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A Level Chemistry - Physical Chemistry > 3.1.3 Bonding > Flashcards

3.1.3 Bonding Flashcards

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1
Q

What is electronegativity

A

The ability of an atom to attract the pair of electrons in a covalent bond.

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2
Q

What 3 factors do electronegativity depend on

A

size of positive charge in the nucleus
Atomic radius - the closer the bonding pair to the nucleus
shielding - greater shielding, lower electronegativity

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3
Q

What forces of attraction are in ionic bonds

A

Electrostatic forces of attraction

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4
Q

Ionic bond is made form a

A

Metal and non-metal

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5
Q

Why do atoms react

A

To achieve electron configuration of a Nobel gas
Full outer shell of electrons

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6
Q

How are electrons transferred between non-metal and metal in ionic bond + charges

A

Metal loses electrons to form a positive ion
Non-metals gains electrons to form a negative ion

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7
Q

How are the ions arranged in an ionic bond

A

A giant lattice structure

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8
Q

Shapes of molecules
2 bond
3 bond
4 bond
5 bond
6 bond

A

Linear
Triangular planar
Tetrahedral
Trigonal biprymadial
Octahedral

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9
Q

Formula of ammonium

A

NH4 +

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10
Q

Formula of Carbonate ion

A

CO3 -2

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11
Q

Formula hydroxide ion

A

OH-

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12
Q

Formula nitrate ion

A

NO3 -

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13
Q

Formula sulphate ion

A

SO4 -2

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14
Q

Ionic compounds - electrical conductivity

A

Only when molten or dissolved not solid
The ions are held in place by electrostatic forces of attraction and are not free to move and carry charge

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15
Q

Ionic compound - Melting point

A

High melting point
The giant ionic lattices are held together by strong electrostatic forces of attraction which act in all directions

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16
Q

Ionic compounds - solubility

A

Tend to be soluable in water.
Water molecules are polar overcomes electron static forces of attraction
Pulls ions away from lattice and dissolves them

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17
Q

Angles in linear molecule

A

180

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18
Q

Angle in Trigonal planar

A

120

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19
Q

Angles in Tetrahedral

A

109.5

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20
Q

Angles in Trigonal biprymidial

A

90
120

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21
Q

Angles in octahedral

A

90

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22
Q

In a covalent bond electrons are….

A

Shared

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23
Q

In simple covalent molecules what determines the property of the molecule

A

Intermolecular forces

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24
Q

What is expansion of the octet rule

A

Usually period 3
Can have more than 8 electrons on outer shell

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25
Q

why do simple covalent compounds have low melting and boiling points

A

Low
strong covalent bonds between atoms in a molecule
weak intermolecular forces of attraction between molecules
which determine their properties

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26
Q

giant covalent is also known as

A

macromolecular

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27
Q

graphite structure

A

sheets of flat hexagons
3 bonds to each carbon
delocalised electrons between layer

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28
Q

properties of graphite

A

lubricant- weak bonds between layers mean they can slide over each other
conductive - delocalised electrons are free to move and carry a charge.
low density- layers are far apart can be used in sports equipment

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29
Q

structure diamond

A

carbon bonded to 4 other carbons
crystal lattice structure

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30
Q

properties diamond

A

cant conduct electricity- no free electrons to move and carry a charge
high melting point- strong covalent bonds, lots of energy to overcome
good thermal conductor - vibrations easily travel through the stiff lattice

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31
Q

give an example of each type of molecule
Ionic
Metallic
Simple molecular
Macromolecular x2

A

ionic - sodium chloride
metallic - magnesium
simple molecular-iodine
macromolecular - diamond, graphite

32
Q

Positive ions are sometimes called

A

cations.

33
Q

Negative ions are sometimes called

A

anion

34
Q

what is a dative covalent bond?

A

where one atom provides both electrons in shared pair

35
Q

how is a dative covalent bond shown on a diagram
(From which atom to which)

A

the arrow points away from the atom that has provided the electrons

36
Q

what 2 conditions must there be for a dative covalent bond to occur

A

1 atom has a lone pair of electrons
the other doesn’t have any electrons to share

37
Q

a dative covalent bond is same or different to a ‘normal’ covalent bond

A

same

38
Q

what is metallic bonding + bonding?

A

a lattice of positively charged ions surrounded by a ‘sea’ of delocalised electrons. This produces a very strong electrostatic force of attraction between these oppositely charged particles.

39
Q

which have greater repulsion loan pairs or bonding pairs

A

loan pairs

40
Q

how much do loan pairs reduce a bonding angle

A

2.5 degrees

41
Q

does a loan pair becoming a dative covalent bond have any effect on the angle degree

A

no the angles would act the exact same as if they were all covalent bonds

42
Q

electron negativity increases as you move ( in general)

A

to the top-right of the periodic table (excluding nobel gases)

43
Q

opposite charges on a polar molecule can only cancel if

A

they are opposite e.g. linear molecule
or equal charges act in all directions

44
Q

3 types of intermolecular forces

A

Van Der Waals forces
permanent dipole-dipole interations
hydrogen bonds

45
Q

Van Der Waals strength

A

weak and easily broken

46
Q

How do van der waals occur

A

Random movement of electrons in one molecule creates a dipole
Induces a dipole in a neighbouring molecule
These temporary dipoles attract

47
Q

the strength of van der Waals depends on the

A

number of electrons

48
Q

which molecules can experience permanent dipole-dipole forces

A

only molecules with a permanent dipole e.g. water

49
Q

the strength of a permanent dipole-dipole interaction decreases as

A

the electronegativity decreases

50
Q

which is the strongest intermolecular force

A

hydrogen bonds

51
Q

what are the two conditions for hydrogen bonding

A

hydrogen atom bonded to a strongly electronegative element
the electronegative atom must have at least 1 pair of electrons

52
Q

which 3 elements for hydrogen bonds

A

oxygen, fluorine, nitrogen

53
Q

why is ice less dense than water

A

molecules arranged in an ordered structure
stabilised by a network of hydrogen bonds
molecules are further apart than in liquid
so ice is less dense

54
Q

suggest why the electronegativity of the elements increases from lithium to fluorine

A

increased number of protons
same shielding

55
Q

2 bonding pairs name

A

Linear

56
Q

2 bonding 1 lone

A

Bent / v-shaped

57
Q

3 bonding pairs

A

Trigonal planar

58
Q

4 bonding pairs

A

Tetrahedral

59
Q

3 bond 1 loan

A

Trigonal pyramidal

60
Q

5 bond

A

Trigonal biprymidal

61
Q

4 bond 1 loan

A

See saw

62
Q

3 bond 2 loan

A

T-shape

63
Q

6 bond

A

Octahedral

64
Q

5 bond 1 loan

A

Square pryramid

65
Q

4 bond 2 loan

A

Square planar

66
Q

Explain how a permanent dipole-dipole forces arise between hydrogen and chlorine molecules

A

Large difference in electronegativity leads to bond polarity
The chlorine has a § - charge and the hydrogen has a §+ charge THERE IS AN ATTRACTION BETWEEN THE §+ AND §- CHARGES
§ - means slight

67
Q

Which type of structure has the intermolecular forces hydrogen bonding dipole-dipole etc

A

Simple molecular covalent

If these are not in the question then talk about ionic, metallic, covalent bonding instead refer to Spring CAT q2) This is very important

68
Q

Metal + water
E.g. Sodium + water

A

Metal hydroxide + hydrogen
Na + H20 —> NaOH + 1/2H2
ALWAYS BALANCE

69
Q

Formula phosphate ion

A

PO4 -3

70
Q

Formula hydrogencarbonate

A

HCO3 -

71
Q

Ammonia formula

A

NH3

72
Q

Acid + metal hydroxide =

A

Salt + water

73
Q

How many loan pairs does oxygen have when drawing hydrogen bonding

A

2

74
Q

Metal + steam

A

Metal oxide and hydrogen

75
Q

3 bond 1 loan bond angle

A

107

A Level Chemistry - Physical Chemistry (8 decks)

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