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Abs Naming

The document discusses writing ionic formulas for salts, bases, and acids. For salts, the formula includes a positive ion and a negative ion. Simple salts follow the format of metal first then non-metal changing to "-ide". Multivalent salts indicate the metal's combining capacity in Roman numerals. Polyatomic ions are treated as single elements. Base formulas contain a positive ion and hydroxide. Acid formulas contain hydrogen and a negative ion, with names changing based on singular or polyatomic ions (dropping endings and adding prefixes/suffixes).

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168 views2 pages

Abs Naming

The document discusses writing ionic formulas for salts, bases, and acids. For salts, the formula includes a positive ion and a negative ion. Simple salts follow the format of metal first then non-metal changing to "-ide". Multivalent salts indicate the metal's combining capacity in Roman numerals. Polyatomic ions are treated as single elements. Base formulas contain a positive ion and hydroxide. Acid formulas contain hydrogen and a negative ion, with names changing based on singular or polyatomic ions (dropping endings and adding prefixes/suffixes).

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Writing Ionic Formulas

(Acids, Bases and Salts)

1. Salts

These formulas include a positive ion (other than hydrogen) and a negative ion (other
than hydroxide)
So far we have learned how to write formulas for three different kinds of salts.

A) Simple formulas

Tips: * Always write the metal first, then the non-metal


* Metal name doesn’t change
* Non-metal name changes to ____ide.

ex. NaCl sodium chloride


MgF2 magnesium fluoride

B) Multivalent

Tips: * Be able to recognize metals that are multivalent


(have more than one combining capacity)
* All of the multivalent metals you’ll need to know for your test can be
found in your data booklet
* The Roman numerals (in brackets) tell you the combining capacity of
the metal
* Follow the rules for writing simple formulas
* ALWAYS indicate which “form” of the metal you are using ie. Tin (II) or
Tin (IV)

ex. PbI4 lead (IV) iodide


Fe2O3 iron (III) oxide

C) Polyatomic Ions

Tips: * If there are more than two elements in a formula, you


are dealing with a polyatomic
* All of the polyatomics you need to know can be found in your data
booklet
* Treat a polyatomic as if it were a single element ion
* The name of the polyatomic doesn’t change

ex. Na HCO3 sodium bicarbonate


Mg(NO3)2 magnesium nitrate

Some formulas will include both multivalent metals and polyatomic ions

ex. CuClO3 copper (I) chlorate


HgSO4 mercury (II) sulphate
2. Bases

These formulas include a positive ion plus a hydroxide ion (OH-)

ex. NaOH sodium hydroxide


Ba(OH)2 barium hydroxide

3. Acids

These formulas include the hydrogen ion plus any negative ion

Naming acids depends on the kind of negative ion involved

A) Singular Negative Ions

* Drop the ending of the second element


* Add the prefix “hydro” and the suffix “ic”
* Ends with the word acid

ex. HCl hydrochloric acid


HF hydrofluoric acid

B) Negative Polyatomic Ions

* If the polyatomic ion has an “___ate” ending, drop the “ate” and add “ic”
ex. (hydrogen and sulphate)
H2SO4 sulphuric acid

* If the polyatomic has an “___ite” ending, drop the “ite” and add “ous”

ex. (hydrogen and nitrite)


HNO2 nitrous acid

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