Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > DEFINITIONS > Flashcards

DEFINITIONS Flashcards

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

Atom

A

The smallest particle of matter and is made up of protons, neutrons and electrons

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

Element

A

Only made up of one sort of atom

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

Molecule

A

Two or more atoms covalently bonded together. Atoms can be the same or different elements

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

Compound

A

Two or more different types of atom bonded together. Boning can be ionic or covalent

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

Mixture

A

Has two or more different elements and/or compounds in the same space.
They can be separated into individual components

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

Sulfuric acid

A

H2SO4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Nitric acid

A

HNO3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Phosphoric acid

A

H3PO4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Ammonium

A

NH4 +

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

Nitrate

A

NO3 -

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

Hydrogencarbonate

A

HCO3 -

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

Carbonate ion

A

CO3 2-

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

Sulfate ion

A

SO4 2-

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

Phosphate ion

A

PO4 3-

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

An acid

A

a substance that donates H+ Ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

A base

A

Substace that accepts H+ ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

An alkali

A

A base that releases hydroxide ions in aqueous solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

A salt

A

Formed when hydrogen ions from an acid are replaced by a metal or ammonium ion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Acid + Alkali

A

Salt + water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Acid + Base

A

Salt + Water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Acid + Metal

A

Salt + Hydrogen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Acid + metal carbonate

A

Salt + water + CO2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Acid + metal hydrocarbonate

A

Salt + water + CO2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What to split for an ionic equation

A

Must be:
-Ionic
-(Acids)
-aqueous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Atomic number

A

Number of protons in the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Mass number

A

Number of protons and neutrons in the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Isotope

A

Atoms of the same element with a different number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Why do isotopes have the same chemical properties

A

They have the same electron configuration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Isotopic mass

A

The mass of an isotope relative to 1/12th the mass of a C-12 atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Relative atomic mass(Ar)

A

the weighted average mass of all the isotopes relative to 1/12th the mass of an atom of c-12

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Relative molwecular mass

A

The mass of a molecule of the compound relative to 1/12th the mass of an atom of C-12.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Relative formular mass

A

Is the mass of one formula unit of an ionic compound relative to 1/12th of the mass of an atom of c-12

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

The mole

A

The amount of substance that contains as many particles as there are in exactly 12g of C-12

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Empirical formula

A

The simplest whole number ratio of atoms of each element present in a molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Molecular formula

A

The actual number of atoms of each element present in a molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Metallic bond

A

The attratction between delocalised outer shell electrons and positive metal ions in a lattice

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Ionic bond

A

The electrostatic attraction between oppositley charged ions in a lattice

38
Q

Covalent bond

A

A shared pair of e-

39
Q

A lone pair

A

A pair of e- which is not bonded

40
Q

Co-ordinate bond

A

A covalent bond in which both e- of the shared pair come from the same atom

41
Q

Electronegativety

A

The power of an atom to attract the pair of e- in a covalent bond

42
Q

Enthalpy change

A

The heat energy change at constant pressure

43
Q

Activation energy

A

The minimum energy required to start a reaction by the breaking of bonds

44
Q

Bond enthalpy

A

The energy required to break one mole of a given covalent bond in he molecules in the gaseous state

45
Q

Mean bond enthalpy

A

The energy required to break a covalent bond, avergaed for the type of bond in a range of different compounds

46
Q

Standard enthalpy of formation

A

The enthalpy change that occurs when one mole of a compound is formed from its constituent elements with all reactants and products in their standard states

47
Q

Standard enthalpy of combustion

A

The enthalpy change tat occurs when one mole of a compound reacts completley in oxygen with all reactants and produucts

48
Q

Hess’s law

A

The enthalpy change for a chemicals reaction is independent of the route taken

49
Q

Rate of reaction

A

The change in concentration of a substance in a given time

50
Q

Le chataliiers principle

A

If a system in euqilibrium is subjected to a change, the postiotn of equilibrium will move in the direction which opposes that change

51
Q

Oxidation

A

Loss of electrons

51
Q

Reduction

A

Gain of electrons

51
Q

Oxidation (OS)

A

Increase in oxidation state

51
Q

Reduction (OS)

A

Decrease in oxidation state

52
Q

Oxidising agent

A

A species that accepts e-

53
Q

Reducing agent

A

Species that donates e-

54
Q

Enthalpy of lattice dissociation

A

The enthalpy change to seperate one mole of solid ionic compound into its gaseous ions.

55
Q

Enthalpy of lattice formation

A

The enthalpy change when one mole of solid ionic compound is formed from its gaseous ions

56
Q

Standard enthalpy of formation

A

The enthalpy change that occurs when one mole of a compound is formed from its constituent elements with all reactants and products in their standard states

57
Q

Standard enthalpy of of atomisation

A

The enthalpy change when one mole of gaseous atoms is formed from the elements in its standard states.

58
Q

Bond ethalpy

A

The energy required to brea one mole of a given covalent bond in the molecules in the gaseous state.

59
Q

First ionisation energy

A

The energy needed to remove one mole of elecrons from one mole of atoms in the gaseous state

60
Q

Second ionisation nergy

A

The enthalpy hcnage when one mole of gaseous 2+ ions are formed from one mole of gaseous +1 ions.

61
Q

First electron affinity

A

The enthalpy change when one mole of gaseous 1- ions are formed from one mole of gaseous atoms.

62
Q

Second electron affinity

A

The enthalpy change when one mole of gaseous 2- ions are formed from one mole of gaseous 1- ions.

63
Q

Perfect ionic model

A

Ions are perfect spheres with only electrostatic forces of atraction.

63
Q

Enthalpy change of solution

A

The enthalpy change when one mole of an ionic substance dissolves in enough solvent to form an infinitely dilute solution

64
Q

Rate determining step

A

The slowest step in a reaction mechansim

65
Q

Standard electrode potentiel

A

The emf of a halfcell compared with the standard hydrogen half-cell. Measured at 298k, all solution have conc of 1moldm-3 and gases at 100kpa.

66
Q

Bronsted-Lowry acid-base reaction

A

Proton transfer

67
Q

Acid

A

Donates H+

68
Q

Strong acid

A

Completley dissociates in siolution

69
Q

Weak acid

A

Partially dissociates in solution

70
Q

Base

A

Accpets H+

71
Q

Alkali

A

A base that releases hydroxide ions in aqueous solutions

72
Q

Buffer

A

A solution that maintains an approximatley constant pH on addition of small amounts of acid or base

73
Q

Molecular formula

A

The actual number of atoms of each element present in a molecule

74
Q

Emperical formula

A

Simplest whole number ratio of atoms of each element present in a molcule

74
Q

Structural formula

A

Shows how the atoms in a molecule are arranged

75
Q

Displayed formula

A

Shows all the atoms and bonds in a molecule

76
Q

Skeletal formula

A

Shows the shape of the carbon skelenton

77
Q

Homologous series

A

A famoly of compounds conatining the same functional group and having the same general formula but having a different carbon chain lenght

78
Q

Functional group

A

An atom or group os atoms which gives an organic compound particular chemical properties

79
Q

Structual isomers

A

Compounds with the same molecular formula but a different structural formula

80
Q

Chain isomers

A

Same molecula formula but their structures have the hydrocarbon chain arranged differently

81
Q

Position isomers

A

Have the functional group in a differetn position

82
Q

Functional group isomers

A

Same molecular formular but different functional group

83
Q

Free-radical

A

A species with an unpaired e-

84
Q

An electrophile

A

An e- pair acceptor

85
Q

Biofuel

A

A fuel derived or produced from renewable biological resources

86
Q

Optical isomers

A

Non-superimposable mirror images

87
Q

Racemic mixture

A

A mixture of equal amounts of the two enantiomers

Chemistry (19 decks)

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