General Chemistry 2, 3d Lewis structure

Question

Draw the three-dimensional shapes (draw good Lewis structure first) Of the reactants and products of the following single step reaction then draw the most likely form of the transition state for the reaction indicate in your transition state, drawing the bonds that are breaking and forming.

NO+Cl2 —-> NOCl2

consider the reaction in the previous question draw an example of a collision that would not lead to reaction, even if the reactant molecules had very high kinetic energies(use arrows to show the direction of travel of each reactant)

Answer 1

1. Lewis Structures and Molecular Shapes

Reactants:

1. NO (Nitric Oxide):
2. Lewis Structure: N=O
3. Shape: Linear
4. Bonding: There is a triple bond between N and O.
5. Cl2 (Chlorine Gas):
6. Lewis Structure: Cl-Cl
7. Shape: Linear
8. Bonding: There is a single bond between the two Cl atoms.

Product:

1. NOCl2 (Nitrosyl Chloride):
2. Lewis Structure:

Cl

|

Cl-N=O

1. Shape: The shape around the nitrogen will be trigonal pyramidal. This is due to the presence of a lone pair on the nitrogen atom.

2. Transition State

For the reaction: NO+Cl2→NOCl2NO+Cl2​→NOCl2​

Transition State Description:

1. Reactants in Transition State:
2. The N-O bond in NO is partially breaking.
3. The Cl-Cl bond in Cl2 is partially breaking.
4. New N-Cl bonds in NOCl2 are forming.

Drawing the Transition State:

1. The transition state can be represented by a structure where the N-O bond is partially broken, and the Cl-Cl bond is partially broken, while two new N-Cl bonds are starting to form.
2. Use dotted lines to show the partial bonds in the transition state.

Transition State Structure:

Cl

|

Cl-N—O

\

Cl

Bonds in the Transition State:

1. Partial N-O bond (breaking)
2. Partial Cl-Cl bond (breaking)
3. Partial N-Cl bonds (forming)

3. Collision Example That Would Not Lead to Reaction

Even if reactant molecules have high kinetic energy, the collision must be oriented correctly to result in a reaction. A collision with incorrect orientation will not lead to a reaction.

Example of Incorrect Collision:

If NO and Cl2 molecules collide, but not in the correct orientation, the collision might not result in a reaction.

Drawing:

NO Cl2

\ /

\ /

\ /

X

Here, the molecules are not oriented in a way that would allow for effective overlap of the orbitals needed for bond formation or breaking. The X denotes an ineffective collision where no reaction occurs.

Arrows for Direction of Travel:

NO → (right direction)

Cl2 → (left direction)

In this example, the direction of travel is not aligned for a successful reaction to occur despite high kinetic energy.