d)

noble gases

23.

Which of the following is NOT an indicator of a chemical change.

a)

iron rusting

b)

baking soda reacts with vinegar to form a gas

c)

water placed on the stove begins to boil

d)

paper burns in the presence of oxygen to produce light and heat

24.

Name the compound Fe(NO3)2.

a)

Iron (II) Nitrate

b)

Iron (II) Nitrite

c)

Iron (III) Nitrate

d)

Iron (III) nitride

25.

What is the formula for the compound formed by calcium ions and chloride ions?

a)

CaCl

b)

Ca2Cl

c)

CaCl3

d)

CaCl2

26.

The energy required to remove an electron from an atom is the atom's

a)

electron affinity

b)

electron energy

c)

electronegativity

d)

ionization energy

27.

The branch of chemistry which studies substances containing carbon is

a)

organic chemistry.

b)

inorganic chemistry.

c)

physical chemistry.

d)

analytical chemistry.

28.

What atom matches this electron configuration?

1s2 2s2 2p6 3s2

a)

Magnesium

b)

Neon

c)

Aluminum

d)

Potassium

29.

Which is the electron configuration for an oxygen atom?

a)

1s22s22p63s23p64s2

b)

1s22s22p6

c)

1s22s22p4

d)

1s22s22p63s23p6

30.

How many valence electrons are represented here?

a)

7

b)

2

c)

5

d)

8

31.

What is this element?

1s22s22p63s23p6

4s23d104p6

a)

Argon

b)

Bromide

c)

Selenium

d)

Krypton

32.

Which is the correct Lewis structure for Nitrogen?

a)
b)
c)
d)
33.

A _______ is a neutral group of atoms that are held together by covalent bonds.

a)

Molecule

b)

Compound

c)

Substance

34.
Which state of matter is represented here?
a)
Solid
b)
Liquid
c)
Gas
35.
What are the units of molarity?
a)
mol/L
b)
g/L
c)
mol/g
d)
g/mol
36.
1.  The number of significant figures in the measurement 170.040 km is ___.
a)
Three
b)
Four
c)
Five
d)
Six
37.
2.   Which of these recorded observations is qualitative, rather than quantitative?
a)
a.  A chemical reaction is complete in 2.3 s.
b)
a.  The solid has a mass of 23.4 g.
c)
The compound melts at 87.5°C.
d)
Iron is denser than aluminum.
38.
3.  A sample of bismuth has a mass of 343g and a volume of 35.0cm3. What is the density of bismuth?
a)
a.  0.102 g/cm3 
b)
b. 9.80 g/cm3 
c)
c. 378 g/cm3 
d)
d. 1.20 x 104 g/cm3
39.
4.  How many meters are there in 1,865 cm?
a)
0.1865 m
b)
1.865 m
c)
18.65 m
d)
186.5 m
40.
6.  Expressed in scientific notation, 0.0930 m is ___.
a)
      93 x 103 m.
b)
       9.3 x 10-3m.
c)
     9.30 x 10-2 m.
d)
     9.30 x 104 m.
41.
7.  Convert the following measurement:  5.4 L to mL
a)
54. mL
b)
5400. mL
c)
540. mL
d)
54000. mL
42.
11.  What electron configuration rule states: An electron occupies the lowest energy orbital that can receive it. 
a)
Pauli Exclusion Principle
b)
Hund's Rule
c)
Aufbau Principle
43.
12.  Which element does the following configuration represent?  1s2,2s2,2p6,3s2,3p5
a)
   Phosphorus
b)
     Chlorine
c)
   Silicon
d)
    Argon
44.
14.  What is the correct formula for copper(I) cyanide?
a)
      CuCy
b)
      CuCy2
c)
    CuCN
d)
  Cu2CN
45.
15.  What is the correct formula for the compound made of magnesium and nitrogen?
a)
   Mg2N3
b)
      Mg3N2
c)
    MgN2
d)
      MgN
46.
16.  Which equation below violates the law of conservation of mass?
a)
     2H2 + O2 --> 2 H2O
b)
   KCl + Br --> KBr + Cl2 
c)
a.  2 Fe2O3 + 3C --> 4Fe + 3CO2
d)
a.  Na 2 CO3 + 2HCl  --> 2NaCl + H2 O + CO2  
47.

For this reaction, how many liters of CO2 will be produced from 12 L of O2 at STP?


2 C4H10 + 13 O2 --> 8 CO2 + 10 H2O

a)

12 L

b)

8 L

c)

7.38 L

d)

2.62 L

48.

What addition to the end of a compound in a reaction indicates that it is a solid?

a)

(aq)

b)

(g)

c)

(s)

d)

(l)

49.

How do you convert from grams to moles of a substance?

a)

Multiply by the molar mass

b)

Divide by the molar mass

c)

Add the molar mass

d)

Subtract the molar mass

50.

What is the volume occupied by 2.3 moles of helium at 1.2 atmospheres and 298 K? (R = 0.082)


PV = nRT

a)

12.7 L

b)

67.4 L

c)

46.8 L

51.

What product forms in this reaction?


HNO3 + LiOH --> __________ + H2O

a)

LiNO3

b)

LiH2O

c)

NO2

d)

LiO3

52.

Calculate the pH of a 0.065 M solution of HBr.

a)

-1.18

b)

1.18

c)

3.63

d)

-3.63

53.

Which of the following compounds is insoluble in water?

a)

KNO3

b)

Li2SO4

c)

AlPO4

d)

MgCl2

54.

A solution has a molarity of 4.5 M. It needs to be diluted to form 1.75 L of a 0.5 M solution. How much of the 4.5 M solution is needed? (M1V1 = M2V2)

a)

3.93 L

b)

1.29 L

c)

0.19 L

d)

1.9 L

55.

What is the volume of this liquid in the graduated cylinder?

a)

66 mL

b)

67 mL

c)

66.0 mL

d)

66.5 mL

56.

What is the density of an object having a mass of 6.5 g and a volume of 30.0 cm3?

a)

0.22 g/cm3

b)

4.6 g/cm3

c)

195 g/cm3

d)

200 g/cm3

57.

What is the SI unit for mass?

a)

gram

b)

kilogram

c)

pound

d)

ounce

58.

During an experiment, the variable that responds to the manipulated variable is the

a)

independent variable

b)

dependent variable

c)

control

59.

How many sig figs are in the number 1.000 g?

a)

0

b)

1

c)

2

d)

4

60.

How many sig figs are in the number 0.00830 km?

a)

2

b)

3

c)

4

d)

6

61.

Manuel measures out 36 grams of sodium on a scale. How many atoms of sodium are in his sample?

a)

9.43 x 1023 atoms

b)

5.49 x 1023 atoms

c)

7.02 x 1023 atoms

d)

6.02 x 1023 atoms

62.

What is the percent composition of magnesium in MgCl2?

a)

25.5 %

b)

33.3%

c)

40.6%

d)

66.7%

63.

Calculate the pH of a solution if [OH-]= 1 x10-4

a)

1

b)

4

c)

10

d)

9

64.

Which of the following are characteristics of bases?

a)

bitter tasting

b)

pH less than 7

c)

turn blue litmus paper red

d)

increases concentration of H3O+ ions

65.

The idea that the number of atoms of molecules in a substance is proportional to its physical mass is accredited to-

a)

Amedeo Avogadro

b)

Timothy Taiwo

c)

Jorge Hernandez

d)

Keisha Vigil

66.

When you use PV=nRT, what must the unit for temperature be in?

a)

degrees Celsius (0C)

b)

Kelvin (K)

c)

degrees Fahrenheit (0F)

67.

In a measurement, significant figure consist of the digits known ___________.

a)

only

b)

plus one estimated digit

c)

plus two estimated digits

68.
Which of the following is the answer for the problem with the correct number of significant digits?
23.91 x 12.861 = 307.50651
a)
308
b)
307.51
c)
307.5
d)
307
69.
The correct chemical formula for magnesium phosphide is
a)
MgP
b)
Mg₂P₃
c)
Mg₃P₂
d)
Mg₃(PO₄)₂
70.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
71.
The formula of calcium phosphate is 
a)
CaPO4
b)
Ca2(PO4)3
c)
Ca3PO4
d)
Ca3(PO4)2
72.
Particles in an atom that are neutral and have no charge are 
a)
negatrons 
b)
electrons 
c)
neutrons 
d)
protons 
73.
If the number of protons equal the number of _____, the atom will have no charge
a)
protons
b)
neutrons
c)
electrons
d)
nucleus
74.
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
75.
Signs that a chemical change has occurred include
a)
a change in color
b)
the release of bubbles
c)
the production of an odor
d)
all of the above
76.

Where on the periodic table are the metalloids found?

a)

Right Side

b)

Along the Zig Zag Line

c)

Left Side

d)

Bottom

77.
Silicon is a semiconductor and has properties of both metals and nonmetals. What type of element is Silicon? 
a)
Metal
b)
Nonmetal
c)
Metalloid
d)
Pretty
78.
Nonmetals are located in what section of this periodic table?
a)
Blue
b)
Yellow
c)
Pink
79.
How many protons does Carbon have?
a)
3
b)
4
c)
5
d)
6
80.
Density is...
a)
the amount of mass in an object
b)
the amount of space an object takes up
c)
the amount of mass in a given space
d)
the weight of an object
81.
Burning a piece of paper 
a)
Chemical Change 
b)
Physical Change 
82.
Melting Ice 
a)
Chemical Change 
b)
Physical Change 
83.
How many MOLECULES are in the following compound:  CaCO3
a)
1
b)
3
c)
5
d)
0
84.

What are the name of the atoms of the same element that have a different number of neutrons ?

a)

Allotropes

b)

Radio actives

c)

Organics

d)

Isotopes

85.
A "group" is a ____________ on the periodic table.
a)
column
b)
row
86.
A "period" is a ____________ on the periodic table.
a)
column
b)
row
87.
Helium, neon, argon, krypton, xenon, and radon are known as  _____________.
a)
halogens
b)
noble gases
c)
metalloids
d)
transition elements
88.
Which of these elements is a metal?
a)
argon
b)
carbon
c)
iron
d)
hydrogen
89.
The element Tellurium has the atomic mass of 127.60 and its atomic number is 52. How many neutrons are in the element Tellurium?
a)
179.60
b)
127.60
c)
52
d)
76
90.
The substance that is dissolved in a solution
a)
Solute
b)
Solvent
c)
Solution
d)
Solubility
91.
This state of matter has a definite volume, but not a definite shape
a)
solid
b)
liquid
c)
gas
92.
AB + CD →AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
93.
Identify this type of reaction,
Cl2 + 2KI -->  I2 + 2KCl
a)
Synthesis
b)
Single displacement
c)
Double displacement
d)
Decomposition
94.
2 C5H5 + Fe --> Fe(C5H5)2 
a)
single displacement
b)
double displacement
c)
decomposition
d)
synthesis
95.
Which of the following is an example of synthesis?
a)
Na + Br2 --> NaBr
b)
KClO3 --> KCl + O2
c)
HgO + Cl2-->HgCl + O2
d)
Cl2 + NaBr --> NaCl + Br2
96.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single diplacement
d)
Double displacement
97.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-5
d)
1-20
98.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
99.

A base is a substance

a)

That releases OH- ions when dissolved in water

b)

That releases H+ ions when dissolved in water

c)

Does not release any ions when dissolved in water

d)

None of the above

100.
Boyle's Law shows the relationship between between which two factors of a gas?
a)
volume and pressure 
b)
temperature and pressure 
c)
pressure and temperature 
d)
Volume and mass
101.
Charles's law shows the relationship between which two factors of a gas ?
a)
volume and temperature 
b)
volume and pressure 
c)
pressure and volume
d)
volume and mass
102.
Charles's law shows that the temperature and volume of a gas are always........
a)
inversely proportional 
b)
directly proportional 
103.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
104.
What is 50 C in Kelvin?
a)
223
b)
323
c)
100
d)
50
105.
Boyle's law :  The pressure and volume of a gas show a _____ relationship. 
a)
Inverse 
b)
Direct 
106.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm (make sure you use the correct R value).
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
107.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
108.
Determine the number of moles in a container of gas at STP with a volume of 99.2 L. 
a)
2222.08 moles
b)
4.43 moles
c)
22.4 moles 
d)
76.8 moles
109.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)
10.1 mol
d)
4.5 mol
110.
How many moles are in 19.82 g Mg? 
a)
1.226mol Mg
b)
481.7mol Mg
c)
1.000mol Mg
d)
 0.82 mol Mg
111.

How many liters of N2, at STP, will react with 53.0 g H2 to form ammonia?


N2 + 3H2 --> 2NH3

a)

396 L

b)

17.6 L

c)

196 L

d)

588 L

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