Name: Unit 6 Bonding and Nomenclature Day Page # Description IC/HW Due Date Completed ALL Warmup IC 1 Ionic Bond Gizmo IC/HW 1 Covalent Bond Gizmo IC/HW 1 Cut Out Activity HW 2 Ionic Bonding Activity IC 2 Ionic Bonding Notes IC 2 Naming Ionic Compounds IC 2 Ionic Bond Naming Worksheet HW 3 Lewis Structures Notes IC 3 Ionic Lewis Activity IC 3 Covalent Bonding Notes IC 3 Covalent Lewis Activity IC 4 Polyatomic Ions Quiz IC 4 Naming Covalent Compounds IC 4 Naming Acids IC 4 Bonding Games IC 4 Covalent Bond Naming Worksheet HW 5 VSPER IC 5 Shapes and Bonding Orbitals Activity IC 5 Prelab Polarity Lab HW 5 VSPER Worksheet HW 6 Quiz on Ionic and Covalent Naming IC 6 Polarity Lab IC 6 Polarity Notes IC 6 Polarity Worksheet IC 7 IMF Lab IC 7 IMF Notes IC 7 Hybridization IC 8 Unit 6 Review HW 9 Unit 6 Test Unit 6: Bonding and Nomenclature Page 1
Polyatomic Ions: These are the ones you need to know! Polyatomic Ions NH 4 + H 3 O + NO 3 OH CN ClO 3 C 2 C 3 O 2 MnO 4 HCO 3 2 SO 4 2 CO 3 2 CrO 4 3 PO 4 Name Ammonium Hydronium Nitrate Hydroxide Cyanide Chlorate Acetate Permanganate Bicarbonate Sulfate Carbonate Chromate Phosphate Unit 6: Bonding and Nomenclature Page 2
Day 2 1. What is an ionic compound? WarmUp 2. What is a covalent compound? Day 3 1. Complete the table Polyatomic Ion PO 4 3 OH ClO 3 Name Cyanide Bicarbonate Acetate Ammonium Day 4 1. Determine if the following compounds are ionic or covalent: a. NaCl b. BaBr 2 c. CCl 4 d. SO 2 e. SnCl 4 f. PF 3 Unit 6: Bonding and Nomenclature Page 3
Day 5 1. Name the following compounds: a. NaCl b. BaBr 2 c. CCl 4 d. SO 2 e. SnCl 4 f. PF 3 Day 6 1. Complete the table below with the name of each shape: Steric Number 0 Lone Pairs 1 Lone Pair 2 Lone Pairs 2 3 4 2. What two shapes are ALWAYS polar? 3. Give the formula for Boron and Chlorine. Day 7 1. Draw the structural diagram for BF 3. What is the shape? Is it polar or nonpolar? Day 8 1. Draw the Dot Diagram for PCl 3 2. Draw the Dot Diagram for CaCl 2 Unit 6: Bonding and Nomenclature Page 4
Ionic Bonding Activity: Writing Chemical Formulas A chemical formula is a combination of symbols and numerical subscripts that represent the composition of a compound. The symbols indicate which elements are present, and the subscripts indicate the relative proportion of each element in the compound. These proportions can be predicted using the oxidation numbers of the elements and charges of the polyatomic ions. When atoms gain or lose electrons, they become ions. Ions consisting of more than one atom are called polyatomic ions. The apparent charge of an atom is its oxidation number. The following rules are used to ensure that all scientists write formulas the same way: 1. In a neutral compound, the sum of the oxidation numbers/charges must equal zero. 2. One positive (+) neutralizes one negative (). 3. Ions with positive oxidation numbers/charges are written first. 4. Only one type of cation and one type of anion can be used in a compound. 5. If more than one atom of an element is in a compound, the symbol for that element must be followed by the appropriate subscript, as in MgBr 2. 6. If more than one polyatomic ion is needed in a compound, the symbol for the ion must be enclosed in parentheses and followed by the appropriate subscript, as in Mg(NO 3 ) 2. Procedure: 1. Cut out each card from the sheet provided. 2. Identify the charge of each ion and write it on the card. Each removed segment represents a positive charge while each added segment represents a negative charge. Mg, for example, has two segments removed, so it would have a 2+ charge. 3. Construct formulas for the substances below and list the information in the data table. For example, for magnesium and chlorine, place a Mg 2+ card in the table in the Ion column. Place enough Cl cards next to it in order to obtain a neutral compound. Then, write the formula in the Formula column. Substances to Bond magnesium and chlorine aluminum and bromine sodium and oxygen calcium and sulfur potassium and sulfate barium and nitrate lithium and phosphate ammonium and fluorine 4. Use the blank cards to create five additional compounds of your choice. Unit 6: Bonding and Nomenclature Page 5
Name: Period: Elements Ions Formula magnesium and chlorine aluminum and bromine sodium and oxygen calcium and sulfur potassium and sulfate barium and nitrate lithium and phosphate Unit 6: Bonding and Nomenclature Page 6
Elements Ions Formula ammonium and fluorine Unit 6: Bonding and Nomenclature Page 7
Metallic and Ionic Bonding Notes There are three main types of bonding: ionic, metallic and covalent. Metallic Bonding Metallic bonds consist of positively charged metallic cations that donate electrons to the. The sea of electrons are shared by all atoms and can move throughout the structure. Properties: o Thermal Conductivity o Electrical Conductivity o Malleability the ability to be hammered down into thin sheets. o Ductility the ability to be drawn into a wire. When a metal bonds with a nonmetal, an Ionic Bonds bond is formed. A positive ion is called a. A negative ion is called an. An ionic bond always involves the TRANSFER of electrons from the. The cation and anion are held together by. to the An ionic compound does not consist of individual molecules. Instead, there is a huge network of positive and negative ions that are packed together in a. Because their bonds are so strong, ionic compounds tend to have very points. Ionic compounds are, which means they can conduct. melting When forming ionic compounds the positive and negative charges must. CrissCross rule Balancing Charges 1. Write out symbols and charge of elements 2. CrissCross charges as subscripts 3. Combine as a formula unit Equation Form of Balancing Charges (Number of Cations)x(Cation Charge) + (Number of Anions)x(Anion Charge) = 0 (1)(+3) + (X)(1) = 0, x = 3 Unit 6: Bonding and Nomenclature Page 8
o EX: Aluminum and Oxygen EX: Barium and Oxygen Balancing Charges Practice: o Lithium Iodide o Aluminum Nitride o Strontium Chloride o Sodium Sulfide Ionic Compound Naming Notes To name ionic compounds: o Name the first. o Name the second change the ending to. o Al 2 O 3 o BaCl 2 o Ca 3 N 2 o KF Ionic Compounds with transition metals: o Transition metals and pblock metals can have multiple oxidation states. Silver (Ag) is always +1 Zinc (Zn) is always +2 Cadmium (Cd) is always +2 o Some elements, such as iron, form two or more cations with different charges. We use to indicate the Unit 6: Bonding and Nomenclature Page 9
ion s charge. For example, Fe +2 would be named and Fe +3 would be named. If an element does not form more than one charge, then you do not use a Roman numeral in its name. EX: Iron (III) Oxide PbO 2 Fe 2 S 3 Tin (II) Chloride Practice Iron (III) Nitride Copper (I) Bromide PbCl 2 Co 2 O 3 SnS Circle the correct chemical formula for each compound below. Make sure the positive and negative charges are balanced. o calcium oxide CaO Ca 2 O CaO 2 o magnesium fluoride MgF Mg 2 F MgF 2 o sodium sulfide NaS Na 2 S NaS 2 o barium nitride BaN Ba 2 N 3 Ba 3 N 2 Unit 6: Bonding and Nomenclature Page 10
Ionic Bonding Naming Worksheet Fill in the table below with the correct ionic formula. Write the name of the compound in the box as well. The first one has been done for you as an example. Don t forget that certain cations use Roman numerals in their names. Cl O 2 N 3 Na + NaCl sodium chloride Cu + Cu +2 Mg +2 Al +3 Fe +3 Unit 6: Bonding and Nomenclature Page 11