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Honors Chemistry Midterm

Total questions: 73

Worksheet time: 2hrs 2mins

Name
Class
Date
1.

Liquid state DOES NOT HAVE which of the following properties?

a)

definite shape

b)

definite volume

c)

flows easily

d)

very hard to compress

2.

1. Homogeneous mixtures are _______

a)

called solutions.

b)

only liquids.

c)

have more than one phase.

d)

pure substances.

3.

What is true of compounds?

a)

only be separated by a chemical reaction.

b)

have variable composition

c)

always have combined physical properties of its elements

d)

can be separated by physical change

4.

Which is chemical property?

a)

ability to burn

b)

boiling point

c)

hardness

d)

color

5.

1. A metric unit of volume is

a)

Liters

b)

grams

c)

meters

d)

gallons

6.

All atoms of the same element have the same number of

a)

protons

b)

neutrons

c)

electrons

d)

protons and neutrons

7.

The number of neutrons can always be calculated by

a)

subtracting atomic number by mass number

b)

adding atomic number to the mass number

c)

adding number of electrons and protons

d)

divide mass number by 2

8.

Which is NOT TRUE about atoms?

a)

Electrons have more mass than protons.

b)

Electrons have a negative charge.

c)

The neutron is found in the nucleus of an atom.

d)

Neutrons have mass but not charge.

9.

The maximum number of electrons that can occupy the second energy level is ____

a)

8

b)

2

c)

18

d)

32

10.

Neutral hydrogen atoms at ground state only have _________ sublevel electrons?

a)

s

b)

d

c)

f

d)

p

11.

Which of the following elements is a metal?

a)

Na

b)

N

c)

F

d)

Br

12.

1. The alkali metals do not include

a)

Mg

b)

Cs

c)

Li

d)

Na

13.

An Aluminium ion has a charge of?

a)

+3

b)

-3

c)

+5

d)

-5

14.

What is the formula for Cesium Sulfide?

a)

Cs2S

b)

CsS

c)

CsS2

d)

Cs3S

15.

When a transition metal , the numerical value of the charge is indicated by a ____

a)

Roman numeral

b)

prefix

c)

suffix

d)

by periodic table only

16.

Which of the following is a chemical change?

a)

Burning oil

b)

Making a solution

c)

Melting wax

d)

Cutting a piece paper

17.

Convert 444 mg into grams

a)

.444 g

b)

4.44 g

c)

44.4 g

d)

.00444 g

18.

What is the name for MgI?

a)

Magnesium Iodide

b)

Magnesium Diodide

c)

Magnesium (II) Iodide

d)

Monomagnesium Diodide

19.
Which of the following is the correct name for MgF2? 
a)
Magnesium Fluorine 
b)
 Magnesium Difluoride 
c)
Magnesium Fluoride 
20.
Which of the following is the correct name for PbCl4?  
a)
Lead Chloride
b)
Lead (I) Chloride
c)
Lead (IV) Chloride
21.
 Which of the following is the correct formula for copper (I) sulfide?  
a)
CuS
b)
Cu2S
c)
CuSO4
22.
Which of the following is the correct name for Fe2(SO4)3?   
a)
 Iron (II) Sulfate
b)
Iron (II) Sulfite
c)
Iron (III) Sulfate
23.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
24.
In which region would the nonmentals be found?
a)
1
b)
4
c)
3
d)
5
25.
The positive particles of an atom are 
a)
electrons 
b)
positrons 
c)
neutrons 
d)
protons 
26.
A "period" is a ____________ on the periodic table.
a)
column
b)
row
27.
Helium, neon, argon, krypton, xenon, and radon are known as  _____________.
a)
halogens
b)
noble gases
c)
metalloids
d)
transition elements
28.
Why would a ball float on top of water?
a)
the ball is more dense than water
b)
the ball is less dense than water
c)
they both have equal densities
29.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
30.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
31.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
32.
Name the compound AlBr3
a)
aluminum bromide
b)
aluminum tribromide
c)
aluminum bromine
d)
monoaluminum tribromide
33.
nitrate
a)
N3-
b)
NO21-
c)
NO2-
d)
NO31-
34.
Experimental Value = 86 cm
Accepted Value = 78 cm
Percent Error?
a)
12%
b)
10 %
c)
8%
d)
6%
35.
How many molecules are in 9.44 moles of aluminum chloride?
a)
5.68 molecules AlCl3
b)
5.68x1024 molecules AlCl3
c)
0.705 molecules AlCl3
d)
1.25x1023 molecules AlCl3
36.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
37.
What is the noble gas configuration for boron?
a)
[He]1s22s2
b)
[He]2s22p2
c)
[He]2s22p1
d)
[Li]2s22p1
38.
What is the formula for disulfur trioxide?
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
39.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
40.

In an atom, an orbital represents

a)

the most probably location of a proton

b)

the most probable location of an electron

c)

the least probably location of a neutron

d)

photons emitted as electrons move to lower energy levels

41.

Which particle has a mass so small, it is considered to be 0 amu?

a)

proton

b)

hydrogen nucleus

c)

neutron

d)

electron

42.

How would you classify NaCl?

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

43.

The type of reaction that releases energy as heat is called

a)

endothermic

b)

exothermic

c)

respiration

d)

photosynthesis

44.

if an acid is diluted it

a)

has a large amount of water mixed into it

b)

has a small amount of water mixed into it

c)

is very 'acidus' sour

d)

is corrosive and cannot be eaten

45.

To neutralise an acid you add a

a)

acid

b)

base

c)

Ph indicator

d)

equal amount of water

46.

Is the equation balanced?: 2H2O + O2 --> 4MgO + 3Fe

a)

yes

b)

no

47.

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

48.
Is this equation balanced?
a)
yes
b)
no
c)
Not enough information
49.
How many particles are in 13.5 grams of Beryllium?
a)
1.5 particles
b)
9 particles
c)
4x1023 particles
d)
9x1023 particles
50.
2 NaClO3 (s) --> 2NaCl (s) +3 O2 (g)  
12.00 moles of NaClO3 will produce how many grams of O2?
a)
256 g of O2
b)
576 g of O2
c)
288 g O2
51.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 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
52.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
53.
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%
54.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
55.
4 Al + 3 O2 –> 2 Al2O3  How much aluminum would be needed to completely react with 45 grams of O2?
a)
1.05 moles
b)
3.75 moles
c)
1.875 grams
d)
1.875 moles
56.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
57.
How many liters of NH3 are needed to react completely with 30.0L of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
5.0 L
b)
20.0 L
c)
7.5 L
d)
120.0 L
58.
What is the formula for phosphorous acid?
a)
H3PO4
b)
H2PO4
c)
H3P
d)
H3PO3
59.
Name HF
a)
hydrofluoric acid
b)
Hypofluoric acid
c)
hydrogen fluorine acid
d)
fluoric acid
60.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

61.
Holly has an unknown substance in a beaker. She wants to determine the relative pH of the unknown substance. She places a piece of blue litmus paper into the substance, and the litmus paper stays blue.
The substance in the beaker
a)
is a base.
b)
has a neutral pH.
c)
is an acid.
d)
does not have a pH.
62.

Which compound is the conjugate acid? (Hint: Determine the base)

PO43- + HNO3 ==> NO3- + HPO42-

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

63.
HSO4- + H2O → H3O++ SO42-
Identify the Acid in the above reaction.
a)
HSO4-
b)
H2O
c)
H3O+
d)
SO42-
64.

KOH has a pOH of 3.0, what is the [OH-]?

a)

0.01 M

b)

0.001 M

c)

0.0001 M

d)

0.1 M

65.

A solution of HCl has a [H+] = 7.2 x 10-9. Is this and acid or a base?

a)

Acid

b)

Base

66.

What is the pOH of a solution with and [OH-] = 4.5 x 10-4?

a)

3.53

b)

3.80

c)

3.35

d)

5.33

67.
What is the [OH-] if the [H+] is 1.0 x 10-3M?
a)
1.0 x 10-3 M
b)
6.02 x 10-23 M
c)
1.0 x 10-14 M
d)
1.0 x 10-11 M
68.

What is this piece of apparatus called

a)

Pipette

b)

Burette

c)

Janette

d)

Cuvette

69.

What is the reading on this burette?

a)

24.0cm3

b)

25.8cm3

c)

24.2cm3

d)

23.9cm3

70.
The reaction of perchloric acid (HClO4) with lithium hydroxide (KOH) is described by the equation
HClO4 + KOH → KClO4 + H2O
Suppose 100 mL of perchloric acid is neutralized by exactly 50,0 mL of 1.0 M of Potassium hydroxide. What is the concentration of the perchloric acid?
a)
0.5M
b)
50M
c)
2.0M
d)
1.0M
71.
The reaction of sulfuric acid (H2SO4) with Sodium hydroxide (NaOH) is described by the equation:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
Suppose 50 mL of NaOH with unknown concentration is placed in a flask with bromthymol blue indicator. A solution of 0.20 M H2SO4 is dripped into the NaOH solution. After exactly 25.0 mL of H2SO4 is added, the indicator changes from blue to yellow. What is the concentration of the KOH?
a)
0.20M
b)
4.0M
c)
2.5M
d)
0.4M
72.
What is the molarity of a NaOH solution if 11.6 mL of 3 M HCl was used to neutralize 25 mL of NaOH?
a)
1.392 M
b)
0.155 M
c)
0.718 M
73.

Calculate the volume of a 0.15 M Ba(OH)2 solution required to completely neutralize 45 ml of a 0.29 M HNO3 solution.

a)

43.5 ml

b)

87 ml

c)

23.3 ml

d)

51.9 ml

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