Module 7 Lecture Notes

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Flashcards about Chemical Reactions, Energy Changes and Reaction Rates

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13 Terms

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Decomposition Reaction

A type of chemical reaction where a single compound breaks down into two or more simpler substances (e.g., CuCO3(s) -> CuO(s) + CO2(g)).

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Precipitation Reaction

A type of chemical reaction that involves the formation of an insoluble solid (precipitate) when two or more solutions are mixed (e.g., Pb(NO3)2(aq) + 2KI(aq) -> PbI2(s) + 2KNO3(aq)).

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Acid-Base Reaction

A type of chemical reaction between an acid and a base, resulting in the formation of a salt and water (e.g., NaOH(aq) + HCl(aq) -> NaCl(aq) + H2O(l)).

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Complex Ion Formation

A reaction in which a central metal ion is surrounded by molecules or ions (ligands) to form a complex ion (e.g., Cu2+(aq) + 4NH3(aq) -> Cu(NH3)4 2+(aq)).

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Redox (Oxidation-Reduction) Reaction

A type of chemical reaction that involves the transfer of electrons between two species (e.g., 2Mg(s) + O2(g) -> 2MgO(s)).

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Heat of Reaction

The change in enthalpy that occurs when a chemical reaction takes place at constant pressure.

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Enthalpy (H)

The internally stored chemical energy (heat content) of a system.

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Exothermic Reaction

A reaction that releases heat energy into the surroundings; change in enthalpy (ΔH) is negative.

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Endothermic Reaction

A reaction that absorbs heat energy from the surroundings; change in enthalpy (ΔH) is positive.

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Activation Energy (Ea)

The minimum energy required for a chemical reaction to occur; the energy needed to reach the transition state.

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Transition State

The highest energy state in a chemical reaction; the intermediate state between reactants and products.

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Collision Theory

For a reaction to occur, molecules must collide with sufficient energy and correct orientation.

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Catalyst

A substance that increases the rate of a chemical reaction by providing an alternative reaction pathway with lowers activation energy, without being consumed in the reaction.