INORGANIC CHEMISTRY DEFINITIONS

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Relative Atomic Mass
The mean mass of an atom of an element compared to 1/12 of a Carbon 12 atom.
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Relative Isotopic Mass
The mass of an atom of an isotope compared to 1/12 of a Carbon 12 atom.
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Relative Molecular Mass
The average mass of a molecule compared to 1/12 of a Carbon 12 atom.
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What goes on the X and Y axis?
The X axis is the independent variable (the cause), the Y axis is the dependent variable (the effect)
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1st Ionisation Energy
The energy required to remove 1 mol of electrons from 1 mol of gaseous ions.
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2 Bond Pairs
Linear, 180
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3 Bond Pairs
Trigonal Planar - 120
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4 Bond Pairs
Tetrahedral - 109.5
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3 Bond Pairs, 1 Lone Pair
Trigonal pyramidal - 107
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2 Bond Pairs, 2 Lone Pairs
'Bent' - 104.5
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6 Bond Pairs
Octahedral - 90
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5 Bond Pairs
Trigonal bipyramidal - 120 and 90
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4 Bond Pairs, 1 Lone Pair
'Seesaw' - 87 and 102
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3 Bond Pairs, 2 Lone Pairs
'Distorted T' 87.5
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4 Bond Pairs, 2 Lone Pairs
Square Planar (cis-platin) - 90
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2 Bond Pairs, 1 Lone Pair
(SO2) 'Bent' 119
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Thermal Stability of group 2 Carbonates down the group?
Increases, as the Cation is less polarising and distorts the Carbonate group less, the bonds are more stable. (lower charge density)
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Flame Colour - Lithium
Red
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Flame Colour - Barium
Green
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Flame Colour - Potassium
Lilac
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Flame Colour - Calcium
Brick Red
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Flame Colour - Sodium
Orange
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Physical State - Fluorine
Pale Yellow Gas
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Physical State - Chlorine
Green Gas
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Physical State - Bromine
Brown Liquid
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Physical State - Iodine
Grey Solid
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Colour in Water for Chlorine, Bromine and Iodine
Chlorine is a colourless solution - Bromine is a yellow/orange solution - Iodine is a brown solution.
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Colour in Hexane for Chlorine, Bromine and Iodine
Chlorine is colourless, Bromine is orange/red, Iodine is Pink
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Standard Lattice Energy
The enthalpy change when 1 mol of an ionic SOLID is formed from its GASEOUS ions under standard conditions
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Enthalpy Change of Hydration
The enthalpy when one mol of GASEOUS ions dissolves in WATER
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Enthalpy Change of Solution
The enthalpy change when I mol of SOLUTE dissolves in WATER
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What affacts your Lattice Energy and why?
The charge on the ion and the size - The larger the charge density, the stronger the electrostatic forces between the ions, so more energy is released making the lattice energy MORE EXOTHERMIC
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Why would experimental values differ from theory values when calculating lattice energy?
The theory value is based on the fact that the ions are purely spherical and there is no distortion/covalent character - this is not always the case, more covlalent character = more exothermic
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What affects Enthalpy of Hydration?
Again, charge density. Ions with a higher charge are better at attracting the polar water molecules, so electrostatic forces of attraction are stronger and more energy is released when the bonds are made, so more exothermic enthalpy of hydration!
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Why is the enthalpy of hydration usually so negative?
Bonds between the ions must break = Endothermic. The energy released when the Ions form bonds with water must be GREATER
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Gibbs Free Energy
DeltaG = DeltaH - TDeltaSsystem
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Standard Electrode Potential of a half cell
The voltage measured under standard conditions when a half-cell is connected to a standard hydrogen electrode
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Standard Conditions
100 kPa (1 atm), 298 K, 1.0 mol dm3 solutions
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Transition Metal
D-Block elements that can form one or more complex ions due to it's variable oxidation states, with partially filled d orbitals
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Complex Ion
A metal ion surrounded by one or more dative covalently bonded ligands.
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Other cards in this set

Card 2

Front

The mass of an atom of an isotope compared to 1/12 of a Carbon 12 atom.

Back

Relative Isotopic Mass

Card 3

Front

The average mass of a molecule compared to 1/12 of a Carbon 12 atom.

Back

Preview of the back of card 3

Card 4

Front

The X axis is the independent variable (the cause), the Y axis is the dependent variable (the effect)

Back

Preview of the back of card 4

Card 5

Front

The energy required to remove 1 mol of electrons from 1 mol of gaseous ions.

Back

Preview of the back of card 5
View more cards

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