Grade 10 Chemistry: Nomenclature, Reactions, Acids, and Bases

Comprehensive vocabulary flashcards covering chemical bonding, ionic and molecular nomenclature, chemical equations, reaction types, and the properties of acids and bases.

Ion

A charged particle that results when an atom gains or loses one or more electrons, forming either a cation or an anion.

Cation

A positively charged ion formed when an atom loses electrons.

Anion

A negatively charged ion formed when an atom gains electrons.

Ionic Compound

A compound formed between a metal and a non-metal (cations and anions) that typically has higher melting and boiling points and is a good conductor of electricity.

Molecular Compound

A neutral compound formed between two non-metals that interact by sharing electrons via one, two, or three pairs of bonds.

HOFBrINCl

A mnemonic representing the seven diatomic molecules: Hydrogen ($H_2$), Oxygen ($O_2$), Fluorine ($F_2$), Bromine ($Br_2$), Iodine ($I_2$), Nitrogen ($N_2$), and Chlorine ($Cl_2$).

Multivalent Ionic Compound

An ionic compound that contains a multivalent metal ion with more than one possible charge, indicated using Roman numerals (I, II, III, IV, V).

Zero Sum Rule

A method used to write chemical formulas for ionic compounds stating that the total positive charge and total negative charge must balance to zero.

Molecular Prefixes (1-10)

Numerical prefixes used to name molecular compounds: mono- (1), di- (2), tri- (3), tetra- (4), penta- (5), hexa- (6), hepta- (7), octa- (8), nona- (9), and deca- (10).

Reactants

Chemicals present and used at the start of a chemical reaction that are consumed during the reaction.

Products

Chemical substances produced during the course of a chemical reaction.

Word Equation

A chemical equation that uses the full names of the reactants and products rather than chemical formulas.

Skeleton Equation

An unbalanced chemical equation that uses chemical formulas to represent the reactants and products.

Law of Conservation of Mass

A scientific law stating that matter can neither be created nor destroyed in a closed system.

Synthesis Reaction

A type of chemical reaction where two or more reactants combine to form a single product: $A + B \rightarrow AB$.

Decomposition Reaction

A type of chemical reaction where a single compound breaks down into two or more simpler substances: $AB \rightarrow A + B$.

Single Displacement Reaction

A type of chemical reaction where an uncombined element displaces another element in a compound: $A + BC \rightarrow AC + B$ (for metals) or $A + BC \rightarrow BA + C$ (for non-metals).

Double Displacement Reaction

A type of chemical reaction where two compounds exchange elements or ions to form two new compounds: $AB + CD \rightarrow AD + CB$.

Complete Combustion

A hydrocarbon reaction with oxygen that always yields carbon dioxide and water ($\rightarrow CO_2 + H_2O$).

Acid

A chemical substance characterized by a sour taste, lower corrosiveness, a low pH (less than 7), the presence of $H^+$ ions, and the ability to turn blue litmus paper red.

Binary Acid

An aqueous acid composed of hydrogen and one other non-metal element, such as hydrofluoric acid ($HF_{(aq)}$) or hydrochloric acid ($HCl_{(aq)}$).

Oxyacid

An acid composed of hydrogen combined with a polyatomic oxyanion, such as acetic acid ($HC_2H_3O_{2(aq)}$), nitric acid ($HNO_{3(aq)}$), or sulfuric acid ($H_2SO_{4(aq)}$).

Base

A chemical substance characterized by a bitter taste, higher corrosiveness, a high pH (greater than 7), the presence of $OH^-$ ions, and the ability to turn red litmus paper blue.

Neutralization Reaction

A chemical reaction that occurs when an acid and a base react together to produce water and an ionic salt ($\text{Acid} + \text{Base} \rightarrow \text{Water} + \text{Ionic salt}$).