L D.2

Molecule Puzzles

Name:

Purpose The purpose of this activity is to fit Lewis dot diagrams for atoms together to construct a molecule, then learn to feel comfortable drawing dot and line structures for molecules.

PART

A

Directions: Working in pairs, use the puzzle pieces you cut out for homework last night to build (one at a time) the Lewis Dot Diagrams for the covalent molecules below. In each of these compounds, only one pair of electrons is shared by any two atoms (this is called a single bond). The remaining electrons are called lone pairs or unpaired electrons. From your completed puzzle, draw what each molecule looks like by replacing each pair of shared electrons with a line (bond). Use the HF example below as a guide.

The first molecule below is HF. Grab an H. Grab an F. Fit them together so that the octet rule is satisfied, like so: Then, draw what you’ve made in the Dot Structure box. Then, replace the bonded pair electrons with lines and draw that result in the Line Structure box. See below.

Covalent Molecule

Dot Structure

Line Structure

HF

CH4 (1 carbon atom, 4 hydrogen atoms)

NH3 (1 nitrogen atom, 3 hydrogen atoms)

1

Duell

Covalent Molecule

Dot Structure

Line Structure

H 2O (2 hydrogen atoms, 1 oxygen atom)

C 2H 6 (2 carbon atoms, 6 hydrogen atoms)

CH2ClBr (1 carbon atom, 2 hydrogen atoms, 1 chlorine atom, 1 bromine atom)

PH3 (1 phosphorus atom, 3 hydrogen atoms)

N 2H 4 (2 nitrogen atoms, 4 hydrogen atoms)

SCl2 (1 sulfur atom, 2 chlorine atoms)

2

Duell

PART

B

Directions: Working in pairs, use the puzzle pieces you cut out for homework last night to build (one at a time) the Lewis Dot Diagrams for the covalent molecules below. In each of these compounds, two pairs (a double bond) or even three pairs (a triple bond) of electrons may be shared between any two atoms. From your completed puzzle, draw what each molecule looks like by replacing each pair of shared electrons with a line (bond). If two atoms share four electrons, then draw two lines (double bond). Or if two atoms share six electrons, then draw three lines (triple bond). Use the O2 example below as a guide.

The first molecule below is O2. Grab an O. Grab another O. Can you fit them together so that each has 8 valence electrons? If not, try grabbing a different type of O to fit together, like so:

Then, draw what you’ve made in the Dot Structure box. Then, replace the bonded pair electrons with lines and draw that result in the Line Structure box. See below. Covalent Molecule

Dot Structure

Line Structure

O2

N2 (2 nitrogen atoms)

HCN (1 hydrogen atom, 1 carbon atom, 1 nitrogen atom)

3

Duell

Covalent Molecule

Dot Structure

Line Structure

C 2H 4 (2 carbon atoms, 4 hydrogen atoms)

N 2H 2 (2 nitrogen atoms, 2 hydrogen atoms)

4

Duell

5

Duell

6

Duell

7

Duell

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