Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

CHEMISTRY > ES > Flashcards

ES Flashcards

1
Q

ES1

A

ES1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Halogens

A

GROUP7

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

colour of aqueous solution (halogens)- Chlorine

A

pale green

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

colour of aqueous solution (halogens)- Bromine

A

yellow/orange

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

colour of aqueous solution (halogens)- Iodine

A

brown

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

colour of solution in cyclohexane (inorganic solution) chlorine

A

pale green

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

colour of solution in cyclohexane (inorganic solution) bromine

A

red/brown

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

colour of solution in cyclohexane (inorganic solution) iodine

A

violet/purple

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

state of fluorine and chlorine

A

gas

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

state of bromine

A

liquid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

state of iodine

A

solid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

group 7 trend(must update this flash card to include reactivity and oxidatising power)

A

as you go DOWN the group, MP and BP INCREASE due to an increase in number of elctrons to van der waals forces strength increases, ore energy required to break them

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

IDIDBs

A

Van der waals forces

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

testing for halides

A

Silver nitrate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

testing for halides CHLORINE

A

white

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

testing for halides BROMINE

A

cream

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

testing for halides IODINE

A

Yellow

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

key rule for halogens

A

the more reactive halogen will oxidise (remove e- from) the halide ions of the less reactive one.
known as DISPLACEMENT REACTION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

ES2

A

ES2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Oxidation

A

loss of electrons
increase in oxidation number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Reduction

A

gain electrons
decrease in oxidation number

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

on an equation which side is the electrons on for OXIDATION

A

e- on right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

on an equation which side is the electrons on for REDUCTION

A

e- on left

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

oxidation state rules

A

F always -1
O always -2
H usually +1
group 1 always +1
group 2 always +2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
atom in an elements oxidation state
always 0
26
steps for balancing redox equations
1. determine all oxidation states 2. how many e- lost or gained BALANCE 3. balance Oxygen (add h20) 4. Balance Hydrogen (add hydrogen)
27
ES3
ES3
28
how to remember what happens at anode and cathode (redox)
ANOX REDCAT
29
cathode is the ___ electrode
negative
30
Anode is the ____ electrode
Positive
31
Cations move to Anions move to
cathode anode
32
reaction for water at cathode
2H20(l) + 2e-----2OH-(aq) + h2 (g)
33
reaction for water at anode
2H20(l)----O2(g) + 4H+ (aq) +4e-
34
ES4
ES4
35
Dynamic equilibrium definition
-the rate of the forward reaction is the same as the reverse reaction -the concentrations of the reactants and products remain CONSTANT -sign is two arrows in opposite directions
36
an exothermic reaction has a __ sign
- and forward
37
an endothermic reaction has a __ sign
+ and reverse
38
Le Chateliers principle
when a system in dynamic equilibrium is subjected to change, the position of equilibrium will shift to minimise change
39
positions of equilibrium can altered by changing
temperature pressure involving reactions including gasses concentrations of aqueous solutions (reactants or products)
40
The deacon process
4HCl (g)+o2(g)------2Cl2 (g) + 2H2O(g)
41
best conditions to optimise yield of chlorine
high pressure, low temperature, and excess oxygen
42
equilibrium constant
Kc
43
Kc
aA+bB= cC+ dD = sign is the sign for equilibrium in this case
44
kc equation
Kc = [C] c [D] d / [A] a [B] b, where [A], [B], [C], [D] are the molar concentrations of the species, and a, b, c, d are the coefficients in the balanced chemical equation. The Kc value is constant for a given reaction at a given temperature.
45
the only thing that will change the value of Kc
temperature
46
exam q for kc mark scheme
1. kc equation 2. calculated value 3. interpretated units
47
effect of equilibrium on changing: TEMPERATURE
Increase in temp = favour endothermic decrease in temp= favour exothermic equilibrium shifts in order to contradict the chnage applied
48
effect of equilibrium on changing: CONCENTRATION
increasing concentration of reactants = moves to right to form more products increasing concentration of products= moves to the left to form more reactants
49
effect of equilibrium on changing: PRESSURE
Will only affect equilibrium if reaction involves gasses The side with the greatest number of moles is at higher pressure
50
effect of catalyst on equilibrium
does not change the position of equilibrium changes the RATE equilibrium is established by increasing the rate of both forward and backward reaction equally
51
equilibrium constant and its meaning Kc>1
more products than reactants at equilibrium
52
equilibrium constant and its meaning Kc>>1
(greater than 10^10) the reaction appears to have gone to completion
53
equilibrium constant and its meaning Kc<1
there are more reactants than products
54
equilibrium constant and its meaning Kc<<1
(less than 10^-10) the reaction appears to not have happened
55
kc will remain conctants as long as BLANK as stays constant
TEMPERATURE
56
ES5
ES5
57
give one problem with transporting chlorine or bromine
very toxic
58
ES6
ES6
59
atom economy equation
[formula mass of desired product/relative formula mass of all reactants used] / 100
60
thermal stability of hydrogen halides
down the group the THERMAL STABILITY DECREASES - bond enthalpy decreases -less energy required to decompose the bond
61
trend in oxidisation agents down group 7
as you go DOWN group 7 -less effective as oxidising agents -fluorine is the most electronegative
62
oxidising agent definition
can attract other e- to make other elements oxidised
63
trend in acidity down group 7
- all hydrogen halides are acidic -they get better at donating protons down the group -HCl HBr HI almost completely dissociate to give oxonium ions
64
reaction of hydrogen halides with ammonia
-salts are formed -'white cloud' of ammonia is made (this is a very fine SOLID)
65
Reaction of hydrogen halides with sulfuric acids
HCl and HF do not react HBr makes SO2
66
test the reaction of HBr and sulfuric acid with__
potassium manganate VIII purple to colourless
67
test the reaction of HI and sulfuric acid with__
Lead ethanoate black precipitate form (this is lead sulphide)

CHEMISTRY (7 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions