Topic 6: s & p Block Elements
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Electronegativity
An atoms ability to draw electron density towards itself
Electronegativity can lead to … of a covalent bond where electron density is pulled towards the … atom. This results in … . A … bond with … like this is sometimes referred to as having … .
polarization most electronegative partial negative and partial positive charges covalent partial charges ionic character
As well as effective nuclear charge and principle quantum number, electronegativity can depend on … and …
oxidation state hybridization
A … can polarise a … in an ionic bond so the ionic bond has …
cation anion covalent character
The polarisability of an atom is … Atoms are polarisable if …
its ability to be distorted by an electric field the electron cloud can be distorted easily (often larger anions)
We … see a purely ionic/covalent bond
rarely
sp3 has a … electronegativity value than sp2
lower
Metals form … oxides while non-metals form … oxides
basic acidic
Electronegativities of metals, metalloids and non-metals
Metals: < 1.9 Metalloids: 1.9-2.2 Non-metals: >2.2
Requirements for something to be metal:
Partially filled band Electrons delocalised so can move easily between orbitals
Amphoteric
display basic and acidic behaviour
Why are there favoured oxidation states?
For the s- and p-block, the most important factor determining oxidation state is a closed shell electronic configuration Atoms prefer to follow the octet rule
The favoured oxidation values tend to vary by … to …
+/- 2 avoid radicals
The favoured oxidation state … down the group as …
can change (lower) there’s an increasing tendency for ns2 electrons to be left out of bonding so only used p electrons for bonding (inert pair effect)
If it costs energy to promote an electron, how can it be energetically favourable?
More strong bonds can be formed
How do electron promotion energies change down the group
general increase
When atoms get larger, their bonds get …
weaker
bond energy
the amount of energy required to break a bond into neutral atoms
larger bond energy =
stronger
…, … and … single bonds are … so go against the trend because …
N-N, O-O and F-F weak they’re small atoms so sit very close together in a single bond. This means their adjacent lone pairs experience significant repulsion
Bonds tend to be … if the atoms are different sizes due to …
weaker poor overlap
Homonuclear bonds tend to be … than heteronuclear bonds
weaker
Whether a reaction is favourable is based on …
the energy required to break bonds and released when forming them
multiple bonding is common in … of the p-block but … because …
the first row not in the other rows larger atoms have poorer p-orbital overlap so form weaker pi bonds