Download Lesson Plans - University High School

Lesson Plans
Subject: Hon. Chemistry
Teacher: Saylor
Week of: April 1
Measurement
Topic
Monday
Tuesday
Unit 11: States of
Matter
Unit 11: States of
Matter
Wednesday
Thursday
Unit 11: States of Matter
Unit 11: States of Matter
Friday
Unit 11: States of
Matter
NGSSS Benchmarks grouped and assessed in this topic:
Benchmark(s)
Kinetic Molecular
Theory
Learning Target
Kinetic Molecular
Theory
apply kineticmolecular theory and
intermolecular forces
of attraction to
explain the different
properties of solids,
liquids, and gasesdefinite/indefinite
shape and volume,
density ,
compressibility,
fluidity, viscosity
apply kineticmolecular theory and
intermolecular forces
of attraction to
explain the different
properties of solids,
liquids, and gasesdefinite/indefinite
shape and volume,
density ,
compressibility,
fluidity, viscosity
differentiate among
the four states of
matter in terms of
particle distance,
particle motion, and
definite/indefinite
shapes and volumes
differentiate among
the four states of
matter in terms of
particle distance,
particle motion, and
definite/indefinite
shapes and volumes
Heat vs.Temp
Intermolecular Forces of
Attraction
describe heat as the
flow of energy from
objects of higher to
lower temperature
apply kinetic-molecular
theory and
intermolecular forces of
attraction to explain the
different properties of
solids, liquids, and gases
○
definite/indefinite shape
and volume, density ,
compressibility, fluidity,
viscosity
differentiate between
intramolecular forces
(bonds – ionic, covalent,
Phase Diagram
define heat of fusion
(ΔHfus) and heat of
vaporization (ΔHvap) and
identify their respective
regions on a heating
curve
calculate the amount of
heat absorbed or
released based on a
liquid’s temperature
change using the
equation: q = mcΔT
interpret the phase
diagram of a substance
including the triple point
and critical point
predict the effect of
temperature or pressure
changes on the phase of
Calorimetry
Students learn to
calculate heat of
combustions using
calorimetry.
metallic) in chemical
reactions and
intermolecular forces in
phase changes
Lesson
1. Students rewrite
the 5 postulates of
KMT in their own
words
2. Students crush a
soda can using air
pressure, then
write an essay
describing the
changes of state
and transfer of
energy in
explaining the
science behind the
implosion.
1. Students complete 1. Students review
an essay
intermolecular
describing the
forces of attraction
endothermic
nature of melting 2. Demonstration of
and evaporation.
heat of reaction
3. Students
/high specific heat
complete a
capacity of water
vocabulary
(burning dollar)
exercise on states
demo
of matter and take
a 10 question quiz 3. Students view 2 film
over matter.
clips to review the
concept of hydrogen
bonding.
4. Students use models
of water molecules
to answer a series of
questions about
water.
Assessment (D,F,S)
Formative- Essay on
Implosion
Formative- Essay on
melting and
evaporation
Formative- Water
Activity questions
NSpire Quiz- Heat vs.
a substance using a
phase diagram
1.
Students take
notes on heat
calculations
using
q = mf
q = mHv and
1. Lab ExperimentHeat of Combustion
of Foods
The heat released by
burning a peanut,
cheese puff and
marshmellow is
determined using
calorimetry.
q= m x C x 

Students take
note on phase
diagrams and learn
to identify the
regions for solid,
liquid, gas, melting,
boiling, normal
melting point,
normal boiling point,
triple point, and
critical temperature.
Formative- Lab report
on heat of
combustion- students
must turn in the data,
Temperature
calculations, and
conclusions for the
experiment
Formative- NSpire
quiz over phase
diagrams.
Learning Target Unit 11 States of Matter
differentiate among the four states of matter in terms of particle distance, particle motion, and
definite/indefinite shapes and volumes
describe temperature as a measure of the average kinetic energy of the particles in a substance
describe matter at absolute zero (0 K)
apply kinetic-molecular theory and intermolecular forces of attraction to explain the different
properties of solids, liquids, and gases
○ definite/indefinite shape and volume, density , compressibility, fluidity, viscosity
describe three intermolecular forces in terms of their causes and relative strengths of attraction
(dispersion forces, dipole-dipole forces, hydrogen bonds) (Honors)
differentiate between intramolecular forces (bonds – ionic, covalent, metallic) in chemical reactions
and intermolecular forces in phase changes
relate stronger intermolecular forces with higher boiling and melting points
describe heat as the flow of energy from objects of higher to lower temperature
explain the role of added or released energy in phase changes
interpret heating/cooling curves in terms of heat absorbed/released, temperature changes, phase
changes, and regions where PE or KE is changing
define heat of fusion (ΔHfus) and heat of vaporization (ΔHvap) and identify their respective regions on a
heating curve (Honors)
calculate the amount of heat absorbed or released based on a liquid’s temperature change using the
equation: q = mcΔT (Honors)
describe phase changes as examples of dynamic equilibrium as a reversible process dependent upon
energy being absorbed or released:
○ melting-freezing or vaporization-condensation
describe phase transitions in terms of kinetic-molecular theory (molecular motion) and intermolecular
forces (attractions)
interpret the phase diagram of a substance including the triple point and critical point (Honors)
predict the effect of temperature or pressure changes on the phase of a substance using a phase
diagram (Honors)
recognize hydrogen bonding as an intermolecular force in water as the source of its special physical
properties (surface tension, cohesion/adhesion, high boiling point, high specific heat capacity (Honors),
liquid/solid density, “universal” solvent) making it suitable for life
Vocabulary
Temperature- A measure of the AVERAGE KINETIC ENERGY of a sample (measured in oC or K)
Heat- thermal energy (measured in Joules)
Celcius- A temperature scale based on the freezing point (0oC) and the boiling point of H2O (100 oC).
Kelvin- The absolute temperature scale. K = oC + 273
Absolute Zero (0 K)- The temperature at which ALL MOLECULAR MOTION CEASES. 0 K = - 273 oC
Heat flow- Heat always flows from an area of high temperature into an area of lower temperature.
Endothermic- A process that ABSORBS HEAT from the surroundings.
Solid
Liquid
Gas
Exothermic- A process that RELEASES HEAT into the surrounding.
Gas
Liquid
Solid
Kinetic Molecular Theory- Molecules are in constant, continuous motion. The temperature of the sample reflects the average KE of the molecules in the sample.
Intermolecular Forces of Attraction- The attraction of one molecule for its neighbor.
Weakest to strongest…
London dispersion force
(caused by motion of electrons)
<
dipole-dipole forces
(caused by the + and – ends of polar molecules
< Hydrogen bonds
( H-N, H-O, H-F)
Heating or Cooling Curve- A graph of temperature versus time
Freezing point- The temperature where a liquid becomes a solid. The temperature remains constant until freezing is complete.
Boiling point- The temp. at which a liquid becomes a gas. Again, once a substance reaches its boiling point, the temperature will level off and remain constant
while the liquid boils.
Heat of fusion- The amount of heat needed to melt material while it is at it melting point.
H fusion (ice) = 334 J/g
334 Joules of heat must be absorbed to melt each gram of ice.
Heat of Vaporization- The amount of heat needed to vaporize the material once it is at its boiling point.
H vaporization (water) = 2260 J/g
2,260 Joules of heat must be absorbed to boil each gram of water.
Heat capacity- The amount of heat needed to raise the temperature of 1 g of substance by 1oC.
Water has one of the HIGHEST heat capacities known. 4.184 J/goC. = Cp water= 1 calorie/gram
Phase Diagram- A plot of pressure versus temperature. The graph shows conditions for the solid, liquid, and gas phases.
Triple point- The point (temp and pressure) where solid, liquid and gas can coexist simultaneously.
Critical point- Above this temperature, liquid can no longer exist.