Matter

Matter Matter is anything that has mass and takes up space (volume) Matter is made up of tiny particles called atoms Atoms combine to form many different types of matter (curling iron, pizza, water, etc.) Law of Conservation of Matter – matter can be neither created nor destroyed https://www.youtube.com/watch?v=SeDaOigLBTU (3 min)

Types of Matter Pure Substances Elements Compounds Impure substances Homogeneous mixtures Heterogeneous mixtures

Pure Substances Element – matter made up of one type of atom Can be found on the periodic table Compound – matter made up of two or more atoms CHEMICALLY bonded together Can only be separated by chemical reactions

Impure Substances Impure mixtures – two or more elements and/or compounds not chemically bonded Can be separated by physical means Homogeneous mixtures – uniform in composition; parts are not easily distinguished Heterogeneous mixtures – components are not evenly distributed; parts can be identified

Separating mixtures Heterogeneous mixtures: filtration Homogeneous mixtures: distillation (2 liquids), crystallization (evaporate), and chromatography

States of Matter Matter occurs in FOUR states Solid Liquid Gas Plasma (flames, lightning, Northern lights, sun)

STATES OF MATTER https://www.youtube.com/watch?v=KCL8zqjXbME (5 min) LIQUID PLASMA SOLID GAS Tightly packed, in a regular pattern Vibrate, but do not move from place to place Close together with no regular arrangement. Vibrate, move about, and slide past each other Well separated with no regular arrangement. Vibrate and move freely at high speeds Has no definite volume or shape and is composed of electrical charged particles

Description of Phase Change PHASE CHANGES Description of Phase Change Term for Phase Change Heat Movement During Phase Change Solid to liquid Melting Heat goes into the solid as it melts. Liquid to solid Freezing Heat leaves the liquid as it freezes.

Description of Phase Change PHASE CHANGES Description of Phase Change Term for Phase Change Heat Movement During Phase Change Liquid to gas Vaporization, which includes boiling and evaporation Heat goes into the liquid as it vaporizes. Gas to liquid Condensation Heat leaves the gas as it condenses. Solid to gas Sublimation Heat goes into the solid as it sublimates.

Properties of Matter Matter has physical properties – characteristics that may be observed without changing the identity of the substance Density, color, melting point, solubility Matter has chemical properties – characteristics that cannot be observed without changing the identity of the substance Flammability

Changes of Matter Matter is not rigid and can change through physical or chemical means Physical change – Change in a material that does not result in producing a new chemical (phase change, dissolving, cutting) Chemical change – change in a material that results in a new chemical being formed (cooking, digestion)

Evidence of a chemical change Form a gas Release of energy Permanent color change Precipitate New odor

Temperature Temperature and heat are NOT the same thing! Temperature = average speed of particles Units = oC, K, oF Heat = a form of energy, can be used to make particles go faster Units = joules (J), calories* (cal) *1 cal = amount of heat needed to raise temp of 1 g of water by 1oC

Specific Heat Specific heat- aka heat capacity The ratio of heat added to a system and the temp change of the system How much heat you need to add to a substance to change its temp Specific heat of liquid water = 4.184 J/goC or 1.00 cal/goC

Calories If a metal absorbs 63.2 calories of heat, how many Joules of energy is this? A) If a metal absorbs 23.45 calories of heat, how many Joules of energy is this?

Law of Conservation of Energy Law of Conservation of Energy – energy can be neither created nor destroyed (but can be transferred or transformed)

Energy Calculations (Q = m x c x ΔT) Energy = specific heat x mass x change in temp (Q = m x c x ΔT) NOTE: mass in g, Temp in oC, Energy in J This formula is slightly different in your book, but this is the one on the AP chemistry formula sheet How much energy is required to raise the temp of 18g ice from -40oC to its normal melting point of 0oC? NOTE: look at page 329 Q = 18g x 2.03 J/goC x 40oC= = 1500 J or 1.5 kJ

Energy Calculations A) How much energy is needed to raise 18g of water from 0oC to 100oC? (s of H2O is 4.184 J/goC) B) A block of aluminum weighing 140. g is cooled from 98.4°C to 62.2°C with the release of 1080 joules of heat. From this data, calculate the specific heat of aluminum.