Concept explainers
(a)
Interpretation:
The approximate values for the indicated bond angles have to be given.
Concept Introduction:
Bond angle is the angle between two bonds of a molecule and it is determined based on the electron-domain geometry.
(b)
Interpretation:
The most polar bond in the molecule has to be given.
Concept Introduction:
The unequal distribution of shared electrons caused by differences in electronegativity between bonded atoms is called bond polarity.
Dipole moment: It is the measure of the charge separation that is describes the polar in the bond between the two atoms.
Electronegativity: It is defined as the capacity of the atom to abstract the pair of electrons towards itself results to have high negative charge.
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Chemistry: The Molecular Science
- Write the Lewis structures of both isomers with the formula C2H7N.arrow_forwardA carbene is a compound that has a carbon bonded to twoatoms and a lone pair remaining on the carbon. Manycarbenes are very reactive. (a) Draw the Lewis structurefor the simplest carbene, H2C. (b) Predict the length of thecarbon–carbon bond you would expect if two H2C moleculesreacted with each other by a combination reaction.arrow_forward(a) Triazine, C3 H3 N3, is like benzene except that in triazineevery other C¬H group is replaced by a nitrogen atom.Draw the Lewis structure(s) for the triazine molecule. (b) Estimatethe carbon–nitrogen bond distances in the ring.arrow_forward
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- (b) Name and describe the three energies associated with the formation of an ionic bond. Use your answer to explain why an ionic form of pure carbon is not observed in nature whereas common salt (NaCl) is an ionic solid.arrow_forward(a) Determine the formal charge of oxygen in the following structure. If the atom is formally neutral, indicate a charge of zero. (b) Draw an alternative Lewis (resonance) structure for the compound given in part (a). Show the unshared pairs and nonzero formal charges in your structure. Don't use radicals. Formal charge on O 0arrow_forwardAn elemental analysis of a hydrocarbon, which contains only carbon and hydrogen, shows the mass%: element mass% carbon 92.26 hydrogen 7.743 (A) * Determine the empirical formula of the hydrocarbon. (B) The compound has a molar mass of 26.04 g/mol. Determine its molecular formula. (C, Draw the Lewis structure of the molecular compound. Count the total number of sigma bonds and pi bonds each, present in the molecule. (D, What is the hybridization of carbon in the molecule? Explain.arrow_forward
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- Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning