The overall order of a reaction is the sum of the exponents of the concentration terms in the rate law expression. For a general rate law, $\text{Rate} = k[A]^x[B]^y$, the overall order is $n = x + y$. Checking the given options:

1. $\text{Rate} = k[A]^0[B]^2$: Order $= 0 + 2 = 2$
2. $\text{Rate} = k[A]^1[B]^1$: Order $= 1 + 1 = 2$
3. $\text{Rate} = k[A]^{1/2}[B]^2$: Order $= \frac{1}{2} + 2 = 2.5$
4. $\text{Rate} = k[A]^{-1/2}[B]^{3/2}$: Order $= -\frac{1}{2} + \frac{3}{2} = \frac{2}{2} = 1$ Therefore, the rate law $\text{Rate} = k[A]^{-1/2}[B]^{3/2}$ corresponds to an overall first-order reaction.