PHA 612: Pharmaceutical Inorganic Chemistry (with Qualitative Analysis) PDF

PHA 612: Pharmaceutical Inorganic Chemistry (with Qualitative Analysis) LAB: FORMULA WRITING AND NAMING OF INORGANIC COMPOUNDS UNIVERSITY OF SANTO TOMAS - FACULTY OF PHARMACY (BS PHARMACY 2026 – 1BPH) [TRANS] FORMULA WRITING AND NAMIN...

PHA 612: Pharmaceutical Inorganic Chemistry (with Qualitative Analysis) LAB: FORMULA WRITING AND NAMING OF INORGANIC COMPOUNDS UNIVERSITY OF SANTO TOMAS - FACULTY OF PHARMACY (BS PHARMACY 2026 – 1BPH) [TRANS] FORMULA WRITING AND NAMING OF INORGANIC COMPOUNDS BRIEF INTRODUCTION Low valence and high valence state 1) NM + NM → Covalent Bond Ex. S + 2O → SO2 (Sulfur dioxide) Hg2+2 = Mercurous 2) M + NM → Ionic Bond Pwedeng ma-cancel ‘yong subscript para ma-simplify Ex. Mg2+ + Br-1 → MgBr2 (Magnesium bromide) siya → Hg+1 3) M + H2O → Base Hg2+ = Mecuric Ex. Na + H2O → NaOH (Sodium hydroxide) For Ni+2+3 = Ni(II) or Ni(III) = charge is in Roman Numeral and Note: Sodium ion/pure sodium alkali metal is very enclosed in parenthesis violent when put in water, so you are more likely to -ous or -ic = Classical System of naming inorganic have an explosive reaction. compounds 4) NM + H2O → Acid Roman Numeral in parenthesis = Stock System Two kinds of acids: Polyatomic Nomenclature Charge(s) a. Hydrohalic (Hx) Ions b. Oxyacid (oxygen-containing acids) ClO-1 Oxyanions (Oxygen- -1 5) Acid + Base → Salt + H2O (Hypochlorite) containing polyatomic Note: This is an example of neutralization reaction. ClO2-1 (Chlorite) anions): Salt can either be organic salt or inorganic salt, Hypo-, ite: with 1 less ClO3-1 (Common depending on the nature of your reactants. form: Chlorate) oxygen than the –ite form Example of organic salt: Sodium tartrate -ite: with 1 less oxygen ClO4-1 Example of inorganic salt: Sodium chloride than the –ate form (Perchlorate) BrO3-1 (Common -ate: Common form NOMENCLATURE OF INORGANIC IONS form: Bromate) Per-, -ate: with 1 more Note: Ions can either be positively or negatively charged. NO2-1 (Nitrite) oxygen than the –ate form NO3-1 (Common Thio-: if O was replaced Monovalent Ions Nomenclature Charge(s) with an S form: Nitrate) Group 1A: H+, Li+, Na+, K Metals: As is +1 OCN-1 Group 1B: Ag+ (Cyanate) Group 2A: Be+2, Mg+2, +2 SCN-1 Ca+2, Sr+2, Ba+2 (Thiocyanate) Group 2B: Zn+2, Cd+2 MnO4-1 Group 6A: O-2,S-2 Non-metals: -2 (Permanganate) Group 7A: F-1, Cl-1, Br-1, I-1 Suffix + ide -1 CO3-2 -2 (Carbonate) Valence – charge SO3-2 (Sulfite) Valence electrons – outermost electrons SO4-2 (Common Ex. Be form: Sulfate) Valence e- = 2 (Group 2A; the number of valence S2O2-2 electrons corresponds to the number of the group, (Thiosulfite) within the A family) S2O3-2 Valence = +2 (Thiosulfate) O CrO4-2 Valence e- = 6 (Group 6A) (Chromate) Valence = -2 Cr2O7-2 (Dichromate) Monovalent Ions/Monocharged Ions MoO4-2 Only have 1 charge; their charge does not vary (Molybdate) An atom with a valency of one, which can form one BO3-3 (Borate) -3 covalent bond PO4-3 Multivalent Ions Nomenclature Charge(s) (Phosphate) Hg+1+2, Cu+1+2 Lower ox. State: +1, +2 SiO4-4 (Silicate) -4 Au+1+3 +ous +1, +3 Fe+2+3,Co+2+3,Ni+2+3 Higher ox. State: +2, +3 Mn+2+3+4 +ic +2, +3, +4 Polyatomic Ions Sn+2+4, Pb+2+4 +2, +4 Made up of 2 or more elements but exist as ions Bi+3+5, As+3+5, Pb+3+5 +3, +5 -ate = common form Multivalent Ions -ite = if nabawasan ng isang oxygen ‘yong -ate form They have 2 or more charges Phosphate: PO4-3 (common form) Examples are most likely transition metals Sulfate: SO4-2 (common form) (Depending on the valence state, their colors change; Chromate: CrO4-2 (common form) aqueous solution) AQUINO, DICHOSO, ENCIENZO, PARRONE, SOLSONA, ZINGAPAN (LAB): FORMULA NAMING AND WRITING OF INORGANIC COMPOUNDS Polyatomic Ions Nomenclature Charge(s) HBr Hydrogen Hydrobromic HC3O-1 Hydrogen- -1 bromide gas acid soln. (Bicarbonate/Hydrogen containing H2S Hydrogen Hydrosulfuric carbonate) polyatomic ions: sulfide gas acid soln. HSO3-1 Monohydrogen (Bisulfite/Hydrogen (or simply iii. Binary Salts sulfite) ‘hydrogen’) or bi-: (Metal + Nonmetal) HSO4-1 1 captured H ions M (cation) + NM (anion) (Bisulfate/Hydrogen Dihydrogen: 2 Prefix: Metal name sulfate) captured H ions Suffix: Non-metal ending in –ide H2PO4-1 (Dihydrogen eg. NaCl – Sodium chloride phosphate) AgBr – Silver bromide HPO4-2 (Biphosphate/ -2 Mg3N2 – Magnesium chloride ZnS – Zinc sulphide Hydrogen phosphate) Al2O3 – Aluminum (tri)oxide A. Stock Method Polyatomic Ions Nomenclature Charge(s) Metal + (Roman Numeral) + Non-metal with suffix –ide (from Organic Compounds) CH3COO-1 or Acetate -1 B. Classical Method Metal (suffix: -ous/-ic) + Non-metal with suffix –ide C2H3O2-1 eg. Formula: C4H5O6-1 Citrate FeCl2 – a. Stock method: Iron(II) chloride C4H4O6-2 Tartrate -2 b. Classical Method: Ferrous chloride FeCl3 – Tartrate is from tartaric acid (DCA: Dicarboxylic Acid) a. Stock method: Iron(III) chloride b. Classical method: Ferric chloride Ewens-Bassett System Type of element nomenclature that gives the charge II. TERNARY COMPOUNDS of the complex ions rather than the oxidation state of 3 elements in a compound the central unit Fe(CN)6-3 = Ferricyanide i. Ternary Acid or Oxyacid Fe(CN)6-4 = Ferrocyanide Hydrogen + non-metal oxides (Oxyanion) Prefix: Hypo- or Per- or None RULES IN FORMULA WRITING AND NAMES Suffix: -ous or –ic acid Anion/Salt In aq. Soln. I. BINARY COMPOUNDS Hypo---ite Hypo...ous acid -ite -ous acid i. Compounds of 2 Non-metals (w/o Hydrogen) -ate -ic acid Prefix: Name of the less electronegative element Per...ate Per...ic acid (Prefix mono- is not used here) Suffix: Second element ending in –ide eg. HClO – Hypochlorous acid eg. HClO2 – Chlorous acid CO – Carbon monoxide HClO3 – Chloric acid (common form) SiO2 – Silicon dioxide HClO4 – Perchloric acid N2O5 – Dinitrogen pentoxide N2O – Dinitrogen monoxide NaOCl – Sodium hypochlorite CCl4 – Carbon tetrachloride PF5 – Phosphorous pentafluoride If mixed with water → HClO SBr6 – Sulfur hexabromide F – most EN element ii. Bases O – 2nd most EN element Named as hydroxides Both classical and stock names are used ii. Binary Acids (2 NM w/ Hydrogen) eg. NaOH – Sodium hydroxide Prefix: Hydro- Al(OH)3 – Aluminum hydroxide Suffix: -ic acid Fe(OH)2 – Iron(III) hydroxide or Ferrous hydroxide HX – hydrohalic acids (aqueous form) Sn(OH)4 – Tin(IV) hydroxide or Stannic hydroxide H + EN element (SONX: Sulfur, Oxygen, Nitrogen, Halogens- F, Cl, Br, I, At, Ts) iii. Ternary Salts or Salts of Oxyacids Prefix of oxyacid (if any) from which they are derived are retained Formula In gaseous In aqueous Suffix: -ite/-ate form form Eg. HCl Hydrogen Hydrochloric acid NaClO – Sodium hypochlorite chloride gas soln. NaClO2 – Sodium chlorite AQUINO, DICHOSO, ENCIENZO, PARRONE, SOLSONA, ZINGAPAN (LAB): FORMULA NAMING AND WRITING OF INORGANIC COMPOUNDS NaClO3 – Sodium chlorate NaClO4 – Sodium perchlorate NaNO2 – Sodium nitrite NaNO3 – Sodium nitrate (basic salt) Na3PO4 – Trisodium phosphate/tribasic sodium phosphate (harsh salt) NaH2PO4 – Monobasic sodium phosphate (default na nakalagay ‘yong two hydrogens) - Sodium dihydrogen phosphate - Acidic salt; can be used for medicine Na2HPO4 – Dibasic sodium phosphate - Disodium hydrogen phosphate/Sodium biphosphate - Acidic salt; can be used for medicine III. ACID SALTS Salts of poluprotic acids (>1 H-atoms remain in the salt) Prefix: Bi- or acid in place of H-atom eg. NaHCO3 – Sodium bicarbonate, sodium acid carbonate, sodium hydrogen carbonate NaHSO3 – Sodium bisulfite NaHSO4 – Sodium bisulfate KHC4H4O6 – Potassium bitartrate C4H4O6-2 (Tartrate) + 1 H+ = HC4H4O6-1 (Bitartartrate) IV. BASIC SALTS >1 O-2 or OH-1 ion remain in the salt eg. BiOCl – bismuth oxide chloride or bismuth oxychloride or bismuthyl chloride Co(OH)NO3 – cobalt(II) hydroxide or cobalt(II) hydroxinate or basic cobalt nitrate or basic cobalt(II) nitrate V. MIXED OR DOUBLE SALTS Salts containing two different cations Cation with lower charge is usually written and named first If same charge, alphabetical 2 cations sharing 1 anion eg. Na2Ca(So4)2 – Disodium calcium sulphate KCaPO4 – Potassium calcium phosphate KAl(SO4)2 – Potassium aluminum sulfate KNaC4H4O6 – Potassium sodium tartrate VI. MISCELLANEOUS INORGANIC SALTS A. Iso – isometric form HOCN – Isocyanic acid B. Meta – low hydrated form of oxyacid HPO3 – Metaphosphoric acid HBO2 – Metaboric acid C. Ortho – highest hydrated form of oxyacid H3P2O7 – Orthophosphoric acid D. Pyro – loss of water H4P2O7 – Pyrophosphoric acid (a disphosphoric acid) AQUINO, DICHOSO, ENCIENZO, PARRONE, SOLSONA, ZINGAPAN