Presentation on theme: "Physical vs Chemical Properties of Matter. Extensive Properties of Matter – Extensive - Properties that do depend on the amount of matter present. Mass."— Presentation transcript:
Extensive Properties of Matter – Extensive - Properties that do depend on the amount of matter present. Mass - A measurement of the amount of matter in a object (grams). Weight - A measurement of the gravitational force of attraction of the earth acting on an object. Volume - A measurement of the amount of space a substance occupies. Length
Intensive Properties – Intensive - Properties that do not depend on the amount of the matter present. Color Odor Luster - How shiny a substance is. Malleability - The ability of a substance to be beaten into thin sheets. Ductility - The ability of a substance to be drawn into thin wires. Conductivity - The ability of a substance to allow the flow of energy or electricity. Hardness - How easily a substance can be scratched. Melting/Freezing Point - The temperature at which the solid and liquid phases of a substance are in equilibrium at atmospheric pressure. Boiling Point - The temperature at which the vapor pressure of a liquid is equal to the pressure on the liquid (generally atmospheric pressure). Density - The mass of a substance divided by its volume
Chemical Properties of Matter Chemical Properties of matter deal with how the substances reacts with other substances
Oxidation Does the substance rust or combine with oxygen
Ph of the substance Is the measure of the H+ ions in a solution
Heat of Combustion The temperature at which something will burn
Physical Change vs Chemical Change There are two possible definitions for Physical and Chemical changes: 1. A physical change is reversible, a chemical change is not. – For example, the freezing of water would be a physical change because it can be reversed – the burning of wood is a chemical change - you can't 'unburn' it. 2. A physical change is a change in which no new substance is formed; a chemical change results in the formation of one or more new substances. -Again, consider the previous examples: -Freezing water into ice just results in water molecules which are 'stuck' together - it's still H 2 O. -Burning wood results in ash, carbon dioxide, etc, all new substances which weren't there when you started.
Mixtures -In Mixtures Substance maintain their chemical properties. -Substances can be seperated -Mixtures are substances held together by physical forces, not chemical. That statement means the individual molecules enjoy being near each other, but their fundamental chemical structure does not change when they enter the mixture.
Solutions Solutions are groups of molecules that are mixed up In a completely even distribution. example: Sugar in water vs. Sand in water. Sugar dissolves and is spread throughout the glass of water. The sand sinks to the bottom. The sugar- water could be considered a solution. The sand-water is a mixture -A simple solution is basically two substances that are going to be combined. -A solute is the substance to be dissolved (sugar)solvent. -A Solvent is the one doing the dissolving (water). As a The rule of thumb, there is usually more solvent than solut then one solvent
Homozygous vs Heterozygous A homogeneous mixture has the same uniform appearance and composition throughout. A heterogeneous mixture consists of visibly different substances or phases. The three phases or states of matter are gas, liquid, and solid.
Different types Alloys- Metal Mixtures Colloids- larger particles in a hoogeneous suspension Suspension- Large particles floating in a solution lifted by flow or motion