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Chemistry > Chemistry (Chapter 2) > Flashcards

Chemistry (Chapter 2) Flashcards

2
Q

S1) Mass

A

A measure of the amount of matter than an object contains; the SI base unit is the kilogram.

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3
Q

S1) Volume

A

A measure of the space occupied by a sample of matter.

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4
Q

S1) Extensive property

A

A property that depends on the amount of matter in a sample.

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5
Q

S1) Inextensive Property

A

A property that depends on the type of matter in a sample, not the amount of matter.

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6
Q

S1) Substance

A

Matter that has a uniform and definite composition; either an element or a compound; also called pure substance.

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7
Q

S1) Physical Property

A

A quality or condition of a substance that can be observed or measured without changing the substance’s composition.

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8
Q

S1) Solid

A

A form of matter that has definite shape and volume.

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9
Q

S1) Liquid

A

A form of matter that flows, has a fixed volume, and an indefinite shape.

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10
Q

S1) Gas

A

A form of matter that takes the shape and volume of its container; a gas has no definite shape or volume.

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11
Q

S1) Vapor

A

Describes the gaseous state of a substance that is generally a liquid or solid at room temperature.

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12
Q

S1) Physical Change

A

A change during which some properties of a material change but the composition of the material does not change.

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13
Q

S1) Physical changes can be classified as reversible or irreversible.

A

BLANK CARD

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14
Q

S1) Every sample of a given substance has identical intensive properties because every sample has the same composition.

A

S1) Three states of matter are solid, liquid, and gas.

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15
Q

S1) Explain why all samples of a given substance have the same intensive properties.

A

Because every sample has the same composition.

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16
Q

S1) Name the three states of matter:

A

Solid, liquid, and gas.

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17
Q

S1) Describe the two categories used to classify physical changes:

A

Reversible and irreversible.

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18
Q

S1) Name two categories used to classify properties of matter.

A

Extensive properties and intensive properties.

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19
Q

S1) Which property in the Physical Properties of Some Substances table can most easily distinguish sodium chloride from the other solids?

A

The color because it is the only one that is white.

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20
Q

S1) In what way are liquids and gases alike? In what ways are liquids and solids different?

A

They use shape and volume. They are different because liquids has an indefinite shape and flow and solids only take the shape and volume of its container.

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21
Q

S1) Is the freezing of mercury a reversible or irreversible physical change? Explain your answer.

A

Reversible. I say this because mercury is a solid and can be melted.

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22
Q

S1) Explain why samples of platinum and copper can have the same extensive properties but not the same intensive properties.

A

Because platinum and copper have different types of intensive properties which means that they have different chemical make-up.

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23
Q

S1) How would understanding the properties of matter be helpful in other fields of study besides chemistry?

A

It would be helpful to understand different kinds of properties.

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24
Q

S2) How are mixtures classified?

A

Mixtures are classified as heterogeneous mixtures or as homogeneous mixtures.

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25
Q

S2) What type of properties can be used to separate mixtures?

A

Differences in physical properties can be used to separate mixtures.

26
Q

S2) Explain the term phase as it relates to homogeneous and heterogeneous mixtures.

A

The term phase is used to describe any part of a sample with uniform composition and properties. A homogeneous mixture consists of a single phase. A heterogeneous mixture consists of two or more phases.

27
Q

S2) In general, what would you use filtration to separate a mixture? When would you use distillation to separate a mixture?

A

When you don’t want solid particles to pass through something; when you want to separate a solid and a liquid mixture. You would want to use distillation to separate a mixture when you want to separate components of the mixture.

28
Q

S2) How are a substance and a solution similar? How are they different?

A

A substance and a solution are similar because a substance can be anything and a solution is a liquid. They are different because a solution consists of solute that is dissolved in a solvent.

29
Q

S3) How is a compound different from an element?

A

Compounds can be broken down into simpler substances by chemical, elements cannot.

30
Q

S3) How can you distinguish a substance from a mixture?

A

If the composition of a material is fixed, the material is a substance. If the composition of a material may vary, the material is a mixture.

31
Q

S3) What are the chemical symbols and chemical formulas used for?

A

Symbols and chemical formulas are used to represent elements and components.

32
Q

S3) What makes the periodic table such a useful tool?

A

It allows you to easily compare the properties of one element to another element.

33
Q

S3) Name two methods that can be used to break down compounds into simpler substances:

A

Chemical process and physical process.

34
Q

S3) Name two elements that have properties similar to those of the element calcium (Ca).

A

Magnesium and Barium.

35
Q

S4) How does a chemical change affect the composition of matter?

A

The composition of matter always changes.

36
Q

S4) Name four possible clues that a chemical change has taken place:

A

A transfer of energy, a change in color, the production of a gas, or the formation of a precipitate.

37
Q

S4) In a chemical reaction, how does the mass of the reactants compare with the mass of the products?

A

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

38
Q

S4) What is the main difference between physical changes and chemical changes?

A

A chemical change affects the composition and it breaks down the bonds in reactants and formation of bonds in products.

39
Q

S4) According to the law of conservation of matter, when is mass conserved?

A

Mass is conserved when there is a physical change in the chemical reaction.

40
Q

S2) Mixture

A

A physical blend of two or more substances that are not chemically combined.

41
Q

S2) Heterogeneous Mixture

A

A mixture that is not uniform in composition; components are evenly distributed throughout the mixture.

42
Q

S2) Homogeneous Mixture

A

A mixture that is composition; components are evenly distributed and not easily distinguished.

43
Q

S2) Solution

A

A homogeneous mixture; consists of salutes dissolved in the solvent.

44
Q

S2) Phase

A

Any part of a sample with uniform composition and properties.

45
Q

S2) Filtration

A

A process that separates a solid from the liquid in a heterogeneous mixture.

46
Q

S2) Distillation

A

A process used to separate components of a mixture using differences in boiling points.

47
Q

S3) Element

A

The simplest form of matter that has a unique set of properties; an element cannot be broken down into simpler substances by chemical means.

48
Q

S3) Compound

A

A substance that contains two or more elements chemically combined in a fixed proportion.

49
Q

S3) Chemical Change

A

A change that produces matter with a different composition that than the original matter.

50
Q

S3) Chemical Symbol

A

A one or two letter representation of an element.

51
Q

S3) Periodic Table

A

An arrangement of elements in which the elements are separated into groups based on a set of repeating elements.

52
Q

S3) Period

A

A horizontal row of elements in the periodic table.

53
Q

S3) Group

A

A vertical column in the period table.

54
Q

S4) Chemical Change

A

The ability substance to undergo a specific chemical change.

55
Q

S4) Chemical Reaction

A

A change in which one or more reactants change into one or more products.

56
Q

S4) Reactant

A

A substance present at the start of a reaction.

57
Q

S4) Product

A

A substance produced in a chemical reaction.

58
Q

S4) Precipitate

A

A solid that forms and settles out a liquid mixture.

59
Q

S4) Law of Conservation of Mass

A

In any physical change or chemical reactions, mass is conserved; mass can be conserved; mass can neither created nor destroyed.

Chemistry (12 decks)

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