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Chemistry > 3.1.3 - Bonding > Flashcards

3.1.3 - Bonding Flashcards

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1
Q

Definition of ionic bonding

A

The electrostatic attraction between positive and negative ions. They are non- directional

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2
Q

In ionic bonding what loses electrons and what gains electrons

A

Metals lose electrons

Non- metals gain electrons

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3
Q

How can your represent an ionic bond ?

What can’t you forget

A

Using a dot and cross diagram

Don’t forget the charges

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4
Q

Definition of covalent bonding

A

The electrostatic attraction between a shared pair of electrons and the nuclei of two atoms. They are directional.

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5
Q

How many covalent bonds does group 4 make ?

A

4

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6
Q

How many covalent bonds does group 3 make ?

A

3 or more

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7
Q

How many covalent bonds do group 2 make?

A

2 or more

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8
Q

How many covalent bonds do group 1 make ??

A

1 or more he p

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9
Q

What is a dative covalent bond ??

A

Where both electrons come from the same atom

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10
Q

How are dative covalent bond presented ?

A

The bond is shown by an arrow rather than a straight line

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11
Q

Definition of metallic bonding

A

The electrostatic attraction between positive ions and delocalised electrons. They are non- directional.

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12
Q

What is the trend across a period of melting point in metals ?

A

Increase
Charge increases
Electrons increase
Therefore strength of metallic bond is increased

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13
Q

What is the trend of melting point down a group of metals

A 
Decreases 
Size of ion decreases 
Charge stays the same 
Electrons stay the same 
Mettalic bond strength decreases
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14
Q 
Ionic 
Mp and Bp 
Conductivity(solid) 
Conductivity (molten) why?
Conductivity (aq) why?
Strength why ? 
Solubility why?
A 
High 
No 
Yes -ions free to move 
Yes-ions free to move 
Brittle- dislocation lead to layers moving and then repelling each other 
High - water is polar separates the ions
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15
Q

Metallic

Mp and bp
Conductivity(solid) why?
Conductivity (liquid) why?
Conductivity (aq ) why? 
Strength   Why ? 
Solubility why ?
A 
High 
Yes 
Yes 
Insoluble 
Strong can slide over each other 
Insoluble
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16
Q

Giant covalent

Mp and bp 
Conductivity (solid) 
Conductivity (liquid) 
Conductivity (aq) 
Strength 
Solubility
A 
Very highly 
No 
No 
Insoluble 
Strong for some 
Insoluble bonds must be broken
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17
Q

Diamond

Structure 
Bp and mp 
Conductor 
Strength 
Solubility
A

Giant covalent

Very high bp and mp many strong covalent bonds need breaking

Poor conductor no mobile electrons or ions

Very strong - rigid tetrahedrald arrangement

Insoluble- many covalent bonds must be broken

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18
Q

Graphite

Structure 
Bp and mp 
Conductivity 
Strength 
Solubility
A

Very high melting point and boiling point many strong covalent bonds need breaking

Conducts some electrons are free to move

Brittle weak can der waals between layers which can slide over each other

Insoluble- many covalent bonds must be broken

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19
Q

Change of state

What is happening at boiling point

A

Heat energy is used to break all the bonds a lot. Energy required

20
Q

Change of state

What happens at melting point

A

Heat energy breaks some bonds so not as much energy is required

21
Q

2 bonding pairs

Name
Angle
How it looks

A

Linear
180

H-Be- He

22
Q

3 bonding pairs

Name
Angle
What it looks like

A

Trigonal planar
120

F
//// B - F
<
F

23
Q

4 bonding pairs

Name
Angle
What it looks like

A

Tetrahedral -

109.5 
             H
              |
    H  <  C > H 
             =
             =
            H
24
Q

5 bonding pairs

Name
Angle
How it looks

A

Trigonal bipyramidal

120 and 90

         F 
F.      |
    //.  P - F 
 F
25
Q

6 bonding pairs

Name
Angle
What it looks like

A 
Octahedral
90 
         F
         |
   F //S \\ F 
   F<       >F 
          |
         F
26
Q

4 pairs
3 bonding
1 lone pair

Name
Angle
What it looks like

A

Trigonal pyramidal
107

   ..
   N 
 /  |   \    H.  H.  H
27
Q

4 bonds
2 bonding pairs
2 lone pairs

Name
Angle
Looks like ?

A

Bent v-shaped
104.5

.. ..
O
/. \
H. H

28
Q

3 bonds

2 Bonding pairs
1 lone pair

Name
Angle
looks like

A

Bent v shaped
118

 ..
S    /    \    O     O
29
Q

5 bonds

3 bonding pairs
2 lone pairs

Name
Angle
Looks like

A

T-shape
89

    ..  F  -Cl  - F 
    |
   F
30
Q

5 bonds

4 bonding pairs
1 lone pair

Name
Angle
Looks like

A

Distorted tetrahedron
89, 103

 .. F- S - F 
<  //   F       F
31
Q

5 bonds
2 bonding pairs
3 lone pairs

Name
Angle
What it looks like

A 
Linear 
180 
       ..     .. 
F -     Xe    - F 
          ..
32
Q

6 bonds

4 bonding pairs
2 lone pairs

Name
Angle
What it looks like

A 
Square planar 
90 
   F         F 
     //  .. \\ t
         X
   F   F
33
Q

6 pairs
5 bonding pairs
1 lone pair

Name
Angle
Looks like

A 
Square pyramidal 
<90 
       F         
        | 
F // Br \\F

F F

34
Q

The order of giving most repulsion in the bonds

A

Bond pair bond pair

Then

Bond pair lone pair

Then

Lone pair lone pair

35
Q

Definition of electronegativity

A

Power of an atom to attract the electrons( electron density) in a covalent bond to itself

36
Q

What does a higher electronegativity value mean?

A

More attraction

37
Q

What is the highest value electronegativity and the lowest?

A
  1. 0 - Fluorine

0. 7 - caesium

38
Q

Electronegativity trend across a period

A

Increase
Nuclear charge increases
Atomic radius decreases
Therefore more attraction between nucleus and atoms

39
Q

What is the electronegativity trend down a group

A

Decrease

Atomic radius decreases
More shielding
Therefore less attraction

40
Q

What does a delta - show and why ?

A

Excess of electron density more to that side

41
Q

What does a delta + show and why ?

A

Show deficiency of electron density because electrons are further away

42
Q

List in order of strength the intermolecular forces

A

Hydrogen bond
Dipole dipole
Van der waals

43
Q

Explain what van der waals are

A

Intermolecular force

Occur between all molecules but are only force of attraction in non polar molecules. Weakest

44
Q

Explain dipole- dipole forces

A

Intermolecular forces

Occur between polar molecules and add to van der waals

45
Q

Explain hydrogen bonds

A

Occur between molecular which contain H bonded to N,O, F have a higher electronegativity. Strongest intermolecular bond

46
Q

What is the relative bp and solubility of non polar molecules

A

Low bp only weak van der waals

Insoluble no attraction to polar water molecules

47
Q

What is the relative bp and solubility of polar molecules

A

Higher bp strong forces ; dipole-dipole and hydrogen bonds to overcome.

Soluble - attraction to polar water molecules

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