Electron Configuration

Principles

100

1. The statement that electron spread out as much as possible when filling orbitals is?

x4 points

Hund’s Rule

200

Why are the arrows pointing in different directions? 

To show that the electrons are spinning in opposite directions.

300

The statement that an electron will fill the lowest energy orbital first is?

x2 points

                                

the Aufbau Principle

400

Label all 4 blocks correctly

A. s block

B. d block

C. p block

D. f block

500

What is wrong with the electron configuration of Lutetium. [Xe] 6s²5d¹

Missing 4f¹⁴ orbital

Orbital Diagrams

100

How many electrons are allowed in an a single orbital? How many orbitals are in each of the sublevels?

2 electrons 

s-1

p-3

d-5

f-7

200

x3 points

B

300

Draw the orbital diagram for Terbium, #65.

400

Draw the orbital diagram for Technetium #43

500

Draw the electron configuration of the Boron ion. B³⁺

1s²

Electron Configurations

100

1. The element with the electron configuration notation 1s²2s²2p⁶3s²3p¹ is?

Al

200

Write the standard long-form electron configuration for Iodine?

 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁵

300

Write the noble gas electron configuration for Nickel. 

x2 points

[Ar]4s²3d⁸

400

How many valence electrons are found in this atom: 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴ ?

6

500

What element is represented by [Kr]4s¹? Give the atomic number of the element as your answer.

4s cant come after Kr, not possible.

Periodic Table

100

The correct sequence in increasing energies of orbitals is?

1. 4d, 5s, 5p, 6s               c.  5s, 4d, 5p, 6s
2. 5s, 4d, 6s, 5f                d.  5s, 5p, 4d, 6s

C

200

1. The correct sequence in decreasing energies of orbitals is
   1. 4d, 5s, 5p, 6s            c.  5s, 4d, 5p, 6s
   2. 5s, 4d, 6s, 5f             d.  5s, 4p, 3d, 4s

x2 points

D

300

1. Which element below is found in the “P” block of the periodic table?
   1. Mg                            c.  U     
   2. Ti                              d.  P

P

400

How many energy levels are found in this atom: 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁴?

4

500

Write the correct electron configuration for the Gold ion, Au⁺. Long-hand notation.

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶6s¹4f¹⁴5d⁹

Random

100

How many different p-orbitals exist?

x2 points

3

200

Which orbital is lower in engery 4s or 3d?

4s 

300

Recall that an ion is an atom that has gained or lost electrons to increase stability. The electron configuration for a typical Oxygen atom is 1s²2s²2p⁴, while the electron configuration for a typical Oxygen ion would be 1s²2s²2p⁶ . How does this increase stability? 

a. It fills the energy level. 

b. It fills the sublevel.

c. Both A and B. 

d. It creates a new energy level.

C

400

According to what we’ve learned in class, the noble gas configuration for a typical Copper atom would be  [Ar]4s² 3d⁹. However, the correct noble gas configuration for a typical Copper atom is [Ar]4s¹ 3d¹⁰. Why?

Generally speaking, electrons fill the lowest energy orbitals first before moving into a higher energy orbital.  They do this in order to preserve the stability of the atom.  However, there are times when it is actually more stable for an electron to move into a higher energy orbital.  For example, a half-full or completely full sublevel is actually a more stable form of the atom.  When possible, electrons will move from the lower energy s-orbital into the higher energy d-orbital in order to be more stable.  In the case of Copper, a single electron moves from the 4s orbital into the nearly full 3d sublevel to increase the stability of the atom.  

500

Write the noble gas configuration for a stable atom of Tungsten (W).

[Xe] 6s²4f¹⁴5d⁴