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topic 2 Flashcards

(51 cards)

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1
Q

what is ionic bonding

A

oppositley charged ions held together by electrostatic attraction

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2
Q

how to work out ionic formula

A

write two ions
Ca 2+ NO3 -
swap charges
Ca - NO3 2+
drop charges
Ca (NO3)2
simplify
Ca(no3)2

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3
Q

what are the properties of ionic bonds

A

most disolve in water - polar
conduct electricity when molten or disolved - ions free
brittle, layers slide, positive aligned with positive, repel
high mp, strong electrostatic forces

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4
Q

what affects the strength of an ionic bond

A

size of the charge
- bigger charge = stronger electrostatic attraction
- more energy

size of ion
- smaller ion = stronger electrostatic attraction
- ions can pack together more closley
- more energy

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5
Q

what happens to ionic radius down a group and why

A

increases
number of shells increases

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6
Q

what are isoelectric ions

A

diffferent atoms that have same number of electrons

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7
Q

what happens to the ionic radius of isoelectric ions ar atomic number increases and why

A

decreases
more protons pulling electron shells

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8
Q

what evidence is there for charged oartickes including colours and ions

A

electrolysis of copper (II) chromate (VI) on wet filter paper - green

positive Cu 2+ ions move towards -ve cathode - blue

negative CrO4 2- ions move towards +ve anode - yellow

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9
Q

what is covalent bonding

A

sharing of outer electrons to obtain a full shell
electrostatic attraction between shared electrons and +ve nucleus

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10
Q

what is a dative bond

A

one atom dontates 2 electrons

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11
Q

draw the bonding in NH4

A

see covalent bonding flash card

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12
Q

how do bond enthalpy and bond length link

A

shorter bond = higher bond enthalpy

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13
Q

what forces are there in covalent molecules and between what

A

forces of attraction - +ve nucleui and -ve electrons

repulsive forces - 2 +ve nuclei and between electrons of atom

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14
Q

what is bond length in terms of forces

A

balance between attractive and repulsive forces

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15
Q

what happens to the atrractive force, bond length and bond enthalpy when high electron density

A

stronger attraction
shorter bond length
higher bond enthalpy

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16
Q

what is the shape and angle in a moleucle when BP=2 and LP=0 with example and draw

A

linear
180
BeCl2

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17
Q

what is the shape and angle in a moleucle when BP=3 and LP=0 with example and draw

A

trigonal planar
120
BF3

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18
Q

what is the shape and angle in a moleucle when BP=4 and LP=0 with example and draw

A

tetrahedral
109.5
CH4

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19
Q

what is the shape and angle in a moleucle when BP=5 and LP=0 with example and draw

A

trigonal bipyramidal
90 and 120
PCl5

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20
Q

what is the shape and angle in a moleucle when BP=6 and LP=0 with example and draw

A

octahedral
90
SF6

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21
Q

what is the shape and angle in a moleucle when BP=3 and LP=1 with example and draw

Study These Flashcards
A

trigonal planar
107
NH3

22
Q

what is the shape and angle in a moleucle when BP=2 and LP=2 with example and draw

Study These Flashcards
A

bent
104.5
H2O

23
Q

what is the shape and angle in a moleucle when BP=3 and LP=2 with example and draw

Study These Flashcards
A

distorted t
87.5
ClF3

24
Q

what is the shape and angle in a moleucle when BP=4 and LP=1 with example and draw

Study These Flashcards
A

seesaw
87 and 102
SF4

25
what is the shape and angle in a moleucle when BP=5 and LP=1 with example and draw
square pyramidal 81.5 and 90 IF5
26
what is the shape and angle in a moleucle when BP=4 and LP=2 with example and draw
square planar 90 XeF4
27
describe the structure and properties of diamond
each carbon bonded 4x in tetrahedral shape heat conducts - tightly packed rigid arrangement very high mp - strong covalent bonds doesnt conduct electricity - no delocalised electrons insoluble - covalent bonds too strong
28
decribe the structure and properties of graphite
each carbon bonded 3x with 4th electron delocalised layers slide - weak forces between layers conducts electricity - delocalised electrons between layers low density - layers far apart high mp - strong covalent bonds insoluble - strong covalent bonds
29
decribe the structure and properties of graphene
1 layer of graphite hexagonal carbon rings conducts electricity - delocalised free moving electrons high strength - delocalised electrons light weight and transparent - one cell thick
30
what is metalic bonding
positive methal ions are formed as metals donate electrons to form sea of delocalised elctrons electrostatic attraction between +ve metal ions and delocalised electrons more elctrons an atom can dontae the higher the mp
31
what are the properties of metalic bonds
good thermal conductors - delocalised e- transfer kinetic energy good electrical conductors - delocalised e- are mobile and can carry current high mp - strong electrostatic attractions insoluble - metalic bonds strong malleable and ductile - ion layers can slide and still retain at5tractionw
32
hat is electronegativity
ability for an atom to attract electrons towarrds itself in a covalent bond
33
where are the most elecronegative elements on the periodic table
up and right
34
what scale measures electronegativity
pauling
35
how do ionic bonds and electronegativity link
biggger difference more ionic the compound
36
what is a polar bond
covalent bonds become polar if atoms have a difference in elecronegativity eg HCl H2O
37
when are compounds not polar
same electronegativity polar bond stmmetrical eg CO2
38
what are london forces
weakest intermolecular force exist between atoms ant molecule with electrons can form a dipole temporary dipole when 2 molecules neare electrons in one molecule can move from one end to another
39
who do london forces hold some molecules in crystal structure
iodine weak london forced hold I2 molecules strong covalent bonds hold the 2 atoms
40
what affects size of london force
size of atom bigger = larger e- cloud = more london forces
41
what is a dipole dipole intermolecular force
exisit in molecules with polarity eg HCl
42
what is the test for a dipole dipole
placing a charged rod near steadt stream of polar liquid bend towards
43
what is a hydrogen intermoleular force
strongest very electronegative elements - hydrogen with nitrogen, oxygen or flurine
44
what differes in the hydrogen bonding of water and ice
ice forms a regular structure, the molecules are further apart making it less dense
45
why are alcohols not as volatile as alkanes
hydrogen bonding in alcohols
46
what solvents do polar molecules dissolve in
polar solvents
47
what must happen for a substance to dissolve
solvent binds must break substance bonds must break new bonds formed between substance and solvant new bonds of same or greater strength
48
what is hydration and draw diagrams
water molecules surrond ion see flash card
49
do alcohols dissolve
dissolve in polar solvants as they can hydrogen bond hydrocarbon doesnt dissolve bigger=less soluble
50
do haloalkanes dissolve
no as dipoles not strong
51
what are non polar substances and what dissolve in them
only have london force alkenes dissolves as they can form london forces between molecules

chemistry (15 decks)

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