Color of [Cr(NH3)6]Cl2 complex
The [Cr(NH3)6]Cl2 complex is indeed colored. The color of a coordination complex is determined by the absorption of light in the visible region of the electromagnetic spectrum. The color arises from the splitting of the d orbitals in the central metal atom/ion in the complex.

Explanation
- In the case of the [Cr(NH3)6]Cl2 complex, the central chromium (Cr) ion is in the +3 oxidation state.
- The six ammonia (NH3) ligands around the chromium ion cause the d orbitals to split into two sets - t2g and eg.
- Electrons in the t2g orbitals absorb light in the visible region, leading to the complex exhibiting a color.
- The specific color of the complex is due to the energy difference between the split d orbitals, which determines the wavelength of light absorbed.

Color of [Cr(NH3)6]Cl2 complex
The [Cr(NH3)6]Cl2 complex appears violet in color. This color is a result of the absorption of light in the visible spectrum by the complex. The specific shade of violet is determined by the electronic structure of the complex, including the ligands present and the oxidation state of the central metal ion.
In conclusion, the [Cr(NH3)6]Cl2 complex is colored due to the splitting of d orbitals and subsequent absorption of light in the visible region. The violet color of the complex is a result of the specific energy differences between the split d orbitals in the chromium ion.