Nomenclature PDF

Learning Competencies: Represent compounds using chemical formulas, structural formulas and models STEM_GC11AMIc-e-21 Name compounds given their formula and write formula given the name of the compound STEM_GC11AMIc-e-23 Review Question 1 What are the...

Learning Competencies: Represent compounds using chemical formulas, structural formulas and models STEM_GC11AMIc-e-21 Name compounds given their formula and write formula given the name of the compound STEM_GC11AMIc-e-23 Review Question 1 What are the three (3) subatomic particles? Protons, Electrons, Neutrons Question 2 What is the isotope notation of Cobalt-60? Question 3 It exist in nucleus and have positive charge? Protons Question 4 It is located in an electron cloud which is the area surrounding the nucleus of the atom. Electrons Question 5 It serves as the identity of an element. Atomic Number (Z) Do you have a funny nickname? What is the story behind your funny nickname?  Naming of Compounds Objectives: 1.Identify ionic and covalent compounds; 2.Write the chemical name given the chemical formula 3.Apply the importance of naming of compounds to real-life situation. Formula Is a representation of the kind and number of atoms chemically combined in a compound. Example: H2O - formula of water - water consist of H and O - water has 2 atoms of H and 1 atom of O Nomenclature of Inorganic Compounds Symbol  is a letter or combination of two (2) letters which represents the chemical elements.  Most symbols are derived from their English names; others are from their Latin or German names: Carbon C Stibium Sb Calcium Ca Cuprum Cu Aurum Au Natrium Na Ferrum Fe Kalium K Plumbum Pb Stannum Sn Argentum Ag Wolfram W Subscript  is the number slightly below and to the right of the symbol.  It represent the number of element whose symbol it follows. atoms Example: H2O CO2 O3 Coefficient  is the number written before the formula or symbol.  represents the number of moles or molecules.  Moles – amount of substance (element/compound) Example: 3H2O - 3 moles or molecules of water Ionic Compounds VS. Covalent Compounds  Ionic compounds A compound whose atoms are bonded via a are neutral covalent bond is known compounds made as a covalent up of positively compound. charged ions called A covalent bond is cations (metals) and formed by sharing one or more pairs of valence negatively charged electrons. ions called anions These bonds are most (nonmetals). commonly found between nonmetals or between two elements of the same element. Write C if the compound given is COVALENT and I if its IONIC. 1. H2O 1. C 2. NaCl 2. I 3. CO2 3. C 4. CaI2 4. I 5. NO 5. C 6. CH4 6. C 7. CsF 7. I 8. PCl3 8. C 9. Mg3N2 9. I 10. LiCl 10. I  3 CATEGORIES IN NAMING COMPOUNDS Ionic Compounds Molecular/Covalent Compounds Acids and Bases A. Binary Ionic Compounds Containing a Metal Forming Only One Type of Cation (metal with fixed oxidation number) The chemical name is composed of the name of the metal followed by the name of the nonmetal, which has been modified to an identifying stem plus –ide.  A. Binary Ionic Compounds Containing a Metal Forming Only One Type of Cation (metal with fixed oxidation number) The chemical name is composed of the name of the metal followed by the name of the nonmetal, which has been modified to an identifying stem plus –ide. Example: Chemical Formula Chemical Name NaCl Sodium Chloride CaBr2 Calcium Bromide Mg3N2 Magnesium Nitride Li2O Lithium Oxide AlCl3 Aluminum Chloride CaC2 Calcium Carbide B. Binary Ionic Compounds Containing Metal that can Form Two or More Type of Cations (transition metals) 1. Stock or Roman Numeral System  A compound containing a metal that can form more than one type of cation, the charge of the cation of the metal is designated by Roman numeral placed in the parentheses () immediately following the name of the metal.  The negative element is treated in the usual manner for binary compounds. Cation Charge +1 +2 +3 +4 Roman Numeral (I) (II) (III) (IV) 1. Stock or Roman Numeral System Examples: Chemical Formula Stock FeCl2 Iron (II) Chloride FeCl3 Iron (III) Chloride CuCl Copper (I) Chloride CuCl2 Copper (II) Chloride SnO Tin (II) Oxide SnO2 Tin (IV) Oxide 2. Classical System  When the metallic ion has only two cations types, the name of the metal (usually the Latin name) is modified with the suffixes –ous and –ic to distinguish between the two. The lower charge cation is given the –ous ending and the higher one, the –ic ending. Examples: Classical Chemical Formula Stock FeCl2 Iron (II) Chloride Ferrous Chloride FeCl3 Iron (III) Chloride Ferric Chloride CuCl Copper (I) Chloride Cuprous Chloride CuCl2 Copper (II) Chloride Cupric Chloride SnO Tin (II) Oxide Stannous Oxide SnO2 Tin (IV) Oxide Stannic Oxide C. Binary Compounds Containing Two nonmetals (Covalent)  In a compound formed between two nonmetals, the element occurs first in this series is written and name first.  The name of the second element retains the –ide ending as though it were an anion.  A Latin or Greek prefixes is attached to the name of each element to indicate the number of atoms of that element in the molecule.  The prefix mono- is never used for the first element.  If the name of the second element begins with a vowel and a prefix for that name ends with either an o or a, these letters are not used, so that the pronunciation is easier. Examples: Chemical Formula Chemical Name CO Carbon Monoxide CO2 Carbon Dioxide PCl3 Phosphorus Trichloride SO2 Sulfur Dioxide P2O5 Diphosphorus Pentoxide CCl4 Carbon Tetrachloride N2O Dinitrogen Oxide N2O4 Dinitrogen Teroxide NO Nitrogen Oxide S2F10 Sulfur Decafluoride D. Binary Acids Write the prefix hydro- follow by the stem of the second element and add the suffix –ic. Write the word acid. Example: Chemical Formula Chemical Name HF Hydrofluoric Acid HCl Hydrochloric Acid HBr Hydrobromic Acid HI Hydroiodic Acid H2S Hydrosulfuric Acid  E. Naming Compound Containing Polyatomic Ions  A polyatomic ion is an ion that contains two or more elements.  Compounds containing polyatomic ions are composed of three or more elements and usually consist of one or more cations combined with a negative polyatomic ion.  Naming compounds containing polyatomic ion is similar to naming binary compounds.  The cation is named first, followed by the name of polyatomic ion.  Many polyatomic ions that contain oxygen are called oxyanions, and generally have the suffix –ate or –ite.  The suffix does not indicate the number of oxygen atom present.  The –ate form contains more O-atoms than the –ite form. Examples Chemical Formula Chemical Name KMnO4 Potassium Permanganate Ca3(PO4)2 Calcium Phosphate Li2CO3 Lithium Carbonate SrSO4 Strontium Sulfate BaSO3 Barium Sulfite  F. Bases Contain the –OH or hydroxide group. Example: Chemical Formula Chemical Name NaOH Sodium Hydroxide Ca(OH)2 Calcium Hydroxide Fe(OH)3 Ferric Hydroxide/ Iron (III) Hydroxide NH4OH Ammonium Hydroxide  What is the importance of knowing the chemical name of compounds? REVIEW Provide the chemical name of the following compounds. 1. CO2 2. CaC2 3. SiC 4. KOH 5. KClO3 6. ZnO 7. PbS 8. HF 9. NH3 10. CCl4 “How would you feel if someone misspelled your name?” FORMULA WRITING Objectives: 1. Identify the compounds as to ionic or covalent; 2. Write the chemical formula given the chemical name; 3. Apply the importance of naming of compounds to real-life situation.  FORMULA WRITING I. Compounds of metals and nonmetals or polyatomic ions  Place the oxidation number over the respective symbol of the element or ion.  Transfer each number (omitting the sign) as a subscript to the other symbol (Crisscross Method). The subscript 1 is never shown in a formula; it is implied if there is no subscript.  The symbol for the component that has the positive oxidation number is written first.  Elements or polyatomic ions with the same numerical oxidation number combine in the ratio of 1:1  Polyatomic ions with subscript 2 or more must be enclosed in parenthesis. If subscript is 1, no parenthesis needed.  Whenever possible, reduce the subscripts to simpler set of subscripts. Examples: Name Chemical Formula Calcium Chloride → Ca2+ Cl1- → CaCl2 Magnesium Oxide → Mg2+O2- → MgO Aluminum Phosphate → Al3+(PO4)3- → Al3(PO4)3 AlPO4 Barium Hydroxide → Ba2+(OH)1- → Ba(OH)2 Stannic Sulfide → Sn4+S2- → Sn2S4 → SnS2 II. Compounds of nonmetals (Molecular/Covalent) The prefix for each nonmetal represents the number of atoms for that element and is shown as subscript of the formula. Examples: Chemical Name Chemical Formula Dinitrogen Tetrxide N2O4 Carbon Monoxide CO Oxygen Hexafluoride OF6 Diphosphorus Pentoxide F2O5