In each row check off the boxes that apply to the highlighted reactant. reaction The highlighted reactant acts as a... (check all that apply)

1. HCH3CO2(aq) + NH3(aq) → CH3CO−2(aq) + NH+4(aq)
A. Brønsted-Lowry acid
B. Brønsted-Lowry base
C. Lewis acid
D. Lewis base

2. BH3(aq) + NH3(aq) → BH3NH3(aq)
A. Brønsted-Lowry acid
B. Brønsted-Lowry base
C. Lewis acid
D. Lewis base

3. HNO2(aq) + C2H5NH2(aq) → NO−2(aq) + C2H5NH+3(aq)
A. Brønsted-Lowry acid
B. Brønsted-Lowry base
C. Lewis acid
D. Lewis base

The given question is incomplete. The complete question is :

In each row check off the boxes that apply to the underlined reactant. The underlined reactant acts as a... (check all that apply)

1.

here underlined is

A. Brønsted-Lowry acid

B. Brønsted-Lowry base

C. Lewis acid

D. Lewis base

2.

Here underlined is

A. Brønsted-Lowry acid

B. Brønsted-Lowry base

C. Lewis acid

D. Lewis base

3.

Here underlined is

A. Brønsted-Lowry acid

B. Brønsted-Lowry base

C. Lewis acid

D. Lewis base

1. Brønsted-Lowry acid

2. Lewis base

3. Brønsted-Lowry base

Explanation:

According to the Bronsted Lowry conjugate acid-base theory, an acid is defined as a substance which donates protons and a base is defined as a substance which accepts protons.

According to the Lewis concept, an acid is defined as a substance that accepts electron pairs and base is defined as a substance which donates electron pairs.

1.  

As is donating a proton , it acts as a bronsted acid.

2.

As contains a lone pair of electron on nitrogen , it can easily donate electrons to and act as lewi base.

3.  

As is accepting a proton , it acts as a bronsted base.

the number of valence electrons for each molecule or ion is shown beneath the structure. remember hydrogen will not have more than two electrons. this hydrogen is part of a covalent bond (sharing two electrons). a double bond here would cause hydrogen to share four electrons with phosphorus.