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Worksheets

7th session

Total questions: 70

Worksheet time: 35mins

Name
Class
Date
1.

Solids have a___shape and are not appreciably_____

a)

definite, compressible

b)

definite, incompressible

c)

indefinite, compressible

d)

indefinite, incompressible

2.

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

3.

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

a)

law

b)

theory

c)

hypothesis

d)

experiment

4.

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

a)

filtration

b)

solvation

c)

distillation

d)

chromatography

5.

The SI unit for mass is .

a)

kilogram

b)

gram

c)

pound

d)

troy ounce

6.

The freezing point of water at 1 atm pressure is

a)

0°F

b)

0 K

c)

0°C

d)

-273°C

7.

In the following list, only_____is not an example of matter.

a)

planets

b)

light

c)

dust

d)

elemental phosphorous

8.

What is the physical state in which matter has no specific shape but does have a specific volume?

a)

gas

b)

solid

c)

liquid

d)

salts

9.

The law of constant composition applies to .

a)

solutions

b)

heterogeneous mixtures

c)

compounds

d)

homogeneous mixtures

10.

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

a)

homogeneous mixture

b)

heterogeneous mixture

c)

compound

d)

pure substance

11.

Which one of the following is a pure substance?

a)

concrete

b)

wood

c)

salt water

d)

elemental copper

12.

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

a)

heterogeneous mixture

b)

compounds

c)

homogeneous mixture

d)

elements

13.

Which states of matter are significantly compressible?

a)

gases only

b)

liquids only

c)

solids only

d)

liquids and gases

14.

Homogeneous mixtures are also known as

a)

solids

b)

compounds

c)

elements

d)

solutions

15.

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

16.

Gases and liquids share the property of

a)

compressibility

b)

definite volume

c)

incompressibility

d)

indefinite shape

17.

Which one of the following is not an intensive property?

a)

density

b)

temperature

c)

melting point

d)

mass

18.

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

19.

________and______reside in the atomic nucleus.

a)

Protons, electrons

b)

Electrons, neutrons

c)

Protons, neutrons

d)

none of the above

20.

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

21.

In the periodic table, the rows are called____ and the columns are called_____ .

a)

octaves, groups

b)

staffs, families

c)

periods, groups

d)

cogeners, families

22.

are found uncombined, as monatomic species in nature.

a)

Noble gases

b)

Chalcogens

c)

Alkali metals

d)

Alkaline earth metals

23.

When a metal and a nonmetal react, the_____tends to lose electrons and the______tends to gain electrons.

a)

metal, metal

b)

nonmetal, nonmetal

c)

metal, nonmetal

d)

nonmetal, metal

24.

Potassium forms an ion with a charge of .

a)

+2

b)

-1

c)

+1

d)

-2

25.

The name of the binary compound N2O4 is .

a)

nitrogen oxide

b)

nitrous oxide

c)

nitrogen(III) oxide

d)

dinitrogen tetroxide

26.

What is the molecular formula for propane?

a)

C2H8

b)

C3H6

c)

C3H8

d)

C4H8

27.

The charge on an electron was determined in the

a)

cathode ray tube, by J. J. Thompson

b)

Rutherford gold foil experiment

c)

Millikan oil drop experiment

d)

Dalton atomic theory

28.

________-rays consist of fast-moving electrons.

a)

alpha

b)

beta

c)

gamma

d)

X

29.

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 Thompson's model of the atom

d)

utilized the deflection of beta particles by gold foil

30.

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

a)

neutron

b)

proton

c)

electron

d)

nucleus

31.

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

32.

Which one of the following basic forces is so small that it has no chemical significance?

a)

weak nuclear force

b)

strong nuclear force

c)

electromagnetism

d)

gravity

33.

Which type of formula provides the most information about a compound?

a)

empirical

b)

molecular

c)

simplest

d)

structural

34.

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 isotope of each element in a compound

35.

A strong electrolyte is one that completely in solution.

a)

reacts

b)

decomposes

c)

disappears

d)

ionizes

36.

A neutralization reaction between an acid and a metal hydroxide produces

a)

water and a salt

b)

hydrogen gas

c)

oxygen gas

d)

sodium hydroxide

37.

Oxidation is the______and reduction is the_________

a)

gain of oxygen, loss of electrons

b)

loss of oxygen, gain of electrons

c)

loss of electrons, gain of electrons

d)

gain of oxygen, loss of mass

38.

Which one of the following is a correct expression for molarity?

a)

mol solute/L solvent

b)

mol solute/mL solvent

c)

mmol solute/mL solution

d)

mol solute/kg solvent

39.

The point in a titration at which the indicator changes is called the

a)

equivalence point

b)

indicator point

c)

standard point

d)

endpoint

40.

is an oxidation reaction.

a)

Ice melting in a soft drink

b)

Table salt dissolving in water for cooking vegetables

c)

Rusting of iron

d)

Neutralization of HCl by NaOH

41.

Which one of the following is an exothermic process?

a)

ice melting

b)

water evaporating

c)

boiling soup

d)

condensation of water vapor

42.

In the Bohr model of the atom,

a)

electrons travel in circular paths called orbitals

b)

electrons can have any energy

c)

electron energies are quantized

d)

electron paths are controlled by probability

43.

is credited with developing the concept of atomic numbers.

a)

Dmitri Mendeleev

b)

Lothar Meyer

c)

Henry Moseley

d)

Ernest Rutherford

44.

is a unique element and does not truly belong to any family.

a)

Nitrogen

b)

Radium

c)

Hydrogen

d)

Uranium

45.

What is the maximum number of double bonds that a carbon atom can form?

a)

4

b)

1

c)

0

d)

2

46.

According to Lewis theory, a Lewis acid is a species that can:

a)

Increase in entropy

b)

Donation of a proton

c)

Donation of an electron pair

d)

Acceptance of an electron pair

47.

Which group of elements on the periodic table is characterized by having a full valence electron shell, making them very stable?

a)

Alkali metals

b)

Alkaline earth metals

c)

Halogens

d)

Noble gases

48.

The process by which a solid changes directly into a gas without first becoming a liquid is called:

a)

Evaporation

b)

Condensation

c)

Sublimation

d)

Melting

49.

Which method would be most effective to separate sand from a mixture of sand and water?

a)

Chromatography

b)

Evaporation

c)

Filtration

d)

Distillation

50.

The ability of an atom in a molecule to attract electrons is best quantified by the

a)

paramagnetism

b)

diamagnetism

c)

electronegativity

d)

electron change- to-mass ratio

51.

A pressure of 1.00 atm is the same as a pressure of of mmHg.

a)

193

b)

101

c)

760.0

d)

29.92

52.

Gaseous mixtures

a)

can only contain molecules

b)

are all heterogeneous

c)

can only contain isolated atoms

d)

are all homogeneous

53.

The first person to investigate the relationship between the pressure of a gas and its volume was

a)

Amadeo Avogadro

b)

Lord Kelvin

c)

Jacques Charles

d)

Robert Boyle

54.

_____solids consist of atoms or molecules held together by dipole-dipole forces, London disperson forces, and/or hydrogen bonds.

a)

Ionic

b)

Molecular

c)

Metallic

d)

Covalent- network

55.

Crystalline solids___

a)

have their particles arranged randomly

b)

have highly ordered structures

c)

are usually very soft

d)

exist only at high temperatures

56.

The process of solute particles being surrounded by solvent particles is known as

a)

salutation

b)

agglomeration

c)

solvation

d)

agglutination

57.

Pairs of liquids that will mix in all proportions are called_____liquids.

a)

miscible

b)

unsaturated

c)

polar liquids

d)

saturated

58.

The phrase "like dissolves like" refers to the fact that____.

a)

gases can only dissolve other gases

b)

polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes

c)

solvents can only dissolve solutes of similar molar mass

d)

condensed phases can only dissolve other condensed phases

59.

When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are best described as a case of.

a)

hydration

b)

supersaturation

c)

crystallization

d)

dehydration

60.

A saturated solution____.

a)

contains as much solvent as it can hold

b)

contains no double bonds

c)

contains dissolved solute in equilibrium with undissolved solid

d)

will rapidly precipitate if a seed crystal is added

61.

Pressure has an appreciable effect on the solubility of______in liquids.

a)

gases

b)

solids

c)

liquids

d)

salts

62.

The process of a substance sticking to the surface of another is called

a)

absorption

b)

diffusion

c)

effusion

d)

adsorption

63.

Which of the following is not a colloid?

a)

air

b)

fog

c)

smoke

d)

whipped cream

64.

Of the following, will lower the activation energy for a reaction.

a)

increasing the concentrations of reactants

b)

raising the temperature of the reaction

c)

adding a catalyst for the reaction

d)

removing products as the reaction proceeds

65.

At equilibrium,_____

a)

all chemical reactions have ceased

b)

the rates of the forward and reverse reactions are equal

c)

the rate constants of the forward and reverse reactions are equal

d)

the value of the equilibrium constant is 1

66.

A substance that is capable of acting as both an acid and as a base is.

a)

autosomal

b)

conjugated

c)

amphoteric

d)

saturated

67.

The most common isotope of hydrogen is sometimes referred to as.

a)

deuterium

b)

protium

c)

tritium

d)

heavy hydrogen

68.

In_______. the bonds are the same but the spatial arrangement of the atoms is different.

a)

structural isomers

b)

linkage isomers

c)

coordination- sphere isomers

d)

stereo isomers

69.

A geometrical isomer with like groups located on opposite sides of the metal atom is denoted with the prefix____

a)

cis-

b)

trans-

c)

bis-

d)

tetrakis

70.

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

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