Chemistry
1. Experimental evidence suggests that the nitrogen atom in ammonia, NH3, has four identical orbitals in the shape of a pyramid or tetrahedron.
a) Draw an energy-level diagram to show the formation of these hybrid orbitals (hint: no electron promotion is required)
b) Name the type of hybrid orbitals found in NH3, of the four hybrid orbitals on the N atom, how many will take part in bonding? Explain
c) Draw for yourself the energy-level diagram showing the hybrid orbitals formed in the C atom when it bonds. Now look at those hybrid orbitals and those of the N atom, and describe how the bonding with a N atom will differ with the bonding that occurs with a C atom, even though both atoms have four hybrid orbitals oriented in a tetrahedral shape.
2. For the ion IO3-,
a) Draw the electron dot diagram and structural formula using the method as taught in this course.
b) Predict the shape.
c) Predict whether it is polar or non-polar, and justify your prediction. Indicate the positive and negative poles.
3. For the molecule CHCl3,
a) Draw the electron dot diagram and structural formula.
b) Predict the shape
c) Predict whether it is polar or non-polar, and justify your prediction. Indicate the positive and negative poles.
4. Consider the following boiling point data for these halogen molecules.
a) Explain the trend in the boiling points of the halogens by describing the intermolecular forces present. (3 marks)
b) Plot a graph of boiling point against the number of electrons. What force is directly related to number of electrons? (4 marks)
c) Use you graph to predict the boiling point of astatine, the remaining member of the halogen family. (1 marks)
5. The molar masses and boiling points of two carbon compounds are given in the following table. Why is there such a large difference between them in boiling point, despite their similarity in molar mass? (Hint: set up a page with columns as was done in the first set of support questions in lesson 4.) (3 marks)
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