Evaluate the students on what they learned from the following topics (Unit I):
Module 1: Respiratory and Circulatory Systems
Module 2: Genetics- Incomplete Dominance/Codominance/ DNA model Module 3: Photosynthesis
II. Topic: Unit 1, Modules 1 to 3 Materials: Quiz Notebook
III. Strategy: Paper and Pencil/ballpen Test
IV. Assessment: Test proper (Please see attached sheet)
V. Assignment:
Illustrate/draw the different atomic models prposed by the following Scientists:
John Dalton, J.J. Thomson, Ernest Rutherford, Niels Bohr, Erwin Schrodinger etc
August 13, 2014 (Wednesday) UP Open Laboratory
August 14, 2014 (Thursday) Absent
August 15, 2014 (Friday) Checking of papers (Unit Test) Remediation
Lesson Plan in Science 9 August 18, 2014 (Monday)
Objectives:
1. Determine the characteristic colors that metal salts emit; and 2. Relate the colors emitted by metal salts to the structure of the atom.
II. Topic: Activity 1: FLAME TEST
Materials: laptop, video showing Flame Test
III. Strategy: Viewing some videos about Flame Test
IV. Assessment: (Discussion/Recitation)
What are the colors emitted by the following elements (based on the video) Lithium Li Calcium Ca
Sodium Na Strontium Sr Potassium K Barium Ba Copper Cu
Questions:
Q1. Why do you think are there different colors emitted?
Q2. What particles in the heated compounds are responsible for the production of the colored light?
Q3. How did the scientists explain the relationship between the colors observed and the structure of the atom?
V. Assignment:
Enrichment:
Why do certain elements give off light of specific color when heat is applied?
Lesson Plan in Science 9 August 19, 2014 (Tuesday)
Objectives:
1. Describe how it is likely to find the electron in an atom by probability.
II. Topic: Activity 2: Predicting the Probable Location of an Electron
Materials: One sheet of short bond paper or half of a short folder pencil or colored marker with small tip
compass ; graphing paper ; one-foot ruler
III. Strategy: Performing the activity
IV. Assessment: (Discussion/Recitation)
What are the colors emitted by the following elements (based on the video) Lithium Li Calcium Ca
Sodium Na Strontium Sr Potassium K Barium Ba Copper Cu
Questions:
Q1. Why do you think are there different colors emitted?
Q2. What particles in the heated compounds are responsible for the production of the colored light?
Q3. How did the scientists explain the relationship between the colors observed and the structure of the atom?
V. Assignment:
Enrichment:
Why do certain elements give off light of specific color when heat is applied?
Lesson Plan in Science 9
August 20, 2014 (Wednesday) (same LP dated Aug. 19, 2014)
- the lesson was not carried out due to disruption of classes Objectives:
1. Describe how it is likely to find the electron in an atom by probability.
II. Topic: Activity 2: Predicting the Probable Location of an Electron
Materials: One sheet of short bond paper or half of a short folder
pencil or colored marker with small tip; compass ; graphing paper ;one-foot ruler
III. Strategy: Performing the activity
IV. Assessment: (Discussion/Recitation)
Q1. What happens to the number of dots per unit area as the distance of the dots go farther from the center?
Q2. Determine the percent probability of finding a dot in each of the circle drawn on the target by multiplying No. of dots /cm2 (column D) by the total number of dots (100).
For example: In circle 1(A)
Percent probability = No. of dots /cm2 X 100 = [0.1920 / 100 ] X 100 = 19.20%
Q3. Based on your graph, what is the distance with the highest probability of finding a dot?
Show this in your graph.
Q4. How many dots are found in the area where there is highest probability of finding dots?
Q5.How are your results similar to the distribution of electrons in an atom?
V. Assignment:
Enrichment:
Activity 1 is an analogy to show you that it is not possible to know the exact position of the electron.
So, Bohr’s idea that electrons are found in definite orbits around the nucleus was rejected.
Three physicists led the development of a better model of the atom. These were Louie de Broglie, Erwin Schrodinger, and Werner Karl Heisenberg.
Question: Describe or explain the atomic model proposed by Louie de Broglie, Erwin Schrodinger and Werner Karl Heisenberg.
III. Strategy: Discussion/ Viewing of Constec Video about atom
IV. Assessment: Discussion of the ff. models
a. Dalton's model d. Bohr's model
b. Thomson's model e. Electron Cloud Model c. Rutherford's model
Questions:
1. Atoms are the smallest particle of matter. Through the models we were able to understand
and even imagine the structure of an atom, but how will you describe each model? Which model
2. How will you describe the structure of the atom?
Enrichment:
Define or describe the following terms:
1. Main energy levels, Orbitals, Sublevels, Electron Configuration
August 25, 2014 (Monday) HOLIDAY
Lesson Plan in Science 9 August 26, 2014 (Tuesday)
Objectives:
1. Write the electron configuration of the elements in the third period;
2. Determine the pattern of filling the orbitals based on the given distribution for the first 10 elements; and 3. Devise rules in filling up the orbitals.
II. Topic: Activity 3: Electron Configurations
Materials: Pen and paper Periodic table Manila Paper Pentel pen
III. Strategy: Performing the activity -August 26, 2014
IV. Assessment: (Discussion/Recitation) -August 27, 2014
Q1. Do you see patterns in the distribution of their electrons?
Q2. What are these patterns you observe?
Q3. What do you think are some rules that apply in filling up the orbitals for the elements from atomic number 1 to 18?
V. Assignment:
Explain the concepts stated in each principle:
1. Aufbau Principle
2. Hund's Rule of Multiplicity 3. Pauli Exclusion Principle
Lesson Plan in Science 9 August 27, 2014 (Wednesday)
Objectives:
1. Write the electron configuration of the elements in the third period;
2. Determine the pattern of filling the orbitals based on the given distribution for the first 10 elements; and 3. Devise rules in filling up the orbitals.
II. Topic: Activity 3: Electron Configurations
Materials: Pen and paper Periodic table Manila Paper Pentel pen
III. Strategy: Performing the activity -August 26, 2014
IV. Assessment: (Discussion/Recitation) -August 27, 2014
Q1. Do you see patterns in the distribution of their electrons?
Q2. What are these patterns you observe?
Q3. What do you think are some rules that apply in filling up the orbitals for the elements from atomic number 1 to 18?
V. Assignment:
Explain the concepts stated in each principle:
Enrichment:
1. Aufbau Principle
2. Hund's Rule of Multiplicity 3. Pauli Exclusion Principle
Lesson Plan in Science 9 August 29, 2014 (Friday)
UNIT TEST Objectives:
Evaluate the students on what they learned from the following topics (Unit 2):
Module 1: Electronic Structure of Matter Activity 1: The Flame Test
Activity 2: Predicting the probable location of an electron Activity 3: Electron Configurations
II. Topic: Unit 2, Module 1, activity 1 to 3 Materials: Quiz Notebook
III. Strategy: Paper and Pencil/ballpen Test
IV. Assessment: Test proper (Please see attached sheet)
V. Assignment:
Questions:
1. How are ionic and covalent compounds formed?
2. Whys is an ionic compound different from a covalent compound?
3. How is a metallic compound formed?
September 1, 2014 (Monday) Please refer to lesson plan dated August 29, 2014 the lesson was not carried out due to disruption of classes
Lesson Plan in Science 9
September 2, 2014 (Tuesday) ABSENT
Lesson Plan in Science 9
September 3, 2014 (Wednesday)
Objectives:
1. Identify the number of valence electrons of atoms.
2. Compare the electronegativity values of metals and non-metals.
II. Topic: Pre-Assessment:
Materials: quiz notebook
IV. Assessment: Pls. see attached sheet
V. Assignment:
1. Identify the number of valence electrons of atoms.
2. Compare the electronegativity values of metals and non-metals.
II. Topic: Activity 1: Mapping the Periodic Table Materials: Periodic Table Crayons
III. Strategy: performing the activity Analyzingtheb periodic table IV. Assessment:
Q1. Where can you find metals, non-metals and noble gases in the periodic table of elements?
Q2. Which number tells you the number of valence electrons?
Q3. What do you notice in the number of valence electrons of metals, non-metals and noble gases?
Q4. What kind of element has:
a. less than 4 valence electrons?
b. more than 4 valence electrons?
c. low electronegativity?
d. high electronegativity?
e. low ionization energy?
f. high ionization energy?
V. Assignment:
Explain the concepts stated in each principle:
Illustrate the LEDSof the of the representative elements
September 5, 2014 (Friday) Refer to lesson plan dated September 4, 2014 for the discussion of the answers to the activity
Lesson Plan in Science 9 September 8, 2014 (Monday)
Objectives:
1. Write the Lewis Symbol of some elements.
2. Identify the number of valence electrons.
II. Topic: LEDS
Materials: Pen and paper Periodic table of elements III. Strategy: Guided Inquiry/Exercises
IV. Assessment:
Determine the number of valence electrons and illustrate the LEDS of the ff elements:- a. Mn - 25 c. Ga - 31 e. Sc - 21 g. Co -27 i. Ag - 47 b. Cs - 55 d. Y - 39 f. Fe - 26 h. Br - 35 j. Sr -38 V. Assignment:
Remediation: Illustrate the LEDS of the transition metals.
Lesson Plan in Science 9 September 9, 2014 (Tuesday)
Objectives:
1. Write the Lewis Symbol of the representative elements.
2. Show the relationship among the number of valence electrons, electronegativity and ionization energy.
II. Topic: Activity 2: Lewis Symbol
Materials: Pen and paper Periodic table of elements III. Strategy: Performing the activity
Guided Inquiry IV. Assessment:
Q1. Arrange these elements in increasing:
a. valence electrons b. electronegativity values. c. Ionization energy.
Q2. What do you notice with the number of valence electrons, electronegativity values and ionization energies of the elements?
Q3. What kind of element has the greatest tendency to attract electrons? Why?
Examine the periodic table below. Does it verify your answers in Q1 and Q2?
V. Assignment:
Enrichment: What is the difference between ionization energy and electronegativity?
Lesson Plan in Science 9
September 10, 2014 (Wednesday)
Objectives:
1. Write the Lewis Symbol of the representative elements.
2. Show the relationship among the number of valence electrons, electronegativity and ionization energy.
II. Topic: Activity 2: Lewis Symbol
Materials: Pen and paper Periodic table of elements III. Strategy: Discussion
IV. Assessment:
Q1. Arrange these elements in increasing:
a. valence electrons b. electronegativity values. c. Ionization energy.
Q2. What do you notice with the number of valence electrons, electronegativity values and ionization energies of the elements?
Q3. What kind of element has the greatest tendency to attract electrons? Why?
Examine the periodic table below. Does it verify your answers in Q1 and Q2?
V. Assignment:
September 11, 2014 (Thursday) Please refer to lesson plan dated September 10, 2014
Lesson Plan in Science 9 September 12, 2014 (Friday)
Objectives:
1. Write the Lewis Symbol of the representative elements.
2. Show the relationship among the number of valence electrons, electronegativity and ionization energy.
II. Topic: ELECTRONEGATIVITY
Materials: Pen and paper Periodic table of elements III. Strategy: Performing Activity/Guided Inquiry
IV. Assessment: Seat work (Exercises)
COMPOUND FORMULA ELECTRONEGATIVITY TYPE OF DIFFERENCE CHEMICAL BOND 1. lithium fluoride
2. oxygen molecules
3. water
4. methane
5. potassium oxide
6. hydrogen chloride
7. magnesium oxide
8. carbon dioxide
9. aluminum oxide
10. sulfur dioxide
V. Assignment:
Enrichment:
Types of Chemical Bonds 1. ionic bond
2. Covalent bond 3. metallic bond