Nomenclature of inorganic Compounds

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1. NOMENCLATURE OF INORGANIC COMPOUNDS Submitted By : Darshan Kotadiya (16BCH028 ) Dhaval Bhimbha ( 16BCH008 ) Arpit Patel (16BCH038)

2. What is Inorganic Compound ? An  I norganic compound   is a  chemical compound that lacks C-H bonds. Inorganic compounds can be defined as any compound that is not organic compound . Ex: CaCl 2 NaCl

3.   IUPAC nomenclature of inorganic chemistry  is a systematic method of naming inorganic chemical compounds

4. Ionic Compounds Compounds made of a metal and non-metal are commonly known as Ionic Compounds. W here the compound name has an ending of  –ide .  Cations have positive charges while anions have negative charges . The net charge of any ionic compound must be zero which also means it must be electrically neutral.

5. These rules are for those cation having only one oxidation charge. There are two rules that must be followed through:    The   cation  (metal) is always named first with its name unchanged. The   anion  ( nonmetal ) is written after the cation , modified to end in – ide. Na +           +          Cl -               =              NaCl         Sodium      +     Chlorine       =       Sodium Chlor ide                           Ca 2 +        + 2Br -             =             CaBr 2         Calcium      +   Bromine       =       Calcium Brom ide

6. These are oxidation charges for some metal and non-metal. 1A 2A 3A 4A 5A 6A 7A 8A Li + Be + 2 N - 3 O - 2 F - Na + Mg + 2 Al + 3 P - 3 S - 2 Cl - K + Ca + 2 As - 3 Se - 2 Br - Rb + Sr + 2 I - Cs + Ba + 2

7. The  transition metals may form more than one ion, thus it is needed to be specified which particular ion we are talking about. This is indicated by assigning a Roman numeral after the metal. The Roman numeral denotes the charge and the oxidation state of the transition metal ion. For example, iron can form two common ions Fe 2+  would be named iron (II) and Fe 3+  would be named iron (III ). However, some of the transition metals charges have specific Latin names.

8. Instead of using Roman numerals, the different ions can also be presented in plain words. The metal is changed to end in  – ous  or  – ic . - ous  ending is used for the  lower  oxidation state - ic  ending is used for the  higher  oxidation state C u + cupr ous ion Fe 2+ ferro us ion C u 2 + cupr ic ion Fe 3+ ferr ic ion

9. Formulas and names of common metal ions with more than one ionic charge. Formula S t o c k Name Classical Name Cu + Copper (I) ion Cuprous ion Cu 2+ Copper (II) ion Cupric ion Fe 2+ Iron (II) ion Ferrous ion Fe 3+ Iron (III) ion Ferric ion Hg + Mercury (I) ion Mercurous ion Hg 2 + Mercury (II) ion Mercuric ion Pb 2+ Lead (II) ion Plumbous ion Pb 4+ Lead (IV) ion Plumbic ion Sn 2+ Tin (II) ion Stannous ion Sn 4+ Tin (IV) ion Stannic ion Cr 2+ Chromium (II) ion Chromous ion Cr 3+ Chromium (III) ion Chromic ion Mn 2+ Manganese (II) ion Manganous ion Mn 3+ Manganese (III) ion Manganic ion C o 2 C o 3 Cobalt (II) ion Cobalt (III) ion Cobaltous ion Cobaltic ion

10. Names of ionic compounds consist of the cation name followed by the anion name. CaCl 2 Calcium chloride Al(NO 3 ) 3 Aluminum nitrate

11. However, this  - ous /- ic  system is inadequate in some cases, so the Roman numeral system is preferred. This method is used commonly in naming acids, where H 2 SO 4  is commonly known as Sulfuric Acid, and H 2 SO 3  is known as Sulfurous Acid. EXAMPLE Compound Cu 2 O CuO FeCl 2 FeCl 3 Charge Charge of copper is +1 Charge of copper is +2 Charge of iron is +2 Charge of iron is +3 Nomenclature Cupr ous  Oxide Cupr ic  Oxide Ferr ous  Chloride Ferr ic  Chloride

12. Polyatomic Ion Polyatomic (many-atoms) anions containing oxygen have names ending in –ate or – ite These are called oxyanions -ate is used for the most common oxyanion of an element - ite is used for an oxyanion that has the same charge but one less O atoms NO 3 - Nitr ate ion SO 4 2- Sulf ate ion NO 2 - Nitr ite ion SO 3 2- Sulf ite ion

13. Some nonmetals form a series of polyatomic ions with oxygen (all having the same charge ) The   -ate  forms (formula and charge) must be memorized.   In some cases, the  - ate  form has three oxygens , and in some cases four oxygens . The  - ite  form has one less oxygen that the  -ate  form. The  hypo-  stem  - ite  form has two less oxygens than the  -ate  form. The  per-  stem  -ate  form has one more oxygen than the  -ate  form. The  -ide  form is the monatomic anion  Formula Name XO n y - stem +  -ate XO n-1 y- stem +  - ite XO n-2 y- hypo-  + stem +  - ite XO n+1 y- per-  + stem +  -ate X y- stem +  -ide Examples SO 4 2- sulfate SO 3 2- sulfite SO 2 2- hyposulfite SO 5 2- persulfate S 2- sulfide

14. Name: Cation   Anion Formula Ammonium ion NH 4 + Hydronium ion H 3 O + Acetate ion C 2 H 3 O 2 - Arsenate ion AsO 4 3- Carbonate ion CO 3 2- Hypochlorite ion ClO - Chlorite ion ClO 2 - Chlorate ion ClO 3 - Perchlorate ion ClO 4 - Chromate ion CrO 4 2- Dichromate ion Cr 2 O 7 2- Cyanide ion CN - Hydroxide ion OH - Nitrite ion NO 2 - Nitrate ion NO 3 - Oxalate ion C 2 O 4 2- Permanganate ion MnO 4 - Phosphate ion PO 4 3- Sulfite ion SO 3 2- Sulfate ion SO 4 2- Thiocyanate ion SCN - Thiosulfate ion S 2 O 3 2- Name: Cation   Anion Formula Ammonium ion NH 4 + Hydronium ion H 3 O + Acetate ion C 2 H 3 O 2 - Arsenate ion AsO 4 3- Carbonate ion CO 3 2- Hypochlorite ion ClO - Chlorite ion ClO 2 - Chlorate ion ClO 3 - Perchlorate ion ClO 4 - Chromate ion CrO 4 2- Dichromate ion Cr 2 O 7 2- Cyanide ion CN - Hydroxide ion OH - Nitrite ion NO 2 - Nitrate ion NO 3 - Oxalate ion C 2 O 4 2- Permanganate ion MnO 4 - Phosphate ion PO 4 3- Sulfite ion SO 3 2- Sulfate ion SO 4 2- Thiocyanate ion SCN - Thiosulfate ion S 2 O 3 2-

15. To combine the topic of acids and polyatomic ions, there is nomenclature of aqueous acids. Such acids include sulfuric acid (H 2 SO 4 ) or carbonic acid (H 2 CO 3 ). To name them, follow these quick, simple rules : If the ion ends in  -ate  and is added with an acid, the acid name will have an  - ic  ending. Examples : nitrate ion (NO 3 - ) + H +  (denoting formation of acid) = nitr ic  acid (HNO 3 ) If the ion ends in  - ite  and is added with an acid, then the acid name will have an  - ous  ending. Example : nitrite ion (NO 2 - ) + H +  (denoting formation of acid) = nitr ous  acid (HNO 2 )

16. Binary Acids An  acid  is a substance that dissociates into hydrogen ions (H + ) and anions  in water . A quick way to identify acids is to see if there is an H (denoting hydrogen) in front of the molecular formula of the compound. To name acids, the prefix  hydro-  is placed in front of the nonmetal modified to end with  – ic . The state of acids is aqueous ( aq ) because acids are found in water.

17. It is important to include ( aq ) after the acids because the same compounds can be written in gas phase with hydrogen named first followed by the anion ending with  –ide . Some common binary acids include : HF (g) = hydrogen fluor ide        -->     HF ( aq ) =  hydro fluor ic   acid HBr (g) = hydrogen brom ide     -->     HBr ( aq ) =  hydro brom ic   acid HCl (g) = hydrogen chlor ide      -->     HCl ( aq ) =  hydro chlor ic   acid H 2 S (g) = hydrogen sulf ide       -->     H 2 S ( aq ) =  hydro sulfur ic acid

18. Anions whose name ends in –ate have associated acids with an – ic ending. Anions whose name ends in – ite have associated acids with an – ous ending . Prefixes in the name of the anion are retained in the name of the acid . ClO - Hypochlor ite ion HClO hypochlor ous acid ClO 2 - Chlor ite ion HClO 2 chlor ous acid ClO 3 - Chlor ate ion HClO 3 chlor ic acid ClO 4 - Perchlor ate ion HClO 4 perchlor ic acid

19. Compounds between Nonmetals and Nonmetals Compounds that consist of a nonmetal bonded to a nonmetal are commonly known as  Molecular Compounds , where the element with the positive oxidation state is written first.   In many cases, nonmetals form more than one binary compound, so  prefixes  are used to distinguish them .

20. EXAMPLE CO = carbon  mon oxide                      BCl 3  = boron tri chloride CO 2  = carbon  di oxide              N 2 O 4 = di nitrogen tetr oxide       N 2 O 5   = di nitrogen   pent oxide The prefix   mono-  is not used for the first element. If there is not a prefix before the first element, it is assumed that there is only one atom of that element.

21. Exercise Name of the following compunds : CuS K 3 N SnCl 2 K 2 S CaI 2 NaI

22. CuS Copper (II) sulfide K 3 N Potassium Nitride SnCl 2 Tin (II) chloride K 2 S Potassium sulfide CaI 2 Calcium Iodide NaI Sodium Iodide