Concept explainers
(a)
Interpretation:
The molecule having a higher boiling point is to be determined, and the reason for it is to be explained.
Concept introduction:
Compounds with strong intermolecular forces have higher boiling points. The dominant intermolecular interaction between nonpolar molecules is called induced dipole–induced dipole interactions or London dispersion forces. Induced dipole–induced dipole interactions between the molecules tend to increase in strength as the contact surface area increases. As the length of the carbon chain increases, the surface area of the molecule also increases. Hence the compounds having a larger surface area have a higher boiling point than the ones having a smaller surface area.
(b)
Interpretation:
The molecule having a higher boiling point is to be determined, and the reason for it is to be explained.
Concept introduction:
Compounds with strong intermolecular forces have higher boiling points. The dominant intermolecular interaction between nonpolar molecules is called induced dipole–induced dipole interactions or London dispersion forces. Induced dipole–induced dipole interactions between the molecules tend to increase in strength as the contact surface area increases. As the length of the carbon chain increases, the surface area of the molecule also increases. Hence the compounds having a larger surface area have a higher boiling point than the ones having a smaller surface area.
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Organic Chemistry: Principles and Mechanisms (Second Edition)
- Draw the curved arrows to show the resonance structure for the following molecules. ( there are 3 molecules )arrow_forwardPlease answer this asap.. you can see the example on the other picture Instruction: Identify the hybrid orbitals used in the given moleculesarrow_forwardProblem What amount (mol) of each ion is in each solution?(a) 5.0 mol of ammonium sulfate dissolved in water(b) 78.5 g of cesium bromide dissolved in water(c) 7.42×1022 formula units of copper(II) nitrate dissolved in water(d) 35 mL of 0.84 M zinc chloridePlan We write an equation that shows 1 mol of compound dissociating into ions. (a) We multiply the number of moles of ions by 5.0. (b) We first convert grams to moles. (c) We first convert formula units to moles. (d) We first convert molarity and volume to moles.arrow_forward
- 4)On the following molecules, draw the curved arrows to convert the left-hand resonance structure form to the right-hand resonance structure formarrow_forwardDescribe with words how you would draw the curved arrow(s) to get to the more stable resonance form for the left-hand pair. Be sure to include how many curved arrows are needed and what atom (or bond) the electrons are coming from or going to. Do the same for the resonance pair on the right-hand side. more stable more stablearrow_forwardFor the molecule shown, what orbital is the lone pair in?arrow_forward
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- Which member in each of the following pairs would have a higher boiling point ?Explain.arrow_forwardProblem Draw Lewis structures for the following:(a) Ethylene (C2H4), the most important reactant in the manufacture of polymers(b) Nitrogen (N2), the most abundant atmospheric gasPlan We show the structure resulting from steps 1 to 4: placing the atoms, counting the total valence electrons, making single bonds, and distributing the remaining valence electrons in pairs to attain octets. Then we continue with step 5, if needed.arrow_forwardOnly typed explanation otherwise leave it Which of these compounds would have the highest boiling point?arrow_forward
- Organic Chemistry: A Guided InquiryChemistryISBN:9780618974122Author:Andrei StraumanisPublisher:Cengage Learning