DEFINITIONS Flashcards

1
Q

Relative isotopic mass

A

the mass of an isotope compared with one-twelfth of the mass of an atom of carbon-12

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2
Q

Relative atomic mass, Ar

A

the weighted mass of an atom of an element compared with one-twelfth of the mass of an atom of carbon-12

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3
Q

Relative molecular mass, Mr

A

the weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12

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4
Q

Relative formula mass, Mr

A

the weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12

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5
Q

1st ionisation energy

A

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

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6
Q

degenerate (when applied to orbitals)

A

of identical energy

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7
Q

amount of substance

A

the quantity whose unit is the mole. Used as a means of counting atoms.

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8
Q

the mole

A

the amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope

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9
Q

Avogadro constant

A

the number of atoms per mole of the carbon-12 isotope (6.02x1023 mol-1)

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10
Q

molar mass

A

the mass per mole of a substance in gmol-1

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11
Q

empirical formula

A

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

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12
Q

molecular formula

A

the actual number of atoms of eachh element in a molecule

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13
Q

anhydrous

A

substance containing no water molecules

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14
Q

hydrated

A

crystalline compound containing water molecules

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15
Q

water of crystallisation

A

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

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16
Q

Oxidation number

A

A measure of the number of electrons that an atom uses to bond with atoms of another element. Derived from a set of rules

17
Q

Reducing agent

A

A reagent that reduces another species

18
Q

Oxidising agent

A

A reagent that oxidises another species

19
Q

Ionic bond

A

The electrostatic attraction between the oppositely charged ions

20
Q

Giant ionic lattice

A

Three dimensional structure of opposite,y charged ions held together by strong ionic bonds

21
Q

Covalent bonds

A

Bond formed by a shared pair of electrons

22
Q

Lone pair

A

An outer shell pair of electrons that is not involved in chemical bonding

23
Q

Dative covalent/coordinate bond

A

Shared pair of electrons provided by one of the bonding atoms only

24
Q

Electronegativity

A

Measure of the attraction of a bonded atom for the pair of electrons in a covalent bond

25
Permanent dipole
A small charge difference across a bond that results from a difference in the electronegativities of the bonded atoms
26
polar molecule
has an overall dipole when you take into account any dipoles across the bonds
27
intermolecular force
an attractive force between neighbouring molecules
28
permanent dipole-dipole force
a weak attractive force between permanent dipoles in neighbouring polar molecules
29
van der Waals' forces
attractive forces between induced dipoles in neighbouring molecules
30
a hydrogen bond
a strong dipole-dipole attraction between: - an electron-deficit hydrogen atom on one molecule; and - a lone pair of electrons on a highly electronegative atom on a different molecule
31
metallic bonding
the electrostatic attraction between positive metal ions and delocalised electrons
32
giant metallic lattice
3d structure of positive ions and delocalised electrons, bonded together by strong metallic bonds
33
simple molecular lattic
3-d structure of molecules, bonded together by weak intermolecular forces
34
giant covalent lattice
3-d structure of atoms, bonded together by strong covalent bonds