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Chemical bonding questions

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1. Consider you would expect a BeF2 molecule to be linear but an SF2 molecule to be angular.

2. a) How would you designate the hybrid orbitals formed by "mixing" one d one s and two p orbitals?

b) How many of the hybrid orbitals would be formed by the mixing?

3. Explain why C20H40 is a solid at 25oC, while C4H8 is a gas at 25oC?

I did a experiment on bonding in liquids. Here are my observations; could you please assist in answering the questions?

Observations

See attached file for full problem description.

Questions

1. Name the types of intermolecular bonding present in each of the liquids used in the experiment.

2. In terms of intermolecular bonding, explain the relative differences in time taken for the vortex to disappear in each liquid.

3. Why is water so much different from the other two substances in each liquid.

4. With the same type of agitation and at the same temperature, why would sugar dissolve in water much faster than does salt?

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1. Consider why you would expect a BeF2 molecule to be linear but an SF2 molecule to be angular.

Answer - BeF2 is more likely to be ionic with 2 single bonds. The farthest that two bonding electrons can get from each other is 180° apart, making BeF2 linear.
S has 6 valence electrons which comprise two pairs and two unpaired electrons. These unpaired electrons form covalent bonds with each F atom, resulting in a total of 4 electron pairs around the S atom. The farthest that 4 electron pairs can get from each other is when they are directed towards the corners of a tetrahedron, or about 109° apart. Hence, making an SF2 molecule angular.

2. a) How would you designate the hybrid orbitals formed by "mixing" one d one s and two p orbitals?

Answer - When mixing one d orbital, one s orbital and 2 p orbitals you get dsp2.

b) How many of the hybrid orbitals would be formed by the mixing?

Answer - The number you put in is ...

Solution Summary

Types of intermolecular bonding and their properties.

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See Also This Related BrainMass Solution

Covalent and Ionic Bonding

Research the answers to the following questions on the internet and write your answers in your own words. For each answer, include the address of the web site (or title and author of a book or article) that you used to help you answer the question.

1. Which type of compound usually has higher melting points: ionic compounds or covalent compounds? What is the reason for this difference in melting points? (3 points)

2. Do ionic compounds conduct electricity as: (3 points)
1. Solids?
2. Liquids?
3. Aqueous solutions (when the ionic compounds are dissolved in water)?

3. Do covalent compounds conduct electricity as: (3 points)
1. Solids?
2. Liquids?
3. Aqueous solutions (when the covalent compounds are dissolved in water)?

4. Explain the differences between ionic and covalent bonding that account for the differences in their melting points.

5. In order to conduct an electrical current, a substance must have charged particle s (ions or electrons) that are free-moving (able to move about throughout the sample).

6. Why do you think ionic compounds are not able to conduct electricity as solids, even though they can as liquids and in solution?

7. why do you think pure (distilled) water does not conduct electricity but tap water usually does?

Part II

Molecular Model for your models of H2O, NH3, CH4, and CO2.
1. Use the information from the lesson to determine the answers to the questions below.
Conclusion:
For each of your molecules, answer the following questions:
1. Determine the electronegativity between the atoms of each molecule.
2. Identify the bond as either ionic or covalent.
3. State whether the molecule is polar or non polar.
4. Identify the structure as having hydrogen bonding, dipole-dipole moments or London dispersion forces (LDF).

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