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Chemistry > Important Definitions- LEARN > Flashcards

Important Definitions- LEARN Flashcards

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1
Q

ISOTOPES

A

Atoms of an element with the same atomic number but different numbers of neutrons.

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2
Q

RELATIVE ISOTOPIC MASS

A

The mass of an atom of an isotope relative to 1/12 the mass of a carbon 12 atom.

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3
Q

RELATIVE ATOMIC MASS

A

The wheighted average mass of an atom of an element relative to 1/12 the mass of a carbon 12 atom.

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4
Q

ORBITAL

A

Region around the nucleus where two electrons can be held with opposite spins.

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5
Q

ACID

A

Any species that can donate H+ ions.

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6
Q

BASE

A

Any species that can receive an H+ ion. This can be soluble or insoluble.

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7
Q

Alkali

A

Soluble species that can accept an H+ ion.

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8
Q

SALT

A

An ionic compound of anions and cations, forming a neutral compound.

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9
Q

WATER OF CRYSTALISATION

A

Water molecules are part of the crystal structure.

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10
Q

HYDRATED SALT

A

Water molecules are part of the crystal structure.

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11
Q

IONIC BONDING

A

The strong electrostaitic forces of attraction between two oppositely charged ions.

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12
Q

COVELANT BONDING

A

The strong electrostatic forces between a shared pair of electrons and the two positive nuclei of the bonded atoms.

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13
Q

DATIVE COVELANT BOND

A

When both shared electrons in a covelant bond come from the same atom.

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14
Q

AVAGADROS CONSTANT

A

6.02 x 10²³ , the number of particles in a mole.

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15
Q

MOLAR VOLUME

A

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

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16
Q

MOLAR MASS

A

The mass of a substance per mole (measured in g mol-1)

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17
Q

MOLECULAR FORMULA

A

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

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18
Q

ATOM ECONOMY

A

The ratio of the mass of desired products to the mass of all the products. A measure of how well atoms have been utilised.

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19
Q

EMPIRICAL FORMULA

A

The simplist whole number ratio between the atoms of each element in a compound.

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20
Q

STRONG ACIDS VS WEAK ACIDs

A
  • strong acids fully ionise (completely dissociates)
  • weak acids partially ionise (partially dissociates)
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21
Q

ELECTRONEGATIVITY

A

The tendancy of an atom to attract a bonding pair of electrons in a covelant bond.

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22
Q

POLAR COVELANT BOND

A

A bonded electron pair is shared unequally between the bonded atoms because of the difference in electronegativity values of the bonded atoms.

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23
Q

DIPOLE

A

A molecule with separated areas of slightly negative and slightly positive charge.

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24
Q

OXIDATION NUMBER

A

Reprisents how many electrons lost or gained by an atom.

25
Q

HOMOLOGOUS SERIES

A

Compounds from the same series with the same functional group but with each successive number differeing by CH
²

26
Q

FUNCTIONAL GROUP

A

Part of the organic molecule responsible for its chemical reactions.

27
Q

HYDROCARBON

A

Composed of only carbon and hydrogen atoms.

28
Q

SATURATED

A

composed of only single c-c bonds

29
Q

ALIPHATIC

A

Carbon atoms joined straight or branched, but with no rings.

30
Q

ALICYCLIC

A

Molecule contains carbon atoms joined in a ring that is NOT AROMATIC.

31
Q

AROMATIC

A

Molecule contains at least 1 benzene ring.

32
Q

DISPROPORTIONATION

A

A redox reaction where the oxidation state of some atoms of a particular element increase, but the oxidation number of other atoms of that same element decrease.

33
Q

RADICAL

A

Species with an unpaired electron.

34
Q

HOMOLYTIC FISSION

A

A bond breaks leaving each atom one electron from the electron pair.

35
Q

HETEROLYTIC FISSION

A

Bond breaks with one atom receiving both electrons from the electron pair.

36
Q

STRUCTURAL ISOMER

A

Compounds with the same mollecular formula but different structural formula.

37
Q

SIGMA BOND

A

overlapping of the 2 s orbitals from each bonding atom.

38
Q

PI BOND

A

The sideways overlapp of 2 P orbitols, one from each bonded atom.

39
Q

ELECTROPHILE

A

A species that accepts a pair of electrons to form a covelant bond.

40
Q

NUCLEOPHILE

A

A species that can donate a pair of electrons to form a covelant bond

41
Q

Average bond enthalpy

A

Energy required to break 1 mol of a specific type of bond in a gaseous molecules

42
Q

Hess’s law

A

States that if a reaction can take place by 2 routes (and starting and finishing conditions are the same) the total enthalpy change is the same.

43
Q

Enthalpy change of reaction

A

The enthalpy change that accompanies a reaction, in the molar quantities shown in a chemical equation, under stated conditions (with all products and reactants in standard states).

44
Q

Enthalpy change of formation

A

The enthalpy change when one mole of a compound is formed from it’s elements (under stated conditions, with all reactants and products in their standard state).

45
Q

Enthalpy of combustion

A

The enthalpy change that takes place when one mole of substance reacts completely with oxygen under stated conditions (with all reactants and products in their standard state).

46
Q

Enthalpy change in neutralisation

A

The energy change that accompanies the reaction of an acid by a base to form one mole of water under stated conditions (with all reactants and products in their standard state).

47
Q

FIRST IONISATION ENERGY

A

The energy required to remove an electron from each atom in a mole of gaseous atoms (to form 1 mole of gaseous 1+ ions).

48
Q

Sterioisomers

A

Molecules with the same structural formulae but a different arrangement of atoms in space/ different 3D arrangement of atoms.

49
Q

hygroscopic

A

absorbs moisture from air.

50
Q

Enthalpy of atomisation

A

the enthalpy change that accompanies the formation if 1 mole of gaseous atoms from its elements in standard form.

51
Q

lattice enthalpy of formation

A

the energy that accompanies the formation of 1 mole of an ionic compound from its gaseous ions under standard conditions.

52
Q

First Electron Affinity

A

the enthalpy change when 1 electron is added to each atom in 1 mol of gaseous atoms to form 1 mole of gaseous 1- atoms.

53
Q

second electron affinity

A

the enthalpy change when 1 electron is added from 1 mole of gaseous 1- ions to form 1 mole of gaseous 2- ions.

54
Q

Hydration Enthalpy

A

the energy change when 1 mol of gaseous ions dissolve in water to make 1 mole of aqueous ions under standard conditions.

55
Q

Enthalpy Of Solution

A

The enthalpy change when 1 mol of solute is dissolved in water under standard conditions.

56
Q

reagent

A

a compound or mixture added to a chemical reaction to start or test a chemical reaction. can be used to determine the presence or absence of a specific chemical substance.

57
Q

partial pressure

A

the contribution each gas in a mixture makes towards the total pressure of the container.

58
Q

orders of reaction

A

the number /exponent that describes the effect that the concentration has on the initial rate of reaction.

59
Q

Arrhenius Equation shows…

A

the exponential relationship between the rate constant K and temperature

Chemistry (21 decks)

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