Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm. 3.54 x 10-19 J 4.27 x 10-19 j 2.34 x 10-19 j O 6.45 x 10-19 J 2.83 x 10-19 j

7 please

Use the equations below to calculate the energy of each color of light shown in the hydrogen's emission spectrum shown in #5. Hint: Violet: 410.0 nm = 4.100 x 107 m Blue-violet: 434.0 nm = 4.340 x 107 m Blue-green: 486.1 nm = 4.861 x 107m Red: 656.2 nm = 6.562 × 107 m c= λχυ c = 3.00 x 10°m/s 1 = wavelength (m) v = Frequency (Hz) E = h xu E = energy (J) h = 6.626 x 10 34 J.s v = Frequency (Hz)

Which of the following forms of electromagnetic radiation have the longest wavelength? O Radio waves O Gamma O X-ray O Ultraviolet O Infrared

Give typed full explanation not a single word hand written otherwise leave it

Calculate the wavelength (in nm) detected when an electron drops from ni = 5 to nf =2 Where on the electromagnetic spectrum will you find the wavelength? What is the energy associated with the wavelength?

3. The following energy levels were recorded for a sodium atom: Orbital Energy -8.235 x 10-19 J -4.870 x 10-19J 3s 3p Calculate the energy of a photon needed to cause an electron in the 3s orbital to be excited to the 3p orbital.

The photoelectric effect can be used in engineering designs for practical applications. For example, infrared goggles used in night-vision applications have materials that give an electrical signal with exposure to the relatively long wavelength of IR light. If the energy needed for signal generation is 7.6 x 10-40 J, what is the minimum wavelength? What is the frequency of light that can be detected? c = 2.998 × 10° m/s h = 6.626 x 10-34 J s m S -1