Bell Ringer How many groups are on the periodic table? How many periods are on the periodic table? How many elements are on the current periodic table? Elements on the left of the staircase are classified as what? Elements on the staircase are classified as what, because? Elements on the right of the staircase are classified as what?

Chemical Bonds Chapter 6

Making bonds Bonding gives the molecule completely different chemical properties than its parent elements. Ex: Salt (NaCl) Sodium is a metal that is violently reactive with water.  Chlorine is a highly toxic, greenish-colored gas.  Bonding stabilizes these two elements.

Valence Electrons Valence electron: an electron that is in the highest occupied energy level of an atom -Each Valence e- has an e- charge Group # = Valence # Think about your Bohr Model

Valence e- and e- charges All valence electrons have charges Group# valence e- e-charge Group1A Group2A Group3A Group4A Group5A Group6A Group7A Group8A

Visualize and Understand the Relationship Be O

Bonding Atoms bond between their _________ e- Represented in a ___________ dot diagram. This show the relationship of bonding between elements.

Electron Configuration ***Valence Electrons in the highest energy level*** Group A 1, 2, 3-8 Electron Dot Diagrams show the number of valence electrons Write the symbol Place a LARGE dot for each valence electron 1 dot on each side before pairing them up end

Electron Configuration end

Electron Configuration Draw diagrams for the following: Sr How many Valence electrons? What is the charge of this electron? end

Draw diagrams for the following: Si How many Valence electrons? What is the charge of this electron?

Draw diagrams for the following: Cl How many Valence electrons? What is the charge of this electron?

Lewis Dot Diagram Fill in your Lewis Dot Structure Worksheet.

E- charges Most metals have _______ charges Most non-metals have a _______ charge L of staircase mostly (___) charge R of staircase mostly (___) charge

Metals and Non Metals, with only a few electrons in the outer energy level, tend to ____ electrons  Non-metals, which lack only one or two electrons in the outer energy level have a tendency to _____ electrons.

Chemical Formulas

Chemical Formulas Chemical Formula NaCl CO2 MgCl2 Na3P Subscripts show the number of atoms of each element in the compound 1 atom = No Subscript! NaCl CO2 MgCl2 Na3P end

Chemical Formulas How many total atoms are in each of these: TRY ON YOUR OWN! H2SO4 KNO3 Fe2O3 Hg2Cl2 end

On your Own Worksheet Problems 1-8 Label the element and the # of atoms

Chemical Formulas Polyatomic Ions OH-, PO43- Last page of your Reference Tables!!! More than 1 Polyatomic Ion = Write inside ( ) Put a subscript OUTSIDE end

Chemical Formulas Ba(OH)2 Cu (NO3)2 NH4NO3 (NH4)2O

Chemical Formulas How many total atoms are in each of these: Cu(NO3)2 end

How many total atoms are in each of these: KMnO4

How many total atoms are in each of these: Al2(SO4)3

How many total atoms are in each of these: (NH4)3PO4

How many total atoms are in each of these: Mg(C2H3O2)2

Counting Atoms Worksheet 1-9

Worksheet On Back of Worksheet Identify and Count Atoms Grab a book and copy onto your worksheet or a separate sheet of paper the following vocabulary words: Electron Dot Diagram Ion Chemical Bond Chemical Formula Molecule Crystal Polyatomic Ion When you are done, I want to check your work.

Bell Ringer Draw a Lewis Dot Structure for the following elements: F Si Mg What is an ion?

Bonding

Electron Configuration All atoms want 8 valence electrons 8 valence = Stable (DO NOT REACT) Noble Gases To get 8 valence, atoms can either: Transfer Electrons: Lose Electrons to drop an energy level Gain Electrons till they have 8 Share Electrons with other atoms, so everyone has 8 end

Chemical Bonding Chemical Bond 3 types Ionic (Metal and Nonmetal) Covalent (Nonmetal and Nonmetal) Metallic (Metal and Metal) end

Chemical Bonding Identify the following as ionic or covalent CaCl2 LiBr CO2 SO3 H2O CH4 end

Classify on Own BaS4 Na2O3 K2O NaF MgO N4Cl HCl KI

Ionic Bonding Ionic Bonding Cation Anion Metal and Nonmetal (or polyatomic ion) Electrons are TRANSFERRED from the cation to the anion Cation Positive (a Metal) Has Lost Electrons Anion Negative (a Nonmetal) Has Gained Electrons end

Ionic Bonding Ions have the same electrons as Noble Gases Making them stable Metals (Groups 1 to 13) become like the noble gas Before the element Na  Lose 1 e-  Ne Sr  Lose 2 e-  Kr end

Ionic Bonding Changing the # of e- makes the atom an ION Nonmetals (Groups 15 to 17) become like the noble gas After the element O  Gain 2 e-  Ne I  Gain 1 e-  Xe Changing the # of e- makes the atom an ION Has a charge called an Oxidation State end

Ionic Bonding Oxidation States follow the # of Valence Electrons Group: 1 2 13 14 15 16 17 18 Valence e-: 1 2 3 4 5 6 7 8 Oxidation #: +1 +2 +3 ±4 -3 -2 -1 0 end

Ionic Bonding Show the transfer of electrons with an Electron Dot Diagram sodium chloride (NaCl) Na + Cl  [ ]+ [ ]- Na Cl end

Bonding Draw Electron Dot Diagrams for: KF MgO MgCl2 end

Bonding On Own Complete Diagram Worksheet

Periodic Table Activity Online to Complete in place of article assignment this week!

Bell Ringer Draw and electron diagram for Table Salt. What is a bond between a metal and non-metal called? What is a bond between two non-metals called? What is a cation? What is an anion? Lab Safety Tip #

Naming Ionic Compound Naming Ionic Compounds: 3 steps Name the Cation (the metal) Name the Anion (the nonmetal) Change the Ending on the anion to –ide IGNORE THE SUBSCRIPTS!!! NaBr Sodium Bromine Sodium Bromide end

Naming Ionic Compounds Name the following: BaS MgF2 Ca3N2 end

Naming Ionic Compounds Complete the following on “Names of Ionic Compounds’ worksheet 1 9 2 13 8 16 6 18 8 19 25

Naming Ionic Compounds More than 2 elements = POLYATOMIC ION!!! LOOK AT YOUR REFERENCE TABLE!!! Follow the same steps to name the compound Get the polyatomic’s name from the reference tables! DON’T change the ending of a polyatomic ion NaNO3 Sodium Nitrate end

Naming Ionic Compounds Name the following: KOH NaC2H3O2 (NH4)2O Sr3(PO4)2 end

Naming Ionic Compounds Complete on “Names of Ionic Compounds” # 3, 4, 5, 7, 11, 12, 14, 15, 17, 21, 24

Writing Ionic Formulas Writing formulas: 3 steps: Write the positive ion, with charge Write the negative ion, with charge Cross the charges to get subscripts Do NOT put the “+” or “-” end

Writing Ionic Formulas Write the formulas for the following: Beryllium Phosphide Calcium Fluoride Lithium Iodide Strontium Sulfide end

Writing Ionic Compounds Complete numbers 1-10 on “Writing Binary Formulas”

Writing Ionic Formulas Remember: Polyatomic Ions ARE A GROUP When you cross charges, the subscript applies to the WHOLE GROUP USE ( ) end

Writing Ionic Formulas Write the formula for the following: Potassium Nitrate Barium Chromate Aluminum Acetate Ammonium Sulfate end

Transition Metals Transition Metals have 2 valence electrons But they have Many Oxidation States So we write their names differently end

Transition Metals Follow the same steps to write the formula The metal's charge is the Roman Numeral Vanadium (III) Sulfide V3+ S2- V2S3 Metal's Charge end

Transition Metals Write formulas for the following: Osmium (V) Fluoride Silver (I) Nitride Technetium (VII) Phosphate end

Transition Metals When naming you MUST put the charge as a Roman Numeral! To figure out the charge, uncross the subscripts! Fe2O3 Fe3+ O2- iron (III) oxide end

Transition Metals Name the following: HgF2 Hf2S5 Y3P7 end

Naming Ionic Compounds Complete the following on “Naming Binary Compounds (Ionic)” 3 12 4 13 5 16 6 19 7 20

Bell Ringer Silver (I) oxide Copper (I) bromide Copper (II) bromide Iron (II) oxide Iron (III) oxide Chromium (II) chloride Chromium (III) chloride Mercury (I) Iodide Manganese (II) oxide

Covalent Bonding Naming and Writing Formulas

Covalent Bonding Covalent Bond Nonmetal and Nonmetal Atoms SHARE electrons 7 nonmetals that never exist by themselves. Form pairs with each other Called Diatomics (H, N, O, F, Cl, Br, I) end

Covalent Bonding The number of electrons shared create different types of bonds 2 shared electrons — single bond 4 shared electrons = double bond 6 shared electrons ≡ triple bond end

Naming Covalent Molecules Number Prefix 1 Mono- 2 Di- 3 Tri- 4 Tetra- 5 Penta- 6 Hexa- 7 Hepta- 8 Octa- 9 Nona- 10 Deca- When naming Covalent Molecules: Use a prefix for the first element If it is 1, do NOT use a prefix Name the first element Use a prefix for the second element Always!!! Name the second element AND change the ending to –ide end

Naming Covalent Molecules Practice: As2O3 N2H4 CCl4 SO end

Naming Covalent Molecules Complete 9-16 on “Naming Covalent Compounds” SKIP #4

Writing Covalent Formulas Writing formulas: Write the symbol of the first element Use the prefix for the subscript Write the symbol of the second element end

Formulas of Covalent Molecules Practice: Disulfur trioxide Dinitrogen monoxide Phosphorus pentachloride Diphosphorus pentoxide Carbon dioxide end

Complete 'Naming Covalent Compounds Worksheet' 1-8

Try 1-20 on your own under Formulas and Nomenclature of Covalent Compounds

USE YOUR EDUCREATION APP MIXED REVIEW USE YOUR EDUCREATION APP

Finish 21-40 on Front of worksheet On the Back Complete the chapeter review problems from the book, when you are done, turn it into the box! IF TIME…WORK ON BONDING DRY LAB