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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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Chemical reaction
A chemical change in which one or more substances are converted into new substances with different atomic arrangements.
Reactant
A starting substance in a chemical reaction that undergoes change.
Product
A substance formed as a result of a chemical reaction.
Arrow (→)
Symbol in an equation indicating the direction from reactants to products.
Evidence of chemical reaction – color change
Visible shift in hue signaling a chemical change.
Evidence of chemical reaction – light production
Emission of light that accompanies certain reactions (e.g., combustion).
Evidence of chemical reaction – precipitate formation
Appearance of a solid from two aqueous solutions in a reaction.
Evidence of chemical reaction – gas formation
Evolution of bubbles or fumes showing a gas is produced.
Evidence of chemical reaction – heat change
Temperature rise or drop indicating energy is released or absorbed.
Chemical equation
Symbolic representation of a chemical reaction showing formulas, states, and coefficients.
Physical-state symbols
(s) solid, (l) liquid, (g) gas, (aq) aqueous—placed after formulas in equations.
Coefficient
Whole number in front of a formula that indicates relative moles or molecules.
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
Skeletal equation
Unbalanced equation that lists correct formulas and physical states only.
Conservation of mass
Law stating matter is neither created nor destroyed in a chemical reaction.
Diatomic molecule
Element that exists as a two-atom molecule in its elemental form (H₂, O₂, N₂, F₂, Cl₂, Br₂, I₂).
Combination (synthesis) reaction
Reaction in which two or more substances combine to form one compound (A + B → AB).
Decomposition reaction
Single compound breaks into elements or simpler compounds (CD → C + D).
Single-displacement reaction
Element replaces another in a compound (A + CD → AD + C).
Metal displacement
Type of single-displacement where a free metal replaces another metal ion in a salt.
Halogen displacement
Single-displacement in which a more reactive halogen (F₂ > Cl₂ > Br₂ > I₂) displaces a halide.
Activity series
Ordered list of metals (or halogens) by decreasing reactivity used to predict displacement.
Double-displacement reaction
Ions in two compounds exchange partners (CD + EF → CF + ED).
Precipitation reaction
Double-displacement whose driving force is formation of an insoluble solid (precipitate).
Gas-formation reaction
Double-displacement that produces an unstable product which decomposes to a gas and water.
Acid-base neutralization
Reaction of an acid with a base to form a salt and water; a type of double-displacement.
Combustion reaction
Rapid reaction with O₂ producing heat, flame, CO₂ and H₂O (for hydrocarbons).
Coefficient adjustment rule
Only coefficients, not subscripts, may be changed when balancing equations.
Polyatomic ion balancing
Treat intact polyatomic ions as units when they appear unchanged on both sides of an equation.
Strong electrolyte
Substance that dissociates completely in water, giving excellent conductivity (e.g., soluble salts, strong acids).
Weak electrolyte
Substance that partially dissociates in water, conducting weakly (e.g., weak acids).
Nonelectrolyte
Molecular compound that does not form ions in water, thus does not conduct electricity.
Molecular equation (ME)
Shows reactants and products as complete formulas, ignoring ionic dissociation.
Ionic equation (IE)
Expanded form displaying strong electrolytes as separate ions in aqueous solution.
Net ionic equation (NIE)
Equation that includes only the species that actually change; spectator ions removed.
Spectator ion
Ion that remains unchanged during reaction, present in both reactants and products of IE.
Solubility rules
Guidelines predicting whether an ionic compound is soluble (aq) or insoluble (s) in water.
Fuel
Hydrocarbon or other substance that reacts with oxygen in combustion to release energy.
Driving force
Factor (precipitate, gas, water, heat) that makes a reaction proceed, especially in double-displacement processes.