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Unit 2 Matter

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Tyquan Paul

on 11 October 2012

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Transcript of Unit 2 Matter

Matter Unit 2 Anything that takes up space =volume
and displays the properties of mass and
inertia. Matter Composition 2 Parts/components Components of a sample and their relative
proportions. Properties Distinguishing qualities or attributes of a sample mater Example: water/h20
Components: Hydrogen and oxygen
2 parts Hydrogen, 1 part oxygen Example:banana
Color: yellow/green
Textures: Squishy/soft
Changes: browning Examples Based on the ability to be broken down or separated Types of Matter Elements Pure Substances (2 Types) Compounds Simple Bonded 115 total
92 naturally occurring Breakdown difficult change Mixtures Main Types of Mixtures Homogeneous Heterogeneous Even Mix Uneven Separate mixtures based on the physical properties of the parts of the mixture Separating Mixtures Distillation vs. Evaporation seawater
(to get salt only) Seawater Evaporation Salt Water vapor/
water Seawater
(to get salt and water Seawater Distillation Salt Water Vapor/
water Sieving Can separate large particles from smaller ones Magnetism Centrifuge Heavy Blood cells sink to the bottom Physical and Chemical Properties Characteristics Two types 1.Physical-Same
2.Chemical-New Physical Properties of matter Thermal Expansion
Surface Area
State/Phase at room temp. Mass
Melting/Freezing Point
Condensation/boiling point
Solubilty Intrinsic vs. Extrinsic Same density,
melting/boiling/freezing point
Heat Fusion/Vaporization,solubility,
color/taste/odor,specific heat, malleability,ductile,Conductivity Changes mass,volume,length,area
circumference, weight, force Chemical Properties of Mater Flammability
Light sensitivity
Oxidative ability D=m/v Physical and Chemical Changes What the substance is doesn't Change Ex. Painting a wall Gas production New substance forms
Signs Precipitate
Changes in color
Energy Released
Odor Phases of Matter Based on three properties of a substance: How the particles are arranged: How much energy the particles have:the distance between the particles Solids Set volume
Set Shape
Each volume is held in place with strong (IMF's)Intermolecular force Solids Atoms still vibrate in place
The vibrations cause a small amount
of thermal energy. Liquids Have a set volume
No set shape
Intermediate thermal energy Particles are no longer orderly Particles are close together but have the freedom to move past each other Particles move more quickly than in solids IMF's are intermediate Gases No shape
Particles arranged has no order to it
No volume
Particles are as far apart as possible
Allows for diffusion
Particles move very quickly
Due to high thermal energy
IMF's are very weak Plasma When a gas is heated at 1000*c or higher
Ionized (has particles with charges)
Good conductor of electricity
Affected by magnetic fields
No shape or volume
Sun Phase changes and Graphs Ionization- to convert wholly or partly into ions
DeIonizaton- to remove ions from
Freezing-to solidify as a result of abstraction of heat
Freezing Point- the temperature at which a liquid solidifies
Melting- to become altered from a solid to a liquid state usually by heat
Melting Point- the temperature at which a solid liquifies
Condensation- : the conversion of a substance (as water) from the vapor state to a denser liquid or solid state usually initiated by a reduction in temperature of the vapor
sublimation- the process of transformation directly from the solid phase to the gaseous phase without passing through an intermediate liquid phase.
Deposition- a process in which gas transforms into solid
Vaporization- the conversion of a solid or liquid into a vapor without chemical change
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