Chapter 2 Matter Mixtures Elements and Compounds Chemical Reactions

Chapter 2Chapter 2

Matter Mixtures Elements and

Compounds Chemical Reactions

What states of matter are represented?What states of matter are represented?

Properties of MatterProperties of Matter

Matter – anything that has mass and takes up space

Mass – amount of matter an object contains

Properties of MatterProperties of Matter

Substance – matter that has a uniform and definite composition

Example: Sugar Pure Substance – only

contains one kind of matter

Properties of MatterProperties of Matter

Physical Property – a quality of condition of a substance that can be observed or measured without changing the substances composition

Example: Color, solubility, odor, hardness, density, melting point

States of MatterStates of MatterProperty Solid Liquid Gas or Vapor

Shape

Volume

Expansion on Heating

Compressibility

States of MatterStates of MatterProperty Solid Liquid Gas or Vapor

Shape Definite Indefinite Indefinite

Volume Definite Definite Indefinite

Expansion on Heating

Very Slight Moderate Great

Compressibility Almost Incompressible

Almost Incompressible

Readily Compressible

Physical ChangesPhysical Changes

Cutting Grinding Bending Melting Freezing Boil Dissolve Split

Chapter 2.2 MixturesChapter 2.2 Mixtures

What is a mixture?

How can it be separated?

Classifying MixturesClassifying Mixtures

Mixture – physical blend of two or more substances

Classifying MixturesClassifying Mixtures

Heterogeneous – a mixture that is not uniform in composition, its components are readily distinguished

Example: Salad

Classifying MixturesClassifying Mixtures

Homogeneous - a mixture that is completely uniform in composition, its components are not readily distinguished

Example: salt water

Classifying MixturesClassifying Mixtures

Solution – homogenous mixture Example: Sterling Silver (Copper in silver)

Classifying MixturesClassifying Mixtures

Phase – any part of a system with uniform composition and particles

PhasePhase

Homogeneous mixture – Single Phase

Heterogeneous mixture – two or more phases

Separating MixturesSeparating Mixtures

Separate physically by shape, size, color, etc…

Separate with a magnet, filter

Separate by distillation

DistillationDistillation

A liquid is boiled to produce a vapor that is condensed back into a liquid

Used to separate impurities in liquids

MatterMatter

Mixtures Pure Substance

Homogenous Mixtures

Heterogeneous Mixtures

Compound Elements

Solution

Ch 2.3 Elements and Ch 2.3 Elements and CompoundsCompounds

Distinguishing Elements and Distinguishing Elements and CompoundsCompounds

Element – simplest form of matter that can exist, cannot be separated into simpler substances by chemical means

Top Ten Elements in the Human Body– Oxygen 65%– Carbon 18%– Hydrogen 10%– Nitrogen 3%– Calcium 1.5%– Phosphorus 1.2%– Potassium 0.2%– Chlorine 0.2%– Sulfur 0.2%– Sodium 0.1%

Distinguishing Elements and Distinguishing Elements and CompoundsCompounds

Compound – 2 or more elements that combine chemically, can be separated into simpler substances by chemical means

SugarSugar

Sugar

compound

Carbon

Element

Water

Compound

+

Water

compound

Hydrogen

element

Oxygen

element

+

HEAT

ELECTRICITY

Symbols and FormulasSymbols and Formulas

Chemical Symbols – One or two letters– First letter always capitalized– Second letter lower case

Name Symbol Latin Name

Sodium Na natrium

Potassium K kalium

Antimony Sb stibium

Copper Cu cuprum

Gold Au aurum

Silver Ag argentum

Iron Fe ferrum

Lead Pb plumbum

Mercury Hg hydrargyrum

Tin Sn stannum

Tungsten W wolfram

Ch 2.4 Chemical ReactionsCh 2.4 Chemical Reactions

Ch 2.4 Chemical ReactionsCh 2.4 Chemical Reactions

Chemical Reaction – the changing of substances to other substances by the breaking of bonds in reactants and the formation of bonds in products

Parts of a ReactionParts of a Reaction

Reactants Products Reactants – starting substances Products – substances formed

Chemical PropertyChemical Property

Ability of a substance to undergo a chemical reaction and form new substances

Examples of Chemical Examples of Chemical ReactionsReactions

Burn Rot Rust Decompose Ferment Explode Corrode

Clues that a chemical reaction Clues that a chemical reaction has occurredhas occurred

Heat given off Heat absorbed Odor given off Irreversibility

Law of Conservation of MassLaw of Conservation of Mass

Total mass of reactants = Total mass of products

In any physical or chemical reaction, mass is neither created or destroyed