ch. 2 - covalent bonding and chemical...

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CH. 2 - COVALENT BONDING AND CHEMICAL REACTIVITY

CONCEPT: HYBRID ORBITAL THEORY

The Aufbau Principle states that electrons fill orbitals in order of increasing energy. If carbon has only two unfilled orbitals,

why does it like to make 4 bonds?

EXAMPLE: Carbon sp3 Hybridization

● Many atoms prefer to blend some of their 2nd shell orbitals together to make new _________________________ orbitals

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CONCEPT: HYBRIDIZATION SUMMARY

Hybridization can be predicted by the determine the number of ________ _________ on an atom

□ Where a bond site is equal to any _________ or _________ ___________

EXAMPLE: Predict the hybridization of the following reactive intermediates

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CONCEPT: MOLECULAR GEOMETRY

Molecular geometry is based on VSEPR theory: “Bond sites will ____________ each other as much as possible.”

□ The molecular geometry predicts what shape the hybridized atom will have.

EXAMPLE: Predict the hybridization and molecular geometry of the following selected atoms:

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PRACTICE: Determine the hybridization and molecular geometry of the following selected atoms:

a.

b.

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CONCEPT: ELECTRONEGATIVITY

Chemical bonds are formed when the sharing of valance electrons between two or more atoms takes place.

● The _____________ of sharing will determine the identity and strength of the chemical bond.

● An unequal sharing of electrons in one direction along a bond is called a __________ _____________ (______)

● The charge between any two bonded atoms is related to their difference in electronegativity

Generalizations:

● Bonds to carbon and hydrogen are always _______________

● Bonds between two identical atoms are always _________________

□ Adjacent atoms on the periodic table are _____________

□ Lone pairs are ____________

● ________ ________________ exist when atoms have asymmetrical dipoles

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PRACTICE: Which of the following molecules contain dipoles? Which contain net dipoles?

PRACTICE: Which of the solvents below is apolar? Which is polar?

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CONCEPT: INTERMOLECULAR FORCES

● IMF’s are what make molecules ______________. Without them everything would be _____________

● Boiling point / melting point questions are always directly referring to the strength of ___________ between molecules.

1. Hydrogen Bonding – (H) Bound to small, highly electronegative atoms: ___________________

2. Dipole-dipole (net dipole force)

3. Van der Waals (London Dispersion Forces)

□ Increase with:

a. Size b. Ring > Chain > Branched

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PRACTICE: Which of the following pairs of molecules would have the highest boiling point?

1. OR

2. OR

3. OR

4. OR

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CONCEPT: SOLUBILITY

Only one rule: _________ dissolves _________

EXAMPLE:

PRACTICE: Circle the following molecules would you expect to be miscible in an aqueous solution?

a. b.

c. d. e. f.

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CONCEPT: FUNCTIONAL GROUPS

● We can group several millions of different molecules into subsets of similar _________________________

1. Hydrocarbons

● All carbon groups regardless of size can be symbolized using an _______ group.

● When an alkane is attached to a greater carbon chain, it is given an ________ suffix. (i.e. __________ group)

● Carbons are given a “degree” based on how many other ____________ they are attached to

□ Hydrogens possess the __________ degree as the carbon they are attached to

□ Degrees are expressed as primary, secondary, tertiary and quaternary (1⁰, 2⁰, 3⁰, 4⁰)

EXAMPLE: Determine the degree of the indicated carbons and hydrogens

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2. Alkyl Halide _________

● Any –R group directly attached to a halogen.

● The degree of alkyl halide is determined the same way as __________________

The carbonyl ____________ is NOT a functional group, but it is a major component of many functional groups

3. Alcohol ____________ 6. Carboxylic Acid ______________(_________) ● Degree of alcohol is determined the same ● The acid of organic chemistry way as ____

4. Amine ______________ 7. Amide _______________(___________)

Degree of alcohol is determined the same ● Degree of alcohol is determined the same way as ____. way as ____.

5. Ether __________________ 8. Ester __________________(___________)

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9. Carbonyls

The term “ carbonyl” is not the proper name of the functional groups because the functionality of the group depends on its location on the carbon chain.

.

● Ketone ______________(__________) ● Aldehyde ______________(__________)

- _______________carbonyl group - _______________carbonyl group

10. Nitrile ________________

11. Benzene

● Directly attached to –R group _______________ (_________)(_____)

● Extra CH2 between –R group _______________ (_____________)(_____)

EXAMPLE: Identify all the functional groups in the following compound. Show degrees where applicable.

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12. Other Carbonyl Compounds

● Acyl Chloride (__________) ● Anhydride (_______________)

13. Sulfur Compounds

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PRACTICE: Identify all the functional groups in the following compound. Show degrees where applicable.

a.

b.

c.

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ch. 2 - covalent bonding and chemical...

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