Chemical Composition and Properties of Matter – Assessment (Chapter 2 and 13)

In this assessment, questions are based on chemical composition, states and properties of matter, compounds and mixtures.

Name two categories used to classify properties of matter.

Intensive and Extensive

Explain why all samples of a substance have the same intensive properties

every sample of a substance have the same chemical composition

Why can samples of gold(Au) and copper (Cu) have the same extensive properties but not the same intensive properties?

Samples of gold and copper can have the same mass and volume(extensive properties), but have different intensive properties because they have different chemical composition

Name three states of matter

solid, liquid and gas

Describe the two categories use to classify physical changes

reversible and irreversible

Is the freezing of mercury(Hg) a reversible or irreversible physical change?

Reversible because solid mercury can be melted

Which property most easily distinguishes sodium chloride (NaCl) from the other solids in Table 2.1?

Color-sodium chloride is the only white solid on the table

How are liquids and solids alike?How are they different?

They are alike because they have definite volumes but different because a solid has a definite shape while a liquid has an indefinite shape

What physical properties could be used to separate iron filings(Fe) from table salt(NaCl)?

Iron is magnetic, salt is not magnetic; salt dissolves in water, iron will not dissolve in water.

How are mixtures classified?

homogeneous of heterogeneous

What type of properties can be used to separate mixtures?

differences in physical properties such as: particle size, phase , solubility, boiling point

Explain the term phase as it relates to homogeneous and heterogeneous mixtures.

A phase is any part of a sample, with a uniform composition. There is one phase in a homogeneous mixture and two or more in a heterogeneous mixture.

Classify each of the following as a homogeneous or heterogeneous mixture:Food Coloring, Ice cubes in liquid water, mouthwash, and mashed, un-peeled potatoes

homogeneous, heterogeneous, homogeneous, and heterogeneous

How are a substance and a solution similar? How are they different?

Both substances, and a solution have a uniform composition throughout. For differences, a substance has a definite composition where as a a solution has a variable composition

When would you use filtration to separate a mixture? When would you use distillation to separate a mixture?

in a heterogeneous mixture;to separate a liquid from substances dissolved into liquids

Describe a procedure that could separate a mixture of sand and table salt.

Add water to the mixture to dissolve the salt, filter the mixtures the sand will remain in the filter paper, the salt solution will pass through, evaporate the water from the salt solution to obtain the salt

Liquid A and Liquid B are clear liquids. They are placed in evaporating dishes and allowed to evaporate. When evaporation is complete, there is a white solid container B but no solid in container A. What can you infer about the two liquids?

Liquid A is probably a pure substance while liquid B is a mixture

How is compound different from an element?

Compounds can be broken down into simpler substances by chemical means, but elements cannot be broken down further

How can you distinguish a substance from a mixture>

a substance has a fixed composition, whereas the composition of a mixture may vary

What are chemical symbols and chemical formulas used for?

Chemical symbols represent elements, chemical formulas represent compounds

Name two methods that can be used to break down compounds into simpler substance.

heat, electric current

Classify each of these samples of matter as an element, compound, or mixture.
table sugar
tap water
cough syrup


Write the chemical symbol for each element


Name the chemical elements for each symbol: C, Ca, Fe, K, Au, Cu

carbon, calcium, iron, potassium, gold and copper

How does a chemical change affect the composition of matter?

the composition of matter always changes during a chemical change

Name four possible clues that a chemical change has taken place.

a transfer of energy, a change in color, the production of a gas and the formation of precipitate

In a chemical reaction, how does the mass of the reactants compare with the mass of the products?

the mass of the products is always equal to the mass of the reactants

What is the main difference between physical changes and chemical changes?

Physical change, the chemical composition of a substance does not change

Classify the following changes as physical changes or chemical changes.
Water boils
salt dissolves in water
milk turns sour
metal rusts


According to the law of conservation of mass, when is mass conserved?

mass is conserved in every physical change of chemical reaction

Hydrogen and oxygen react chemically to form water. How much water would form if 4.8 grams of hydrogen reacted with 38.4 grams of oxygen?

4.8 g hydrogen+ 38.4 g oxygen=43.2 g water

Briefly describe the assumptions of kinetic theory as applied to gases.

a gas is composed of tiny particles whose motion is rapid, constant, and random; collisions between particles are perfectly elastic

Use kinetic theory to explain what causes gas pressure.

Gas pressure is the result of simultaneous collisions of billions of rapidly moving particle with an object

how is the Kelvin temperature of a substance related to the average kinetic energy of its particles ?

The kelvin temperature is directly proportional to the average Kinetic energy of the particles

Convert the following pressures to kPa
45 mm Hg


By what factor does the average kinetic energy of the oxygen molecules in the cylinder decrease if a cylinder of oxygen gas is cooled from K(27 degrees Celsius) to 150 K (-124 degrees Celsius)

by one-half

What factors help determine the physical properties of liquids?

the interplay between the disruptive motions of particles in a liquid and the attractions among the particles

In terms of kinetic energy, explain how a molecule in a liquid evaporates.

a molecule with a certain minimum kinetic energy can escape from the surface of the liquid and vaporize

A liquid is in a closed container and has a constant vapor pressure. What is the relationship between the rate of evaporation of the liquid and the rate of condensation of the vapor in the container?

Rate of evaporation of the liquid equals the rate of condensation of the vapor

What conditions must exist for a liquid to boil?

particles throughout the liquid must have enough kinetic energy to vaporize

Use figure 13.9 to determine the boiling point of each liquid.
ethanoic acid at 27kPa
chloroform at 80 kPa
ethanol at 50 kPa

76 degree Celsius
52 degree Celsius
62 degree Celsius

Explain why the boiling point of a liquid varies with atmospheric pressure

Boiling occurs when the vapor pressure of a liquid equals the external pressure. If the atmospheric pressure changes, the boiling point will change

Explain how evaporation lowers the temperature of a liquid

When the molecules with the highest kinetic energy escape from the liquid, the average kinetic energy of the remaining particles is lower and the temperature decreases

In general, how are particles arranged in solids?

Particles in solids are packed tightly together in an orderly arrangement. The locations of the particles are fixed

What does the shape of a crystal tell you about the structure of a crystal?

The shape of a crystal reflects the arrangement of the particle within the solid

How do allotropes of an element differ?

Allotropes are different molecular forms of the same element in the same physical state

What phases are in equilibrium at a substance’s melting point?

solid and liquid

How do the melting points of ionic solids generally compare with those of molecular solids?Explain.

Ionic solids generally have, higher melting points than molecular solids

What is the difference between a crystal lattice and a unit cell?

a crystal lattice is a repeating array of unit cells