Description
This chemistry unit introduces the concept of atoms sharing valence electrons to gain full valence shells during covalent bonding. Electron sharing is contrasted with the transfer of electrons that enables atoms to achieve full valence shells during ionic bonding. Covalent bonds are distinguished as polar or nonpolar based on electronegativity difference and ionic bonds are recognized as a case of extreme electronegativity difference. Physical properties of covalent compounds are then contrasted with the physical properties of ionic compounds.
Next, Students learn how to draw Lewis structures for covalent molecules. Students will also learn to name binary inorganic covalent compounds.
In the final portion of this lecture valence shell electron pair repulsion (VSEPR) and hybrid orbital theory are introduced. Students apply VSEPR and hybrid orbitals to molecular Lewis structures to understand molecular geometry and associated molecular polarity.
Content has sufficient stretch to be a meaningful challenge most high school students. This unit is based around PowerPoint lecture slides that have been beautifully animated and contain speaker notes to guide you through each slide's content. The PowerPoint lecture notes also serve as a teaching/planning guide. The slides indicate at what point included activities should be completed. These activities include small guided lab, practice assignments, quizzes, a review game, a summative assessment, and a summative lab activity. Answer keys are typed and show step-by-step work for calculations. It is intended that students have access to practice assignment keys while working, however this access is optional. Learning objectives for this unit are listed below.
For more teaching materials on related chemistry topics other units are available and the entire year-long course "The Complete Chemistry Course" is available as a bundle.
Covalent Compounds Learning Objectives:
1. Explain the role and location of electrons in a covalent bond.
2. Describe the change in energy and stability as a covalent bond forms.
3. Use electronegativity to distinguish bond types.
4. Compare properties of ionic and covalent substances.
5. Draw Lewis structures for atoms.
6. Distinguish between single, double, and triple covalent bonds.
7. Draw Lewis structures for molecules.
8. Draw resonance structures when needed.
9. Name binary inorganic covalent compounds.
10. Understand VSEPR.
11. Understand hybrid orbital theory.
12. Apply VSEPR and hybrid orbital theory to Lewis structures.
13. Relate molecular properties to polarity.
Covalent Compounds Unit – Chapter 6
Highlights
Description
This chemistry unit introduces the concept of atoms sharing valence electrons to gain full valence shells during covalent bonding. Electron sharing is contrasted with the transfer of electrons that enables atoms to achieve full valence shells during ionic bonding. Covalent bonds are distinguished as polar or nonpolar based on electronegativity difference and ionic bonds are recognized as a case of extreme electronegativity difference. Physical properties of covalent compounds are then contrasted with the physical properties of ionic compounds.
Next, Students learn how to draw Lewis structures for covalent molecules. Students will also learn to name binary inorganic covalent compounds.
In the final portion of this lecture valence shell electron pair repulsion (VSEPR) and hybrid orbital theory are introduced. Students apply VSEPR and hybrid orbitals to molecular Lewis structures to understand molecular geometry and associated molecular polarity.
Content has sufficient stretch to be a meaningful challenge most high school students. This unit is based around PowerPoint lecture slides that have been beautifully animated and contain speaker notes to guide you through each slide's content. The PowerPoint lecture notes also serve as a teaching/planning guide. The slides indicate at what point included activities should be completed. These activities include small guided lab, practice assignments, quizzes, a review game, a summative assessment, and a summative lab activity. Answer keys are typed and show step-by-step work for calculations. It is intended that students have access to practice assignment keys while working, however this access is optional. Learning objectives for this unit are listed below.
For more teaching materials on related chemistry topics other units are available and the entire year-long course "The Complete Chemistry Course" is available as a bundle.
Covalent Compounds Learning Objectives:
1. Explain the role and location of electrons in a covalent bond.
2. Describe the change in energy and stability as a covalent bond forms.
3. Use electronegativity to distinguish bond types.
4. Compare properties of ionic and covalent substances.
5. Draw Lewis structures for atoms.
6. Distinguish between single, double, and triple covalent bonds.
7. Draw Lewis structures for molecules.
8. Draw resonance structures when needed.
9. Name binary inorganic covalent compounds.
10. Understand VSEPR.
11. Understand hybrid orbital theory.
12. Apply VSEPR and hybrid orbital theory to Lewis structures.
13. Relate molecular properties to polarity.
