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| Curative Catalyst M.D. Introduction To Chemistry Activity | Metric Madness:
Learn the Metric System on Line
This is Fun Interactive with Mr. Light Bulb |
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Chemical Bonds
Atomic and Molecular Structure
1. The Periodic Table displays the elements in increasing atomic number and shows how periodicity of the physical and chemical properties of the elements relates to atomic structure. As a basis for understanding this concept, students know:
d. how to use the Periodic Table to determine the number of electrons available for bonding.
2. Biological, chemical, and physical properties of matter result from the ability of atoms to form bonds based on electrostatic forces between electrons and protons, and between atoms and molecules. As a basis for understanding this concept, students know:
a. atoms combine to form molecules by sharing electrons to form covalent or metallic bonds, or by exchanging electrons to form ionic bonds.
b. chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many large biological molecules are covalent.
c. salt crystals such as NaCl are repeating patterns of positive and negative ions held together by electrostatic attraction.
d. in a liquid the inter-molecular forces are weaker than in a solid, so that the molecules can move in a random pattern relative to one-another.
e. how to draw Lewis dot structures.
f.* how to predict the shape of simple molecules and their polarity from Lewis dot structures
g.* how electronegativity and ionization energy relate to bond formation
h.* how to identify solids and liquids held together by Van der Waals forces or hydrogen bonding, and relate these forces to volatility and boiling/melting point temperatures.
Organic and Biochemistry
10. The bonding characteristics of carbon lead to many different molecules with varied sizes, shapes, and chemical properties, providing the biochemical basis of life. As a basis for understanding this concept, students know:
a. large molecules (polymers) such as proteins, nucleic acids, and starch are formed by repetitive combinations of simple sub-units.
b. the bonding characteristics of carbon lead to a large variety of structures ranging from simple hydrocarbons to complex polymers and biological molecules.
c. amino acids are the building blocks of proteins.
Knowledge Targets
·
I can explain how atoms combine to form molecules by sharing electrons to form covalent or metallic bonds, or by exchanging electrons to form ionic bonds.·
I can describe how electronegativity and ionization energy relate to bond formation.·
I can show how salt crystals such as NaCl are repeating patterns of positive and negative ions held together by electrostatic attraction.·
I can use the octet rule and Lewis Dot Structures for cations and anions to describe ionic bonds.·
I can describe single, double, triple and coordinated covalent bonds·
I can explain how the chemical bonds between atoms in molecules such as H2 , CH4 , NH3 , H2 CCH2 , N2 , Cl2 , and many large biological molecules are covalent.·
I understand the ideas of VESPR or Valence Electron Shell Pair Repulsion theory.·
I can explain the ideas of hybrid orbits.Reasoning Targets
·
I am able to write using my own words, how electronegativity and ionization energy relate to bond formation.·
I can use the periodic table to identify the type of bond formed between metals and non metals, with in metals and between two non metals.·
I can use the octet rule to explain how ionic and covalent bonds are formed.·
I can compare and contrast ionic, metal and covalent bonds.·
I will be able to relate sigma and pi bonds to the single, double, and triple bonds.·
I can evaluate the combination of orbitals that create sp, sp2, and sp3 bonds in covalently bonded molecules.·
I can evaluate the polarity of bonds in terms of electronegativity using electronegativity values in the period table.Skill Targets
·
Students will construct models of ionic and covalently bonded atoms.·
I can develop and answer high level questions according to Costas levels of question pertaining to ionic and covalent bonds.Product Targets
·
I will create drawings of atomic structures using Valence Shell Electron Pair Repulsion, VSEPR, and hybrid orbital ideas.·
I will demonstrate my understanding of ionic and covalent bonding by diagramming the electron configurations using Lewis dot structures and hybrid orbitals for those bonds.Chemistry Schedule Chapter 15: Ionic Bonding and Ionic Compounds
and Chapter 16: Covalent Bonds (Semester 2: Week 7 March 5-19)
Monday: Ionic bonds
Knowledge Targets
·
I can explain how atoms combine to form molecules by sharing electrons to form covalent or metallic bonds, or by exchanging electrons to form ionic bonds.·
I can describe how electronegativity and ionization energy relate to bond formation.·
I can show how salt crystals such as NaCl are repeating patterns of positive and negative ions held together by electrostatic attraction.·
I can use the octet rule and Lewis Dot Structures for cations and anions to describe ionic bonds.Reasoning Targets
·
I am able to write using my own words, how electronegativity and ionization energy relate to bond formation.·
I can use the periodic table to identify the type of bond formed between metals and non metals, with in metals and between two non metals.·
I can use the octet rule to explain how ionic and covalent bonds are formed.Skill Targets
·
I can develop and answer high level questions according to Costas levels of question pertaining to ionic and covalent bonds.Product Targets
·
I will demonstrate my understanding of ionic and covalent bonding by diagramming the electron configurations using Lewis dot structures and hybrid orbitals for those bonds.15 minutes Hand back tests and test corrections
15 minutes Mini Lecture: Valence electrons and electron dot structures: neutral, cation, and anion
20 minutes Activity: Ionic bonding and predicting what will react to form a molecule
Homework: Pre-lab Experiment 25
Tuesday: Experiment and review
Knowledge Targets
·
I can explain how atoms combine to form molecules by sharing electrons to form covalent or metallic bonds, or by exchanging electrons to form ionic bonds.·
I can describe how electronegativity and ionization energy relate to bond formation.·
I can show how salt crystals such as NaCl are repeating patterns of positive and negative ions held together by electrostatic attraction.·
I can use the octet rule and Lewis Dot Structures for cations and anions to describe ionic bonds.Reasoning Targets
·
I am able to write using my own words, how electronegativity and ionization energy relate to bond formation.·
I can use the octet rule to explain how ionic and covalent bonds are formed.Skill Targets
·
Students will construct models of ionic and covalently bonded atoms.Product Targets
·
I will demonstrate my understanding of ionic and covalent bonding by diagramming the electron configurations using Lewis dot structures and hybrid orbitals for those bonds.10 minutes Introduction to Experiment 25: Crystal Structures
35 minutes Perform the laboratory
10 minutes Answer the laboratory question and write a conclusion
Homework Read pages 427-249 and do questions 15-19
Wednesday or Thursday: Valence Shell Electron-Pair Repulsion Theory
Knowledge Targets
·
I understand the ideas of VESPR or Valence Electron Shell Pair Repulsion theory.Skill Targets
·
I can develop and answer high level questions according to Costas levels of question pertaining to ionic and covalent bonds.Product Targets
·
I will create drawings of atomic structures using Valence Shell Electron Pair Repulsion, VSEPR, and hybrid orbital ideas.20 minutes Mini Lecture on metal bonds and properties of metals and ionic substances
15 minutes Acting out ionic and metal bonds
30 minutes Mini Lecture: Single, Double, and Triple bonds, Octet rule, Coordinated bonds and exceptions to the octet rule
20 minutes Video: Molecular structures
15 minutes Practice problems 7-12 page 451
Homework Pre-laboratory for laboratory on Laboratory 22 on the handout.
Friday: Shapes of Covalent Molecules and Polarity
Knowledge Targets
·
I can use the octet rule and Lewis Dot Structures for cations and anions to describe ionic bonds.·
I can describe single, double, triple and coordinated covalent bonds·
I can explain how the chemical bonds between atoms in molecules such as H2 , CH4 , NH3 , H2 CCH2 , N2 , Cl2 , and many large biological molecules are covalent.·
I understand the ideas of VESPR or Valence Electron Shell Pair Repulsion theory.·
I can explain the ideas of hybrid orbits.Reasoning Targets
·
I can evaluate the polarity of bonds in terms of electronegativity using electronegativity values in the period table.Skill Targets
·
Students will construct models of ionic and covalently bonded atoms.Product Targets
·
I will create drawings of atomic structures using Valence Shell Electron Pair Repulsion, VSEPR, and hybrid orbital ideas.20 minutes Mini Lecture: Valence shell electron-pair repulsion theory (VSEPR)
10 minutes Introduction to the activity Laboratory 22: Shapes of covalent Molecules and Polarity
20 minutes Perform laboratory 22: Shapes of Covalent Molecules and Polarity
Homework - SQ3R pages 452-459
Chemistry Schedule Chapter 15: Ionic Bonding and Ionic Compounds
and Chapter 16: Covalent Bonds (Semester 2: Week 8 March 12-16)
Monday: Shapes of Covalent Molecules and Polarity and Hybridization and Resonance
Knowledge Targets
·
I can use the octet rule and Lewis Dot Structures for cations and anions to describe ionic bonds.·
I can describe single, double, triple and coordinated covalent bonds·
I can explain how the chemical bonds between atoms in molecules such as H2 , CH4 , NH3 , H2 CCH2 , N2 , Cl2 , and many large biological molecules are covalent.·
I understand the ideas of VESPR or Valence Electron Shell Pair Repulsion theory.·
I can explain the ideas of hybrid orbits.Reasoning Targets
·
I can evaluate the polarity of bonds in terms of electronegativity using electronegativity values in the period table.Skill Targets
·
Students will construct models of ionic and covalently bonded atoms.Product Targets
·
I will create drawings of atomic structures using Valence Shell Electron Pair Repulsion, VSEPR, and hybrid orbital ideas.10 minutes Review the activity Laboratory 22: Shapes of covalent Molecules and Polarity
30 minutes Finish collecting the data for the laboratory
10 minutes Answer the questions from the laboratory
Homework Answer the questions from the laboratory
Tuesday: Review for the Test on Chapters 15 and 16 Bonding
Knowledge Targets
·
I can use the octet rule and Lewis Dot Structures for cations and anions to describe ionic bonds.·
I can describe single, double, triple and coordinated covalent bonds·
I can explain how the chemical bonds between atoms in molecules such as H2 , CH4 , NH3 , H2 CCH2 , N2 , Cl2 , and many large biological molecules are covalent.·
I understand the ideas of VESPR or Valence Electron Shell Pair Repulsion theory.·
I can explain the ideas of hybrid orbits.Reasoning Targets
·
I can evaluate the polarity of bonds in terms of electronegativity using electronegativity values in the period table.Skill Targets
·
Students will construct models of ionic and covalently bonded atoms.Product Targets
·
I will create drawings of atomic structures using Valence Shell Electron Pair Repulsion, VSEPR, and hybrid orbital ideas.25 minutes Mini lecture on hybridization and resonance
25 minutes Worksheet on hybridization
Homework - Questions 13-18 on page 459
Wednesday and Thursday: Review for the Test on Chapters 15-16
20 minutes Go over the homework
30 minutes Mini Lecture on Attraction between molecules
20 minutes Class review for the test on Chapter 15 and 16
30 minutes Finish Spiral notebooks.
Friday: Test on Chapters 15-16
5 minutes Collect the spiral notebooks and hand out the test
40 minutes Begin the poster test on chapters 15 and 16
Homework Work on test
Chemistry Schedule
Semester 2: Week 9 March 19-23
Monday: Finish the Test on Chapters 15-16 Chemical Bonding
50 minutes - Test on Chapters 15-16
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