CLASSIFICATION of MATTER

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CLASSIFICATION ofMATTER
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What is matter?

• Matter is anything that has mass and takes up
  space.

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Matter

• Anything that has both mass AND volume
• MASS
• A measure of the amount of matter contained in an
  object
• VOLUME
• A measure of the amount of space an object takes
  up
• Substances
• Matter that has a uniform and unchanging chemical
  composition
• EX. Water (H2O) Table salt (NaCl)

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Properties of Matter

• How It Looks (Shiny ,Dull, Color, etc.)
• How It Feels (Hard, Soft, Rough , Smooth, etc.)
• How It Smells (Sweet, Sharp, Terrible, No Smell,
  etc.)
• How It Sounds (Loud, Soft, Echo, No Sound, etc.)
• What It Does (Bounce, Stretch, Tear, Break,
  Magnetism etc.)

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Physical Properties of Matter

• A characteristic that can be observed or measured
  without changing the samples composition
• Also used to describe pure substances
• There are two types of physical properties
• EXTENSIVE PROPERTIES
• dependent on the amount of the substance present
• INTENSIVE PROPERTIES
• NOT dependent on the amount of the substance
  present

DENSITY
LENGTH
VOLUME
MASS
COLOR
ODOR
TASTE
HARDNESS
MELTING POINT
BOILING POINT
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Chemical Properties of Matter

• Ability OR inability of a substance to combine
  with or change into one or more other substances

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Identify Properties

• Classify each of the properties below into either
  PHYSICAL or CHEMICAL

PHYSICAL
CHEMICAL
melting point of 97.81C
bright, silvery metal
decomposes it to evolve hydrogen and form the
hydroxide
floats on water
may ignite spontaneously on water
soft
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5 States of Matter

• Solids
• Liquids
• Gases
• Plasma
• Bose-Einstein Condensate (This one only happens
  in a lab within a few billionths of a degree
  above absolute zeroso, yeah. You wont see this
  unless you are in a lab

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SOLIDS
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SOLID

• A solid is matter that has that has definite size
  and shape.
• Example Put a sneaker in a box. It stays the
  same.

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States of Matter

• Solid
• Form of matter that has its own definite shape
  and volume
• Particles within a solid are tightly packed
• When heated, it will expand only slightly
• Cannot be compressed
• Low Kinetic Energy (KE)

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Liquids
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LIQUID

• A liquid takes the shape of any container.
• Example Pour juice into a glass. The juice
  will take on the shape of the glass.

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States of Matter

• Liquid
• Form of matter that flows, has a constant volume,
  and takes the shape of its container
• Less tightly packed
• When heated, it will expand
• Is virtually incompressible
• Moderate Kinetic Energy (KE)

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GAS
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Gas

• Gas is matter that has no definite shape. Gases
  take the shape of whatever container they are in
  .
• Example The air all around us is a gas.

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States of Matter

• Gas
• Form of matter that flows to conform to the shape
  of its container and fills the entire volume of
  its container
• Very loosely packed
• When heated, it will expand and sometimes escape
• Easily compressed
• High Kinetic Energy (KE)
• Gas vs. Vapor
• Gas the state of matter
• Vapor gaseous state of a substance that is
  either a liquid or gas at room temperature
• BOTH liquids and gases are fluids because they
  flow

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Physical changes in matter

• A Physical change is a change in how matter
  looks, but not the kind of matter is it is.
• Tear
• Cut
• Folded
• Written
• Liquid
• Solid
• Gas
• Mixture
• Solution

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Physical Changes

• Changes that DO NOT alter the composition of a
  substance
• Physical changes are those that are causing a
  change in a physical property
• Examples
• Cutting paper
• Breaking a crystal

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PHYSICAL CHANGES
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Changes in States of Matter

• Changes in the state of matter are all PHYSICAL
  CHANGES as they do NOT alter the arrangement of
  the substance

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Chemical changes in matter

• New Matter is formed.
• Burning
• Rusting
• Cooking

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Chemical Changes

• Process that involves one or more substances
  changing into new substances
• a.k.a. Chemical reaction
• Reactants Starting substances
• Products Resulting substances
• Newly formed substances will have different
  compositions and properties than the original
  substances

Fe O ? FeO
Iron reacts with Oxygen to produce Iron Oxide
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CHEMICAL CHANGES
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Four Indications of a Chemical Change

1. release of a gas
2. release of heat, light or sparks
3. formation of a precipitate
4. color change

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Law of Conservation of Mass

• Mass is neither created nor destroyed, it is only
  rearranged.
• The total mass you have in the beginning of a
  reaction must be present at the end of the
  reaction
• Mercury Oxygen ? Mercury Oxide
• If there are 200g of mercury and 16g of oxygen,
  what mass of mercury oxide is produced.
• Mercury Oxygen ? Mercury Oxide
• 200g 16g
  ?
• 
  216g

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Is this a solid, a liquid, or a gas?Can you find
more than one type of matter in any of the
pictures?
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Is this a physical change or a chemical change?
Can you find more than one physical or chemical
change in the pictures?
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Lets watch a video clip about matter!

• States of Matter

Click to go to the next slide.
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Mixtures

• A combination of two or more pure substances in
  which each pure substance retains its own
  individual chemical properties
• physical combination
• can be separated physically
• has no definite ratio

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Mixtures versus Compounds
S
Fe
Physically mixed, can be separated by physical
means.
Chemically reacted, cannot be separated by
physical means.
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Elements

• A pure substance that cannot be separated into
  simpler substances by physical or chemical means.
• 91 occur naturally
• Allotropes- element is found in more than one
  form.
• Ex. Carbon- diamond graphite, Oxygen- O2 O3.
• Diatomic elements- found as a pair with itself
• Ex. O2, N2, F2, Cl2, H2, I2, Br2
• Expressed with a chemical symbol
• -one, two or three letters
• -only the first letter is capitalized
• -organized on the Periodic Table

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Periodic Table

• ?Horizontal rows-periods
• ??Vertical row-groups/family
• Elements in a group/family together have similar
  properties

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Compounds

• Chemical combination of two or more elements
• definite ratio
• can only be separated by chemical changes
• Compounds that occur naturally are more stable
  than the individual component elements.
• properties of a compound are different from the
  properties of the elements that make it
• Water
• aspirin
• sugar
• NaCl (salt)
• NH3 (ammonia)
• HCl (hydrochloric acid)
• Fe2O3 (Iron III Oxide)