Unit 3. Inorganic formulation

Unit 3. Inorganic formulation Index 1. Stoichometric names of binary compounds...2 1.1.. With multiplying prefix...2 1.2.- With oxidation numbers...3 1.3.- With charge number...4 Binary or Non-oxygen Acids...5 2. Ternary compounds...6 2.1 Hydroxides...6 2.2 Oxyacids...8 2.2.1. Common nomenclature...8 2.2.2.The additive names...9 2.2.3 The hydrogen names...9 2.3 Oxysalts...12 2.2.1.Common name...12 2.2.2.The additive names and stoichometric name...13 Practice exam...18 Periodic Table with Oxidation Numbers. Table III...19 Page 1 of 19

1. Stoichometric names of binary compounds 1.1.. With multiplying prefix When constructing a stoichiometric name for a binary compound, one element is designated as the electropositive constituent and the other the electronegative constituent. The electropositive constituent is by convention the element that occurs last in the sequence of Table I and its name is the unmodified element name. The name of the electronegative constituent is constructed by modifying the element name with the ending ide, The stoichiometric name of the compound is then formed by combining the name of the electropositive constituent, cited first, with that of the electronegative constituent, both suitably qualified by any necessary multiplicative prefixes (Table II) The multiplicative prefixes precede the names they multiply, and are joined directly to them without spaces or hyphens. The final vowels of multiplicative prefixes should not be elided (although monoxide, rather than monooxide,is an allowed exception because of general usage). The two parts of the name are separated by a space in English. Prefix + name of 1st element in the formula Prefix + stem of 2nd element + ide Table I Table II--Prefixes for number of atoms Number of atoms Prefix 1 mon 2 di 3 tri 4 tetra or tetr* 5 penta or pent* 6 hexa or hex* 7 hepta or hept* *The first spelling is used if the stem of the element begins with a consonant and the second spelling if the Page 2 of 19

stem of the element begins with a vowel. The stem of an element is formed by dropping the last syllable of the element's name. Prefixes are assigned by the number of atoms of each element in the formula, and the prefix corresponding to a given number of atoms can be found Table II. The prefix "mon" is dropped with the exception of carbon monoxide, and the suffix "ide" is used with all two element compounds. Carbon dioxide is a familiar example of a systematic name. Example 1--What is the formula of sulfur hexafluoride? The elements composing the compound are S and F. Also the prefix hex says there are 6 F atoms so the formula is SF 6. Example 2--Name the compound N 2 O 4 The name is dinitrogen tetroxide. 1.2.- With oxidation numbers When constructing a stoichiometric name for a binary compound, one element is designated as the electropositive constituent and the other the electronegative constituent. The electropositive constituent is by convention the element that occurs last in the sequence of Table I and its name is the unmodified element name. The name of the electronegative constituent is constructed by modifying the element name with the ending ide, The electropositive constituent, cited first, is followed by a roman numeral between parentheses, just in the case that this element has more than one oxidation number in the table III. The two parts of the name are separated by a space in English. Name the electropositive element (roman numerals if they have more than one) followed by the stem name of the electronegative with an -ide ending. Examples: NaCl = sodium chloride SO 3 = sulfur(vi) oxide CaO = calcium oxide CaF 2 = calcium fluoride CuO = copper(ii) oxide If you know the name and you want to write the formula then it is more complex. This system does not use prefixes and assumes a knowledge of the law of electrical neutrality, the octet rule, and ionic theory. It will be very helpful use the table III of the oxidation numbers. Example 2- What is the chemical formula of cesium sulfide? The compound is composed of cesium and sulfur. From Table, we have Cs has + 1 S has - 2 Note the ions composing cesium sulfide are Cs + and S 2. Cs 2 S. Page 3 of 19

If the metal exhibits more than one oxidation state, the oxidation state of the metal, in the compound of interest, is indicated by a Roman numeral placed in parentheses following the name of the metal. The Roman numeral equals the charge on the metal ion. The following examples show how the names in these compounds are assigned and used to determine the chemical formula from the name. Example 1--The color of ruby and sapphire is due to a small quantity of Cr 2 O 3 in these gem stones. What is the systematic name of Cr 2 O 3? The name of the compound is Chromium(III) oxide. Example 2--The compound Lead(IV) oxide is used in car batteries. What is the chemical formula of Lead(IV) oxide? Pb has + 4 (from Lead(IV)) O has -2 (from Table III) The chemical formula is PbO 2. Example 3.- What is the name of HgBr? Bromine has number -1 (the last element always with the negative oxidation number)(see table III) mercury can have oxidation numbers of and. All the compounds are neutral so the oxidation number of mercury has to be It is named mercury(i) bromide For similar reasons HgBr 2 is named mercury(ii) bromide 1.3.- With charge number When constructing a stoichiometric name for a binary compound, one element is designated as the electropositive constituent and the other the electronegative constituent. The electropositive constituent is by convention the element that occurs last in the sequence of Table I and its name is the unmodified element name. The name of the electronegative constituent is constructed by modifying the element name with the ending ide, The electropositive constituent, cited first, is followed by an Arabic number and a plus sign (+) between parentheses, just in the case that this element has more than one oxidation number in the table III. The two parts of the name are separated by a space in English. Name the electropositive element (Arabic numbers (+)if they have more than one) followed by the stem name of the electronegative with an -ide ending. Examples: NaCl = sodium chloride Page 4 of 19

CaO = calcium oxide CaF 2 = calcium fluoride CuO = copper(2+) oxide If you know the name and you want to write the formula then it is more complex. This system does not use prefixes and assumes a knowledge of the law of electrical neutrality, the octet rule, and ionic theory. It will be very helpful use the table III of the oxidation numbers. Example 1--The color of ruby and sapphire is due to a small quantity of Cr 2 O 3 in these gem stones. What is the systematic name of Cr 2 O 3? The name of the compound is Chromium(3+) oxide. Example 2--The compound Lead(4+) oxide is used in car batteries. What is the chemical formula of Lead(4+) oxide? Pb has + 4 (from Lead(4+)) O has -2 (from Table III) The chemical formula is PbO 2. Example 3.- What is the name of HgBr? Bromine has number -1 (the last element always with the negative oxidation number)(see table III) mercury can have oxidation numbers of and. All the compounds are neutral so the oxidation number of mercury has to be It is named mercury(1+) bromide For similar reasons HgBr 2 is named mercury(2+) bromide Some binary compounds have an special and traditional name and this is the name that we usually are going to use. O NH 3 CH 4 water ammonia methane Binary or Non-oxygen Acids Binary acids consist of hydrogen combined with an element of the groups VI or VII. Binary acids are named by using the prefix hydro- followed by the stem name of the non-metal element (the second element in the formula) with an -ic ending. The name is followed by the word acid. Examples: HCl is named hydrochloric acid HBr is named hydrobromic acid HI is named hydroiodic acid S is named hydrosulfuric acid Page 5 of 19

2. Ternary compounds 2.1 Hydroxides Bases are compounds which consist of a metal ion combined with the hydroxide polyatomic ion (OH). To name a base, name the metal (include the oxidation number in parentheses if the metal is one which has more than one oxidation state) followed by the word hydroxide. Or you can use multiplying prefix Examples: NaOH is named sodium hydroxide Ba(OH) 2 is named barium hydroxide or barium dihydroxide Fe(OH) 2 is named iron(ii) hydroxide or iron dihydroxide Fe(OH) 3 is named iron(iii) hydroxide or iron trihydroxide Chemistry exercises on Inorganic Nomenclature 1. Name the following a) SO 3 b) CO 2 c) O 5 Cl 2 d) O 7 Br 2 e) OI 2 f) SO 2 g) N 2 O h) P 2 O 5 2. Write the formula for: a) phosphorus pentachloride b) carbon monoxide c) dinitrogen trioxide d) phosphorus trichloride e) heptoxygen dichloride f) palladium dioxide g) sulfur trioxide h) diphosphorus pentoxide 3. Name the following a)asf 3 b)al 2 S 3 c)pbo 2 Page 6 of 19

d)cocl 2 e) CuO 4. Write the formula for a)gold(iii) chloride b)strontium fluoride c)sodium oxide d) Dinitrogen pentoxide e)potassium sulfide 5. Write the chemical formula a) nickel (III) sulfide b) carbon dioxide c) sodium chloride d) silver iodide e) calcium oxide f) mercury(i) bromide g) cobalt(ii) chloride h) iron(iii) chloride 6. Name the following: a) Mg(OH) 2 b) Sn(OH)2 c) NaOH d) Ni(OH)3 e) Pb(OH)4 7. Write the chemical formula a) copper(ii) hydroxide b) silver hydroxide c) cadmium hydroxide d) tin(ii) hydroxide e) mercury(i) hydroxide 8. Write the chemical formula: a) ammonia b) water Page 7 of 19

c) methane d) hydrochloric acis e) hydrosulfuric acid 9 Write the name of the following: a) HBr b) HI c) H2S d) NH3 2.2 Oxyacids 2.2.1. Common nomenclature. To formulate these compounds need to know the oxidation numbers of nonmetal X. They are as follows Halogens,, +5, +7 Chalcogens, +6 Group of N, +5 Group of C The oxidation number of X shown by some prefixes and suffixes. Oxidation numbers Highest High Low Lowest Acid per- -ic -ic -ous hypo- -ous In the formula: Deduce the oxidation number of the central element, Hydrogen oxidation number and oxygen -2 and all the molecules are neutral, and as (highest, high, low or lowest) we termination appropriate (per- -ic, -ic, ous- or hypo- -ous). HClO 3 chloric acid In the name: Based on the prefixes and suffixes deduce the oxidation number of the central element. Hydrogen oxidation number and oxygen -2. We look after coefficients so that the Page 8 of 19

charge provided by the oxygens is equal and opposite to that provided by the hydrogens and the central element. 2.2.2.The additive names Sulfuric acid SO 4 The additive names are based on the structure of the acid, naming differently the oxygen that are tied to the acid hydrogens (hydroxido), and the oxygen only united central element (oxido). These names carry prefixes corresponding di-, tri-, tetra- and so on. And are named in alphabetical order followed by the name of the central atom. Prefix-hydroxido-prefix-oxido-CENTRAL ELEMENT HClO 3 ClO 2 (OH) hydroxidodioxidochlorine 2.2.3 The hydrogen names The hydrogen names are formed by the word "hydrogen" with the prefix that shows us the number of atoms of hydrogen, between brackets the word "oxido" with the prefix that shows us the number of atoms of oxygen, followed by the central atom finished -ate. Prefix-hydrogen(Prefix-oxido-CENTRAL ELEMENT-ate) HClO 3 hydrogen(trioxidochlorate) Activity 9. Formula Structural formula Additive names Hydrogen names HClO Cl(OH) hydroxidochlorine hydrogen(oxidochlorate) HClO 2 ClO(OH) hydroxidooxidochlorine hydrogen(dioxidochlorate) HClO 3 ClO 2 (OH) hydroxidodioxidochlorine hydrogen(trioxidochlorate) HClO 4 ClO 3 (OH) hydroxidotrioxidochlorine hydrogen(tetraoxidochlorate) SO 3 SO(OH) 2 dihydroxidooxidosulfur dihydrogen(trioxidosulfate) SO 4 SO 2 (OH) 2 dihydroxidodioxidosulfur dihydrogen(tetraoxidosulfate) HNO 2 NO(OH) hydroxidooxidonitrogen hydrogen(dioxidonitrate) HNO 3 NO 2 (OH) hydroxidodioxidonitrogen hydrogen(trioxidonitrate) H 3 PO 3 P(OH) 3 trihydroxidophosphorus trihydrogen(trioxidophosphate) Page 9 of 19

H 3 PO 4 PO(OH) 3 trihydroxidooxidophosphorus trihydrogen(tetraoxidophosphate) CO 3 CO(OH) 2 dihydroxidooxidocarbon dihydrogen(trioxidocarbonate) H 4 SiO 4 Si(OH) 4 tetrahydroxidosilicon tetrahydrogen(tetraoxidosilicate) CrO 4 CrO 2 (OH) 2 dihydroxidodioxidochromium dihydrogen(tetraoxidochromate) Cr 2 O 7 (HO)Cr(O) 2 OCr(O) 2 ( OH) μ-oxidobis(hydroxidodioxidochromium) dihydrogen(heptaoxidodichromate) MnO 4 MnO 2 (OH) 2 dihydroxidodioxidomanganese dihydrogen(tetraoxidomanganate) HMnO 4 MnO 3 (OH) hydroxidotrioxidomanganese hydrogen(tetraoxidomanganate) 10. Write the three names HNO 3 HClO SO 4 CO 3 HIO 4 HMnO 4 SeO 3 H 3 PO 4 Cr 2 O 7 HClO 2 11. Write the formula Chloric acid Sulfuric acid Phosphoric acid Carbonic acid Periodic acid Sulfurous acid Silicic acid Hypobromous acid Page 10 of 19

Arsenous acid Permanganic acid 12. Write the formula Hydrogen(trioxidochlorate) Dihydrogen(tetraoxidosulfate) Trihydrogen(tetraoxidophosphate) Dyhydrogen(trioxidocarbonate) Hydrogen(tetraoxidoiodate) Dihydrogen(trioxidosulfate) Tetrahydrogen(tetraoxidosilicate) Hydrogen(oxidobromate) Trihydrogen(trioxidoarsenate) Hydrogen(tetraoxidomanganate) Dihydrogen(tetraoxidochromate) Dihydrogen(tetraoxidoselenate) Hydrogen(dioxidochlorate) Dihydrogen(tetraoxidomanganate) Dihydrogen(heptaoxidodichromate) Hydrogen(trioxidonitrate) Hydrogen(tetraoxidochlorate) Dihydrogen(tetraoxidotellurate) Hydrogen(dioxidonitrate) Trihydrogen(trioxidophosphate) 13. Write the formula hydroxidochlorine hydroxidooxidochlorine hydroxidodioxidochlorine hydroxidotrioxidochlorine dihydroxidooxidosulfur dihydroxidodioxidosulfur Page 11 of 19

hydroxidooxidonitrogen hydroxidodioxidonitrogen trihydroxidophosphorus trihydroxidooxidophosphorus dihydroxidooxidocarbon tetrahydroxidosilicon dihydroxidodioxidochromium hydroxidotrioxidomanganese 2.3 Oxysalts 2.2.1.Common name It was named following the same rules for oxyacids, but changing suffixes. For the low oxidation numbers the suffix is -ITE, and the high oxidation numbers the suffix is -ATE. Oxidation numbers Acid Anion Highest per- -ic per- -ate High Low Lowest -ic -ous hypo- -ous -ate -ite hipo- -ite In the formula:na 2 SO 4 a) Separate from the salt cation and anion Deduces the charge of the anion (negative ion) from the charge of the cation (positive ion) b) Deduces the oxidation number of the central atom, knowing that the oxygen has oxidation number -2. c) Recalls oxidation numbers of central element, and writes the prefixes and suffixes. The first word is the name of the metal, followed immediately by the oxidation number between brackets and in Roman numbers. If the oxidation number of the metal is invariable, it is not indicated. The second word is the name of the anion with the suffixes and prefixes that correspond. Sodium sulfate In the name: Calcium nitrate a) Write the symbol of the cation with its electrical charge. Based on the prefixes and suffixes deduces the number of oxidation central element involved in the anion: Page 12 of 19

b) Formulates the oxyacid of N+5 c) Deduces the anion from the acid. The anion has so many negative electrical charges as hydrogens has the acid. Calculate the fewest ions of each type that you need so that the compound be neutral. Examples: Calcium bromate Ca(BrO 3 ) 2 Sodium hypochlorite NaClO Aluminum sulfate Al 2 (SO 4 ) 3 Magnesium phosphate Mg 3 (PO 4 ) 2 Iron(III) nitrate Fe(NO 3 ) 3 2.2.2.The additive names and stoichometric name The additive names : are based on the structure of the anions, naming first the first element in the formula (with oxidadtion number in brackets just if the element has more than one, then oxygen united central element (oxido). These names carry prefixes corresponding di-, tri-, tetra- and so on. And are named in alphabetical order followed by the name of the central atom finished in ate, followed by the charge number of the anion, with a negative sign, between brackets. Na 2 CO 3 Sodium trioxidocarbonate(2-) The stoichiometric names : are formed by the word "oxido" with the prefix that shows us the number of atoms of oxygen, followed by the central atom finished in ate. Also we write prefix in the firs element if we need it. Na 2 CO 3 Disodium trioxidocarbonate 14. Write the not common names for the following Salt Additive names Stoichiometric names Na 2 CO 3 Sodium trioxidocarbonate(2-) Disodium trioxidocarbonate KNO 2 Potassium dioxidonitrate(1-) Potassium dioxidonitrate Ca(NO 3 ) 2 Calcium trioxidonitrate(1-) Calcium bis(trioxidonitrate) AlPO 4 Aluminum tetraoxidophosphate(3-) Aluminum tetraoxidophosphate Na 2 SO 3 Sodium trioxidosulfate(2-) Disodium trioxidosulfate Fe 2 (SO 4 ) 3 Iron(3+) tetraoxidosulfate(2-) Diiron tris(tetraoxidosulfate) NaClO Sodium oxidochlorate(1-) Sodium oxidochlorate Ca(ClO 2 ) 2 Calcium dioxidochlorate(1-) Calcium bis(dioxidochlorate) Ba(IO 3 ) 2 Barium trioxidoiodate(1-) Barium bis(trioxidoiodate) Page 13 of 19

KIO 4 Potassium tetraoxidoiodate(1-) Potassium tetraoxidoiodate CuCrO 4 Copper(2+) tetraoxidochromate(2-) Copper tetraoxidochromate K 2 Cr 2 O 7 Potassium μ-oxidobis(trioxidocromate)(2-) Dipotassium Heptaoxidodicromate Na 2 MnO 4 Sodium tetraoxidomanganate(2-) Disodium tetraoxidomanganate Ba(MnO 4 ) 2 Barium tetraoxidomanganate(1-) Barium bis(tetraoxidomanganate) 15. Write the three names for this compounds: KNO 3 CuSO 4 KMnO 4 NaClO CaCO 3 NH 4 NO 3 K 2 Cr 2 O 7 Ba(ClO 4 ) 2 Fe 2 (SO 4 ) 3 Ni 3 (PO 4 ) 2 16. Write the formula Aluminium nitrate Cadmium carbonate Potassium sulfate Calcium phosphate Lead(II) sulfite Iron(II) nitrate Sodium nitrite Potassium permanganate Calcium silicate Iron(III) sulfate 17.Write the three names for this compounds: Page 14 of 19

NaNO 2 PbSeO 4 CuCO 3 Li 4 SiO 4 CaTeO 3 FeSO 3 Cr 2 (SO 3 ) 3 Al(ClO 3 ) 3 HgCrO 4 AgNO 3 18. Write the formula Barium hypochlorite Lead(II) dicromate Copper(II) chromate Cadmium selenate Zinc arsenate Calcium bromate Sodium periodate Copper(II) tellurite Manganese(III) sulfate Cobalt(II) phosphate Aluminium tris(trioxidonitrate) Cadmium trioxidocarbonate Dipotassium tetraoxidosulfate Calcium bis(tetraoxidophosphate) Lead trioxidosulfate Iron bis(trioxidonitrate) Ammonium dioxidonitrate Potassium tetraoxidomanganate Page 15 of 19

Dicalcium tetraoxidosilicate Diiron tris(tetraoxidosulfate) Barium bis(oxidochlorate) Lead heptaoxidodichromate Copper tetraoxidochromate Cadmium tetraoxidoselenate Trizinc bis(tetraoxidoarsenate) Calcium bis(trioxidobromate) Sodium tetraoxidoiodate Copper trioxidotellurate Dimanganese tris(tetraoxidosulfate) Tricobalt bis(tetraoxidophosphate) More activities: 1) http://www.easynotecards.com/quiz/10545 19. Write the chemical formula: a) Chlorine(VII) oxide b) Tin(4+) oxide c) copper(2+) oxide d) disodium oxide e) sulfur trioxide f) barium oxide g) barium dihydride h) copper(i) hydride I) carbon disulfide j) carbon(4+) chloride k) phosphorus(5+) chloride l) Strontium sulfide m) boron trichloride n) iron(iii) sulfide o) barium chloride p) mercury(2+) hydroxide Page 16 of 19

q) potassium selenide r) nitric acid s) hydrosulfuric acid t) hydrofluoric acid 20. Name in the 3 ways: a) Fe 2 S 3 b) Na 2 S c) KBr d) HgCl 2 e) HI f) SO 2 g) PbO 2 h) Li 2 O I) Au(OH) 3 j) SnO Page 17 of 19

Practice exam 1.- Write the names of the following compounds 1. Hg(OH) 2 2. FeCl 3 3. P 2 O 3 4. CsH 5. CaSeO 4 6. Sr(BrO 4 ) 7. HClO 8. TeO 3 9. Li 2 CO 2 10. NO 2 11. NaOH 12. O 7 Br 2 13. B 2 S 3 14. Au(OH) 3 15. NH 3 16. CaNO 3 17. SO 4 18. KIO 3 19. HClO 2 20. NiI 2 2.- Write the chemical formula: 21. hydrochloric acid 22. Iron(III) oxide 23. aluminum hydroxide 24. chloric acid 25. sulphur trioxide 26. cobalt(iii) bromide 27. phosphorus pentachloride 28. Aluminum bromate 29. Beryllium tetraoxidochromate 30. potassium hydride 31. hydrosulfuric acid 32. lead(ii) sulfide 33. calcium hydride 34. heptoxygen diiodide 35. Hydrogen(tetraoxidochlorate) 36. strontium bromide 37. dihydroxidooxidosulfur 38. gold(iii) iodide 39. nitric acid 40. copper(ii) hydroxide Page 18 of 19

Periodic Table with Oxidation Numbers. Table III 1A 2A 3B 4B 5B 6B 7B 8B 1B 2B 3A 4A 5A 6A 7A 8A 1 H -1 3 Li 11 Na 19 K 37 Rb 55 Cs 4 Be 12 Mg 20 Ca 38 Sr 56 Ba 26 Fe 27 Co 28 Ni 46 Pd 78 Pt 29 Cu 47 Ag 79 Au 30 Zn 48 Cd 80 Hg 5 B 13 Al 6 C -4 14 Si -4 50 Sn 82 Pb 7 N +5-3 15 P +5-3 33 As +5-3 51 Sb +5-3 8 O -2 16 S +6-2 34 Se +6-2 52 Te +6-2 9 F -1 17 Cl +7 +5-1 35 Br +7 +5-1 53 I +7 +5-1 Page 19 of 19