Chemical Nomenclature

Learning Targets Write name & write symbol of selected elementsWrite name & write symbol of selected elements Write name & write formula of a variety of compounds.Write name & write formula of a variety of compounds.

Naming Inquiry FormulaName l NaClSodium Chloride l KIPotassium Iodide l MgCl 2 Magnesium Chloride What is a binary compound?

Naming Inquiry FormulaName l NaClSodium Chloride l KIPotassium Iodide l MgCl 2 Magnesium Chloride What does the chemical formula of each indicate? What does the chemical formula of each indicate?

Naming Inquiry FormulaName l NaClSodium Chloride l KIPotassium Iodide l MgCl 2 Magnesium chloride Why are there two chlorines for one magnesium? Why are there two chlorines for one magnesium?

Naming Inquiry FormulaName l NaCl Sodium Chloride l KI Potassium Iodide l MgCl 2 Magnesium Chloride What are some naming rules that can be discovered from these examples? What are some naming rules that can be discovered from these examples?

I. Elements (periodic table) A.Symbols: come from the first letter, or first two letters of the element’s name. 1.First letter is always UPPERCASE, second letter always lower case. a.Co, cobalt vs. CO, carbon monoxide b.No, nobelium vs. NO, nitrogen oxide 2.Some use latin name for symbol, ex. Gold (latin name = aurum or Au)

NOTES II.Formula: Represents composition of a compound A.Tells proportions of elements in a compound relative to each other. 1.Subscripts are used to indicate number of atoms of each element in a compound. (ALWAYS Whole numbers!!) 2.The subscript follows the atom or atoms it refers to. If subscript follows “( )” then everything inside the “( )” is multiplied by the subscript.

l Examples: CO 2 One atom of C, 2 atoms of O H2OH2O 2 atoms of H, one atom of O Fe 3 (PO 4 ) 2 3 atoms of Fe, 2 atoms of P & 8atoms of O

Formulas, continued B.All atoms have oxidation numbers (valence charge). This is the combining power of the atom. ex : Everything in Group 1 has a +1 charge. Group 17 has -1 charge Na +1 Cl -1 combined = 0 ** You want your valences to always = 0

Examples continued l What happens when it doesn’t = 0? Mg +2 Cl -1 = 0 Mg +2 Cl -1 = 0 You add another Cl so… it now looks like this: so… it now looks like this: MgCl 2 MgCl 2 Now the “combined power” is 0

You Try Ca +2 N -3 K + P -3 Al +3 O -2

C.Polyatomic ions or “radicals” are groups of atoms that behave as if they are single atoms. They also have oxidation numbers. Examples: SO 4 -2 (sulfate ion), NO 3 -1 (nitrate ion)

D.We will use the concept of valence to write formulas 1.Valence is either “+” or “-” 2.In ALL compounds, the sum of the valences adds up to zero. 3.Metals are always “+” 4.Non-metals can be “+” or “-” 5.Most radicals are “-”, only common “+” radical is NH 4 +1 (ammonium)

Application 1.Example 1: Lithium Chloride …Li 1+ and Cl 1-, so the formula must be LiCl. 2.Example 2: Calcium Oxide …Ca 2+ and O 2-, so the formula must be CaO 3.Example 3: What about Lithium Oxide? 4.Answer: you need two lithium atoms for every one oxygen to balance…Li 2 O

E.Atoms that have a constant valence: 1.(+1) = first column and Ag, 2.(+2) = 2 nd column plus Zn and Cd 3.(+3) Al. (See columns already marked on your periodic table.) (H can be -1 in some special cases)

III.Naming Binary Salts & Writing their Formulas A.Metal plus a non-metal (two elements). B.Named by adding the name of the first element (metal) to the second element (non-metal) whose name is modified to end in “ide.” 1.Examples: oxygen becomes “oxide”oxygen becomes “oxide” chlorine becomes “chloride”chlorine becomes “chloride” sulfur becomes “sulfide”sulfur becomes “sulfide” etc…etc…

Now… The Rules l Rule #1: ends in “ide” = Binary salt NaCl Sodium chloride Al 2 O 3 Aluminum oxide KI Potassium iodide Rule #2: valences must = 0 Rule #2: valences must = 0

C.Most metals have a variable valence and this must be indicated in the name of the compound. 1.The Stock System: The valence (+) of the metal is given as a Roman numeral. 2.How does the Stock System Work?

How does the Stock System Work? l For metals in Groups 3-16 l Iron (II) chloride l The (II) tells me the valence of Fe. l I know that each Cl has a -1 charge. I have 2 Cl’s for a total charge of -2, so the Fe has to be +2 to make the valences add up to zero l FeCl 3 what is the oxidation of Fe? l Iron (III) chloride, Fe +3

You Try - l Write the name or the formula using the Stock System l CuCl –Copper (I) chloride l CrO 3 –Chromium (VI) oxide l Tin (IV) oxide –SnO 2 **if you have subscripts that can be reduced… DO IT!! –Nickel (II) oxide –NiO

IV.Salts with Radicals (polyatomic ions) (polyatomic ions) A.Four ways to identify salts 1.Metal + non-metal (binary) 2.Metal + Radical 3.Radical + Non-metal 4.Radical + Radical

IV.Salts with Radicals (polyatomic ions) Rule #3: B. Naming Salts (other than binary) 1.Name of metal + name of radical 2.Name of radical + name of non-metal (still ends in “ide”) or radical

IV.Salts with Radicals (polyatomic ions) C.The “common-form” of the radical MUST BE MEMORIZED 1.“common form” = “ate” ending a. Make Flash-Cards!!!!! a. Make Flash-Cards!!!!! 2. Other endings are based on “ate” ending

You Try: Write formula or name Calcium phosphate Ca +2 PO 4 -3 Potassium acetate K +1 C 2 H 3 O 2 -1 NaOH Al 2 (CO 3 ) 3 = Ca 3 (PO 4 ) 2 = KC 2 H 3 O 2 = Sodium hydroxide = Aluminum carbonate

IV.Salts with Radicals (polyatomic ions) 3. More Rules: Rule #4: if there is one less oxygen, then name ends in “ite” Rule #5: If there are 2 less oxygens the name starts with “hypo” & ends in “ite” Rule #6: I more oxygen then common form starts with “per” and ends in “ate”

l 4. Examples: NaNO 3, NaNO 2, NaNO, and NaNO 4 Naming compounds w/Radicals: l One more Oxygen: l Common Form: l One less Oxygen: l 2 less Oxygen:

l 4. Examples: NaNO 3, NaNO 2, NaNO, and NaNO 4 Naming compounds w/Radicals: l One more Oxygen: NaNO 4 – Sodium pernitrate l Common Form: NaNO 3 – Sodium nitrate l One less Oxygen: NaNO 2 – Sodium nitrite l 2 less Oxygen: NaNO – Sodium hyponitrite So… what is the difference?

You Try l Na 2 SO 5 –Sodium persulfate l Ca 3 (PO 2 ) 2 –Calcium hypophosphite l Magnesium hypofluorite –Mg(FO) 2 l Iron (II) nitrite –Fe(NO 2 ) 2

V. Naming Acids (Yep…More Rules!! ) 1. Binary Acids: all have H as first element and are aqueous  dissolved in water. 2. Can be named as common salts if not dissolved in water. hydrogen + non-metal. hydrogen + non-metal. Rule #7 - Named by: a. Change hydrogen  hydro b. Change non-metal -ide  -ic. c. Followed by the word acid. d. Example: HCl (aq) is Hydrochloric acid

You Try… l What would these be? –HF (aq) –Hydrofluoric Acid –HBr (aq) –Hydrobromic Acid (Most are from Group 17) l H 2 S (aq) l hydrosulfuric acid

3. Ternary Acids: hydrogen + radical. a.Rule #8: Named for the radical. “ate” ending changes to “ic” & is followed by “acid” 1.Ex: HNO 3 (aq) = Nitric Acid b.Rule #9: “ite” ending (Rule #4) changes to “ous” Ex: HNO 2(aq)Ex: HNO 2(aq) Common form = NO 3 -1 “nitrate” one less O, nitrous acid one less O, nitrous acid c.Also uses “hypo” “ous” & “per” “ic”

You Try – Ternary Acids Name Formula # of Oxygens HClO 4 (aq) HClO 3 (aq) HClO 2 (aq) HClO (aq) Perchloric acid +1 Common form -2 Chloric acid Chlorous acid Hypochlorous acid

REVIEW…so far l Binary Salts l Ternary Salts –Different # of O l Binary Acids l Ternary Acids –Different # of O How do you recognize…what are the clues?

VI. Molecular Compounds A.Greek System of naming 1.Only used for 2 non-metals 2.Ends in “ide” 3.Number of each kind of atom is indicated by a Greek numerical prefix (list on next slide)

Greek prefixes used for molecular compounds. Mono = 1Hexa=6 Di= 2Hepta=7 Tri=3Octa=8 Tetra=4Nona= 9 Penta=5Deca=10

Examples l CO 2 l Carbon dioxide l You Try: P 2 O 5, N 2 O 4, PCl 3, Chlorine heptoxide –Diphosphorous pentoxide –Dinitrogen tetroxide –Phosphorous trichloride –ClO 7

Can you fill in the blanks? FormulaName CO 2 Carbon Dioxide N 2 O 5 ______________ N 2 O 4 _______________ _____Phosphorous Trichloride P 4 O 10 _______________

A few more rules for naming binary compounds of non-metals: Rule #10: The prefix mono- is usually omitted except where it is used for emphasis, as in carbon monoxide. Rule #11: Common usage omits the double vowel – as in the example above carbon monoxide is not carbon mono-oxide. FYI: Some names for compounds don’t fit the rules (ex: H 2 O = water NH 3 = ammonia)

Naming Test l 3 rd Period Test 10/20 l 6 th Period Test 10/21 l Assignments due on Test day: Worksheets #1 – 9 Worksheets #1 – 9 Graphs for Elements & Naming Graphs for Elements & Naming