Questions: Draw the Lewis structure for HSO4^- (where the H is bonded to an O atom) and answer the following questions: a) How many resonance structures are in the Lewis structure for HSO4^-?: 2 b) How many bonding electrons are in the Lewis structure for HSO4^-? 14 c) How many non-bonding electrons are in the Lewis structure for HSO4? 18 d) What is the bond order between S and the terminal O atoms? 1.5

Draw the Lewis structure for HSO4^- (where the H is bonded to an O atom) and answer the following questions:
a) How many resonance structures are in the Lewis structure for HSO4^-?: 2
b) How many bonding electrons are in the Lewis structure for HSO4^-? 14
c) How many non-bonding electrons are in the Lewis structure for HSO4? 18
d) What is the bond order between S and the terminal O atoms? 1.5

Transcript text: Draw the Lewis structure for $\mathrm{HSO}_{4}^{-}$(where the H is bonded to an O atom) and answer the following questions: a) How many resonance structures are in the Lewis structure for $\mathrm{HSO}_{4}^{-}$?: 2 - $\square$ b) How many bonding electrons are in the Lewis structure for $\mathrm{HSO}_{4}$-? 14 - $\square$ c) How many non-bonding electrons are in the Lewis structure for $\mathrm{HSO}_{4}$ ?: 18 - d) What is the bond order between S and the terminal O atoms?: 1.5 $\square$

Solution

Solution Steps

Step 1: Understanding the Lewis Structure of $\mathrm{HSO}_{4}^{-}$

The Lewis structure of $\mathrm{HSO}_{4}^{-}$ involves sulfur (S) as the central atom bonded to four oxygen (O) atoms, with one of these oxygens also bonded to a hydrogen (H) atom. The overall charge of the ion is $-1$.

Step 2: Determining Resonance Structures

Resonance structures occur when there are multiple valid Lewis structures for a molecule or ion. For $\mathrm{HSO}_{4}^{-}$, the negative charge can be delocalized over the oxygen atoms, leading to multiple resonance structures. Typically, there are two main resonance structures for $\mathrm{HSO}_{4}^{-}$.

Step 3: Counting Bonding Electrons

Bonding electrons are those involved in covalent bonds. In $\mathrm{HSO}_{4}^{-}$, sulfur forms double bonds with two of the oxygen atoms and single bonds with the other two (one of which is bonded to hydrogen). This results in a total of 16 bonding electrons (8 pairs).

Step 4: Counting Non-Bonding Electrons

Non-bonding electrons, or lone pairs, are those not involved in bonding. Each oxygen atom typically has 6 valence electrons, and after accounting for bonding, the remaining electrons are non-bonding. In $\mathrm{HSO}_{4}^{-}$, there are 20 non-bonding electrons.

Step 5: Calculating Bond Order

The bond order between sulfur and the terminal oxygen atoms is determined by the number of bonds divided by the number of oxygen atoms. With resonance, the bond order is averaged, resulting in a bond order of 1.5.