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9.6: Key Terms

Last updated

Jul 17, 2023
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- 9.5: Strengths of Ionic and Covalent Bonds
- 9.7: Key Equations

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bomb calorimeter: device designed to measure the energy change for processes occurring under conditions of constant volume; commonly used for reactions involving solid and gaseous reactants or products

bond energy: (also, bond dissociation energy) energy required to break a covalent bond in a gaseous substance

Born-Haber cycle: thermochemical cycle relating the various energetic steps involved in the formation of an ionic solid from the relevant elements

calorie (cal): unit of heat or other energy; the amount of energy required to raise 1 gram of water by 1 degree Celsius; 1 cal is defined as 4.184 J

calorimeter: device used to measure the amount of heat absorbed or released in a chemical or physical process

calorimetry: process of measuring the amount of heat involved in a chemical or physical process

chemical thermodynamics: area of science that deals with the relationships between heat, work, and all forms of energy associated with chemical and physical processes

endothermic process: chemical reaction or physical change that absorbs heat

energy: capacity to supply heat or do work

enthalpy (H): sum of a system’s internal energy and the mathematical product of its pressure and volume

enthalpy change (ΔH): heat released or absorbed by a system under constant pressure during a chemical or physical process

exothermic process: chemical reaction or physical change that releases heat

expansion work (pressure-volume work): work done as a system expands or contracts against external pressure

first law of thermodynamics: internal energy of a system changes due to heat flow in or out of the system or work done on or by the system

heat (q): transfer of thermal energy between two bodies

heat capacity (C): extensive property of a body of matter that represents the quantity of heat required to increase its temperature by 1 degree Celsius (or 1 kelvin)

Hess’s law: if a process can be represented as the sum of several steps, the enthalpy change of the process equals the sum of the enthalpy changes of the steps

hydrocarbon: compound composed only of hydrogen and carbon; the major component of fossil fuels

internal energy (U): total of all possible kinds of energy present in a substance or substances

joule (J): SI unit of energy; 1 joule is the kinetic energy of an object with a mass of 2 kilograms moving with a velocity of 1 meter per second, 1 J = 1 kg m²/s and 4.184 J = 1 cal

kinetic energy: energy of a moving body, in joules, equal to $\frac{1}{2} m v^{2}$ (where m = mass and v = velocity)

lattice energy (ΔH_lattice): energy required to separate one mole of an ionic solid into its component gaseous ions

nutritional calorie (Calorie): unit used for quantifying energy provided by digestion of foods, defined as 1000 cal or 1 kcal

potential energy: energy of a particle or system of particles derived from relative position, composition, or condition

specific heat capacity (c): intensive property of a substance that represents the quantity of heat required to raise the temperature of 1 gram of the substance by 1 degree Celsius (or 1 kelvin)

standard enthalpy of combustion $(Δ H_{c} °)$: heat released when one mole of a compound undergoes complete combustion under standard conditions

standard enthalpy of formation $(Δ H_{f} °)$: enthalpy change of a chemical reaction in which 1 mole of a pure substance is formed from its elements in their most stable states under standard state conditions

standard state: set of physical conditions as accepted as common reference conditions for reporting thermodynamic properties; 1 bar of pressure, and solutions at 1 molar concentrations, usually at a temperature of 298.15 K

state function: property depending only on the state of a system, and not the path taken to reach that state

surroundings: all matter other than the system being studied

system: portion of matter undergoing a chemical or physical change being studied

temperature: intensive property of matter that is a quantitative measure of “hotness” and “coldness”

thermal energy: kinetic energy associated with the random motion of atoms and molecules

thermochemistry: study of measuring the amount of heat absorbed or released during a chemical reaction or a physical change

work (w): energy transfer due to changes in external, macroscopic variables such as pressure and volume; or causing matter to move against an opposing force

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