1429596
Description
Mind Map by Matthew Orr, updated more than 1 year ago
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Created by Matthew Orr
about 10 years ago
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Advanced Higher Chemistry - Unit 1
- Electromagnetic Spectrum
- Wavelength is the distance
between adjacent crests of a
wave
- Frequency is the number of
wavelengths that pass a
certain point in one second
- Increasing wavelength:
Gamma rays, X-rays,
Ultra-violet, Visible, Infra-red,
Microwaves, Radio waves
- E=Lhc/λ
- kJ per mol
- L=Avogadro's
Constant
6.02*10^23
- h=Planck's
Constant
6.63*10^-34
- c=velocity
(3*10^8 for light)
- λ=wavelength
- kJ per mol
- Wavelength is the distance
between adjacent crests of a
wave
- Oxidation States
- Uncombined elements are 0
- Monatomic ions are the charge on the ion e.g. Cl- is -1
- In most of its compounds, oxygen is -2
- In most of its compounds, hydrogen is +1
- In metallic hydrides, it is -1
- In metallic hydrides, it is -1
- Fluorine is always -1
- Oxidation is an increase in oxidation number.
Reduction is a decrease in oxidation number.
- Uncombined elements are 0
- Shapes of Molecules
- Resonance Structures
- The bonds in ozone are all the same length
- Shapes
- 2 electron pairs give a
linear arrangement
- BeCl2
- BeCl2
- 3 electron pairs give a trigonal
arrangement
- BCl3
- BCl3
- 4 electron pairs give a
tetrahedral arrangement
- CH4
- CH4
- 5 electron pairs give a
trigonal bipyramidal
arrangement
- PCl5
- PCl5
- 6 electron pairs give an
octahedral arrangement
- SF6
- SF6
- 2 electron pairs give a
linear arrangement
- Resonance Structures
- Ionic Lattices, Superconductors and Semiconductors
- Ionic Lattices
- Face Centred Cubic
- NaCl
- Cation:Anion ratio less than 0.8
- NaCl
- Body Centred Cubic
- CsCl
- Cation:Anion ratio more than 0.8
- CsCl
- Face Centred Cubic
- Superconductors
- Superconductors
have almost no
electrical resistance
at low temperatures
- "High temperature"
superconductors can remain
superconductive above -196 C
- Used in transmission
of energy, electronics
and medicine (MRI)
- Used in transmission
of energy, electronics
and medicine (MRI)
- Superconductors
have almost no
electrical resistance
at low temperatures
- Semiconductors
- These are part of
the metalloids
- Electrical conductivity
increases with temperature
- Also increases
with exposure
to light
- Also increases
with exposure
to light
- These can be "doped"
with either a group 3 or
group 5 element
- Group 5 gives an "n" type
semiconductor with an
extra electron which
increases the conductivity
- Group 3 gives a "p" type
semiconductor with a small
positive hole which
increases the conductivity
- Group 5 gives an "n" type
semiconductor with an
extra electron which
increases the conductivity
- These are part of
the metalloids
- Ionic Lattices
- Chemical Bonding
- Electronegativity
- A high difference in
electronegativity
values between the
elements gives an ionic
bond while a low one
gives a non-polar
covalent bond
- A high difference in
electronegativity
values between the
elements gives an ionic
bond while a low one
gives a non-polar
covalent bond
- Dative Bonds
- These occur when
one atom provides
both electrons for a
covalent bond
- These occur when
one atom provides
both electrons for a
covalent bond
- Lewis Electron Dot Diagrams
- These are used to
represent bonding and
non-bonding pairs in
molecules and
polyatomic atoms
- These are used to
represent bonding and
non-bonding pairs in
molecules and
polyatomic atoms
- Electronegativity
- Orbital Shapes
- There are four main
quantum numbers
which determine the
properties of the atom
- Principal=n.
This describes
the shell
occupied by an
electron
- Angular momentum=l.
This describes the
shape of the orbital
- Magnetic=m.
This describes
the orientation
of the orbital
- Spin=s. This
describes the
electron spin
of the electron
in the orbital
- Principal=n.
This describes
the shell
occupied by an
electron
- Heisenberg's Uncertainty Principle
- It is impossible to define with
absolute precision, simultaneously,
both the position and momentum of
an electron
- It is impossible to define with
absolute precision, simultaneously,
both the position and momentum of
an electron
- Pauli Exclusion Principle
- No two electrons in an
atom can have the
same four quantum
numbers
- No two electrons in an
atom can have the
same four quantum
numbers
- Orbitals
- S Orbitals
- Spherical in shape
- Only have one orientation
- Spherical in shape
- P Orbitals
- Dumbbell shaped
- Three orientations: px, py and pz
- px lies on x-axis etc
- px lies on x-axis etc
- Dumbbell shaped
- D Orbitals
- Four are double
dumbbells, one is
dumbbell with a ring
around the centre
- Five orientations: dz^2,
dx^2-y^2, dxy, dyz, dxz
- dz^2 has a ring,
dx^2-y^2 lies on x and y
axes, rest lie between
corresponding axes
- dz^2 has a ring,
dx^2-y^2 lies on x and y
axes, rest lie between
corresponding axes
- Four are double
dumbbells, one is
dumbbell with a ring
around the centre
- S Orbitals
- There are four main
quantum numbers
which determine the
properties of the atom
- Transition Metal Complexes
- Ligands and Complexes
- Ligands are negative ions or
uncharged molecules with
one or more lone pairs of
electrons
- Monodentate ligands
have one lone pair
- Bidentate ligands
have two lone pairs
- Monodentate ligands
have one lone pair
- Complexes are metal ions
surrounded by ligands
- Ligands are negative ions or
uncharged molecules with
one or more lone pairs of
electrons
- Naming Complexes
- Ligands first in
alphabetical order then the
metal and its oxidation
state
- Ligands that end with -ide
change the ending to -o
- Ammonia becomes ammine
and water becomes aqua
- If the complex is
a negative ion,
the metal ends in
-ate
- Iron becomes ferrate
- Ligands first in
alphabetical order then the
metal and its oxidation
state
- Colour in Transition Metal Complexes
- The colour of a
complex is caused by
the splitting of the 3d
orbital of the central
metal ion
- CN->NH3>H2O>OH->F->Cl->Br->I-
- The ligands cause the split
- The colour seen will be complimentary to the
colour that corresponds to the colour with the
same energy as that of the d-d transition
- The colour of a
complex is caused by
the splitting of the 3d
orbital of the central
metal ion
- Ligands and Complexes
- Oxides, Chlorides and Hydrides
- Oxides
- Go from Na2O to Cl2O
- Go from ionic
lattice to
covalent
molecular
- Go form basic to
amphoteric and
then to acidic
- Go from Na2O to Cl2O
- Chlorides
- Go from NaCl to Cl2
- Go from ionic lattice to
covalent molecular
- The first two are soluble in
water, AlCl3 to SCl2 all give off
fumes of HCl and Cl2 dissolves
to form an acidic solution
- Go from NaCl to Cl2
- Hydrides
- Go from NaH to HCl
- Go from ionic lattice to covalent molecular
- Go from strongly
alkaline to neutral
then to strongly
acidic
- Go from NaH to HCl
- Oxides
- Emission Spectra
- Each element
produces a different
emission spectrum
- The lines seen are due to photons being emitted
when electrons drop from one energy level to a
lower one. Each line corresponds to a certain
energy which in turn corresponds to a colour
- When an electron absorbs
energy of a certain amount, it
moves from its ground state
to a higher energy level.
- There are three main series of
lines: the Paschen Series, the
Lyman series and the Balmer
series
- The Paschen series is the
infra-red area of the spectrum
and involves electrons falling
to the n=3 energy level
- The Lyman series is the
ultra-violet area of the
spectrum and corresponds to
falls into the n=1 energy level
- The Balmer series is the
visible area of the
spectrum and
corresponds to falls into
the n=2 energy level
- The Paschen series is the
infra-red area of the spectrum
and involves electrons falling
to the n=3 energy level
- Each element
produces a different
emission spectrum
- Electronic Configuration
- Aufbau Principle
- Sub-shells with lower energy are filled first
- 4s filled before 3p
- Sub-shells with lower energy are filled first
- Hund's Rule
- Electrons fill degenerate
orbitals singly before
pairing up
- Electrons fill degenerate
orbitals singly before
pairing up
- Spectroscopic Notation
- e.g. Lithium: Normal= 2, 1
Spectroscopic= 1s^2, 2s^1
- e.g. Lithium: Normal= 2, 1
Spectroscopic= 1s^2, 2s^1
- Orbital Box
- Aufbau Principle
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