5. Bonding Flashcards
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Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
89⁰, 119⁰
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Draw and name the shape.
Find the bond angle
Formula for Nitrate
NO3⁻
Formula for Nitrite
NO2⁻
Formula for Hydrogencarbonate
HCO3⁻
Formula for Chlorate(I)
ClO⁻
Formula for Chlorate(V)
ClO3⁻
Describe Metallic Bonding
- between 2 or more metals
- giant metallic lattice
- metallic → strong electrostatic attraction between positive metal ions and delocalised e-
Describe Ionic Bonding
- between metal and non metal
- giant ionic lattice
- ionic → strong electrostatic attraction between oppositely charged ions
Describe Covalent (Macromolecular) Bonding
- uses either Carbon or Silicon
- macromolecular structure
- covalent bonds between atoms
Examples of Macromolecular
Diamond
- each C atom has 4 covalent bonds
- tetrahedral shape
- very high mpt, very strong
- non-conductor = no free (delocalised) e-
Graphite
- layered
- each 3 atom has 3 covalent bonds
- each C atoms has delocalised e-
- layers held together by weak intermolecular forces
- soft layers can slide over each other
- conductor = has delocalised e-
- high mpt
Describe covalent (simple molecular) bonding
- Hydrogen bonding: H,F, H-N, H-O
- P.D.D: polar molecule
- I.D.D: non-polar molecular
- structure: simple molecular
- bodning: intermolecular (Hydrogen, P.D.D, I.D.D) forces between molecules
Coordinate Bond Definition:
a shared pair of e- which have both come from the same atom
represented by an arrow coming from the atom that is sharing it e-.
is exactly like a normal covalent bond
Rank the strength of repulsions between e- pairs:
- LP to LP > LP to BP > BP to BP
- to minimise repulsion, e- pairs repel each other as much as possible
- LP repel more than BP
Electronegativity Definition:
the power of an atom to attract a pair of e- in a covalent bond
Factors affecting electronegativity
- shielding
- nuclear charge (proton number)
- (atomic radius)
How do you work out if a molecule is polar?
- assymetrical
- all atoms around the central atom are the same
- lone pair
- all atoms around the central atom are the same
- 1 atom around the central atom is different
- no lone pairs OR - >1 lone pair
- 1 atom around the central atom is different
How do you work out if the molecule is non-polar?
- symmetrical
- all atoms around central atom are the same
- no lone pairs
Name and decribe the type of bonding
Name and decribe the type of bonding
Name and decribe the type of bonding
Name and decribe the type of bonding
Name and decribe the type of bonding
Name and decribe the type of bonding
When does H bonding occur?
- strongest IMF
- between a H atom (boded to an O/F/N) and a lone pair on a N/O/F atom
How does H bonding arise?
- large difference in electronegativity between N/O/F and H atom
- creates a dipole on the H-F/H-N/H-O bond
- lone pair on N/O/F atom on 1 molecules strongly attracts a 𝝳+ H atom on a different molecule
Draw H bonding between 2 NH3 atoms
When does P.D.D occur?
- generally weaker than H bonding
- occurs between polar (assymetrical molecules)
How does P.D.D arise?
- difference in electronegativity leads to bond polarity
- dipoles don’t cancel and therfore molecule has an overall permanent dipole
- attraction between 𝜹+ on one molecules and 𝜹- on another molecule
Draw P.D.D forces between 2 SbCl3 molecules
When does I.D.D occur?
- generally the weakest force, but can be stronger than both P.D.D and hydrogen bonding if the molecule is large
- occurs between all molecules (as well as atoms of nobles gases)
- most important for non-polar molecules (as they don’t have any other IMFs)
How does it arise?
RUTID
- R: random Movement of e- in 1 molecules leads to …
- U: uneven distribution of e-, creating a …
- T: temporary dipole in 1 molecules (atom). This …
- I: induces a dipole in the neighbouring molecule (atom).
- D: dipole attract
How to draw it?
Importance of H bonding:
1) ice: ice less dense than water bc the H bonds in ice hold the molecules further apart
2) proteins: proteins are held in their specific complex 3D shape by H bonds (secondary/tertiary structure)
3) DNA: 2 strands are held together by H bonds. strong enought to hold strands together but weak enough to allow strands to separate for DNA replication
