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Personal CHEM > 5. Bonding > Flashcards

5. Bonding Flashcards

1
Q

DELETE

A
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2
Q

Draw and name the shape.
Find the bond angle

A
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3
Q

Draw and name the shape.
Find the bond angle

A
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4
Q

Draw and name the shape.
Find the bond angle

A
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5
Q

Draw and name the shape.
Find the bond angle

A
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6
Q

Draw and name the shape.
Find the bond angle

A
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7
Q

Draw and name the shape.
Find the bond angle

A
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8
Q

Draw and name the shape.
Find the bond angle

A

89⁰, 119⁰

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9
Q

Draw and name the shape.
Find the bond angle

A
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10
Q

Draw and name the shape.
Find the bond angle

A
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11
Q

Draw and name the shape.
Find the bond angle

A
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12
Q

Draw and name the shape.
Find the bond angle

A
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13
Q

Draw and name the shape.
Find the bond angle

A
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14
Q

Formula for Nitrate

A

NO3⁻

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15
Q

Formula for Nitrite

A

NO2⁻

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16
Q

Formula for Hydrogencarbonate

A

HCO3⁻

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17
Q

Formula for Chlorate(I)

A

ClO⁻

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18
Q

Formula for Chlorate(V)

A

ClO3⁻

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19
Q

Describe Metallic Bonding

A
  • between 2 or more metals
  • giant metallic lattice
  • metallic → strong electrostatic attraction between positive metal ions and delocalised e-
20
Q

Describe Ionic Bonding

A
  • between metal and non metal
  • giant ionic lattice
  • ionic → strong electrostatic attraction between oppositely charged ions
21
Q

Describe Covalent (Macromolecular) Bonding

A
  • uses either Carbon or Silicon
  • macromolecular structure
  • covalent bonds between atoms
22
Q

Examples of Macromolecular

A

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

23
Q

Describe covalent (simple molecular) bonding

A
  • 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
24
Q

Coordinate Bond Definition:

A

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

25
Q

Rank the strength of repulsions between e- pairs:

A
  • 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
26
Q

Electronegativity Definition:

A

the power of an atom to attract a pair of e- in a covalent bond

27
Q

Factors affecting electronegativity

A
  • shielding
  • nuclear charge (proton number)
  • (atomic radius)
28
Q

How do you work out if a molecule is polar?

A
  1. assymetrical
      • all atoms around the central atom are the same
        • lone pair
    • 1 atom around the central atom is different
      - no lone pairs OR - >1 lone pair
29
Q

How do you work out if the molecule is non-polar?

A
  • symmetrical
  • all atoms around central atom are the same
  • no lone pairs
30
Q

Name and decribe the type of bonding

A
31
Q

Name and decribe the type of bonding

A
32
Q

Name and decribe the type of bonding

A
33
Q

Name and decribe the type of bonding

A
34
Q

Name and decribe the type of bonding

A
35
Q

Name and decribe the type of bonding

A
36
Q

When does H bonding occur?

A
  • strongest IMF
  • between a H atom (boded to an O/F/N) and a lone pair on a N/O/F atom
37
Q

How does H bonding arise?

A
  • 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
38
Q

Draw H bonding between 2 NH3 atoms

A
39
Q

When does P.D.D occur?

A
  • generally weaker than H bonding
  • occurs between polar (assymetrical molecules)
40
Q

How does P.D.D arise?

A
  • 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
41
Q

Draw P.D.D forces between 2 SbCl3 molecules

A
42
Q

When does I.D.D occur?

A
  • 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)
43
Q

How does it arise?

A

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

44
Q

How to draw it?

A
45
Q

Importance of H bonding:

A

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

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