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Chemistry Nov Mocks > 3.1 the periodic table > Flashcards

3.1 the periodic table Flashcards

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1
Q

how is the periodic table arranged

A

.in order of increasing proton number
.elements on the same period = same number of shells
.elements on the same group = same num of outer electrons(similar chemical properties)

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2
Q

what happens to atomic radius as you go along a period

A

.it decreases
.due to increase in nuclear charge with the same amount of shells = greater attraction to outer electrons = outer pulled closer to nucleus

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3
Q

what happens to atomic radius as you go down a group

A

.it increases
.as you go down = 1 more electron shell = + distance between outer electrons and nucleus = less attraction
.more shells = more electron shielding = less nuclear attraction = atomic radius increases

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4
Q

what is first ionisation energy

A

minimum energy required to remove one mole of electrons from one mole of atoms in a gaseous state(KJmol-1)

.Na(g) –> Na+(g) + e-

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5
Q

why does successive ionisation energy increase as more electrons are removed

A

.as atomic radius decrease = greater attraction between nucleus and outer electrons

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6
Q

what is the trend of first ionisation energy along a period

A

.increases = decreasing atomic radius and greater forces of attraction

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7
Q

what is the trend of first ionisation energy down a group

A

.decreases = increasing atomic radius and electron shielding = less forces of attraction

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8
Q

what does a large jump in successive ionisation energy mean

A

.which group the element is in
e.g. a big jump between 3rd and 4th means that there were 3 outer electrons on the shell meaning that is was in group 3

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9
Q

what is the first ionisation energy trend in period 2

A

.general increase = - atomic radius and + nuclear charge

.boron is lower = energy diff between 2s and 2p sub-shell = electron being removed from a higher energy level = further away = held less strongly

.oxygen is lower = repulsion within 2p orbital = destabilising compared to N = easer to be removed

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10
Q

what is the first ionisation energy trend in period 3

A

.general increase = decreasing atomic radius and increasing nuclear charge = held more strongly

.aluminium is lower = energy diff between 3s and 3p = higher energy level = further from nucleus = held less strongly

.sulfur is lower = repulsion in the 3p orbital = destabilising compared to P = electron is removed easier

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11
Q

metallic bonding trend

A

.greater charge on positive ion = stronger force of attraction
.larger ions = weaker attraction due to larger atomic radius = decreasing nuclear charge

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12
Q

what are metallic properties

A

.good conductors as sea of delocalised electrons is able to move and carry flow
.malleable as the layers of positive ions can slide over each other
.high mp as the electrostatic forces of attraction are strong = require alot of energy to overcome

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13
Q

what is a giant covalent lattice

A

.network of atoms bonded by many strong covalent bonds
.high mp due to many strong covalent bonds

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14
Q

properties of diamond

A

.gaint covalent lattice
.each carbon is covalently bonded to 4 other carbons = rigid and very strong

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15
Q

properties of graphite

A

.gaint covalent lattice
.each carbon is covalently bonded to 3 other carbon in flat sheets = 1 delocalised electron per carbon = can move between layers = can conduct electricity
.strong covalent but weaker intermolecular = layers can slide over each other = good lubricant

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16
Q

properties of graphene

A

.single sheet of graphite = 1 atom thick and form hexagonal carbon rings = very strong and rigid and lightweight
.can conduct electricity due to a delocalised electron on each carbon

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17
Q

what is the melting points of period 2 elements

A

.lithium and beryllium = giant metallic = strong attraction between posi ion and electrons = metallic bonding = Be higher due to more outer electrons with same num of shell = smaller atomic radius = stronger attraction

.boron and carbon = gaint covalent = stronger covalent bonds = more energy to break = higher bp = C higher due to more outer electrons in same num of shells = smaller atomic radius = stronger attraction

.last four = small simple covalent molecules = weak van der waals = less energy to break = low mp

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18
Q

melting points of period 3 elements

A

.sodium, magnesium and aluminium = giant metallic = strong attraction between posi ion and electrons = metallic bonding = Al highest due to more outer electrons with same num of shell = smaller atomic radius = stronger attraction

.silicon is a giant covalent = stonger covalent bonds = more energy to break = higher mp

.P,S,Cl,Ar = simple covalent molecules = weaker van der waals = less energy = lower mp

19
Q

group 2 metal + water —->

A

metal hydroxide(alkaline) + hydrogen

Mg + 2H2O —> Mg(OH)2 + H2

19
Q

physical propeties of group 2 elements

A

.atomic radius increase down group = as more electron shells
.increased electron shielding and atomic radius down group = outer electrons held weaker = easier to lose = reactivity increases
.1st and 2nd ionisation energies decrease down the group due to greater atomic radius and electron shielding = easier to remove electrons

20
Q

Mg + steam —>

A

MgO + H2

21
Q

what is the trend of group 2 metals reacting with water

A

.reactivity with water increases down the group

22
Q

group 2 metal oxide + water —->

A

metal hydroxide

23
Q

group 2 metal + chlorine gas —->

A

metal chlorides(white precipitates)
.reaction more vigourous down the group

Mg + Cl2 –> MgCl2

24
Q

group 2 metal + oxygen –>

A

.oxides
.vigourous reaction
.strontium and barium react with excess oxygen and heat to form metal peroxides

2M + O2 –> 2MO

Sr and Ba:
M + O2 -> MO2

25
Q

group 2 metal + dilute acids –>

A

.bubbles of hydrogen gas and solutions of metal compounds

X + 2HCl –> XCl2 + H2
x + H2SO4 –> XSO4 + H2
X + 2HNO3 –> X(NO3)2 + H2

26
Q

group 2 hydroxide + dilute acid –>

A

.salt + water

Ca(OH)2 + 2HCl –> CaCl2 + 2H2O

27
Q

solubility of group 2 hydroxides trend

A

.increases down group

28
Q

uses of hydroxides

A

magnesium/calcium carbonate - in medicine as a antacid to neutralise acids

calcium - agriculture to neutralise acidic soils

29
Q

solubility of group 2 sulfate trend

A

.decreases down group
.barium used for medicine as a medical tracer

30
Q

halogen physical properties

A

.atomic radius increases and electron shielding down the group
.simple covalent = weak van der waals = strength of van der waals increases down group = higher mp and bp
.down group reactivity increases

31
Q

why are halogens good oxidising agents

A

they accept electrons
.oxidising power decreases down the group due to increased shielding and atomic radius
.halogens displace any halide(halogen ions) below it

32
Q

why are halide ions good reducing agents

A

they donate electrons so becoming oxidised
.reducing power increases down the group due to electrons being easier to lose = increase shielding and atomic radius

33
Q

chlorine + water –>

A

CIO- + Cl - + 2H+
.reaction used in water treatment systems to kill bacteria but is toxic

34
Q

chlorine + sodium hydroxide –>

A

NaCIO + NaCl + H2O
.used in bleach production

35
Q

Group 1/2 metals + chlorine gas –>

A

.metal chlorides(white precipitates)

.Mg + Cl2 –> MgCl2

36
Q

hydrogen halides + ammonia gas –>

A

ammonium salt

HCl + NH3 –> NH4Cl
HBr + NH3 –> NH4Br
HI + NH3 –> NH4I

37
Q

hydrogen halides + water –>

A

dilute acids

HCl + H2O –> Cl- + H3O

38
Q

what is the order for ion testing

A

carbonate, sulfate, halide

39
Q

what is the carbonate test

A

.when acid is added = carbonate ions will fizz and CO2 gas is given off
.gas collected and bubbled through lime water which turns cloudy = CO2

XCO3 + 2HCl –> CO2 + H2O + XCl2

40
Q

what is the test for sulfates

A

.use acidified BaCl2 = forms white percipitate of barium sulfate

.BaCl2 + XSO4 –> BaSO4 + XCl2

41
Q

what is the test for halide ions

A

.add acidified silver nitrate
.Cl- = white precipitate
.Br- = cream precipitate
.I- = yellow precipitate

add dilute ammonia :
Cl- dissolves
Br/I = no change

conc ammonia:
Cl/Br = dissolves
I = no change

42
Q

ammonium test

A

.add NaOH and warm = ammonia gas
.holding damp red litmus paper over substance = turn blue

Chemistry Nov Mocks (3 decks)

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