sc.912.p.10.1 the student will be able to perform calorimetric calculations to determine how much...
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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
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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?
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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.
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Energy is stored in chemical bondsin every compound or moleculeBreaking bonds uses
energyMaking bonds releases energy
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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)
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In chemical reactions…
Energy is converted from chemical (bond energy) to thermal and/or sound and/or light energy.
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Consider the energy changes in this process
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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
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SC.912.P.12.10the student addresses the properties of gases based on kinetic molecular theory
https://www.youtube.com/watch?v=_rsqBNhFG1Y
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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
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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
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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?
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Will this reaction proceed?3FeCl2 + 2 Al 2 Al Cl3 + 3Fe
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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____________________
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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 ________________
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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
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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 _________________
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SC.912.P.8.7The student will be able to draw and identify Lewis dot diagrams
water
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Lewis dot diagrams
ExceptionNot followingOCTET rule
Hydrogen peroxide
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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?
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SC.912.P.12.13The student understands what dynamic equilibrium is