definitions Flashcards

1
Q

isotope

A

atoms of the same element with the same number of protons but different number of neutrons

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2
Q

relative atomic mass

A

the weighted mean mass
of an atom of an element
compared to the mass of 1/12th of an atom of carbon-12

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3
Q

relative isotopic mass

A

the weighted mean mass
of an atom of an isotope
compared to the mass of 1/12th of an atom of carbon-12

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4
Q

atomic orbital

A

a region within an atom that holds up to 2 electrons with opposite spins

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5
Q

ionic bonding

A

electrostatic attraction between oppositely charged ions

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6
Q

metallic bonding

A

electrostatic attraction between positive metal ions and a sea of delocalised electrons

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7
Q

covalent bonding

A

electrostatic attraction between positive nuclei and shared pair of electrons

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8
Q

dative bond

A

a type of covalent bond in which both of the electrons
in the shared pair come from one atom.

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9
Q

mass spectometry

A

an instrument which gives accurate information about relative isotopic
mass and the relative abundance of isotopes.

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10
Q

amount of substance

A

the number of particles in the substance, measured in moles

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11
Q

mole

A

a unit containing exactly 6.02x10’23 elementary entities

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12
Q

molar mass

A

mass per mole of a substance (units: g mol-1)

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13
Q

waters of crystallisation

A

water molecules that form part of the crystalline structure of a
compound

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14
Q

hydrated

A

a crystalline compound that contains water

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15
Q

anhydrous

A

a crystalline compound that contains no water

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16
Q

empirical formula

A

the simplest whole number ratio of atoms of each element present in a
compound

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17
Q

acid

A

compounds that release H+ ions in aqueous solution.

18
Q

alkali

A

water soluble bases. Alkalis release OH- ions into aqueous solution

19
Q

base

A

a substance that can accept H+ ions from another substance.

20
Q

strong acid

A

an acid that completely dissociates in solution

21
Q

weak acid

A

an acid that partially disassociates in solution

22
Q

oxidation

A

loss of electrons

23
Q

reduction

A

gain of electrons

24
Q

oxidation number

A

a number that represents the number of electrons lost/gained by an
atom of an element

25
energy level
the shell that an electron is in
26
subshell
a subdivision of the electronic shells into different orbitals
27
average bond enthalpy
the average energy required to break a bond, used as a measurement of the strength of a covalent bond
28
bonding pair
a pair of outer-shell electrons involved in bonding
29
electronegativity
the ability of an atom to attract bonding electrons in a covalent bond
30
lone pair
a pair of outer-shell electrons not involved in bonding
31
enthalpy change
the change in heat energy of a substance at constant pressure
32
hess' law
the enthalpy change for a chemical reaction is independent of the route taken sum of clockwise enthalpy= sum of anti-clockwise enthalpy
33
standard conditions
100kPa 298k
34
standard enthalpy change of formation
- when one mole of product is formed - from it's products - under standard conditions
35
standard enthalpy change of combustion
-when one mole of substance - burns completely in excess oxygen - under standard conditions
36
standard enthalpy change of neutralisation
- when one mole of water is formed - from a neutralisation reaction - under standard conditions
37
ionisation
removal of an electron form an atom to form a positive ion
38
first ionisation energy
the energy needed to remove one electron from each atom in a mole of gaseous atoms to make one mole of gaseous unipositive ions.
39
second ionisation energy
the energy needed to remove one electron from each atom in a mole of gaseous unipositive ions to make one mole of gaseous dipositive ions
40
successive ionisation energy
amount of energy needed to remove the first, second, and subsequent electrons from one mole of gaseous atoms
41
ionic lattice
a repeating pattern of oppositely charged ions