Specify which hybrid orbitals are used by carbon atoms in these species: (a) $\mathrm{CO}$, (b) $\mathrm{CO}_2$, (c) $\mathrm{CN}^{-}$.

Write the ground-state electron configurations of the following transition metal ions: (a) $\mathrm{Sc}^{3+}$, (b) $\mathrm{Ti}^{4+}$, (c) $\mathrm{V}^{5+}$, (d) $\mathrm{Cr}^{3+}$, (e) $\mathrm{Mn}^{2+}$, (f) $\mathrm{Fe}^{2+}$, (g) $\mathrm{Fe}^{3+}$, (h) $\mathrm{Co}^{2+}$, (i) $\mathrm{Ni}^{2+}$, (j) $\mathrm{Cu}^{+}$, (k) $\mathrm{Cu}^{2+}$, (l) $\mathrm{Ag}^{+}$, (m) $\mathrm{Au}^{+}$, (n) $\mathrm{Au}^{3+}$, (o) $\mathrm{Pt}^{2+}$.

The electron configurations described in Chapter 2 all refer to gaseous atoms in their ground states. An atom may absorb a quantum of energy and promote one of its electrons to a higher-energy orbital. When this happens, we say that the atom is in an excited state. The electron configurations of some excited atoms are given. Identify these atoms and write their ground-state configurations:
$1 s^2 2 s^2 2 p^2 3 d^1$.

The electron configurations described in this chapter all refer to gaseous atoms in their ground states. An atom may absorb a quantum of energy and promote one of its electrons to a higher-energy orbital. When this happens, we say that the atom is in an excited state. The electron configurations of some excited atoms are given. Identify these atoms and write their ground-state configurations: (a) $1s^12s^1$
(b) $1s^22s^22p^23d^1$ (c) $1s^22s^22p^64s^1$ (d) $[\mathrm{Ar}]4s^13d^{10}4p^4$ (e) $[\mathrm{Ne}]3s^23p^43d^1$

What are the hybrid orbitals of the carbon atoms in the molecule $\mathrm{CH}_3 \mathrm{COOH}$.

What are the hybrid orbitals of the carbon atoms in the molecule $\mathrm{CH}_3 \mathrm{CH}=\mathrm{O}$.

What are the hybrid orbitals of the carbon atoms in the molecule $\mathrm{CH}_3-\mathrm{C} \equiv \mathrm{C}-\mathrm{CH}_2 \mathrm{OH}$.

What are the hybrid orbitals of the carbon atoms in the molecule $\mathrm{H}_3 \mathrm{C}-\mathrm{CH}=\mathrm{CH}_2$.

What are the hybrid orbitals of the carbon atoms in the molecule $\mathrm{H}_3 \mathrm{C}-\mathrm{CH}_3$.

What hybrid orbitals are used by nitrogen atoms in these species? (a) $\mathrm{NH}_3$, (b) $\mathrm{H}_2 \mathrm{N}-\mathrm{NH}_2$, (c) $\mathrm{NO}_3^{-}$.

Consider the reaction

$$\mathrm{BF}_3+\mathrm{NH}_3 \longrightarrow \mathrm{F}_3 \mathrm{B}-\mathrm{NH}_3$$

Describe the changes in hybridization of the B and N atoms as a result of this reaction.

Describe the change in hybridization of the $\mathrm{Al}$ atom in this reaction:

$$\mathrm{AlCl}_3+\mathrm{Cl}^{-} \longrightarrow\mathrm{AlCl}_4^{-}$$

What is the hybridization state of $\mathrm{Si}$ in $\mathrm{SiH}_4$ and in $\mathrm{H}_3\mathrm{Si}-\mathrm{SiH}_3$ ?

Describe the bonding scheme of the $\mathrm{AsH}_3$ molecule in terms of hybridization.