This page encompasses all of the patterns in the periodic table including the: atomic radius, ionic radius, ionisation energy, electron affinity, electronegativity, metallic characteristics, oxides for Chapter 3. For Chapter 13, all of the characteristics of transition metals are described.
Samenvatting Ib Course Book Chemistry 2014 - Scheikunde
Option D: Medicinal Chemistry (IB Chemistry)
Chapter 11 & 21, Measurements & Data Processing (IB Chemistry)
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Periodic table trends
Transition Metals
electron affinity *
ionisation
energy VARIABLE OXIDATION STATES
D
A A • when orbitals are occupies, the expulsion between electrons pushes 4s into a higher energy
METALLIC CHARACTERISTICS
state, so it becomes lightly higher in energy then 3d, losing its electron first
• METALS: 1-3 outer shell
• transition metal ions with +3 tend to be POLARISING, have a HIGH CHARGE Density and
Alkaline
metals vigorously
be * electrons, low IE, low
pull on electrons
-react Het d
electronegativities (due to
-
-
S
with halogens
h A
delocalised electrons COMPLEX IONS
• NON-METALS: 4-7 electrons in • central metal ion + ligand
h T character 8 outer shell, high electronegativity, • LIGAND: a molecule or ion that form complexes which consist of a central metal ion and ligands
E
+ E & high EA (tendency to share —> LEWIS BASE, NUCLEOPHILE
non-metallic
S -'
W
: character - i P
5
↑
electrons and form covalent bonds • CO-ORDINATION NUMBER: number of co-ordinate bonds to the central metal atom or ion
r - • NAMING COMPLEXES: prefix for number of ligands/ligands name/element/oxidation number
metallic
8
OXIDES:
-
d e • Na and Mg oxides are basic
V
=
• Al oxides are amphoteric CATALYTIC PROPERTIES
#
• Si to Cl oxides are acidic
• can catalyse certain REDOX REACTIONS —> can be readily oxidised and reduced
*
* • HETEROGENOUS catalyst has a different physical state (phase) from the reactants
atomic radius
# • HOMOGENOUS catalyst is the same physical state (phase) as the reactants
ELECTRON AFFINITY • BIOLOGICAL catalysts
ATOMIC RADIUS
• distance between nucleus of an atom & outermost electron shell • amount of energy released when 1 mole of
electrons is gained by 1 mole of atoms of gaseous MAGNETIC PROPERTIES
• ACROSS A GROUP: nuclear charge increases = greater pull
state to form gaseous ion (- charge) • DIAMAGNETISM: the property of all materials and produces a very weak opposition to an
• DOWN A GROUP: increase in number of shells, increase in
• first EA = exothermic applied magnetic field —> from repulsion of electrons to the applied magnetic field, create a tiny
shielding, weak pull
• second EA = endothermic (overcoming repulsion magnetic dipole
between electrons and - ion) • PARAMAGENTISM: only occurs in substances which have unpaired electrons, produces
IONIC RADIUS
magnetism proportional to the applied field in the same direction
• measure of size of an ion
• FERROMAGNETISM: the alignment of the unpaired electrons in an external field can be
• DOWN A GROUP = increases ELECTRONEGATIVITY
retained so that material becomes permanently magnetised
• ACROSS A PERIOD: ionic radii increases with an increase • the ability of an atoms to attract a pair for electrons
in - charge, ionic radii decreases with an increase in + charge towards itself in a covalent bond
COLOURED COMPOUNDS:
• arises form the + nucleus ability to attract - charged
• d-block elements have unpaired electrons
electrons
IONISATION ENERGY • the d-orbitals are split into two energy levels
• PAULING SCALE - assigned electronegativity value
• DOWN A GROUP= increase in nuclear charge, increase in • electrons can transition between these energy levels
• FLUORINE most electronegative
shells, increase in shielding, increase in atomic radius, • in the meantime they can absorb energy form light at a visible wavelength and thus, one can
• DOWN A GROUP = negligible nuclear charge increase,
electrons held more loosely observe the complimentary colour
increase in shielding, increase in atomic radius, decrease
• ACROSS A PERIOD = increase in nuclear charge, shells
in attraction of nucleus and electron
remain the same, shielding remains constant, decrease in
atomic radius, electrons held more tightly
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