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CORE Define the terms relative atomic mass (Ar) and relative molecular mass (Mr). relative atomic mass weighted mean mass of all the naturally occuring isotopes of an element relative to the mass of an atom of 12 C relative molecular mass average mass of the molecules in a sample of pure substance relative to the mass of an atom of carbon 12 Define the terms first ionization energy and electronegativity. The first ionization energy minimum energy required to remove the outermost electron from each atom in a mole of gaseous atoms Electronegativity measure of the ability of an atom to attract a pair of electrons in a covalent bond The standard enthalpy change of a reaction is the enthalpy change when one mole of reactants is transformed into products at 298K and 101.3 KPa (1atm) The average bond enthalpy is the average energy change when 1 mole of a particular covalent bond is broken to give atoms; reactants and products being in the gaseous state. e.g. HCl (g) --> H (g) + Cl (g) The rate of a chemical reaction is the rate of disappearance of reactants or the rate of appearance of products . (can be a rate of concentration change, pressure change, volume change…) N.B. colour change is an indirect measurement of concentration change Activation energy (E a ) is the minimum energy required for a chemical reaction to occur 6

IB Chem Definitions

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IB Definitions

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Define the terms relative atomic mass

(Ar) and relative molecular mass (Mr).relative atomic mass weighted mean mass of all the naturally occuring isotopes of an element relative to the mass of an atom of 12Crelative molecular mass average mass of the molecules in a sample of pure substance relative to the mass of an atom of carbon 12

Define the terms first ionization energy

and electronegativity.

The first ionization energy minimum energy required to remove the outermost electron from each atom in a mole of gaseous atomsElectronegativity measure of the ability of an atom to attract a pair of electrons in a covalent bond

The standard enthalpy change of a reaction is the enthalpy change when one mole of reactants is transformed into products at 298K and 101.3 KPa (1atm)

The average bond enthalpy is the average energy change when 1 mole of a particular covalent bond is broken to give atoms; reactants and products being in the gaseous state.e.g. HCl (g) --> H(g) + Cl(g)

The rate of a chemical reaction is the rate of disappearance of reactants or the rate of appearance of products. (can be a rate of concentration change, pressure change, volume change)

N.B. colour change is an indirect measurement of concentration changeActivation energy (Ea) is the minimum energy required for a chemical reaction to occurOxidising agent is a substance which will usually easily remove electrons from other substances in a redox reaction (eg halogens, O2, Ag+ --> Ag(s) ).

Reducing agent is a substance which will usually easily lose electrons to other substances in a redox reaction (eg Al in: 2Al(s) + Fe2O3 (s) ---> 2Al2O3 + 2Fe HL

A ligand is an molecule or ion capable of donating a pair of electrons to a central metal atom or ion

Standard stateis the accepted form of the substance at 298K and 101.3KPa (1atm) (eg graphite for carbon and not diamond, O2 for oxygen and not O3)

Standard enthalpy change of formation is the enthalpy change when one mole of a substance is formed from its elements in their standard states. Reactants and products at 298K and 101.3 Kpa (1 atm)e.g. Hfo C(graphite) =0 KJ mol-1, Hfo S8 = 0 KJ mol-1, Hfo SO2 = -296.84 KJ mol-1

Standard enthalpy change of combustion is the enthalpy change when one mole of a substance is completely burned in oxygen. Reactants and products at 298K and 101.3 Kpa (1 atm)

S(s) + O2 (g) --> SO2(g)

Hco = -296.84 KJ mol-1

N.B. for reactions of elements with oxygen Hco equals HfoDefine and apply the terms lattice

enthalpy and electron affinity.

The lattice enthalpy is the energy evolved when one mole of an ionic compound is formed from gaseous ions under standard conditionsElectron affinity is the energy change that occurs when an electron is added to a gaseous atom or ion

Define the term standard electrode

potential (Eo )The standard electrode potential is the potential of a half cell compared to the standard hydrogen electrode (SHE) at 298K and 101.3 KPa (1atm). All solutions at a concentration of 1MStereoisomerism same struct. Form, diff arrange. in space.

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