Chapter 1: Problem 46
Draw structural formulas for the three tertiary \(\left(3^{\circ}\right)\) amines with the molecular formula \(\mathrm{C}_{5} \mathrm{H}_{13} \mathrm{~N}\).
Chapter 1: Problem 46
Draw structural formulas for the three tertiary \(\left(3^{\circ}\right)\) amines with the molecular formula \(\mathrm{C}_{5} \mathrm{H}_{13} \mathrm{~N}\).
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Get started for freeWhich molecules are polar? For each that is polar, specify the direction of its dipole moment. (a) \(\mathrm{CH}_{2} \mathrm{Cl}\), (b) \(\mathrm{HCN}\) (c) \(\mathrm{H}_{7} \mathrm{O}\),
Draw Lewis structures for these ions and show which atom in each bears the formal charge. (a) \(\mathrm{CH}_{3} \mathrm{NH}_{3}^{+}\) (b) \(\mathrm{CO}_{3}{ }^{2-}\) (c) \(\mathrm{OH}^{-}\)
Identify the atom that has each ground-state electron configuration. (a) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{4}\) (b) \(1 s^{2} 2 s^{2} 2 p^{4}\)
Write Lewis structures for these ions. Show all valence electrons and all formal charges. (a) Amide ion, \(\mathrm{NH}_{2}{ }^{-}\) (b) Bicarbonate ion, \(\mathrm{HCO}_{3}{ }^{-}\) (c) Carbonate ion, \(\mathrm{CO}_{3}{ }^{2-}\) (d) Nitrate ion, \(\mathrm{NO}_{3}^{-}-\) (e) Formate ion, \(\mathrm{HCOO}^{-}\) (f) Acetate ion, \(\mathrm{CH}_{3} \mathrm{COO}^{-}\)
Describe the bonding in these molecules in terms of hybridization of \(\mathbf{C}\) and \(\mathbf{N}\) and the types of bonds between carbon and nitrogen. If there are any lone pairs, describe what type of orbital contains these electrons. (a) \(\mathrm{CH}_{3} \mathrm{CH}=\mathrm{CH}_{2}\) (b) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\)
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