Physical Chemistry > Bonding > Flashcards

Bonding Flashcards

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1
Q

What is ionic bonding?

A

a strong, electrostatic force of attraction between oppositely charged ions

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2
Q

structure of ionic compounds

A

a giant ionic lattice consisting of a regular arrangement of oppositely charged ions

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3
Q

properties of ionic compounds

A

strong
high melting and boiling points
conducts electricity when molten or aqueous, but not solid
brittle

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4
Q

Why can ionic compounds conduct electricity when molten/in solution, but not when solid?

A

Ions are able to move around and carry the charge when molten or in solution, but not when solid

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5
Q

Why are ionic compounds brittle?

A

When the compound is hit, the layer arrangement is no longer regular and alternate, in terms of ions, so the same charged ions are next to each other, causing repulsion

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6
Q

Why do ionic compounds have a high melting and boiling point?

A

Strong electrostatic forces of attraction between oppositely charged ions require little energy to overcome

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7
Q

Factors affecting melting point in metallic elements

A

size of ion (smaller ions = higher MP)
charge of ion (bigger charge = higher MP)

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8
Q

If 2 ions have the same number of electrons, why is the one with the most protons smaller than the other ion?

A

The one with more protons can attract the electrons more closely, so its atomic radius is smaller

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9
Q

Explain how the compound MgO is formed, and state its structure and bonding

A

giant ionic lattice
ionic bonding
Mg needs to lose 2 electrons and O needs to gain 2 electrons so Mg donates 2 electrons to O
This forms Mg2- and O2- ions

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10
Q

metallic bonding

A

electrostatic force of attraction between the positive ions and sea of delocalised electrons

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11
Q

structure of metallic compounds

A

giant metallic structure consisting of a regular arrangement of positive ions in a sea of delocalised electrons

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12
Q

properties of metallic compounds

A

malleable
ductile
conducts electricity and heat
high melting and boiling point
insoluble

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13
Q

why are metallic compounds malleable and ductile?

A

Positive ions are all the same size so layers are able to slide over each other

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14
Q

why can metallic compounds conduct electricity?

A

delocalised electrons can move through the structure and carry the charge

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15
Q

why can metallic compounds conduct heat?

A

delocalised electrons possess kinetic energy that can be transferred to positive ions, causing them to vibrate

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16
Q

why do metallic compounds have a high melting and boiling point?

A

strong, electrostatic force of attraction between positive ions and sea of delocalised electrons that require lots of energy to overcome

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17
Q

Factors affecting the strength of a metallic bond

A

size of ion (small)
charge of ion (big)

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18
Q

How does the size of the ion affect the strength of a metallic bond?

A

The smaller the ion, the closer electrons are to the positive nucleus, so the stronger the bond.

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19
Q

How does the charge of an ion affect the strength of a metallic bond?

A

The higher the charge, the more delocalised electrons there are, so there is a stronger electrostatic FOA

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20
Q

covalent bonding

A

electrostatic force of attraction between positive nucleus and shared electrons that occurs between non - metals

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21
Q

types of covalent bonding

A

single
double
triple
co-ordinate or dative covalent

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22
Q

examples of giant covalent structures

A

diamond
graphite
silica
nanotubes/graphene

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23
Q

properties of diamond

A

high melting point
strong
doesn’t conduct electricity
uses: jewellery, drill bits

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24
Q

why does diamond have a high melting point?

A

strong covalent bonds require lots of energy to overcome

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25
why can't diamond conduct electricity?
no delocalised electrons or charged particles that can move through the structure and carry the charge
26
why is diamond strong?
tetrahedral structure where each carbon atom forms 4 bonds with other carbon atoms
27
properties of graphite
high melting point soft each carbon atom forms 3 bonds conducts electricity uses: pencils and electrodes
28
why does graphite have a high melting point?
strong, covalent bonds require lots of energy to overcome
29
why is graphite soft?
hexagonal layers have intermolecular forces (van Der Waals) that allow layers to slide easily over each other
30
why can graphite conduct electricity?
each carbon atom has 1 delocalised electron so there are lots of delocalised electrons that can move through the structure and carry the charge
31
properties of silica
high melting point very strong cannot conduct electricity
32
why is silica strong?
tetrahedral structure where each silicon atom bonds with 4 oxygens and each oxygen atom bonds with 2 silicons
33
why does silica have a high melting point?
strong covalent bonds require lots of energy to overcome has formula S8
34
why doesn't silica conduct electricity?
no charged particles that can move through the structure and carry the charge
35
examples of simple molecular structures
atmospheric gases buckminsterfullerene (uses: drug delivery in the body, electronics)
36
why do simple molecular structures have a low melting point?
weak intermolecular forces between molecules require little energy to overcome
37
why can't simple molecular structures conduct electricity?
no charged particles that can move through the structure and carry the charge
38
co-ordinate bond
1 atom/ion has a lone pair of electrons, which it can donate to another atom/ion
39
properties of simple molecular structures
low melting point cannot conduct electricity
40
Electron repulsion theory
electron pairs will position themselves as far away from each other to stop repulsion each pair of electrons repel other pairs lone pairs repel more than bonding pairs
41
AX2
linear bond angle: 180
42
AX3
trigonal planar bond angle: 120
43
AX4
tetrahedral bond angle: 109.5
44
AX5
trigonal bipyramidal bond angle: 120 and 90
45
AX6
octahedral bond angle: 90
46
How much do lone pairs reduce the bond angle by?
2.5 degrees per lone pair as lone pairs repel more than bonding pairs
47
Shape of molecule: 2 lone and 2 bonding
bent
48
Shape of molecule: 1 lone and 2 bonding
bent
49
Shape of molecule: 2 lone and 3 bonding
T - shape
50
Shape of molecule: 1 lone and 5 bonding
square pyramidal
51
Shape of molecule: 2 lone and 4 bonding
square planar
52
Shape of molecule: 1 lone and 3 bonding
trigonal pyramidal
53
Shape of molecule: 1 lone and 4 bonding
seesaw
54
electronegativity
the power of an atom to attract a pair of electrons towards itself in a covalent bond the larger an element's EN value, the greater its ability to attract the pair of electrons towards itself
55
factors affecting electronegativity
shielding nuclear charge (number of protons)
56
How does shielding affect electronegativity?
More shielding means a lower electronegativity as the attraction between the nucleus and outer shell electron gets weaker
57
How does nuclear charge affect electronegativity?
more protons = higher electronegativity because electrons are pulled more strongly
58
polar bond
forms between 2 atoms with a difference in electronegativity - if one side is positive and one side is negative, then it is a polar molecule
59
non - polar molecules
any diatomic molecules or symmetrical molecules where there is an even distribution of bonding pairs (the same charge is pointing in opposite directions so dipoles cancel out)
60
dipole moment
uneven distribution of charge
61
Van Der Waals
weakest intermolecular force occurs between all atoms and molecules when electrons are orbiting and come close to electrons in another atom, they'll repel and a temporary dipole is induced
62
How Van Der Waals forces arise
electron movement in one atom/molecule creates a temporary dipole this induces a temporary dipole in the neighbouring atom/molecule the delta +ive attracts the delta -ive in adjacent atoms/molecules
63
Factors affecting the strength of Van Der Waals forces
size of molecule (bigger molecule = more VdW forces as there are more electrons)
64
How could a non - polar molecule have a higher boiling point than a polar molecule?
even though a polar molecule can have dipole - dipole forces and VdW forces, the non - polar molecule may have lots of electrons, so the strength of the VdW forces is a lots stronger than the dipole - dipole and VdW forces from the polar molecule combined.
65
Dipole - dipole forces
occurs between molecules with an overall permanent dipole (drawn with a dotted line with labelled electronegativity and arrow showing showing dipole)
66
How dipole - dipole forces arise
difference in electronegativity leads to bond polarity is an overall permanent dipole as dipoles don't cancel out attraction forms between delta +ive from one molecule and delta -ive from another
67
hydrogen bonding
occurs between N, O, F bonded to H bonding occurs between atoms with a high difference in electronegativity Examples: formic acid, ammonia, ethanol
68
How hydrogen bonding arises
large electronegativity difference between H and --- forms delta +ive on hydrogen and delta -ive on --- lone pair on --- attracts H on adjacent molecule
69
types of molecules that dissolve in water
any molecule that can H bond ionic compounds
70
Why does ice float?
Ice is less dense than water Hydrogen bonds form between water molecules forming a lattice structure - bonds are further apart in ice compared to water so it can float
71
Why does water have a higher boiling point than HF?
water can form 4 hydrogen bonds and HF can form 2 hydrogen bonds (it only has 1 hydrogen, so the number of Hs that can bond to lone pairs is limited)
72
Arrangement of particles in a solid: Evidence?
regular arrangement crystals have straight edges
73
Arrangement of particles in a liquid: Evidence?
random arrangement will change shape to fill its container
74
Arrangement of particles in a gas: Evidence?
random arrangement will fill whole container
75
Spacing of particles in a solid: Evidence?
close cannot be compressed easily
76
Spacing of particles in a liquid: Evidence?
close cannot be compressed easily
77
Spacing of particles in a gas: Evidence?
far apart can be easily compressed
78
Movement of particles in a solid: Evidence?
vibrate slow diffusion - expands when heated
79
Movement of particles in a liquid: Evidence?
rapid 'jostling' slow diffusion - can evaporate
80
Movement of particles in a gas: Evidence?
rapid movement rapid diffusion - can exert pressure
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