Molecular Geometry Quiz



Name _____________________________________Period_______Date_______

Unit 12 Test Review: Bonding & Molecular Geometry

I. Vocabulary

Fill in the blanks below:

A. A(n) _________________is a force that holds 2 atoms together.

B. A(n) ________________bond consists of shared electrons.

Name an example:________________

C. A(n) _____________bond consists of transferred electrons.

Name an example: _________________

D. In the __________________model:

- Once the Lewis structure is drawn determine the shape

-shapes are formed to create the greatest distance between electrons (remember they __________________each other)

E. The general character and type of a chemical bond can be predicted using the ___________________________difference (∆E.N.) of the elements that are bonded (use the chart and subtract).

II. Lewis Dot Structures

For each of the following, draw the appropriate Lewis dot structure.

A. Carbon atom

B. Nitrogen atom

C. Fluoride ion

III. Covalent Compounds, Lewis Dot Structures, Geometry, Polarity & Hybridization

For each of the following formulas fill in the columns as indicated.

|Formula |Electron Dot Structure |AXE Designation |Name of Shape (Molecular |Polarity |

| | | |Geometry) |(Polar or nonpolar) |

| | | | | |

| | | | | |

|H2Se | | | | |

| | | | | |

| | | | | |

| | | | | |

|PCl3 | | | | |

| | | | | |

| | | | | |

| | | | | |

|PBr4+ | | | | |

| | | | | |

| | | | | |

| | | | | |

| | | | | |

|NF3 | | | | |

| | | | | |

| | | | | |

| | | | | |

|H2O | | | | |

| | | | | |

| | | | | |

| | | | | |

| | | | | |

| | | | | |

|CO2 | | | | |

| | | | | |

|N2 | | | | |

| | | | | |

| | | | | |

| | | | | |

| | | | | |

| | | | | |

|SO42- | | | | |

| | | | | |

| | | | | |

| | | | | |

|PO43- | | | | |

| | | | | |

| | | | | |

| | | | | |

|OH 1- | | | | |

| | | | | |

| | | | | |

| | | | | |

|SO3 | | | | |

| | | | | |

IV. Electronegativity and Types of bonds

Use your electronegativity table to calculate the electronegativity differences between each pair of elements listed in the chart below. Then indicated whether the bond would be nonpolar covalent, polar covalent, or ionic.

| |Electronegativity Difference |Types of Bond |

|1. F-S | | |

|2. C-H | | |

|3. Rb-Cl | | |

|4. Be-Cl | | |

|5. C-O | | |

|6. Mg-O | | |

|7. F-F | | |

Information on Reference Sheet for Test:

• Also included: periodic table, table of electronegativity values

|AXE Notation |Molecular |3-D Shape |Bond |

| |Geometry | |Angles |

|AX2 |Linear |[pic] |180° |

|AX3 |Trigonal Planar |[pic] |120° |

|AX2E |Bent | |118° |

| | |A | |

| | |X X | |

|AX4 |Tetrahedral |[pic] |109.5° |

|AX3E |Trigonal Pyramid |[pic] |107° |

|AX2E2 |Bent |[pic] |104.5° |

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Table of Electronegativities

Bond Character Difference in electronegativity

Non polar 0.0( 0.4

Polar >0.4( 1.7

Ionic >1.7

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