Nomenclature and writing chemical equations CHEM 1411

Naming Binary Compounds TYPE 1 – if the compounds contain a metal and a non-metal 1.The cation is always named first and the anion second. 2.The cation takes its name from the name of the element (ex: Na + is sodium) 3.The anion is named by taking its root name and adding “ide”. (ex: Cl - is chloride)

Examples of Type 1 binary compounds CompoundIons presentName NaClNa +, Cl - Sodium Chloride KIK +, I - Potassium Iodide CaSCa 2+, S 2- Calcium sulfide CsBrCs +, Br - Cesium Bromide MgOMg 2+, O 2- Magnesium oxide

Name the following compounds: 1.CsF 2.AlCl 3 3.MgI 2 4.ZnS 5.Al 2 S 3 Write the formula of the following compounds: 1.Lithium bromide 2.Magnesium phosphide 3.Strontium oxide 4.Barium chloride

TYPE 2- if compound contains a metal that can form more than one type of cations (the transitions metals). Examples: Fe 2+, Fe 3+, Cu 2+, Cu 1+ 1.The cation is named first, the anion is named second. 2.Because the cation can assume more than one charge, the charge is specified by a Roman numeral in parenthesis. 3.The anion is named as it is with type 1 where the anion ends with “ide”. Examples: CompoundIons presentname CuClCu +1, Cl -1 Copper (I) Chloride HgOHg 2+, O 2- Mercury (II) oxide Fe 2 O 3 Fe 3+, O 2- Iron (III) oxide

Name the following compounds: 1.CoCl 3 2.CuI 3.SnBr 4 4.HgCl 2 5.PbS Write the formula of the following compounds 1.Iron (II) chloride 2.Chromium (III) oxide 3.Gold(III) chloride 4.Lead (IV) bromide

TYPE 3: compounds that contain only nonmetals RULES 1.The first element is named first, and the full element name is used. 2.The second element is named as though it were an anion. 3.Prefixes are used to denote the number of atoms present. 4.The prefix mono- is never used for naming the first element. Ex: CO is called carbon monoxide, NOT monocarbon monoxide 1Mono 2Di 3Tri 4Tetra 5Penta 6Hexa 7Hepta 8Octa BF 3 Boron trifluoride NONitrogen monoxide N2O5N2O5 Dinitrogen pentoxide Examples

Naming compounds that contain polyatomic ions. These are a group of atoms bound together, with a single overall charge. Examples: NH 4 +1 – ammonium ion SO sulfate ion NO 3 -1 – nitrate ion Naming of these compounds follow the same rules as naming type I and type II ionic compounds. Examples: 1.Na 2 SO 4 – sodium sulfate 2.Fe(NO 3 ) 3 – Iron (III) nitrate 3.NH 4 ClO 3 – ammonium chlorate

Name the following compounds: 1.NH 4 Cl 2.NaCN 3.K 3 PO 4 4.Fe 2 (SO 4 ) 3 5.NaC 2 H 3 O 2 Write the formula for the following compounds 1.Barium sulfate 2.Copper(II) sulfite 3.Iron (III) nitrate 4.Calcium carbonate 5.Ammonium dichromate

Naming Acids- In all acids, the cation is always the hydrogen ion, H + Binary acids- contains H + and a simple anion Rule: Hydro + name of anion ending in “ic” + “acid” Examples: HCl- hydrochloric acid HF- hydrofluoric acid Ternary acids- contains H + and a polyatomic ion Rule1: If the polyatomic ion ends with “ate”, change the “ate” to “ic” then add the word acid. Example: HNO 3 - nitric acid Rule2: if it ends with “ite”, change “ite” to “ous” then add the word acid. Example: HNO 2 - nitrous acid

Name the following acids: 1.HI 2.H 2 SO 4 3.H 3 PO 4 4.H 2 CO 3 5.HF Write the formula of the following compounds: 1.Sulfurous acid 2.Permanganic acid 3.Acetic acid 4.Hypochlorous acid 5.Hydrobromic acid

Copyright © Cengage Learning. All rights reserved. 2 | 12 What are the names of the following compounds? OF 2 S 4 N 4 BCl 3 OF 2 is oxygen difluoride S 4 N 4 is tetrasulfur tetranitride BCl 3 is boron trichloride

Copyright © Cengage Learning. All rights reserved. 2 | 13 What are the formulas for the following binary molecular compounds? carbon disulfide nitrogen tribromide dinitrogen tetrafluoride The formula for carbon disulfide is CS 2. The formula for dinitrogen tetrafluoride is N 2 F 4. The formula for nitrogen tribromide is NBr 3.

Copyright © Cengage Learning. All rights reserved. 2 | 14 Bromine has an oxoacid, HBrO 2, bromous acid (compare to HClO 2, chlorous acid). What are the name and formula of the corresponding anion? The anion corresponding to HBrO 2 is bromite, BrO 2 -.

Copyright © Cengage Learning. All rights reserved. 2 | 15 Hydrate A compound that contains water molecules weakly bound in the crystals. The formula of a hydrate is written with a dot before the water molecule(s) included. For example: CuSO 4  5H 2 O

Copyright © Cengage Learning. All rights reserved. 2 | 16 Hydrates are named using the anhydrous (without water) compound name followed by the prefix for the number of water molecules included and the word “hydrate.” For example: CuSO 4  5H 2 O is named copper(II) sulfate pentahydrate.

Copyright © Cengage Learning. All rights reserved. 2 | 17 A compound whose common name is green vitriol has the chemical formula FeSO 4  7H 2 O. What is the chemical name of this compound? FeSO 4  7H 2 O is iron(II) sulfate heptahydrate.

Copyright © Cengage Learning. All rights reserved. 2 | 18 A chemical equation is the symbolic representation of a chemical reaction in terms of chemical formulas. For example:2Na + Cl 2  2NaCl Reactants are the starting materials; they are written on the left of the equation. Products are the materials at the end of the reaction; they are written on the right of the equation.