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Chemistry M2 > Section 4 > Flashcards

Section 4 Flashcards

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1
Q

Shapes of molecules

What does the dotted line show

A

Bond pointing away

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2
Q

Shapes of molecules

What does block line show

A

Bond facing towards you

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3
Q

Shapes of molecules

2 bonding pairs

A

Linear

180

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4
Q

Shapes of molecules

3 bonding pairs

A

Trigonal planar

120

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5
Q

Shapes of molecules

4 bonding pairs

A

109.5

Tetrahedral

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6
Q

Shapes of molecules

3 bonding pair and 1 lone pair

A

Trigonal pyramidal

107

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7
Q

Shapes of molecules

5 bonding pairs

A

120 and 90

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8
Q

Shapes of molecules

6 bonding pairs

A

90

Octahedral

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9
Q

Why do shapes become squished when there’s a lone pair?

A

Because the lone pair/bonding pair repulsion is stronger than the bonding pair/bonding pair repulsion

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10
Q

Electronic structure

s electrons

A

2

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11
Q

Electronic structure

p electrons

A

6

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12
Q

Electronic structure

d electrons

A

10

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13
Q

Electronic structure

f electrons

A

14

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14
Q

Electronic structure

1st shell

A

2

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15
Q

Electronic structure

2nd shell

A

8

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16
Q

Electronic structure

3rd shell

A

18

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17
Q

Electronic structure

4th shell

A

32

18
Q

Electronic structure

p orbital shape

A

3 p-orbitals at right angles to each other

19
Q

Electronic structure

Why does 4s fill up before 3d?

A

It has a lower energy level even though it has a higher principal quantum number

20
Q

Electronic structure

Electron configuration up to 3d

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10

21
Q

Ionic bonding

A

Attraction between oppositely charged ions

22
Q

Ionic bonding

Electrical conductivity

A

Conduct when molten or dissolved but not when solid because ions are free to move in liquid but are fixed in place by ionic bonds in solid

23
Q

Ionic bonding

Melting and boiling points

A

High mp and bp because a lot of energy is needed to overcome these forces

24
Q

Ionic bonding

Solubility

A

Dissolve in water

Water molecules are polar so have small charges which pull ions away from lattice

25
Q

Covalent bonding

A

Electrostatic attraction between a shared pair of electrons

26
Q

Covalent bonding

Dative covalent bonding

A

One of the atoms provides both the sharing electrons

27
Q

Covalent bonding - special cases

6 electrons in outer shell

A

boron trifluoride

28
Q

Covalent bonding - special cases

12 electrons in outer shell

A

sulphur hexafluoride

29
Q

Covalent bonding

How to find out strength

A

Average bond enthalpy

Energy required to break covalent bond

30
Q

Polarisation

Electronegativity

A

The ability for an atom to attract electrons in a covalent bond

31
Q

Polarisation

Non-polar

A

No overall dipole

32
Q

Polarisation

Polar

A

Has an overall dipole

33
Q

Intermolecular forces

Induced - larger molecules

A

Have a larger electron cloud meaning stronger induced dipole dipole

34
Q

Intermolecular forces

Permanent

A

Delta charges cause weak electrostatic forces of attraction between molecules

35
Q

Intermolecular forces

Hydrogen - ice less dense

A

Ice has more hydrogen bonds are they’re relatively long so the molecules will be further apart making it less dense

36
Q

Simple covalent compounds

A

Have weak forces between molecules which affects their physical properties

37
Q

Simple covalent compounds

Electrical conductivity

A

The covalent molecules are uncharged so cannot conduct electricity

38
Q

Simple covalent compounds

Melting and boiling points

A

Normally low due to weak intermolecular forces

39
Q

Simple covalent compounds

Solubility

A

If doesn’t have hydrogen bonds, won’t be very soluble

40
Q

Simple covalent compounds

Trends in mp and bp

A

As you go down group, less polar so weaker permanent dipole-dipole interactions
More electrons which increases induced dipole-dipole interactions

Chemistry M2 (6 decks)

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