The Characteristics of Matter. States of Matter Solid: Liquid: Gas: Plasma:

The Characteristics of

Matter

States of Matter

• Solid:

• Liquid:

• Gas:

• Plasma:

States of Matter

• Solid: definite volume & shape, hard to compress, dense

• Liquid:

• Gas:

• Plasma:

States of Matter

• Solid: definite volume & shape, hard to compress, dense

• Liquid: definite volume, takes shape of container, hard to compress, somewhat dense

• Gas:

• Plasma:

States of Matter

• Solid: definite volume & shape, hard to compress, dense

• Liquid: definite volume, takes shape of container, hard to compress, somewhat dense

• Gas: indefinite volume, fills container, easy to compress, not dense

• Plasma:

States of Matter

• Solid: definite volume & shape, hard to compress, dense

• Liquid: definite volume, takes shape of container, hard to compress, somewhat dense

• Gas: indefinite volume, fills container, easy to compress, not dense

• Plasma: like gas but ionized (with + or – charge)

Phase Changes (Changes of State) • Solid liquid: • Liquid solid:• Liquid gas: • Gas liquid:• Solid gas: • Gas solid: • Gas plasma: • Plasma gas:

Phase Changes (Changes of State) • Solid liquid: melting• Liquid solid: freezing (solidification)• Liquid gas: boiling (evaporation) • Gas liquid: condensation • Solid gas: sublimation• Gas solid: deposition • Gas plasma: ionization• Plasma gas: recombination

Phase Changes (Changes of State)

Phase Changes in Water

• Boiling point of water =

• Melting point of water =

• Freezing point of water =

Phase Changes in Water

• Boiling point of water = 373.15K

• Melting point of water = 273.15K

• Freezing point of water = 273.15K

Phase Changes in Water

• Boiling point of water = 373.15K

• Melting point of water = 273.15K

• Freezing point of water = 273.15K

• Notice that these are the same? They are interchangeable

The Kinetic Molecular Theory• Particles are always moving

• The more energy they have, the faster they move

• Heat is the measure of total kinetic energy

• Temperature is the average kinetic energy of all the molecules

The Kinetic Molecular Theory• Solid particles: closely packed (dense), low energy

and little space to move so they vibrate in place

• Liquids particles: more space and more energetic so they can flow (slide past each other)

• Gas particles: lots of space, most energetic and move freely within a container

Physical and Chemical Changes in

Matter

Physical Properties vs. Chemical Properties

• Properties that can be found without a chemical reaction (without creating a new substance)

• E.g. density, colour, hardness, malleability, ductility, lustre, viscosity, melting point, boiling point

• Describe the ability of a substance to undergo chemical reactions and change into new substances

• E.g. H2 can burn in air to produce H2O; H2 combines with Cl2 to form HCl

Physical Change

• Change in the shape or state of a substance

• No new substances formed (same chemicals)

• Reactants are the same as products

• Generally possible and easy to reverse

• E.g. changes in state (liquid water ice), changes in shape or volume

Physical Change

Chemical Change

• A change where new substances are formed

• Reactants are different from the products

• Difficult or impossible to reverse

• Often include changes in physical properties

• E.g. cooking an egg, burning a match

Chemical Change

Homework

• Read Hebden p.44-52• HW check on p.44 #13 and p.52 #33, 35-41, 44