Chemical Names and Formulas

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1 Ionic compounds are compounds made up of ions of opposite charges A chemical formula is the lowest whole number ratio of the ions present in the compound Na 2 Cl 2 can be reduced to NaCl The ratio of the ions will depend on the charge of those ions

2 Chemical Names and Formulas The charge is sometimes referred to as the oxidation number or oxidation state Ions formed from one atom are called monoatomic ions Group Number Charge

3 There are three types of ionic compounds to write formulas for and name Binary ionic compound Transition metal compound Ionic compound containing polyatomic ions Covalent compounds have a different naming system It uses prefixes Acids

4 Binary ionic compounds are made up of only 2 different elements There can be more than 2 or more atoms though NaCl K 2 O Al 2 S 3

5 To name a binary ionic compound Write the name of the cation first (always a metal) Write the name of the anion, but change the ending to ide Note that any subscripts do not change the name NaCl sodium chlorine chloride sodium chloride

6 K 2 O Al 2 S 3

7 Name the following compounds KI MgO SrS BeF 2 Li 2 O Al 2 O 3 Cs 3 N Ba 3 P 2

8 To write formulas it is important to remember that the charges on the compound must be balanced Same total number of positive and negative charges Determine if the charges are balanced NaCl LiO KI BeBr NaBr

9 When charges are not balanced, it is necessary to add subscripts They represent the quantity of each element No subscript equals 1 atom Li + O 2- the charges are not equal There is only one positive and two negatives We need another positive charge to make them equal Li 2 O

10 Write formulas for the following compounds Sodium sulfide Potassium iodide Calcium bromide Aluminum oxide Boron bromide Rubidium selenide

11 Sometimes the metal in a compound is a transition metal Groups 3-12 contain the transition metals Transition metals can move their electrons from the s to the d orbitals This gives them various oxidation numbers or charges For example iron can be either Fe 2+ or Fe 3+

12 Since these metals do not have a set charge, we must indicate their charge in the name, using Roman numerals For example look at the three possible compounds that chromium can form with fluoride Cr 2+ and F - yields CrF 2 called chromium (II) fluoride Cr 3+ and F - yields CrF 3 called chromium (III) fluoride Cr 6+ and F - yields CrF 6 called chromium (VI) fluoride

13 When writing a formula for a transition metal compound remember that the charge of the metal is in the parentheses Write formulas for the following: Lead (IV) chloride Iron (III) oxide Titanium (II) nitride Niobium (V) bromide Tin (II) oxide

14 Please note that several metals not in groups 3-12 are named this way Tin Lead Bismuth And others There are two transition metals that do have set charges We do not use Roman numerals when naming them Silver Ag + Zinc Zn 2+

15 To write formulas for compounds containing transition metals, we must work backwards: You will always start with a balanced formula: FeO Fe 2 O 3

16 Polyatomic ions are ions that contain more than one atom SO 4 2- OH - PO 4 3- NH 4 + It is important to note that the charge is distributed throughout all the atoms in the ion Not only on the last atom!

17 To name a formula containing a polyatomic ion we must first identify it If the ionic compound formula contains more than two elements, you have a polyatomic ion present We do not change the endings of any polyatomic ion

18 For example, NaOH is sodium hydroxide Na 2 SO 4 is sodium sulfate Ca(OH) 2 is calcium hydroxide We do not include the subscript outside of the parentheses when naming the compound

19 To write formulas of ionic compounds containing polyatomic ions: Calcium carbonate - Charges are balanced so Calcium hydroxide - Charges are not balanced - we need an additional OH -, but we must use parentheses Sodium carbonate Charges are not balanced we need an additional Na +, but we do not need parentheses Parentheses are only needed when you add a subscript to a polyatomic ion

20 We use a different system to name covalent compounds Prefixes are used to indicate the number of atoms in each molecule We need to know the number of atoms since there are not any charges to balance It would be impossible to determine the formula without the prefixes

21 Chemical Names and Formulas These are the prefixes for values 1-10 The number of atoms in the formula is represented in the name with the prefix H 2 S is Dihydrogen monosulfide Value Prefix 1 Mono 2 Di 3 Tri 4 Tetra 5 Penta 6 Hexa 7 Hepta 8 Octa 9 Nona 10 Deca

22 The naming system is straightforward except We never begin a formula name with mono CS 2 Carbon disulfide We eliminate the a or o in the prefix if the element begins with a or o N 2 O 5 dinitrogen pentoxide We still change the second element s ending to -ide

23 Bases (ending in OH - ) are named as taught before A common base with a different name is NH 3 ammonia Acids have a completely different naming system There are two types of acids Binary acid contains H + and anion (-) Oxy (Ternary) acid - contains H + and polyatomic ion (-)

24 To name a binary acid Use a prefix hydro Add the anion name with an ic ending Finish with acid HCl becomes hydrochloric acid HBr becomes hydrobromic acid H 2 S becomes hydrosulfuric acid

25 To write a formula for a binary acid Identify that it s a binary acid must start with hydro Write the H + and the other element with the charge Balance the charges Hydronitric acid becomes H + N 3- H 3 N

26 To name an oxy (ternary) acid Start with the polyatomic name If the polyatomic ends in -ate, change the ending to ic If the polyatomic ends in ite, change the ending to ous Finish with acid H 2 SO 4 becomes sulfuric acid H 2 SO 3 becomes sulfurous acid

27 To write a formula for an oxy (ternary) acid Identify that it s an oxy acid (no hydro in name) Start with H + Add name of polyatomic Remember that -ic means it ends in -ate and -ous means it ends in -ite Balance the charges Nitric acid becomes H + NO 3 - HNO 3

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