Cheat sheets for nomenclature PDF

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Summary

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Description

Covalent=electrons shared=molecular compounds • Usually formed with other nonmetal atoms • Non-polar 1.7 Metal is always the cation (gives the electron)* -i.e. Na, Mg, Fe or the cationic polyatomic ion (NH4+) Nonmetal is always the anion (gets the electron)* Ionic compounds are neutral overall For dipoles to cancel, they need go in the same direction, angle, and intensity.

Monoatomic ionic

Ionic compound composed of only atomic ions (i.e., not polyatomic)

Naming the anion:

Polyatomic ionic

Name of nonmetal (anion) with suffix ide (e.g. fluoride, chloride, nitride).

Polyatomic ions are named as is, have an overall charge, cation naming is the same as monoatomic ions, and it does NOT use prefixes.

i.e. LiCl, MgO, FeCl3

Covalent/Molecular Compounds

Nomenclature Prefixes used for covalent 1: mono2: di3: tri-

Ionic hydrates

Ionic compound is named by its cation and then its anion. Roman numberals show the oxidation number, but in simple ionic compounds, it will be the metal's ionic charge.

Ionic compounds that contain water molecules as an integral part of their crystals *Water molecules don't get a charge and don't contribute to ionic charges*

4: tetra5: penta

Naming the cation: •1. Name of the metal (cation) unchanged •*If transition metal (d or f block), indicate charge with Roman numberals in parentheses

Transition Metals

6: hexa7:hepta 8: octaDo not use numeric prefixes or change the cation name

9: nona10: deca-

Mercury (I) is an exception--Never Hg+, always Hg22+

Ionic formula [bullet operator] #H2O E.g., CuSO4∙5H2O = copper(II) sulfate pentahydrate

•

ammonia - NH3

+

• • • • • •

ammonium - NH4 Hypobromite—BrOBromite—BrO2Bromate—BrO3Perbromate—BrO42carbonate - CO3

• • • •

bicarbonate - HCO3 carbonic acid - H2CO3 Hypochlorite—ClOchlorite - ClO2

• • • • • • • • • • • • • • • •

chlorate - ClO3 Perchlorate—ClO4Hypochlorous acid--HClO Hypofluorite—FOFluorite—FO2Fluorate—FO3Perfluorate—FO4Hypoiodite—IOIodite—IO2Iodate – IO3Periodate—IO4Hydronium—H3O+ Hydroxide—OHPeroxide—O22nitrite - NO2 Nitrous acid - HNO2

• •

• •

dihydrogen phosphate - H2PO4 phosphoric acid - H3PO4

• •

sulfite - SO3 sulfurous acid - H2SO3

• •

sulfate - SO4 sulfuric acid - H2SO4

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2-

2-

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Key Hypo-: Loses an oxygen atom Per-: Gains an oxygen atom -Ite: Will most of the time be an O2 atom with a single negative charge 2• Exceptions: sulfite - SO3 , -ate: Will most of the time be an O3 atom with a single negative charge 23• Exceptions: sulfate - SO4 , phosphate - PO4 , &

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2-

carbonate - CO3 -ous: adds an H Bi, Hydrogen, hydro-,hydra-: has H Dihydrogen: has H2 -ic: adds an H and gives the polyatomic charge to the H; for nonmetals Oxyacids: acid that has O, H, and other element Oxyanions: Have an O atom and a charge

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• •

nitrate - NO3 Nitric acid - HNO3 phosphite—PO333phosphate - PO4

•

hydrogen phosphate - HPO4

2-...