Term
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Definition
| The mass of one mole of any substance, expressed in grams per mole |
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Definition
The average mass of an atom taking into account the relative abundances of all the naturally occurring isotopes of the element relative to one atom of C-12
Realative term so no units |
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Definition
| The average mass of a molecule calculated by adding the relative atomic masses of its constituent atoms. Relative term so no units |
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Definition
| The simplest whole number ratio of the atoms a compound contains |
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Definition
| The actual number of atoms of each element present. A multiple of the empirical formula |
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Definition
| The substance dissolved in a solvent in forming a solution |
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Definition
| The liquid that dissolves another substance to form a solution |
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Definition
| A homogeneous mixture of the solvent and the solute |
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Definition
| The amount of solute in a known volume of solution expressed in mol/dm3 |
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Definition
| The total of protons plus neutrons in the nucleus of an atom |
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Definition
The number of protons in an atoms nucleus
Equal to the number of electrons
Determines placement on periodic table |
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Definition
| Atoms of the same element with different numbers of neutrons |
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Definition
| An unbroken spectrum of frequencies such as the spectrum of visible light |
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Definition
| A broken spectrum of frequencies, showing only certain frequencies of visible light |
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Definition
| The vertical column of elements on the periodic table of elements |
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Definition
| The horizontal row of elements on the periodic table of elements |
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Definition
| The minimum energy required to remove one mole of electrons from a mole of gaseous atoms |
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Term
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Definition
| The tendency to attract electrons |
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Term
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Definition
| An ion or molecule that donates a pair of electrons to a metal atom or ion |
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Term
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Definition
Releases heat to the surroundings Products stronger than reactants -ΔH |
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Term
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Definition
Absorbs heat from the surroundings Products weaker than the reactants
+ΔH |
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Term
| Standard Enthalpy Change of Reaction |
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Definition
| The heat transferred in a reaction carried out under standard conditions |
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Term
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Definition
| The energy required to break a mole of covalent bonds in a reactant, all reactants and products being in their gaseous states |
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Term
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Definition
| The most stable state of an element under the specified conditions |
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Term
| Standard Enthalpy Change of Formation |
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Definition
| The enthalpy change on the formation of one mole of a compound from its elements in their standard states under specified conditions |
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Term
| Standard Enthalpy Change of Combustion |
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Definition
| The enthalpy change on the complete combustion of one mole of a compound in its standard state in excess oxygen under standard conditions |
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Term
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Definition
| The enthalpy change that occurs on the formation of one mole of ionic compound from its isolated ions in their gaseous state |
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Term
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Definition
| The energy change occurring when a gaseous atom gains and electron to form a negative ion |
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Definition
| The increase in concentration of products per unit time. Expressed in Mol/Dm3S |
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Definition
| The minimum energy required for a chemical reaction to take place |
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Term
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Definition
K in the rate equation
Rate=k[A]m[B]n |
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Term
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Definition
| With respect to a reactant is the power to which its concentration is raised in the rate equation |
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Term
| Bronsted-Lowry Acids and Bases |
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Definition
| Bronsted-Lowry acid= Proton donor Bronsted-Lowry base=Proton acceptor |
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Term
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Definition
Lewis Acid=Electron Pair acceptor
Lewis Base= Electron Pair Donor |
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Term
| Strong and Weak Acids and Bases |
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Definition
| Strong acids and bases are almost completely dissociated Weak acids and bases are only partially dissociated |
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Term
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Definition
pH=-Log10[H+]
pOH=-Log10[OH-]
pKw=-Log10Kw
[H+]=10^-PH
[OH-]=10^-pOH
Kw=10^-pKw |
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Term
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Definition
| Oxidation is the loss of electrons and reduction is the gain of electrons |
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Term
| Oxidizing Agent and Reducing Agent |
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Definition
| Oxidising agents accept electrons and get reduced reducing agents donate elctrons and get oxidised |
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Term
| Standard Electrode Potential |
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Definition
| The electrode potential relative to a hydrogen half cell measured under standard conditions |
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Term
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Definition
| Precise Measurements have small random errors and accurate measurements have small systematic errors |
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