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EDEXCEL AS Chemistry > definitions > Flashcards

definitions Flashcards

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1
Q

Isotopes

A

Isotopes are atoms with the same number of protons, but different numbers of neutrons

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2
Q

Relative isotopic mass

A

Relative isotopic mass is the mass of one atom of an isotope compared to one twelfth of the mass of one atom of carbon-12

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3
Q

Relative atomic mass

A

Relative atomic mass is the average mass of one atom compared to one twelfth of the mass of one atom of carbon-12

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4
Q

The first ionisation energy

A

The first ionisation energy is the energy required when one mole of gaseous atoms forms one mole of gaseous ions with a single positive charge

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5
Q

Periodicity

A

Periodicity is the repeating pattern of physical or chemical properties going across the periods

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6
Q

Ionic bonding

A

Ionic bonding is the strong electrostatic force of attraction between oppositely charged ions formed by electron transfer

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7
Q

A covalent bond

A

A covalent bond is caused by the electrostatic attraction between the bonding shared pair of electrons and the two nuclei

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8
Q

dative covalent bond

A

A dative covalent bond forms when the shared pair of electrons in the covalent bond come from only one of the bonding atoms.

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9
Q

Electronegativity

A

Electronegativity is the relative tendency of an atom in a covalent bond in a molecule to attract electrons in a covalent bond to itself.

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10
Q

Metallic bonding

A

Metallic bonding is the electrostatic force of attraction between the positive metal ions and the delocalised electrons

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11
Q

Disproportionation

A

Disproportionation is the name for a reaction where an element in a single species simultaneously oxidises and reduces.

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12
Q

empirical formula

A

An empirical formula is the simplest ratio of atoms of each element in the compound.

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13
Q

Hydrocarbon

A

Hydrocarbon is a compound consisting of hydrogen and carbon only

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14
Q

Saturated

A

Saturated: Contain single carbon-carbon bonds only

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15
Q

Unsaturated

A

Unsaturated : Contains a C=C double bond

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16
Q

Molecular formula

A

Molecular formula: The formula which shows the actual number of each type of atom

17
Q

General formula

A

General formula: algebraic formula for a homologous series e.g. CH2n

18
Q

Structural formula

A

Structural formula shows the minimal detail that shows the arrangement of atoms in a molecule

19
Q

Displayed formula

A

Displayed formula: show all the covalent bonds present in a molecule

20
Q

Homologous series

A

Homologous series are families of organic compounds with the same functional group and same general formula.

21
Q

Structural isomers

A

Structural isomers: same molecular formula different structures (or structural formulae)

22
Q

Stereoisomers

A

Stereoisomers have the same structural formulae but have a different spatial arrangement of atoms.

23
Q

Cracking

A

Cracking: conversion of large hydrocarbons to smaller molecules by breakage of C-C bonds

24
Q

Enthalpy change

A

Enthalpy change is the amount of heat energy taken in or given out during any change in a system provided the pressure is constant

25
Q

The standard enthalpy change of formation

A

The standard enthalpy change of formation of a compound is the enthalpy change when 1 mole of the compound is formed from its elements under standard conditions (298K and 100kpa), all reactants and products being in their standard states

26
Q

The standard enthalpy of combustion

A

The standard enthalpy of combustion of a substance is defined as the enthalpy change that occurs when one mole of a substance is combusted completely in oxygen under standard conditions.
(298K and 100kPa), all reactants and products being in their standard states

27
Q

Enthalpy change of reaction

A

Enthalpy change of reaction is the enthalpy change when the number of moles of reactants as specified in the balanced equation react together

28
Q

The standard enthalpy change of neutralisation

A

The standard enthalpy change of neutralisation is the enthalpy change when solutions of an acid and an alkali react together under standard conditions to produce 1 mole of water.

29
Q

The mean bond enthalpy

A

The mean bond enthalpy is the enthalpy needed to break the covalent bond into gaseous atoms, averaged over different molecules

30
Q

The Activation Energy

A

The Activation Energy is defined as the minimum energy which particles need to collide to start a reaction

31
Q

The rate of reaction

A

The rate of reaction is defined as the change in concentration of a substance in unit time

32
Q

The enthalpy of atomisation

A

The enthalpy of atomisation of an element is the enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state

33
Q

The first electron affinity

A

The first electron affinity is the enthalpy change that occurs when 1 mole of gaseous atoms gain 1 mole of electrons to form 1 mole of gaseous ions with a -1 charge

34
Q

The second electron affinity

A

The second electron affinity is the enthalpy change when one mole of gaseous 1- ions gains one electron per ion to produce gaseous 2- ions.

35
Q

The Enthalpy of lattice formation

A

The Enthalpy of lattice formation is the standard enthalpy change when 1 mole of an ionic crystal lattice is formed from its constituent ions in gaseous form.

36
Q

The enthalpy of solution

A

The enthalpy of solution is the standard enthalpy change when one mole of an ionic solid dissolves in a large enough amount of water to ensure that the dissolved ions are well separated and do not interact with one another

EDEXCEL AS Chemistry (13 decks)

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