Unit 2 Lesson #1Types of Matter

Matter Anything that has mass &

take up space

Mass = measurement of the amount of matter an object contains

Chemistry = the study of matter & the changes that it undergoes

Classifying Matter

Quantitative – numerical information

how much, how little, how big, how small

Qualitative – descriptive information

condition, color, size, shape, odor, texture

Matter Flowchart

MATTER

Can it be physically separated?

Homogeneous Mixture

(solution)

Heterogeneous Mixture Compound Element

MIXTURE PURE SUBSTANCE

yes no

Can it be chemically decomposed?

noyesIs the composition uniform?

noyes

Pure Substances

Every sample has same:1. Characteristic properties

2. Composition

Are made of: 1. one type of atom: element

Ex: iron, gold, oxygen

2. Two or more types of atoms: compound Ex: salt, sugar, water

Which are pure substances?

Element Simplest form of matter that has its own unique

set of properties Can not be separated into simpler substances

by physical or chemical means Each element is made up of a single type of

atom

ex. hydrogen, nitrogen, lead

Compound1. A substance that contains 2 or more elements

chemically combined in a fixed proportion (Law of Definite Proportion) Ex.

2. Properties are different than the individual elements

ex. Glucose (sugar)

Glucose – sweet, white solidCarbon – black, tasteless solidOxygen – colorless, tasteless gas Hydrogen – colorless, tasteless gas

Breaking Down Compounds Physical methods do not work Recall…

Chemical changes – a change that produces matter with a different composition than the original matter

Symbols & Formulas Chemical Symbol

each element is represented by a one- or two-letter symbol

Trends:1st letter = always capitalized2nd letter (for an element) = always lowercaseSubscripts = indicate the relative proportions of the elements

in a compound

H K Au H2O C6H12O6

Hydrogen Potassium Gold Water Glucose

Mixtures1. A combination of 2 or more types of matter2. Each component keeps its own identity & properties 3. Components are only physically mixed & can be separated using physical means

Chicken noodle soup

Cinnamon & Sugar

Air

Types of Mixtures1. Heterogeneous mixture -

a mixture in which the substances are not evenly distributed

Salad

Ice tea with ice

Oil & vinegar

2. Homogeneous mixture –

a mixture or ‘solution’ in which the substances are evenly distributed

Kool-Aid

Water

Stainless Steel

Phase – used to describe any part of a sample with uniform composition & properties

Homogeneous mixture

1 phase

Heterogeneous mixture

2 phases

Practice Examples:

graphite

pepper

sugar (sucrose)

paint

soda

Type of Matter

element

hetero. mixture

compound

hetero. mixture

solution

1. Filtration – a technique that uses a porous barrier to separate a solid from a liquid

Can you think of any common applications?

Separating Mixtures

‘Plays’ on differences in physical properties

2. Distillation – a technique that can be used to physically separate most homogeneous mixtures based on differences in the boiling points of the substances involved

3. Chromatography – a technique that is used to physically separate the components of a mixture based on the tendency of each component to travel or be drawn across the surface of another material

Crystallization

Separation technique that results in the formation of pure solid particles from a solution containing the dissolved substance

As one substance evaporates, the dissolved substance comes out of solution and collects as crystals

Produces highly pure solids Rocky candy is an example of

this

Practice Examples:

tea

muddy water

fog

saltwater

Italian salad dressing

Answers: Solution

Heterogeneous

Heterogeneous

Solution

Heterogeneous

Substances vs. Mixtures

Unit 2 Lesson #2Properties of Matter

Properties of Matter1. Extensive – a property that depends on the amount of

matter in a sample ex. mass, volume, amount of energy 2. Intensive – a property that depends on the type (or

identity) of matter in a sample ex. hardness, density, boiling point, electrical

conductivity

Substances – matter that has uniform & unchanging composition have identical intensive

properties… Why?

because every sample has the same composition

Extensive vs. Intensive

Examples:

boiling point

volume

mass

density

conductivity

Answers:

intensive

extensive

extensive

intensive

intensive

3. Physical Properties – a characteristic that can be observed or measured w/out changing the identity of a substance

ex. color, odor, taste, hardness, density, melting/boiling points, state of matter

States of Matter – the physical forms in which all matter exists on Earth

Can you identify these 3 states?

Solid def. shape & volume shape

independent of container

particles are packed together

Liquid def. volume shape depends on container particles can move freely

Gas indefinite volume & shape particles move quickly & spread apart

Chemical Properties Chemical Property

describes the ability of a substance to undergo changes in identity

any of the properties of matter that may only be observed and measured by performing a chemical change or chemical reaction.

Ex. heat of combustion, reactivity with water, pH

Properties of Copper

Physical vs. Chemical Properties

Examples:

melting point

flammable

density

magnetic

tarnishes in air

Answers:

physical

chemical

physical

physical

chemical

Unit 2 Lesson #3Changes in Matter

Phase Changes Evaporation =

Condensation =

Melting =

Freezing =

Sublimation =

Liquid -> Gas

Gas -> Liquid

Solid -> Liquid

Liquid -> Solid

Solid -> Gas

All Physical Changes

Physical Change – a change that occurs in the physical

appearance of a substance, but does not change its identity

breaking, splitting, grinding, cutting, crushing

Ex. melting, boiling, freezing, evaporating, dissolving, condensing

Physical Changes

Chemical Properties – relates to a substance’s ability to undergo changes that transform it into a different substance easiest to see when a chemical is reacting

Chemical changes – a change that produces matter with a different composition than the original matter

ex. burning, rotting, rusting, reacting, cooking, digestion, respiration

Chemical Changes

The process of photosynthesis is a chemical reaction in which light energy, carbon dioxide and water, are transformed to create glucose and oxygen.

The photosynthetic chemical reaction can be shown by writing out the element symbols for each compound.

Reactants substances to the left of the arrow ‘ingredients’ CO2 and H2O

Products substances to the right of the arrow ‘what is made’ or produced C6H12O6 and O2

1. Ammonium Chloride + Water

2. Sodium Bicarbonate + Calcium Chloride

3. Sodium Bicarbonate + Acetic Acid

Did a Chemical Reaction Occur?

Recognizing Chemical Changes

1. Transfer of energy

Energy may be given off

in the form of heat or light

2. Change in color

or odor

Substances may

‘brown’ Indicators

How can you tell whether a chemical change

has taken place?

3. Precipitate

A solid that settles

out of a liquid mixture

4. Gas production

Indicated by the formation

of ‘gas bubbles’

1. Ammonium Chloride + Water

NH4Cl(s) + H2O(l) + Heat ----> NH4 + (aq) + Cl -(aq) + H2O(l)

2. Sodium Bicarbonate + Calcium ChlorideNaHCO3(s) + CaCl2(s) ----> CaCO3(s) + NaCl(aq) + HCl (aq)

3. Sodium Bicarbonate + Acetic Acid NaHCO3(s) + CH3COOH(aq) ----> NaCH3COO-

(aq) + CO 2(g) + H2O(l)

Did a Chemical Reaction Occur?

Physical vs. Chemical Changes

Examples:

rusting iron

dissolving in water

burning a log

melting ice

grinding spices

Answers:

chemical

physical

chemical

physical

physical

Law of Conservation of Matter During any chemical reaction, the mass of the

products is always equal to the mass of the reactants

+ O2

+ CO2 + H2O vapor

I. Law of Conservation of Mass

Although chemical changes occur, mass is neither created nor destroyed in a chemical reaction

Mass of reactants equals mass of productsmassreactants = massproducts

A + B C

Conservation of mass also applies to physical changes…

10g of ice 10g of liquid H2O