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Chemistry paper 1 > 3.1.3 Bonding > Flashcards

3.1.3 Bonding Flashcards

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1
Q

Ionic bonding definition

A

he electrostatic forces of attraction between oppositely charged ions

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2
Q

Properties of ionically bonded compounds

A

Solid at room temp
Giant structures
High melting points - the energy must break the ionic bonds in the lattice
Conduct electricity when molten or dissolved un water as they are free to carry current
Brittle

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3
Q

Covalent bonding definition

A

Electrostatic forces of attraction between the shared electrons and the positive nuclei of the other atom

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4
Q

Ionic bonding affected by

A

AR
Nuclear charges

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5
Q

Co ordinate / dative bond

A

One atom provides both electrons in the covalent bond

Have exactly the same strength and length as ordinary covalent bonds between same pair of atoms

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6
Q

Metallic bonding definition

A

Outer main levels of the atom merge causing delocalisation
The electrostatic forces of attraction between the positive metal ions i and the sea of delocalised electrons

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7
Q

Properties of metals

A

Metals are good conductors of heat and electricity
Good conductors of heat - as energy spread by increasingly vigorous vibrations of the closely packed ions
Strong
Malleable
Ductile - still in the exact same environment
High melting point

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8
Q

What is strength of metals determined by

A

Charge of the ion - the greater the charge of the ion the greater the number of delocalised electrons = stronger the electrostatic forces of attraction
Size of the ion - smaller the ion the closer the electrons are to the positive nucleus and the stronger the bond
The number of delocalised electrons - stronger the bond

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9
Q

Melting point of a metal affected by

A

Amount of delocalised electrons
The charge of the nucleus

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10
Q

ionic compounds structure - effected by

A

Effected by the size or charge of the ion
Types of lattice formed - depends on the size fo the pos and neg ions which are arranged in alternate fashion

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11
Q

Linear

A

2bp
0lp
180 degrees

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12
Q

Trigonal planar

A

3bp
0lp
120 degrees

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13
Q

Tetrahedral

A

4bp
0lp
109.5 degrees

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14
Q

Trigonal pyramidal

A

3bp
1lp
107 degrees

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15
Q

Bent

A

2bp
2lp
104.5 degrees

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16
Q

Trigonal bipyramidal

A

5bp
0lp
120 and 90 degrees

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17
Q

Octahedral

A

6bp
0lp
90 degrees

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18
Q

How to explain shape

A

State number of bonding pair and lone pair electrons
State that electron pairs repel and try to get as far as possible
No lp then state that electron pairs repel equally - lp repel more than bonding pairs
State the shape and bond angle

19
Q

Lp effect on bond angle

A

Reduce the bond angle by 2.5

20
Q

Electronegativity

A

The power of an atom to attract the bonding pair of electrons in a covalent bond towards itself

21
Q

Electron density

A

Describes the distribution of neg charge in a molecules

22
Q

What does electronegativity depend on

A

Nuclear charge

Distance between the nucleus and the outer shell electrons

The shielding of the nuclear charge by electrons in inner shells

23
Q

Trends in electronegativity

A

Down the group = decreases - more shielding
Across a period = increases - nuclear charge increases - smaller atom

24
Q

Polarity of covalent bonds

A

Unequal sharing of electrons between atoms that are covalently bonded together
Affected by electronegativity - more electronegative attract the electrons towards itself in a double bond
Greater difference in electronegativity = more polar
really polar= some level of ionic character
Small difference = purely covalent

25
Q

PD - PD forces

A

The attractive forces between two neighboring molecules with a permanent dipole
Polar molecules have permanent dipole
Have a pos and neg charged end

26
Q

ID - ID forces

A

Also called van der waals
Not affected by electronegativity
Electron charge clouds are constantly moving
Causes a temporary dipole which induced a dipole on neighbouring molecules
Means the

27
Q

Hydrogen bonding

A

Type of PD PD forces
Takes place in NOF molecules - as have a lage enough difference in electronegativity when bonded to hydrogen - bond becomes polarised
H becomes delta neg meaning it can bond with the lp of electrons in neighbouring NOF

28
Q

Water

A

Hydrogen bonding in water causes anomalies
High mp and bp
Lots of energy required to break the hydrogen bonds
Id - id - affected by electrons
High surface tension
The ability of liquid surface to resist any external forces
External molecules form hydrogen bonds with the internal molecules
Meaning molecules pull downwards the surface molecules causing the surface of them to become compressed and more tightly together at the surface
Increases tension
Density
Solids more dense than liquids - solid is more closely packed together
Solids are in an open lattice
Bond length remains constant in solid
Tetrahedral shape

29
Q

key phase when describing shapes with no lone pairs

A

equal repulsion force

30
Q

macromolecular

A

giant molecule with covalent bonding

31
Q

intermolecular force between one ammonia and one water

A

hydrogen bonding

32
Q

why a substance is almost insoluble in water

A

no hydrogen bonding with the water

33
Q

PH3 molecule

A

looks like ammonia

34
Q

bond between the PH3 molecule and H+

A

dative/ cordinate bond
pair of elctrons in the PH3 are donated to the H+

35
Q

squre planar molecule

A

XeF4 - as the dipoles calncel out - non polar
(Cu(Oh)2)2+

36
Q

what statement about inorganic ionic compounds is always correct

A

they form giant ionic structures

37
Q

how to workout which molecules have all the atoms in the same plane

A

present of a pi bond means no rotation
meaning alkenes have to have all atoms in the same plane

38
Q

ammonia fact

A

has permanent dipoles

39
Q

Kevlar bonding between chains

A

hydrogen bonding

40
Q

when drawing the shape of an ion key point

A

MUST OUT SQUARE BRACKETS AND THE CAHRGE

41
Q

ionic bonds strength

A

ionic bonds strongest
stronger than metallic bonding

42
Q

ketones an aldehydes and hydrogen bonding

A

do not have hydrogen bonding !
do have dipole dipole

43
Q

working out the shap of a charged compound

A
  1. workout the numb of valence electrons
  2. workout what the charge dies to the number of valence electrons
  3. workout the number of bonding pair
  4. workout how many left - lpss
44
Q

square planer

A

4bp, 2lp
same element attached
repelling equally
bond angle of 90

Chemistry paper 1 (19 decks)

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