chemistry

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Isotope
Same number of protons and electrons, different number of neutrons
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acid
Proton donor
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base
proton acceptors
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strong acid
Dissociates fully in water
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weak acid
Partially dissociates in water
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salt
When the H+ ion in an acid is replaced with a metal (ammonium) ion
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alkali
Dissociate to give hydroxide ions in water
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acid reactions
Metal+acid=Salt+hydrogen Metal oxide+acid=Salt+water Metal hydroxide + acid à Salt + water Metal carbonate+acid=Salt+water=carbon dioxide
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% element
No of that element x Ar x 100 Mr
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oxidation and reduction
Oxidation is loss of electrons Reduction is gain of electrons
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relative isotopic mass
mass of an atom of an isotope compared with 1/12 of the mass of an atom of 12C
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relative atomic mass
weighted mean mass of an atom of an element compared with 1/12 of the mass of an atom of 12C
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relative molecular mass
weighted mean mass of an molecule compared with 1/12 of the mass of an atom of 12C
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relative formula mass
weighted mean mass of a formula unit compared with 1/12 of the mass of an atom of 12C
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relative atomic mass equation
(% x Ar) + (% x Ar) 100
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empirical formula
simplest whole number ratio of atoms of each element in a compound
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molecular formula
actual whole number ratio of atoms of each element in a compound
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moles s
mass (g) / Mr
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moles aq
(Aq) = Conc (mol dm-3) x Vol (dm3)
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moles g
(g) = Vol (dm3) / 24 (dm3)
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1st ionisation energy
energy required to remove 1 electron from each atom in a mole of gaseous atoms to form 1 mole of gaseous 1+ ions
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orbital
region in space around the nucleus that can contain 2 electrons with opposite spins
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ionic bonding
Electrostatic force of attraction between oppositely charged ions
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covalent bond
Formed by a pair of shared electrons
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dative covalent bond
Formed by a pair of shared electrons where both electrons are provided by one atom
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what determines the shape of a molecule
Pairs of electrons repel as far as possible This determines the shape · Lone pairs repel more than bonding pairs as closer to central atom Each lone pair reducing the bond angle by 2.5o as it is closer to the central atom
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electronegativity
The power of an atom to attract bonding pairs of electrons towards itself
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metallic bonding
Electrostatic forces of attraction between metal ions and delocalised electrons
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conductivity of metals
Electrons are free to move
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conductivity of ionic compounds
Solid – does not conduct as ions in a fixed position Molten / dissolved – does conduct electricity as ions are free to move
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Other cards in this set

Card 2

Front

acid

Back

Proton donor

Card 3

Front

base

Back

Preview of the front of card 3

Card 4

Front

strong acid

Back

Preview of the front of card 4

Card 5

Front

weak acid

Back

Preview of the front of card 5
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