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Chemistry > 2.2.2: Bonding and structure > Flashcards

2.2.2: Bonding and structure Flashcards

1
Q

Give the shape of water molecule H20

A

Non linear
104.5

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2
Q

Give shape of methane CH4

A

Tetrahedral
109.5

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3
Q

Give shape of ammonia molecule NH3

A

Trigonal pyrimidal
107

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4
Q

What is average bond enthalpy

A

Measurement of covalent bond strength

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5
Q

Define covalent bond

A

The strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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6
Q

Define ionic bonding

A

Electrostatic force of attraction between oppositely charged ions

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7
Q

Define dative covalent bond

A

A shared pair of electrons where both electrons are donated by one atom

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8
Q

What molecule has 2bp 0lp ?

A

Linear
180

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9
Q

What molecule has 2bp 1lp ?

A

Non linear
118

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10
Q

What molecule has 2bp 2lp ?

A

Non-linear
104.5

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11
Q

What molecule has 2bp 3lp ?

A

Linear
180

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12
Q

What molecule has 3bp 0lp ?

A

Trigonal planar
120

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13
Q

What molecule has 3bp 1lp ?

A

Trigonal pyrimidal
107

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14
Q

What molecule has 3bp 2lp ?

A

T shape
90

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15
Q

What molecule has 4bp 0lp ?

A

Tetrahedral
109.5

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16
Q

What molecule has 4bp 1lp ?

A

See-saw
90 +120

17
Q

What molecule has 4bp 2lp ?

A

Square planar
90

18
Q

What molecule has 5bp 0lp ?

A

Trigonal Bipyrimidal
120 + 90

19
Q

What molecule has 6bp 0lp ?

A

Octahedral
90

20
Q

What type of bonding is signaled by a salt ?

A

Ionic

21
Q

Give a feature of an ammonium ion

A

Has a dative covalent bond

22
Q

Why don’t solid ionic compounds conduct electricity but molten do ?

A

Solid: No mobile ions/ ions fixed in place as ionic lattice
Molten: Mobile ions

23
Q

What colour will cyclohexane turn with the addition of Cl2 to I- ions

A

Lilac

24
Q

What colour will cyclohexane turn with the addition of Br2 to Cl- ions

A

Orange

25
Q

What comment is made if there is no lone pairs ?

A

Pairs of electrons repel equally

26
Q

What comment is made if there are lone pairs ?

A

Lone pairs repel more than bond pairs

27
Q

Why does NF3 have a permanent dipole ?

A
  • F is more electronegative than N
  • Dipoles don’t cancel as molecule is pyrimidal so assymetrical
28
Q

How do London forces arise ?

A

Uneven distribution of electrons creates a temporary dipole which causes induced dipole in neighbouring
molecules

29
Q

Explain difference in melting point between Na and Mg

A
  • Mg ions have greater charge
  • Mg has more delocalised electrons
  • Mg ions have a greater charge
30
Q

Why is a 109.5 degree angle created around an atom ?

A

4 bond pairs REPEL

31
Q

Explain how the structure and bonding in bromine account for it’s relatively low melting point

A
  • London forces between molecules which are the weakest intermolecular force so require little energy to overcome
32
Q

Explain how a molecule can have a permanent dipole

A

Individual bond dipoles add up to form a molecular dipole when there are differences in electronegativity

33
Q

Explain differences in HCl and F2 boiling points interms of forces acting between molecules

A

HCl has a permanent dipole due to high electronegativity of chlorine whereas F2 has london forces between molecules

34
Q

Define electronegativity

A

The ability of an atom to attract the bonding electrons in a covalent bond

35
Q

Are hydrocarbons polar or non polar ?

A

Non polar

36
Q

Where do p.d.d ineractions exist ?

A

In molecules with a polarity

37
Q

Where can hydrogen bonds be found?

A

Between molecules containing H bonded to N,O,F

38
Q

Describe properties of water

A

-Polar molecule with H bonding
- Ice less dense than liquid water as regular lattice structure is held by hydrogen bonds with molecules further apart, reducing density
- High mp + bp as strong hydrogen bonds require a lot of energy to break

39
Q

Describe properties of simple molecular compounds

A
  • Covalent bonding
  • Low melting and boiling point
  • Soluble if polar
  • No electrical conductivity as no mobile delocalised electrons

Chemistry (38 decks)

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