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Physical Properties
Atomic Radius: size of atoms
• Down the group: increases
• Across the period: decreases
Ionic Radius: size of stable ions
• Down the group: increases
• Across the period: decreases
First Ionisation Energy: (KJ mol-1)energy required to remove a mole
of electrons from a mole of gaseous atom
• Down the group: decreases
• Across the period: increases
First Electron Affinity: Energy change when adding an electron to a
mole of gaseous atom
Electronegativity: the ability of an atom to attract electron in a
chemical bond
...
e
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1 and Chlorine: 3
...

Thus Cl- while H+
• Down the group: decreases
• Across the period: increases
Melting Point:
• Down the group: decrease (increases for non-metal: halogens)
• Across the period: increase for metals (decrease for non metal)

EXPLANATION (mainly because):
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Nuclear Charge: Nuclear Attraction
Repulsion from inner-shell electrons: shielding effect
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Sc and Zn are not Transition Metals
• Sc can only form Sc[3+], so no d electron
• Zn can only form Zn[2+], which have completely filled 3d orbitals
Variable Oxidation Number
Usually form 2[+] because their outer shells have two electrons
(4s[2])
They can form multiple oxidation numbers because d electrons
have similar energy:adding and removing electrons are easier
Formation of Complexes
Ligands: species that can donate lone electron pair to a central
transition metal ion/atom to form dative covalent bond
Transition metals can act as a central metal ion/atom because they
can receive lone electron pair
Complexes form when ligands donate their lone electron pairs to a
central transition metal atom/ ions
Formation of colour
• d electrons have the same energy
• When transition metal forms Complex, d orbitals to splits in two (3
and 2)
• there will be an energy difference between the splitter orbitals
• when it is supplied with energy
• electrons from a lower energy level will absorb energy
• when absorbing certain energy that matches the energy difference
• electrons will excite to a higher energy level
• the complex of the colour will be complementary to the absorbed
light
Catalytic behaviour: Speed up the chemical reaction but remain
chemically unchanged
Magnetism:

Ferromagnetic - Fe Co Ni
Paramagnetic - any transitional metals with lone electrons
Diamagnetic - all electrons in d orbitals are paired
 



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