the structure of matter matter – anything that has mass and takes up space mass – the amount of...
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The Structure of Matter
Matter – Anything that has mass and takes up space
Mass – The amount of matter in
an object
Molecule – The smallest particle of a substance (such as water) that can still be identified as that substance (Latin = little mass)
Ex. – 60 million H2O – diameter of a
penny
Ex. All water molecules are the same
-Once a molecule is divided it is no longer that substance
Ex. H2O H2 Not water
O Not water
OH H
Physical & Chemical Properties of Matter
Physical Properties – A characteristic of matter that can be observed by using any of your senses
Ex. Hardness, density, melting pt. /
boiling pt., State (solid, liquid, gas)
Size, shape, color, odor, taste
Physical & Chemical Properties of Matter
Chemical Properties – A description of how one kind of matter behaves in the presence of another kind of matter.
Ex. Vinegar & baking soda
- When vinegar is added to baking soda, CO2 is produced
States of Matter
State Definite Shape Definite Volume
Solid
Liquid
Gas NoYes
Yes YesNo
NoSolid Liquid Gas
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Solid
Liquid
Gas
PlasmaPlasma- State of matter where gas
molecules have separated into electrically charged particles
Ex. STARS (fusion)
Physical & Chemical ChangesPhysical Change- a change in which
the form or appearance of matter changes but not its composition
Ex. Shape – crumpled paper
Dissolving – Koolaid
Change in State
Physical Changes
Solid Liquid GasFreezing
Melting
Condensation
Vaporization
Deposition
Sublimation
- Only the MOTION of the molecules has changed!
Chemical ChangesChemical Change – a change in which the composition of a substance changes
Ex. Fireworks, Rust
- causes a new substance to form.
Chemical ChangesSigns of Chemical Changes
- Color Changes Ex. Trees, apples, toast
- EnergyReleased – fire – heat, light
Gained – cooking/cake
Chemical ChangesSigns of Chemical Changes
- Odor Ex. Rotten food
- Bubbles formedEx. Vinegar + Baking soda
Antacid
Chemical ChangesSigns of Chemical Changes
- Solid formed - PrecipitateEx. Sodium iodide = lead nitrate
- Not easily reversed Ex. Ice melting vs.
Wood burning
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Physical Chemical
EASY HARD
VS.
Anton Lavoisier – 18th CenturyThe LAW of Conservation of Mass-- States that mass is neither created nor destroyed
(and as a result, the mass of the substance before a physical or chemical change is equal to the mass of the substances present after the change)
Ex. Apple cut up, candle burning
GasesThe Kinetic Theory of Matter-
- The scientific principal that says that all matter is made of particles whose MOTION determines if the matter is solid, liquid, or gas
-Each of the 3 states of matter is called a phase
State Definite Shape Definite Volume
Solid
Liquid
Gas NoYes
Yes YesNo
No
4 Properties of Gases- explained by the Kinetic theory of matter
1. Gas molecules move VERY FAST-A gas is mostly empty space
(large distance between gas molecules)-Particles collide MANY times per second
(particles are NOT affected by collisions)
- No definite shape, they expand to fill all available space
2.Moving gas molecules cause pressure
Ex. Balloon
(All that moving and colliding into things causes a force to be applied)
Pressure- The amount of force applied to a unit of area
3.Gases have NO definite volume
-can be crowded together
-This the pressure (more collisions)
-can be allowed to expand
-This the pressure (fewer collisions)
4.The temperature of a gas measures how fast molecules move
- Heat = in particle movement
(particles tend to move further apart)
- volume or the pressure
Ex. Bicycle tire on a hot day
- Heat = in particle movement
Absolute Zero - -The Temperature at which particles of matter stop moving -273 oC-No Kinetic Energy at absolute zero-Kelvin (K) Temperature scale - -A temperature scale on which zero is equal to absolute zero
GAS LAWS!
Boyle’s Law
Pressure = Volume
Pressure = Volume
No Temperature change
V1 . P1 = V2 . P2 Ex. The air in a balloon occupies a space of 1000mL and has a pressure of 5 N/cm2. When Gary grabs the balloon the pressure increases to 10 N/cm2. What is the new volume of the balloon?
V1= V2=
P2= P2=
V1= 1000mL V2= ? mL
P1= 5 N/cm2 P2=10N/cm2
1000 . 5 = V2 . 10
V1 . P1 = V2 . P2
5000 = V2 . 10 5000 = V2 . 10 10 = 10 500 = V2V2 = 500 mL
GAS LAWS!
Charle’s Law
Temperature = Volume
Temperature= Volume
V1 . T2 = V2 . T1
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V1 . T2 = V2 . T1 Charle’s Law
10o C
V1= V2=
T2= T1=
30o C
30mL ? mL
30mL
30oC
? mL10oC
V1 . T2 = V2 . T1
Charle’s Law
10o C
V1= V2=
T2= T1=
30o C30mL ? mL
30mL
30oC
? mL
10oC 30 . 30 = V2 . 10 900 = V2 . 10
10 10 90 = V2
V2 = 90mL
Solids & Liquids
(the molecules stay in a fixed patteren)
Solids- A piece of solid matter cannot change shape by itself
Ex. crystal
Crystal- A solid whose orderly arrangement of particles gives it a
regular shape
- The shape (of the crystal) is determined by the way the particles are arranged
-Almost all solids are made of crystals
Ex. salt(different crystals break in different ways)
Super cooled liquids- Solids that have been cooled soooooo quickly that they
have NO crystal pattern-Almost all solids are made of crystals
Ex. Volcanic glass
Liquids- molecules (can move from one place to another) have NO fixed
pattern.
-Can flow (change shape)- when not moving it will have a level surface
Change to a Liquid
-Heat is added (to a solid)- Motion / Temp
- particles can’t stay in crystal pattern
Change to a Liquid
Melting point- the temperature at which a solid becomes a liquid
- each crystalline solid has its own melting point Mercury = -39 oC
Salt = 801 oC
Sugar = 186 oC
Water = 0 oC
Change to a Liquid
Heat of fusion- the amount of heat required to change 1 gram of solid to a liquid
- the energy used to break the crystalline structure
(at the same temp
no temp change)
Sublimation
- Changing from a Solid Gas
Ex. Dry ice
Change to a Gas- In most liquids (at ordinary Temps.) Some molecules have enough energy to (escape and) become a gas
Ex. Water evaporation
Heat = evaporation
Boiling point –The Temp (at ordinary pressure) at which the molecules of a liquid have enough energy to become a gas
Exact boiling point depends on:
1. Energy needed to make particles separate
2. Pressure of the air pressure = boiling point pressure = boiling point
- Water (at normal pressure) will never be hotter than 100oC
Heat of Vaporization-The amount of heat required to change 1 gram of liquid to a gas (No temperature change)
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