Answer:
D.) When HX adds to an asymmetrical alkene, the halogen attaches to the least substituted sp² carbon.
Explanation:
Which of the following statements is NOT true?
A.) When HX adds to an asymmetrical alkene, the sp² carbon bonded to the most H atoms is protonated. TRUE. This is known as Markovnikov's rule.
B.) When HX adds to an asymmetrical alkene, protonation leads to the most stable carbocation intermediate. TRUE. The order of stability of carbocations is tertiary > secondary > primary.
C.) When HX adds to a symmetrical alkene, either of the sp² carbons can be protonated. TRUE. Since the alkene is symmetrical, either carbon can be protonated.
D.) When HX adds to an asymmetrical alkene, the halogen attaches to the least substituted sp² carbon. FALSE. The halogen attaches to the most substituted sp² carbon.
Bromine is a reddish-brown color.
Benzene is clear or colorless
According to Le cha telier's principle when we increase the pressure of a equilibrium reaction the reaction shift to the side where few moles of gas present.
Your reaction (Notice - I guess the reaction you written is wrong, but still I'm solving with your given prediction)
3NaI (g) + H2 (g) = 2NaHI (g)
Where access of sodium iodide is reacting with Hydrogen gas to form NaHI molecule.
Number of moles of gas on reaction side - 3+2 = 5 moles
Number of moles of gas on product side - 2 moles
<em>Conclusion- the reaction will shift to the right of the reaction</em>
The wording of your question is a bit strange (we usually don't say that bonds have IMFs and ionic compounds don't consist of molecules), but the answer to your question has to do with bond polarity. Strong IMFs are associated with very polar bonds (because increased polarity means greater magnitudes of charges at the poles and, hence, greater electrostatic attraction). Since ionic bonds involve the transfer of entire units of charge (to form cations and anions), they are highly polar (and highly polar means strong IMFs). Polarity in covalent bonds, however, does not arise from transfer of entire units of charge. Rather, they involve unequal sharing of electrons, and thus partial charge. Covalent bonds are, therefore, not as polar as ionic bonds (and less polar means weaker IMFs). I think it would be a good idea to keep in mind, though, that your question should be more along the lines of "Why are ionic bonds more polar than covalent bonds?".