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Chemistry > Electron Bonding, Structure, Polarity > Flashcards

Electron Bonding, Structure, Polarity Flashcards

(58 cards)

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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

Study These Flashcards
A

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

25
TETRAHEDRAL
Shape: Tetrahedral Bond angle: 109.5* Bond pairs: 4 Lone pairs: 0
26
TRIAGONAL BIPYRAMIDAL
Shape: Triagonal bipyramidal Bond angle: 120* and 90* Bond pairs: 5 Lone pairs: 0
27
OCTAHEDRAL
Shape: Octahedral Bond angle: 90* Bond pairs: 6 Lone pairs: 0
28
PYRAMIDAL
Shape: Pyramidal Bond angle: 107* Bond pairs: 3 Lone pairs: 1
29
NON-LINEAR
Shape: Non-Linear Bond angle: 104.5* Bond pairs: 2 Lone pairs: 2
30
SQAURE PLANAR
Shape: Square Planar Bond angle: 90* Bond pairs: 4 Lone pairs: 2
31
How work out shape of molecule
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
What is electronegativity?
The ability of an atom to attract the bonding electrons in a covalent bond
33
Electronegativity with different atoms
- More electronegative atom will have a greater share of electrons - It is a polar molecule
34
Electronegativity with the same atom
- Electrons are shared equally | - Non-polar molecule
35
Electronegativity with very different atoms
- Increasing polarisation will turn the bond from covalent from ionic - Most electronegative atom takes electrons completely, turning the bond from covalent to ionic
36
What is the electronegativity trend across the periodic table?
Electronegativity increases up and group and across a period
37
What are the electronegativity difference values on the Pauling Scale?
Covalent - 0 Polar covalent - 0-1.8 Ionic - >1.8
38
How does symmetry affect the polarity of a molecule?
Symmetry will cancel out any dipoles, causing the molecules to be non-polar
39
How to work out the dipole of a molecule?
1) Work out shape 2) Assign dipoles 3) Work out symmetry 4) Work out overall dipole
40
What is the structure of ice?
- Diamond-like structure | - Volume larger than liquid
41
How does water change at certain temperatures?
- 4*C < ice forms a simple molecular lattice - at 4*C water is at its maximum density - when ice melts, its structure collapses
42
What bonds/forces are in simple molecular lattices?
- Covalent bonds between atoms | - Weak intermolecular forces
43
What intermolecular forces does water have?
Hydrogen bonding
44
Why does water have hydrogen bonding?
There is a lone pair on an oxygen atoms that attracts the hydrogen bond
45
What is the trend for boiling point in group 18?
Down group 18, the boiling point increases
46
What is the trend of boiling point in group 14?
Down group 14, the boiling point increases
47
What are the intermolecular forces in order of strength? (strongest at top)
- Hydrogen bonding - Permanent dipole-dipole interactions - London forces (induced dipole)
48
What are permanent dipole-dipole interactions?
- Weak attractive force between permanent dipole dipoles | - Forces get stronger when electronegativity difference is higher (dipoles are larger)
49
How does London forces form?
- There is an uneven distribution of electrons - Which creates an instantaneous dipole when electrons get close - Which causes induced dipoles in neighbouring molecules
50
When do London forces get stronger?
- When the atom has more electrons | - Greater inst. dipole, ind. dipole larger, electrostatic attraction greater
51
What are the requirements for hydrogen bonding?
- Hydrogen must be bonded to a N, F or O | - Must have a lone pair on N, F or O
52
What causes 'irregular shape molecule' to have its shape?
- Comment on bonding pairs and lone pairs - Comment on bonding angle - Comment that lone pair repels MORE than bonding pair
53
What causes 'regular shape molecule' to have its shape?
- Comment on bonding pairs and lone pairs (none) - Comment on bond angle - Comment that bonding pair repels
54
Why are polar solvents miscible in water?
- 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
What is the solubility of non-polar simple molecules?
- 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
Why are non-polar simple molecules typically not soluble in polar solvents?
- Very little interaction between molecules in lattice and molecules in solvent - Intermolecular bonding within solvent is too strong to be broken
57
Why can iconic compounds conduct electricity when molten and aqueous but not when solid?
Because the ions are mobile and therefore can carry a charge
58
Why can metal conduct electricity in any state?
- When molten, ions are mobile | - When solid, delocalised electrons can carry a charge

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