There are five C6H14 isomers, shown below as abbreviated line

There are five C6H14 isomers, shown below as abbreviated line formulas (A through E):
Although these distinct compounds all have the same molecular formula, only one (A) can be called hexane. How
then are we to name the others?
(A) hexane
(B) 2-methylpentane
Name the following organic compounds according to IUPAC rules.
1. Draw graphical formulae for;
(i) 2-methylpropane
(ii) 2,2,6-trimethyloctane
2. Name;
(i) CH3C(CH3)2CH2CH3
3. Draw graphical formulae for;
(i) 4-methylhex-1-yne
(ii) 3,4-diethylhex-2-ene
4. Name;
(i) CH3CH2CH=CH2
(ii) CH3CH2CH(CH3)C≡CCH3
5. Draw graphical formulae for;
(i) triiodomethane
(ii) 1-bromo-3-chloro-4-methylhexane
6. Name;
7. Draw graphical formulae for;
(i) pentan-2-ol
(ii) cyclohexane-1,3-diol
8. Name;
(ii) CH3C(CH3)(OH)CH2CH3
9. Draw graphical formulae for;
(i) cyclohexanone
(ii) 3-chlorobutan-2-one
10. Name;
(ii) CH3CH(CH3)COCH3
11. Draw graphical formulae for;
(i) 3-aminopropanoic acid
(ii) chloroethanoic acid
12. Name;
(i) CH3CH2CO2H
propanoic acid
3-hydroxypentanoic acid
Summary of Reaction Predictions
Note: The following summary is not comprehensive. It is meant to be a simple and concise
prediction help.
Acid Base Reactions
A. HX + MOH → _____HM____________ + _____H2O____________
B. Remember: Weak acids and bases must be written in the NIE as _molecules______.
Precipitation Reactions
A. Generally both reactants are salts in solution:
AX + BY → ___AY (s)___________ + ______BX(aq)________
(Where AY and/or BX are salts in solution.)
B. Net Ionic Equation:
A+ + Y- → ___AY(s)______________
Hydrolysis Reactions
A. A metal oxide reacts with water to form a ___bases (metal hydroxides)__________.
B. A nonmetal oxide reacts with water to form an __acids________________.
C. A metal hydride reacts with water to form a ___base___________ and
__hydrogen gas______.
Decomposition Reactions
A. Occurs when a single reactant is __breaks up into two or more pieces____.
B. Metallic carbonates decompose to form a _metallic oxide___ and
_carbon dioxide gas__.
C. Metallic hydroxides decompose to form _metallic oxides__ and
D. Metallic chlorates decompose to form __metallic chlorides__ and
__oxygen gas___.
E. Metallic sulfates decompose to form __metallic oxides___ and
__sulfur trioxide gas____.
F. Some acids decompose to form __nonmetal oxides_____ and
G. Sulfurous acid decomposes in water to form ____sulfur dioxide____ and
H. Hydrogen peroxide decomposes to form ___water_______ and
__hydrogen gas____.
Ligand Reactions
A. Occur between the following metals:__ Fe, Cu, Pb, Ag, Au, Sn, Pt, Co, etc__.
and the following ligands: CN-, SCN-, NO2- , NH3, H2O, OH-, halides (F-, Cl-, Br-, I-)_.
B. To determine how many ligands to attach to a metal center usually
____double ______ the metal cation’s charge.
Redox Reactions
A. Metal and nonmetal react to form ___an ionic salt_____.
B. When a solid metal replaces the metal anion from a metallic compound it is
called a _single replacement reaction____,
C. A redox reaction occurs when a halogen replaces a___halide____ salt.
D. When MnO4- is placed in an acidic solution with a metal cation, the MnO4- is
reduced to ___Mn2+_____________; the metal in solution is oxidized.
E. When Cr2O72- is placed in acidic solution with a metal cation, the Cr2O72- is reduced
to __Cr3+______________; the metal in solution is oxidized.
F. Cu(s) + HNO3(dilute) → __Cu2+__ + ___NO___ + ____H2O____
Reaction Predictions Assignment
Write balanced net-ionic (only ions that participate in the reaction are shown) equations below.
1. A solution of potassium phosphate is mixed with a solution of calcium acetate.
2 PO43- + 3 Ca2+ → Ca3(PO4)2
2. A solution of hydrogen peroxide is exposed to strong sunlight.
2 H2O2 → H2O + O2
3. Solid sodium hydride is added to water
NaH + H2O → NaOH + H2
4. Propanone is burned in air.
C2H6O + 3 O2 → 2 CO2 + 3 H2O
5. A solution of sodium iodide is added to a solution of lead (II) acetate.
2 I- + Pb2+ → PbI2
6. Solid cesium oxide is added to water.
Cs2O + H2O → 2 CsOH
7. Solid zinc carbonate is added to 1.0 M sulfuric acid.
ZnCO3 + 2 H+ → Zn2+ + CO2 + H2O
8. Solid dinitrogen pentoxide is added to water.
N2O5 + H2O → 2 HNO3
9. Magnesium ribbon is burned in oxygen.
2 Mg + O2 → 2 MgO
10. Ammonia gas is mixed with hydrogen chloride gas.
NH3 + HCl → NH4Cl
11. Solid sodium acetate is added to 1.0 M hydrobromic acid.
NaC2H3O2 + H+ → Na+ HC2H3O2
12. A bar of strontium metal is immersed in a 1.0 M copper (II) nitrate solution.
Sr + Cu2+ → Sr2+ + Cu
13. Pure solid phosphorus is burned in air.
P4 + 5 O2 → P4O10
14. Sulfur trioxide gas is bubbled into water.
SO3 + H2O → H2SO4
15. Excess concentrated potassium hydroxide solution is added to a solution of nickel (II) chloride.
Ni2+ + 4 OH- → [Ni(OH)4]216. Excess concentrated aqueous ammonia is added to solid silver chloride.
AgCl + NH3 → [Ag(NH3)2]+ + Cl17. Hot hydrogen gas is passed over heated copper (II) oxide solid.
H2 + CuO → Cu H2O
18. A 0.02 M hydrochloric acid solution is mixed with an equal volume of a 0.01 M calcium
hydroxide solution.
H+ + OH- → H2O
19. Excess concentrated hydrochloric acid is added to a 1.0 M solution of cobalt (II) chloride.
Co2+ + 4 Cl- → [Co(Cl)4]220. Liquid bromine is carefully added to a solution of potassium iodide.
Br2 + 2 I- → 2 Br- I2