Additional Notes to the Packet That Were Given on Friday 5/9/2014 Or Monday 5/12/14

Additional notes to the packet that were given on Friday 5/9/2014 or Monday 5/12/14:

We are learning RedOx to:

- practice balancing equations

-review basic terminology: ion, cation, anion, reactant, product, transition metal, alkali metal, alkali earth metals, halogens, noble (inert) gas

- understand batteries better

-review activity series of metals ( and explore reactivity of other compounds)

- etc. etc. etc

Thermite reaction (notes at end of this file) and magnesium HCl battery will be done as demos

Balancing a chemical equation gives you lots of information. Some equations are more difficult to balance. The technique of half reactions will allow you to balance some equations that you would find difficult otherwise.

Oxidation numbers help us keep track of the movement of electrons (what chemistry is really all about)

We need to learn how to assign oxidation numbers

RedOx notes:

Remember electrons are Negative (losing electron makes you positive)

You MUST remember the basic definitions, which are often summarized as

Oil Rig Oxidation is Loss of electrons; Reduction is Gain (of electrons)

LEO GR Loss of Electrons is Oxidation, Gain is Reduction

v In Oxidation half reactions, the oxidation number (value) of the element increases (like a big Ox)

Na à Na+ + 1e-

In Reduction half reactions, the oxidation number (value) gets smaller (this is what reduction means)

2 e- + Cu+2 à Cu

Oxidizing Agents allow oxidation to proceed (by being reduced)

Reducing agents allow reduction to proceed (by being oxidized)

Steps to take in solving the Redox problems

(how partial credit will be determined on the test)

1) Assign oxidation numbers (elements have just as many protons as electrons, Ions have a net charge).

2) Identify the two half reactions: what is being oxidized and what is being reduced.

3) Balance each half reaction (keep the subscripts in mind now so you don’t get confused later).

4) Balance the two half reactions so that just as many electrons are produced as are needed.

5) Add the two half reactions and transfer these values to the overall reaction.

6) Take into account the spectators (adjust the numbers in step 5 as necessary).

OXIDATION NUMBERS; for every rule there is an exception; you must get the feel of assigning oxidation numbers Please look at several sources (the example on the desk; this one; the one in the book, others on-line, etcetera, etcetera, etcetera)

These are pretty good rules for assigning oxidation numbers

1. The oxidation number for an atom in its elemental form is always zero.

o A substance is elemental if both of the following are true:

§ only one kind of atom is present

§ charge = 0

o Examples:

§ S8: The oxidation number of S = 0

§ Fe: The oxidation number of Fe = 0

2. The oxidation number of a monoatomic ion = charge of the monatomic ion.

o Examples:

§ Oxidation number of S2- is -2.

§ Oxidation number of Al3+ is +3.

3. The oxidation number of all Group 1A metals = +1 (unless elemental).

4. The oxidation number of all Group 2A metals = +2 (unless elemental).

5. Hydrogen (H) has two possible oxidation numbers:

o +1 when bonded to a nonmetal

o -1 when bonded to a metal

6. Oxygen (O) has two possible oxidation numbers:

o -1 in peroxides (O22-)....pretty uncommon

o -2 in all other compounds...most common

7. The oxidation number of fluorine (F) is always -1.

The sum of the oxidation numbers of all atoms (or ions) in a neutral compound = 0.
The sum of the oxidation numbers of all atoms in a polyatomic ion = charge on the polyatomic ion.

When assigning oxidation numbers to the elements in a substance, take a systematic approach. Ask yourself the following questions:

1. Is the substance elemental?

2. Is the substance ionic?

3. If the substance is ionic, are there any monoatomic ions present?

4. Which elements have specific rules?

5. Which element(s) do(es) not have rules?

Use rule 8 or 9 from above to calculate these.

Not great rules but get you the feel of assigning oxidation numbers:

0) elements have zero charge (or they would be ions); just like compounds

1) Poly atomics choose first (Know your poly-atomics if more than 2 elements)

(“The needs of the many outweigh the needs of the few”)

2) Remember they are called oxidation numbers (oxygen chooses -2, usually (can be -1 in peroxides); Fluorine is -1)

3) Give a little, alkali metals choose +1 (by giving up one electron). Hydrogen is above it all and is special (usually +1, but hydrogen can be -1 when in a metal hydride)

4) Alkali earth metals choose +2

5) With all this giving up of electrons there must be some taking, Halogens take one electron to become -1

6) Continue with elements picking their preferred charges (work from outside columns to the inner “valley of confusion”) until there is only one left; if the element is last to choose it must have the charge that makes everything else sum to zero.

Mr P’s summary:

- Know the preferred charges (+1, +2, skip a few, +3,+/-4, -3, -2, -1, 0)

- Neutral atoms/compounds are neutral (zero)

-Know the polyatomics (“the needs of the many outweigh the needs of the few”)

- give a little (alkali metals and alkali earth metals tend to form cations (by giving up electrons)

- take a little (halogens take electrons to become anions)

- they are called Oxidation numbers so oxygen is almost always the -2 anion; (except in peroxides, H2O2)

- hydrogen can be both a cation or an anion (hence metal hydride batteries) SURPRISE

- the elements in the middle of the periodic table choose last so they have to take on a charge to balance the rest

(you can’t always get what you wanted, but if you try real hard you (might just get) what you(“We, the compound”) need)

Practice; YES I know some don’t make sense I put them in to see if you are following the rules

Formula / Known oxidation number / Inferred oxidation number
ZnO / O = -2 / Zn = +2
NaCl2 / Na= +1 / Cl =
MnCl2 / Mn =
MnO2 / Mn =
NiCl / Ni =
Sb2O3
Sb2 O5
MgO
Mg2N3
CaCl2
NH3
N2O5
SnO
BiCl3
CuCl
CCl4
CrCl3
P2O5

Compound polyatomic ION

KNO3 / NO3 = / K = / N = / O =
K2SO4 / SO4 = / K = / S = / O =
Ca3(PO4)2 / PO4 = / Ca = / P = / O =
NaClO3 / ClO3 = / Na = / Cl = / O =
Na2B4O7 / B4O7 = / Na = / B = / O =

Practice; YES I know some don’t make sense I put them in to see if you are following the rules ANSWERS

Formula / Known oxidation number / Infered oxidation number
ZnO / O = -2 / Zn = +2
NaCl2 / Na= +1 / Cl = -1/2 Crazy
MnCl2 / Cl =-1 / Mn = +2
MnO2 / O= -2 / Mn = +4
NiCl / Cl= -1 / Ni = +1
Sb2O3 / O= -2 / Sb = +3
Sb2 O5 / O= -2 / Sb= +5
MgO / O= -2 / Mg= +2
Mg2N3 / Mg= +2 / N= -4/3 Crazy
CaCl2 / Ca= +2 / Cl= -1
NH3 / H= +1 / N= -3
N2O5 / O= -2 / N= +5
SnO / O= -2 / Sn= +2
BiCl3 / Cl= -1 / Bi= +3
CuCl / Cl= -1 / Cu= +1
CCl4 / Cl= -1 / C= +4
CrCl3 / Cl= -1 / Cr= +3
P2O5 / O= -2 / P= +5

Compound polyatomic ION

KNO3 / NO3 = -1 / K = +1 / N = +5 / O = -2
K2SO4 / SO4 = -2 / K = +1 / S = +6 / O = -2
Ca3(PO4)2 / PO4 = -3 / Ca = +2 / P = +5 / O = -2
NaClO3 / ClO3 = -1 / Na = +1 / Cl = +7 +5 / O = -2
Na2B4O7 / B4O7 = -2 / Na = +1 / B = +3 / O = -2

Oxidation –Reduction Reactions Basic Skills

Oxidation Numbers

Using the guidelines from the Nomenclature packet, those described in the book, on-line or elsewhere.

Identify the oxidation number for each of the elements in the following compounds (remember the oxidation number is for the element NOT the gross charge on the group)

NaCl H2O H2SO4

CO2 FeBr2 NH4F

PbBr2 KNO3 CuS

CaCl2 AlF3 SbCl3

Now for some that may be trickier, remember that the oxidation state of the last remaining element is determined by the electro negativity of the elements it combines with.

K3PO4 K2CO3 CaCO3

CO2 CO K2CrO7

CaSO4 K2CrO4 Na2MoO4

FeO Fe2O3 Na2B4O7

Oxidation –Reduction Reactions Basic Skills

Balancing equations

Identify as oxidation or reduction and fill in any missing numbers:

1) Mg à Mg+2 + 2e- Oxidation or Reduction

2) Fe à Fe+3 + __ e- Oxidation or Reduction

3) 1 e- + Fe+3 à Fe+2 Oxidation or Reduction

4) Mg à Mg+2 + 2 e- Oxidation or Reduction

5) __ e- + Mn+5 à Mn+2 Oxidation or Reduction

In the following examples identify the oxidation half-reaction and the reduction half reaction.

6) 2 Mg + O2 à 2 MgO

Oxidation:

Reduction:

7) 2 Fe + O2 à 2 FeO

Oxidation:

Reduction:

8) Mg + S à MgS

Oxidation:

Reduction:

9) __ H2 + __ O2 à __ H2O

Oxidation:

Reduction:

20 tough (and not so tough) RedOx practice problems

(Select 10 from this sheet of 20 practice problems, show all work as described in class

1.) __Cu + __HNO3 à Cu(NO3)2 + __ NO2 + __ H2O

2.) __ H2S + __HNO3 à __ NO2 + __S + __ H2O

3.) __ HCl + __MnO2 à __ MnCl2 + __ H2O + __Cl2

4.) __Cu + __HNO3 à __Cu(NO3)2 + __ NO + __ H2O

5.) __HNO3 + __ H2SO4 + __FeSO4 à __Fe2(SO4)3 + __ H2O + __ NO

6.) __Br2 + __SO2 + __H2O à __ H2SO4 + __HBr

7.) __Na2CrO4 + __ SnCl2 + __HCl à __ NaCl + __ SnCl4 + __ H2O + __ CrCl3

8.) __K2Cr2O7 + __ H2SO4 + __FeSO4 à __K2SO4 + __ Cr2(SO4)3 +__ Fe2(SO4)3 + __ H2O

9.) __KClO3 + __ HCl à __KCl + __ H2O + __ Cl2

10.) __S + __ HNO3 à __H2SO4 __ NO

11.) __Bi2S3+ __HNO3 à __ Bi(NO3)3 + __S + __NO + __ H2O

12.) __FeCl3 + __ H2SO3 + __ H2O à __FeCl2 + __ H2SO4 + __ HCl

13.) __K2Cr2O7 + __HCl à KCl + __ CrCl3 + __ Cl2 + __ H2O

14.) __Cu + __H2SO4 à CuSO4 + __ SO2 + __ H2O

15.) __H2SO4 + __HI à __ H2S + __ I2 + __ H2O

16.) __HNO2 + __ H2SO4 + __KMnO4 à __ K2SO4 + __ MnSO4 + __ HNO3 + __ H2O

17.) __PH3 + __ KMnO4 + __H2SO4 à __ K2SO4 + __ MnSO4 + __ H3PO4 + __ H2O

18.) __Zn + __HNO3 à Zn(NO3)2 + __ NH4NO3 + __ H2O

19.) __K2Cr2O7 + __ NaNO2 + __H2SO4 à __K2SO4 + __ Cr2(SO4)3 +__ NaNO3 + __ H2O

20.) __Sb2S3 + __ HNO3 + __H2O à __H3SbO4 + __ H2SO4 +__ NO

(Can do all 20 for extra credit)

RedOx practice sheet for the test on: do at least 10 problems use your own notebook to practice

(select from the sheet of 20 practice problems)

In the following problems identify:

a) The oxidation numbers of all reactants and products.

b) The oxidation half-reaction.

c) The reduction half-reaction

d) Balance the half-reactions.

e) Balance the complete reaction (by transferring the coefficients and balancing the spectator ions).

__)

Oxidation:

Reduction:

Substance being oxidized ______ (if it’s an ion make sure you include the charge) Reducing agent ______