The following are possible energy values for the electron orbiting the nucleus in Bohr’s model for the hydrogen atom.    n = 1:    E1 = -21.79 x 10–19 J;        n = 2:    E2 = - 5.45 x 10–19 J;    n = 3:    E3 = - 2.42 x 10–19 J;    n = 4:    E4 = - 1.36 x 10–19 J; If an electron jumps from the orbit n = 4 to orbit n = 2, and a quantum of energy is emitted in the form of light, what is the wavelength of the emitted light in nm?             (A) 365 nm           (B) 486 nm           (C) 1095 nm           (D) 1460 nm

$ 4 F In the Bohr model of the hydrogen atom, the electron occupies distinct energy states. One transition between energy states of the hydrogen atom is represented by the picture. R n=∞ V n=4 n=3 n-2 n=1 In this transition an electron moves from the n = level to the n = Energy is in this process. The electron moves I Submit Answer % 5 T G [Review Topics] [References] Use the References to access important values if needed for this question. B Retry Entire Group 9 more group attempts remaining 6 Cengage Learning Cengage Technical Support the nucleus. Y H MacBook Pro N & 7 U J * 8 M | K 9 L I level. O O L P > { Previous [ ? + 11 11 Next Save and Exit } ] delete

6. An electron starts from rest 24.5 cm from a fixed point charge with Q = - 6.50 nC (-6.50 x 10 °C). How fast will the electron be moving when it is very far away. Mass of electron m =9.11 x 10-31 kg and charge of the electron is e = -1.6022 x 10-19 C.

What aspect of the Bohr model is correct? (i.e. agrees with the quantum mechanical model) O electrons have set energy levels that depend on distance from the nucleus O energy levels are equally spaced in an atom O the position and energy of an electron can be precisely determined simultaneously O electrons move in circular orbits around the nucleus 99+ hp