Net Ionic equationsA solution of Barium Chloride reacts with a

solution of sodium sulfateBaCl2 + Na2SO4 →

BaCl2 + Na2SO4 → BaSO4 + 2NaCl

Ba2+ + 2Cl1- + 2Na1+ + SO42- → BaSO4 + 2Na1+

2Cl1-

Ba2+ + 2Cl1- + 2Na1+ + SO42- → BaSO4 + 2Na1+

2Cl1-

Ba2+ + SO42- → BaSO4

Using Stoichiometry in the LaboratoryUsing Stoichiometry in the Laboratory

Na2SO3(aq) + 2AgNO3(aq) Ag2SO3(s) + 2NaNO3(aq)

20 ml 20 ml0.12 M 0.35 M

1. How many grams of silver sulfite would be produced?2. What would be the molarity of the sodium nitrate?3.What volume of silver nitrate is needed to completely

precipitate all of the sulfite ions.

Patterns of ReactivitySubstance + Oxygen gas Oxide of element

Active metals and oxygen: Li(s) + O2 Li2O(s)

sulfides and oxygen: ZnS(s) + O2 ZnO + SO2(g)

CS2(s) + O2 CO2(g) + SO2

ammonia and oxygen: NH3 + O2 NO2 + H2O(g)

Substances reacting with water

Metallic oxide reacting with water BaseLi2O + HOH Li+ + OH-

MgO (s) + HOH Mg(OH)2

Metal hydrides reacting with water Base + Hydrogen

LiH(s) + HOH Li+ + OH- + H2

CaH2 (s) + HOH Ca2+ + OH- + H2

Nonmetal halides reacting with water weak acid + strong acid (Keep ox # the same)PCl5 (s) + H2O H3PO4(aq) + H+ + Cl-

PBr3 (s) + H2O H3PO3(aq) + H+ + Br-

Nonmetal oxide reacting with water Acid (Keep ox # the same)

SO2(g) + H2O H2SO3(aq)

N2O5 + H2O H+ + NO31-

SO3 + H2O H+ + HSO4-

N2O3 + H2O HNO2(aq)

Hydrocarbon and oxygen: CH3OH(s) + O2 CO2 + H2O

Substances reacting with nonmetal oxide salt

Metal oxide and nonmetal oxide yields a saltCaO(s) + CO2 CaCO3(s)

MgO(s) + SO2 MgSO3

Base reacting with nonmetal oxide:OH- +CO2(g) CO3

2- +H2O (base is aqueous)

NaOH(aq) + CO2(g) Na+ + HCO3- + H2O

Ca(OH)2 (aq) + SO2(g) Ca+ + HSO3- + H2O

Ca(OH)2 (s) + SO2(g) CaSO3(s) + H2O

Metal sulfides reacting with water Base + gas

Fe2S3(s) + HOH Fe(OH)3(s) + H2S(g)

Metal carbides reacting with water Base + hydrocarbon

Na2C2(s) + H2O Na+ + OH- + C2H2

Salt of an amphoteric metal reacting with water complex

Al(NO3)3(s) + H2O Al(H2O)63+ + NO3

-

Substances reacting with an acidmetals reacting with acid salt + hydrogen

Zn(s) + H+ Zn2+ + H2

Cu(s) + H+ + HSO4- Cu2+ + SO2 + H2O (hot

conc. sulfuric acid)

Ca(s) + H+ Ca2+ + H2 (cold sulfuric acid)

Ag(s) + H+ + NO3- Ag+ + NO + H2O

(dilute (6M) nitric acid)

Ag(s) + H+ + NO3- Ag+ + NO2 + H2O (conc. nitric acid)

metal oxide reacting with hydrogen gas salt + water

FeO(s) + H+ + NO3- Fe3+ + NO2 + H2O

(conc. nitric acid)

metal oxide reacting with acid salt + gas + water

Fe2O3(s) + H2 Fe + H2O

Salt of a weak acid and strong acid salt of strong acid + weak acid

C2H3O2- + H+ HC2H3O2

C2H3O2- + H+ + HSO4

- HC2H3O2 + HSO4-

(equimolar sulfuric acid)

SO22- + H+ H2SO3 H2O + SO2

Na2S(s) + H+ Na+ + Cl- + H2S

Substances reacting with an Base

Al and Zn hydroxides with a strong base

Al(OH)3 + OH- [Al(OH)6]3-

Zn(OH)2 + OH- [Zn(OH)4]2-

salt of an amphoteric metal reacting with a strong acid

salt of a weak acid reacting with a strong baseNH4Cl + OH- NH3(g) + H2O + Cl-

HCO3- + OH- CO3

-2 (g) + H2O

Al(OH)3 + H+ Al3+ + H2O

Complex ions

Zn2+ + NH3(excess) [Zn(NH3)4]2+

Zn(OH)2(s) + NH3(ex) [Zn(NH3)4]2+ + OH-

Ag+1 + NH3(excess) [Ag(NH3)2] +

Cu(OH)2 + NH3(ex) [Cu(NH3)4]2+ + OH-

Fe+3 + NCS1- → FeNCS2+

orange/brown blood red

Oxidation-Reduction

Single Replacement (metals)

Al(s) + Cu2+ (aq) Cu(s) + Al3+ (aq)

Zn(s) + Sn2+ (aq) Sn(s) + Zn2+ (aq)

H2(g) + CuO(s) Cu(s) + H2O (aq)

Single Replacement (halogens)

F2(g) + Cl- (aq) Cl2(g) + F- (aq)

Oxidation-Reduction

Redox in an Acid Environment

Cr2O72- + Fe2+ + H+ Cr3+ + Fe3+ + H2O

Cr2O72- + I- + H+ Cr3+ + I2

+ H2O

MnO4- + Cl- + H+ Mn2+ + Cl2

+ H2O

H2O2 + I- + H+ H2O + I2 + H2O

Oxidation-Reduction

Redox in a Basic Environment

H2O2 (aq) + MnO4- O2 + MnO2(s) + H2O

Oxidation-Reduction

Important Oxidizers

MnO4- in acidic solution

Mn2+

Formed in the Reaction

MnO2 in acidic solution

Mn2+

MnO4- in basic solution

MnO2

Cr2O72- in acidic solution

Cr3+

HNO3, concentrated

NO2

HNO3, dilute NO

H2SO4, hot SO2

Oxidation-Reduction

Important Oxidizers Formed in the Reaction

Metal-ic ions Metal-ous ions

Free halogens halide ionsNa2O2 NaOH

HClO4 Cl-

H2O2 (in acidic sol’n)

H2O

H2O2 (in basic sol’n)

OH-

Important Reducers Formed in the Reaction

Halide ions Free halogens

Oxidation-Reduction

Free metals Metal ions

Sulfite ions (or SO2)

Sulfate ions

Nitrite ions

Nitrate ions Free Halogens (dil., basic)

Hypohalides (e.g. ClO-) Free Halogens (conc., basic) Halate ions (e.g. ClO3

-) Metal-ous Metal-ic

H2O2 O2