Name___________________________________ Per. ______

Bonding- Chapter 6 OTHS Academic Chemistry

Objectives: Construct electron dot formulas to illustrate ionic and covalent bonds

Describe the nature of metallic bonding and apply the theory to explain metallic properties such as thermal and electrical conductivity, malleability, and ductility

Predict molecular structure for molecules with linear, trigonal planar, or tetrahedral electron pair geometries using Valence Shell Electron Pair Repulsion (VSEPR) theory

Describe the unique role of water in chemical and biological systems

Vocabulary: Bond, metallic bond, ionic bond, covalent bond, valence electrons, energy level, octet, malleable, ductile, lustrous, opaque, cation, anion, Lewis structure, structural formula, resonance, VSEPR, molecular geometry, lone pair, single bond, double bond, triple bond, intermolecular force, electronegativity, dipole, polarity, surface tension, and evaporate

Topics to Master: Difference between metallic, ionic, and covalent bonds

Properties of metals, ionic compounds, and molecular compounds

Correctly draw Lewis structures/structural formals for molecular compounds

Correctly identify a molecule’s molecular geometry based on the Lewis structure/ structural formula

Understand hydrogen bonding and its purpose/effect on water

Strong vs. weak intermolecular forces

Provided: Periodic Table

VSEPR Chart

CHECKLIST: How to be successful in OTHS Academic Chemistry

Pay attention and take notes in class Ask questions in class on material that is not clear Work every page in the practice packet for the unit Check answers to the practice packet online at http://othschem.weebly.com/ Come to tutorials with any chemistry teacher Do the online homework and check solutions once they become available Always do the practice test for every test & ask good questions on review day Keep up with the calendar for the class/be aware of approaching quizzes, tests, & other deadlines Use videos posted on website as a quick and convenient tutorial Read the chapter in the book

VSEPR Chart: Covalent Bonding

# of atoms bonded to

central atom

# of lone pairs on

central atom

Molecular Geometry

Sketch (Note: Bonds may not all be

single)

2

0

Linear

2

1

Bent 120o

2

2

Bent 109.5o

3

0

Trigonal Planar

3

1

Trigonal Pyramidal

4

0

Tetrahedral

Name___________________________________ Per. ____

Ionic OR Covalent Bonding?

Use your covalent bonding notes (pp. 1-3) to classify the following as characteristics of a compound that contains ionic (I) or covalent (C) bonding.

_____ 1. Contains a metal and a nonmetal ion (and possibly polyatomic ions)

_____ 2. Contains nonmetals and possibly metalloids

_____3. The smallest particle is the formula unit

_____ 4. The smallest particle is the molecule

_____ 5. Particles are held together by strong electrostatic forces

_____ 6. Particles are held together by relatively weak intermolecular forces

_____ 7. The elements in the compound share valence electrons

_____ 8. The elements in the compound gain and lose valence electrons

_____ 9. Are usually soluble in water

_____ 10. Are electrolytes when dissolved in water or molten (liquid)

_____11. Have low melting and boiling points

_____ 12. Have high melting and boiling points

_____ 13. Often exist as gases or vaporize easily at room temperature

_____ 14. Are hard crystalline solids at room temperature

_____ 15. Are soft if solid

_____ 16. Are rigid and brittle

_____ 17. An example is MgCl2

_____ 18. An example is CCl4

_____ 19. Its structure looks like this:

_____ 20. Its structure looks like this:

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Name______________________ Per. _____

Worksheet: Lewis Structures

Calculations Lewis Structure Structural Formula 1. PBr3 phosphorus tribromide N = A = S =

2. CO2 carbon dioxide N = A = S =

3. H2O2 hydrogen peroxide N = A = S =

4. N2 nitrogen N = A = S =

5. O2 oxygen N = A = S =

2

6. NH3 ammonia N = A = S =

7. NO3 -1 nitrate ION

N = A = S =

8. CO3 2- carbonate ION N = A = S =

9. HCl hydrogen chloride N = A = S =

10. C2H4 ethene N = A = S =

11. C2H2 acetylene N = A = S =

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Name____________________________ Per. _____ VSEPR Worksheet

Draw the Lewis structure for each molecule or ion and then determine the geometry (shape). Use the chart in your notes. Molecule or Ion Lewis Structure Molecular Geometry (shape)

(e.g. tetrahedral, etc.) 1.

SO2

2.

CO2

3.

SCl2

4.

PH3

5.

BF3

6.

NO3 –

7.

CCl4

8.

H2S

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Name___________________________________ Per. ______ Wondrous Water

Read the article and answer the following questions:

1. Why is a compound as common as water considered a “weird” chemical substance? 2. Which atoms make up a water molecule? What holds the atoms in a water molecule together?

3. Water exists in three forms:

4. How does temperature affect water?

5. Explain how water molecules move through the water cycle.

6. Why does life on Earth depend on the water cycle?

7. Explain the difference between cohesion and adhesion. Give an example of each.

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8. Water molecules move from a plant’s roots to its leaves. How?

9. Why don’t water striders sink?

10. Why doesn’t ice sink?

11. How do the oceans help control Earth’s climate?

12. Explain how pollution and water are related?

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