Chemistry Chapter 1 Matter and Change

Chemistry is… …the study of the composition, structure, and properties of matter and the changes it undergoes C 2 H 5 OH + 3 O 2  2 CO H 2 O + Energy Reactants  Products

Matter- anything that has mass and occupies space

Solid Solid – definite volume and shape; particles packed in fixed positions. Liquid Liquid – definite volume but indefinite shape; particles close together but not in fixed positions Gas Gas – neither definite volume nor definite shape; particles are at great distances from one another

Three Phases

Copper Phases - Solid

Copper Phases - Liquid

Copper Phases – Vapor (gas)

Solid Liquid Gas Melting Freezing Vaporization condensation sublimation deposition

Physical Property Is tested without changing the substance Physical properties of the left test tube are: a)Clear color of solution B ) boiling point of 60˚C c) Physical state-liquid d) The volume of 25 mL e) The mass of 2.5 g f) The density of 0.1 g/mL

Chemical Property Ability to form new substances Flammability- New substances formed are Carbon dioxide and water Reactivity New substances Formed are hydrogen Gas and a salt

Physical Change A change in a substance that does not involve a change in the identity of the substance. Phase Changes (to melt) Tearing of paper Dissolving In water

Chemical Change A change in which one or more substances are converted into different substances. Different chemical compounds are ignited in fireworks. Burning is also an example

Classification of Matter

Pure substances Cannot be separated by physical means Always have the same composition Subdivided into elements and compounds Sulfur (S) Potassium (K) Carbon (C) Copper Cu Table Salt NaCl

Elements Fundamental substances Cannot be broken down into other substances by physical or chemical means Contain only one kind of atom

The Periodic Table Period Group or family Period Group or Family

New IUPAC naming system with numbers Old IUPAC naming system with Roman numerals

Compound A substance that is made from the atoms of two or more elements that are chemically bonded. Sucrose – C 12 H 22 O 11 Sucrose is also known as table sugar, and is used to make Gummy Bears!

Homogenous mixture Same throughout No phase boundaries

Heterogeneous mixture Not same throughout Has phase boundaries Particles large enough to see Gas in liquid Gas in solidLiquid in gas Liquid in liquid

Physical separation techniques for mixtures: A) Filtration B) Crystallization C) Distillation D) Chromatography

Separation of a mixture- filtration separation of a solid residue from a liquid using a funnel

Separation of a Mixture Two solid residues of ink are separated using Paper chromatography

Separation of a Mixture Two liquids are separated by distillation- a way to Separate a mixture by taking advantage of different Boiling points

Crystallization Separation of a solid residue from a volatile liquid

Separation of a Compound Separation of a Compound The Electrolysis of water Water  Hydrogen + Oxygen H 2 O  H 2 + O 2 Reactant  Products Compounds are separated by chemical means. With the application of electricity, water can be separated into its elements

Properties of Metals  Metals are good conductors of heat and electricity  Metals are malleable  Metals are ductile  Metals have high tensile strength  Metals have luster

Examples of Metals Potassium, K reacts with water and must be stored in kerosene Zinc, Zn, is more stable than potassium Copper, Cu, is a relatively soft metal, and a very good electrical conductor. Mercury, Hg, is the only metal that exists as a liquid at room temperature

Propertiesof Nonmetals Properties of Nonmetals Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.  Nonmetals are poor conductors of heat and electricity  Nonmetals tend to be brittle  Many nonmetals are gases at room temperature

Examples of Nonmetals Sulfur, S, was once known as “brimstone” Microspheres of phosphorus, P, a reactive nonmetal Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure

Properties of Metalloids Metalloids straddle the border between metals and nonmetals on the periodic table.  They have properties of both metals and nonmetals.  Metalloids are more brittle than metals, less brittle than most nonmetallic solids  Metalloids are semiconductors of electricity  Some metalloids possess metallic luster

Silicon, Si – A Metalloid  Silicon has metallic luster  Silicon is brittle like a nonmetal  Silicon is a semiconductor of electricity Other metalloids include:  Boron, B  Germanium, Ge  Arsenic, As  Antimony, Sb  Tellurium, Te