Naming ChemicalsChapter 9

Naming and Writing Stuff Ions Ionic CompoundsMolecular CompoundsAcids and BasesFormulas and Names

MONATOMIC IONSCationsAnions

–ide

Ions of Transition Metals IRefer to the main 8 Groups we’ve seen as being in

set Group ARefer to the other Groups as being in set Group B If you look at your periodic tables, you should notice

that labelingThese are the transition metals

Ions of Transition Metals IIMany have multiple chargesException:

Silver Ag+

Cadmium Cd2+

Zinc Zn2+

Ions of Transition Metals IIIRoman numerals = valence e-

Go from low to high: (think Oh, I See - OIC)–ous –ic

POLYATOMIC IONS (More than one atom make up an ion) ALL are negatively charged

EXCEPT ammonium NH4+ and Hg2

2+

Sometimes Hydrogen @ the beginning:H+ ion presentWrite as “Hydrogen Something”

E.g. Hydrogen Phosphate HPO42-

Go from low to high (“I ate”)–ite–ate

BINARY IONIC COMPOUNDSAn Ionic Compound with 2 components to it

Components can be 2 AtomsMolecules

2 Essential Steps:1. Write the CATION, then ANION (go + -)

2. Balance the charges

Compounds with Polyatomic IonsSame process as with binary ionic compounds

Molecular CompoundsLook at the prefix to tell you how many atoms of that

element are in each molecule.

N2O – dinitrogen monoxide

CO – carbon monoxide

If the first atom is only 1, leave off the mono-

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ACIDS & BASES IaNormally, you have a compound that gets dissolved

in water.These can even be gasses

To indicate they are dissolved in water, we will note them as (aq)

(aq) is the abbreviation for aqueous

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ACIDS & BASES Ib Water dissolves itself and splits up into H+ and (OH-)

Nonmetals are usually anions (-), so they would want to be near a positively charged H+

Since we write the cation first, acids will begin with H

Metals are usually cations (+), so they would want to be near a negatively charged (OH-)

Since we write the anion last, bases will end with OH

So, in general, a nonmetal dissolved in water will form an acid A metal dissolved in water will form a base

ACIDS & BASES – Acids 1When the anion ends in –ide

Front of name gets: hydro-End of name gets: –icAdd: acid

HClhydrogen chloride (aq) Hydrochloric acid

ACIDS & BASES – Acids 2 If anion ends in –ite

Front drops hydrogen End gets –ous Add: acid

H2SO3

hydrogen sulfite (aq) sulfurous acid

If anion ends in –ate Front drops hydrogen End gets –ic Add: acid

HNO3

hydrogen nitrate (aq): nitric acid

Very similar to –ide, but no hydro-

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ACIDS & BASES – BasesBASES

End in Hydroxide (OH)NaOH – Sodium Hydroxide

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acids

IDEHCl hydrogen chlor ide

HCl (aq) hydro- chlor ic acid

hydrochloric acid

ITEH2SO3 hydrogen sulf ite

H2SO3 (aq)

sulf ous acid

sulfurous acid

ATEHNO3 hydrogen nitr ate

HNO3 (aq) nitr ic acid

nitric acid

bases

NaOH sodium hydroxide

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Last note… see pages 262, 277-278…Remember to flip the charges with the number of

atoms to balance compounds.Example: Fe3+ O2- Flip: Fe2O3

Charges: (3+)*2 + (2-)*3 = +6 + -6 = 0

Remember there is a very handy flowchart on pages 277-278 to help name chemicals given their formulas and vice-versa