Objectives:
1. I can classify matter into substances and mixtures.
2. I can identify and distinguish between physical and
chemical properties.
3. I can identify and distinguish between the two types of
forces that affect the nature of compounds.
4. I can understand and distinguish between physical and
chemical changes.
5. I can apply energy changes with changes matter
undergoes.
6. I can identify techniques used to separate mixtures.
Chem I: 8.31.15
Infinite Campus:
• Scientific Skills Quiz
Due:
• Elements, Compounds; Mixtures Worksheet
Objectives:
• I can classify matter into substance or mixtures
Homework:
Classifying Matter Worksheet
What is Matter?
• One or more atoms that take up space
and has mass.
Classification of Matter-2nd
Classification of Matter-3rd
Classification of Matter-6th
Elements
Simplest substance
Compounds
• Chemical combination of elements in a fixed
amount (always the same way).
• A compound’s fixed amount is called a
chemical formula.
Ex. Sodium chloride = NaCl
•When elements chemically combine the
compound produced has new properties.
Sodium (Na)
+
Chlorine (Cl)
=
Salt (NaCl)
Mixture
• Substances (elements or compounds) are
physically mixed together to produce a
mixture.
• The composition of substances in a mixture
varies from one sample to another.
• The physical properties of each substance in
a mixture is preserved.
Heterogenous Mixures
Observe multiple phases (parts) because
the substances do NOT mix well.
Homogenous Mixtures
•Also called solutions
•Substances mix so well they look like one phase.
Substances in Matter
The symbol/formula for matter identifies
•Kind and number of substances in matter
•Identifies class of matter
Sodium: Na
Element
Salt: NaCl
Compound Salt Water: NaCl + H2O
mixture: homo mix
Classifying Matter:
Substances vs. Mixtures
Substances
•Definite chemical
make-up
•Elements or
compounds
•Ex. Silicon chip or H2O
Mixtures
•Varied chemical makeup
• 2 or more substances
physically combined
•Homo or Hetero
Mixtures
• Pizza and salt water
Classifying Matter:
Substances vs. Mixtures
Element
•Pure and simplest substance
•One type of atom
•Periodic table
•Symbol, (He= Helium)
Homogenous Mixture
•2 or more substances physically
combined.
•Substances are very soluble in one
another-mix well – one phase
•Substances in mix properties are
preserved
•Separated by physical processes.
•Also called a solution
•Ex. salt water, kool-aid
Compound
• 2 or more substances chemically
combined
•Definite composition
•Break-down only thru chemical
processes
•Substances making up cmpd gain
new properties.
•Chemical Formula, H2O
Heterogenous Mixture
•2 or more substances physically
combined.
•Substances are not soluble in one
another-do not mix well-multiple phases
•Substances in mixture properties are
preserved.
•Separated by physical processes
•Ex. Oil and water, pizza, soil
Chem I: 9.1.15
Due:
• Elements, Compounds; Mixtures Worksheet
Objectives:
• I can classify matter into substance or mixtures.
(Classification of Matter Lab)
• I can identify chemical and physical changes.
Homework:
Classification of Matter and Changes Worksheets
Chem I:
nd
rd
9.1.15(2 /3 )
Infinite Campus Updated:
• Scientific Skills Quiz(14pts.)
• Graduated Cylinder Lab (12pts.)
• Scientific Skill Measurement Lab (8pts.)
• Scientific Skills Gallery Walk (5pts.)
• Notebook Check (5pts.)
*Extended School Services (ESS)
-computer lab/make-up assessments/peer tutoring
-Every Thursday, starting Sept. 8th from 2:30-4
-ESS Bus available-must sign-up in guidance before
noon on Thursdays
Chem I:
th
9.1.15(6 ))
Infinite Campus Updated:
• Scientific Skills Quiz(14pts.)
• Graduated Cylinder Lab (12pts.)
• Scientific Skill Measurement Worksheet (8pts.)
• Scientific Skills Gallery Walk (5pts.)
*Extended School Services (ESS)
-computer lab/make-up assessments/peer tutoring
-Every Thursday, starting Sept. 8th from 2:30-4
-ESS Bus available-must sign-up in guidance before
noon on Thursdays
Chem ICP: 9.1.15
Due:
• Elements, Compounds; Mixtures Worksheet
Objectives:
• I can classify matter into substance or mixtures.
(Classification of Matter Lab)
• I can identify chemical and physical changes.
Homework:
Classification of Matter and Changes Worksheets
Chem ICP: 9.1.15
Extended School Services (ESS)
-computer lab/make-up assessments/peer tutoring
-Every Thursday, starting Sept. 8th from 2:30-4
-ESS Bus available-must sign-up in guidance before
noon on Thursdays
Classification of Matter
Chem I: Homework (9.1.15)
• Classification of matter worksheet-review
.
Chem I:
nd
rd
9.2.15(2 /3 )
Due:
• Classifying Matter Lab-read background
• Classifying Matter Worksheet
Objectives:
• I can classify matter into substance or mixtures.
(Classification of Matter Lab)
• I can identify chemical and physical changes.
Homework:
Identify properties/changes of matter worksheet
Chem I: 9.2.15(6th)
Due:
• Classifying Matter Lab-read background
Objectives:
• I can classify matter into substance or mixtures.
(Classification of Matter Lab)
• I can identify chemical and physical changes.
Homework:
• Classify Matter Worksheet
• Identify properties/changes of matter worksheet
Chem I: 9.2.15 ICP
Due:
• Classify Matter Worksheet
Objectives:
• I can classify matter into substance or mixtures.
(Classification of Matter Lab)
• I can identify chemical and physical changes.
Homework:
• Classify Matter Worksheet
• Identify properties/changes of matter worksheet
Bell Ringer: Classification of Matter
1. How would a chemist define matter?
2. Explain AND illustrate the difference between a
substance and a mixture if you were looking at them
under the microscope.
3. Explain AND illustrate the difference between a
compound and a mixture if you were looking at
them under a microscope.
Bell Ringer: Classification of Matter
1. How would a chemist define matter?
2. Explain AND illustrate the difference between a
substance and a mixture if you were looking at them
under the microscope.
3. Explain AND illustrate the difference between a
compound and a mixture if you were looking at
them under a microscope.
Chem I: 9.3.15
Due:
• Classifying Matter Worksheet
Objectives:
• I can classify matter into substance or mixtures.
(Classification of Matter Lab)
• I can identify chemical and physical changes.
Homework:
Identify properties/changes of matter worksheet
Chem I: 9.3.15
Due:
• Classifying Matter Worksheet
Objectives:
• I can classify matter into substance or mixtures.
(Classification of Matter Lab)
• I can identify chemical and physical changes.
Homework:
Identify properties/changes of matter worksheet
Bell Ringer: Classify Matter
1. Classify each of the following examples as:
element, compound, hetero mix, or homo mix
a. corn starch (C27H48O20)
b. calcium carbonate solution
c. aluminum foil
d. iron rust (FeO)
e. italian dressing
Elements
Simplest substance
Compounds
• Chemical combination of elements in a fixed
amount (always the same way).
• A compound’s fixed amount is called a
chemical formula.
Ex. Sodium chloride = NaCl
•When elements chemically combine the
compound produced has new properties.
Sodium (Na)
+
Chlorine (Cl)
=
Salt (NaCl)
Classification Matter Lab
Salt: NaCl
Sodium: Na
Salt Water: NaCl + H2O
Classification of Matter Lab
Purpose:
• Evaluate and classify matter as either an
element, compound, homo mix, or hetero mix.
• Must provide evidence for your classification.
Conclusion:
Identify what helped you classify matter into
these subgroups.
Classification of Matter
Matter: Physical vs. Chemical Properties
Physical Properties
Chemical Properties
Chem I: 9.4.15
Due:
• Classification of Matter Lab-place in tray
• Physical vs. Chemical Change Worksheet
Objectives:
• I can understand and distinguish between
physical and chemical properties/changes.
• I can identify what forces are affected during
changes with matter.
Homework:
Identify properties/changes of matter worksheet
Matter: Physical vs. Chemical Properties
1. Physical Properties
Chemical Properties
Matter: Physical vs. Chemical Properties
1. Physical Properties
Chemical Properties
Matter: Physical vs. Chemical Properties
Physical Properties
• Does not change the
chemical make-up of
the matter.
• Color, shape, mass,
length, odor, states of
matter, solubility
Chemical Properties
• Does change the
chemical make-up of
matter.
• flammable,
neutralization,
rusting,decomposing
Matter: Propertes/Changes
Solubility
•How well one substance dissolves (physically
mixes) with another substance.
Salt added to water
Soluble
Insoluble
Soluble Solutions
Solutions are composed of:
Solute:
• what is dissolved in the
solution.
• substance you have less of
Solvent:
•
what dissolves the solute
• substance you have more of
• water is a common solvent
Neutralization
Change in pH of a solution by the addition of an
acid (H+ ions) or a base (OH- ion).
Flammability and Combustion
• Matter that can catch on fire and produce
a lot of energy.
www.astm.org
http://magillservicesinc.com/flammability/
Phase Changes
Sublimation
solid directly to a gas.
en.wikipedia.org
chemistryjournal104dianegan8.blogspot.com
Deposition
gas directly to a solid.
www2.volstate.edu
n.wikipedia.org/wiki/Hail
Chemical vs. Physical Change
Chemical Change:
Physical Change:
Physical vs. Chemical Changes
Intramolecular Forces
.
Intermolecular Forces
Chemical vs. Physical Change
Chemical Change:
Physical Change:
ICP: 9.4.15
Due:
• Classification of Matter Lab-place in tray
• Physical vs. Chemical Change Worksheet
Objectives:
• I can identify physical and chemical
properties/changes.
• I can identify what forces are affected during
changes with matter.
Homework:
Identify properties/changes of matter worksheet
Bell Ringer: Classify Matter
1. Classify each of the following examples as an:
element, compound, hetero mix, or homo mix
a. corn starch (C27H48O20)
b. calcium carbonate solution
c. aluminum foil
d. iron rust (FeO)
e. italian dressing
Chemical vs. Physical Change
Chemical Change:
Physical Change:
Chemical vs. Physical Change
Chemical Change:
• Matter’s chemical make-up changes.
• New matter is produced with new properties.
• Ex. Iron Rust (FeO)
Physical Change:
• Physical properties change, but chemical
properties are preserved.
• Matter’s chemical make-up stays the same.
• Ex. cutting paper
Chem I: 9.8.15
Infinite Campus:
• Classification of Matter Lab-17pts.
• Classification of Matter Bell Ringer- 5pts.
Objectives:
• I can identify physical and chemical
properties/changes.
• I can identify what forces are affected during
changes with matter.
Homework:
Apply forces with changes worksheet
Chemical vs. Physical Change
Chemical Change:
Physical Change:
ICP: 9.8.15
Infinite Campus:
• Classification of Matter Lab-17pts.
• Classification of Matter Bell Ringer- 5pts.
Objectives:
• I can identify physical and chemical
properties/changes.
• I can identify what forces are affected during
changes with matter.
Homework:
Apply forces with changes worksheet
Forces affected during physical and chemical changes.
Intramolecular Forces
.
Intermolecular Forces
Identify what forces are affected during each
change on your homework assignment.
Intramolecular Forces
.
Intermolecular Forces
Physical vs. Chemical Changes Lab
• Goggles must be worn at all times or you will be
dismissed from the lab-NO exceptions!
• Remember to record all observations.
(needs to be legible and descriptive)
• Caution: Working with HCl acid, so be careful.
• Disposal of Materials: Most can be discarded
down drains except metal waste (Mg).
Chem I: 9.9.15
Objectives:
• I can understand the difference between
physical and chemical properties/changes
• I can apply forces with changes in matter.
Homework:
Apply forces with changes worksheet
Physical vs. Chemical Changes
1.P (dissolve)
2.C (reacts/new subst.)
3.P (sliced)
4.P (change to steam)
5.C (decomposes)
6. C (rusts)
7. C (catches on fire)
8.P (evaporation)
9. P (melting)
10. C (sours)
11. P (dissolves)
12. C (rotting)
13. C (cooking)
14. C(plant grows)
15. P (tire inflates)
16. C (digested)
17. P (absorbed)
18. P (freezing)
Identify which force below is affected during each
change on your homework assignment.
Intramolecular Forces
.
Intermolecular Forces
Physical vs. Chemical Changes Lab
• Goggles must be worn at all times or you will be
dismissed from the lab-NO exceptions!
• Remember to record all observations.
(needs to be legible and descriptive)
• Caution: Working with HCl acid, so be careful.
• Disposal of Materials: Most can be discarded
down drains except metal waste (Mg).
Chem I: 9.10.15
Objectives:
• I can understand the difference between physical
and chemical properties/changes
• I can apply forces with changes in matter.
• I can identify what physical separation techniques we
used during the changes lab.
Homework:
• Establish conclusion for changes lab.
• Apply physical separation techniques with changes
lab.
• *Matter and Change Quiz tomorrow-study!
Forces affected by changes with matter
Intramolecular Forces
.
Intermolecular Forces
Intramolecular Forces
•Forces within a compound that hold the atoms
together. (chemical bonds)
•Affected/altered during a chemical change.
H2O compound
Chemical Changes
•
•
•
•
•
•
Burning(combustion,flammable)
Growing(chemical reactions)
Reacts with….
Spoiled
Decomposing
Neutralizion (acid reacting with a base)
Intermolecular Forces
•Forces between compounds in a sample of
matter. (group forces)
• Affected/altered during a physical change.
Types of Physical Changes
•
•
•
•
Phase change proccesses (ex. melting/freezing)
Cutting or slicing
Absorbing
Dissolving
Chem I: 9.10.15
Objectives:
• I can understand the difference between physical
and chemical properties/changes
• I can apply forces with changes in matter.
• I can identify what physical separation techniques we
used during the changes lab.
Homework:
• *Matter and Change Quiz tomorrow-study!
Physical vs. Chemical Changes Lab
• Complete lab.
• Conclusion: Homework-due Friday.
*Format: Needs to in be paragraph form; complete
sentences. Write conclusion on back of lab.
*Give two examples of a physical change. Explain
your reasoning with data from the lab.
*Give two examples of a chemical change from the
lab. Explain your reasoning with data from the lab.
Chemical Vs. Physical Changes
Examples
sulfur’s odor
Sucrose’s
solubility
In water
Magnesium
reacting with the
flame
Sugar burning
Sodium
bicarbonate
reacting with HCl
Chemical or
Physical
Change
Evidence
from
Lab
Intermolecular or
Intramolecular
Forces affected?
Chem I: 9.11.15
Due:
• Physical vs. Chemical Changes Lab with conclusion
Objectives:
• I can understand the difference between physical
and chemical properties/changes
• I can apply forces with changes in matter.
• I can identify what physical separation techniques we
used during the changes lab.
Homework:
• Phase Changes Worksheet
Physical vs. Chemical Change Lab
Mixtures
• Substances in a mixture can be separated
from one another through physical
processes.
• Some common methods to separate
mixtures are:
*Filtration
*Extraction
*Distillation
*Chromatography
• Which of these separation techniques did
we use in the lab?
Chem I: 9.14.15
Due:
• Phase Changes Worksheet
• Physical vs Chemical Changes Lab with conclusion
Objectives:
• I can identify separation techniques for mixtures.
• I can understand the relationship between
intermolecular forces and kinetic energy.
Homework:
Matter and Change Study Guide
ICP: 9.14.15
Objectives:
• I can identify separation techniques for mixtures.
• I can understand the relationship between
intermolecular forces and kinetic energy.
Homework:
Matter and Change Study Guide
Intramolecular Forces
.
Intermolecular Forces
Mixtures
• Substances in a mixture can be separated
from one another through physical
processes.
• Some common methods to separate
mixtures are:
*Filtration
*Extraction
*Distillation
*Chromatography
• Which of these separation techniques did
we use in the lab?
Filtration
•
Separating a solid from a liquid in a heterogenous
mixture by their size difference.
Extraction
1. Extraction- separating substances in a heterogenous mixture
from one another based on their unique physical properties.
Sand and Iron Filings
Distillation
Separation of liquids in a mixture by their differences in
boiling points. Ex. Ethanol (78 0C) and Water (1000C)
ICP: 9.15.15
Infinite Campus Update:
• Matter and Change Quiz
Due:
• Green Pen Chromatography Lab-Post Lab Qts.
Objectives:
• I can identify separation techniques for mixtures.
• I can understand the relationship between
intermolecular forces and kinetic energy.
Chromatography
Separates substances present within a homogenous mixture.
•Stationary phase
Usually in solid state:
ex.chromotography paper
•Mobile Phase
Liquid or gas solvent
•The two phases help separate
substances in a homogenous
mixture based on solubility.
Physical Separation Techniques
Separation
Techniques
Filtration
Extraction
Distillation
Chromotography
Physical
property used
for separation
For homo or
hetero mixtures
ICP: 9.16.15
Infinite Campus:
• Physical vs. Chemical Change Lab
• Matter and Change Quiz
• Green Pen Chromatography Lab
Objectives:
• I can identify separation techniques for mixtures.
• I can connect speed of particles with kinetic energy
and intermolecular forces.
• I can understand that mass is conserved during
changes (physical or chemical)
Homework:
• Matter and Change Study Guide
Common Phases of Matter
Types of Energy
Potential Energy: Stored Energy
• Chemical bonds
Kinetic Energy: Energy of motion
•particle movement
•Heat energy
phase change Speed of
of system
Particles
(increase/
decrease)
evaporation of
water
condensation
of alcohol
deposition of
copper
melting of
snow
Kinetic
Energy
(absorbed
/released
by system)
Intermolecular
Forces:
(stronger/weaker)
Chemistry: 9.15.15
Due:
• Heating Curve Graph Worksheet
• Phase Change Table
Objectives:
• I can understand the relationship between
intermolecular forces and kinetic energy.(KMT Theory)
• I can identify separation techniques for mixtures
• I can understand that mass is conserved during
changes.
Homework:
Matter and Change Study Guide
Heat Energy
• Energy that is transferred between matter of
different temperatures. (kinetic energy)
Energy flows between:
• The System:
The matter you are studying/measuring.
• The Surrounding :
The matter (environment) around the system.
Energy Processes:
• Endothermic Process:
When more heat is absorbed by the system.
• Exothermic Process:
When more heat is released by the system.
Types of Energy
Potential Energy: Stored Energy
• Chemical bonds
Kinetic Energy: Energy of motion
•particle movement
•Heat energy
phase change Speed of
of system
Particles
(increase/
decrease)
evaporation of
water
condensation
of alcohol
deposition of
copper
melting of
snow
Kinetic
Energy
(absorbed
/released
by particles)
Intermolecular
Forces:
(stronger/weaker)
Primary Phase Changes
Deposition
gas directly to a solid.
www2.volstate.edu
n.wikipedia.org/wiki/Hail
Sublimation
solid directly to a gas.
en.wikipedia.org
chemistryjournal104dianegan8.blogspot.com
Kinetic Molecular Theory (KMT):
Establishes a relationship between energy flow,
speed of particles, and intermolecular forces during
phase changes. (Physical Changes!)
Chemistry: 9.16.15
Infinite Campus:
• Phase Table/Heating Curve Graph Wksht
• Physical vs. Chemical Change Lab
• Matter and Change Quiz
Objectives:
• I can understand the relationship between
intermolecular forces and kinetic energy.(KMT Theory)
• I can identify separation techniques for mixtures
• I can understand that mass is conserved during
changes.
Homework:
Separation Technique Wksht
phase change Speed of
of system
Particles
(increase/
decrease)
evaporation of
water
condensation
of alcohol
deposition of
copper
melting of
snow
Kinetic
Energy
(absorbed
/released
by particles)
Intermolecular
Forces:
(stronger/weaker)
Kinetic Molecular Theory
Applications
http://webmail.warwickschools.org
Chemistry: 9.17.15
Due:
Separation of Mixtures Worksheet
Objectives:
• I can understand the relationship between
intermolecular forces and kinetic energy.(KMT Theory)
• I can identify separation techniques for mixtures
• I can understand that mass is conserved during
changes.
Homework:
Atomic Models Worksheet
Mixtures
• Substances in a mixture can be separated
from one another through physical
processes.
• Some common methods to separate
mixtures are:
*Filtration
*Extraction
*Distillation
*Chromatography
• Which of these separation techniques did
we use in the lab?
Filtration
•
Separating a solid from a liquid in a heterogenous
mixture by their size difference.
Extraction
1. Extraction- separating substances in a heterogenous mixture
from one another based on their unique physical properties.
Sand and Iron Filings
Distillation
Separation of liquids in a mixture by their differences in
boiling points. Ex. Ethanol (78 0C) and Water (1000C)
Chromatography
Separates substances present within a homogenous mixture.
•Stationary phase
Usually in solid state:
ex.chromatography paper
•Mobile Phase
Liquid or gas solvent
•The two phases help separate
substances in a homogenous
mixture based on solubility.
Physical Separation Techniques
Separation
Techniques
Filtration
Extraction
Distillation
Chromatography
Physical
property used
for separation
For homo or
hetero mixtures
Physical Separation Techniques
Separation
Techniques
Filtration
Extraction
Distillation
Chromotography
Physical
property used
for separation
For homo or
hetero mixtures
Chemistry Homework
• Separation Mixtures Worksheet
• Matter and Change Worksheet (qts.7-9)
Thermochemistry
• Study of energy changes when matter
undergoes physical or chemical changes.
What is energy?
• What does energy feel like?
• What does energy look like?
• What does energy smell like?
• What does energy sound like?
Thermochemistry
• Study of how energy changes when matter
undergoes a change (physical or chemical).
•
What are the two forms of Energy?
Heat Energy
Heat Energy (Kinetic Energy):
• Energy that is transferred between matter of
different temperatures.
• Unit for Energy: Joules (J) or calories (cal)
• Energy is NOT matter because it does not
have mass or volume.
• How does heat energy flow between objects
of different temperatures?
Heat Energy Flow
Energy flows between:
• The System:
The matter you are studying/measuring.
• The Surrounding :
The matter (environment) around the system.
Energy Processes:
• Endothermic Process:
When more heat is absorbed by the system.
• Exothermic Process:
When more heat is released by the system.
Primary Phase Changes
System’s Energy Diagram:
Endothermic or Exothermic ?
System’s Energy Diagram:
Endothermic vs. Exothermic?
Energy Changes and Temp. of System
Kinetic Molecular Theory (KMT):
Establishes a relationship between energy flow,
speed of particles, and intermolecular forces during
phase changes.
Kinetic Molecular Theory
Applications
http://webmail.warwickschools.org
Conservation of Matter and Energy
• Matter can go through
physical and chemical
changes, but the atoms
are always conserved.
• Energy naturally flows
from warm to cold matter
and in that process take
many forms (solar,
electrical, mechanical,
but it is always conserved
during physical and
chemical changes.
phase change Speed of
of system
Particles
(increase/
decrease)
evaporation of
water
condensation
of alcohol
deposition of
copper
melting of
snow
Kinetic
Energy
(absorbed
/released
by system)
Intermolecular
Forces:
(stronger/weaker)
Chromatography Lab
• Follow instructions from textbook, pg. 45.
*Modifications:
1. Place dot with marker about 2 cm from
bottom of chromatography paper.
2. Will use straw instead of pencil.
4. Do not need to put plastic wrap over it.
Energy Changes: Thermometer
•Energy changes within a system is measured
using a thermometer.
•(Energy changes = Temperature changes)
•Temp. change indicates change in speed of
particles comprising the system.
•Primary unit of measurement by scientists:
Celsius (oC) and Kelvin (K) scales
Thermometers
K = oC + 273
Visionlearning.com
Kinetic Molecular Theory
Applications
http://webmail.warwickschools.org
ICP: 2.6.14
Infinite Campus Update:
• Heat Energy Calculations Worksheet
Objectives:
• I can identify classes and changes of matter.
• I can identify what forces are affected during changes
with matter. (inter-vs. intramolecular forces)
• I can understand how energy is associated with
changes matter through qualitative and quantitative
examples.
Ice Cream Lab
Purpose:
To distinguish between endothermic and
exothermic processes for a system
• Complete Pre-Lab Questions
• After lab, complete post-lab qts.
http://naturesdelighticecream.wordpress.com
Energy Changes: Quantitative Data
• Thermochemists can use the following
equation to calculate energy changes with a
system.
Q=mc T
Specific Heat Capacity
Specific Heat Capacity (c ):
• The amount of energy needed to increase the
temperature of a 1 gram sample 1oC.
• Units for specific heat capacity:
- J/g oC or cal/g oC
• Use table below to answer the following qts.
How does the data table on specific heat capacity
explain why metals are better conductors of
heat then non-metals? Use evidence from
table to support your evidence.
Heat Energy Calculations
• The temperature of a 95.4 gram piece of copper
increases from 25.0oC to 48.0oC when the copper
absorbs 849 Joules of heat energy. What is the
specific heat of copper?
Ice Cream Lab
Extension Qts:
Explain how the kinetic molecular theory is
applied when making ice cream.
http://naturesdelighticecream.wordpress.com
Energy Changes
1. The specific heat of ethanol is 2.46J/goC.
Calculate the heat required to raise the
temperature of the 0.193 kg sample of ethanol
from 19oC to 35oC.
2. Circle the energy diagram below that
represents the above energy change for
ethanol. Explain how you know this.
Energy Changes
1. The specific heat of ethanol is 2.46J/goC.
Calculate the heat required to raise the
temperature of the 0.193 kg sample of ethanol
from 19oC to 35oC.
2. Circle the energy diagram below that
represents the above energy change for
ethanol. Explain how you know this.
Chromatography Lab
• Follow instructions from textbook, pg. 45.
*Modifications:
-Will replace pencil with straw.
-Will measure out 10mL of isopropyl alcohol
(rubbing alcohol)
• Complete analysis and conclusion
questions.
Chem I Block : 9.19.14
Infinite Campus:
• Green Pen Chromatography-due today (10pts.)
Objectives:
• I can apply separation techniques in the lab.
(Chromatography Lab)
• I can understand how matter and energy are
conserved during changes (physical/chemical)
• Matter and Energy Gallery Walk
(will collect answers from gallery walk)
Homework:
• Review Matter and Energy Concepts-Test Monday
• power points/practice problems on my webpage
Chromatography Lab
Separates substances from a solution based on solubility
toward the two phases (mobile/stationary)
• Stationary phase?
•
Mobile Phase ?
Energy Calculation Quiz
Conservation of Matter and Energy
• Matter can go through
physical and chemical
changes, but the atoms
are conserved.
• Energy is also conserved
as it flows from hot to
cold matter.
Ex. If the system absorbs
50J of energy, that means the
surrounding released 50J of
energy.
Matter and Energy Gallery Walk
.Will turn in work (primarily study guide qts)
as evidence you were participating in the
gallery walk.
Atomic Structure Ranking Task
Matter and Energy
Chromotography
1. What kind of mixture can
be separated by chromatography?
2. From the chromatogram, what
is the stationary and mobile phase?
3. What dye is most soluble in the
mobile phase? How do you know
this?
4. What dye is most soluble in the
stationary phase? How do you
know this?
Types of Energy
Potential Energy: Stored Energy
• Chemical bonds
Kinetic Energy: Energy of motion
•particle movement
•Heat energy
Heat Energy
Heat Energy:
• Energy that is transferred between matter of
different temperatures.
• Heat energy is also called kinetic energy.
• Unit for Energy: Joules (J) or calories (cal)
• Energy is NOT matter because it does not
have mass or volume.
• How does heat energy flow between objects
of different temperatures?
Heat Energy Flow
Energy flows between:
• The System:
The matter you are studying/measuring.
• The Surrounding :
The matter (environment) around the system.
Energy Processes:
• Endothermic Process:
When more heat is absorbed by the system.
• Exothermic Process:
When more heat is released by the system.
Energy Changes: Thermometer
•Energy changes within a system is measured
using a thermometer.
•(Energy changes = Temperature changes)
•Temp. change indicates change in speed of
particles comprising the system.
•Primary unit of measurement by scientists:
Celsius (oC) and Kelvin (K) scales
Thermometers
K = oC + 273
Visionlearning.com
System’s Energy Diagram:
Endothermic or Exothermic ?
System’s Energy Diagram:
Endothermic vs. Exothermic?
Energy Changes and Temp. of System
Thermometers
K = oC + 273
Visionlearning.com
Kinetic Molecular Theory (KMT):
•Establishes a relationship between energy flow,
speed of particles, and affect of forces for a
system during a chemical or physical change.
• We are going to apply KMT to phase changes
Kinetic Molecular Theory (KMT):
Establishes a relationship between energy flow,
speed of particles, and intermolecular forces during
phase changes.
Primary Phase Changes
Ice Cream Lab
Purpose:
To distinguish between endothermic and
exothermic processes for a system
Ice Cream Lab:
1. What do you predict would be the system?
2. What do you predict would be the
surroundings?
3. Do you predict the making of ice cream is
endothermic or exothermic? Explain your
answer.
http://naturesdelighticecream.wordpress.com
Ice Cream Lab
Post Lab Questions:
• Discuss questions with peers from lab group.
http://naturesdelighticecream.wordpress.com
Kinetic Molecular Theory (KMT):
Establishes a relationship between energy flow,
speed of particles, and intermolecular forces during
phase changes.
phase change Speed of
of system
Particles
(increase/
decrease)
evaporation of
water
condensation
of alcohol
deposition of
copper
melting of
snow
Kinetic
Energy
(absorbed
/released
by system)
Intermolecular
Forces:
(stronger/weaker)
Infinite Campus Update:
• Heating Curve Worksheet (8pts.)
• Ice Cream Lab (will go in tonight)
Objectives:
• I can apply the Kinetic Molecular Theory (KMT) during
phase changes. Heating Curve Worksheet
• I can predict and calculate energy changes when matter
undergoes physical changes.
Homework:
• Heat Energy Problems
• Review Energy changes-quiz tomorrow
Energy Changes: Quantitative Data
• Thermochemists can use the following
equation to calculate energy changes with a
system.
Q=mc T
Specific Heat Capacity
Specific Heat Capacity (c ):
• The amount of energy needed to increase the
temperature of a 1 gram sample 1oC.
• Units for specific heat capacity:
- J/g oC or cal/g oC
• Use table below to answer the following qts.
How does the data table on specific heat capacity
explain why metals are better conductors of
heat then non-metals? Use evidence from
table to support your evidence.
Specific Heats of Common Substances
Substances
Specific Heat
J/g* 0C
Specific Heat
Cal/g*0c
water
4.18
1.00
Grain alcohol
2.4
0.58
ice
2.1
0.50
steam
1.7
.40
aluminum
0.90
0.21
silver
0.24
0.057
mercury
0.14
0.033
Kinetic Molecular Theory (KMT):
Establishes a relationship between energy flow,
speed of particles, and intermolecular forces during
phase changes.
Kinetic Molecular Theory
Applications
http://webmail.warwickschools.org
Specific Heat Calculations
• The temperature of a 95.4 gram piece of copper
increases from 25.0oC to 48.0oC when the copper
absorbs 849 Joules of heat energy. What is the
specific heat of copper?
Heat Energy Problems Gallery Walk
• If you are NOT productive, will work at desk
alone on problems.
• Will take-up problems tomorrow to ensure
100% participation by all students.
Heat Energy Calculations
Worksheet-Key (sig. figs)
a. 6,000 cal
b. 115,060 J
c. 121,550 J
d. 392 J/kgoC
Specific Heat Capacity
Specific Heat Capacity (c ):
• The amount of energy needed to increase the
temperature of a 1 gram sample 1oC.
• Units for specific heat capacity:
- J/g oC or cal/g oC
• Use table below to answer the following qts.
How does the data table on specific heat capacity
explain why metals are better conductors of
heat then non-metals? Use evidence from
table to support your evidence.
Specific Heats of Common Substances
Substances
Specific Heat
J/g* 0C
Specific Heat
Cal/g*0c
water
4.18
1.00
Grain alcohol
2.4
0.58
ice
2.1
0.50
steam
1.7
.40
aluminum
0.90
0.21
silver
0.24
0.057
mercury
0.14
0.033
Energy Changes: Quantitative Data
• Thermochemists can use the following
equation to calculate energy changes with a
system.
Q=mc T
Heat Energy Calculations
Worksheet-Key (sig. figs)
a. 6,000 cal
b. 115,060 J
c. -0.392J/goC
d. 139.6J/kgK
e. 121,550 J
f. -20 g (negative sign refers to energy
being released, exothermic process)