1. SC.912.P.10.1 The student will be able to perform calorimetric calculations to determine how much heat is absorbed or released. q = m c ∆T q = heat in Joules (J) m = mass in grams (g) c = specific heat constant J/g O C ∆ T = T final - T initial

2. Example  The specific heat of copper is 0.385 J/g o C. When 5.0g of copper are heated from 22 o C to 35 o C how many joules of energy are used?

3. SC.912.P.10.1 the student will be able to relate the behavior and kinetic energy of a molecule with the temperature of the substance  Energy is neither created nor destroyed only transferred from one form into another.

4. Energy is stored in chemical bonds in every compound or molecule  Breaking bonds uses energy Making bonds releases energy

5. Heat of fusion  When water freezes bonds are made between water molecules Therefore the process is exothermic (releases energy)  When ice melts bonds between water molecules are broken Therefore the process is endothermic (requires energy)

6. In chemical reactions…  Energy is converted from chemical (bond energy) to thermal and/or sound and/or light energy.

7. Consider the energy changes in this process

8. SC.912.P.12.10 student interpret relationship between the properties such as pressure, volume and temperature as explained by various gas laws  Boyles Law: If pressure goes up, volume goes down  Charles’ Law: if volume goes up, temperature goes up  Gay Lussac’s Law: if temperature goes up, pressure goes up

9. SC.912.P.12.10 the student addresses the properties of gases based on kinetic molecular theory  https://www.youtube.com/watch?v=_rsqBNhFG1Y https://www.youtube.com/watch?v=_rsqBNhFG1Y

10. SC.912.P.8.8 the student will be able to classify different types of reactions  Synthesis Reaction : A + B  AB  Decomposition reaction : AB  A + B  Single replacement reaction: A + BC  AC + B  Double replacement reaction: AB + CD  AD + CB  Combustion reaction: Carbon compound + O 2  CO 2 + H 2 O

11. Classify 1. CaCO 3  CaO + CO 2 2. P 4 + 3 O 2  2 P 2 O 3 3. P 4 + 3 O 2  2 P 2 O 3 4. C 6 H 12 + 9 O 2  6 CO 2 + 6 H 2 O 5. Pb + FeSO 4  PbSO 4 + Fe

12. SC.912.P.8.8 the student recognizes if a single replacement reaction occurs based on the activity series for metal and halogens  2 AlCl 3 + 3 Pb  2 Al + 3 PbCl 2 Will this reaction proceed?

13. Will this reaction proceed? 3FeCl 2 + 2 Al  2 Al Cl 3 + 3Fe

14. SC.912.P.8.7 The student will be able to properly name and write formulas for ionic and covalent bonds  CO 2 carbon dioxide  CO carbon monoxide  SO 2 _______________N 2 O 3 _______________  IF 7 ________________ SF 6 ____________________

15. SC.912.P.8.7 The student will be able to properly name and write formulas for ionic and covalent bonds  KClpotassium chloride  MgSmagnesium sulfide  Ca 3 P 2 ________________Ba 2 N 3 _____________________  Al 2 O 3 ________________

16. SC.912.P.8.7 The student will be able to properly name and write formulas for ionic and covalent bonds Write the formulas: Calcium and oxygen Magnesium and nitrogen Sodium and sulfur

17. SC.912.P.8.7 The student will be able to properly name and write formulas for ionic and covalent bonds Transition metal use Roman Numerals Write the formula for the following: Iron II oxide _________________ Copper I sulfide _________________

18. SC.912.P.8.7 The student will be able to draw and identify Lewis dot diagrams water

19. Lewis dot diagrams Exception Not following OCTET rule Hydrogen peroxide

20. SC.912.P.12.13 the student will demonstrate Le Chatelier’s Principle by determining the direction of shift that occurs H 2 + I 2 ⇄ 2HI What change in reaction will occur If HI was added? N 2 + 3H 2 ⇄ 2NH 3 What change in reaction will occur If H 2 was added?

21. SC.912.P.12.13 The student understands what dynamic equilibrium is