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Chemistry > Bonding > Flashcards

Bonding Flashcards

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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
Q

What is an alloy

A

When you add another element to a metal

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26
Q

How do we know particles in a solid are arranged regularly

A

It has a fixed shape

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27
Q

How do we know solids vibrate around a certain point

A

When it is heated it expands and there is no diffusion

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28
Q

What does jostling mean

A

Move around each other

29
Q

How do we know that liquids have a random particle arrangement

A

Particles can move around each other and fill a container

30
Q

How do we know that particles in a liquid are close together

A

It can’t be compressed

31
Q

How do we know that particles in a liquid jostling

A

Slow diffusion and convection of heat

32
Q

How do we Know that particles are arranged randomly in a gas

A

Fill a containerc

33
Q

How do we know that particles in a gas are far away from each other

A

Easily compressed

34
Q

How do we know particles in a gas move rapidly

A

Can exert pressure on a surface
Convection
Quick diffusion

35
Q

Enthalpy change of melting

A

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
Q

Electronegativity

A

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
Q

What three elements have the highest electronegativity

A

FON
Fluorine. Oxygen. Nitrogen

38
Q

What affects electronegativity

A

Affective nuclear charge. Distance from the nucleus. Shielding

39
Q

How does electronegativity charge across a period

A

Increases

40
Q

How does electronegativity change down a group

A

Decreases down a group

41
Q

Why does electronegativity increase across a period

A

Because of a higher affective nuclear charge despite more shielding

42
Q

Why does electronegativity decrease down a group

A

Due to increased shielding although there’s a higher affective nuclear charge

43
Q

Why does electronegativity decrease down a group

A

Due to increased shielding although there’s a higher affective nuclear charge

44
Q

What type of bonding does polarity refer too

A

Covalent

45
Q

What is polarity

A

The unequal sharing of electrons between atoms in a bond

46
Q

How are there non polar covalent bonds

A

If the atoms are the same. Eg chlorine and chlorine

47
Q

What happens in polar bonding

A

Electron cloud is distorted ( pulled) towards the more electronegative element

48
Q

What does intra mean

A

Within

49
Q

What does inter mean

A

Between

50
Q

What type of bond contains intermolecular forces

A

Covalent only

51
Q

What are the three types of intermolecular forces

A

Van der walls

Dipole-dipole

Hydrogen bonds

52
Q

What is the weakest type of intermolecular force

A

Van der waals

53
Q

What is the strongest type of intermolecular force

A

Hydrogen bonding

54
Q

Intermolecular forces strength in order weakest to strongest

A

Van der waals
Dipole dipole
Hydrogen bonding

55
Q

What molecules or atoms does van der waals happen in

A

All atoms and molecules (Nobel gasses)

56
Q

Where does dipole dipole happen

A

Between certain types of molecules

57
Q

Where does hydrogen bonding happen

A

Between certain types of molecules

58
Q

Dipole moment

A

Sums up the effect of polarity of all the bonds in a molecule

59
Q

Are non polar or polar things dipole and why

A

Polar things are dipole because there is permanent dipoles
Non polar don’t have dipole forces

60
Q

What type of faint force are dipoles

A

Electrostatic forces of attraction

61
Q

Non polar things are often shaped and have

A

Symmetrical and have the same groups

62
Q

Dipole dipole definition

A

Forces that act between two molecules that have permanent dipoles
They orientate themselves to attract each other

63
Q

Van der waals summary

A

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
Q

How does van der waals happen

A

Two neutral neighbouring atoms
One has a dipole due to charge distribution
Induces a dipole in the neighbouring atom

65
Q

What elements are hydrogen bonds between

A

The FON and hydrogen
Fluorine oxygen or nitrogen

66
Q

Why do only the fon make hydrogen bonds

A

Only ones that are electronegative enough

67
Q

How are hydrogen bonds shown

A
      • dashes
68
Q

What happens down the group of the Nobel gasses and why

A

BP increases due to the increased number of van der waals because there are more electrons

69
Q

What type of crystal is graphane

A

Giant covalent

Chemistry (10 decks)

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