Questions: Classify each species as a Lewis acid or a Lewis base. Lewis acid Lewis base Answer Bank BeCl2 SO3 NH3 Na+ O2-

Classify each species as a Lewis acid or a Lewis base.

Lewis acid
Lewis base

Answer Bank
BeCl2
SO3
NH3
Na+
O2-
Transcript text: Classify each species as a Lewis acid or a Lewis base. Lewis acid Lewis base Answer Bank $\mathrm{BeCl}_{2}$ $\mathrm{SO}_{3}$ $\mathrm{NH}_{3}$ $\mathrm{Na}^{+}$ $\mathrm{O}^{2-}$
failed

Solution

failed
failed

Solution Steps

Step 1: Understanding Lewis Acids and Bases

A Lewis acid is a species that can accept an electron pair, while a Lewis base is a species that can donate an electron pair.

Step 2: Classifying Each Species
  • $\mathrm{BeCl}_{2}$: Beryllium chloride can accept electron pairs due to the electron deficiency of beryllium, making it a Lewis acid.
  • $\mathrm{SO}_{3}$: Sulfur trioxide can accept electron pairs due to the presence of an empty d-orbital in sulfur, making it a Lewis acid.
  • $\mathrm{NH}_{3}$: Ammonia has a lone pair of electrons on the nitrogen atom, which it can donate, making it a Lewis base.
  • $\mathrm{Na}^{+}$: Sodium ion can accept electron pairs due to its positive charge, making it a Lewis acid.
  • $\mathrm{O}^{2-}$: Oxide ion has extra electrons and can donate electron pairs, making it a Lewis base.

Final Answer

  • Lewis acid: \(\mathrm{BeCl}_{2}, \mathrm{SO}_{3}, \mathrm{Na}^{+}\)
  • Lewis base: \(\mathrm{NH}_{3}, \mathrm{O}^{2-}\)

\[ \boxed{\text{Lewis acid: } \mathrm{BeCl}_{2}, \mathrm{SO}_{3}, \mathrm{Na}^{+}} \] \[ \boxed{\text{Lewis base: } \mathrm{NH}_{3}, \mathrm{O}^{2-}} \]

Was this solution helpful?
failed
Unhelpful
failed
Helpful