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chemistry paper 1 > inorganic chemistry > Flashcards

inorganic chemistry Flashcards

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1
Q

does reactivity increase/decrease down group 2

A

increase due to increased electron shielding and atomic radius

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2
Q

what does a metal and water make

A

metal hydroxide and hydrogen

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3
Q

how do the metals react differently with steam

A

Mg has a much faster reaction due to the extra energy so it burns in steam with a bright white flame

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4
Q

what do metals and chlorine produce

A

metal chloride (white ppt)

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5
Q

what do metals and oxygen make

A

metal oxides
more vigorous down group so barium and strontium may produce peroxides

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6
Q

what do metals and dilute acids make

A

hydrogen gas bubbles and metal compounds eg MgCl2

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7
Q

what do group 2 hydroxides and dilute acids make

A

a salt and water

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8
Q

what is the trend of group 2 hydroxide solubility

A

increases down group therefore MgOH2 used in medicine to neutralise acids

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9
Q

what is the trend of group 2 sulfate solubility

A

decreases down group therefore BaSO4 used as medical tracer to image internal organs as it cannot be absorbed into bloodstream

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10
Q

what can you use to test for sulfate ions

A

BaCl2 as it produces BaSO4 which is a white ppt

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11
Q

what does thermal decomposition of group 2 carbonates produce

A

metal oxide (white powder) and carbon dioxide

XCO3 -> XO + CO2

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12
Q

what does thermal decomposition of group 2 nitrates produce

A

metal oxide, nitrogen dioxide and oxygen

2X(NO3)2 -> 2XO + 4NO2 + O2

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13
Q

what does thermal decomposition of group 1 nitrates produce

A

lithium - same as group 2 (metal oxide, nitrogen dioxide and oxygen)

other metals - metal nitrite and oxygen (rarely goes to completion)

2XNO3 -> 2XNO2 + O2

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14
Q

why do down group 1 and 2 elements form more stable carbonates?

A

-ionic radius increases for same overall charge so charge density decreases
-larger ions can polarise the carbonate/nitrate less
-less polarised, more heat is required to seperate the 2 ions

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15
Q

describe a flame test procedure

A

1) dip nichrome wire in conc HCl to clean it and then in a blue bunsen burner flame
2) repeat cleaning until no colour is produced in flame
3) dip wire into unknown metal compound and place into flame, observe colour produced

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16
Q

what colour flame does lithium produce

A

red

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17
Q

what colour flame does sodium produce

A

yellow/orange

18
Q

what colour flame does potassium produce

A

lilac

19
Q

what colour flame does magnesium produce

A

no colour change

20
Q

what colour flame does calcium produce

A

brick red

21
Q

what colour flame does strontium produce

A

crimson red

22
Q

what colour flame does barium produce

A

pale green

23
Q

how do flame tests work

A

energy supplied from flame promotes electrons to orbitals with a higher energy
electrons drop back down to original orbital, releasing energy some of which is in the form of light

24
Q

why does magnesium and other metals produce no colour change

A

the energy emitted has a wavelength which is not in the visible light part of electromagnetic spectrum

25
Q

trend in electronegativity of group 7 elements

A

decreases down group due to atomic radius increasing therefore more shielding so electrons are less attracted to the positive nucleus so more easily removed

26
Q

trend in melting point of group 7 elements

A

increases down group as halogens have more electrons so more London forces to overcome

27
Q

trend in reactivity of halogens

A

decreases down group - atomic radius and shielding increases

28
Q

trend in halogens oxidising agents

A

decreases down group

29
Q

trend in halide ions reducing agents

A

increases down group

30
Q

redox of H2SO4 by sodium Cl and F

A

NaF + H2SO4 -> NaHSO4 + HF
doesnt reduce - same for chlorine

produces misty fumes

31
Q

redox of H2SO4 by sodium Br

A

NaBr + H2SO4 -> NaHSO4 + HBr (misty fumes)
2HBr + H2SO4 -> Br2 + SO2 + 2H2O (orange fumes of Br2 + choking fumes of SO2)

32
Q

redox of H2SO4 by sodium I

A

NaI + H2SO4 -> NaHSO4 + HI
2HI + H2SO4 -> I2 + SO2 + 2H2O (solid iodine and choking fumes)
6HI + SO2 + -> H2S + 3I2 + 2H2O (toxic gas produces smelling of egg)

33
Q

how does chlorine react with cold water

A

Cl2 + H2O -> ClO- + Cl- + 2H+
used in water treatment systems to use small portions of chlorine to kill bacteria

34
Q

how does chlorine react with cold dilute alkali NaOH compared to hot concentrated

A

cold:
2NaOH + Cl2 -> NaClO + NaCl + H2O
used in bleach production

hot:
3Cl2 + 6NaOH -> NaClO3 + 5NaCl + 3H2O

35
Q

how do the halogens react with acidifed silver nitrate (AgNO3)

A

Cl- white ppt
Br- cream ppt
I- yellow ppt

36
Q

add dilute NH3

A

Cl- ppt dissolves
Br + I- no change

37
Q

add conc NH3

A

Cl + Br- ppt dissolves
I- no change

38
Q

what do hydrogen halides and ammonia gas form

A

ammonium salts in acid base reaction

HCl + NH3 -> NH4Cl

39
Q

what do hydrogen halides and water form

A

dilute acids, the H+ ions in hydrogen halide dissociating to form hydroxonium ions with water

HCl +H2O -> Cl- + H3O+

40
Q

how to test for carbonate/hydrogen carbonate ions

A

add any acid and it should fizz as CO2 gas is given off, bubble through limewater

XCO3 + 2HCl -> CO2 + H2O + XCl2

41
Q

how to test for ammonium ions

A

add NaOH and ammonia gas will be produced which turns damp red litmus paper blue

chemistry paper 1 (7 decks)

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