sc.912.p.10.1 the student will be able to perform calorimetric calculations to determine how much...

SC.912.P.10.1The student will be able to perform calorimetric calculationsto 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 OC

∆ T = Tfinal - T initial

Example

The specific heat of copper is 0.385 J/goC. When 5.0g of copper are heated from 22oC to 35oC how many joules of energy are used?

SC.912.P.10.1the 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.

Energy is stored in chemical bondsin every compound or moleculeBreaking bonds uses

energyMaking bonds releases energy

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)

In chemical reactions…

Energy is converted from chemical (bond energy) to thermal and/or sound and/or light energy.

Consider the energy changes in this process

SC.912.P.12.10student 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

SC.912.P.12.10the student addresses the properties of gases based on kinetic molecular theory

https://www.youtube.com/watch?v=_rsqBNhFG1Y

SC.912.P.8.8the 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 + O2 CO2 + H2O

Classify

1. CaCO3 CaO + CO2

2. P4 + 3 O2 2 P2O3

3. P4 + 3 O2 2 P2O3

4. C6H12 + 9 O2 6 CO2 + 6 H2O

5. Pb + FeSO4 PbSO4 + Fe

SC.912.P.8.8the student recognizes if a single replacement reaction occurs based on the activity series for metal and halogens

2 AlCl3 + 3 Pb 2 Al + 3 PbCl2 Will this reaction proceed?

Will this reaction proceed?3FeCl2 + 2 Al 2 Al Cl3 + 3Fe

SC.912.P.8.7The student will be able to properly name and write formulas for ionic and covalent bonds

CO2 carbon dioxide

CO carbon monoxide

SO2 _______________ N2 O3 _______________

IF7 ________________ SF6____________________

SC.912.P.8.7The student will be able to properly name and write formulas for ionic and covalent bonds KCl potassium chloride

MgS magnesium sulfide

Ca3 P2 ________________ Ba2N3 _____________________

Al2 O3 ________________

SC.912.P.8.7The 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

SC.912.P.8.7The 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 _________________

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

water

Lewis dot diagrams

ExceptionNot followingOCTET rule

Hydrogen peroxide

SC.912.P.12.13the student will demonstrate Le Chatelier’s Principle by determining the direction of shift that occurs

H 2 + I 2 ⇄ 2HIWhat change in reaction will occurIf HI was added?

N 2 + 3H 2 ⇄ 2NH 3 

What change in reaction will occurIf H2 was added?

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