NaCl electrolysis with copper electrodes

Considering the aqueous $\ce{NaCl}$ is already concentrated. If we were to use copper electrodes instead of inert graphite electrodes:

Would copper react with the evolved chlorine gas to give $\ce{CuCl2}$ in solution, whilst still giving hydrogen gas at the cathode? Since in my experimentation, I obtained a teal blue green colored salt that was soluble in water. I do not have appropriate lab equipment to test for the identity of the salt, so I am hoping someone here could shed some light on the reactions taking place and the identity of the obtained substance. Thanks.