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States of Matter Powerpoint Presentation
1.
2. What is Matter?
Matter is anything that has mass and volume.
Matter consists of states, which are four physical forms of matter.
Two properties of matter:
1. Extensive- depends on the amount of matter in the sample
Example: volume, mass, length
2. Intensive- matter depends only on the type in the sample
Example: color, density, boiling/melting point, hardness
3. Law of Conservation of Mass
Matter is neither created nor destroyed; it is simply transformed into something
else
Example: Coal is transformed to generate electricity.
4. States of Matter and Their Characteristics
Solid Liquid Gas
● Has a fixed shape that does
not conform to the container
● Has a definite volume
● Particles of a solid have low
kinetic energy. The atoms are
in motion (small vibrations),
but are in a fixed position
● Varying shape that conforms
to the shape of the container
● Cannot be compressed
● Definite volume
● Particles of a liquid have
greater kinetic energy.
Particles are close together,
but disorganized.
● No definite shape or volume.
Conforms to the shape of the
container.
● Pressure reduces space
between gas particles.
● Particles of a gas have a high
kinetic energy and will spread
out indefinitely.
6. Fourth State of Matter…… PLASMA!
● Most common state of matter in the universe
● Requires a massive amount of energy to ionize particles to the plasma state
● Similar to gases, but the atoms are “stripped” and move around freely as ions
(atoms with charges)
● Highly charged particles have an extremely high kinetic energy.
7.
8. Phase Diagram
A phase diagram is a graph that shows the conditions required (specific pressure
and temperature) for a substance to exist as a solid, liquid, or gas.
9. Characteristics of the Phase Diagram
Phase Transitions:
1. Solid→ Liquid is melting.
2. Liquid→ Solid is freezing.
3. Liquid→ Gas is evaporation.
4. Gas → Liquid is condensation.
5. Solid → Gas is sublimation.
6. Gas→ Solid is deposition.
10. Physical and Chemical Changes
Physical property- a characteristic shown by a substance itself, without interacting
with or changing into other substances
Physical change- a change in which the physical form of a substance, but not its
composition, is altered
Chemical property- a characteristic of a substance that appears as it interacts
with, or transforms into, other substances
Chemical change- a change in which one or more substances are converted into
one or more substances with different composition and properties
12. Physical Changes
Examples:
● Popsicle melting on a hot, summer day.
● Ripping a piece of paper into two pieces.
● Chopping wood to build a fire.
● Painting your fingernails with nail polish.
● Boiling water on the stove top.
● Making a sugar solution.
13. Chemical Changes
Examples:
● Burning wood.
● Baking a birthday cake.
● The process of digesting food.
● Making a salt water solution.
● Lighting fireworks during a celebration.
● The decomposition of food.
15. Pure Substances-Elements
Element- building blocks of matter; consists of only one type of atom
● Cannot be broken down through physical or chemical means
● Each element is unique because its atoms have unique properties
● Elements are classified metals, nonmetals, or metalloids.
Metals Nonmetals Metalloids
Solids at room temperature
(except Hg), lustrous,
malleable, ductile, good
conductors, hard, and high
boiling/melting points
Generally solids and gases
at room temperature
(except Br), poor
conductors, non-malleable,
etc. (Opposite of metals)
Solids at room temperature,
properties are a mixture of
metals and nonmetals
17. Pure Substances- Compounds/Molecules
Compound- substance composed of two or more different elements
Examples: H2O, NaCl, CH4, CaCl2
Molecule- composed of two or more atoms of an element joined together
Examples: H2O, diatomic molecules
*All compounds are molecules, but not all molecules are compounds*
18. Pure Substances- Compounds/Molecules Cont’d
Monatomic particles- substances composed of particles containing single atoms
Example: Noble gases (He, Ne, Ar, Kr, Xe)
Diatomic particles- composed of molecules containing two atoms bonded to each
other. They can consist of the same element or two different elements.
Examples: HCl, diatomic molecules, CCl4
The Super 7- H2, N2, F2, O2, I2, Cl2, Br2
*They only exist as diatomic molecules when they are not bonded to other
elements*
19. Mixtures- Homogeneous
Mixture- two or more substances are combined that can be separated by chemical
means or physically separated
Homogeneous mixture- substances are evenly distributed throughout the mixture
(components not visible)
Types of heterogeneous mixtures:
1. Colloids-small particles of one substance is evenly distributed throughout
another substance; particles are suspended in a solution and not fully
dissolved
2. Solutions- solute is dissolved into the solvent
22. Mixtures- Heterogeneous
Heterogeneous mixture- substances in the mixture are not evenly distributed
(components are visible)
Types of heterogeneous mixtures:
1. Suspensions- mixture between a liquid and particles of a solid; particles are
suspended throughout the liquid. A key characteristic is that the solid particles
will settle and separate over time.
