From top to bottom down the periodic table, atomic radii tends to increase. This is best explained by: a) electrons occupying orbitals located further from the nucleus. b) the increase in size of the nucleus. c) an increase in the number of electrons. d) Hund's Rule.

In the Bohr model for the hydrogen atom, which of the following transitions results in the emission of the highest energy photon?       A. n=3  →  n=4    B. n=4  →  n=3   C. n=4  →  n=2   D. n=1  →  n=3     E. n=1  →  n=4

n=4 V In the Bohr model of the hydrogen atom, the electron occupies distinct energy states. n=3 One transition between energy states of the hydrogen atom is represented by the picture on the left. n-2 Niels Bohr n=1 1. In this transition an electron moves from the n = level to the n = level. A. Absorbed 2. Energy is in this process. B. Emitted A. Closer to 3. The electron moves the nucleus. B. Further from

Where do you find elements that have energy levels that are all full of electrons? *       A:on the right side of the periodic table       B:across the bottom of the periodic table       C:on the left side of the periodic table     D:across the top of the periodic table

Please help with question 7

Write the complete electron configuration for the follwing. a. sulfur b. potassium c. nickel d. xeon

Which statement regarding the Bohr model of the atom is true?a. An element produces a continuous spectrum.b. Electrons lose quantized amounts of energy when moving to the ground state.c. Electrons can be anywhere, even between energy levels.d. Light is emitted when an electron moves from the ground state to an excited state.e. Electrons in the lowest energy level are in an excited state.

Which of the following is the correct electron configuration of Mg2+? A.  1s22s22p6 B.  1s22s22p63s1 C.  1s22s22p63s2 D.  1s22s22p63s23p1

B. Based on the items in A, draw an orbital diagram for each element. 1. S (sulfur) 2. Sc (scandium)