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Honors Chemistry MID- Mrs. Knowlton

Total questions: 145

Worksheet time: 1hrs 28mins

Name
Class
Date
1.

Chemistry is a natural science that deals with the study of

a)

living things and their life processes

b)

the physical features of Earth

c)

the composition, structure, properties, and changes of matter

d)

the composition, motion, and relative positions of stars and planets

2.

What is the physical state in which matter has a specific volume but does not have a specific shape?

a)

gas

b)

solid

c)

liquid

d)

salt

3.

A combination of sand, salt, and water is an example of a ____.

a)

homogenous mixture

b)

heterogeneous mixture

c)

compound

d)

pure substance

4.

Which one of the following is often separated into its components by simple techniques such as filtering or decanting?

a)

heterogeneous mixture

b)

compounds

c)

homogeneous mixture

d)

elements

5.

An element cannot _____.

a)

be part of a heterogeneous mixture.

b)

be part of a homogeneous mixture

c)

be separated into other substances by chemical means

d)

interact with other elements to form compounds

6.

The law of constant composition says ____.

a)

that the composition of a compound is always the same

b)

that all substances have the same composition

c)

that the composition of an element is always the same

d)

that the composition of a heterogeneous mixture is always the same

7.

In the following list, only ____ is not an example of a chemical reaction.

a)

dissolution of a penny in nitric acid

b)

the condensation of water vapor

c)

a burning candle

d)

the rusting of iron

8.

Of the following, only ____ is a chemical reaction.

a)

melting of lead

b)

dissolving sugar in water

c)

crushing of stone

d)

tarnishing of silver

9.

Which one of the following is not an intensive property?

a)

density

b)

temperature

c)

melting point

d)

mass

10.

Of the following, only ____ is an extensive property.

a)

density

b)

volume

c)

boiling point

d)

freezing point

11.

Precision refers to ____.

a)

how close a measured number is to other measured numbers

b)

how close a measured number is to the true value

c)

how close a measured number is to the calculated value

d)

how close a measured number is to zero

12.

Accuracy refers to ____.

a)

how close a measured number is to zero

b)

how close a measured number is to the calculated value

c)

how close a measured number is to other measured numbers

d)

how close a number is to the true value

13.

A separation process that depends on differing abilities of substances to form gases is called ____.

a)

filtration

b)

solvation

c)

distillation

d)

chromatography

14.

The freezing point of water at 1 atm pressure is ____.

a)

    0 °F0\ \degree F  

b)

0 K 

c)

0 °C0\ \degree C

d)

−273 °C-273\ \degree C  

15.

Which one of the following has the element name and symbol correctly matched?

a)

Ne, nitrogen

b)

Si, sulfur

c)

Ca, carbon

d)

Be, beryllium

16.

If matter is uniform throughout and cannot be separated into other substances by physical processes, but can be decomposed into other substances by chemical processes, it is called a(n) ____.

a)

heterogeneous mixture

b)

element

c)

homogeneous mixture

d)

compound

17.

If some measurements agree closely but differ widely from the actual value, these measurements are

a)

both accurate and precise

b)

neither precise nor accurate

c)

precise but not accurate

d)

accurate but not precise

18.

The homogeneous mixture in the illustration above is in container

a)

a

b)

b

c)

c

d)

d

19.

To determine density, the quantities that must be measured are

a)

mass and weight

b)

volume and weight

c)

volume and concentration

d)

volume and mass

20.

How many significant figures are in the number 30.80?

a)

3

b)

4

c)

0

d)

1

21.

How many significant figures are in the measurement 5000 g?

a)

4

b)

3

c)

2

d)

1

22.

The number with the most significant zeroes is ____.

a)

0.08

b)

0.00090

c)

90.300

d)

0.008001

23.

Round the number 0.00625 to two significant figures.

a)

0.0062

b)

0.0063

c)

0.00625

d)

0.006300

24.

The correct result (indicating the proper number of significant figures) of the following addition is ____. 12 + 1.2 + 0.12 + 0.012 = ?

a)

13

b)

13.3

c)

13.33

d)

13.332

25.

The correct result (indicating the proper number of significant figures) of the following problem is ____.

(0.002843)(12.80184)÷0.00032(0.002843)(12.80184)\div0.00032  

a)

113.73635

b)

113.736

c)

113

d)

110

26.

Sara and Jamal determined the density of a liquid three times. The values they obtained were 2.84 g/mL, 2.85 g/mL, and 2.80 g/mL. The accepted value is known to be 2.40 g/mL.

Are Sarah and Jamal's values precise? Explain why or why not. Are they accurate? Explain why or why not.

4 lines
27.

The charge on the manganese in the salt MnF3 is ________.

a)

1+

b)

1-

c)

3+

d)

3-

28.

Barium  forms an ion with a charge of ________.

a)

1+

b)

1-

c)

2+

d)

2-

29.

Iodine forms an ion with a charge of ________.

a)

1+

b)

1-

c)

2+

d)

2-

30.

What is the formula for sodium flouride?

(a)  

31.

What is the formula for magnesium iodide?

(a)  

32.

What is the formula for aluminum oxide?

(a)  

33.

What is formula for iron (III) oxide

(a)  

34.

What is the formula for dinitrogen pentaphosphide?

(a)  

35.

What is the formula for magnesium hydride?

(a)  

36.

What is the name of CuO?

(a)  

37.

What is the name of

NO3

(a)  

38.

What is the name of

K2S

(a)  

39.

What is the name of SO?

(a)  

40.

What is the name of

CaCl2

(a)  

41.

What is the name of

H2S (g)

(a)  

42.

The formula of bromic acid is

a)

H BrO4

b)

H Br (aq)

c)

H BrO

d)

H BrO3

43.

The correct formula of iron (III) bromide is

a)

FeBr3

b)

Fe3Br

c)

FeBr

d)

FeBr2

44.

The formula of ammonium carbonate is

a)

NH4CO3

b)

NH4(CO3)2

c)

(NH4)2CO3

d)

(NH3)2(CO3

45.

The formula for aluminum hydroxide is

a)

AlOH

b)

Al3OH

c)

Al(OH)3

d)

Al2(OH)3

46.

The formula for sodium perbromate is

a)

NaBrO3

b)

NaBrO4

c)

NaBrO5

d)

NaBr5

47.

The formula for hydrochloric acid is

a)

HCl

b)

HCl (aq)

c)

HClO3 (aq)

d)

H2Cl (aq)

48.

Write the formula for arsenic tribromide

a)

ArBr3

b)

Ar3Br

c)

As3Br

d)

AsBr3

49.

The correct formula for mercury (II) fluoride is

a)

HgF2

b)

Hg2F

c)

HgF

d)

HgFO2

50.

The correct formula for Cadmium (III) nitride is

a)

CdN

b)

Cd3N

c)

CdN3

d)

CaN

51.

The formula for perphosphoric acid is

a)

H3PO3

b)

H3PO4

c)

H3PO5

d)

H3PO2

52.

The formula for sodium hydride is

a)

NaH2

b)

NaH

c)

HNa

d)

H2Na

53.

The formula for calcium hydroxide is

a)

Ca2OH

b)

CaOH

c)

CaOH2

d)

Ca(OH)2

54.

What is the correct name for

K2S

a)

potassium sulfate

b)

potassium disulfide

c)

potassium bisulfide

d)

potassium sulfide

55.

What is the correct name for

Al2O3

a)

aluminum oxide

b)

dialuminum oxide

c)

dialuminum trioxide

d)

aluminum trioxide

56.

What is the correct name for

CaH2

a)

calcium dihydride

b)

calcium hydroxide

c)

calcium dihydroxide

d)

calcium hydride

57.

What is the correct name for SO?

a)

sulfur oxide

b)

sulfur monoxide

c)

sulfate

d)

monosulfur monoxide

58.

What is the correct name for

CrI3

a)

chromium iodide

b)

chromium (I) iodide

c)

chromium (III) iodide

d)

cobalt (III) iodide

59.

What is the correct name for

MgCl2

a)

manganese (II) chloride

b)

magnesium chloride

c)

magnesium (II) chloride

d)

magnesium dicholoride

60.

What is the correct name for

ZnSO4

a)

sinc (II) sulfate

b)

zinc sulfate

c)

zinc sulfide

d)

zinc (II) sulfite

61.

What is the correct name for

H2SO4

a)

sulfuric acid

b)

hydrosulfuric acid

c)

hydrogen sulfate

d)

persulfuric acid

62.

What is the correct name for

Cu2S

a)

copper sufide

b)

copper disulfide

c)

copper (I) sulfide

d)

copper (II) sulfide

63.

What is the correct name for

Zn(BrO)2

a)

zinc (II) hypobromite

b)

zinc hypobromite

c)

zinc (II) bromite

d)

zinc bromite

64.

What is the correct name for HBr (aq)?

a)

hydrogen bromide

b)

bromic acid

c)

hydrogenbromic acid

d)

hydrobromic acid

65.

What is the correct name for

Mg3(PO5)2

a)

magnesium phosphate

b)

magnesium (II) perphosphate

c)

magnesium (II) phosphate

d)

magnesium perphosphate

66.

What is the correct name for

Ba(ClO2)2

a)

barium chlorite

b)

barium hypochlorite

c)

barium (II) chlorite

d)

barium (II) hypochlorite

67.

Consider the following selected postulates of Dalton's atomic theory:

(i) Each element is composed of extremely small particles called atoms

(ii) Atoms are indivisible

(iii) Atoms of a given element are identical

(iv) Atoms of different elements are different and have different properties

Which of the postulates is(are) no longer considered valid?

a)

(i) and (ii)

b)

(ii) only

c)

(ii) and (iii)

d)

(iii) only

e)

(iii) and (iv)

68.

Which pair of substances could be used to illustrate the law of multiple proportions?

a)

SO2, H2SO4SO_2,\ H_2SO_4  

b)

CO, CO2CO,\ CO_2  

c)

H2O, O2H_2O,\ O_2  

d)

NaCl, KClNaCl,\ KCl  

69.

Which one of the following is not true concerning cathode rays?

a)

They originate from the negative electrode.

b)

They travel in straight lines in the absence of electric or magnetic fields.

c)

They are made up of electrons.

d)

The characteristics of cathode rays depend on the material from which they are emitted.

70.

Cathode Rays are deflected away from a negatively charged plate because _____.

a)

they are not particles

b)

they are positively charged particles

c)

they are neutral particles

d)

they are negatively charged particles

71.

The charge on an electron was determined in the _____.

a)

cathode ray tube, by J.J. Thomson

b)

Rutherford gold foil experiment

c)

Millikan oil drop experiment

d)

Dalton atomic theory

72.

_____- consist of fast-moving electrons.

a)

Alpha particles

b)

Beta rays

c)

Gamma rays

d)

X rays

73.

_____-consist of Helium nuclides.

a)

Alpha particles

b)

Beta rays

c)

Gamma rays

d)

X rays

74.

The gold foil experiment performed in Rutherford's lab _____.

a)

confirmed the plum-pudding model of the atom

b)

led to the discovery of the atomic nucleus

c)

was the basis for Thomson's model of the atom

d)

proved the law of multiple proportions

75.

In the Rutherford nuclear-atom model, _____.

a)

the heavy subatomic particles, protons and neutrons, reside in the nucleus

b)

the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass

c)

mass is spread essentially uniformly throughout the atom

d)

the three principal subatomic particles (protons, neutrons, and electrons) all have essentially the same mass and mass is spread essentially uniformly throughout the atom

76.

Of the following, the smallest and lightest subatomic particle is the _____.

a)

neutron

b)

proton

c)

electron

d)

nucleus

77.

All atoms of a given element have the same _____.

a)

mass

b)

number of protons

c)

number of neutrons

d)

number of electrons and neutrons

78.

Which combination of protons, neutrons, and electrons is correct for the isotope of copper,

2963Cu?_{29}^{63}Cu?  

a)

29 p+, 34 n°, 29 e−29\ p+,\ 34\ n\degree,\ 29\ e-  

b)

29 p+, 29 n°, 63 e−29\ p+,\ 29\ n\degree,\ 63\ e-  

c)

63 p+, 29 n°, 63 e−63\ p+,\ 29\ n\degree,\ 63\ e-  

d)

34 p+, 29 n°, 34 e−34\ p+,\ 29\ n\degree,\ 34\ e-  

79.

Isotopes are atoms that have the same _____ but differing _____.

a)

atomic masses, charges

b)

mass numbers, atomic numbers

c)

atomic numbers, mass numbers

d)

charges, atomic masses

80.

The atomic mass unit is presently based on assigning an exact integral mass (in amu) to an isotope of _____.

a)

hydrogen

b)

oxygen

c)

sodium

d)

carbon

81.

In the periodic table, the elements are arranged in _____.

a)

alphabetical order

b)

order of increasing atomic number

c)

order of increasing metallic properties

d)

increasing atomic mass

82.

Elements _____ exhibit similar physical and chemical properties.

a)

with similar chemical symbols

b)

with similar atomic masses

c)

in the same period of the periodic table

d)

in the same group of the periodic table

83.

An element in the upper right corner of the periodic table _____.

a)

is either a metal or metalloid

b)

is definitely a metal

c)

is either a metalloid or a nonmetal

d)

is definitely a nonmetal

84.

An element in the lower left corner of the periodic table _____.

a)

is either a metal or a metalloid

b)

is definitely a metal

c)

is either a metalloid or a nonmetal

d)

is definitely a nonmental

85.

Elements in the same group of the periodic table typically have _____.

a)

similar mass numbers

b)

similar physical and chemical properties

c)

similar physical properties only

d)

similar chemical properties only

86.

A molecular formula always indicates _____.

a)

how many of each atom are in a molecule

b)

the simplest whole-number ratio of different atoms in a compound

c)

which atoms are attached to which in a molecule

d)

the geometry of a molecule

87.

An empirical formula always indicates _____.

a)

how many of each atom are in a molecule

b)

the simplest whole-number ratio of different atoms in a compound

c)

which atoms are attached to in a molecule

d)

the geometry of a molecule

88.

Formulas that show how atoms are attached in a molecule are called _____.

a)

molecular formulas

b)

ionic formulas

c)

diatomic formulas

d)

structural formulas

89.

Sodium forms an ion with a charge of _____.

a)

1+

b)

1-

c)

2+

d)

0

90.

Name, describe, and explain JJ Thomson's model of the atom.

4 lines
91.

Rutherford's Gold foil experiment had three outcomes. What were they and how did Rutherford explain them?

4 lines
92.

The element X has three naturally occurring isotopes. The masses (amu) and % abundances of the isotopes are given in the table. Calculate the average atomic mass.

(a)  

93.

What is the % of aluminum in aluminum sulfate rounded to three significant figures?

a)

7.90%

b)

35.7%

c)

15.8%

d)

342.2%

94.

How many grams of hydrogen are in 46 g of CH4O?

a)

5.8g

b)

1.5g

c)

2.8g

d)

0.36

95.

The molar mass of magnesium nitrate, rounded to one decimal place, is ____ g/mol.

a)

148.3

b)

164.0

c)

204.2

d)

150.1

96.

How many molecules of CH4 are in 24.2 g of this compound?

a)

2.34 x 10^-26

b)

1.51 x 10^23

c)

9.11 x 10^23

d)

1.81 x 10^24

97.

what is the empirical formula of a compound that is 66.6% C, 11.2% H, and 22.2% O by mass?

a)

C6HO2

b)

C8H16O2

c)

C6H11O

d)

C4H8O

98.

A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular formula?

a)

C8H8O2

b)

C8H4O

c)

C4H4O

d)

C9H12O

99.

How many sulfur dioxide molecules are there in 0.180 mol of sulfur dioxide?

a)

6.94 x 10^24

b)

1.08 x 10^23

c)

1.91 x 10^23

d)

6.02 x 10^24

100.

What is the physical state in which matter has a specific volume but does not have a specific shape?

a)

gas

b)

solid

c)

liquid

d)

salts

e)

ice

101.

A combination of sand, salt, and water is an example of a ________.

a)

homogeneous mixture

b)

heterogeneous mixture

c)

compound

d)

pure substance

e)

solid

102.

Which one of the following is often separated into its components by simple techniques such as filtering ?

a)

heterogeneous mixture

b)

compounds

c)

elements

d)

solutions

103.

For which of the following, can the composition vary?

a)

pure substance

b)

element

c)

both homogeneous and heterogeneous mixtures

d)

homogeneous mixture

e)

heterogeneous mixture

104.

If matter is uniform throughout and cannot be separated into other substances by physical means, it is ________.

a)

a compound

b)

either an element or a compound

c)

a homogeneous mixture

d)

a heterogeneous mixture

e)

an element

105.

An element cannot ________.

a)

be part of a heterogeneous mixture

b)

be part of a homogeneous mixture

c)

be separated into other substances by chemical means

d)

interact with other elements to form compounds

e)

be a pure substance

106.

Which of the following is an illustration of the law of constant composition?

a)

Water boils at 100 °C at 1 atm pressure.

b)

Water is 11% hydrogen and 89% oxygen by mass.

c)

Water can be separated into other substances by a chemical process.

d)

Water and salt have different boiling points.

e)

Water is a compound.

107.

In the following list, only ________ is not an example of a chemical reaction.

a)

dissolution of a penny in nitric acid

b)

the condensation of water vapor

c)

a burning candle

d)

the formation of polyethylene from ethylene

e)

the rusting of iron

108.

Gases and liquids share the property of ________.

a)

compressibility

b)

definite volume

c)

incompressibility

d)

indefinite shape

e)

definite shape

109.

Of the following, only ________ is a chemical reaction.

a)

melting of lead

b)

dissolving sugar in water

c)

tarnishing of silver

d)

crushing of stone

e)

dropping a penny into a glass of water

110.

Which one of the following is not an intensive property?

a)

density

b)

temperature

c)

melting point

d)

mass

e)

boiling point

111.

Which one of the following is an intensive property?

a)

mass

b)

temperature

c)

length

d)

volume

e)

amount

112.

Of the following, only ________ is an extensive property.

a)

density

b)

volume

c)

boiling point

d)

freezing point

e)

temperature

113.

Which of the following are chemical processes? 1.  rusting of a nail 2.  freezing of water 3.  decomposition of water into hydrogen and oxygen gases 4.  compression of oxygen gas

a)

2, 3, 4

b)

1, 3, 4

c)

1, 3

d)

1, 2

e)

1, 4

114.

In the following list, only ________ is not an example of a chemical reaction.

a)

burning a plastic water bottle

b)

the production of hydrogen gas from water

c)

the tarnishing of a copper penny

d)

chopping a log into sawdust

e)

charging a cellular phone

115.

How many grams are in 10.20 X 10²³ molecules of magnesium nitride?

a)

1.011 x 10²³ g

b)

170.9 g

c)

6.142 x 10⁴⁷ g

d)

1.029 x 10²⁶ g

116.

How many molecules are in 2000 grams of cesium hydride?

a)

3.0 x 10⁵ molecules

b)

13.3 molecules

c)

8 x 10²⁴ molecules

d)

3 x 10⁻²¹

117.

Reaction Prediction:

Iron(III) Carbonate (heated)

(a)  

118.

Reaction Prediction:

Water plus dinitrogen pentoxide

(a)  

119.

Reaction prediction:

C6H14 + oxygen

(a)  

120.

Reaction Prediction:

sodium plus oxygen

(a)  

121.

Problem 1:

A compound is composed of 4.80 g of carbon and 0.400 g of hydrogen. The molar mass of the compound is 78.0 g.

What is the empirical formula of this compound?

(a)  

122.

Problem 1:

A compound is composed of 4.80 g of carbon and 0.400 g of hydrogen. The molar mass of the compound is 78.0 g.

What is the molecular formula of this compound?

(a)  

123.

Problem 2:

You have a 36.0 g sample of barium nitrate.

What is the percent composition of barium nitrate?

(a)  

124.

Problem 2:

You have a 36.0 g sample of barium nitrate.

How much of the 36.0 g sample is barium?

(a)  

125.

Problem 3:

 Iron (III) oxide can be prepared from a mixture of 0.76 moles of Iron and 0.76 moles of oxygen.  

What is the limiting reactant?

(a)  

126.

Problem 3:

 Iron (III) oxide can be prepared from a mixture of 0.76 moles of Iron and 0.76 moles of oxygen.  

How many moles of iron(III) oxide are produced?

(a)  

127.

Problem 3:

 Iron (III) oxide can be prepared from a mixture of 0.76 moles of Iron and 0.76 moles of oxygen.  

How many moles of the excess reactant are left over?

(a)  

128.

Problem 4:

Methane burns in oxygen to produce carbon dioxide and water in the following reaction: CH₄ + 2 O₂ → 2 H₂O + CO₂. 1000.g of CH₄ react with an excess of O₂ to produce 2300.g of CO₂?

What is the theoretical yield of CO₂?



(a)  

129.

Problem 4:

Methane burns in oxygen to produce carbon dioxide and water in the following reaction: CH₄ + 2 O₂ → 2 H₂O + CO₂. 1000.g of CH₄ react with an excess of O₂ to produce 2300.g of CO₂?

What is the percent yield of CO₂?

(a)  

130.

When the following equation is balanced, the coefficient of HNO3 is ________.

a)

1

b)

2

c)

3

d)

4

131.

When the following equation is balanced, the coefficient of oxygen is ________.

a)

1

b)

3

c)

2

d)

4

132.

When a hydrocarbon burns in air, the products produced are ________.

a)

oxygen and water

b)

carbon dioxide and water

c)

carbon dioxide and oxygen

d)

methane and water

133.

What type of reaction is the following reaction? Sulfur trioxide + water

a)

combination/synthesis

b)

decomposition

c)

combustion

134.

The reaction sulfur trioxide + water produces what product(s)

a)

sulfuric acid + oxygen

b)

sulfurous acid

c)

sulfuric acid

d)

sulfur hydroxide

135.

When lithium and flourine combine, the coefficients  of the flourine and the product are

a)

1,1

b)

2,1

c)

1,2

d)

2,2

136.

When the following equation is complete and balanced, the coefficient of water is ________.

K2O + H2O -->

a)

1

b)

2

c)

3

d)

4

137.

When calcium oxide and water combine the coefficients of calcium oxide and the product are

a)

1,1

b)

1,2

c)

2,1

d)

2,2

138.

When potassium chlorate decomposes, the coefficients of the products are

a)

2, 2

b)

1, 2

c)

2, 3

d)

3, 2

139.

When calcium hydroxide decomposes the products are

a)

calcium and water

b)

calcium oxide and oxygen

c)

calcium and oxygen

d)

calcium oxide and water

140.

When sulfuric acid decomposes the products are

a)

sulfur oxide and water

b)

sulfur trioxide and water

c)

sulfur dioxide and water

d)

disulfur pentoxide and water

141.

When dinitrogen pentoxide and water combine, the coefficient of the dinitrogen pentoxide is

a)

1

b)

2

c)

3

d)

4

142.

Which one of the following substances is the product of this combination reaction?

Al + I2 -->

a)

ALI2

b)

ALI

c)

AL3I

d)

ALI3

143.

When the following equation is balanced, the coefficients are ___________.

NH3 + O2 --> NO2 + H2O

a)

1, 1, 1, 1

b)

4, 7, 4, 6

c)

2, 3, 2, 3

d)

1, 3, 1, 2

144.

When the following hydrocarbon is burned, the coefficients of the reactants and products in the balanced chemical equation are  ________.

C10H22

a)

1, 16, 10, 11

b)

2, 31, 20, 22

c)

2, 25, 16, 18

d)

1, 4, 8, 9

145.

hen the following equation is balanced, the coefficients are ________.

Al(NO3)3 + Na2S --> Al2S3 + NaNO3

a)

2, 3, 1, 6

b)

2, 1, 3, 2

c)

1, 1, 1, 1

d)

4, 6, 3, 2

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