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Chemistry > Chapter 2 (Matter) > Flashcards

Chapter 2 (Matter) Flashcards

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0
Q

Mixtures

A

Composed of more than one substance and can be physically separated into its component substances.
Two types:
1. Homogenous mixtures
2. Heterogenous mixtures

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1
Q

Matter

A

Any substance that has a mass and occupies volume.
Can be divided into two classes:
1. Mixtures
2. Pure substance

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2
Q

Pure substance

A 
Composed of one substance and CANT be physically separated. 
Has constant composition 
Two types:
1. Compounds 
2. Elements
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3
Q

Compounds

A

Can be chemically separated into individual elements

water -h2o- separated into hydrogen and oxygen

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4
Q

Elements

A

A single atom
Cannot be broken down any further by chemical reactions and still retain same properties
(Gold, iron, oxygen)

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5
Q

Homogenous mixtures

Ex: apple juice

A

Uniform properties through out.
Also called solutions; evenly mixed
(Ex: salt dissolved into water)

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6
Q

Heterogenous mixtures

Ex: blood

A

NO uniform properties; visible

Ex: sand & water

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7
Q

Atom

A

Basic building block of all matter

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8
Q

Molecule

A

Smallest particle of a compound

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9
Q

Law of constant composition

A

The ration by mass of the elements in a compound is always the same.

-Compounds have a constant composition, mixtures do NOT (can be used to differentiate b/w the two)

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10
Q

Colloid

A

A heterogenous mixture whose particle size in intermediate between those of a solution and a suspension

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11
Q

Law of definite proportions

A

States that compounds always contain the same elements in a constant proportion by mass.

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12
Q

Chemical formula

A

Sulfuric –> H2SO4

Number of types of atoms in a compound

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13
Q

Dispersion Medium

A

The material in which the particles are distributed

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14
Q

Tyndall effect

A

Phenomenon in which the dispersed particles of a colloid cannot be separated by filteration but scattered by light
– chattering of visible light by colloidal particles

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15
Q

Emulsions

A

A colloidal dispersion of a liquid or solid

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16
Q

Physical property

A

Observed without changing the identity of a substance

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17
Q

Chemical property

A

Observed when a substance is changed into a new substance

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18
Q

Physical changes

A

Changes that do NOT alter the identity of a substance.
; (separation of mixtures, physical deformation like cutting, denting, & stretching)
; (changes of state)

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19
Q

Chemical changes

A

One substance turned into another.

Ex: burning paper

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20
Q

Solid

A

Has a definite shape and volume

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21
Q

Liquid

A

Definite volume, but indefinite shape

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22
Q

Gas

A

No definite shape, no definite volume

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23
Q

Distillation

A

For two or more pure liquids
Vaporized, condensed, isolated
Takes advantage of differences in boiling points

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24
Q

Evaporation

A

Removes a liquid from a solution to leave a solid material

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25
Q

Filtration

A

Separates solids of different sizes

Separates pure substances

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26
Q

Calorimeter

A
  • device used to measure changes in thermal energy or heat transfer
  • It measures calories
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27
Q

Calorie

A

the amount of energy required to raise one gram of water by one degree Celsius.

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28
Q

Calorimetry

A

A way to measure the energy change of a reaction or the energy contained in matter

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29
Q

Another example of a physical change

A

Ice melting and then water boiling

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30
Q

Silicon is a

A

Metalloid

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31
Q

Liquid state

A

No definite shape, but definite volume

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32
Q

The greater the kinetic energy the

A

Higher the temperature of particles

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33
Q

A heterogenous mixture example

A

Chocolate chop cookie

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34
Q

What is he method used to obtain pure water from contaminated water?

A

Distillation

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35
Q

A nonmetal is usually

A

Brittle

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36
Q

The vertical columns on period tables are

A

Groups

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37
Q

Example of homogenous mixture

A

Clear air

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38
Q

Metalloids are often

A

Semiconductors of electricity

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39
Q

What happens to energy in a substance when it changes state ?

A

Neither increased nor destroyed, but changes form

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40
Q

Method used to separate water form sand?

A

Filtration

41
Q

Chemical defined as

A

Any substance that has a definite composition

42
Q

A substance is metal if it’s

A

A good conductor of heat and electricity

43
Q

Chemical change

A

New identity

44
Q

Zinc is a

A

Metal

45
Q

When there are particles that settle in a mixture it’s called

A

Suspension

46
Q

Another example of a physical change

A

Ice melting and then water boiling

47
Q

Silicon is a

A

Metalloid

48
Q

Liquid state

A

No definite shape, but definite volume

49
Q

The greater the kinetic energy the

A

Higher the temperature of particles

50
Q

A heterogenous mixture example

A

Chocolate chop cookie

51
Q

What is he method used to obtain pure water from contaminated water?

A

Distillation

52
Q

A nonmetal is usually

A

Brittle

53
Q

The vertical columns on period tables are

A

Groups

54
Q

Example of homogenous mixture

A

Clear air

55
Q

Metalloids are often

A

Semiconductors of electricity

56
Q

What happens to energy in a substance when it changes state ?

A

Neither increased nor destroyed, but changes form

57
Q

Method used to separate water form sand?

A

Filtration

58
Q

Chemical defined as

A

Any substance that has a definite composition

59
Q

A substance is metal if it’s

A

A good conductor of heat and electricity

60
Q

Chemical change

A

New identity

61
Q

Zinc is a

A

Metal

62
Q

When there are particles that settle in a mixture it’s called

A

Suspension

63
Q

Kinetic energy

A

Any form of energy that cannot be stored

64
Q

Thermal energy

A

Total mechanical energy of an objects or a materials particles
Extensive property

65
Q

Temperature

A

Average mechanical energy of the particles that compose a material

66
Q

Kinetic molecular theory

A

Explains what happened to matter when the kinetic energy of particles changes
Key points:
1. All matter is made up of tiny particles
2. There is empty space between particles
3. Particles are always moving
4. Particles move because of energy

67
Q

Evaporation (vaporization)
Condensation
Sublimation
Deposition

A

Liquid to gas
Gas to liquid
Solid to gas
Gas to solid

68
Q

Vapor

A

Gas formed by a substance that boils above room temperature

69
Q

Volatile substances

A

Substances that readily evaporate or evaporate at high rates

70
Q

Heat of fusion

A

The amount of heat required to melt a specific amount of a substance at its melting point

71
Q

Potential energy

A

Stored energy

72
Q

Heat of vaporization

A

The amount of heat required to evaporate a specified amount of a substance at its boiling point

73
Q

Heat of formation

A

The heat released when a substance is formed from its elements (J/g)

74
Q

Heat of combustion

A

The heat released when a specified amount of a substance undergoes complete combustion with oxygen

75
Q

Alloys

A

Mixtures containing metals

76
Q

Binary compound

A

Composed of only two elements

77
Q

Ion & ionic bond

A

Charged atom & the bond attraction b/w oppositely charged ions

78
Q

Molecular compound

A

Any compound with a nonmetal (NM+NM) except for any containing ammonia (ionic)

79
Q

Covalent bond

A

A shared pair of valence electrons that holds two atoms together

80
Q

Acid

A

A special type of molecular compound ..

81
Q

Base

A

A hydroxide

82
Q

Salt

A

An ionic compound other than a hydroxide

83
Q

Two types of Ionic compounds

A

Salts and bases

84
Q

Two types of Homogeneous mixtures

A

Solutions and colloids

85
Q

Physical separations

A 
Those not involving a chemical reaction
Centrifugation
Chromatography
Distillation
Filtration
86
Q

Non-mechanical physical separation

A

Includes techniques that use heat, electricity, magnetism, dissolving etc

87
Q

Mechanical means of separation

A

Gravity, contact forces, or motion to sort the components of a mixture

88
Q

Sediment

A

To fall or sink to the bottom of a liquid

Matter that has called or sunk to the bottom of a liquid

89
Q

Is there such thing as a charged compound?

A

No, all compounds are neutral

90
Q

Multivalvent ions

A

Ions that have more than one valence shell electron. Many of the transitions metals do.
Ex) fe3+ fe2+

91
Q

Polyatomic ion

A

A charged group of covalently bonded atoms (like a molecule, except with a charge)

92
Q

To determine the names of ionic compounds

A
  1. Write the names of the possible ions

2. Write the formulas to see which one is correct

93
Q

You only use prefixes when you are naming which type of compound?

A

Binary Molecular compounds (two nonmetals), never ionic

Ex) xenon tetra fluoride –> XeFe4

94
Q

The names if all binary compounds have a suffix of what?

Do we use the prefix “mono” for the first element?

A

-ide

No, “Mono” is understood for the first element, so it is not needed.

95
Q

Hydrates

A

a compound (salts), typically a crystalline one, in which water molecules are chemically bound to another compound or an element.

96
Q

Gently warming a hydrated salt will usually…

A

Remove the water from the crystal

97
Q

Anhydrous

A

Refers to the form of a salt without water

98
Q

Some salts are hygroscopic which means..

A

They can absorb water from the air to form hydrates

99
Q

How to determine the formula of a hydrate from its name

A
  1. Write the sum hold of the ions named
  2. Combine the ions to form the equation
  3. Tack on the appropriate number of water molecules to compensate the formala

Ex) copper(II) sulphate heptahydrate

Cu2+ SO4 2- —> CuSO4
Heptahydrate—> 7H2O
So: CuSo4 * 7H2O

100
Q

To name an acid without an oxygen atom

A

“Hydro”(proceeds the name of the anion) & “-ic” (replaces -ide)

Ex) HF (hydrogen fluoride) = hydroflouric acid
HCN (hydrogen cyanide) = hydrocyanic acid

101
Q

To name an acid with an oxygen atom

A

“-ic” replaces “-ate” ex) hydrogen sulfate (h2so4) is sulfuric acid
“-ous” replaces “-ite” ex) hydrogen sulfite (h2so3) is sulfurous acid

Chemistry (7 decks)

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