AP Chem Catalyst Catalyst Questions To Do & Homework Binder The following atoms in their neutral form are unstable (don’t have 8 valence electrons): Ca, F, N, and S. Find the charges that they would form to become stable Tell me whether they are cations or anions. Homework: Complete Nomenclature Problems Wednesday Aug 5 You will have 6 tabs: (Use sticky notes if you don’t have dividers) In Class Notes 3. Tests/Quizzes/Study Guides 5. Classwork Outlines 4. Problem Sets 6. Homework (Place In Class Notes in Tab 1) Binder

1.5 Nomenclature

Forming Chemical Bonds The force that holds two atoms together is called a chemical bond. There are three types of bonds: Ionic bonds (Metal & Nonmetal) Covalent bonds (Nonmetal & Nonmetal) Metallic bonds (Metal & Metal)

The Formation and Nature of Ionic Bonds Cations are atoms with a positive charge. Anions are atoms with a negative charge. The electrostatic force holds ions of opposite charge together, forming an ionic bond.

Ionic Bonds Characteristics of ionic bonds: Formed between metals and nonmetals High melting point and boiling point. Able to conduct electricity when dissolved in water. Unable to conduct electricity in the solid phase. The strength of the bond depends on the charges, and distance between ions Ionic bonds form a lattice structure

Covalent Bonds Characteristics of covalent bonds: Formed between nonmetal pairs Electrons are shared between atoms Lower melting points, Lower Boiling Points Do not conduct electricity Brittle solids

Metallic Properties of metallic bonds: Delocalized electrons High electrical conductivity High luster (shiny) Remember that transitional metals have a varying number of valence electrons.

Predict if the following bonds are ionic or covalent: a) C-N b) N-O c) Na-F d) Mg-S e) C-H f) Ca-F

The oxidation number of an ion can be determined with the aid of the periodic table. For transitional metals below, charges vary so when naming ionic compounds with these elements, put the charge in parenthesis after the metal. +1 +2 +3 +4 -3 -2 -1

Example Copper can have a +2 or +3 charge so to know which it is you put parenthesis next to the transitional metal. Cu (II) means copper with a positive 2 charge Cu2+ Cu (III) means copper with a positive 3 charge Cu3+

Predict the oxidation number of the following elements: a) Al b) Mg c) Si d) O e) Cl

Predict the oxidation number of the following elements: a) Al +3 b) Mg +2 c) Si +4 d) O -2 e) Cl -1

Nomenclature for Ionic Formula Units There are over 50 million substances! We CANNOT have unique names for all these substances, that would be too much! That is why we have naming rules.

Nomenclature Steps for writing ionic formulas: Determine the symbol and oxidation number of the elements If the charges are not the same, subscripts must be added to achieve equal number of positive and negative ions. Criss-cross, ignore charge, write formula Metals always first, then nonmetal NO prefixes needed. Ionic formulas end in -ide Show on Dry Erase: Example 1: calcium chloride Example 2: Potassium oxide

Examples Write the formula of the following ionic compounds: Magnesium chloride Aluminum oxide Iron (III) chloride Chromium (III) oxide

You try first, then confirm with partners. Write the formula of the following ionic compounds: a) Cesium nitride b) Barium sulfide c) Calcium oxide d) Aluminum fluoride e) Sodium oxide What if the charges are the same, then just ignore charges, and write the formula, no need for criss- crossing!

Write the formula of the following ionic compounds: Iron (II) oxide Iron (III) oxide Copper (II) chloride Lead (IV) iodide Iron (II) chloride Chromium (III) sulfide Titanium (II) oxide Lead (IV) sulfide Copper (I) nitride

Ionic compounds with polyatomic ions

Memorize, will be using all year Polyatomic ions are groups of atoms with a charge: Ammonium (NH4) + Hydronium (H3O)+ Hydroxide (OH)- Sulfate (SO42-) Nitrate (NO31-) Chromate (CrO42-) Carbonate (CO32-) Phosphate (PO43-) Cyanide (CN-)

Review Ionic Formulas using polyatomic ions Write the formula of the following ionic compounds. Use the flashcards: a) Calcium nitrate b) Sodium sulfate c) Ammonium oxide d) Lead (II) phosphate e) Lead (IV) phosphate

You Try a) Chromium (III) hydroxide b) Nickel (II) nitrate Write the formula of the following ionic compounds: a) Chromium (III) hydroxide b) Nickel (II) nitrate c) Ammonium sulfate d) Silver (I) nitrate e) Magnesium chlorate

You try one more time Write the formula of the following ionic compounds: Potassium carbonate Hydrogen carbonate c) Iron (III) hydroxide d) Ammonium phosphate e) Sodium sulfate

Now backwards – ionic no prefixes! Write the names of each of the following formulas: Na2O CuCl2 c) Cr2O3 HINT: Cu and Cr are transitional metals, so they need roman numerals.

Nomenclature for Covalent Compounds

Molecules that are made from a combination of two nonmetals (covalent Molecules that are made from a combination of two nonmetals (covalent?) require Greek prefixes in their names Mono- 1 Hexa- 6 Di- 2 Hepta- 7 Tri- 3 Octa- 8 Tetra- 4 Nona- 9 Penta- 5 Deca- 10

Examples Find the formula of the following a) Phosphorus trifluoride b) Nitrogen dioxide c) Carbon trioxide Mono is not required for the first nonmetal in the covalent compound

You Try a) Sulfur dibromide b) Sulfur hexachloride c) Phosphorus pentafluoride d) Nitrogen trihydride e) Oxygen difluoride

Now backwards, you try Name the following compounds: a) SF2 b) NI3 c) CF4

Name the following compounds: a) PCl3 b) N2O3 c) PF3 d) NF3 e) SCl2

Naming Organic Compounds

Organic Compounds containing carbon and hydrogens Hydrocarbons are named by counting the number of carbon atoms: C1 – meth C6 – hex C2 – eth C7 – hept C3 – prop C8 – oct C4 – but C9 – non C5 – pent C10 – dec

3 types of hydrocarbons The ending depends on the type of bond formed: Single bond: -ane (Alkanes) Double bond: -ene (Alkenes) Triple bond: -yne (Alkynes)

Is it a ring or a chain? The number of carbon atoms in a compound is calculated by the formulas: CXH2X+2 for chains CXH2X for rings

Examples Write the formula/name for each of the following: a) methane b) butane c) cyclopropane d) C5H12 e) C6H14 f) C10H20

You try Write the formula/name for each of the following: a) heptane b) cyclononane c) ethane d) C3H6 e) C5H12 f) C7H14 NEED TO CREATE HOMEWORK PROBLEMS

Nomenclature for Acids

Naming Acids Binary acids are named using the prefix hydro- and the suffix –ic acid. No prefixes HCl hydrochloric acid HBr hydrobromic acid HI hydroiodic acid H2SO4 sulfuric acid (no hydro- needed) HCN hydrocyanic acid