Grade 10 Chemistry Vocabulary Review

Comprehensive vocabulary review flashcards covering key definitions, principles, processes, and chemical classification concepts across Grade 10 Chemistry.

Physical Change

A change that does not involve the formation of a new substance with a new chemical composition.

Chemical Change

A change that results in the formation of one or more new substances with new chemical compositions.

Chemical Equation

A shorthand representation of an actual chemical reaction using chemical symbols and formulas.

Stoichiometry

The quantitative study of reactants and products and their relationships in a chemical reaction.

Combination Reaction

A reaction in which two or more pure substances react directly to form a single new substance.

Decomposition Reaction

A reaction that involves the breaking down of a single compound into two or more simpler elements or compounds.

Single Displacement Reaction

A reaction in which a more reactive element displaces another element from its compound.

Double Displacement Reaction

A reaction in which two compounds react together to form two new compounds by exchanging their positive and negative ions.

Oxidation

The loss of one or more electrons by an atom, corresponding to an increase in its oxidation number.

Reduction

The gain of one or more electrons by an atom, corresponding to a decrease in its oxidation number.

Oxidizing Agent

A substance that gains electrons, causes another substance to be oxidized, and is itself reduced.

Reducing Agent

A substance that loses electrons, causes another substance to be reduced, and is itself oxidized.

Avogadro's Number

The number of entities contained in exactly $12\,g$ of carbon-12, equal to $6.022 \times 10^{23}$.

Molar Mass

The mass in grams of one mole of a substance, numerically equal to its molecular mass or formula mass.

Empirical Formula

The formula of a chemical compound written with the smallest whole-number ratio of subscripts.

Molecular Formula

A chemical formula that specifies the exact number of atoms of each element present in a molecule.

Limiting Reactant

The reactant that is completely consumed first in a chemical reaction, limiting the amount of product that can be formed.

Theoretical Yield

The calculated quantity of product that would be obtained if a chemical reaction proceeds completely to completion.

Actual Yield

The measured quantity of product experimentally obtained from a chemical reaction.

Percentage Yield

The ratio of actual yield to theoretical yield multiplied by $100\%$, calculated as $\text{Percentage Yield} = \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100\%$.

Solution

A homogeneous mixture composed of a solute dissolved uniformly in a solvent.

Suspension

A heterogeneous mixture in which fine solid particles are dispersed throughout a liquid or gas without dissolving.

Colloid

A heterogeneous mixture containing insoluble particles ranging from $1\,nm$ to $100\,nm$ in diameter suspended uniformly throughout a continuous medium.

Tyndall Effect

The scattering of a beam of light by colloidal particles, rendering the light path visible through the mixture.

Saturated Solution

A solution that is at equilibrium and contains the maximum amount of dissolved solute at a given temperature in the presence of undissolved solute.

Unsaturated Solution

A solution containing less solute than its capacity to dissolve at a specific temperature.

Supersaturated Solution

A solution that temporarily contains more dissolved solute than a saturated solution at the same conditions.

Henry's Law

A law stating that the solubility ($C$) of a gas in a liquid is directly proportional to the partial pressure ($P$) of the gas above the liquid ($C = kP$).

Molarity

The concentration of a solution expressed as the number of moles of solute per liter ($1\,dm^3$) of solution ($\text{Molarity} = \frac{\text{moles of solute}}{\text{liters of solution}}$).

Molality

The concentration of a solution expressed as the number of moles of solute dissolved per kilogram of solvent ($\text{Molality} = \frac{\text{moles of solute}}{\text{kilograms of solvent}}$).

Normality

The concentration of a solution expressed as the number of gram equivalent weights of solute per liter ($1\,dm^3$) of solution.

Acidic Oxide

An oxide formed by the combination of oxygen with a non-metal that reacts with water to form an acid (acid anhydride).

Basic Oxide

An oxide formed by a metal and oxygen that reacts with water to form a base or with acids to form a salt and water.

Amphoteric Oxide

An oxide that displays both acidic and basic properties, reacting with both strong acids and strong bases to produce salt and water.

Neutral Oxide

An oxide that shows neither acidic nor basic properties and does not react with acids or bases to form salts.

Peroxide

A compound containing oxygen in an oxidation state of $-1$ and characterized by a covalent $-\text{O}-\text{O}-$ linkage.

Arrhenius Acid

A substance that releases hydrogen ions ($H^+$) or hydronium ions ($H_3O^+$) when dissolved in an aqueous solution.

Arrhenius Base

A substance that produces hydroxide ions ($OH^-$) when dissolved in an aqueous solution.

Monoprotic Acid

An acid capable of releasing only one ionizable hydrogen ion ($H^+$) per molecule in aqueous solution.

Polyprotic Acid

An acid that yields more than one ionizable hydrogen ion ($H^+$) per molecule in aqueous solution.

pH

A logarithmic scale measuring acidity, defined as the negative common logarithm of hydrogen ion concentration ($\text{pH} = -\log[H^+]$).

Normal Salt

A salt produced by the complete replacement of all ionizable hydrogen ions ($H^+$) of an acid by a metal or ammonium ion.

Acidic Salt

A salt formed by the partial replacement of ionizable hydrogen ions ($H^+$) of a polyprotic acid by metal or ammonium ions.

Basic Salt

A salt containing unreplaced hydroxide ions ($OH^-$) resulting from incomplete neutralization of a polyhydroxy base by an acid.

Exothermic Reaction

A chemical reaction that releases energy in the form of heat to its surroundings, resulting in $\Delta H < 0$.

Endothermic Reaction

A chemical reaction that absorbs heat energy from its surroundings, resulting in $\Delta H > 0$.

Electrochemistry

The branch of chemistry dealing with the relationship and interconversion between chemical energy and electrical energy.

Galvanic Cell

An electrochemical cell that converts chemical energy into electrical energy through a spontaneous redox reaction.

Electrolytic Cell

An electrochemical cell that utilizes electrical energy from an external voltage source to drive a non-spontaneous chemical reaction.

Salt Bridge

A tube filled with an electrolyte gel connecting two half-cells in a voltaic cell to maintain electrical neutrality.

Metallurgy

The science and industrial technology of extracting metals from their ores and preparing useful alloys.

Gangue

The commercially worthless earthly impurities, such as sand, clay, and soil, mixed with a mineral ore.

Ore

A naturally occurring solid material or mineral from which a metal can be extracted profitably.

Alloy

A mixture composed of two or more metals, or a metal and a non-metal, combined while molten.

Hall-Héroult Process

The industrial electrolytic method used to extract pure aluminum metal by electrolyzing alumina ($Al_2O_3$) dissolved in molten cryolite ($Na_3AlF_6$).

Blast Furnace

A tall metallurgical furnace used to reduce iron ores with coke, limestone, and hot air to produce pig iron.

Slag

A waste glass-like byproduct formed when flux reacts with silica and other impurities during metal smelting (e.g., $CaSiO_3$).

Allotropy

The phenomenon in which an element exists in two or more distinct physical or structural forms in the same physical state.

Frasch Process

An industrial extraction method that uses superheated water and compressed air to melt and lift elemental sulfur from underground deposits.

Organic Chemistry

The study of carbon-containing compounds, excluding simple oxides, carbonates, hydrogen carbonates, cyanides, and cyanates.

Hydrocarbon

An organic compound consisting entirely of hydrogen and carbon atoms.

Homologous Series

A group of organic compounds sharing the same functional group and general formula, where consecutive members differ by a $\text{-CH}_2-$ unit.

Structural Isomers

Compounds having identical molecular formulas but differing in the order or way their atoms are connected.

Alkane

A saturated hydrocarbon containing only single covalent bonds between carbon atoms, with the general formula $C_n H_{2n+2}$.

Alkene

An unsaturated hydrocarbon containing at least one carbon-carbon double bond, with the general formula $C_n H_{2n}$.

Alkyne

An unsaturated hydrocarbon containing at least one carbon-carbon triple bond, with the general formula $C_n H_{2n-2}$.

Aromatic Hydrocarbon

A unsaturated hydrocarbon possessing a stable benzene ring or related cyclic resonance structure.

Cracking

The industrial process of decomposing large, heavy hydrocarbon molecules into smaller, more useful hydrocarbons using high heat or catalysts.