Chapter 5 – Chemical Reactions: Core Vocabulary

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40 vocabulary flashcards covering fundamental terms, reaction types, balancing principles, electrolytes, and aqueous-solution representations from Chapter 5 lecture notes.

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39 Terms

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Chemical reaction

A chemical change in which one or more substances are converted into new substances with different atomic arrangements.

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Reactant

A starting substance in a chemical reaction that undergoes change.

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Product

A substance formed as a result of a chemical reaction.

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Arrow (→)

Symbol in an equation indicating the direction from reactants to products.

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Evidence of chemical reaction – color change

Visible shift in hue signaling a chemical change.

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Evidence of chemical reaction – light production

Emission of light that accompanies certain reactions (e.g., combustion).

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Evidence of chemical reaction – precipitate formation

Appearance of a solid from two aqueous solutions in a reaction.

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Evidence of chemical reaction – gas formation

Evolution of bubbles or fumes showing a gas is produced.

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Evidence of chemical reaction – heat change

Temperature rise or drop indicating energy is released or absorbed.

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Chemical equation

Symbolic representation of a chemical reaction showing formulas, states, and coefficients.

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Physical-state symbols

(s) solid, (l) liquid, (g) gas, (aq) aqueous—placed after formulas in equations.

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Coefficient

Whole number in front of a formula that indicates relative moles or molecules.

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Balanced equation

the number of atoms of each element is the same in the products as in the reactants.

conservation os mass is always maintained

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Skeletal equation

Unbalanced equation that lists correct formulas and physical states only.

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Conservation of mass

Law stating matter is neither created nor destroyed in a chemical reaction.

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Diatomic molecule

Element that exists as a two-atom molecule in its elemental form (H₂, O₂, N₂, F₂, Cl₂, Br₂, I₂).

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Combination (synthesis) reaction

Reaction in which two or more substances combine to form one compound (A + B → AB).

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Decomposition reaction

Single compound breaks into elements or simpler compounds (CD → C + D).

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Single-displacement reaction

Element replaces another in a compound (A + CD → AD + C).

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Metal displacement

Type of single-displacement where a free metal replaces another metal ion in a salt.

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Halogen displacement

Single-displacement in which a more reactive halogen (F₂ > Cl₂ > Br₂ > I₂) displaces a halide.

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Activity series

Ordered list of metals (or halogens) by decreasing reactivity used to predict displacement.

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Double-displacement reaction

Ions in two compounds exchange partners (CD + EF → CF + ED).

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Precipitation reaction

Double-displacement whose driving force is formation of an insoluble solid (precipitate).

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Gas-formation reaction

Double-displacement that produces an unstable product which decomposes to a gas and water.

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Acid-base neutralization

Reaction of an acid with a base to form a salt and water; a type of double-displacement.

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Combustion reaction

Rapid reaction with O₂ producing heat, flame, CO₂ and H₂O (for hydrocarbons).

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Coefficient adjustment rule

Only coefficients, not subscripts, may be changed when balancing equations.

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Polyatomic ion balancing

Treat intact polyatomic ions as units when they appear unchanged on both sides of an equation.

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Strong electrolyte

Substance that dissociates completely in water, giving excellent conductivity (e.g., soluble salts, strong acids).

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Weak electrolyte

Substance that partially dissociates in water, conducting weakly (e.g., weak acids).

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Nonelectrolyte

Molecular compound that does not form ions in water, thus does not conduct electricity.

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Molecular equation (ME)

Shows reactants and products as complete formulas, ignoring ionic dissociation.

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Ionic equation (IE)

Expanded form displaying strong electrolytes as separate ions in aqueous solution.

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Net ionic equation (NIE)

Equation that includes only the species that actually change; spectator ions removed.

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Spectator ion

Ion that remains unchanged during reaction, present in both reactants and products of IE.

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Solubility rules

Guidelines predicting whether an ionic compound is soluble (aq) or insoluble (s) in water.

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Fuel

Hydrocarbon or other substance that reacts with oxygen in combustion to release energy.

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Driving force

Factor (precipitate, gas, water, heat) that makes a reaction proceed, especially in double-displacement processes.