Chemical formula and equations

Ionic compounds that are insoluble in water, consequently, not very basic.
Formula Name
Cu(OH)2 copper (II) hydroxide
Fe(OH)2 iron (II) hydroxide
Fe(OH)3 iron (III) hydroxide
Zn(OH)2 zinc (II) hydroxide
Mg(OH)2 magnesium hydroxide

Formula Name
LiOH lithium hydroxide
NaOH sodium hydroxide
KOH potassium hydroxide
RbOH rubidium hydroxide
CsOH cesium hydroxide
Ca(OH)2 calcium hydroxide
Sr(OH)2 strontium hydroxide
Ba(OH)2 barium hydroxide
Notice that they are all hydroxides of IA and IIA metals

Formula Name
HF hydrofluoric acid
CH3COOH acetic acid (vinegar)
HCN hydrocyanic acid
HNO2 nitrous acid
H2CO3 carbonic acid (soda water)
H2SO3 sulfurous acid
H3PO4 phosphoric acid
(COOH)2 oxalic acid

Acid Anion Name
HF F- fluoride ion
CH3COOH CH3COO- acetate ion
HCN CN- cyanide ion
HNO2 NO2- nitrite ion
H2CO3 CO32- carbonate ion
H2SO3 SO32- sulfite ion
H3PO4 PO43- phosphate ion
(COOH)2 (COO)22- oxalate ion

Formula Name
HCl hydrochloric acid
HBr hydrobromic acid
HI hydroiodic acid
HNO3 nitric acid
H2SO4 sulfuric acid
HClO3 chloric acid
HClO4 perchloric acid

Acid Anion Name
HCl Cl- chloride ion
HBr Br- bromide ion
HI I- iodide ion
HNO3 NO3- nitrate ion
H2SO4 SO42- sulfate ion
HClO3 ClO3- chlorate ion
HClO4 ClO4- perchlorate ion

Outer shells contain four or more electrons
Form anions by gaining electrons
Form ionic compounds with metals and covalent compounds with other nonmetals
Form covalently bonded molecules; noble gases are monatomic

CO2 H2O

CH4 HF

Na + Br-

NH4 + SO4 2- SO3 2-

MnO4 - BrO3 -

Electron Transfer Reactions:
Oxidation-reduction (also called redox) reactions have been shown earlier.
Combination:
C + O2 => CO2
Single replacement:
C + Fe2O3 => Fe + CO2
Decomposition
NaNO3 => NaNO2 + O2

Inorganic
Acids – HF, HBr, HI, HCl, HNO3 & H2SO4
Bases – LiOH, NaOH, KOH, Ca(OH)2 Ba(OH)2
Organic
Acids – have COOH group, acetic acid CH3COOH
Bases – contain nitrogen and are called amines, methylamine CH3NH2

All carbonates(CO32-), chromates(CrO4 2- ) and phosphates(PO4 3- ) are insoluble except ammonium and alkali elements.
All hydroxides (OH-) are insoluble except those of alkali elements, ammonium ions, except Sr2+ , Ba2+ and Ca2+
All metal sulfides (S 2- ) are insoluble except those of alkali elements and ammonium ions

All ionic compounds of alkali elements (lithium, sodium, potassium, rubidium & cesium) and ammonium ions are soluble.
All nitrates, chlorates and perchlorates are soluble.
Chlorides, bromides and iodides are soluble except Pb2+, Ag+ & Hg22+
All sulfates are soluble except Sr2+ , Ba2+ Pb2+ and Hg22+

**Single Replacement Reactions
an element is substituted into a compound for another element in the compound:
A + BY => AY + B
Example: the reduction of metal oxides with carbon

**Double Replacement Reactions
two compounds exchange atoms or groups of atoms to produce two different compounds:
AX + BY => AY + BX

Example: the reaction of a metal carbonate with an acid
Precipitation
two soluble ionic compounds form an insoluble product, a precipitate, when mixed based

on

AX (aq) + BY (aq) => AY (s) + BX (aq)

AX (s) + H2O (l) => A+ (aq) + X- (aq)

BY (s) + H2O (l) => B+ (aq) + Y- (aq)

Identify an element that appears in only one substance on each side of the equation.
If several atoms satisfy this condition, select the substance that has the largest

number of atoms of a single element.
Balance the number of atoms of that element by placing the proper coefficients in front

of each substance with that element on each side of the equation.
Balance atoms of other elements by the same process.
Next, balance atoms that appear in two or more places.
Examples of Balancing Equations:
-Nitrogen and hydrogen react to form ammonia
-Aluminum hydroxide reacts with sulfuric acid to yield aluminum sulfate and water

1869 - Mendeleev & Meyer
Discovered the periodic law
The properties of the elements are periodic functions of their atomic numbers.
Groups or families
Vertical group of elements on periodic table
Similar chemical and physical properties
Some chemical properties of metals
Outer shells contain few electrons
Form cations by losing electrons
Form ionic compounds with nonmetals
Solid state characterized by metallic bonding