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Chemistry > Definitions > Flashcards

Definitions Flashcards

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1
Q

Define isotopes

A

Isotopes are atoms of the same element with different numbers of neutrons and different masses

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2
Q

Define relative atomic mass

A

The relative atomic mass for an element is the weighted mean mass of an atom of the element compared with 1/12th the mass of an atom of carbon-12 which has a mass of 12

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3
Q

Define relative isotopic mass

A

The mass of one isotope relative to 1/12th the mass of a carbon-12 atom which has a mass of 12

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4
Q

Define mole

A

The amount of substance which contains as many elementary particles as there are atoms in exactly 12g of carbon-12

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5
Q

Define molar mass

A

The mass of one mole of substance

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6
Q

Define molar gas volume

A

The volume per mole of gas molecules at a stated temperature and pressure

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7
Q

Define Lowry-Bronsted acid

A

A proton donor

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8
Q

Define alkali

A

A substance which releases -OH in solution

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9
Q

Define Lowry-Bronsted base

A

A proton acceptor

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10
Q

Define a salt

A

A substance produced when the H+ ion of an acid is replaced by a specific metal ion or NH4+

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11
Q

Define an orbital

A

A region of space that can hold up to two electrons with opposite spin

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12
Q

Define first ionisation energy

A

The energy required to remove one electron from each atom in one mole of gaseous atoms to make one mole of gaseous unipositive ions

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13
Q

Define second ionisation energy

A

The energy required to remove one electron from each unipositive ion in one mole of gaseous unipositive ions to make one mole of gaseous dipositive ions

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14
Q

Define covalent bond

A

The electrostatic attraction between a positively charged nucleus and a shared pair of electrons

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15
Q

Define dative covalent bond

A

A covalent bond where only one of the bonded atoms donates both electrons being shared

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16
Q

Define electronegativity

A

The power of attraction between a bonded atom and a pair of electrons in a covalent bond

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17
Q

Define hydrogen bonding

A

The interaction between the lone pair of electrons on a nitrogen, oxygen or fluorine atom and a hydrogen atom which is bonded to an N, O or F atom

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18
Q

Define ionic bond

A

The electrostatic attraction between oppositely charged ions

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19
Q

Define metallic bond

A

The electrostatic attraction between positively charged metal ions and delocalised electrons

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20
Q

Define periodicity

A

The repeating pattern of properties of elements across different periods in the Periodic table

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21
Q

Define disproportionation

A

When an element is being both oxidised and reduced in a redox reaction

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22
Q

Define the rate of reaction

A

The change in concentration of reactant or product per unit time

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23
Q

Define Le Chatelier’s Principle

A

When a system under dynamic equilibrium is subjected to a change, the equilibrium will shift so as to oppose the change

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24
Q

Define standard conditions

A

Temp= 298K, Pressure= 100kPa, solution conc= 1moldm-3

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25
Q

Define standard enthalpy of formation

A

The enthalpy change when 1 mole of a compound is formed in its standard state from its constituent elements in their standard states, under standard condition

26
Q

Define standard enthalpy of combustion

A

The enthalpy change when 1 mole of a substance in its standard state reacts completely with oxygen under standard conditions

27
Q

Define standard enthalpy change of neutralisation

A

The enthalpy change when 1 mole of water is created by the neutralisation of an acid with an alkali under standard conditions

28
Q

Define homologous series

A

A series of organic compounds with the same functional group but with each successive member differing by CH2

29
Q

Define structural isomer

A

Have the same molecular formula but a different structural formula

30
Q

Define homolytic fission

A

Where the covalent bond breaks equally so each product receives one of the shared pair of electrons to form radicals

31
Q

Define heterolytic fission

A

Where the covalent bond breaks unequally so one product gets both of the electrons from the shared pair and the other gets nothing, producing ions

32
Q

Define radical

A

A species with an unpaired electron

33
Q

Define nucleophile

A

Electron pair donor

34
Q

Define electrophile

A

Electron pair acceptor

35
Q

Define sigma bond

A

Sigma bonds are formed by the direct overlap of orbitals directly between the bonding atoms

36
Q

Define stereoisomerism

A

Compounds with the same structural formula but a different arrangement of atoms in space

37
Q

Define IR spectroscopy

A

Method used to identify which functional groups are present in a given molecule

38
Q

Define fingerprint region

A

Unique to a particular molecule, used to identify known substances from a database

39
Q

Define half life

A

The time taken for the concentration of one reactant to fall by half the original value

40
Q

Define the rate determining step

A

The slowest step in the reaction mechanism of a multistep reaction which determines the overall rate

41
Q

Define partial pressure

A

The pressure exerted if one gas in a mixture occupied the whole container alone

42
Q

Define Ka

A

[H+][A-]/ [HA]

43
Q

Define buffer

A

A solution that resists changes in pH when small amounts of acid or alkali are added

44
Q

Define standard electrode potential

A

The voltage measure when the named electrode is connected to the standard hydrogen electrode at 298K under 100kPa with solutions of 1 moldm-3

45
Q

Define fuel cell

A

A fuel cell uses the energy generated from the reaction between a fuel and oxygen to create a voltage

46
Q

Define transition metal

A

A d-block element that forms one or more stable ions with incompletely filled d-orbitals

47
Q

Define complex

A

A complex consists of a central metal ion/metal surrounded by ligands which are bonded coordinately

48
Q

Define ligand

A

A molecule or ion which donates a lone pair of electrons to the transition metal by coordinate bonding

49
Q

Define coordination number

A

The number of coordinate bonds in the complex

50
Q

Define bidentate

A

Some ligands can donate two pairs of electrons to make two coordinate bonds

51
Q

Define arenes

A

Compounds which contain unsaturated rings with delocalised electrons within the ring

52
Q

Define chiral centre

A

A carbon with 4 different groups/atoms attached to it

53
Q

Define condensation polymerisation

A

The joining of bifunctional monomers with the elimination of a small molecule such as water or HCl

54
Q

Define lattice enthalpy

A

The energy change when 1 mole of solid ionic compound is formed from its ions in the gaseous state under standard conditions of 298K and 100kPa

55
Q

Define atomisation of metal/non-metal

A

The energy change when 1 mole of gaseous atoms are formed from the element in its standard state

56
Q

Define first ionisation of metal

A

The energy change when each atom in 1 mole of gaseous atoms loses 1 electron to become 1 mole of gaseous unipositive ions

57
Q

Define electron affinity

A

The energy change when one mole of atoms gain 1 mole of electrons in the gaseous state

58
Q

Define enthalpy of hydration

A

The energy change when 1 mole of gaseous ions are completely hydrated by water

59
Q

Define enthalpy of solution

A

The energy change when 1 mole of a solute in dissolved in water

60
Q

What is the gradient of the graph of ln k against 1/T?

A

-Ea/R

61
Q

What is the intercept of the graph of ln k against 1/T?

A

lnA

Chemistry (3 decks)

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