Electronic Configuration

Question 1

What are the rules for electron shells?

Answer 1

1) Electrons always occupy shells (energy levels). 2) Lowest energy levels are filled first. 3) Maximum electrons per shell: * 1st shell: 2 electrons * 2nd shell: 8 electrons * 3rd shell: 8 electrons

Question 2

How many electrons can the 1st, 2nd, and 3rd shells hold?

Answer 2

• 1st shell: 2 electrons * 2nd shell: 8 electrons * 3rd shell: 8 electrons

Question 3

What is the electronic configuration of nitrogen?

Answer 3

2.5

Question 4

How do you determine the electronic configuration of an element?

Answer 4

1) Find the atomic number (number of protons/electrons). 2) Apply the Electron Shell Rules.

Question 5

What is the electronic configuration of argon?

Answer 5

2.8.8

Question 6

How do the period and group of an element relate to its electronic configuration?

Answer 6

The number of shells is the same as the period. The group number indicates the number of electrons in the outer shell.

Question 7

What is the electronic configuration of sodium?

Answer 7

2.8.1

Question 8

Fill in the blank: The electronic configuration of aluminium (atomic number = 13) is _______.

Answer 8

2.8.3

Question 9

What defines a simple ion?

Answer 9

1) Atoms that gain or lose electrons. 2) Negative ions (anions) gain electrons. 3) Positive ions (cations) lose electrons.

Question 10

What happens to elements in Group 1 of the periodic table?

Answer 10

They lose one electron.

Question 11

What do elements in Group 6 of the periodic table do?

Answer 11

They pair up electrons.

Question 12

True or False: The electronic configuration can be derived from the periodic table.

Answer 12

True

Question 13

What do you need to calculate ionic compounds?

Answer 13

You need to balance the charges.

Question 14

Where in the periodic table would an element be with the configuration 2.8.8.2?

Answer 14

It would be in period 4 and group 2.