PLEASE help!!! chemistry!!!?

Question

I would be so grateful for ANY help!!!!

Consider the following unbalanced single-displacement redox reaction.

potassium(s) + zinc nitrate (aq) ----> potassium nitrate(aq) + zinc(s)

a. Write the balanced molecular, ionic, and net-ionic equation (using molecular formulas or ions as appropriate). Include all subscripts (s, aq...)

molecular:

ionic:

net-ionic:

b. Specify the species from the net-ionic equation that is oxidaized and reduced. Justify your answers.

Species oxidized:
reason:

Species reduced:
reason:

Answer 1

a. Molecular: 2K(s) + Zn(NO3)2(aq) --> 2KNO3(aq) + Zn(s)
ionic: 2K(s) + Zn2+(aq) + 2NO3-(aq) --> 2K+(aq) + 2NO3-(aq) + Zn(s)
Net-ionic: 2K(s) + Zn2+(aq) --> 2K+(aq) + Zn(s)

b. Potassium (K) is oxidized. Reason: It's oxidizing number INCREASES from 0 to +1.
Zinc (Zn) is reduced. Reason: It's oxidizing number decreases from +2 to 0.

Answer 2

Molecular:

2 K + Zn(NO3)2 --> 2 KNO3 + Zn

Ionic:

2 K(s) + Zn[2+](aq) + 2 NO3[-](aq) --> 2 K[+](aq) + Zn(s) + 2 NO3(aq)

Net Ionic is same as Ionic, but without the Nitrates (they cancel out)

Potassium is oxidized since its charge increases from neutral to 1+ (it has lost electrons)

Zinc is reduced since its charge decreases from 2+ to neutral (it has gained electrons)