Study Guide For The Electron (Page 3 of 4) in pdf

Study Guide For The Electron Page 3

Complete the chart below.

Energy Level

Sublevel(s)

Orbital(s)

Maximum Number of Electrons

(1 “s”)

(2 “s”)

s & p

(1 “s” and 3 “p”)

(2 “s” and 6 “p”)

s, p, & d

(1 “s”, 3 “p”, & 5 ”d”)

(2 “s”, 6 “p”, & 10 ”d”)

s, p, d, & f

(1 “s”, 3 “p”, 5 “d”, & 7 “f”)

(2 “s”, 6 “p”, 10 “d”, & 14 “f”)

Answer the following questions.

24. How many orbitals are found in 2f?

25. How many electrons can be held in n = 2?

8 electrons

26. How many orbitals are found in a d-sublevel with n = 6?

5 orbitals

27. What two elements have exactly 5 electrons in their 3d sublevel?

Cr and Mn

28. State/Explain Aufbau Principle.

Electrons will occupy the lowest energy orbital first.

29. State/Explain Pauli’s Exclusion Principle.

Each orbital can hold a maximum of two electrons with opposite spins.

30. State/Explain Hund’s rule.

When filling equal energy orbitals, maximize unpaired electrons.

31. How many p-orbitals are found in the first energy level?

32. How many sublevels are in the fourth principal energy level?

4 (s, p, d, and f)

33. What element has an electron configuration that ends in 5p

Sn, tin

34. What element has an electron configuration: [Xe]6s

W, tungsten

35. What element has the electron configuration, 1s

Si, silicon

Study Guide For The Electron Page 3