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A Level Chemistry > Definitions > Flashcards

Definitions Flashcards

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1
Q

Define relative atomic mass

A

the weighted mean mass of an atom of an element relative to 1/12 of the mass of an atom of 12C

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2
Q

Define relative isotopic mass

A

the mass of an atom of an isotope compared to 1/12 the mass of an atom of 12C

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3
Q

Define 1st ionisation energy

A

the energy required to remove 1 electron from each atom in 1 mole of a gaseous element to form 1 mole of gaseous 1+ ions

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4
Q

Define nuclear attraction

A

the attractive force that the outer shell of electrons experiences from the nucleus

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5
Q

Define shielding

A

the repulsion between electrons in inner shells

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6
Q

Define an orbital

A

a region within an atom that can hold up to 2 electrons with opposite spin

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7
Q

Define a subshell

A

a group of the same type of atomic orbitals within a shell

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8
Q

Define electronegativity

A

the ability of an atom to attract the bonding pair of electrons in a covalent bond

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9
Q

Define a hydrogen bond

A

the attraction between the d+ H atom on 1 molecule and the lone pair of electrons on the d- Fluorine, Nitrogen or Oxygen on a different molecule

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10
Q

What is the equation for finding the number of particles in a substance?

A

number of particles = ( mass (g) / molar mass (g/mol) ) x 6.02x10^23
(number of particles = moles x 6.02x10^23)

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11
Q

What is the equation for atom economy?

A

atom economy = ( sum of molar masses of desired products / sum of molar masses of all products ) x 100

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12
Q

What is the equation for percentage yield?

A

percentage yield = (actual yield / theoretical yield ) x100

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13
Q

What is the ideal gas equation? What are the units?

A

pV = nRT

pressure(Pa) x volume(m^3) = number of moles x gas constant x temperature(K)

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14
Q

What is the gas constant?

A

8.314 J/mol/K

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15
Q

How do you convert celsius to kelvin?

A

add 273 degrees

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16
Q

What is Avagadro’s constant?

A

6.02 x10^23

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17
Q

Define molecular formula

A

the exact number of atoms of each element present in a molecule

18
Q

Define empirical formula

A

the simplest whole number ratio of atoms in a molecule

19
Q

Define homologous series

A

a series of compounds with the same functional group, with each successive member differing by a CH2 group, and having the same general formula

20
Q

Define homolytic fission

A

when a covalent bond breaks and one electron from the bonding pair is given to each atom previously involved in the bond to create 2 free radicals

21
Q

Define a radical

A

an atom with a single unpaired electron that is very reactive

22
Q

Define heterolytic fission

A

when a covalent bond breaks and one atom takes both of the bonding pair of electrons to become a negative ion, leaving the other atom as a positive ion

23
Q

Define a sigma bond

A

the overlapping of 2 orbitals directly in the plane of the 2 atoms

24
Q

Define hydrolysis

A

using water to break chemical bonds

opposite of condensation

25
Q

Define standard enthalpy of combustion

A

the enthalpy change when 1 mole of a substance is completely combusted with oxygen under standard conditions with all products and reactants in their standard states

26
Q

Define standard enthalpy of neutralisation

A

the enthalpy change when 1 mole of water is produced by the reaction of an acid and a base, under standard conditions

27
Q

Define standard enthalpy of formation

A

the enthalpy change when 1 mole of a substance is formed from its elements under standard conditions

28
Q

Define standard enthalpy of atomisation

A

the enthalpy change when 1 mole of gaseous atoms of a substance are formed from the substance in its standard state, under standard conditions

29
Q

What are standard conditions?

A

298 degrees K and 100kPa

30
Q

Define enthalpy change of reaction

A

the enthalpy change accompanying a reaction in the molar quantities shown under standard conditions, with reactants and products in their standard states

31
Q

Define first electron affinity

A

the enthalpy change when each atom in one mole of gaseous atoms gains one electron to form one mole of gaseous 1- ions

32
Q

Define second electron affinity

A

enthalpy change when each ion in one mole of gaseous 1- ions gains one electron to form one mole of gaseous 2- ions.

33
Q

Define hydration enthalpy

A

enthalpy change when one mole of gaseous ions becomes hydrated (dissolved in water) (g) => (aq)

34
Q

Define enthalpy of solution

A

the enthalpy change when one mole of an ionic solid is dissolved
in an amount of water large enough so that the dissolved ions are well separated and do not interact with each other

35
Q

Define bond dissociation enthalpy

A

the enthalpy change when one mole of covalent bonds is broken in the gaseous state

36
Q

Define lattice enthalpy of formation

A

the enthalpy change when one mole of a solid ionic compound is formed from its constituent ions in the gas phase (g) => (s)

37
Q

Define lattice enthalpy of dissociation

A

the enthalpy change when one mole of a solid ionic compound is broken up into its constituent ions in the gas phase (s) => (g)

38
Q

Define enthalpy of vaporisation

A

enthalpy change when one mole of liquid is turned into a gas (l) => (g)

39
Q

Define enthalpy of fusion ?

A

the enthalpy change when one mole of a solid is turned into a liquid (s) => (l)

40
Q

Define enthalpy of neutralisation

A

the enthalpy change when 1 mole of water is formed in a reaction between an acid and an alkali under standard conditions

41
Q

Define standard electrode potential

A

the electromotive force of a half cell compared to the standard hydrogen electrode measured at 298K, solution conc. 1 moldm-3 and at a pressure of 100kPa

42
Q

Define a condensation polymer

A

a long chain molecule formed by the joining together of monomers with the loss of a small molecule (H2O or HCl)

A Level Chemistry (30 decks)

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