Matter, Properties, and Separation Techniques Flashcards

Matter: Anything that has mass and takes up space.
Pure Substance: Matter with distinct properties and a composition that does not vary between samples (e.g., salt $NaCl$ , water $H_2O$ ).
- Element: Substance that cannot be decomposed into simpler substances, composed of only one kind of atom (e.g., Magnesium, Carbon).
- Compound: Substance composed of two or more elements chemically combined (e.g., Potassium Fluoride, Carbon permanganate).
Mixture: Combination of two or more substances in which each substance retains its chemical identity.
- Solution (Homogeneous): Uniform mixture where components cannot be distinguished even under a microscope (e.g., Saltwater, Brass, Black coffee).
- Suspension (Heterogeneous): Mixture with particles larger than 1000\n,nm (1\n,\nmu m) that do not dissolve and settle out under gravity over time.
- Colloid: Mixture with particle sizes between 1\n,nm and 1000\n,nm (1\n,\nmu m) that remain suspended without settling (e.g., Milk, Mayonnaise).

Scalar Quantity: Numerical value of a physical magnitude with a unit.
Precision: Measure of how closely individual measurements agree with one another.
Accuracy: Measure of how closely individual measurements agree with the correct or true value.
Physical Properties: Characteristics observable without changing the composition of matter (e.g., luster, solubility, malleability, ductility, color, viscosity).
Chemical Properties: Characteristics describing how matter changes into another type of matter (e.g., flammability, toxicity, reactivity, acidity).
Extensive Properties: Physical properties that depend on the amount of substance present (e.g., mass, weight, volume).
Intensive Properties: Properties independent of the amount of substance present (e.g., melting point, boiling point, electrical conductivity, heat conductivity).

Nucleus: Central core containing positively charged protons and neutral neutrons.
Electrons: Negatively charged particles surrounding the nucleus.
Atomic Number: Equals the number of protons (or electrons in a neutral atom): \ntext{Atomic Number} = \ntext{Protons}
Atomic Mass: Sum of protons and neutrons: \ntext{Atomic Mass} = \ntext{Protons} + \ntext{Neutrons}

Kinetic Theory of Matter: Explains the physical states of matter (solid, liquid, gas) based on the concept that matter is composed of tiny particles in constant motion.
Kinetic Energy: Energy of motion, measured in Joules ( $J$ ).
Gases: Highly compressible states of matter with large amounts of space between particles (e.g., atmosphere contains 20\n% oxygen $O_2$ ).

Physical Change: Changes physical appearance without altering chemical composition.
Chemical Change: Transforms a substance chemically into a new substance.
Filtration: Uses a paper filter to separate a solid from a liquid.
Distillation: Separates homogeneous mixtures (liquid-liquid or solid-liquid) through boiling and condensation.
Chromatography: Separates mixtures based on differing abilities of substances to adhere to solid surfaces.
Gradiation (Sieving): Mechanical method separating solids based on particle size.
Decantation: Separates immiscible liquids or solid-liquid mixtures based on density differences.
Sublimation: Separates solid mixtures by converting one solid directly to gas.
Magnetic Separation: Uses a magnet to separate a magnetic solid from a solid mixture.
Evaporation: Separates liquid components from solid components in a mixture.

Law of Conservation of Matter: Mass is neither created nor destroyed in a chemical reaction: \ntext{Mass}_{\ntext{Reactants}} = \ntext{Mass}_{\ntext{Products}}
Example: $CH_4 + 2O_2 \nrightarrow CO_2 + 2H_2O$ 16\n,g + 64\n,g = 80\n,g