Chem 11 - Chapter 2.1

Front 1

chemistry concerns with

Back 1

matters properties, composition, and behavior

Front 2

matter is

Back 2

anything that has mass and occupies space

Front 3

mass is the amount

Back 3

of matter contained in a thing

Front 4

usually the mass of common things is measured in

Back 4

grams or kilograms

Front 5

define properties

Back 5

qualities of a thing, especially those qualities common to a group of things

Front 6

extensive properties

Back 6

qualities that are or depends on the amount o the material

example) mass, volume, electrical resistance of a copper wire (depends on diameter and length)

flexibility of a metal sheet (depends on its thickness)

Front 7

intensive properties

Back 7

qualities that do not depends on the amount of the material

example) melting point, density, temperature, concentration, tension

Front 8

golds melting point and density are two

intensive properties

Back 8

that can be used to identify samples

Front 9

properties depends on

Back 9

material

Front 10

physical properties

Back 10

describe physical changes, which are changes of state or form

Front 11

physical changes also describe

Back 11

physical characteristics of a material

Front 12

chemical properties desbribe

Back 12

chemical changes

chemical changes are those in which a new substance or species

Front 13

chemical properties also describe the tendency

Back 13

of a chemical to react

Front 14

chemical properties describe

Back 14

the relationships or interactions between different forms of matter

Front 15

chemical properties include

Back 15

chemical's stability, its reactivity with other chemicals, its toxicity, and its flammability

Front 16

physical properties also describe the

Back 16

relationships or interactions between matter and energy

Front 17

physical changes involve

Back 17

the rearrangement of a material's own particles

Front 18

chemical changes involve the

Back 18

reorganization of two or more substances' atoms in relation to each other

Front 19

physical properties depend solely

Back 19

on the relationship between the materials owm particles

Front 20

chemical properties depend

Back 20

on the difference between the atom's current relationship and other atoms new relationships with different atoms

Front 21

kinetic energy

Back 21

any form of energy that cannot be stored

Front 22

the particles of matter posses a type of kinetic energy called

Back 22

mechanical energy due to their continuous movement

Front 23

independent atoms have three types of mechanical energy/motion:

Back 23

translational (movement from place to place)

rational (movement about an axis)

vibrational (a repetitive back and forth motion)

Front 24

thermal energy

Back 24

total mechanical energy of an objects or a materials particles

- also a extensive property

Front 25

temperature

Back 25

average mechanical energy of a particle that compose a material

- intensive property

Front 26

increase in materials temperature indicates

Back 26

average speed of the particles has increased

Front 27

heat

Back 27

energy transferred from one body to another because of a difference in temperature

Front 28

catch 22

Back 28

thermometer cannot measure the temperature without altering it

Front 29

operational definition

Back 29

consists of observable characteristics that help us classify things as belonging or not belonging to the defined group

Front 30

conceptual definitions

Back 30

explain what operational definitions describe

Front 31

kinetic molecular theory exaplins

Back 31

what happens to matter when the kinetic energy of particles changes

Front 32

kinetic molecular theory key points

Back 32

- all matter made up of tiny particles

- there is empty space between particles

- particles are always moving. their freedom to move depends on whether they are in a solid, liquid, or gas

- the particles move because of energy. the amount of energy particles have determine how fast the particles move and how much or far they move

Front 33

solid conceptual definiton

Back 33

- each particle bounces around pushing the ones surrounding it outward

- the particles have not spread far enough apart for any particle to fit in the gap between the particles surrounding it so the structure remains intact

Front 34

liquid conceptual definition

Back 34

the particles are travelling faster and striking each other harder

as a result they have spread apart to an extent where they can slip by one another

Front 35

gas conceptual definition

Back 35

the particles have been struck with enough force to escape their attractions to other particles in the liquid

they are now either too far apart of moving too fast for their attractions to affect their movement

Front 36

phase change

Back 36

freezing: liquid to solid

melting: solid to liquid

evaporation (vaporization): liquid to gas

condensation: gas to liquid

sublimation: solid to gas

deposition: gas to solid

Front 37

particles can mean

Back 37

atoms, molecules, or ions

Front 38

melting point

Back 38

temperature of its solid as it changes to a liquid

Front 39

melting point depends on

Back 39

- strength of the attractive forces (bond strength)

- mass/symmetry of particles

Front 40

vapour

Back 40

gas formed by substance that boils above room temperature is called vapour

Front 41

boiling

Back 41

vigorous bubbling that occurs within the body of a liquid as it vaporizes internally

Front 42

bubble

Back 42

is a quantity of gas or vapour surrounded by liquid

Front 43

one definition of boiling point is

Back 43

the temperature at which the substances vapour pressure (the pressure inside that bubble) equals the surrounding air pressure

Front 44

another definition of boiling point is

Back 44

substancese highest possible temperature in the liquid state at any given atmospheric pressure

Front 45

what are the properties relevant to boiling

Back 45

boiling point, vapour pressure, volatility

Front 46

volatile substances are

Back 46

substances that readily evaporate or evaporate at high rates

- high vapour pressure and low boiling points

Front 47

heat of gusion

Back 47

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

Front 48

potential energy

Back 48

stored energy

Front 49

heat of fusion measured in

Back 49

joules per gram

Front 50

heat of vaporization

Back 50

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

Front 51

as the s olid melts slowly in its own liquid

Back 51

the temperature of the liquid does not rise because any added kinetic energy is absorbed by the solid and converted into potential energy through melting

Front 52

height = thickness

Back 52

= mass/l*w*density

Front 53

reactivity

Back 53

refers to whether a substance reacts to its reaction rate

Front 54

reactivity depends on

Back 54

- path from reactants to products, particularly which reactant bonds require breaking

- depend on properties such as reactant concentration

- whether or not a reaction will occur depends on the beginning and end states

Front 55

heat of formation

Back 55

heat released when a substance is formed from its elements

- measured in joules per gram

Front 56

heat of combustion

Back 56

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

- measured in joules or kilojoules pere gram