In groups discuss: How would you define a compound? Use some key vocabulary terms from the first chemistry test to help you. If H2O and H2O2 are both compounds, how are they different? How do atoms combine to form compounds? How do ionic bonds and covalent bonds differ? How are they the same? Think back to our global warming project. What compounds (greenhouse gases) have we already studied? Explain how the electrons move in order for each of the greenhouse gases to form. Label each greenhouse gas as an ionic or covalent bond.

Adapted from http://sciencespot.net/ Bonding Basics 8th Grade Science Adapted from http://sciencespot.net/

Section A: Complete the chart using a periodic table to help you.

NEGATIVE POSITIVE ION CATION ANION Answer these questions: An atom that gains one or more electrons will have a ____________________ charge. An atom that loses one or more electrons will have a ____________________ charge. An atom that gains or loses one or more electrons is called an ____________. A positive ion is called a ______________ and a negative ion is called an _______________. NEGATIVE POSITIVE ION CATION ANION “An-Eye-On” “Cat-Eye-On”

ELECTRONS COMPLETE METAL NONMETAL What is an ionic bond? Atoms will transfer one or more ________________ to another to form the bond. Each atom is left with a ________________ outer shell. An ionic bond forms between a ___________ ion with a positive charge and a ________________ ion with a negative charge. Example B1: Sodium + Chlorine Example B2: Magnesium + Iodine ELECTRONS COMPLETE METAL NONMETAL

Example B3: Potassium + Iodine Example B4: Sodium + Oxygen Example B5: Calcium + Chlorine Example B6: Aluminum + Chlorine

SHARE COMPLETE NONMETAL What is a covalent bond? Atoms ___________ one or more electrons with each other to form the bond. Each atom is left with a ________________ outer shell. A covalent bond forms between two _________________. Example C1: Hydrogen + Hydrogen Example C2: 2 Hydrogen + Oxygen SHARE COMPLETE NONMETAL

Example C3: Chlorine + Chlorine Example C4: Oxygen + Oxygen Example C5: Carbon + 2 Oxygen Example C6: Carbon + 4 Hydrogen

Review Vocab… What is an oxidation number? How is it determined? What is a subscript? What does it tell you about the atoms in the compound? What is a chemical formula?

Oxidation Numbers Same thing as typical charge an atom will have once it has lost or gained electrons Shortcut to writing chemical formulas: 1. Ca I 2. Ca+2 I1- 3. Ca+2 I1- Ca1 I2 CaI2

Bond With A Classmate Purple = Cations ; Pink = Anions Find a classmate to “bond” with and together decide on the correct chemical formula (use the oxidation numbers to help you!) You will have to decide how many of each ion you need to make a STABLE IONIC BOND. Record all bonds on your Date Book (data table) Look at the box on your paper for helpful hints You will have 5 minutes to make as many bonds as possible.

Oxidation #’s Backwards Give me the oxidation state (charge) for each atom in the compound for the following chemical formulas:No Periodic Tables Allowed! BaCl2 CaF2 Mg3N2 MgBr2 KCl K2O

What’s in a Name? Naming Compounds

Compound Naming- 3 minutes Separate the cards into 2 groups: 1 group = (18 cards) with exactly 2 elements 1 group = (6 cards) with more than 2 elements Keep the group of 6 separated

Card Sorting – 5 minutes How do you tell the difference between ionic and covalent compounds? Identify 6 cards that have only two elements that have formed a covalent bond (look in your group of 18) 3. Similar to #1 how are ionic different than covalent? Once I have approved those 6, set them back in the bag

Discuss (only) in groups What are transition metals? How are they different from metalloids? Find 6 compounds that start with a transition metal

Ionic group #1 Transition elements: 5 minutes Answer #1-4 Copy the chemical formulas exactly as they appear on your cards. Copy the compound name exactly as it appears on the card (THE ROMAN NUMERAL TOO!!!!) What pattern in the names of the compounds do see for the cation and for the anion? We will fill out #6 together 

Ionic group #1 Transition Metals 6. Give me the oxidation state (charge) for each atom in the compound for the following chemical formulas:No Periodic Tables Allowed! V2O5 Cu3As FeBr2 Fe2O3 PbO VF4

Ionic group #1 7. How are the names of compounds containing transition metals related to the oxidation state of the cation?

Transition Metal + Nonmetal Patterns Cation = (+) Roman numeral = cation charge Metal name is unchanged Anion= (-) Change ending to -ide

Ionic Group # 2 Polyatomic Ions Find the 6 cards that contain more than two elements and fill in the blanks for #8 We will do #9 together Red = cation Black = anion

Polyatomic Ions Find the 2 compounds that contain a polyatomic ion for the cation and for the anion

Polyatomic + Polyatomic Cation Only NH4+ Anion Name = polyatomic ion chart

Metal + Polyatomic Find the 3 compounds that contain a metal ion for the cation and a polyatomic for the anion

Name = Name as it appears on periodic table Anion Metal + Polyatomic Cation Metal Name = Name as it appears on periodic table Anion Name = polyatomic ion chart

Polyatomic + Nonmetal Find the 1 compound that contain a polyatomic ion for the cation and a nonmetal for the anion

Cation Only NH4+ Anion Name = nonmetal Change ending to -ide Polyatomic + Nonmetal Cation Only NH4+ Anion Name = nonmetal Change ending to -ide

Transition Metal + Polyatomic Do you have any cards that have a transition metal for the cation and a polyatomic ion for the anion?

Transition Metal + Polyatomic Cation Roman numeral = cation charge Metal name is unchanged Anion Name = polyatomic ion chart

What are the patterns in naming the cation and anion? Metal and Nonmetal Find the 6 cards that have just one metal (not transition) and one non metal What are the patterns in naming the cation and anion?

Anion Name = nonmetal Change ending to -ide Cation Metal Metal and Nonmetal Cation Metal Name = Name as it appears on periodic table Anion Name = nonmetal Change ending to -ide

Naming Ionic Compounds For #1-20 Write a P to the left of the # if the compound contains a polyatomic ion Write a T to the left of the # if the compound contains a transition metal Write MNM if the compound is a metal and a nonmetal

Name that Compound… NaCl NaCO3 NaOH NH4OH Fe2(SO4)3

Show me the formula Ammonium Chloride Potassium Nitrate Calcium hydroxide Sodium Oxide Copper (II) Sulfate

Naming Ionic Compounds Metal and nonmetal: Name the metal and change the nonmetal to –ide Transition metals and nonmetals: Use roman numerals to represent the charge and name the nonmetal using –ide Polyatomic Ions : If positive are more like metals and come first, if negative are more like nonmetals and come second. They have their own names and oxidation numbers (see chart on back)

More Polyatomics...

Polyatomic ions Kinda annoying But super cool when you react them together and light them on FIRE!!! COOL VIDEO OF ammonium dichromate and mercury thiocyanide We’ll watch it if you can write the correct chemical formula for each!

Naming Ionic Bonds Practice What is the chemical formula for the compound that results when Magnesium and Chlorine combine? Use the lewis dot structures and the criss cross method to show how you get the same formula. How do you name this compound?

Compound Naming How do you tell the difference between ionic and covalent compounds? Identify 6 cards that have only two elements that have formed a covalent bond Once I have approved those, fill out #1-5 on your naming notes sheet

Naming Covalent Compounds Guidelines for Inorganic Compounds 1 Mono- 2 Di- 3 Tri- 4 Tetra- 5 Penta- 6 Hexa- 7 Hepta- 8 Octa- 9 Nona- 10 Deca- In covalent compounds, the least electronegative element comes first and its name is unchanged. 2. The more electronegative element comes second and takes on the –ide ending like in ionic bonds Subscripts are represented by Greek prefixes Example: H2O –dihydrogen monoxide

Name that Compound Can you use the inorganic guidelines for all of these? 4. CH4

Show me the formula hexaboron monosilicide chlorine dioxide hydrogen monoiodide iodine pentafluoride dinitrogen monoxide