1. How To Be Successful in Second Semester Chemistry

2. Skills Chances are, you are good at video games, sports, playing an instrument, or some extra curricular activity. But how did you get good at that?

3. Video Games Was anyone born good at video games? Could anyone who has never played Halo or Black Ops beat the last level first try?

4. Video Games So how does someone get good at video games? What happens if you can’t get past a level?

5. The Video Game of Chemistry You are starting the second half of the game of Chemistry. You are Level 4 students. You have 5 more levels to pass before you beat the game

6. The Video Game of Chemistry Games teach us that different choices have different outcomes and we control the choices we make. Your grade is not something that just “happens”. No one is just “good” at chemistry. Some people just have to practice less.

7. The Video Game of Chemistry You have unlimited lives. You have someone who beat the game before to show you pointers. The game is designed to be won.

8. Chemistry Lies “I am just not good at math” “I can just do better on the next test” “It doesn’t matter what I do I always get the same grade on the test” “There is nothing I can do to bring up my grade”

9. Chemistry Truth I strongly believe that everyone here can win this game and have a good grade this semester. I will do everything in my power to make sure that happens.

10. First Semester Review Substances can be classified as elements, compounds, or mixtures. – Elements are substances made of _____type of atom – Compounds are two or more elements chemically combined by sharing or transferring __________. – Mixtures are elements and compounds physically mixed together. Atoms are the smallest part of an element that has the same properties. Atoms are made of _________________________________. one electrons protons, neutrons, and electrons

11. First Semester Review The model of the atom has changed over time as ____________have given us new knowledge about the atom. The periodic table contains all the known elements in the universe. – The periodic table is arranged by atomic number, the number of ___________. – The periodic table is also arranged with all of the elements in the same column have similar properties. – Patterns in the periodic table exist with atomic size and electronegativity. Metals and Nonmetals are separated by the dark zigzag line running through the “p” block. experiments protons

13. First Semester Review Elements make bonds to become more stable by sharing or transferring _______________. – All elements want to have the same number of valence electrons as the ____________________. – Energy is given off when bonds are formed and energy is required to break bonds. Compounds are named using the ionic naming system or the covalent naming system. – Ionic compounds are named using the ________________. FeCl 2 is Iron (II) chloride – Covalent compounds are named using ______________. P 2 O 5 is diphosphorus pentoxide electrons noble gases ion sheet prefixes

14. Ch. 8 Notes -- Chemical Reactions Chemical equations give information in two major areas: 1. _____________ and ______________ of the reaction. 2. Coefficients of a balanced chemical equation tell us the ______ of the substances involved. Example of a Balanced Chemical Equation: 2H 2 (g) + O 2 (g)  2H 2 O (g) Reactants are on the ______ side of the arrow, and the products are on the __________ side. The arrow means “________”, or “reacts to produce” when read aloud. From our example, hydrogen reacts with oxygen in a ___:___ ratio. The coefficients represent either the number of _________ or molecules present. Reactantsproducts amount left yieldsright 2 1 moles

15. Remember, the number of atoms of each element must be ___________ on both sides. Example: __ H 2 + __O 2  __H 2 O Balancing Chemical Equations equal 212

16. Six General Types of Reactions 1) ________________________: A reaction that breaks apart ______ ______________ into simpler substances, (usually two elements or an element and a smaller compound.) General Form:_____  ___ + ___ Examples: H 2 O  _____ + _____ KCl  _____ + _____ Remember that “HONClBrIF” elements are diatomic when alone!! Decomposition one compound AX H2H2 O2O2 + KCl 2

17. 2) _______________: (sometimes called “Combination” or “Synthesis”) A reaction of _____ __________________, typically a metal and a nonmetal to form ______ ______________. It is the opposite of decomposition. General Form: ___ + ___  _____ Examples: Al + Cl 2  _______ K + S  ___ General Types of Reactions (Continued) Composition two substances one compound AXAX + AlCl 3 K2SK2S

18. 3) _____________ Replacement: A reaction between ____ ______________ and ___ ____________ that produces a different _____________ and ______________. General Forms: ____ + __  ____ + __ ____ + __  ____ + __ The element that is trying to replace the other must be ________ _______________ than the one it is replacing. You must use the Activity Series to see if the reaction will happen. Activity Series _________ ___ = more reactive Elements from ____ to ____ can displace hydrogen in water to form a metallic hydroxide and H 2 gas. General Types of Reactions (Continued) Single one compoundone element compoundelement Y B X A AXAY BXAX more reactive Higher up LiNa + +

19. Activity Series

20. Single Replacement Reactions Examples: NaCl + F 2  _____ + _____ FeCl 2 + K  _____ + _____ HCl + Zn  _____ + _____ HCl + Au  _____ + _____ H 2 O + Na  _____ + _____ AgNO 3 + Cu  _____ + _____ H(OH) NaF Cl 2 KCl Fe ZnCl 2 H 2 No Reaction NaOH H 2 CuNO 3 Ag

21. 4) _______________ Replacement: (sometimes called “Ionic”) A reaction between _____ ________________ that are dissolved in water that produces _____ ________________, one of which is ________________. Water or a gas may be one of the two compounds being produced. General Form: ____ + ____  ____ + ____ You must use the Solubility Chart to see which product is the precipitate. Solubility Chart ___ or _____= precipitate Examples: CaCl 2 (aq) + AgNO 3 (aq)  _________ + ________ NaOH (aq) + HCl (aq)  ________ + ________ General Types of Reactions (Continued) Double two compounds insoluble AX (aq) BY (aq) AY (aq) BX (s) IsS ++ Ca(NO 3 ) 2 (aq) AgCl (s) NaCl (aq) H 2 O (l)

22. General Types of Reactions (Continued) 5) _________________: A reaction between a Carbon/Hydrogen (and sometimes Oxygen) _________________ with _____. The products are always the same… ________ + ________ This reaction is too easy!! Don’t miss it! General Form: C x H y + O 2  ____ + ____ Examples: C 2 H 2 + O 2  _______ + _______ C 7 H 6 O + O 2  _______ + _______ Combustion compound O2O2 CO 2 H2OH2O H2OH2O H2OH2O H2OH2O

23. General Types of Reactions (Continued) 6) _________________: There are two types of Nuclear reactions, ________________ –Fission reactions involve a heavy nucleus that will split into two or three pieces. –Fusion reactions involve two light nuclei that combine into a heavier one. –New elements are formed! You will not be asked to predict products! Examples of nuclear fission reactions: Nuclear Fission and Fusion Nuclear Weapons (atom bomb)

24. General Types of Reactions (Continued) More examples of nuclear fission reactions: Nuclear Medicine /Medical Imaging Nuclear Power Plants

25. General Types of Reactions (Continued) Examples of nuclear Fusion reactions: Hydrogen on the sun becomes Helium Fusion