Name: Na 2 O _____________________ BaS _____________________ CO 2 _____________________ NF 3 _____________________ Sodium Oxide Barium Sulfide Carbon Dioxide Nitrogen Triflouride

Take Out Homework 1.Which ones would conduct electricity? Ionic Compounds- Na 2 O, BaS 2.Which ones are not very hard, and have an easier bond to break? Covalent Compounds CO 2, NF 3 Na 2 O

Those with Phys Science Book with Satellite Dish 1.Go to page Answer: Why do atoms combine? 2.Explain the 2 types of covalent bonds (polar and non-polar) 3.Go to page 616 – what are the charges (oxidation numbers) for transition metals Copper (I), Iron (III) and Lead (II)? 4. Go to p. 626 Do Write out the word and the phrase for 1-10 Just answer 11-18, no need to write it out Those with Phys Science Book with Roller Coaster 1.Go to page Answer: Why do atoms combine? 2.Explain the 2 types of covalent bonds (polar and non-polar) 3.Go to page 315 – what are the charges (oxidation numbers) for transition metals Copper (I), Iron (III) and Lead (II)? 4. Go to p. 321 Do Write out the word and the phrase for 1-10 Go to page 322 answer 1-10 (answer only)

Things to know for the quiz tomorrow… Know differences between Ionic and Covalent bonds Melting points, electricity conduction, which elements know that metallic bonds are bonds between metals only Know what covalent bonds look like when sharing electrons with dot diagrams Be able to identify correct formula for an ionic bond, you need to memorize the charges in groups 1, 2, 13, 15, 16, 17 Be able to identify correct formula and names of covalent bonds

Tips on Ionic and Covalent Compounds– stuff in your notes… Ionic or Covalent? If you only have formula of a compound, see if it contains a metal. Ionic if it has a metal, Covalent if no metals Naming compounds from formulas: Rule for both: 2 nd part ends with “ide” unless it is a polyatomic ion (it keeps its given name) Covalent, you need prefixes: mono, di, tri, tetra… IONIC Formula writing, total + charges must equal total – charges ** Use charge of one ion to decide the subscript of the other one Be +2 P -3 Be 3 P 2

Chemical Reactions Indicators: – Fizzing (gas produced) – Color change – Gets cloudy/precipitant (solid produced) – Heat released or absorbed – Light emitted – Odor changes

Chemical Reactions Reactants  Products H 2 O 2  H 2 O + O 2 – What are the reactants? What are the products?

Chemical Reactions There are 4 kinds of Chemical Reactions that occur: Synthesis Decomposition Single Double Replacement Replacement

Types of Chemical Reactions Synthesis – Two or more reactants are combined to form one product. +

Types of Chemical Reactions Decomposition – One reactant breaks down into two or more products. +

Types of Chemical Reactions Single Replacement – An element and a compound combine. – One element from the reactants replaces another in the products. ++

Types of Chemical Reactions Double replacement – Two compounds combine. – Two elements in the reactants switch places in the products. ++

Chemical Reactions-Practice Identifying Example #1 H 2 + O 2  H 2 O Which is it? Synthesis Decomposition Single Replacement Double Replacement

Chemical Reactions Example #2 Li 3 P  Li + P Which is it? Synthesis Decomposition Single Replacement Double Replacement

Chemical Reactions Example #3 Na + MgCl 2  Mg + NaCl Which is it? Synthesis Decomposition Single Replacement Double Replacement

Chemical Reactions Example #4 SiCl 4 + O 2  SiO + Cl 2 Which is it? Synthesis Decomposition Single Replacement Double Replacement

Chemical Reactions Example #5 C 5 O 3  C + O 2 Which is it? Synthesis Decomposition Single Replacement Double Replacement

Chemical Reactions Example #6 Rb 2 O + AlF 3  RbF + Al 2 O 3 Which is it? Synthesis Decomposition Single Replacement Double Replacement

Chemical Reactions Law of conservation of Matter – Atoms are not created or destroyed – The number of atoms at the START of a reaction, there must be the same number of atoms AFTER the reaction. – Equations must be balanced!

Chemical Reactions Balancing Chemical Equations STEPS: – Count the number of atoms for each element in the reactants and in the products. – Compare the numbers to see if each element is balanced (equal) with itself. – Use WHOLE NUMBER coefficients to “fix” unbalanced elements. Do not change the subscripts!

Chemical Reactions Example #1 H 2 + O 2  H 2 O

Chemical Reactions Example #2 Li 3 P  Li + P

Chemical Reactions Example #3 Na + MgCl 2  Mg + NaCl

Chemical Reactions Example #4 SiCl 4 + O 2  SiO + Cl 2

Chemical Reactions Example #5 C 5 O 3  C + O 2

Chemical Reactions Example #6 Rb 2 O + AlF 3  RbF + Al 2 O 3

Chemical Reactions Example #7 SnO 2 + H 2 → Sn + H 2 O

Chemical Reactions Example #8 Mg(ClO 3 ) 2 + Na  NaClO 3 + Mg

Chemical Reactions Example #9 Al 2 (SO 4 ) 3 + RbF  AlF 3 + Rb 2 SO 4

Chemical Reactions Identify and Balance Al + F 2  AlF 3

Chemical Reactions Identify and Balance Ca(MnO 4 ) 2 + FeCl 4  CaCl 2 + Fe(MnO 4 ) 4

Chemical Reactions Identify and Balance Si 3 O  Si 8 + O 2

Chemical Reactions Identify and balance Cs 2 O + N 2  Cs 3 N + O 2

Welcome Back! Schedule for the week: Monday: Classify types of Chemical Reactions and Balance Chemical Equations Tuesday: Acids and Bases – quick lab and practice more chemical equations Wednesday: Radioactive Decay – review Acids/Bases and Chemical Reactions Thursday: 1 st and 3 rd period: Recap Radioactive Decay: quiz on Chemical Reactions and Acids/Bases REVIEW PACKET –Test Practice Friday 4 th period: Recap Radioactive Decay: quiz on Chemical Reactions and Acids/Bases REVIEW PACKET –Test Practice

Warm Up

Chemical Reactions Law of conservation of Matter – Atoms are not created or destroyed – The number of atoms at the START of a reaction, there must be the same number of atoms AFTER the reaction. – Equations must be balanced!

Chemical Reactions Balancing Chemical Equations STEPS: – Count the number of atoms for each element in the reactants and in the products. – Compare the numbers to see if each element is balanced (equal) with itself. – Use WHOLE NUMBER coefficients to “fix” unbalanced elements. Do not change the subscripts!

Acids and Bases

0 c Draw a Line Like this in the middle of your paper \ STRONGEST NEUTRAL 7

Acids and Bases

0 c Acids and Bases pH scale \ NEUTRAL 7 Acids get weaker as you go toward the #7 Bases get weaker as you go toward the #7 ACIDIC Basic (Alkaline) pH 7

Acids & Bases-pH Scale

Acids properties 1. Conduct electricity (electrolytes) 2. Produce H+ ions 3. Sour taste 4. Corrosive 5. pH values 0-6.9

Acids pH range = Examples: Citric Acids, Gastric Acid, Battery Acid, Sodas, tomatoes, etc. Examples of Formulas: HCl, H 2 SO 4, H 3 PO 4, HNO 3, etc SPOILED MILK Acids

1. Conduct electricity (electrolytes) 2. OH - ions 3. Bitter taste 4. Corrosive 5. Have a slippery feeling (like soap) 6. pH values Bases properties

Bases pH range 7.1 to 14 Examples: Soaps, Cleaning supplies, Hair Relaxers, etc. Examples of Formulas: NaOH, KOH, Mg(OH) 2, Al 3 (OH), NH 3, NH 4 OH Bases

Acids & Bases Neutralization Reactions Only an Acid can neutralize a base Only a Base can neutralize an acid H + comes off of the Acid and OH - comes off of the Base (OH and H make water!) Acid + Base  Water + Salt Ex: HCl + KOH  H 2 O + KCl

NEUTRALIZATION REACTION In your stomach CaCO 3 + 2HCl ==> CaCl 2 (salt) + H2O + CO 2 Hydrchloric ACID

Acid/Base Neutralization HBr + LiOH  _________ + _________ FrOH + HCl  _________ + _________ H 2 S + Mg(OH) 2  ________ + _______ ______ + HF  H KF ______ + CsOH  H CsI

Acids and Bases—Identify Acid, Base, Both or Neutral 1.pH =2 2.HF 3.pH= 7 4.RbOH 5.Ca(OH) 2 6.pH= 9 7.Sour taste 8.Slippery feel 9.Electrolyte 10.pH = pH = 4 12.H 2 SO 4 13.HBr 14.FrOH 15.Corrosive 16.Bitter taste

Acids and Bases-Compare & Contrast