(a) Atomic emission spectra arise from electron transitions from higher-energy orbitals to lower-energy orbitals. The blue line at 434.7 nm (Fig. 1) in the emission spectrum for mercury arises from an electron moving from a 7d to a 6p orbital. Mercury (Hg) 400 550 600 650 700 nm Wavelength, A (nm) (Fig. 1) Line emission spectrum for mercury (i) Give the principal (n) and angular momentum (1) quantum numbers and give the range of possible magnetic (m) quantum numbers for the higher energy 7d orbital. (ii) Give the principal (n) and angular momentum (1) quantum numbers and give the range of possible magnetic (mi) quantum numbers for the lower energy 6p orbital. (iii) Calculate the energy difference between the 7d and 6p orbitals in the units of kJ/mol. (b) (i) State and briefly discuss the Heisenberg uncertainty principle. (ii) Use the Heisenberg uncertainty principle to calculate the uncertainty in meters in the position of a sprinter weighing 53.7 kg and running at a velocity of 8.83 ms. Assume that the uncertainty in the velocity is 10% of the registered velocity.