Grade 10 Chemistry Lecture Review

Comprehensive vocabulary flashcards covering the key principles of the Grade 10 Chemistry curriculum, including history, matter, stoichiometry, electrochemistry, kinetics, and biochemistry.

Stoichiometry

The study of relative amounts of substances involved in a chemical reaction based on a balanced chemical equation.

Scientific Paradigm

A theoretical model, set of ideas, or rules that guide scientists in their research and help explain the natural world.

Repeatability

The idea that scientific results from experiments should be possible to verify by conducting the experiment again under the same physical conditions and equipment.

Reproducibility

The ability to produce the same or similar results when a measurement is made under different conditions, by a different method, or in a different laboratory.

Plum Pudding Model

A 1904 atomic model by J.J. Thomson suggesting atoms are negatively charged electrons (plums) scattered in a positively charged soup (pudding).

Confidence Intervals

Tools used to measure the precision of a measurement; for example, a 95% confidence interval indicates that the true value is 95% likely to be within a specific range.

P-values

A statistical tool to check if results are meaningful; a value of 0.01 indicates only a 1% chance the result is random.

Bayesian Probability

A method in chemistry used to update the likelihood of a hypothesis by combining previous data with new evidence.

Internal Energy

The total energy of a substance composed of temperature-related kinetic energy and potential energy derived from particle positions and interactions.

Sublimation

The process in which molecules of a solid state go directly to the vapor state without passing through the liquid phase.

Deposition

The phase transition where a gas turns directly into a solid without passing through the liquid phase.

Latent heat of fusion

The absorbed heat energy used to overcome intermolecular forces holding a solid together during melting, occurring at a constant temperature.

Boyle's Law

States that for a fixed amount of gas at a constant temperature, the volume is inversely proportional to its pressure: $PV = ext{constant}$.

Charles's Law

States that for a fixed amount of gas at constant pressure, the volume of a gas is directly proportional to its absolute temperature: $rac{V}{T} = ext{constant}$.

Avogadro's Law

States that for a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas.

Graham's law of diffusion

States that the rate of diffusion is inversely proportional to the square root of the molar mass of the gas particles: ext{Rate} imes rac{1}{ ext{molar mass}}.

Mole

The SI unit to express the amount of a substance, represented by the atomic mass, formula mass, or molecular mass of a substance expressed in grams.

Molar Volume

The volume occupied by one mole of any gas at RTP ($25^ ext{o}C$ and $1 ext{ atm}$), which is $24,dm^3$.

Limiting reactant

The reactant that is completely consumed in a reaction and produces the lowest amount of product.

Theoretical Yield

The amount of product as calculated from a balanced chemical equation.

Molarity (M)

A concentration unit defined as the number of moles of solute dissolved per $dm^3$ of solution ($mol/dm^3$).

Electrolysis

The decomposition of ionic compounds in a molten state or aqueous solution by the passage of an electric current.

Galvanic Cell

An electrochemical cell that involves a spontaneous redox reaction to generate electricity, such as the Daniel Cell.

Electrochemical Series

A table showing the arrangement of metals based on their increasing reduction potentials.

Haber Process

The industrial process used to produce ammonia ($NH_3$) from nitrogen and hydrogen using an iron catalyst at $450^ ext{o}C$ and $200 ext{ atm}$.

Contact Process

The industrial method for manufacturing sulphuric acid ($H_2SO_4$) via the catalytic oxidation of $SO_2$ using vanadium(V) oxide.

Collision Theory

States that for a reaction to occur, particles must collide with sufficient energy (activation energy) and correct orientation.

Activation energy

The smallest or minimum amount of kinetic energy required for interacting particles to undergo a chemical reaction.

Amphoteric oxides

Oxides that can react with both acids and bases to produce salt and water, such as $Al_2O_3$ and $ZnO$.

Photochemical Smog

A type of air pollution formed when sunlight reacts with nitrogen oxides ($NO_x$) and unburned hydrocarbons to produce pollutants like PAN.

Cracking

The process of breaking down large alkane molecules into smaller hydrocarbons, including alkenes, using high temperature and a catalyst.

LPG (Liquefied Petroleum Gas)

The refinery gas fraction of petroleum consisting of hydrocarbons with 1-4 carbon atoms, used for heating and cooking.

Esterification

The reaction between a carboxylic acid and an alcohol in the presence of an acid catalyst to form a sweet-smelling ester and water.

Polymers

Large molecules built up from many smaller repeating units called monomers.

Nylon-6,6

A synthetic polyamide formed by the condensation polymerization of hexamethylenediamine and adipic acid.

Peptide bond

The specific amide linkage ($-NH-CO-$) that joins amino acid units together to form proteins.

Genetic Engineering

A process using laboratory-based technologies to manipulate and modify the genetic material (DNA) of an organism.