Chapter 1.2, 1.3, 12.1 Matter and Element Properties West Valley High School General Chemistry Mr. Mata Bravo! – 15,000 kiloton atomic bomb!!!

Standard 1A Students will know how the atomic structure is related to an element’s position on the Periodic Table of Elements.

Essential Question How is chemistry used to study the world around us?

Introduction Chemistry connects us to the world. All we see, taste, & touch is matter. Matter makes the world real. Chemistry = study of matter: (properties, composition, how matter interacts). Chemistry involved in many interesting jobs. Making perfumes, colognes, cosmetics. Crime scenes (forensics). Preparing great tasting and safe foods. Developing life-saving drugs.

Section 1-1 Chemistry is a physical science. Chemical = substance with a definite composition. Ex: water is always H2O. Everything made of chemicals.

6 Branches of Chemistry Organic Chemistry- study of carbon containing compounds. Example: C6H12O6 (Glucose) Inorganic Chemistry- study of compounds that do not contain carbon. Example: H2O Water. Physical Chemistry- study of properties, changes, & relation of energy and matter.

Analytical chemistry- study of components & composition of materials. Biochemistry- study of living things. Ex: photosynthesis, fermentation Theoretical Chemistry- study of math & computers to design/predict new stuff.

Types of Research Basic Research-how and why things work. Applied Research- solve specific problem. Ex: depletion of the ozone layer. Technological Development- application of science to solve problems. Ex: biodegradable materials

Section 1-2 Mass: amount of matter. Matter: anything with mass & volume Ex: air, smoke, water . Atom: smallest unit of element. Element: made of one kind of atom. Periodic Table contains 118 elements. 92 naturally occurring (found in nature) Other 26 synthetically made.

Compound: 2+ elements chemically bonded. Physical properties: measured without altering material. Ex: MP of ice Extensive Physical Properties: depend on the amount of matter. Ex: mass & length Intensive Physical Properties- does NOT depend on amount of matter. Ex: MP, BP, FP, density, color, crystal shape

Physical change - does NOT result in change in identity Physical change - does NOT result in change in identity. Ex: cutting wire, crushing a solid, gas expanding. Changes in state(S <-> L <-> G) Ex: melting, boiling, freezing. Chemical Properties: undergo changes that alters identity. Ex: reactivity.

Chemical change or reaction (rxn); new substance made Chemical change or reaction (rxn); new substance made. Ex: bread baking, nail rusting, moldy orange Basic Chemical Formula A + B  C A & B are called reactants  is read “yields” = “produces” C is the product (s)

4 states of matter Solids: definite shape &volume. Liquids: definite volume; no definite shape. Gases: no definite volume; no definite shape. Plasma: gaseous system of charged particles.

Weight vs. Mass Weight: pull of gravity on object. Mass: quantity of matter. Astronauts in space experience weightless since gravity changes. Ex: 120 lb person on earth would only weigh 20 lb on moon (1/6th gravity), but would still have a mass of 120 lb.

Law of conservation of mass: matter CANNOT be created nor destroyed. Ex: burning wood, nuclear reactions Law of conservation of energy : energy CANNOT be created nor destroyed, but can be converted. Ex: Kinetic & potential energy.

Classification of Matter Mixture: 2+ kinds of matter; each retains identity & properties; can be separated physically. 2 types of mixtures Homogeneous (solutions); uniform composition. Ex: air, sugar in water, stainless steel. Heterogeneous; not uniform. Ex: granite, wood, blood.

Pure substances Compound: made from atoms of 2+ elements that are chemically bonded. Ex: water, salt, sucrose. Cannot be separated physically. Element: made of one pure substance that cannot be broken down. Examples: gold, silver, hydrogen.

What is a Solution? Solution = homogeneous mixture of two or more substances. (solute & solvent) Solute = substance being dissolved. Solvent = substance doing the dissolving. Homogeneous mixture = completely dissolved & uniform solute in solvent Aqueous solution = solution in which the solvent is water.

Parts of a Solution

Homogeneous vs. Heterogeneous 24-karat gold is pure gold = homogeneous 14-karat gold is an alloy (mixture) Au, Ag, Cu = heterogeneous 14-karat gold is 14/24 (58.3%) gold

Solubility Terminology Soluble = substance that can be dissolved. Insoluble = substance that cannot be dissolved. Solubility = measure of how much solute will dissolve in solvent. Miscible = two liquids that dissolve in each other (ex: water & ethanol). Immiscible = two liquids that don’t dissolve in each other(ex: H2O & oil).

Immiscible Liquids

Solubility Terminology SATURATED—contains the maximum amount of solute. UNSATURATED—contains less solute than a saturated solution. SUPERSATURATED—contains more solute than it should.

Solution Saturations

Suspensions Suspension – particles in a solvent are so large that they settle to bottom unless agitated. Ex: muddy water Soil particles will sink to bottom. Can be separated from heterogeneous mixtures by filtering.

Colloids Particles are intermediate in size between those in solutions and suspensions. 1 nanometer (nm) to 1000 nm. Cause mixture to look “cloudy”. Ex: mayonnaise Egg yolk keeps the oil droplets dispersed.

Ch. 1.2,1.3,12.1 SUTW Prompt Describe how physical and chemical changes differ from each other. Complete an 8-10 sentence paragraph using the SUTW paragraph format. Use green, yellow, pink hilighers. Due Date: Monday, Aug. 16th at beginning of your regular class.