Introduction to Matter and its Properties

Introduction to Matter

• Chemistry defines matter as anything that possesses mass and occupies space.
• This definition separates the chemistry term from the use of "matter" when speaking of conflict.
• Living and non-living things fall under matter.

Properties of Matter

• The focus is on physical properties, with chemical properties discussed in a later chapter.
• Matter consists of tiny particles called atoms.
• Atoms are too small to be seen by a normal microscope, needing a high-powered one.
• Potassium Permanganate (KMnO4) demonstrates that matter comprises tiny particles.
• A small crystal of KMnO4 is put in water, turning it purple, and serially diluted.
• Even after several dilutions, the color persists, implying one crystal contains millions of tiny particles.
• Matter's particles have space between them.

Properties of Matter - Spaces in Between

• Dissolving salt or sugar in water without increasing the water level exemplifies spaces between water molecules.
• The dissolved product's molecules fit into these spaces.
• The "Chintu Lal and Mintu Lal" example illustrates the "molecules making space for each other" analogy.
• Matter's Particles Are in Constant Motion is exemplified by perfume sprayed at one point of a room being smelled across the room due to the constant motion of gas particles.

Properties of Matter - Constant Motion

• Diffusion: the mixing of a substance with another due to the motion of particles in solid, liquid, or gas.
• Diffusion occurs fastest in gases and slowest in solids.
• Kinetic Energy: The energy possessed by a moving particle.
• Faster kinetic energy means faster diffusion.
• Higher temperature means higher kinetic energy and thus faster diffusion, showing diffusion depends on kinetic energy.
• The faster smell of cooking food compared to cooled food is due to higher temperature, thus higher kinetic energy and faster diffusion.

Properties of Matter - Attract Each Other

• Matter's particles attract each other with a force, keeping the molecules together.
• Evidence of this is easier hand displacement in air versus water, and impossibility in ice.
• The force of attraction is greatest in solids, less in liquids, and least in gases.

Properties of Matter Overall

• Matter is made up of very small particles.
• Matter has spaces in between.
• Matter is constantly moving.
• Matter's particles attract each other.
• All four properties can be demonstrated by a test.

States of Matter - Solid, Liquid, Gas

• The states of matter are solid, liquid, and gas.
• Properties such as space between particles, force of attraction, particle arrangement, shape, volume, compressibility, Kinetic Energy, and Movement are compared in a table.

States of Matter - Space Between Particles

• Gases have the greatest space between particles.
• Solids have the least space between particles.
• Liquids fall between solids and gases in terms of space between molecules.

States of Matter - Force of Attraction

• Solids have the greatest force of attraction.
• Gases have the least force of attraction.
• Liquids fall between solids and gases in terms of force of attraction.

States of Matter - Particle Arrangement

• Solids have particles closely arranged.
• Liquids have loosely arranged particles.
• Gases have very loosely arranged and scattered particles.
• Analogy: students in line for morning assembly (solid) vs. students at lunch (liquid) vs. at day's end (gas).

States of Matter - Shape

• Solids have a fixed shape.
• Liquids take the shape of their container.
• Gases have no definite shape.

States of Matter - Volume

• Solids have a fixed volume.
• Liquids have a fixed volume.
• Gases have no fixed volume.

States of Matter - Compressibility

• Solids are non-compressible.
• Liquids have almost negligible compressibility.
• Gases have high compressibility.

States of Matter - Kinetic Energy

• Solids have the least kinetic energy.
• Liquids have moderate kinetic energy.
• Gases have the highest kinetic energy.

States of Matter - Movement

• Solids have very little movement, restricted to the same place.
• Liquids exhibit some movement.
• Gases have a lot of free movement.

States of Matter - Gases

• Gases exert pressure on their container walls, often overlooked.
• Gas molecules move with a lot of kinetic energy in random motion, hitting the container walls.

States of Matter - Rubber Bands

• Rubber bands can change shape, but are actually solid.
• They can stretch (elasticity) but return to their original shape, proving they remain solid.

States of Matter - Salt and Sugar

• Salt and sugar take the shape of a jar when poured in, but are solids.
• Solid salt/sugar are made of granules or pieces, small enough to arrange in this way.
• The jar isn't filled to volume, so it's the arrangement of solid granules, not a liquid substance.

States of Matter - Sponges

• Sponges can be compressed and have volume reduced, but are solid.
• Sponges are solids with air trapped inside holes, and compression pushes the air out, reducing volume.

States of Matter - Plasmas

• Plasma is a fourth state of matter with very large amounts of energy.
• Plasmas are so energetic that their matter disassociates from structure.
• The sun and stars exist in a plasma state.
• Manmade plasma occurs in neon sign boards.

States of Matter - Bose-Einstein Condensate

• The Bose-Einstein Condensate is a state achieved when a gas is cooled to very low temperatures at very low densities.

Temperature

• The SI unit of temperature is Kelvin (K), not Celsius (°C).
• Celsius to Kelvin conversion: K = °C + 273.
• Kelvin to Celsius conversion: °C = K - 273.
• Absolute zero is 0 K, which is -273 °C.
• Example conversions: 293 K = 20 °C, and 470 K = 197 °C.

Change in Matter State

• Matter may shift between solid, liquid, and gas through temperature and/or pressure.

Change in Matter State - Temperature

• Solid to liquid: Fusion.
• Liquid to gas: Vaporization.
• Gas to liquid: Condensation.
• Liquid to solid: Solidification.
• Solid to gas: Sublimation, bypassing the liquid state entirely.
• Gas to solid: Deposition.
• State changes due to temperature happen as heat increases the kinetic energy in the molecules.
• Vibration speed breaks the force of attraction keeping a certain state together, changing the state.

Change in Matter State - Temperature Cont.

• Melting Point: Temperature at which a solid becomes a liquid (e.g., 0 °C for ice).

Change in Matter State - Latent Heat

• Latent Heat of Fusion: Additional energy input turns solid (ice) at 0°C to liquid (water) at 0°C, because the energy transforms the state, not the temperature.
• Boiling Point: Temperature at which a liquid becomes a gas (e.g., 100 °C for water).
• Latent Heat of Vaporization: Continued heating past 100°C turns water to vapor but remains at 100°C as energy turns water to vapor.
• Sublimation: Solid changes directly to a gas (e.g., naphthalene balls).
• Latent Heat of Fusion: Heat needed to change 1 kg of substance from solid to liquid.
• Latent Heat of Vaporization: Heat needed to change 1 kg of substance from liquid to gas.
• Test Question: If ice at 0°C is melted, the water remains 0°C; the heat was used to change the state.
• Temperature breaks down solid molecular shapes in the water example.
• It provides kinetic energy and facilitates movement.

Change in Matter State - Pressure

• Pressure typically functions inversely to heat.
• To go from solid to gas, either heat the solid or reduce pressure.
• Gases can be turned to liquid by increasing pressure.

Change in Matter State - Dry Ice

• Dry Ice: Carbon Dioxide solidified by extreme changes.
• It's frozen as a solid and stored in high pressure to prevent gassing off.

Change in Matter State - Evaporation

• Evaporation: When a liquid becomes a gas from the surface below the boiling point.
• This happens when molecules gain energy from their surroundings.
• It happens on the surface because the molecules are freed there.

Key Factors Affecting Evaporation

• Increased temperature accelerates evaporation.
• Larger surface area (e.g., a puddle) facilitates evaporation.
• Lower humidity means easier evaporation.
• Wind speed affects evaporation speed due to increased rate.

Cooling Due To Evaporation

• Evaporation causes cooling, as water absorbs heat from the surroundings, decreasing the overall temperature.
• This is known as the latent heat of vaporization, in which it loses its force of attraction.
• Example: Indian clay pot with small pores allows liquid to come out and evaporate, cooling the liquid as water carries away heat.
• Cotton clothes have more pores, causing sweat to evaporate and cool the body.

Review - What about the cold water drops

• Cold water drops appear along container by condensing water vapor in the air, not leaking.

Review - Evaporation Vs. Boiling

• Evaporation happens on the liquid surface; boiling happens throughout.
• Evaporation is slow; boiling is intense.
• Evaporation causes a cooling effect; boiling is a heating effect.

Review and Q&A

• Example question: Boiling point of alcohol in Kelvins (simple math).
• Evaporation always leads to cooling.
• Transfer of K permanganate without stirring in water exemplifies diffusion.
• Gas can be turned into liquid by low temperature and high pressure.
• High temperature (in °C) causes expansion and diffusion.

Chapter Conclusion

• Solid = Be strong.
• Liquid = Be flexible.
• Gas = Expand and dream big.
• Trust yourself.