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chemistry > paper 1 mistakes > Flashcards

paper 1 mistakes Flashcards

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1
Q

% uncertainty formula

A

uncertainty/ measured value x100 xnumber of measuremnts

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2
Q

what is a salt bridge soaked in

A

filter paper saturated with potassium nitrate KNO3

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3
Q

aq copper (ii) ions with excess NH3

A

[Cu(H2O)6] 2+ + 4NH3 > [Cu(NH3)4(H20)2] 2+

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4
Q

carbonate ion and charge

A

CO3 2-

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5
Q

partial pressure=

A

total pressure x mole fraction

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6
Q

mole fraction of A =

A

mols of A/ total number of mols of gas

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7
Q

is the bond entlaphy of C-H exo or endo

A

endo

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8
Q

is the second electron affinity for oxygen exo or endo

A

endo

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9
Q

is the standard enthalpy change of formation of magnesium endo or exo

A

exo

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10
Q

enthalpy of hydration definition

A

enthalpy change when 1 mole of gaseous ions forms 1 mole aq ions STP

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11
Q

how do the enthalpy changes of hydration of F- and Cl- differ

A

F- smaller than Cl-
more exothermic enthalpy change of hydration
F is smaller, greater attraction to water

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12
Q

average bond enthalpy

A

energy required to break 1 mole of bonds in gaseous molecules

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13
Q

if temp is lowered and forward reaction is favoured, forward reaction is,

A

exo

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14
Q

% dissociation =

A

(H+/HA) X 100

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15
Q

what re lattice enthalpies always

A

exothermic

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16
Q

what does the magnitude of lattice enthalpy indicate

A

ionic bond strength ( more exothermic= stronger ionic bond)

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17
Q

can lattice enthalpies be measured directly

A

no (gaseous ion)

18
Q

downwards arrow on bon harbour cycle

A

exo

19
Q

upwards arrow on born harbur cycle

A

endo

20
Q

two factors that affect magnitude of LE

A

ionic radius
ionic charge
(charge density)

21
Q

how does ionic radius affect enthalpy change of hydration

A

becomes more exothermic with decreasing ionic radiu
(smaller ions, greater charge density, stronger ion-dipole attractions between water and ions, more energy released when they are hydrated

22
Q

how does ionic charge affect enthalpy of hydration

A

larger ionic charge, more exothermic
( greater charge density, stronger ion-dipole attractions, between water molecules and ions therefore more energy released when they are hydrated)

23
Q

what structure are the halogens
what does this mean

A

simple covalent
weak L forces between molecules

24
Q

H2O + Cl2

A

> HCl + HClO (Chloric acid )

25
Q

disadvantage of chlorinated of water

A

chlorine reacts with organic compounds in water to form halogenated organic molecules- carcinogenic

26
Q

Cl2 + 2NaOH

A

> NaClO + NaCl + H2O

27
Q

what is sodium chlorate (i)

A

bleach

28
Q

what must NaOH be to produced bleach

A

cold, aq

29
Q

if NaOH is hot and conc

A

3Cl2+ 6NaOH> 5NaCl + NaClO3 + 3H2O

30
Q

trend in oxidising power down group 7

A

decreases

31
Q

reactivity of halogens down group and why

A

decreases
AR increases
shielding increases
less nuclear attraction to attract electron

32
Q

group 2 metal + water

A

M + 2H2O > M(OH)2 + H2

33
Q

what are metal hydroxides
and trend

A

alkalis
solubility of metal increases down group
pH of alkali solution increases down group

34
Q

reactivity of group 2

A

increases down group
AR increases
shielding increases
attraction between nucleus and outer electrons decrease
outer e lost more easily

35
Q

metal oxide/ hydroxide + acid

A

> salt + water

36
Q

metal oxide + water

A

> metal hydroxide

37
Q

what do metal hydroxides do in water

A

dissolve / dissociate
because they are alkalis (soluble bases )

38
Q

heat and group 2 carbonate

A

thermal decomposition
CaCO3> CaO + CO2

39
Q

trend of thermal decomposition

A

more difficult to decompose down group

40
Q

how many mg is 0.301 g

A

301

41
Q

explain why a reaction has a negative enthalpy change

A

more energy released to make bonds than energy required to break the bonds

chemistry (6 decks)

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