Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

EDEXCEL AS Chemistry > definitions > Flashcards

definitions Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

Isotopes

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Periodicity

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Ionic bonding

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Metallic bonding

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Disproportionation

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

empirical formula

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Hydrocarbon

A

Hydrocarbon is a compound consisting of hydrogen and carbon only

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Saturated

A

Saturated: Contain single carbon-carbon bonds only

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Unsaturated

A

Unsaturated : Contains a C=C double bond

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions