Based on the equation: $$\Delta E = -2.0 \times 10^{-18}$$ J $$\left(\frac{1}{n_2^2} - \frac{1}{n_1^2}\right)$$, the wavelength of the light that must be absorbed to excite hydrogen electron from level n = 1 to level n = 2 will be: (h = $$6.625 \times 10^{-34}$$ Js, C = $$3 \times 10^8$$ ms$$^{-1}$$)

The given equation is $$\Delta E = -2.0 \times 10^{-18} \, \text{J} \left( \frac{1}{n_2^2} - \frac{1}{n_1^2} \right)$$. This represents the change in energy when an electron transitions from an initial energy level $$n_1$$ to a final level $$n_2$$. For absorption, energy is absorbed to move the electron from a lower level to a higher level. Here, the electron is excited from $$n_1 = 1$$ to $$n_2 = 2$$.

Substitute $$n_1 = 1$$ and $$n_2 = 2$$ into the equation:

$$\Delta E = -2.0 \times 10^{-18} \left( \frac{1}{2^2} - \frac{1}{1^2} \right) = -2.0 \times 10^{-18} \left( \frac{1}{4} - 1 \right)$$

Compute the expression inside the parentheses:

$$\frac{1}{4} - 1 = \frac{1}{4} - \frac{4}{4} = -\frac{3}{4}$$

Now substitute back:

$$\Delta E = -2.0 \times 10^{-18} \times \left( -\frac{3}{4} \right) = 2.0 \times 10^{-18} \times \frac{3}{4}$$

Calculate the multiplication:

$$2.0 \times 10^{-18} \times \frac{3}{4} = \frac{2.0 \times 3}{4} \times 10^{-18} = \frac{6.0}{4} \times 10^{-18} = 1.5 \times 10^{-18} \, \text{J}$$

The energy absorbed, $$\Delta E = 1.5 \times 10^{-18} \, \text{J}$$, corresponds to the energy of the photon absorbed. The energy of a photon is given by $$E = \frac{hc}{\lambda}$$, where $$h$$ is Planck's constant, $$c$$ is the speed of light, and $$\lambda$$ is the wavelength. Therefore,

$$\Delta E = \frac{hc}{\lambda}$$

Solving for $$\lambda$$:

$$\lambda = \frac{hc}{\Delta E}$$

Given $$h = 6.625 \times 10^{-34} \, \text{Js}$$ and $$c = 3 \times 10^8 \, \text{ms}^{-1}$$, substitute the values:

$$\lambda = \frac{(6.625 \times 10^{-34}) \times (3 \times 10^8)}{1.5 \times 10^{-18}}$$

First, multiply the numerator:

$$6.625 \times 10^{-34} \times 3 \times 10^8 = 6.625 \times 3 \times 10^{-34 + 8} = 19.875 \times 10^{-26}$$

Now divide by the denominator:

$$\lambda = \frac{19.875 \times 10^{-26}}{1.5 \times 10^{-18}} = \frac{19.875}{1.5} \times 10^{-26 - (-18)} = \frac{19.875}{1.5} \times 10^{-8}$$

Compute $$\frac{19.875}{1.5}$$:

$$19.875 \div 1.5 = 13.25$$

So,

$$\lambda = 13.25 \times 10^{-8} \, \text{m} = 1.325 \times 10^{-7} \, \text{m}$$

Comparing with the options, $$1.325 \times 10^{-7} \, \text{m}$$ corresponds to option A.

Hence, the correct answer is Option A.