EL - Inorganic chemistry and the periodic table *01 Flashcards

1
Q

how does the periodic table arrange elements?

A

by atomic number

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2
Q

what does the periodic table tell us?

A

can be used to make predictions concerning the properties of an element in a group

arranged into period and columns

  • all the elements in the same period have the same number of electron shells
  • all the elements in the same group have the same number of electrons in their outer shell
  • elements in the same group have similar chemical and physical properties
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3
Q

periodic trends in the melting points - periods one and two, (group 1-2)

A

show similar trends
1. for the metal melting point increases across the period - metal-metal bonds get stronger - metal ions have increasing number of delocalised electrons and decreasing ionic radius (electrons are pulled in closer as the number of protons in the nucleus increases) = HIGHER CHARGE DENSITY.

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4
Q

periodic trends in the melting points - periods one and two (group 3+4)

A

elements with giant covalent structures have strong covalent bonds.
a lot of energy is needed to break these bonds

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5
Q

periodic trends in the melting points - periods one and two (group 5-7)

A

simple molecular substances

melting point depends on strength of intermolecular forces between molecule
intermolecular forces are weak and easily broken so have low melting points

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6
Q

periodic trends in the melting points - periods one and two, (group 8)

A

noble gases

have the lowest melting points because they exist as individual atoms so have very weak intermolecular forces

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7
Q

what is ionisation enthalpy?

A

the energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of 1+ gaseous atoms

X (g) –> X+ (g) + e-

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8
Q

what effects the size of ionisation enthalpies?

A

atomic radius

nuclear charge

electron shielding

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9
Q

how does atomic radius affect ionisation enthalpies?

A

the further the outer shell electrons are from the +ve nucleus the less they’ll be attracted towards the nucleus. So, the ionisation enthalpy will be LOWER

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10
Q

how does nuclear charge affect ionisation enthalpy?

A

nuclear charge = the +ve charge on the nucleus caused by the presence of protons

the more protons there are in the nucleus the more it’ll attract the outer electrons
- it will be harder to remove electron so ionisation enthalpy HIGHER

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11
Q

how does electron shielding affect ionisation enthalpy?

A

the inner electrons shield the outer electrons from the attractive force of the nucleus.
more electrons mean more shielding which means LOWER ionisation enthalpy

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12
Q

trend of 1st ionisation enthalpy down a group

A

decreases
less attraction between nucleus and outer electrons as you go down a group

  • outer shells further from nucleus
  • shielding increases
  • although number of protons increase this doesn’t lead to an increase because it is a less important factor
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13
Q

trend of 1st ionisation enthalpies across a period

A

increases, it gets harder to remove electrons

  • number of protons increasing so outer electrons attracted more strongly to the nucleus
  • and since all outer shell electrons are roughly at the same energy level, generally little extra shielding or extra distance to lessen attraction
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14
Q

what block of the periodic table has lower 1st ionisation enthalpies?

A

s-block metals

  • have relatively low nuclear charges, so lose outer electrons more easily a less attraction between nucleus and the outer electrons

this makes s-block metals reactive

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15
Q

what block of the periodic table has higher 1st ionisation enthalpies?

A

p-block

have higher nuclear charges than s-block metals of the same period

  • increased number of protons
  • so harder to remove outer electron as outer electrons more attracted to nucleus

Less likely to lose an electron

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16
Q

thermal stability trend in group 2 carbonates?

A

increases down the group

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17
Q

factors that affect thermal stability in group 2 carbonates

A

carbonate ions are large anions and can be made unstable by the presence of a cation

  • the cations polarises the anion by drawing the electrons towards it
  • this distorts the carbonate ion, the greater the distortion the less stable the carbonate ion

larger anions cause LESS distortion - have a LOWER CHARGE DENSITY (the charge relative to vol.)

so further down the group the larger the cations so the less distortion caused and the more stable the carbonate ion.

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18
Q

how do group 2 elements react?

A

form ions with a charge of 2+

because group 2 atoms contain 2 electrons in their outer shell and lose both electrons when they react

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19
Q

reactions of group 2: with water

A

react with water to produce a metal hydroxide and H2

eg. M (s) + 2H2O (l) –> M(OH)2 (aq) + H2 (g)

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20
Q

reactivity down group 2

A

increases down group 2

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21
Q

reactions of group 2: with oxygen

A

to produce a metal oxide

eg. 2M (s) + O2 (g) –> 2MO (s)

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22
Q

reactions of group 2: in water

A

form metal hydroxides M(OH)2

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23
Q

acid + base —->

A

salt + water

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24
Q

soluble or insoluble? - lithium salt

A

soluble

25
Q

soluble or insoluble? - sodium salts

A

soluble

26
Q

soluble or insoluble? - potassium salts

A

soluble

27
Q

soluble or insoluble? - ammonium salts

A

soluble

28
Q

soluble or insoluble? - sulfates

A

soluble

except - barium/calcium/lead sulfates form white percepitates

29
Q

soluble or insoluble? - chlorides, bromides, iodides

A

soluble

except for silver halides

30
Q

soluble or insoluble? - hydroxides

A

most insoluble

except - lithium, sodium, potassium, strontium, barium and ammonium hydroxides

31
Q

soluble or insoluble? - carbonates

A

most insoluble

except - lithium, sodium, potassium, ammonium compounds

32
Q

colour of copper carbonate

A

blue-green

33
Q

colour of silver carbonate

A

yellow

34
Q

colour of most carbonates

A

white

copper = blue-green
silver = yellow
35
Q

how do you make an insoluble salt

A

precipitation reaction

occur in aqueous solutions when cation and anions combine to form an insoluble ionic salt

react what you need —> salt will precipitate

filter solution, wash and dry

36
Q

how do you make a soluble salt - using a metal or an insoluble base

A

need the right acid and a suitable metal or an insoluble base (metal oxide or hydroxide)
eg, chlorides = HCl, sulfates = H2SO4, nitrates = HNO3

add solid metal to acid, it will dissolve —> will know its neutralised as no more acid will dissolve

filter out excess metal (that hasnt dissolved)

to get pure solid crystals of salt - evaporate off the water, then leave the rest to evaporate slowly
—> CRYSTALLISATION

37
Q

how do you make a soluble salt - using an alkali

A

titration

  • need to add exactly the right amount of alkali (cant just add excess and filter - both aq)
  • need to use an indicator

then evaporate off water and leave to crystalise

38
Q

FLAME TEST COLOURS - Lithium

A

red

39
Q

FLAME TEST COLOURS - sodium

A

yellow

40
Q

FLAME TEST COLOURS - potassium

A

lilac

41
Q

FLAME TEST COLOURS - calcium

A

brick red (orange red)

42
Q

FLAME TEST COLOURS - barium

A

green

43
Q

FLAME TEST COLOURS - copper

A

blue-green

44
Q

flame test - how to

A

dip nichrome wire in conc. HCl

then dip wire loop into sample

hold loop in clear blue part of bunsen flame

observe colour change

45
Q

NaOH coloured precipitate - sliver, Ag+

A

brown

46
Q

NaOH coloured precipitate - Calcium, Ca2+

A

white

47
Q

NaOH coloured precipitate - copper (II), Cu2+

A

blue

48
Q

NaOH coloured precipitate - lead (II), Pb2+

A

white

49
Q

NaOH coloured precipitate - Iron (II)

A

green

50
Q

NaOH coloured precipitate - iron (III)

A

reddish brown

51
Q

NaOH coloured precipitate - zinc, Zn2+

A

white at first

redissolved in excess NaOH to form a colorless solution

52
Q

NaOH coloured precipitate - aluminium, Al3+

A

white at first

redissolves in excess NaOH to form a colourless solution

53
Q

Test for carbonates

A

with dilute HCl carbonates, CO3 2- will fizz as give off CO2

CO3 2- + 2H+ —-> CO2 + H2O

test for CO2 using limewater —> turns it cloudy (bubble it through)

54
Q

test for sulfates, SO4 2-

A

HCl and barium chloride

Ba 2+ + SO4 2- —> BaSO4 (s)

white precipitate forms - barium sulfate

55
Q

test for ammonium compounds

A

litmus paper

ammonia gas is alkaline - turns red litmus blue

test for NH4+ add NaOH and heat gently
NH4+ + OH- —> NH3 (g) + H2O

56
Q

test for hydroxides

A

litmus paper

red litmus –> blue

57
Q

tests for halides

A

silver nitrate

chloride - white
bromide - cream
iodide - yellow

58
Q

test for nitrates

A

NaOH and aluminium

1) warm with NaOH and Al foil (devadras alloy)
2) Al reduces the nitrate ions to ammonium ions
3) ammonium ions then react with with the hydroxide ions to give off ammonia gas and water
- test red litmus –> blue