Acids Formation

Naming "non-acids"

Naming ionic "non-acid" names are similar to naming other ionic compounds.

Step 1: First name the positive ion (typically a metal).
Step 2: Now name the negative ion (typically a non-metal).
Step 3: Change the ending of the negative ion to "-ide"

Note that the total charge on a compound must always be zero.

Some examples are: NaCl, K₂S; Sodium Chloride, Potassium Sulphide.

Naming simple acids

Simple acids are solutions of hydrogen bonded with non-metals from group 16 and 17 on the Periodic Table.

Step 1: Place the prefix "hydro" at the beginning of the name

Step 2: The name of the non-metal follows and its ending is to be substituted  to "ic"
            - E.g. S- sulphur will be become sulphuric.

Step 3: Lastly, the word acid is added to the very end.

Some examples of simple acids are listed below,

Formula                       Non-metal Names                        Acid Names

HBr                             hydrogen bromide                     hydrobromic acid

HI                               hydrogen iodide                         hyrdroiodic acid

HF                              hydrogen fluoride                       hydrofluoric acid

Naming Complex Acids

Complex acids are defined as solutions of hydrogen bonded with a poly-atomic ion that's negatively charged.

Step 1: The word or prefix of "hydrogen" or "hydro" is taken away in this type of naming.

Step 2: If the negatively charged poly-atomic ion name ends in the following suffix, it must be changed accordingly as shown below,

            "-ate"  →  "-ic"             E.g.  Chromate →Chromic

            "-ite"   →  "-ous"          E.g.  Nitrite →Nitrous

Step 3: Now, the word acid is placed at the end.

Some of the examples of complex acids are listed below,

Formula Name                        Acid Name

H₃PO₄                                 phosphoric acid

HNO₃                                     nitric acid

H₂SO₄                                sulphurous acid

Law of Definite Composition (Proust's Law)

• Every chemical compound always contain a fixed proportion of its composite elements by mass
• For instance, CO₂(carbon dioxide) has 1 atom of C(carbon) and 2 atoms of  O(oxygen). The total mass of CO₂ is 44g (C=12g, and 2xO=2x16g=32g) which would apply anywhere in the universe.

Law of Multiple Proportion (Dalton's Law)

• Two or elements can be bonded differently to form multiple compounds where the ratios of the composite masses are different. 
• For example, the elements of C(carbon) and O(oxygen) may bond to form CO compound (C:O=3:4) and CO₂ compound (C:O=3:8)