Properties of Matter

States Of Matter Solid: maintains a fixed volume and shape

Liquid: maintains a fixed volume but takes the shape of the container

Gas: occupies the entire volume available

Plasma: occurs at high temperatures

Phase Changes

Phase Change Diagram

Physical and Chemical Properties

Physical Properties:examples: texture, shape, size, color,

odor, volume, mass, weight, and density

Chemical Properties: example: color change, energy

given off or absorbed, gas given off, odor change, light, solid produced from solution

Physical and Chemical Changes

Physical Change: when objects undergo a change that does not change their chemical nature. Involves a change in physical properties

Chemical Change: substances are changed into different substances. The composition of the substance changes.

Intensive and Extensive Properties

Intensive Properties: Properties that do not depend on how much of the substance you have.

Examples: Temperature, pressure, density, boiling point, solubility, color

Extensive Properties: Depend on the amount of the substance.

Examples: Mass  and  volume  

Density Density= Mass/Volume

Describes the degree of compactness of a substance – ( how closely packed together the atoms of an element, molecule or compound are.) Is a physical or intensive property.

Properties of an Element:Element: a pure chemical

substance composed of atoms with the same number of protons

not easily broken down into it’s smaller parts

very distinctive properties

properties are different from the compounds they make up

Gold

Mercury

Sodium

Chlorine Gas

Properties of Compounds:

COMPOUND:

has a constant composition with fixed ratios of elements

physical properties such as boiling point or melting point of pure substances constant.

Example: pure water boils at 100 °C

Table salt: NaCl

Pure Water: H2O

Carbon Dioxide: CO2

WHAT ARE MIXTURES?  MIXTURE : •a combination of two or more substances that are not chemically united

• do not exist in fixed proportions

•most natural substances are mixtures

Properties of MixturesMIXTURES: can be physically

separated into pure compounds or elements.

just about everything that you can think of is probably a mixture.

may exhibit a changing set of physical properties.

Concrete

Sea Water

Vegetable soup

Heterogeneous MixtureHetero: indicates difference

consists of visibly different substances or phases

the four phases are gas, liquid, solid, and plasma

Example: beach sand, vinegar and oil salad dressing, air with clouds

Italian Salad Dressing

Jello with Fruit

Air with Clouds

Examples of heterogeneous mixtures:

"Dancing Raisins" shows liquid, solid, and gas substances in a heterogeneous mixture.

•Vinegar + Baking Soda – forms a heterogeneous solution: there are liquids and gases present.

Homogeneous MixturesHomo: indicates sameness

has the same uniform appearance and composition throughout.

are commonly referred to as solutions.

Examples: corn oil , white vinegar , sugar solution, air (with no clouds)

Kool-Aid

Swimming Pool Water

Air with no Clouds

Solutions Are distinguished by particle size.

Homogeneous solutions have particles which are the size of atoms or molecules - too small to be seen.

Homogeneous solutions are two or more substances in a single phase.

The concentrations may be expressed using a variety of measures.

Law of conservation of Matter Fundamental principle that states that

matter cannot be created or destroyed. In a chemical reaction the sum of all the

masses of the substances involved in the reaction (reactants) is equal to the sum of all of the masses of the substances produced by the reaction (products) .

No matter is gained or lost.

Percent (%) Mass The mass of the part (usually in grams) divided by

the mass of the whole (usually in grams) times 100.

mass % = mass of part / mass of whole X 100

Example: Hot Chocolate with Marshmallows mass of marshmallows: 2.5 grams mass of hot chocolate with marshmallows: 105.26 grams % Mass of Marshmallow: (2.5 g / 105.26 g) X (100) = 2.38 %

Symbols for Elements To write a symbol for an element -

you must follow these rules: 1st letter is always a capital letter. 2nd letter (if there is one) is always

lower case

Examples:Hydrogen: H Mercury: HgChlorine: Cl Lead: PbPhosphorus: P Potassium: K

Formulas for Compounds Compounds have a definite composition. The formula is very specific for that compound. If the formula changes in any way –it becomes a

different compound. Examples:

Water: H2O Hydrogen Peroxide: H2O2

Iron (II) Oxide: FeO Iron (III) Oxide: Fe2O3

Carbon Dioxide: CO2 Carbon Monoxide: CO