Intramolecular bonding, chemistry homework help

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Homework #6G (Ch. 10-12) 1. Which are stronger, intermolecular or intramolecular forces for a given molecule? What observation(s) have you made that supports this position? Explain. 2. The enthalpy of vaporization of water is about seven times larger than water’s enthalpy of fusion (41 kJ/mol vs. 6 kJ/mol). What does this tell us about the relative similarities among the solid, liquid, and gaseous state of water? 3. Discuss the types of intermolecular forces acting in the liquid state of each of the following substances. a. Kr b. S8 c. NF3 d. H2O 4. Which substance in each pair would be expected to be more volatile at a particular temperature? Explain your reasoning. a. H2O(l) or H2S(l) b. H2O(l) or CH3OH(l) c. CH3OH(l) or CH3CH2OH(l) 5. Which of the substances in each of the following sets would be expected to have the highest boiling point? Explain why. a. Ga, KBr, O2 b. Hg, NaCl, He c. H2, O2, H2O 6. Which of the substances below exhibit hydrogen bonding interactions? a. CCl2H2 b. BeF2 c. NO3d. HCN 7. You have equal masses of different solutes dissolved in equal volumes of solution. Which of the solutes listed below would make the solution with the highest concentration measured in molarity? Defend your answer. NaCl, MgSO4, LiF, KNO3 8. As with all quantitative problems in chemistry, make sure not to get “lost in the math.” In particular, work on visualizing solutions at a molecular level. For example, consider the following. You have two separate beakers with aqueous solutions, one with 4 “units” of potassium sulfate and one with 3 “units” of barium nitrate. a. Draw molecular-level diagrams of both solutions. b. Draw a molecular-level diagram of the mixture of the two solutions before a reaction has taken place. c. Draw a molecular-level diagram of the product and solution formed after the reaction has taken place. 9. How many grams of KBr are contained in 125 g of a 6.25% (by mass) KBr solution? 10. For each of the following solutions, the mass of solute is given, followed by the total volume of the solution prepared. Calculate the molarity of each solution. a. 5.59 g CaCl2; 125 mL b. 2.34 g CaCl2; 125 mL c. 8.73 g CaCl2; 125 mL d. 11.5 g CaCl2; 125 mL 11. Calculate the new molarity that results when 250. mL of water is added to each of the following solutions. a. 124 mL of 0.251 M HCl b. 445 mL of 0.499 M H2SO4 c. 5.25 L of 0.101 M HNO3 d. 11.2 mL of 14.5 M HC2H3O2 12. A 50.00 mL sample of aqueous Ca(OH)2 requires 34.66 mL of a 0.944M nitric acid for neutralization. Calculate the concentration (molarity) of the original solution of calcium hydroxide. 13. Write a chemical equation showing how each of the following species can behave as indicated when dissolved in water. a. O2- as a base b. NH3 as a base c. HSO4- as an acid d. HNO2 as an acid 14. Calculate the hydrogen ion concentration and the hydroxide ion concentration in moles per liter, for solutions with each of the following pH values. a. pH = 1.04 b. pH = 13.1 c. pH = 5.99 d. pH = 8.62 15. What two components make up a buffered solution? Give as example of a combination that would serve as a buffered solution. Which component of a buffered solution consumes added strong base? Using your example from above, show how this component would react with added NaOH.
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1. Intramolecular bonding.
Reason:- Consider a vessel full of water. The water molecules are associatted by intermolecular
hydrogen bonding. When we heat the water in that vessel , it is found that these intermolecular bonding
breaks and change of state takes place( from liquid to gas). In a water molecule , there is two hydrogen
and one oxygen. The bond that holds these atoms are called intramolecular bonding. When the water as
reached its boiling point ( 100 degrees) , the water molecules , without breaking into it's constitutent
element goes to vapour state.
Hence , intramolecular bonding is stronger than intermolecular bonding

2. Enthalpy of fusion is the amount of heat required to change the state from solid to liquid state.
Enthalpy of vapourisation is defined as the amount of heat required to change the phase from liquid to
vapour. It is found that enthalpy of vapourisaion is 7 times larer than enthalpy of fusion , due to the fact
that , More amount of energy is needed to convert the water from liquid to vapour than converting it
from solid to liquid. This signifies that...


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