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chemistry > Electron Bonding, Structure, Polarity > Flashcards

Electron Bonding, Structure, Polarity Flashcards

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1
Q

How to write an ionic equation?

A
  • Write out equation with charges
  • Cross out repeating aspects
  • You have your equation
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2
Q

Oxidation Numbers

A 
Elemental form-0
Group 1- +1
Group 2- +2
Group 7- -1
Hydrogen- +1
Oxygen- -2
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3
Q

Oxidation numbers (exceptions)

A

Metal hydrides, hydrogen- -1
Peroxides, oxygen- -1
Oxygen bonded to fluorine, oxygen- +2

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4
Q

How to calculate the oxidation number

A

Sum of oxidation numbers=Total charge

1) Take oxidation number you know
2) Write into equation
3) Rearrange equation
4) This will give you oxidation number

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5
Q

Calculation oxidation number example

A 
NO3
(3xO) + N = -1
(3x-2)+N= -1
-6 +N= -1
Therefore N=+5
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6
Q

What is OILRIG?

A

Oxidation is loss

Reduction is gain

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7
Q

What is the s sub shell?

A

Can hold a max of 2 electrons as each s sub shell has only 1 orbital
S orbitals are spherical

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8
Q

What is the p sub shell?

A

Can hold a max of 6 electrons as each sub shell has 3 orbitals
P orbitals are dumbbell shaped

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9
Q

What is the d sub shell?

A

Has 5 orbitals and can hold up to 10 electrons

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10
Q

What is the f sub shell

A

Has 7 orbitals so can hold up to 14 electrons

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11
Q

What is an orbital?

A

A 3D region of space around the nucleus that can hold a maximum of 2 electrons

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12
Q

How many electrons can shell 1 hold?

A

2 electrons

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13
Q

How many electrons can shell 2 hold?

A

8 electrons

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14
Q

How many electrons can shell 3 hold?

A

18 electrons

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15
Q

How many electrons can shell 4 hold?

A

32

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16
Q

What is the rule for how many electrons a shell can hold?

A

2n^2

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17
Q

What is the order of sub shell notation?

A

1s
2s 2p
3s 3p 3d
4s 4p 4d 4f

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18
Q

What is the rule of 4s and 3d?

A

Count 4s first but write it AFTER 3d

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19
Q

What is the electrons in box model?

A

Each box has an up and down electron represented as an arrow

Boxes should be filled singly first before doubling them up

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20
Q

What is the sub shell notation for Chromium

A

1s2 2s2 2p6 3s2 3p6 3d5 4s1

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21
Q

What is the sub shell notation for Copper?

A

1s2 2s2 2p6 3s2 3p6 3d10 4s1

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22
Q

What happens when d block elements form ions?

A

They lose 4S electrons FIRST

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23
Q

LINEAR

A

Shape: Linear
Bond Angle: 180*
Bond pairs: 2
Lone pairs: 0

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24
Q

TRIAGONAL PLANAR

A

Shape:Triagonal Planar
Bond angle: 120*
Bond pairs: 3
Lone pairs: 0

25
Q

TETRAHEDRAL

A

Shape: Tetrahedral
Bond angle: 109.5*
Bond pairs: 4
Lone pairs: 0

26
Q

TRIAGONAL BIPYRAMIDAL

A

Shape: Triagonal bipyramidal
Bond angle: 120* and 90*
Bond pairs: 5
Lone pairs: 0

27
Q

OCTAHEDRAL

A

Shape: Octahedral
Bond angle: 90*
Bond pairs: 6
Lone pairs: 0

28
Q

PYRAMIDAL

A

Shape: Pyramidal
Bond angle: 107*
Bond pairs: 3
Lone pairs: 1

29
Q

NON-LINEAR

A

Shape: Non-Linear
Bond angle: 104.5*
Bond pairs: 2
Lone pairs: 2

30
Q

SQAURE PLANAR

A

Shape: Square Planar
Bond angle: 90*
Bond pairs: 4
Lone pairs: 2

31
Q

How work out shape of molecule

A

1) Use dot and cross diagram to work out total no. of electron pairs
2) Find regular/irregular shape based of the information of bond and lone pairs.

32
Q

What is electronegativity?

A

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

33
Q

Electronegativity with different atoms

A
  • More electronegative atom will have a greater share of electrons
  • It is a polar molecule
34
Q

Electronegativity with the same atom

A
  • Electrons are shared equally

- Non-polar molecule

35
Q

Electronegativity with very different atoms

A
  • Increasing polarisation will turn the bond from covalent from ionic
  • Most electronegative atom takes electrons completely, turning the bond from covalent to ionic
36
Q

What is the electronegativity trend across the periodic table?

A

Electronegativity increases up and group and across a period

37
Q

What are the electronegativity difference values on the Pauling Scale?

A

Covalent - 0
Polar covalent - 0-1.8
Ionic - >1.8

38
Q

How does symmetry affect the polarity of a molecule?

A

Symmetry will cancel out any dipoles, causing the molecules to be non-polar

39
Q

How to work out the dipole of a molecule?

A

1) Work out shape
2) Assign dipoles
3) Work out symmetry
4) Work out overall dipole

40
Q

What is the structure of ice?

A
  • Diamond-like structure

- Volume larger than liquid

41
Q

How does water change at certain temperatures?

A
  • 4*C < ice forms a simple molecular lattice
  • at 4*C water is at its maximum density
  • when ice melts, its structure collapses
42
Q

What bonds/forces are in simple molecular lattices?

A
  • Covalent bonds between atoms

- Weak intermolecular forces

43
Q

What intermolecular forces does water have?

A

Hydrogen bonding

44
Q

Why does water have hydrogen bonding?

A

There is a lone pair on an oxygen atoms that attracts the hydrogen bond

45
Q

What is the trend for boiling point in group 18?

A

Down group 18, the boiling point increases

46
Q

What is the trend of boiling point in group 14?

A

Down group 14, the boiling point increases

47
Q

What are the intermolecular forces in order of strength? (strongest at top)

A
  • Hydrogen bonding
  • Permanent dipole-dipole interactions
  • London forces (induced dipole)
48
Q

What are permanent dipole-dipole interactions?

A
  • Weak attractive force between permanent dipole dipoles

- Forces get stronger when electronegativity difference is higher (dipoles are larger)

49
Q

How does London forces form?

A
  • There is an uneven distribution of electrons
  • Which creates an instantaneous dipole when electrons get close
  • Which causes induced dipoles in neighbouring molecules
50
Q

When do London forces get stronger?

A
  • When the atom has more electrons

- Greater inst. dipole, ind. dipole larger, electrostatic attraction greater

51
Q

What are the requirements for hydrogen bonding?

A
  • Hydrogen must be bonded to a N, F or O

- Must have a lone pair on N, F or O

52
Q

What causes ‘irregular shape molecule’ to have its shape?

A
  • Comment on bonding pairs and lone pairs
  • Comment on bonding angle
  • Comment that lone pair repels MORE than bonding pair
53
Q

What causes ‘regular shape molecule’ to have its shape?

A
  • Comment on bonding pairs and lone pairs (none)
  • Comment on bond angle
  • Comment that bonding pair repels
54
Q

Why are polar solvents miscible in water?

A
  • Negative ions attracted to partially positive hydrogen atoms and positive ions attracted to partially negative oxygen atoms
  • Ionic lattice breaks down as it dissolves
  • Water molecules surround the ions
55
Q

What is the solubility of non-polar simple molecules?

A
  • Tend to be soluble in non-polar solvents as interactions occur between the molecule and the solvent
  • Interaction weaken the intermolecular forces in the simple molecular lattice and force it to break down and the compound dissolves
56
Q

Why are non-polar simple molecules typically not soluble in polar solvents?

A
  • Very little interaction between molecules in lattice and molecules in solvent
  • Intermolecular bonding within solvent is too strong to be broken
57
Q

Why can iconic compounds conduct electricity when molten and aqueous but not when solid?

A

Because the ions are mobile and therefore can carry a charge

58
Q

Why can metal conduct electricity in any state?

A
  • When molten, ions are mobile

- When solid, delocalised electrons can carry a charge

chemistry (11 decks)

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