Review and Final

Post date: Jan 20, 2009 2:54:20 PM

Final is Tuesday for block 2 and Wednesday for block 3

    • Review

      • Chapter 2 - Matter

        • Classifying Matter

          • Matter is anything that is made of atoms and takes up space

          • All matter is either and element, a compound, or a mixture

            • Element - made of only one kind of atom

            • Compound - each molecule of a compound contains two or more elements that are chemically bonded

            • Mixture - Combination of elements and/or compounds that are not chemically bonded

            • Elements and compounds are pure substances, mixtures are not

        • Properties of Matter

          • Physical Properties

            • Can be observed without changing the identity of the substance

            • Examples: color, mass, melting point, boling point, density

            • Density = mass / volume

          • Chemical Properties

            • describes how a substance changes into a new substance, either by combining with other elements or by breaking apart into new substances

            • Examples: flammability and reactivity

        • Changes of Matter

          • Physical Changes

            • Affect one or more of the physical properties of a substance without changing its identity

            • Examples: melting, freezing, crushing, cutting, bending

          • Chemical Changes

            • Substance(s) are changed into new substances with different properties

            • Examples: burning, alka-seltzer in water, digesting, breathing

          • Breaking them down

            • Mixtures can be separated physically

            • Compounds must be broken down through a chemical change

      • Chapter 3 - States of Matter

        • Matter and Energy

          • Kinetic Theory - All matter is made up of atoms and molecules that are constantly in motion

          • States of Matter - matter can be classified as solid, liquid, or gas based on whether the shape and volume depend on the container or not

          • Energy's Role - Because they are in motion, all particle of matter have kinetic energy

        • Changes of State

          • The identity of a substance does not change, but the amount of energy it holds does

          • Mass and energy are both conserved (neither can be created or destroyed)

        • Fluids

          • Pressure

            • Fluids exert pressure equally in all directions

            • P = F / A

          • Buoyant Force

            • Fluids exert an upward buoyant force on matter

          • Pascal's Principle

            • If pressure is changed at one point in a fluid, the pressure changes by the same amount at all other points in the fluid

          • Fluid in motion

            • Fluids move faster through smaller openings than larger ones

            • The faster a fluid is moving, the lower the pressure in that fluid

        • Behavior of Gases

          • Properties of Gases

            • Expand to fill their container

            • Low densities

            • Compressible

            • Mostly empty space

          • Gas Laws

            • Help predict behavior of gases given certain changes

      • Chapter 6 - The Structure of Matter

        • Compounds and Molecules

          • Chemical Bonds - The forces that hold atoms or ions together

          • Chemical structure - the shape of compounds, shown with various models

          • The structure of a compound determines its properties

        • Ionic and Covalent Bonding

          • Atoms bond to complete their outer electron level

          • Ionic - one atom gives electrons to another

          • Covalent - electrons shared between several atoms

          • Metallic - electrons shared between all atoms in a substance

          • Polyatomic ion - group of bonded atoms that act as a single unit

        • Compound Names and Formulas

          • Ionic - names of ions, anion ending changed to -ide

          • Covalent - names of elements, farthes to the right changed to -ide, use prefixes to tell number of each type of atom

          • Empirical formulas - smallest whole-number ratio of atoms in a compound

      • Chapter 8 - Solutions

        • Solutions and other mixtures

          • Heterogeneous Mixtures

            • No fixed composition

            • Amount of each substance varies from sample to sample

            • "chunky"

          • Homogeneous Mixtures

            • Looks uniform, even under a microscope

            • Individual components are too small to be seen

            • Mixing at the molecular level

        • How Substances Dissolve

          • Water

            • Universal solvent - dissolves many substances

            • Polar molecules make it a good solvent

          • The dissolving process

            • Molecules at the surface of the solute get hit by molecules of the solvent

            • Collisions and attractive forces from the solvent knock molecules of the solute off

            • Rate depens on

              • Temperature - faster moving particles knock off pieces more easily

              • Size of solute pieces - more surface area = more of solute exposed

              • Stirring - moves solvent closer to solute, moves dissolved particles away