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Thursday, June 4, 2015

Chem
Acidic = H+ ions and solution (water)
ClO3 + I2 -> Cl- + IO3
I2 has 2 iodine atoms, so the change is a loss of 10e- (5 e- for each atom)
Add 3 H2O to make up for the unbalanced 15:18 O2 mol
...

NOW
3 H20 + 5ClO + 3 I2 -> 5Cl- + 6 IO3 + 6 H+
*MAKE SURE CHARGES BALANCE ON EACH SIDE
5- on reactants side and 5- on products side, therefore it is finished

Basic = OHCH30H + MnO4- -> CO3 ^2- + MnO4 ^225 O`s: 27 O`s
Add 2 H2O to balance oxygen atoms on reactants side
Add 8 H`s to balance hydrogen mol
...
The CO(g) used in this reaction is
called the REDUCING AGENT
...

-1
2Al (s) + 3 Cl2 (g) -> 2AlCl3 (s)

In this reaction, the Al (s) is OXIDIZED to AlCl3 (s)
...

Oxidizing Agent (OA)- a sub
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Through a vast number of experiments, a redox table (see Appendix C11) has been
constructed to outline the relative strengths of reducing agents and oxidizing agents
...

Negative value=strong reducing agent, but it gets oxidized (M/C QUESTION)
Organization of a Redox Table
> 1/2 Reactions are written as reductions (e- on left)
> Strongest oxidizing agent is at the top left

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Monday, June 8, 2015
> Strongest reducing agent is at the bottom right
> Double arrows indicate that the reactions can be read from left to right (a reduction) or
right to left (an oxidation)
Redox Spontaneity Rule
A spontaneous redox reaction occurs only if the OA is ABOVE the RA in the redox table
OA
Spontaneous

RA
Non spontaneous

+
Reaction
RA

+
Reaction
OA

In general,
non-metals are stronger OA and metals are stronger RAs and ACIDIC SOLUTIONS
tend to be stronger OAs
...
solutions contain H2O (l) (relatively strong RA)
> Acidic solutions contain H+ (aq) ions
> Basic solutions contain OH- (aq) ions
> Some OA and RAs are combinations (MnO ^4- (aq) and H+ (aq))
> Some substances can act as either OA or RA (H2O (l) , Fe ^ 2+ (aq), Cu+ (aq), Sn
^2+ (aq), and Cr ^2+ (aq)) MEMORIZE AND BE ABLE TO RECOGNIZE
Step 2: Label all of the possible entities as either OA or RA
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Monday, June 8, 2015
> Find the strongest OA present in the solution (from Appendix C11)
> Find strongest RA present in solution (“)
Step 3: Use this info
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Ex
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Will there be a spontaneous redox reaction?
K+ Fe ^+2, MnO4-, SO4 ^2-, H+, H20
Step 1: List all possible entities

K+ (aq), Fe ^+2 (aq), MnO4-(aq), SO4 ^2-(aq), H+(aq), H20 (l)

Step 3: Use this info
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K+ = OA -2
...
51 HIGHEST + VALUE = STRONGEST OA
Mn04- with H2O =+ 0
...
77
Fe ^ 2+ = OA -0
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93
SO4 ^2- = OA +0
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23 HIGHEST - VALUE = STRONGEST RA
H20 = OA -0
...
51) IS ABOVE THE STRONGEST RA (+1
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HW: PAGE 683 #6,11
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Monday, June 8, 2015
NOT A QUESTION ON THE EXAM!!!!!!!!!!!!!!! GOOD M/C CHOICE QUESTION
THOUGH (IS REACTION SPONTANEOUS OR NOT)
Batteries
over extended periods of time (several years) the chem
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energy available will then decrease
The power (Watts (W)) of a cell or battery
> is the rate at which it produces electrical energy
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For ex
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If the energy density is high ( lots of joules but a low mass) it would be much more
practical to be used in a car
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Once the chemicals are all used up, the cells can no l longer produce
any electrical current (typically one time use, short life) 1
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than secondary
cells that only produce 1
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The chemical process used to produce the electric current can be
REVERSED by using electricity to restore the original compounds
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2V

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Monday, June 8, 2015
Fuel cells are a special type of primary cell,
> Where the chemical reactants (fuel) are continuously supplied
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Hydrogen-oxyggen
fuel cell, the H fuel cell (Ballard fuel cell) the aluminum-air fuel cell and the phosphoric
acid fuel cell
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Since redox reactions involve the transfer of e-, these chemical reactions can be used
to produce electricity
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energy into electrical energy; it
consists of 2 electrodes (usually 2 metals) and an electrolyte (an aq
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Battery = 1
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consists of 6 - 1
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electrode = ANODE
E- flow from the anode to cathode
The amount of electrical energy that a cell can produce is dependent on the electric
potential diff
...
This is the voltage of the
cell and is measured in volts (V)
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It is not dependent on the size of the cell but
rather the chem
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Electric current (amperes (A) or coulombs/sec
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This is dependent on the speed of the eproduction by the chem
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The larger the cell the greater the current that can be produced by the cell
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Diff
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5V, however, the bigger the
battery the bigger the current production
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87 V
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04 V
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87- (-3
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91 V
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One uses a ‘salt bridge’ which is a u-shaped
tube filled with a non-reactive electrolyte (+ and - ions that are not part of the net
reaction)
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The other uses porous porcelain cup that contains one of the electrodes and
electrolytes
...
1 : Determine which metal is the cathode and which is the anode
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15 (cathode)
Zn (s) = -0
...
(Cu (s) is the cathode)
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In this case, the anode would therefore be the Zn (s) and it will LOSE 2 eZn (s) -> Zn ^ 2+ (aq) + 2eEx
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Cu 9s) / Cu (NO3)2 (aq) // AgNO3 (aq) / Ag (s)
The SOA present is Ag + (aq) (gets reduced) = cathode
Ag + (aq) and the silver ions will GAIN an e- and become a metal
Ag+ (aq) + e- -> Ag (s) GAIN MASS
This makes Ag (s) the cathode
The SRA is Cu (s) and undergoes an oxidation at the anode (-)
In this case, the anode would therefore be the Cu (s) and it will LOSE 2e- and become
part of the aq
...
0 mol/L for the (aq)
entities
Standard Reduction Potential (Er0) - The ability of a standard 1/2 cell to attract e- The 1/2 cell with the more positive standard
reduction potential will gain e- from the 1/2 cell with the lower standard reduction
potential
Standard Cell Potential- The max
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2: A voltmeter indicates that in a standard copper-scandium galvanic cell (using Cu
2+), copper is the cathode and the standard cell potential is 2
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Since copper is the cathode, the 1/2 reaction for copper is:
Cu ^2+ (aq) +2e- —> Cu (s) (i
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written as a reduction)
Write the 1/2 reaction for the scandium as an OXIDATION (opposite)
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Monday, June 8, 2015
Sc (s) —> Sc ^3+ (aq) + 3eCOMMON FACTOR OF 6
3Cu ^2+ (aq) + 6e- —> 3Cu(s)
2Sc (s) —> 2Sc ^3+ (aq) + 6e-

3Cu ^ 2+ (aq) + 2Sc (s) —> 3Cu (s) + 2Sc ^3+ (aq)
The shorthand cell notation for this galvanic cell is :

Cu (s) / Cu ^2+ (aq) // Sc ^3+ (aq) / Sc (s)
The standard reduction potential for the scandium ion (Sc ^3+) is:

delta E0 = Er 0 - Er0
cell

cathode

anode

2
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34 - Er0 (Sc ^3+)
Er0 (Sc ^3+ )= -2
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Homework pg
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(Mass`s aren`t the same bc copper has a higher molar mass than zinc)

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Monday, June 8, 2015

EXAM REVIEW
ORGANIC CHEM M/C NAMING
Hydrocarbons - only hydrogen and carbon
/C

/C-C

C-C-C-C-C-C
/C
4- ethyl, 2,2-dimethyl hexane

-C/C-C
C-C-C-C-C-C-C-C
/C-C-C/C
5-t-butyl-3-isopopylnonane
REACTIONS
Hydrocarbons =non reactive (single bonds not as reactive)
C-C-C + Cl 2 —>
/Cl
C-C-C (using Heat, UV light, Fe catalyst) + HCl (g)
Cyclohexane undergoes substitution
ALKENE
/C
C-C-C=C-C
/C


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Thursday, June 11, 2015
trans -2 - pentene
/-C=C-C-C-C-C
1-pentene
C(n)H(2n + 2)
Isomers- same chem
...
structure
C=C-C +H2O —> H-C-C-C
/OH (reacts with H2SO4)
2-propanol (COMMON NAME: isopropyl)
Above is a hydration reaction
Markovnikov`s Rule- H goes to Carbon with most H bonds to begin with
C=C-C + F2 (HALOGEN) —> (ROOM TEMP
...
) C-C-C
/H /Cl
C-C-C-C
/OH
2- butanol
s-butyl alcohol

/OH

Secondary alcohol (attached to 2 other Carbons) (C-C-C)
C-C-C-C-C —> (H2SO4) C-C-C=C-C + H2O
/OH

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Thursday, June 11, 2015

C-O-C-C-C (Methoxypropane)
C-C-C=O
/H
propanal
Aldehyde
//O
C-C-C-C-OH (CARBOXYLIC ACID)
//O

//O

C-C-C-H + C-C-OH—> (H2SO4) C-C-C-O-C-C
ethyl propanoate (ONLY ONE WITH A SPACE, ONLY ESTERS GET THE
SPACE) Ester- smell sweet (LIKE EASTER)
Amine
C-C-C-N-C
/C
N,N-dimethyl-1-aminopropane
SAPONIFICATION - MAKING A SOAP M/C QUESTION
Alkyl - refers to a carbon chain/branch (methyl, ethyl , propyl)
Alkyl halide - alkyl with a halide on it
Amides (GET A SPACE IN THE NAMING AS WELL AS ESTERS)
C-C-C-N
//O
propanamide

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Thursday, June 11, 2015

PICTURE ON PHONE, GIVEN NAME,
TOLD TO MAKE FROM AN ACID C-C-C=O
/C
+ C-N-C-C-C (l)

/OH (l)

POLYMERS
-Know diff
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C) - Bohr = prism
Rutherford- Gold foil, nucleus is small and positively charged

- Heisenberg = uncertainty principle
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Thursday, June 11, 2015

- Shrodinger = wave equation
- E- configuration & atoms / ions
- 1s, 2s, 2p, 3s, 3p, 4s, 4p
- Given the e- configuration and asked what element (M/C)
- Fe 2+ and Fe 3+ —— (diff
...
5 (no hybridization,needs p orbital)
/H /H

- H-N-H (pyramidal ) Bond angle = 107
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5
-

/H

- 4 ON EXAM ( 3 M/C) - NAME IT, OR BOND ANGLES
- E- COMPOUNDS, COVALENT NETWORKD, 4 FORMS OF
CARBON (DIAMOND, GRAPHITE, BUCKYBALLS, nanotubes)

- IONIC COMPOUNDS + PROPERTIES

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Thursday, June 11, 2015

EXAM
4 WAYS A REACTION CAN BE SPED UP (s/a) - catalyst, increase in temp, increase in
SA, agitation
MAKE A BUTANOIC ACID FROM BUTANOL (DRAW STRUCTURE, REACTION
CONDITIONS)
No new problems , basic concepts
POLYMERS - e- configuration, explain why iron has a +2 and +3 charge
BONDS (PI )
WHAT IS CALORIMETRY, DEFINITIONS FOR THERMOCHEMISTRY (HESS`S LAW)
THERMO CHEM TEST THE 8/9 MARK QUESTION IS THE PROBLEM QUESTION
REACTION RATES- DIAGRAM LABEL TRANSITION STATE, THINGS THAT CHANGE
REACTION RATES, EXOTHERMIC OR ENDOTHERMIC, 4 MARK
QUESTION…
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surrounding decreases
Exothermic = system decreases in temp
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of 2+ reaction
is the algebraic sum of the heat of other reactions (DELTA H )

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Monday, June 15, 2015
q = mc
q=

amount of heat transferred

m= mass
c = specific heat capacity (J/g 0C)
T = change in temp
...
5 kJ )
H = -601
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that gets used up in reaction, hence why it isn`t in the net reaction)

- Slowest step = Rate Determining Step (RDS)
- RATE = k (A) (B) (C)
- 1st order reaction (all are to the exponent 1 )
- 0 Order Reaction - no effect on reaction
- 1st order = double concentration of reactant , rate doubles
- 2nd Order = double concentration of reactant, rate quadruples
- Empirically = an investigation / experiment to find result
- 4 mark question to find rate law, given table with rate law and concentrations
Equilibrium - Closed system, where the forward reaction and the reverse reactions
occur at the same rate and the [ ] of products and reactants stays constant *** M/C
QUESTION definitions where 3 words are changed !!!
Keq not constant when temp
...

INCREASE
CH3COOH —> CH3COO- + H+
If CH3COO- IS INCREASED , [H+] ions will decrease as reaction favours reactants to
balance out
Ksp - m/c (multiplying concentrations together )
PbCl2 —> Pb ^ 2+ + 2ClSolubility of PbCl2 is 2
...
0x 10 ^ -5 moles of PbCl2 dissolved
[Pb ^2+] = 2
...
0 x 10 ^-5)
= 4
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5 mol/L
Solubility of PbCl2? (How much will dissolve in the solution)
PbCl2 (s) —> Pb ^2+ +2Cl- (aq)
0
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5

C

-

+x

+2x

E

-

x

2x + 0
...
2 x 10 ^-12 = (x) (2x + 0

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