When writing conclusions or explaining any phenomena, always use the claim, evidence, reasoning, format.
Claim-A statement that answers the original question or problem. What conclusion can you make about your original question?
Evidence-Scientific data that supports the claim. The data needs to be appropriate and sufficient to support the claim. What data do you have to support your claim?
Reasoning-A justification that links the claim and evidence and includes appropriate and sufficient chemistry principles to defend the claim and evidence. What is chemistry explanation/connection between the claim and evidence?
OVERVIEW: the goal of grading and reporting is to provide the students with feedback that reflects their progress towards the mastery of the indicators and objectives found in the science curriculum framework progress guide.
class work 35%
This may include any written work, media presentation, or oral exercise based on daily objectives completed by an individual or group of students. May be reported as total point or percentage grade.
Homework 15%
This may include any written or media presentation based on daily or weekly objectives completed by an individual or group of students. Teacher may check for completion and assign points accordingly.
Assessment (includes labs and projects) 50%
This may include any evaluation that reflects the student’s performance on a summary of chapter, unit, or module objectives and any labs or hands on activities, reports and projects. Evaluative indicator reported as percentage of mastery of content and skills.
_________________________________________________________________________________
CHEMISTRY COURSE OUTLINE
Quarter 1
September 6, 2017 - November 9, 2017 (46 days)
|
Quarter 2
November 10, 2017 - January 25,
2018 (44 days)
|
Unit 1: Integrating the Atom Into Your World
Instructional Focus
· Apply scientific principles and evidence
to provide an explanation about
the effects of changing the temperature or concentration of the reacting particles on the rate at which a reaction occurs.
· Use
the periodic table as a model to predict the relative properties of elements
based on the patterns of electrons in the outermost energy level of atoms.
Content Specifics
· Introduction to Chemistry and Measurement
· Matter and Change
· Atomic Structure
· The Periodic Table
Assessments
· SLO
Chemistry Pre- Test
· Teacher-created Formative
Assessments
· Semester
One- Engineering Design Project
|
Unit 2: Linking
the Submicroscopic and Macroscopic
Instructional Focus
· Construct an explanation for the outcome of a simple chemical reaction based on the outermost electron state of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.
· Use mathematical representations to support the claim that atoms are conserved during a chemical reaction.
Content Specifics
· The
Periodic Table
· Ionic
and Metallic Bonding
· Covalent
Bonding
· Classifying
and Balancing Chemical Reactions
Assessments
· SLO
Chemistry Post- Test
· Teacher-created Formative
Assessments
|
Quarter 3
January 26, 2018 - March 28, 2018 (42 days)
|
Quarter 4
March 29, 2018 - June 13,
2018 (48 days)
|
Unit 3: Stoichiometry and Aqueous Solutions
Instructional Focus
· Construct
and revise an explanation for the outcome of a simple chemical reaction based
on the outermost electron states of atoms, trends in the periodic table, and
knowledge of the patterns of chemical properties.
· Develop
and use a model of two objects interacting through electric or magnetic
fields to illustrate the forces between objects and the changes in energy of
the objects due to the interaction.
Content Specifics
· Chemical
Quantities
· Stoichiometry
· Reactions
in Aqueous Solutions
Assessments
· Teacher-created Formative
Assessments
· Semester
Two- Engineering Design Project
|
Unit 4: Bonds
Matter!
Instructional Focus
· Plan and
conduct an investigation to gather evidence to compare the structure of
substances at the bulk scale to infer the strength of electrical forces
between particles.
· Develop
and use models to illustrate that energy at the macroscopic scale can be
accounted for as a combination of energy associated with the motions of
particles (objects) and energy associated with the relative positions of
particles (objects).
Content Specifics
· Acids, Bases, and Salts
· Gas Behavior
· Thermochemistry
· States of Matter and Reaction Rates
Assessments
· Teacher-created Formative
Assessments
|
RETAKES
Students may retake an assignment/assessment if:
1.
The original assignment/assessment was completed
on time
2.
The student put in a good faith effort into the
original assignment
3.
The retake must occur within 2 classes from the
date of the original assignment.
The retaken assignment will be an equivalent but not
identical assignment, where the content and format will be the same as the
original, but the questions will be different. The higher of the two grades
will be recorded.
CLASS BLOG
I maintain a class blog at hepburnscience.blogspot.com. You can see
what the warm-up question was for each day, record any home work, and the topic
of the classwork. It is a good idea to check the blog when you are absent so
you can keep up with what is happening in class.
TUTORIALS
Students may receive extra help after school provided they
inform me a day in advance. All tutorials will be held in the school’s media
center/library for 1hrs. starting at 2: 45 pm. Please be on time because I will
wait for only 5 min. before leaving.
CONTACTING ME
The best way to get into contact with me is via email, which
is khepburn@pgcps.org. If any parent wishes
to have a one-on-one conference with me please feel free to contact our
professional school counselors department to arrange a meeting.
1. A composition book for warm-ups
2. A 3 ring binder for notes
3. Pens and pencils
4. A simple calculator
5. A flash drive
6. Access to the internet
6. Access to the internet
_____________________________________________________________________________
HOW TO WRITE A CHEMISTRY LAB REPORT
All lab reports must be typed using 12-14 point fonts. The report must contain the following sub-sections:
Aim/purpose:
Here you write the question/purpose for doing the lab
Materials:
Make a list of all chemical compounds and lab equipment used during the lab.
Procedure:
Write the steps you used in the lab to complete the activity. It should be in the PAST TENSE AND with a passive voice.
For example:
DO NOT SAY, we/my partner and I, added 25 ml of water to the beaker. Instead, say, 25 ml of water was added to the beaker.
Data
If you made measurements during the lab, then they can given as a table. Also, you can make qualitative description of the data and that information will be added here.
Calculations:
So labs involve completing some math calculations. Give an example of the calculation here.
Conclusion:
Here you state the answer to the research question asked at the beginning of the lab and the answer should be based on the data collected. Also make inferences based on the data collected and the calculations done. In some cases specific questions may be asked during the lab and they should be answered in the conclusion section.
---------------------------------------------------------------------------------------------------------
Chemistry review questions
A.
Chapter 1
1.
Name the 5 branches of chemistry
and describe what each area of chemistry they focus on.
2.
Explain the difference
between theory, law, & hypothesis.
3.
Which step in the
scientific method uses the 5 senses to gather information?
B. Chapter 2
4.
Define matter.
5.
How are extensive
properties different from intensive properties? Give an example in each case.
6.
Describe the difference
between elements, compounds, & mixtures giving an example in each case.
7.
List the ways that solids,
liquids and gases are different from each other.
8.
How is a physical change
different from a chemical change? Give examples.
9.
How are homogeneous and
heterogeneous mixtures different from each other? Give examples.
10. A compound has the name Potassium dichromate. Name the elements
found in this compound.
11. What term is used to describe
the following phase changes (a) solid to gas (b) liquid to gas (c) solid to
liquid (d) gas to liquid (e) liquid to solid
12. At what temperature does
pure water (a) freeze (b) melt (c) boil
C. Chapter 3
13. Define density and write the equation used to calculate density.
14. If an object has a mass of 25g and a volume of 30ml. What is the
density of this object?
15. If the density of an
object is 34.7 g/ml and its volume is 3ml. What is the mass of the object?
16. Temperature can be measured on degrees Celsius or degrees
Kelvin. How do you convert degrees Celsius to degrees Kelvin?
D. Chapter 4
17. Name the 3 main types of subatomic particles found in the atom.
18. Describe the relative mass, charge, and location within the
atom, of each subatomic particle.
19. Define atomic number, mass number, and isotope.
20. An atom has 13 protons and 12 neutrons within its nucleus. (a)
What is the atomic number (b) mass number (c) number of electrons (d) name of
the element (e) location on the periodic table.
21. An isotope of Carbon is Carbon-14. What is the (a) atomic number
(b) mass number (c) # of protons, electrons, & neutron for this isotope?
E. Chapter 5
22. An element has an atomic number of 35. Write its (a) electron
configuration (b) electron configuration for the valence level only (c) draw
the orbital diagram for the valence level only.
23. An element has an electron configuration of 1s2 2s2
2p6 3s2 3p4. What is the (a) atomic number (b)
group, period, and & block to which this element belong?
F. Chapter 6
24. How many (a) groups (b)
periods (c) blocks are there on the periodic table?
25. To which group does each
of the following belong: (a) noble/inert gases (b) alkali metals (c) halogens
(d) alkaline earth metals (e) transition metals
26. What doe elements within
the same (a) group (b) period have in common?
Due
May 29 (a day) or May 30 (b day)
G. Chapter 7, 8, & 9
27. How are ions formed?
28. How is an ionic bond different from a covalent bond?
29. Which type of elements
are involved in (a) ionic (b) covalent bond?
30. Give some properties of
(a) ionic (b) molecular compounds
31. Write the formula for
each of the following: (a) Aluminum oxide (b) phosphorus pentachloride (c)
copper (II) sulfate (d) magnesium acetate (e) chlorine gas
32. Name the following compounds: (a) Ba(OH)2 (b) NI3
(c) Cs2O
H. Chapter 10
33. The mole can be used to measure the quantity of matter in 3
different ways. What are these 3 ways?
34. How is molar mass
calculated?
35. Calculate the molar mass of (a) C6H12O6
(b) Fe
36. 1 mole of any substance
contains how many particles?
37. 1 mole of any gas
occupies what volume?
38. 1 mole of any compound
has mass equal to_________grams
39. What is the mass of 2.3
moles of NaCl?
40. What is the volume of 2.3
moles NH3 gas?
41. How many molecules are
2.3 moles of CH4?
42. How many moles are there
in (a) 234g of CuS (b) 29 liters of O2 gas (c) 1.5 x 1025
molecules of CO2?
Due
June 11 (b day) or June 12 (a day)
I. Chapter 11 & 12
43. Name the 5 general types
of chemical reactions
44. Write a skeleton equation
for the reaction: hydrogen gas combines with sulfur to produce hydrogen
sulfide.
45. Balance the equations:
(a) Al + O2 ----------> Al2O3 (b) FeCl3 + NaOH --------> Fe(OH)3 + NaCl
46. 4K + O2
------->
2K2O. How many moles of O2 are need to produce 3 moles of
K2O?
J. Chapter 14
47. Name the 2 factors that are compared in the following gas laws
and state how they vary with each other: (a) Boyle’s law (b) Charles’ law (c)
Gay-Lussac’s law
48. If a 250ml of a gas has pressure of 24 atm. at 27 degrees
Celsius. If the temperature changes to 35°C, what will be the new volume?
K.
Chapter 16
49. Define molarity
50. If 2 moles of CaS are dissolved in 250ml of a solvent. What is
the molarity of the solution?
51. Name 3 ways to make a
solute dissolve faster in a solvent
L. Chapter 17
52. How are exothermic and
endothermic reactions different? Give an example of each.
53. Describe and explain the
flow of heat energy, when 2 objects of different temperatures come into contact
with each other.
54. If ΔH
for a reaction is -1234kJ. Is the reaction exothermic or endothermic? Explain.
M. Chapter 19
55. How does (a) Arrhenius (b)
Bronsted-Lowry define an acid and a base.
56. Give 2 properties of (a)
acids (b) bases
57. Give an example of a
diprotic acid
58. NH3 + H2O <-----------> H3O+ + NO3- identify the Bronsted acids and bases
on both sides of the equation.
59. What does pH measure?
60. If a solution has [H+]
= 1 x 10-9, what is its pH?
Due before your final exam date
___________________________________________________________
DUE DATE FOR ALL EXTRA CREDIT WORK IS JUNE 8, 2018
Total = 25 pts.
Total = 25 pts.
DUE DATE FOR ALL EXTRA CREDIT WORK IS JUNE 8, 2018
Extra credit assignment
This assignment will serve as extra credit and the credit earned will be added to the assessment category at the end of the quarter.
These assignments are designed to be used 1 per quarter to supplement final grades for a quarter. Projects cannot be used more than once. A new project must be completed for each quarter.
This assignment should be typed using 12 pt. fonts and double-spaced. A cover page should be included with student’s name, Title of your project, class period, and the teacher’s name.
There must be a reference page containing the source of the information used in the project. This includes pictures as well. IF AN ASSIGNMENT IS TURNED IN WITHOUT A REFERENCE PAGE THE ASSIGNMENT WILL RECEIVE A SCORE OF ZERO.
All completed now must be turned in to me via turnitin.com. Get the code from me in class.
All completed now must be turned in to me via turnitin.com. Get the code from me in class.
No late assignments will be accepted. Students are encouraged to turn in their assignment electronically.
Project 1
A study of elements and their compounds.
A. Each student will select an element (give the teacher the name of your element before starting the project.) and provide information about the element such as atomic number, symbol, atomic mass, electron configuration, physical state at room temperature, position on the periodic table, when was it discovered and by whom. Include pictures where possible (10 pts)
B. 3 compounds made from the elements that are used in society today. For each of the compounds selected give the chemical name, chemical formula and how it is used today. You must provide several pieces of chemistry related information in order to receive full credit.(10 pts.)
5 special pieces of chemistry information connected with the element. (5 pts.)Total = 25 pts.
Project 2
Black Scientist research paper
Each student must select a black scientist from anywhere in the world and give the name of the person to the teacher before starting the project. Students will provide the following information (details are expected):
1. Name of the individual
2. Place and date of birth and place and date of death (if not alive today)
3. Formal education (if any)
4. What was/is he/she famous for? (Invention/discovery), give details of the work done by this person.(this section should be more than just a few lines about their work)
5. Any special circumstances surrounding the life and legacy of the individual.
Remember to include pictures of the individual and examples of the work the individual is known for. All papers must be presented to the class in order to receive full credit.
No late assignments will be accepted. Students are encouraged to turn in their assignment electronically.
Total = 25 pts.
____________________________________________________________________
