Chemistry 1

Front 1

Matter

Back 1

Anything that occupies space and has mass

Front 2

Mass

Back 2

Measure of the quantity of matter that an object contains

Front 3

Classification of matter can be

Back 3

Classify according to its:

Physical State

Composition

Front 4

Classifying Matter

Back 4

Front 5

Pure Substances

Back 5

Elements or Compounds:

Compounds can be further reduced into two or more elements

Front 6

Elements

Back 6

Consists of only one type of atom. They cannot be decomposed of further simplified by ordinary means

The elements are recorded on the periodic table

There are 118 recorded elements at this time

Front 7

Compound

Back 7

Combination of two or more elements in a definite, reproducible way

Front 8

Learn the names and symbols of the 1st 20 elements, alkali metals, alkaline earth metals, halogens, noble gases, Ti, Fe, Cu, Ag, Au, Pb

Back 8

Front 9

Mixtures

Back 9

A combination of two or more pure substances

Homogeneous: mixture consists of two or more substances in the same phase

Heterogeneous: uneven texture of the material can often be detected by the naked eye

When separated, the components of both types of mixtures yields pure substances

Front 10

Mixtures may be separated by physical properties

Back 10

Front 11

Heterogeneous Mixtures can be separated by ________

Back 11

Filtration

Front 12

Homogeneous Mixtures

Back 12

Solutions:

Solid/liquid

Liquid/liquid

Solid/Solid

Solute: minor component of a solution

Solvent: substance that contains solutes

Compositions can vary:

Amount of solute in solvent

Front 13

Chemical Compounds

Back 13

Chemical compounds are composed of two or more elements

*compounds have different properties than the elements

All compounds are made up of molecules or ions

Ionic compounds:

Molecules:

Fixed Ratio

Compounds represented by a chemical formula

1) Compounds have different properties than elements

2) Fixed composition ratio (definite proportion):

Definite % composition by mass

Front 14

Physical Properties

Back 14

Characteristics that can be evaluated without changing the composition of the material:

Color

Odor

Density

Melting Point

Thermal Conductivity

Volume

Hardness

Front 15

Some Physical Properties

Back 15

Color

State

Melting and boiling point

Density (mass/unit volume)

Extensive properties

(mass depend upon the amount of substance)

Intensive Properties

(density) do not

Intensive -> independent of sample size

Density: ratio of mass to volume

d=m/v

Front 16

Density Lab units

Back 16

Mass--> grams (g)

Volume (v)

Solids: cm^3

Liquids: ml

Gases: L

3)Densityof acetic acid at 20 °C is1.05 g/mLWhatvolume do I need to have 275 g of acetic acid?

Front 17

Physical Change

Back 17

A change that does not entail any change in chemical composition

Front 18

Chemical Changes

Back 18

One substance or more are transformed into one or more new substances

Chemical Reaction

Reactants ---> Products

The reactants and products are very different

Involves a change in chemical composition

Results in a change in composition or structure

Iron reacts metal reacts with oxygen to form rust

Front 19

Physical and Chemical changes often accompanied by energy changes

Back 19

Energy ---> Capacity to do work

Classified as Kinetic or Potential

Kinetic energy is energy associated with motion

Matter consists of atoms and molecules in motion

Front 20

Review Units of Measurements

Back 20

Front 21

Length

Back 21

Standard=Meter (m)

1000m = 10^3m = 1 km (kilometer)

10^-2 m = 1 cm (centimeter) and 100 cm =1 m.

10^-3 m = 1 mm (millimeter) and 1000 mm =1 m.

Front 22

Sizes of molecules are in the ____ range

Back 22

Nanometer

10^-9 m = nanometer

Front 23

Selected Prefixes used in the metric system

Back 23

Front 24

Volume

Back 24

Not a base unit --> from length

Meter is length unit ---> a cubic meter is a volume unit

m=length

m^3= volume

Common units:

L

mL

cm^3 also as cc

1cm^3 = 1mL

Front 25

Mass

Back 25

Base Unit = Kilogram (kg)

1kg = 1000 grams

Common units in chemistry are grams and milligrams (mg)

n250mL of water= 250 g of water = 1 cupn250kg = 250 L --> à ~tub.

Front 26

Time

Back 26

Base Unit = second

For smaller time frames

Milliseconds (ms), microseconds (us)

nanseconds (ns), etc. SI units prefixes

Front 27

Energy

Back 27

SI ---> joule (J)

kj = kilojoule = 1000 J

Non SI unit for food:

calories and Calories

cal Cal

Front 28

Dimensional Analysis

Back 28

Front 29

More practice at home

Back 29

Howmany inches in ¼ mile?

¼mile= 0.250 mile

0.250mile --> inches

1mile = 5280 ft

12in= 1 ft

0.250 mile

Ifthe speed of a molecule of oxygen at 25 °C is 490 m/s, and 1 mile is 1.609km, what is the speed of oxygen in mph?

Speedof light --> 6.71 x 108 mph --? m/s

Howmany grams in 4100 mg?