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DC MIDTERM STUDY GUIDE

Total questions: 150

Worksheet time: 7hrs 49mins

Name
Class
Date
1.

Shown are the units for....

a)

specific heat capacity

b)

mass

c)

temperature

d)

energy

2.
Thermal energy ALWAYS moves from _____ to _____.
a)
solid to liquid
b)
ice to water
c)
hot to cold
d)
solid to gas
3.
LT3: If two objects have different temperatures, heat will flow from the warmer object to the cooler one UNTIL ____________
a)
one reaches a temperature of zero
b)
they both have an equal temperature
c)
one runs out of energy
4.
If the specific heat of water is 4,186 J/kg∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? 
a)
-80,371.2
b)
44,938.6
c)
80,371.2
d)
112,575.9
5.
How many Joules of energy are required to change 10 gram of water from 20 οC to 90 οC?
a)
1400 J
b)
2800 J
c)
210,000 J
d)
1,400,000 J
6.
How many Joules of energy are required to make 100 grams of ice at 0 οC completely melt?
a)
200 J
b)
400 J
c)
30,000 J
d)
2,000,000 J
7.
Water molecules have the greatest kinetic energy in
________________
a)
Ice at 0 °C.
b)
Water at 373 K.
c)
Water at 98 °C
d)
Steam at 150 °C.
8.
A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C.  Calculate the specific heat capacity of iron.    
a)
0.46 J/gxoC
b)
1.654 J/gxoC
c)
2,567,446.875 J/gxoC
9.
 How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/gx°C?    
a)
297 Joules
b)
0.003 Joules
c)
297 J/gx°C
d)
0.003 J/gx°C
10.
A 0.3 g piece of copper is heated and fashioned into a bracelet.  The amount of energy transferred by heat to the copper is 66,300 J.  If the specific heat of copper is 390 J/g 0C, what Is the change of the copper's temperature? 
a)
566.7 °C
b)
77,571,000 Joules
11.
When a  piece of aluminum foil is taken out of the oven and cools from 100° to 50°, What is the change in temperature?
a)
50°
b)
0°
c)
100°
d)
150°
12.
The specific heat of aluminum is 0.21 J/g°C.  How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?
a)
105 J
b)
10.5 J
c)
1.05 J
13.
20 g of water. specific heat of water is 4.18 J/x°C.  temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings?
a)
418 Joules
b)
209 J
c)
83 J
d)
4.18 J
14.
If 200 grams of water is to be heated from 24.0° C to  100.0° C to make a cup of tea, what is the mass and what is the change in temperature?
a)
m=200g
∆t= 66
b)
m=200g
∆t=124
c)
m=200
∆t=100
d)
m=200g
∆t=76
15.
The specific heat(c) of copper is 0.39 J/g °C. What is the temperature change(∆t) when 100 Joules of heat(Q) is added to 20 grams?
a)
12.82 °C
b)
24.12°C
c)
351 °C
16.

The Combined Gas Law involves what three variables?

a)
Solid Liquid Gas 
b)
Speed Velocity Acceleration 
c)
Elements Compounds Mixtures 
d)
Pressure Temperature Volume 
17.
A gas is heated from 263K to 298K. The volume is increased from 24.0L to 35.0L. If the original pressure was 1.00 atm, what is the new pressure?
a)
0.78 atm
b)
1.65 atm
c)
1.28 atm
d)
0.61 atm
18.

A weather balloon has a volume of 105L at 0.97 atm when the temperature is 318K. What is the volume at 293K and 1.05 atm?

a)

89.4 L

b)

0.32 L

c)

93.8 L

d)

3.13 L

19.

If I initially have a gas at a pressure of 12.0 atm, a volume of 23.0 liters, and a temperature of 200. K, and then I raise the pressure to 14.0 atm and increase the temperature to 350. K, what is the new volume of the gas?

a)

12.8 liters

b)

34.5 liters

c)

51 liters

d)

6.4 liters

e)

none are correct

20.

If I have 27 liters of gas at a temperature of 67oC and a pressure of 93 atm, what will be the pressure of the gas if I raise the temperature to 94oC and decrease the volume to 12 liters?

a)

225.9 atm

b)

238.9 atm

c)

114.5 atm

d)

149.1 atm

21.

A sample of gas is heated in a 2 L container at a temperature of 320 Kelvin. The pressure in the container is 2.5 atm. What is the new pressure if the volume is decreased to 1 L and the temperature is reduced to 250 K?

a)

4.6 atm

b)

1.7 atm

c)

3.9 atm

d)

5.9 atm

22.
A gas of volume V is placed in a balloon. The absolute (Kelvin) temperature is tripled. The volume will be _____ what it was originally. 
a)
1/3
b)
1/6
c)
3 times
d)
6 times
23.

If 3.0 L of helium at 293 K with a pressure of 1.97 atm is allowed to expand to 4.4 L with the pressure staying constant. What is the new temperature?

a)

702 K

b)

430 K

c)

157 K

d)

0 K

24.

A weather balloon has a volume of 105 L at 0.97 atm when the temperature is 318 K. What is the volume at 293 K and 1.05 atm?

a)

89.4 L

b)

0.32 L

c)

93.8 L

d)

3.13 L

25.

A balloon contains 3.5 L of He gas at 27 oC and 1.00 atm.  At what temperature in Celsius will its volume be 3.0 L at 1.09 atm?

a)
8 oC
b)
281 oC
c)
123 oC
d)
10oC
26.
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
27.
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
28.
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
29.

2Al + 6HCl --> 2AlCl3 + 3H2

Aluminium reacts with hydrochloric acid. How many grams of aluminum are necessary to produce 11 L of hydrogen gas at STP?

a)

13

b)

8.8

c)

0.99

d)

1.0

30.

1Mg + 2H2O --> Mg(OH)2 + H2

What volume of hydrogen will be produced at STP by the reaction 67.3 g of magnesium?

a)

62.0 L

b)

0.12 L

c)

2.77 L

d)

1.15 L

31.

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

32.

How many liters of SO2 will be produced from 55.0 L of O2 at STP?


2H2S + 3O2 --> 2SO2 + 2H2O

a)

55.0 Liters

b)

36.7 Liters

c)

18398 Liters

d)

2.45 Liters

33.
Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3.  If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.
a)
AlCl3
b)
Cl2
c)
Al
34.

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
35.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
36.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
37.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
38.

Find the empirical formula for a compound which contains 32.8% chromium and 67.2% chlorine.

a)

CrCl

b)

CrCl3

c)

Cr3Cl

d)

Cr2Cl6

39.

A compound containing 92.3 percent carbon and 7.7 percent hydrogen. What is the empirical formula?

a)

CH

b)

CH2

c)

C2H

d)

C2H2

40.

Fe + S →\rightarrow  FeS

How many grams of FeS are formed from 7.62g of Fe reacted with excess S?

a)
3.82g
b)
7.62g
c)
12.2g
d)
11.4g 
41.

CuCl2 + 2NaNO3 --> Cu(NO3)2 + 2NaCl


If 15.0 grams of CuCl2 react with 20 g of NaNO3, how much NaCl can be formed?

a)

13.0 g of NaCl

b)

98 g of NaCl

c)

26 g of NaCl

d)

17.4 of NaCl

42.

4NH3 + 5O2 → 4NO + 6H2O

Based on reaction above, oxygen is a limiting reactant. Calculate the mass of NO formed if the mass of oxygen reacted is 1.80g.

a)

0.37g

b)

0.045g

c)

1.35g

d)

11.1g

43.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g
44.

If you start with 3.88 x 1024 atoms of Na and an excess of Cl2, how many grams of NaCl should you get?

2Na + Cl2 −−〉 2NaCl

a)

376.66

b)

6.45

c)

753.31

d)

188.33

45.

If 3.29 x 1023 atoms of potassium react with excess water, APPROXIMATELY how many liters of hydrogen gas would be produced at STP?

2 K + 2 H2O --> 2 KOH + H2

a)

6L

b)

5L

c)

4L

d)

3L

46.
2H2  +   O2  →  2H2O
How many moles of oxygen are consumed if 8 moles H2 are used?
a)
2
b)
4
c)
6
d)
8
47.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO 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
48.
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
49.
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
50.
 SiO2 + 3C → SiC + 2CO
I need to add 8 moles of Carbon to the reaction. How many grams of Carbon should I weigh?
a)
96 g
b)
0.67 g
c)
2.67 g
d)
48 g
51.

Cl2 + 2 KBr → Br2 + 2 KCl How many grams of potassium chloride can be produced from 356 g of potassium bromide?

a)
749 g
b)
223 g
c)
479 g
d)
814 g
52.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
53.
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
54.
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
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.
Which molecule would have this molecular geometry?
a)
BF3
b)
CH4
c)
PCl5
d)
CO2
57.
Who could this molecule be?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
58.
Who could this be? 
a)
CO2
b)
NH3
c)
H2S
d)
CH4
59.
Who could this be?
a)
H2O
b)
NH3
c)
CO2
d)
CH4
60.
Which of the following molecular shapes would have a bond angle of 180 Degrees?
a)
Bent
b)
Trigonal Planar
c)
Tetrahedral
d)
Linear
61.
In a polar bond, the more electronegative element will assume a partial ________ charge.
a)
positive
b)
negative
62.

What kind of bond would form between, F & F?

a)

Ionic

b)

Polar Covalent

c)

Nonpolar Covalent

63.

Does the following reference Polar, Nonpolar, or both:

"affected by an electrical charge"?

a)

Polar

b)

Nonpolar

c)

Both

64.

True or False

Attractions between polar molecules are STRONGER than attractions between nonpolar molecules.

a)

True

b)

False

65.
In a polar covalent bond, electrons are shared ___________.
a)
equally
b)
unequally
c)
between non-metals with similar electronegativities
d)
between a metal and a non-metal
66.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
67.

Which molecule contains bonds with the LEAST polarity?

a)
HCl
b)
CCl4
68.

Which substance would have the strongest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

C3H8

69.

The STRONGER the intermolecular forces of a substance the _____________ the boiling point

a)

higher

b)

lower

70.
Hydrogen bonding occurs when hydrogen is bonded to N, O, or F.  Which of the following has hydrogen bonding?
a)
CBr4
b)
NO2
c)
H2S
d)
NH3
71.

London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the WEAKEST London forces?

a)
F2
b)
Br2
c)
I2
d)
Cl2
72.
What will be the state of the following molecule?
a)
gas
b)
liquid
c)
solid
73.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
74.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
75.
What is the measure of a tetrahedral bond angle?
a)
90 Degrees
b)
109.5 Degrees
c)
120 Degrees
d)
180 Degrees
76.

Does the following reference Polar, Nonpolar, or both:

"electronegativity values are the same"?

a)

Polar

b)

Nonpolar

c)

Both

77.

Is this molecule polar or nonpolar?

a)

polar

b)

nonpolar

78.

Which is the correct molecular structure for carbon monoxide?

a)
b)
c)
d)
79.

What is the correct Lewis Dot Structure for ammonia NH3

a)
b)
c)
d)
80.

What is the name of CF4?

a)

carbon tetrafluoride

b)

monocarbon tetrafluoride

c)

tetracarbon monofluoride

d)

carbon fluoride

81.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
82.

If a compound were to form between these ions Sn+4 and O-2 what would its formula be?

a)

SnO

b)

Sn4O2

c)

Sn2O4

d)

SnO2

83.
Which of these compounds is ionic? 
a)
Carbon dioxide
b)
Dinitrogen trioxide
c)
Silicon tetrachloride
d)

Magnesium Phosphide

84.

Name this formula:  BaSO4

a)

Barium Sulfuroxide

b)

Barium Sulfite

c)

Barium (II) Sulfate

d)

Barium Sulfate

85.

The proper formula for Aluminum Cyanide is...

a)

AlCN

b)

Al3CN

c)

Al(CN)3

d)

AlCN3

86.

what is the name of CuMnO4

a)

Copper Manganese Tetraoxide

b)

Copper Permanganate

c)

Copper (IV) Permanganate

d)

Copper (I) Permanganate

87.

Name this compound, NF6

a)

Nitrogen Fluoride

b)

Nitrogen hexafluoride

c)

Hexanitrogen monofluoride

d)

Mononitrogen hexafluoride

88.
When calcium binds with iodine, the compound formed is
a)
CaI
b)
Ca₂I
c)
CaI₂
d)
Ca₂I₂
89.

What is the name for MgF2 ?

a)

magnesium fluoride

b)

magnesium difluoride

c)

magnesium(II) fluoride

d)

magnesium fluoride(II)

90.
What is the formula for potassium chromate
a)
K2CrO4
b)
K2Cr
c)
KCr2
d)
K(CrO4)2
91.
What is the formula for Sulfur hexafluoride? 
a)
SF6
b)
S6F5
c)
S6F8
d)
SF9
92.
Name Al2S3
a)
Aluminum sulfide
b)
Dialuminum trisulfide
c)
ammonium sulfide
d)
aluminum (II) sulfice
93.
Name the compound NH4OH
a)
ammonium hydroxide
b)
ammonia oxyhydride
c)
mononitrogen tetraoxihydride
d)
hydrogen nitrate
94.
What is the formula for tin (II) chromate 
a)
Sn2(CrO4)4
b)
Sn(CrO4)2
c)
Sn4(CrO4)2
d)
SnCrO4
95.

Name the compound Mg3(PO4)2

a)

magnesium phosphate

b)

magnesium (III) phosphate

c)

magnesium phosphite

d)

trimagnesium diphosphate

96.

Name the compound CuO

a)

copper (II) oxide

b)

copper oxide

c)

copper (I) oxide

d)

copper monoxide

97.
What formula results when Fe+3 and CO3-2 ions bond?
a)
FeCO3
b)
Fe2CO3
c)
Fe2(CO3)3
d)
Fe3(CO3)2
98.

The proper name for this compound, P2O5, is ________

a)

phosphorus dioxide

b)

diphosphorus pentoxygen

c)

phosphate

d)

diphosphorus pentoxide

99.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
100.

Does HCN have hydrogen bonding?

a)
yes
b)
no
101.

Does SiH4 have hydrogen bonding?

a)
yes
b)
no
102.
Which is the second strongest intermolecular force, after hydrogen bonding?
a)
dipole-dipole attraction
b)
London forces
103.

________________________ have the strongest intermolecular forces of attraction.

a)

Dipole- Dipole

b)

Dispersion

c)

Hydrogen Bonds

104.

The model used to describe and explain the bonding and arrangement of atoms in a solid metal is the

a)

ball and stick model

b)

electron sea model

c)

metalloid model

d)

valence shell electron pair repulsion theory

105.
Which is the strongest intermolecular force below"
a)
Ionic
b)
Dispersion
c)
Hydrogen
d)
Metallic
106.

Identify the following chemical reaction.

2 NaBr + 1 Ca(OH)2 ----> 1 CaBr2 + 2 NaOH

a)

Synthesis (or combination)

b)

Decomposition

c)

Single displacement

d)

Double displacement

107.

Identify the following chemical reaction.

3 HBr + 1 Al(OH)3 ----> 3 H­2O + 1 AlBr3

a)

Synthesis (or combination)

b)

Decomposition

c)

Single displacement

d)

Double displacement

108.

Identify the following chemical reaction.

Pb + FeSO4 ----> PbSO4 + Fe

a)

Synthesis (or combination)

b)

Decomposition

c)

Single displacement

d)

Double displacement

109.

What reaction has the following general formula:

AB --> A + B

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

110.

What reaction has the following general formula:

A + CD --> C + AD

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

111.

What reaction has the following general formula:

A + B --> AB

a)

Synthesis

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

112.

Combustion reactions will always produce

a)

Oxygen and a solid

b)

Liquid nitrogen and heat

c)

Oxygen and heat/energy

d)

CO and H2O

113.

Which chemical reaction always starts with a hydrocarbon that reacts with oxygen and produces carbon dioxide and water?

a)

Decomposition

b)

Synthesis

c)

Combustion

d)

Single Replacement

114.

Which phrase describes what happens to atoms in a chemical reaction?

a)

never lost or gained, just rearranged

b)

sometimes lost, never rearranged

c)

sometimes lost, gained, or rearranged

d)

lost or gained, never rearranged

115.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
116.

Fill in the blank. (Copper has a charge of 2+)

Cu+ AgNO3 → Ag + _____

a)

Cu(NO3)2

b)

CuNO3

c)

CuAg

d)

Cu

117.

What type of reaction is this?

2 C6H14 + 19 O2 → 12 CO2 + 14 H2O

a)

Single Replacement

b)

Double Replacement

c)

Combustion

d)

Decomposition

118.

Predict the products for the this Single Replacement reaction:

K + HCl →

a)

KCl + H2

b)

KHCl

c)

KH + Cl2

d)

HCl + K2

119.

Predict the products for the this Double Replacement reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

120.

Complete the balanced equation for this Double Replacement reaction.

3 NaOH + Fe(NO3)3 →

a)

NaFe + OH(NO3)3

b)

NaNO3 + Fe(OH)3

c)

3 NaNO3 + Fe(OH)3

d)

3 NaFe + 3 (OH)NO3

121.

Predict the products for the decomposition of aluminum oxide, Al2O3 →

a)

Al + O2

b)

O + Al2

c)

Al2 + O3

d)

Al + O

122.

Predict the products for the this Single Replacement reaction: (Copper has a charge of 1+)

Mg + CuCl →

a)

MgCl2 + Cu

b)

Mg + Cu

c)

MgCu + Cl2

d)

MgCl + Cu2

123.

What are the products of this reaction:

C2H4 + O2 →

a)

C2O2 + H4

b)

CO2 + H2 + O2

c)

CO + H

d)

CO2 + H2O

124.

What would the missing product be?


Au2S3 + 3 H2 ➔ 2 Au + ____________

a)

2 H3S

b)

2 AuH3

c)

3 H2S

125.

What is the missing product?


Na2CO3 + 2 AgNO3 ➔ 2 NaNO3 + __________

a)

2 Ag3Na

b)

2 AgCO3

c)

Ag2CO3

126.

Predict the products of this reaction:

AgNO3 + KCl →

a)

AgCl + KNO3

b)

AgK + ClNO3

c)

KAg + NO3Cl

d)

AgCl + 3 KNO

127.
Balance this equation:
 2Li + Cl2 -> LiCl
a)
2Li + Cl2 -> 4LiCl2
b)
2Li + Cl2 -> LiCl2
c)
2Li + Cl2 -> 2LiCl
128.
What are the coefficient used to balance the equation below?
__Ag2O →__ Ag +___O2
a)
2,4,1
b)
1,1,1
c)
2,1,2
d)
2,2,2
129.
 Balance this equation:

__ Al + __ HCl → __ H2 + __ AlCl3
a)
2, 6, 3, 2
b)
it is already balanced
c)
4, 12, 3, 4
d)
2, 1, 4, 5
130.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__Na + __H2O --> __NaOH + __H2
a)
2,2 --> 2,1
b)
4,4 --> 4,1
c)
1,2 --> 2,4
d)
1,2 --> 2,1
131.

What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?

__Ca + __H2O --> __Ca(OH)2 + __H2

a)
2,1 --> 2,1
b)
1,2 --> 1,1
c)
1,2 --> 2,4
d)
1,2 --> 2,1
132.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__CO + __Fe2O3--> __Fe + __CO2
a)
3,1 --> 2,3
b)
3,2 --> 1,1
c)
3,2 --> 2,4
d)
3,2 --> 2,1
133.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__CH4 + __O2 --> __CO2+ __H2O
a)
2,1 --> 2,1
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1
134.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__AgNO3 + __H2S --> __Ag2S+ __HNO3
a)
2,1 --> 1,2
b)
1,2 --> 1,1
c)
1,2 --> 1,2
d)
1,2 --> 2,1
135.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__H2 + __S --> __H2S
a)
1,1 --> 1
b)
2,2 --> 2
c)
1,2 --> 1
d)
1,2 --> 2
136.
What is the right ratio of chemicals for the BCE (Balanced Chemical Equation)?__FeCl3 + __Ca(OH)2 --> __Fe(OH)3 + __CaCl2
a)
4,3--> 2,1
b)
3,2 --> 3,1
c)
2,3 --> 2,2
d)
2,3 --> 2,3
137.
Fill in the blanks with coefficient:
PCl5+_ H2O→_ HCl+H3PO4
a)
4, 5
b)
1, 6
c)
3, 8
d)
2,2
138.
Balance this equation.
_Mg + _Cl2 --> _MgCl2
a)
1, 2,1
b)
already balanced
c)
2,1,1
d)
1,1,2
139.

Determine which product is the precipitate.


MgCl2 + K2CO3 --> 2NaCl + MgCO3

a)

MgCl2

b)

K2CO3

c)

NaCl

d)

MgCO3

140.

Determine which product is the precipitate.


CaSO4 + Pb(NO3)2 --> PbSO4 + Ca(NO3)2

a)

CaSO4

b)

Pb(NO3)2

c)

PbSO4

d)

Ca(NO3)2

141.

Determine which product is the precipitate.


BaI2 + CaSO4 --> BaSO4 + CaI2

a)

BaI2

b)

CaSO4

c)

BaSO4

d)

CaI2

142.

Determine which product is the precipitate.


NaCl + AgNO3 --> NaNO3 + AgCl

a)

NaCl

b)

AgNO3

c)

NaNO3

d)

AgCl

143.

Determine which product is the precipitate.


2KBr + Hg(NO3)2 --> 2KNO3 + HgBr2

a)

KBr

b)

Hg(NO3)2

c)

KNO3

d)

HgBr2

144.

Determine which product is the precipitate.


2LiCl + Pb(C2H3O2)2 --> 2LiC2H3O2 + PbCl2

a)

LiCl

b)

Pb(C2H3O2)2

c)

LiC2H3O2

d)

PbCl2

145.

Determine which product is the precipitate.


FeI2 + 2NaOH --> 2NaI + Fe(OH)2

a)

FeI2

b)

NaOH

c)

NaI

d)

Fe(OH)2

146.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
147.

Which atom has the largest atomic radius?

a)

Potassium (K)

b)

Rubidium (Rb)

c)

Francium (Fr)

d)

Cesium (Cs)

148.

Atoms in the same family on the periodic table have

____ numbers of valence electrons and _____ properties.

a)

different, different

b)

different, similar

c)

similar, similar

d)

similar, different

149.

Which elements have properties that are in between metals and nonmetals.

a)

Halogens

b)

Alkali Metals

c)

Metalloids

d)

Alkaline Earth Metals

150.

What makes a valence electron more attracted to the nucleus?

a)

less distance between the nucleus and having less protons

b)

less distance between the nucleus and having more protons

c)

more distance between the nucleus and having less protons

d)

more distance between the nucleus and having more protons

e)

less distance and having more valence electrons

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