Matter Classification and States of Matter

Matter Classification

• Matter is anything with mass and occupies space.
• Classified as either pure substances or mixtures.
• Composed of tiny particles.
• Chemistry is the study of matter and its changes.

Particle Theory

• Explains physical characteristics of matter.
• Matter is composed of particles.
• Particles have spaces between them.
• Particles attract each other.
• Gas temperature affects particle speed.
• Particles constantly move due to kinetic energy.
• Particle properties are identical in one substance.

States of Matter

• Solids: Particles close together, strong attraction, fixed shape and volume, locked in a pattern, vibrate in place.
• Liquids: Particles farther apart, less attraction, able to slide past each other, larger spaces between particles than solids.
• Gases: Particles far apart, weak attraction, no fixed shape or volume, expand to fill container.

Particle Theory of Different States

• Solids: Particles held tightly together, slow movement, vibrate.
• Liquids: Particles close together, move in all directions, can't move far due to attraction.
• Gases: Particles have minimal attraction, move rapidly in all directions, collide with each other and container.

Atoms vs. Molecules

• Atoms: Smallest particles, indivisible, building blocks of matter.
  • Elements are either single atoms or multiple identical atoms bonded
• Molecules: Groups of atoms bonded together.
• Compound: a molecule of two or more different elements bonded together.

Pure Substances

• Elements or compounds.
• Consist of only one element or compound.
• Examples: Hydrogen, water, sugar, salt, baking soda, aluminum, gold.

Mixtures

• Two or more types of elements or compounds.
• No chemical reaction between particles.
• Retain individual properties.
• Can be separated by physical means.
• Mixtures can be homogenous or heterogeneous.

Heterogeneous Mixtures

• Different types of particles are visible.
• Not uniform in composition.
• Examples: Cereal in milk, oil and water.
• Components can be separated easily.

Homogenous Mixtures

• Looks like one type of particle, uniform mixtures.
• Particles are evenly distributed and arranged.
• Examples: Apple juice, sugar and water, blood, sports drinks.
• Composition remains the same throughout.

Mixtures: Mechanical Mixtures

• Heterogeneous mixtures, distinct components visible after mixture forming.
• Examples: Salad, asphalt (gravel, sand, and bitumen), oil and vinegar dressing.
• Each component retains its properties

Solutions

• Homogenous mixtures.
• Solute dissolves into solvent.
• Solute: substance dissolved.
• Solvent: substance doing the dissolving.
• Examples: Saltwater (salt as solute, water as solvent).

How Solutions Form

• Particles of one substance are more attracted to another than themselves.
• Solute particles break away and evenly fill the spaces in the solvent particles.
• Dissolving is the process.

Water as a Solvent

• Universal solvent—water dissolves many substances.
• Important for transporting nutrients/chemicals.
• Makes up 70% of human bodies.
• Pollution occurs when solutes contaminate water.

Solid Solutions

• Solutions with both solid solute and solvent.
• Example: 14 karat gold (14 parts gold, 10 parts other metals).

Universal Solvent – Water

• Water's chemical composition makes it a good solvent.
• Two hydrogen atoms and one oxygen atom.
• Positive electrical charge on hydrogen side, negative on oxygen side.
• This charge allows water to attract many different types of molecules.

Solutions - Dissolving Salt in Water

• Water molecules break down and dissolve salt molecules.
• Positive sodium and negative chloride atoms separate in water.
• These attract to water molecules, forming new saltwater molecules.

Insoluble Substances

• Some substances, like oil, do not dissolve in water.
• Atoms in insoluble substances are strongly attracted/bonded.

Factors Affecting Solubility

• Concentration: Higher concentration means less solubility.
• Temperature: Increased temperature usually increases solid solubility and decreases gas solubility.
• Pressure: Increased pressure usually increases gas solubility.
• Size: Smaller solute particles dissolve faster.

Concentration

• Measured qualitatively (words) or quantitatively (numbers).
• Concentrated: Large amount of solute, small amount of solvent.
• Dilute: Solution becoming less concentrated, more solvent added.

Solubility with Numbers

• Concentration expressed as grams of solute per milliliters of solvent
• Examples: 5g/500ml (1%/100ml), 50g/250ml (20%), 100g/250ml(40%), 25g/250ml (10%)

Kinetic Energy

• Energy of movement.
• Substances with higher temperature have more kinetic energy.
• Temperature is the average kinetic energy of substance particles.
• Increased heat transfers to lower temperature objects

Carbon Dioxide

• Colourless, slightly sour-smelling gas.
• 0.03% of atmosphere.
• Vital for plants.
• Formed from burning carbon-containing materials.
• Produced from mixing baking soda and vinegar.
• Forms carbonic acid in solutions.

Pure Substances - Elements/Compounds

• Needed for modern life but mining and refining create environmental problems.
• Often not found in nature in pure form so extraction is required.
• The refining process often involves acids which create water and air pollution.

Suspensions

• Liquid mixtures with solid particles that do not dissolve.
• Particles eventually settle.
• Examples: Sand in water, flour in water.

Colloids

• Even distribution of very small particles in another substance.
• Particles do not settle.
• Appear as solutions but are mixtures.
• Examples: Milk (butterfat in water), smoke.

Emulsions

• Heterogeneous mixtures of two or more immiscible liquids.
• One liquid forms tiny droplets within another.
• Examples: Oil and water emulsions.
• Classified into oil-in-water or water-in-oil
• Immiscible liquids do not mix well.

Saturation

• Unsaturated: Can hold more solute at a given temperature.
• Saturated: Cannot hold any more solute (without heating).
• Supersaturated: Saturated solution heated, more solute added, then cooled.

Explore the fundamental concepts of matter, including its classification into pure substances and mixtures. Learn about the particle theory that explains the physical characteristics of solids, liquids, and gases. This quiz will help reinforce key principles in chemistry related to the properties and behaviors of different states of matter.