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38 Cards in this Set
- Front
- Back
Activation energy
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minimum amount of energy required for a chemical reaction
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Covalent bond
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electrostatic attraction between a pair of electrons and +vly charged nuclei
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Atomic number
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number of protons in the nucleus
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Enthalpy change
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H(products) - H(reactants)
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Standard electrode potential
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potential of a half-reaction under standard conditions, as measured against potential of standard hydrogen electrode
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Solution
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A homogeneous solution comprised of one or more solutes dissolved in a solvent
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Solvent
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dissolving medium in a solution
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Acids and bases according to Lewis theory
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acid: electron pair acceptor.
base: electron pair donor. |
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Buffer solution
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aqueous solution that resists changes in pH when small amount of acid, base or water are added
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Acids and bases according to Bonsted-Lowry theory
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Acids: proton donor
Bases: proton acceptor |
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Enthalpy
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Heat energy converted from energy in chemical bonds
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Standard enthalpy change
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enthalpy change when molar quantities of reactants in normal state react to form products in normal state under standard conditions (298K, 101.3kPa or 1atm)
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Oxidizing agent
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A substance that is able to oxidize other substances.
agent itself undergoes reduction |
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Ionic bond
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Electrostatic attraction between oppositely charged ions
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Rate of reaction
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change in concentration of a reactant or product per unit of time
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Isotopes
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Atoms of same element with different number of neutrons
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Reducing agent
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Able to reduce other substances
- undergoes oxidation |
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Mass number
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Sum of atom's protons and neutrons
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Solute
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a substance dissolved in liquid to form a solution
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Concentration
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1cm³ = 1ml
1000cm³ = 1dm³ = 1L g/L = g x dm-³ molarity = mol/L = M = mol x dm-³ |
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Describe features of a homologous series
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-Same general formula (CnH2n)
-differ by methyl group -similar chemical properties -gradually changing physical properties (viscosity, temp etc.) |
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Define Molecular mass
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Sum of relative atomic masses of a given molecule
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Average bond enthalpy
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energy change when 1 mol of covalent bond in gaseous state is formed from gaseous atoms
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Relative atomic mass
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weighted average of atomic masses of all naturally occurring isotopes of an element
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Delocalized electrons
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valence electrons that are detached from the atoms so they are free to move around
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Standard Hydrogen Electrode
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platinum electrode
hydrogen gas at 1 atm aqueous solution of acid H + ions = 1M temperature = 298K |
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Lattice enthalpy
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enthalpy change when an ionic salt is formed from gaseous ions under standard conditions
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Oxidation
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Loss of electrons from one or more substance
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Reduction
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Gain of electrons from one or more substance
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Standard enthalpy change of combustion
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change in enthalpy that accompanies formation of one mole of compound from its complete reaction with oxygen gas
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Standard enthalpy change of formation
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change in enthalpy that accompanies the formation of one mole of compound from its elements
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Exothermic reaction
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releases heat to surroundings
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Electron affinity
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enthalpy change associated with the addition of an electron to a gaseous ion
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First ionization energy
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energy required to remove one electron from an atom in gaseous state
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Electronegativity
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a measure of an atom's ability to attract a bonding pair of electrons to itself
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Ligand
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neutral molecules or negative ions that contain a non-bonding pair of electrons
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Endothermic reaction
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absorbs heat from surroundings
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Standard state
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Temperature of 25°C, 298K
Pressure of 1 atm Liquids and solids are pure Aqueous solutions are 1M |