Magnetic and acidic properties of nitric oxide I was faced with the following question:

PART C – CHEMISTRY
Which one of the following properties is not shown by $\ce{NO}$?

It combines with oxygen to form nitrogen dioxide

Its bond order is $2.5$

It is diamagnetic in the gaseous state

It is a neutral oxide



I am confused about (3) &amp; (4). I know $\ce{NO}$ reacts with water &amp; oxygen to produce $\ce{HNO2}$, and then $\ce{NaOH}$ to produce $\ce{NaNO2, N2O, H2O}$. So, obviously it's acidic.
But there is one unpaired electron in the $\ce{N}$ atom. So, I see no reason for $\ce{NO}$ to be diamagnetic in gaseous state.
But, these questions do not have two correct answers. So, one of them has to be wrong. I am not sure which one.
$$\ce{2NO + O2 → 2NO2}$$
Nitric oxide reacts with oxygen to produce nitrogen dioxide. This reaction takes place quickly at room temperature in air. (chemiday)
The bond order in $\ce{NO}$ is 2.5
The oxidation state of $\ce N$ is +2, and this is a colourless, paramagnetic gas (ie. it is a radical, or contains an unpaired electron). (source)
Neutral oxides are those oxides which show neither basic nor acidic properties when they react with water. Examples include carbon monoxide $(\ce{CO})$ and nitrous oxide $(\ce{N2O})$ which are only slightly soluble in water, and nitric oxide $\mathbf{(NO)}$ which is appreciably soluble in cold water. (source)


So, option 3 is the correct answer as it is an inaccurate statement.