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Chemistry A-level > Definitions > Flashcards

Definitions Flashcards

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1
Q

Isotope

A

Atoms of the same element with different numbers of neutrons and therefore different masses

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2
Q

Relative isotopic mass

A

the mass of an atom of an isotope compared with 1/12th of the mass of an atom of carbon-12

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3
Q

Relative atomic mass

A

the wieghted mean mass of an atom of an element compared with 1/12th of the mass of an atom of carbon-12

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4
Q

Relative molecular mass

A

the weighted mean mass of a molecule compared with 1/12th of the mass of carbon-12

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5
Q

Relative formula mass

A

the weighted mean mass of a formula unit compared with 1/12th of the mass of carbon-12

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6
Q

1st ionisation energy

A

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

  • Nuclear charge
  • shielding
  • atomic radius
  • nuclear attraction
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7
Q

Oxidation

A

the loss of electrons ((formation of +ions))

an increase in the oxidation number (becomes more positive)

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8
Q

Reduction

A

the gain of electrons ((formations of -ions))

a decrease in oxidation number (becomes less positive)

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9
Q

Oxidising agent

A

a reagent that oxidises (takes electrons from) another species

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10
Q

Reducing agent

A

a reagent that reduces (gives electrons to) another speicies

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11
Q

Acid

A

an acid releases H+ ions in aqueous solution

an acid is a proton donor

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12
Q

weak acid / strong acid

A

A strong acid is fully dissociated in solution and a weak acid partially partially dissociated

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13
Q

Base

A

A proton acceptor

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14
Q

Alkali

A

A soluble base that releases OH- ions in water (/solution)

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15
Q

Salts

A

Salts are ionic compounds formed when the H+ ions in an acid are replaced by metal or ammonium ions

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16
Q

ionic bonding

A

electrostatic attraction between positive and negative ions

17
Q

covalent bonding

A

The stong electrostatic attractions between a shared pair of electrons and the nuclei of bonded atoms

18
Q

lone pair

A

a pair of electrons in the outer shell not used in the bonding

19
Q

dative covalent bond

A

A shared pair of electrons in which the bonded pair is provided by one of the bonded atoms only

20
Q

Average bond enthalpy

A

The average enthalpy that takes place when breaking by homolytic fission one mole of a given type of bond in molecules of a gaseous species

21
Q

metallic bonding

A

The electrostatic attraction between positive metal ions and delocalised electrons

22
Q

malleable

A

can easily be bent into different shapes

23
Q

ductile

A

can be drawn into a wire

24
Q

gaint ionic lattice

A

there is a continuous lattice arrangement of + and - ions in three dimensions

25
Q

VSEPR

A

Valence shell electron pair repulsion

  • electron pairs repel each other
  • the repulsion between lone pair-lone pair>lone pair-bonded pair>bonded pair-bonded pair
26
Q

Van der Waals

A

London forces and permanent dipole-dipole forces

27
Q

London forces

A

The London dispersion force is the weakest intermolecular force. The London dispersion force is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. This force is sometimes called an induced dipole-induced dipole attraction.

28
Q

electronegativity

A

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

29
Q

Pauling value

A

defines the electronegativity of an element.

30
Q

permanent dipole

A

a small charge difference that does not change across a bond with partial charges on the bonding atoms (the result of the bonded atoms having different electronegativities)

31
Q

Polar covalent bond

A

A bond with a permanent dipole, with positive and negative partial charges on bonded atoms

32
Q

Polar molecule

A

a molecule with an overall dipole hving taken into account any dipoles across bonds and the shape of the molecule and its structure

33
Q

Hydrogen bond

A

a hydrogen bond is a strong dipole-dipole attraction between an electron difficient -NH, OH, HF on one molecule and a lone pair of electrons on a highly electronegative atom (N,O,F) on a different atom

34
Q

Group (on periodic table)

A

A vertical column in the periodic table. Elements in a group have similar chemical properties and their atoms have the same number of outer shell electrons.

35
Q

Period (on periodic table)

A

Horizontal rows in periodic table. Elements show trends in properties across the period

36
Q

Subshell

A

A subshell is a group of the same type of orbital

37
Q

Orbitals

A

Orbitals are regions of an atom containing up to two electrons with opposite spin

Chemistry A-level (4 decks)

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