Free Printable Chemistry final test chap 1+2

1.

Solids have a __________ shape and are not appreciably __________.

a)

definite, compressible

b)

definite, incompressible

c)

indefinite, compressible

d)

indefinite, incompressible

e)

sharp, convertible

2.

__________ is the chemical symbol for elemental sodium.

a)

S

b)

W

c)

So

d)

Na

e)

Sn

3.

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

a)

heterogeneous mixture

b)

element

c)

homogeneous mixture

d)

compound

e)

mixture of elements

4.

The symbol for the element potassium is __________.

a)

Pt

b)

P

c)

K

d)

S

e)

Ca

5.

The symbol for the element magnesium is __________.

a)

Rb

b)

Mn

c)

Ne

d)

Si

e)

Mg

6.

The initial or tentative explanation of an observation is called a(n) __________.

a)

law

b)

theory

c)

hypothesis

d)

experiment

e)

test

7.

A concise verbal statement or mathematical equation that summarizes a broad variety of observations and experiences is called a(n) __________.

a)

law

b)

theory

c)

hypothesis

d)

experiment

e)

test

8.

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

a)

filtration

b)

solvation

c)

distillation

d)

chromatography

e)

all of the above are correct

9.

The SI unit for mass is __________.

a)

kilogram

b)

gram

c)

pound

d)

troy ounce

e)

none of the above

10.

A one degree of temperature difference is the smallest on the __________ temperature scale.

a)

Kelvin

b)

Celsius

c)

Fahrenheit

d)

Kelvin and Celsius

e)

Fahrenheit and Celsius

11.

A common English set of units for expressing velocity is miles/hour. The SI unit for velocity is __________?

a)

km/hr

b)

km/s

c)

m/hr

d)

m/s

e)

cm/s

12.

The SI unit of temperature is __________.

a)

K

b)

°C

c)

°F

d)

t

e)

T

13.

The temperature of 25°C is __________ in Kelvins.

a)

103

b)

138

c)

166

d)

248

e)

298

14.

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

a)

0°F

b)

0 K

c)

0°C

d)

-273°C

e)

-32°F

15.

A temperature of 400 K is the same as __________°F.

a)

261

b)

286

c)

88

d)

103

e)

127

16.

1 kilogram = __________ milligrams

a)

1 × 10−6

b)

1,000

c)

10,000

d)

1,000,000

e)

none of the above

17.

An object will sink in a liquid if the density of the object is greater than that of the liquid. The mass of a sphere is 9.83 g. If the volume of this sphere is less than __________ cm3 , then the sphere will sink in liquid mercury (density = 13.6 g/cm3 ).

a)

0.723

b)

1.38

c)

134

d)

7.48

e)

none of the above

18.

The density of silver is 10.5 g/cm3 . A piece of silver that occupies a volume of 23.6 cm3 would have a mass of __________g.

a)

0.445

b)

2.25

c)

112

d)

23.6

e)

248

19.

1. The density of mercury is 13.6 g/cm3 . The density of mercury is __________ kg/m3 .

a)

1.36 × 10^-2

b)

1.36 × 10^4

c)

1.36 × 10^8

d)

1.36 × 10^-5

e)

1.36 × 10^-4

20.

1. The law of constant composition applies to __________.

a)

solutions

b)

heterogeneous mixtures

c)

compounds

d)

homogeneous mixtures

e)

solids

21.

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

a)

P, potassium

b)

C, copper

c)

Mg, manganese

d)

Ag, silver

e)

Sn, silicon

22.

Which one of the following is a pure substance?

a)

concrete

b)

wood

c)

salt water

d)

elemental copper

e)

milk

23.

1. 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 homogeneous mixture is always the same

e)

that the composition of a heterogeneous mixture is always the same

24.

1. Which one of the following is not an intensive property?

a)

density

b)

temperature

c)

melting point

d)

mass

e)

boiling point

25.

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

26.

1. If an object is accelerating at a rate of 25 m/s2 , how fast will it be moving (in m/s) after 1.50 min? (Assume an initial velocity of zero.)

a)

17

b)

3.6

c)

38

d)

2.3 × 10^3

e)

0.060

27.

One angstrom, symbolized Å, is 10^-10m. 1 cm^3 = __________ Å^3

a)

10^−24

b)

10^30

c)

10^−30

d)

10^−9

28.

The width, length, and height of a large, custom-made shipping crate are 1.22 m, 3.22 m, and 0.83 m, respectively. The volume of the box using the correct number of significant figures is __________ m3 .

a)

3.26057

b)

3.3

c)

3.26

d)

3.261

e)

3.2606

29.

The density of air under ordinary conditions at 25°C is 1.19 g/L. How many kilograms of air is in a room that measures 11.0 ft × 11.0 ft and has an 10.0 ft ceiling? 1 in. = 2.54 cm. (exactly); 1 L = 103cm3

a)

3.66

b)

0.152

c)

4.08 × 104

d)

0.0962

e)

40.8

30.

1. What is the volume (in cm3) of a 63.4 g piece of metal with a density of 12.86 g/cm3?

a)

4.93

b)

19.5

c)

.425

d)

6.65

e)

none of the above

31.

A certain mass of carbon reacts with 13.6 g of oxygen to form carbon monoxide. __________ grams of oxygen would react with that same mass of carbon to form carbon dioxide, according to the law of multiple proportions?

a)

25.6

b)

6.8

c)

13.6

d)

136

e)

27.2

32.

Methane and ethane are both made up of carbon and hydrogen. In methane, there are 12.0 g of carbon for every 4.00 g of hydrogen, a ratio of 3:1 by mass. In ethane, there are 24.0 g of carbon for every 6.00 g of hydrogen, a ratio of 4:1 by mass. This is a statement of the law of

a)

constant composition

b)

multiple proportions

c)

conservation of matter

d)

conservation of mass

e)

octaves

33.

1. __________ and __________ reside in the atomic nucleus.

a)

Protons, electrons

b)

Electrons, neutrons

c)

Protons, neutrons

d)

none of the above

e)

Neutrons, only neutrons

34.

1. 200 pm is the same as __________

a)

2000

b)

20

c)

200

d)

2

e)

2 × 10-12

35.

1. The atomic number indicates __________.

a)

the number of neutrons in a nucleus

b)

the total number of neutrons and protons in a nucleus

c)

the number of protons or electrons in a neutral atom

d)

the number of atoms in 1 g of an element

e)

the number of different isotopes of an element

36.

1. Which group in the periodic table contains only nonmetals?

a)

1A

b)

6A

c)

2B

d)

2A

e)

8A

37.

1. Horizontal rows of the periodic table are known as __________.

a)

periods

b)

groups

c)

metalloids

d)

metals

e)

nonmetals

38.

Vertical columns of the periodic table are known as __________.

a)

metals

b)

periods

c)

nonmetals

d)

groups

e)

metalloids

39.

1. Elements in Group 1A are known as the __________.

a)

chalcogens

b)

alkaline earth metals

c)

alkali metals

d)

halogens

e)

noble gases

40.

1. Elements in Group 2A are known as the __________.

a)

alkaline earth metals

b)

alkali metals

c)

chalcogens

d)

halogens

e)

noble gases

41.

1. Elements in Group 6A are known as the __________.

a)

alkali metals

b)

chalcogens

c)

alkaline earth metals

d)

halogens

e)

noble gases

42.

1. Elements in Group 7A are known as the __________.

a)

chalcogens

b)

alkali metals

c)

alkaline earth metals

d)

halogens

e)

noble gases

43.

1. Elements in Group 8A are known as the __________.

a)

halogens

b)

alkali metals

c)

alkaline earth metals

d)

chalcogens

e)

noble gases

44.

1. Oxygen is a __________ and nitrogen is a __________.

a)

metal, metalloid

b)

nonmetal, metal

c)

metalloid, metalloid

d)

nonmetal, nonmetal

e)

nonmetal, metalloid

45.

1. Calcium is a __________ and silver is a __________.

a)

nonmetal, metal

b)

metal, metal

c)

metalloid, metal

d)

metal, metalloid

e)

nonmetal, metalloid

46.

1. __________ are found uncombined, as monatomic species in nature.

a)

Noble gases

b)

Chalcogens

c)

Alkali metals

d)

Alkaline earth metals

e)

Halogens

47.

1. The formula of a salt is XCl2 . The X-ion in this salt has 28 electrons. The metal X is __________.

a)

Ni

b)

Zn

c)

Fe

d)

V

e)

Pd

48.

1. Sodium forms an ion with a charge of __________.

a)

+1

b)

-1

c)

+2

d)

-2

e)

0

49.

1. Calcium forms an ion with a charge of __________.

a)

-1

b)

-2

c)

+1

d)

+2

e)

0

50.

1. Fluorine forms an ion with a charge of __________.

a)

-1

b)

+1

c)

+2

d)

+3

e)

-3

51.

1. Oxygen forms an ion with a charge of __________.

a)

-2

b)

+2

c)

-3

d)

+3

e)

+6

52.

1. Predict the empirical formula of the ionic compound that forms from magnesium and oxygen.

a)

Mg2O

b)

MgO

c)

MgO2

d)

Mg2O2

e)

Mg3O2

53.

1. Predict the empirical formula of the ionic compound that forms from aluminum and oxygen.

a)

AlO

b)

Al3O2

c)

Al2O3

d)

AlO2

e)

Al2O

54.

1. The correct name for N2O5 is __________.

a)

nitrous oxide

b)

nitrogen pentoxide

c)

dinitrogen pentoxide

d)

nitric oxide

e)

nitrogen oxide

55.

1. The formula of bromic acid is __________.

a)

HBr

b)

HBrO4

c)

HBrO

d)

HBrO3

e)

HBrO2

56.

1. Element M reacts with fluorine to form an ionic compound with the formula MF₃ . The M-ion has 18 electrons. Element M is __________.

a)

P

b)

Sc

c)

Ar

d)

Ca

e)

Cr

57.

1. What is the molecular formula for propane __________?

a)

C2H8

b)

C3H6

c)

C3H8

d)

C4H8

e)

C4H10

58.

1. What is the molecular formula for heptane __________?

a)

C6H12

b)

C6H14

c)

C7H14

d)

C7H16

e)

C7H18

59.

1. Which one of the following is not one of the postulates of Dalton's atomic theory?

a)

Atoms are composed of protons, neutrons, and electrons.

b)

All atoms of a given element are identical; the atoms of different elements are different and have different properties.

c)

Atoms of an element are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions.

d)

Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms.

e)

Each element is composed of extremely small particles called atoms.

60.

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 valid?

a)

(i) and (ii)

b)

(ii) only

c)

(ii) and (iii)

d)

(iii) only

e)

(iii) and (iv)

61.

1. Which isotope has 45 neutrons?

a)

80 Kr 36

b)

80 Br 35

c)

78 Se 34

d)

34 Cl 17

e)

103 Rh 45

62.

1. Isotopes are atoms that have the same number of _________ but differing number of __________.

a)

protons, electrons

b)

neutrons, protons

c)

protons, neutrons

d)

electrons, protons

e)

neutrons, electrons

63.

1. The nucleus of an atom does not contain __________.

a)

protons

b)

protons or neutrons

c)

neutrons

d)

subatomic particles

e)

electrons

64.

1. Different isotopes of a particular element contain the same number of __________.

a)

protons

b)

neutrons

c)

protons and neutrons

d)

protons, neutrons, and electrons

e)

subatomic particles

65.

1. Different isotopes of a particular element contain different numbers of __________.

a)

protons

b)

neutrons

c)

protons and neutrons

d)

protons, neutrons, and electrons

e)

None of the above is correct.

66.

1. In the symbol below, x = __________. x C 6

a)

19

b)

13

c)

6

d)

7

e)

not enough information to determine

67.

1. 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

e)

helium

68.

The elements in groups 1A, 6A, and 7A are called, __________, respectively

a)

alkaline earth metals, halogens, and chalcogens

b)

alkali metals, chalcogens, and halogens

c)

alkali metals, halogens, and noble gases

d)

alkaline earth metals, transition metals, and halogens

e)

halogens, transition metals, and alkali metals

69.

1. Which one of the following does not occur as diatomic molecules in elemental form?

a)

oxygen

b)

nitrogen

c)

sulfur

d)

hydrogen

e)

bromine

70.

1. Which compounds do not have the same empirical formula?

a)

C2H2,C6H6

b)

CO, CO2

c)

C2H4,C3H6

d)

C2H4O2,C6H12O6

e)

C2H5COOCH3, CH3CHO

Chemistry final test chap 1+2

Total questions: 70

Worksheet time: 2hrs 20mins

Similar Resources on Wayground