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Bonding Flashcards

1
Q

what is ionic bonding

A

the result of electrostatic attraction between oppositely charged ions

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2
Q

how are electrons transferred in ionic bonding

A

electrons transferred from the metal to the non metal

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3
Q

what do ionic compounds exist as

A

lattices that are strong because of the electrostatic attraction that acts in all directions and extends throughout the lattice

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4
Q

Electrical conductivity in ionic bonding

A

can’t conduct when solid since ions are not free to move and carry charge
can when molten or in solution

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5
Q

Melting points in ionic bonding

A

High because the electrostatic forces of attraction which act in all directions require a lot of energy to overcome

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6
Q

solubility in ionic bonding

A

tend to be soluble in polar solutions since the ions are pulled by the solvent causing them to dissociate away from the lattice and dissolve

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7
Q

Why are ionic compounds brittle

A

They contain a lattice of alternating positive and negative ions in fixed positions so when force acts on it from one side it shatters

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8
Q

Covalent bonding

A

Sharing a pair of electrons between two non metals to have a more stable electron configuration

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9
Q

How are covalent bonds held together

A

The forces of repulsion and attraction are equal so it keeps the particles at the same distance

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10
Q

Why can’t simples covalent structures conduct

A

Because there are no delocalised electrons or ions that are free to carry charge can’t conduct in solution either

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11
Q

Are covalent mp and no high or low

A

Low

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12
Q

Why are covalent mp and bp low

A

Weak intermolecular forces between molecules which require little energy to overcome

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13
Q

How can acids conduct electricity in water

A

Acids are covalent but they become ions in water

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14
Q

What is it called when both electrons are shared from one atom covalently

A

Coordinate bonding

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15
Q

What is coordinate bonding

A

Where both shared electrons are from one atom

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16
Q

How is coordinate bonding shown

A

As an arrow

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17
Q

How does coordinate bonding happen

A

The atom accepts it doesn’t have a full outer shell (electron deficient)
The donating atom donates a non bonding pair of electrons ( a lone pair)

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18
Q

What is metallic bonding

A

Bonding WITHIN a metal

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19
Q

What are metallic bp and mp like

A

Very high since there are strong electrostatic forces of attraction which acts in all direction throughout the lattice which requires alot energy to overcome

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20
Q

Why are metals good conductors

A

They have a sea of delocalised electrons free to carry charge and thermal energy

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21
Q

What does ductile mean

A

Can stretch it into a wire

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22
Q

What does maleable mean

A

Can be bent

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23
Q

Are metals maleable and ductile

A

Because layers can slide over each other and electrons move with them

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24
Q

How can you increase the strength of a metal

A

Make it an alloy so layers can’t slide

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25
What is an alloy
When you add another element to a metal
26
How do we know particles in a solid are arranged regularly
It has a fixed shape
27
How do we know solids vibrate around a certain point
When it is heated it expands and there is no diffusion
28
What does jostling mean
Move around each other
29
How do we know that liquids have a random particle arrangement
Particles can move around each other and fill a container
30
How do we know that particles in a liquid are close together
It can’t be compressed
31
How do we know that particles in a liquid jostling
Slow diffusion and convection of heat
32
How do we Know that particles are arranged randomly in a gas
Fill a containerc
33
How do we know that particles in a gas are far away from each other
Easily compressed
34
How do we know particles in a gas move rapidly
Can exert pressure on a surface Convection Quick diffusion
35
Enthalpy change of melting
Solid to liquid energy supplied to weaken forces acting between particles Temp doesn’t change when heat energy is supplied because it’s absorbed as the forces are weakened
36
Electronegativity
The power of an atom to attract the shared pair of electrons in a covalent bond towards it self On a scale of 0-4 ( highest is 4)
37
What three elements have the highest electronegativity
FON Fluorine. Oxygen. Nitrogen
38
What affects electronegativity
Affective nuclear charge. Distance from the nucleus. Shielding
39
How does electronegativity charge across a period
Increases
40
How does electronegativity change down a group
Decreases down a group
41
Why does electronegativity increase across a period
Because of a higher affective nuclear charge despite more shielding
42
Why does electronegativity decrease down a group
Due to increased shielding although there’s a higher affective nuclear charge
43
Why does electronegativity decrease down a group
Due to increased shielding although there’s a higher affective nuclear charge
44
What type of bonding does polarity refer too
Covalent
45
What is polarity
The unequal sharing of electrons between atoms in a bond
46
How are there non polar covalent bonds
If the atoms are the same. Eg chlorine and chlorine
47
What happens in polar bonding
Electron cloud is distorted ( pulled) towards the more electronegative element
48
What does intra mean
Within
49
What does inter mean
Between
50
What type of bond contains intermolecular forces
Covalent only
51
What are the three types of intermolecular forces
Van der walls Dipole-dipole Hydrogen bonds
52
What is the weakest type of intermolecular force
Van der waals
53
What is the strongest type of intermolecular force
Hydrogen bonding
54
Intermolecular forces strength in order weakest to strongest
Van der waals Dipole dipole Hydrogen bonding
55
What molecules or atoms does van der waals happen in
All atoms and molecules (Nobel gasses)
56
Where does dipole dipole happen
Between certain types of molecules
57
Where does hydrogen bonding happen
Between certain types of molecules
58
Dipole moment
Sums up the effect of polarity of all the bonds in a molecule
59
Are non polar or polar things dipole and why
Polar things are dipole because there is permanent dipoles Non polar don’t have dipole forces
60
What type of faint force are dipoles
Electrostatic forces of attraction
61
Non polar things are often shaped and have
Symmetrical and have the same groups
62
Dipole dipole definition
Forces that act between two molecules that have permanent dipoles They orientate themselves to attract each other
63
Van der waals summary
Positive and negative charges in everything that are overall neutral Always very weak electrostatic forces of attraction in everything Electrons constantly move and so do their distribution of charge
64
How does van der waals happen
Two neutral neighbouring atoms One has a dipole due to charge distribution Induces a dipole in the neighbouring atom
65
What elements are hydrogen bonds between
The FON and hydrogen Fluorine oxygen or nitrogen
66
Why do only the fon make hydrogen bonds
Only ones that are electronegative enough
67
How are hydrogen bonds shown
- - - dashes
68
What happens down the group of the Nobel gasses and why
BP increases due to the increased number of van der waals because there are more electrons
69
What type of crystal is graphane
Giant covalent
70
What does a higher bond enthalpy mean
More energy is needed to break the bond It is a stronger bond
71
Displayed formula
Shows all the atoms and the bonds with a line and their element
72
Structural
Order of atoms without showing bonds
73
Skeletal
Lines that show single carbon to carbon bonds
74
Homologous series
Series of organic compounds with the same functional group but different carbon chain length
75
Physical properties of a homologous series
Different melting and boiling points Different viscosity Ones that contain O or N would decrease in solubility since it becomes non polar
76
Chemical properties of a homologous series
Similar chemical reactions
77
Meth
1
78
Eth
2
79
Prop
3
80
Pent
5
81
Hex
6
82
Hept
7
83
Oct
8
84
Non
9
85
Dec
10
86
Cyclo
It’s joined up in a ring (Like pentose in DNA)
87
But
4
88
How are bond broken
When something has a higher energy than it

Chemistry (15 decks)

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