Total number of protons and neutrons in the nucleus
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Relative atomic mass
The Average mass of an atom of an element relative to 1/12 the mass of an atom of carbon-12
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Relative isotopic mass
The mass of a single isotope of an element relative to 1/12 the mass of an atom of carbon-12
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Ionisation energy
The energy required to remove one mole of electrons from one mole of a gaseous atom to form one mole of gaseous 1+ atom
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Empirical formula
The simplest whole-number ratio of the atoms of each element in a compound
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Molecular formula
The actual number of atoms in one molecule of the substance
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Avogadro constant
Numbers of particles in one mole(6.02x10^23)
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Lattice
Regular repeated three-dimensional arrangement of atoms, ions or molecules in a metal or crystalline solid
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Electronegativity
The power of an atom to attract the pair of electrons in a covalent bond
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Enthalpy change
The heat energy change at constant pressure
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Activation energy
The minimum amount of energy to start a reaction
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Standard enthalpy of reaction
The enthalpy changes when substances react under standard conditions
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Standard enthalpy of formation
The enthalpy change when 1 mole of a compound is formed from its constituent elements with all reactants and products in the standard state under standard conditions
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Standard enthalpy of combustion
The enthalpy changes when 1 mole of a substance is burned completely in excess oxygen with all reactants and products in their standard state under standard conditions
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Hess's Law
The enthalpy change for a chemical reaction is independent of the route taken and only depends on the initial and final state
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Mean bond enthalpy
A measure of the energy required to break one mole of a covalent bond measured in the gaseous state in KJ mol-1
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Rate of reaction
The change in concentration of reactants or products in a given period of time
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Le Chatelier's Principle
If a factor is changed which affects a system in equilibrium, the position of the equilibrium will move in a direction as to oppose that change
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Functional group
A group of atoms which are responsible for the characteristic reactions of a compound
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Structural formulae
Shows the arrangement of atoms, carbon by carbon with the attached hydrogen functional group without showing the bonds
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Skeletal formulae
Abbreviated diagrammatic description of a compound
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Standard state
The state the element is found in the periodic table
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Structural isomers
Compounds that have the same molecular formulae but a different structural formula
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Chain isomers
Occurs when there is more than one way of arranging carbon atoms in the longest chain
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Positional isomerism
Isomers that have the same carbon chain and the same functional group but is attached in a different point along the carbon atom
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Functional group isomerism
Compounds with the same molecular
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Stereoisomerism
Molecules with the same molecular and structural formula but a different arrangement of atoms in 3D space
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Other cards in this set
Card 2
Front
Mass number
Back
Total number of protons and neutrons in the nucleus
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