Take out this Periodic Table:

Naming Compounds What's in a name? That which we call a rose by any other name would smell as sweet." - William Shakespeare, Romeo and Juliet (II, ii)

Predicting Charges on Monatomic IONS KNOW THESE!!!! +1 +2-3 -2-1 0 Cd +2

Chemical Formulas Chemical formula- Consists of element symbols and subscripts C 6 H 12 O 6 Formula Units simplest whole # ratios of ions present in a compound (for ionic compounds) Molecular Formulas- used for covalently bonded compounds. (show EVERY atom present in a molecule) Ex. H 2 O Water has 2 hydrogen atoms and 1 oxygen atom

Writing Balanced Chemical Formulas Criss-Cross Rule for Ionic Compounds Step 1: Example: Aluminum Chloride write symbols & charge of elements Cation (metal) always written 1 st! Aluminum Chloride Step 2: criss-cross charges as subscripts Step 3: Al Al 3+ 1- Cl Cl 1 3 AlCl 3 combine as formula unit ( 1 is never shown) (use smallest whole # ratio) Make sure you remove charges!!

charge on cation becomes subscript of anion charge on anion becomes subscript of cation ** Warning: Reduce subscripts to lowest terms. Ones are not included in formulas!! Al 3+ and O 2 Ba 2+ and S 2 In 3+ and Br 1 Al 2 O 3 Al 2 O 3 Ba 2 S 2 BaS In 1 Br 3 InBr 3 aluminum oxide barium sulfide indium bromide

Criss-Cross Rule Example: Magnesium Oxide Step 1: Magnesium Oxide Step 2: Mg 2+ O 2- Step 3: Mg O 2 2 Step 4: Mg 2 O 2 Step 5: MgO

Putting Ions Together Na + + Cl - = NaCl Ca +2 + O -2 = CaO Ca +2 + Cl - = CaCl 2 Na + + O -2 = Na 2 O Al +3 + S -2 = Al 2 S 3 Ca +2 + N -3 = Ca 3 N 2 You try these! Li + + Br - = LiBr Mg +2 + F - = MgF 2 Al +3 + I - = AlI 3 K + + Cl - = KCl Sr +2 + P -3 = Sr 3 P 2

Crisscross Switch the numerical value of the charges Ba 2+ N 3-3 Ba 3 N 2 Reduce ratio if possible

Learning Check Write the correct formula for the compounds containing the following ions: 1. Na +, S 2- a) NaS b) Na 2 S c) NaS 2 2. Al 3+, Cl - a) AlCl 3 b) AlCl c) Al 3 Cl 3. Mg 2+, N 3- a) MgN b) Mg 2 N 3 `c) Mg 3 N 2

Solution 1. Na +, S 2- b) Na 2 S 2. Al 3+, Cl - a) AlCl 3 3. Mg 2+, N 3- c) Mg 3 N 2

Polyatomic Ions There are some ions that are made up of more than one type of atom, these are called Polyatomic ions groups of covalently bonded atoms with a charge For example, the polyatomic ion known as ammonium, NH 4+,has 4 atoms of hydrogen and one atom of nitrogen, HOWEVER, the whole group has an overall charge of +1 NH 4 + ** you need to memorize the formulas & the charges of many polyatomic ions!

Formula Writing & Naming of Compounds

Naming Ternary Ionic Compounds contain at least 3 elements & the 1 st is a metal: there MUST be at least one polyatomic ion (it helps to circle the ions) Examples: NaNO 3 Sodium nitrate K 2 SO 4 Al(HCO 3 ) 3 Potassium sulfate Aluminum bicarbonate or Aluminum hydrogen carbonate

Al(HCO3)3

What About... What if I have to put multiple polyatomic ions in a compound, for example, magnesium nitrate? Magnesium has a charge of +2 Nitrate is polyatomic ion and has a charge of -1 Therefore, we need 2 nitrate ions for each magnesium In this case, we put the entire polyatomic ion in parenthesis and put the subscript outside the parenthesis Our answer would be Mg(NO 3 ) 2

Ionic Metal + non-metal/ polyatomic Reduce Criss-Cross Apple Sauce Roman numerals????

Ternary Ionic Nomenclature Sodium Sulfate Na + and SO 4-2 Na 2 SO 4 Iron (III) hydroxide Fe +3 and OH - Fe(OH) 3 Ammonium carbonate NH 4+ and CO 3 2 (NH 4 ) 2 CO 3

ammonium chloride, NH 4 Cl IONIC COMPOUNDS Remember: they have oppositely-charged ions in a RIGID 3-D pattern NH 4 + Cl -

Writing Formulas w / Polyatomic Ions Reminder: Parentheses are required only when you need more than one bunch of a particular polyatomic ion. Ba +2 and SO 4 2 Mg +2 and NO 2-1 BaSO 4 Mg(NO 2 ) 2 barium sulfate magnesium nitrite NH 4 +1 and ClO 3-1 Sn +4 and SO 4-2 NH 4 ClO 3 Sn(SO 4 ) 2 ammonium chlorate tin (IV) sulfate Fe +3 and Cr 2 O 7-2 NH 4 +1 and N -3 Fe 2 (Cr 2 O 7 ) 3 (NH 4 ) 3 N iron (III) dichromate ammonium nitride

Learning Check 1. aluminum nitrate a) AlNO 3 b) Al(NO) 3 c) Al(NO 3 ) 3 2. copper(ii) nitrate a) CuNO 3 b) Cu(NO 3 ) 2 c) Cu 2 (NO 3 ) 3. Iron (III) hydroxide a) FeOH b) Fe 3 OH c) Fe(OH) 3 4. Tin(IV) hydroxide a) Sn(OH) 4 b) Sn(OH) 2 c) Sn 4 (OH)

Naming Compounds Binary Ionic Compounds (metal & nonmetal): 1. Cation first, then anion 2. Monatomic cation = name of the element Ca 2+ = calcium ion 3. Monatomic anion = root + -ide Cl - Final Answer: CaCl 2 = chloride = calcium chloride

Naming Binary Ionic Compounds Examples: NaCl ZnI 2 Al 2 O 3 sodium chloride zinc iodide aluminum oxide

Formulas to Names: Ternary Compounds 1. Write the names of the ions KMnO 4 I m a polyatomic ion potassium permanganate Final Name If the positive ion has a fixed charge, you are finished.

Learning Check Match each set with the correct name: 1. Na 2 CO 3 a) magnesium sulfite MgSO 3 b) magnesium sulfate MgSO 4 c) sodium carbonate 2. Ca(HCO 3 ) 2 a) calcium carbonate CaCO 3 b) calcium phosphate Ca 3 (PO 4 ) 2 c) calcium bicarbonate

Multiple OXIDATION Numbers When the metal in an ionic compound is multivalent (has more than 1 charge) there are 2 naming methods: Latin and Stock Systems Latin is older (not useful for some compounds) The metal is named with it s Latin or English root and ends in -ic or ous to denote charge. Lower = ous, Higher = ic ex. Cu +1 is cuprous, e.g. Cu +2 is cupric

Write the balanced formula for copper chloride & name it: Cu +2 + Cl -1 = CuCl 2 copper (II) chloride cupric chloride Cu +1 + Cl -1 = CuCl copper (I) chloride cuprous chloride

Binary Compounds Containing a Metal of Variable Oxidation Number To name these compounds, give the name of the metal (Type II cations) followed by Roman numerals in parentheses to indicate the oxidation number of the metal, followed by the name of the nonmetal, with its ending replaced by the suffix ide. Examples FeCl 2 FeCl 3 Stock System Iron chloride Iron chloride Traditional (OLD) System Ferrous chloride Ferric chloride SnO Tin (II) oxide SnO 2 Tin (IV) oxide Stannous oxide Stannic oxide ic ending = higher oxidation state; ous is lower oxidation state

Ternary Ionic Nomenclature Writing Formulas 1.Write each ion, cation first. Don t show charges in the final formula. 2.Overall charge must equal zero. 1. If charges cancel, just write symbols. 2. If not, use subscripts to balance charges. 3.Use parentheses to show more than one of a particular polyatomic ion. 4.Use Roman numerals to indicate the ion s charge when needed (Stock System)

When do I need Roman Numeral? Fe 2 O 3 Look on PERIODIC TABLE OF IONS If metal in formula has multiple ion numbers name needs Roman Numberal Fe has 2 choices on table: Fe 3+ and Fe 2+

How do I figure out the Roman Numeral? Solving for the Roman numeral (charge) of Fe 2 O 3 1. Do reverse crisscross and ID charge on metal ion 2. Check table of ions not there formula was reduced Fe 2 O 3 Fe 3+ O 2- Iron (III) Oxide

Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr 2 CuCl SnO 2 Fe 2 O 3 Hg 2 S iron ( ) bromide copper ( ) chloride ( )

How do I name a molecular binary compound? A molecular (Covalent) binary compound is made of two nonmetals.

Uses a Prefix System 1. Less electronegative atom comes first (towards left side of P.T.) 2. Add numerical prefixes to indicate # of atoms of each element. 3. Change the ending of the second element to ide (since it s binary)

When a compound contains 2 non-metals, you may need to use a prefix. Prefixes to memorize: 1. mono 2. di 3. tri 4. tetra 5. penta 6. hexa 7. hepta 8. octa 9. nona 10.deca

Remember: Prefix refers to # of atoms, NOT charge example: N 2 O 4 = dinitrogen tetroxide Note: this is a covalent compound so subscripts are not reduced. N 2 O 4 NO 2

Remember: EXCEPTION: Don t use mono for the first element example: CO 2 = carbon dioxide Do use mono for second element. - The first vowel is often dropped to avoid the combination of ao or oo. CO = carbon monoxide (NOT monooxide) P 4 O 10 = tetraphosphorus decoxide (NOT decaoxide)

Covalent Compounds: Name to Formula You ll like this! For covalent compounds, simply use the numerical prefixes to tell you the number (subscript) of each element **No charges **No criss-cross **No balancing needed! What is the formula for dinitrogen trioxide? dinitrogen monoxide? N 2 O N 2 O 3

Example #1-Names to Formulas Two Non metals: I m a Binary Compound Sulfur trioxide 1. Write symbols of elements 2. Write number of atoms S O 1 3 Final Formula If no prefix, then 1 is implied and not written

Example #2-Names to Formulas I m a Binary Compound dichlorine heptaoxide 1. Write symbols of elements 2. Write number of atoms Cl O 2 7 Final Formula

Example #3-Names to Formulas I m a Binary Compound oxygen difluoride 1. Write symbols of elements 2. Write number of atoms O F 1 2 Final Formula If no prefix, then 1 is implied and not written

Example #4-Names to Formulas I m a Binary Compound dinitrogen tetraoxide 1. Write symbols of elements 2. Write number of atoms N O 2 4 Final Formula

Example #5-Names to Formulas I m a Binary Compound phosphorus pentachloride 1. Write symbols of elements 2. Write number of atoms P Cl 1 5 If no prefix, then 1 is implied Final and Formula not written

Examples #2- Formulas to Names 1. Write names of elements last element ends in -ide 2. Write prefix for number of atoms XeF 3 I m a Binary Compound monoxenon If first prefix is mono, it is implied and not written Final Name trifluoride

Example - Formulas to Names 1. Write names of elements (-ide on last) 2. Write number of atoms AsI 3 I m a Binary Compound monoarsenic If first prefix is mono, it is implied and not written Final Name triiodide

Examples #1- Formulas to Names 1. Write names of elements Two Non metals: 2. Write number of atoms CCl 4 I m a Binary Compound monocarbon If first prefix is mono, it is implied and not written tetrachloride Final Name

Write and name the following covalent compounds (IUPAC) CCl 4 carbon tetrachloride P 2 O 3 diphosporus trioxide IF 7 iodine heptafluoride International Union of Pure & Applied Chemistry they make the final decision in naming rules

Learning Check Fill in the blanks to complete the following names of covalent compounds. CO CO 2 PCl 3 CCl 4 N 2 O carbon oxide carbon phosphorus chloride carbon chloride nitrogen oxide

http://www.dhmo.org/facts.html

Take out this Periodic Table:

H SO sulfuric acid Acid Nomenclature Acids Compounds that form H + in water. Formulas usually begin with H. In order to be considered an acid, they must be aqueous (dissolved in water formulas end in (aq) ) Examples: HCl (aq) hydrochloric acid HNO 3 (aq) nitric acid

Acid Nomenclature Examples: HCl (aq) hydrochloric (acid in your stomach) HNO 3 (aq) nitric acid (TNT) H 2 SO 4 (aq) sulfuric acid (Car batteries)

Naming Binary Acids H bonded w/ another element : HX (aq) If the anion attached to hydrogen ends in -ide, add the prefix hydro- and change -ide to -ic acid For example: HCl - hydrogen chloride becomes hydrochloric acid H 2 S - hydrogen sulfide becomes hydrosulfuric acid

Naming Ternary Acids H bonded to a polyatomic ion: HXO (aq) change the suffix -ate to -ic acid x. HNO 3(aq) not hydrogen nitrate, but nitric acid change the suffix -ite to -ous acid x. HNO 2(aq) not hydrogen nitrite, but nitrous acid Ternary Acid names DO NOT begin with hydro-

Acid Nomenclature Binary Ternary emember: Anion Ending -ide -ate -ite Acid Name hydro-(stem)-ic acid (stem)-ic acid (stem)-ous acid In the cafeteria, you ATE something ICky

Examples #1- Formulas to Names HBrO 2(aq) 1. The hydrogen out front & the (aq) subscript indicates an acid 2. Determine the ion and it s acid ending. bromite bromous acid Final Name

Writing Acid Formulas Hydrogen will always be first (The name will tell you the anion) If it starts with hydro- it s binary, and H+ is bonded to a non-metal If it doesn t start with hydro-, it s ternary and H+ is bonded to a polyatomic ion.

Writing Acid Formulas Remember: -ate comes from -ic, -ite comes from ous Finally: Balance charges.

Example #1-Names to Formulas chloric acid 1. Determine the formula & charge of the polyatomic ion 2. Add hydrogen ions 3. Balance charge with ions 4. Add the subscript: (aq) chlorate +1 H ClO 3-1 =0 (aq) Final Formula

Acid Nomenclature Flowchart ACIDS start with 'H' 2 elements 3 elements hydro- prefix -ic ending no hydro- prefix -ate ending becomes -ic ending -ite ending becomes -ous ending

Stop Here?

per- is one more oxygen than the ate -ite is one less oxygen than the ate hypo- is one less oxygen than the ite HNO NO 2 = nitrite NO 3 = nitrate

per- is one more oxygen than the ate -ite is one less oxygen than the ate hypo- is one less oxygen than the ite

Naming Simple Chemical Compounds Ionic (metal and nonmetal) Covalent (2 nonmetals) Metal Nonmetal First nonmetal Second nonmetal Forms only one positive ion Forms more than one positive ion Single Negative Ion Polyatomic Ion Use the name of element Use element name followed by a Roman numeral to show the charge Use the name of the element, but end with ide Use the name of polyatomic ion (ate or Ite) Before element name use a prefix to match subscript Use a prefix before element name and end with ide

Naming Simple Chemical Compounds Metal Ionic (metal and nonmetal) Nonmetal TOMORROW Grade HW Work on Study Guide Create your Cheat Sheet Forms only one positive ion Use the name of element Forms more than one positive ion Use element name followed by a Roman numeral to show the charge Single Negative Ion Use the name of the element, but end with ide Polyatomic Ion Use the name of polyatomic ion (ate or Ite) FRIDAY JEOPARDY (BRING YOUR NB!!!)

PRACTICE Two nonmetals Multiple-charge cation Everything else carbon sulfur NCl tetrabromide 2 dichloride O 35 vanadium niobium Mn Pt(IO (V) (II) 2 Sperchlorate 53 chromate ) 4 rubidium barium NH 4 KI ClOoxide sulfate 3 Greek prefixes Roman numeral for name only Roman numeral Charge Polyatomic ions OK Polyatomic ions OK Criss- Cross Rule Roman numeral Where would you file this? VCrO 4 dinitrogen pentoxide BaO platinum (IV) iodate CBr 4 ammonium chlorate Nb(ClO 4 ) 5 potassium iodide SCl 2 nitrogen trichloride Rb 2 SO 4 manganese (V) sulfide

Rainbow Matrix Game Link on Chemistry Geek.com on Chemistry I page http://chemistrygeek.com/rainbow Use [ ] to represent subscripts since you can t enter subscripts into the computer So H 2 O would be H[2]O And Al 2 (SO 4 ) 3 would be Al[2](SO[4])[3] Additional Polyatomic Ions (you do not have to memorize these, but they are in the game!) Borate = BO 3-3 ; Silicate = SiO 4-4 ; Manganate = MnO 4-2 (permanganate is -1)