Wize High School Grade 11 Chemistry Textbook > Properties of Matter

Naming Ionic Compounds
Naming Binary Ionic Compounds
Binary ionic compounds are composed of a monoatomic cation and a monoatomic anion
Example: NaCl is made up of Na+ cations and Cl- anions
To name a binary ionic compounds. first name the metal cation, followed by the base name of the non-metal anion with the ending -ide. Subscripts in the formula do not affect the name
Example: MgO  magnesium oxide
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Naming Binary Ionic Compounds with Multivalent Cations
Transition metals could form different charged ions. These atoms are known as multivalent atoms. You have to indicate the charge when naming the compound
AtomIonsCr3+6+Mn2+4+7+Fe2+3+Co2+3+\small \def\arraystretch{1.5}
   \begin{array}{c:c}
   \text {Atom} & \text {Ions} \\ \hline
   Cr & 3+ & 6+\\
Mn &2+&4+&7+\\
Fe &2+&3+\\
Co &2+&3+
\end{array}AtomCrMnFeCo​Ions3+2+2+2+​6+4+3+3+​7+​​
To name this type of ionic compounds, first name the metal cation, followed by the ion charge in roman numerals in parenthesis then the base name of the non-metal anion with the ending -ide
Example: Fe2O3 is iron (III) oxide

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Naming Ionic Compounds with Polyatomic Ions
Naming ionic compounds that contain polyatomic ions are very similar to the naming of binary ionic compounds.  First name the cation, followed by the base name of the anion. Subscripts in the formula do not affect the name
Example: NaNO3 is sodium nitrate
	\footnotesize IonNameIonNameIonNameNH4+ammoniumOH−hydroxideCN−cyanideSO42−sulfateO22−peroxideCNO−cyanateHSO4−bisulfateCH3COO−acetateSCN−thiocyanateSO32−sulfiteCℓO4−perchlorateCO32−carbonateNO3−nitrateCℓO3−chlorateHCO3−bicarbonateNO2−nitriteCℓO2−chloriteOOCOO2−oxalatePO43−phosphate ionCℓO−hypochlorite ionS2O32−thiosulfateHPO42−hydrogen phosphateCrO42−chromateHg22+mercuryH2PO4−dihydrogen phosphateCr2O72−dichromate ionH3O+hydroniumPO33−phosphite ionMnO4−permanganate ionSiO32−silicate\small \def\arraystretch{1.5}
   \begin{array}{c:c||c:c||c:c}
\text {Ion} & \text{Name} &\text {Ion} & \text{Name} &\text {Ion} & \text{Name} \\ \hline
NH_4^+ & \text{ammonium} & OH^- & \text{hydroxide} & CN^- & \text{cyanide} \\

SO_4^{2-} & \text{sulfate} & O_2^{2-} & \text{peroxide} &CNO^-& \text{cyanate}\\

HSO_4^- & \text{bisulfate} &CH_3COO^-& \text{acetate} & SCN^- & \text{thiocyanate}\\

SO_3^{2-} & \text{sulfite}&C\ell O_4^- &\text{perchlorate}&CO_3^{2-}& \text{carbonate}\\

NO_3^- & \text{nitrate}&C\ell O_3^-&\text{chlorate}&HCO_3^-&\text{bicarbonate}\\

NO_2^-& \text{nitrite}&C\ell O_2^-&\text{chlorite}&OOCOO^{2-}&\text{oxalate}\\

PO_4^{3-}&\text{phosphate ion}&C\ell O^-&\text{hypochlorite ion}&S_2O_3^{2-}&\text{thiosulfate}\\

HPO_4^{2-}&\text{hydrogen phosphate}&CrO_4^{2-}&\text{chromate}&Hg_2^{2+}&\text{mercury}\\

H_2PO_4^-&\text{dihydrogen phosphate}&Cr_2O_7^{2-}&\text{dichromate ion}&H_3O^+&\text{hydronium}\\

PO_3^{3-}&\text{phosphite ion}&MnO_4^-&\text{permanganate ion}&SiO_3^{2-}&\text{silicate}\\
\end{array}IonNH4+​SO42−​HSO4−​SO32−​NO3−​NO2−​PO43−​HPO42−​H2​PO4−​PO33−​​Nameammoniumsulfatebisulfatesulfitenitratenitritephosphate ionhydrogen phosphatedihydrogen phosphatephosphite ion​IonOH−O22−​CH3​COO−CℓO4−​CℓO3−​CℓO2−​CℓO−CrO42−​Cr2​O72−​MnO4−​​Namehydroxideperoxideacetateperchloratechloratechloritehypochlorite ionchromatedichromate ionpermanganate ion​IonCN−CNO−SCN−CO32−​HCO3−​OOCOO2−S2​O32−​Hg22+​H3​O+SiO32−​​Namecyanidecyanatethiocyanatecarbonatebicarbonateoxalatethiosulfatemercuryhydroniumsilicate​​

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Naming Molecular Compounds
Covalent bonds are formed between two non-metals. The resulting compound is known as a molecular element or compound.
Molecular elements are named the same as the element itself
Example: O2 is oxygen
, H2 is hydrogen
Molecular compounds are usually written from least to most electronegative. 
To name a molecular compound:
Name the first element using the proper prefix (di, tri, etc.). If only one atom, avoid the prefix mono
Name the second element with the proper prefix (including mono) using the “ide” ending
Number  of  AtomsPrefixNumber  of  AtomsPrefix1mono-6hexa-2di-7hepta-3tri-8octa-4tetra-9nona-5penta-10deca-\small \def\arraystretch{1.5}
   \begin{array}{c:c||c:c}
 \text{Number \ of \ Atoms} &\text{Prefix} &\text {Number \ of \ Atoms} &\text{Prefix}\\ \hline
1 &\text{mono-}&6 &\text{hexa-} \\ \hline
2 &\text{di-} &7 &\text{hepta-} \\ \hline
3 &\text{tri-}&8 &\text{octa-} \\ \hline
4 &\text{tetra-} &9 &\text{nona-} \\ \hline
5 &\text{penta-} & 10 &\text{deca-} \\
 \end{array}Number  of  Atoms12345​Prefixmono-di-tri-tetra-penta-​Number  of  Atoms678910​Prefixhexa-hepta-octa-nona-deca-​​

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Example:
CO = carbon monoxide
CO2 = carbon dioxide
N2O4 = dinitrogen tetroxide 

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Naming Acids and Bases
Naming Acids without Oxygen
A binary acid is an acid that consists of hydrogen and one other element. 
To name a binary acid, start with the prefix hydro-, followed by the base name of the anion and the ending -ic then the word acid
Example: HCl is hydrochloric acid
Naming Acids with Oxygen
Acids that are made out of hydrogen, oxygen and a third element are known as oxyacids. The third element is usually a nonmetal.
If the anion has the -ite ending, the name of the acid is the root of the anion followed by the suffix -ous.
Example: HNO2 is nitrous acid
If the anion has the -ate ending, the name of the acid is the root of the anion followed by the suffix -ic. 
Example: HNO3 is nitric acid
Naming Bases
Most common bases are ionic hydroxides. Use the naming convention for ionic compounds with polyatomic ionds
Example: NaOH is sodium hydroxide

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Example: Providing Chemical Formulae for Ionic Compounds
Give a chemical formula for the following compounds:
a) Potassium fluoride

KF

b) Manganese(II) oxide

MnO

c) Ammonium sulfate

(NH4)2SO4

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Example: Naming Molecular Compounds
Name the following molecular compounds:

a) NF3

Nitrogen trifluoride

b) CCl4

Carbon tetrachloride

c) N2O

Dinitrogen monoxide

Practice: Naming Conventions
In naming a binary molecular compound, the number of atoms of each element present in the molecule is indicated by:

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Practice: Naming Compounds 
Name the following compounds.
KClO
BaOH
PCl3
FeO

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Practice: Determining Chemical Formulas based on Names
Write out the formula for the following. Make sure to use subscripts and brackets where appropriate.

magnesium hydroxide: 
sodium chromate: 
ammonium nitrate: 
iron (III) phosphate: 

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