Energy Levels and Electron Configuration



Energy Levels and Electron Configuration Notes Name _____________________________ Per _____

Mrs. Zeiders

Purpose: It is important to learn how to configure the electrons in the electron orbitals in order to determine how many electrons are in the final orbital. These electrons in the outer most part of the atom will determine how it behaved and bonds with other atoms.

Basic Rules:

• Electrons are filled from the ____________________ of the atom, near the nucleus, outwards.

• ___________________________ are filled first then higher energy levels.

o Lower energy levels are near the nucleus; higher energy levels are farther out.

o Check out the energy level diagram*, it will tell you what order to fill the orbitals in.

• There are several sub shells of electrons (also known as _____________ ):

o ________ orbitals

o ________ orbitals

o ________ orbitals

o ________ orbitals

• Each sub level has a maximum number of electrons it can hold:

o s orbitals can hold up to _______ electrons

o p orbitals can hold up to _______ electrons

o d orbitals can hold up to _______ electrons

o f orbitals can hold up to ________ electrons

Written Electron Configuration Notation:

Fill the orbitals with electrons from lower energy levels to higher energy levels. According to the diagram above the order to fill orbitals in:

1s☐2s☐2p☐3s☐3p☐4s☐3d☐4p☐5s☐4d☐5p☐ etc… (☐ will contain a number)

[pic]

The first number is the ___________________________.

The lowercase letter is the ____________________. The sub-shells are named ___________________. The number of available sub-shells increases as the energy level increases. For example, the first energy level only contains an s sub-shell and will only contain up to 2 electrons, while the second energy level contains both an s sub-shell and a p sub-shell and can hold up to 8 electrons.

The number in superscript is the _____________________________. Each sub-shell can hold only a certain number of electrons. The s sub-shell can hold no more than _________ electrons, the p sub-shell can hold __________, the d sub-shell can hold _________ and the f sub-shell can hold as many as _______. If you add up all the superscript numbers it should add up to the ___________________________________ for that atom.

Example: Sulfur has 16 electrons: 1s22s22p63s23p4 = 2+2+6+2+4 = 16 electrons

Sulfur has 2 electrons in the first energy level (1s2)

8 electrons in the second energy level (2s2 2p6)

6 electrons in the third energy level (3s2 3p4)

|Nitrogen Bohr Model |Nitrogen REFINED Bohr Model |

|[pic] |[pic] |

|7 protons, 7 neutrons, 7 electrons |7 protons, 7 neutrons, 7 electrons |

|Electron configuration: 1s2 2s2 2p3 |Electron configuration: 1s2 2s2 2p3 |

|Two electrons in the first energy level 1s2), and five in the second energy level|Two electrons in the first s sublevel (1s2), two electrons in the s orbital of |

|(2s2 2p3) |the second energy level (2s2), and 3 electrons in the p orbital of the second |

| |energy level (2p3). |

|(THIS SIMPLIFIED VERSION IS WHAT WE WILL USE) | |

Valence Electrons

Now that we have figured out where the electrons are in the atom, now we can figure out how many electrons are in the outer orbital. This is important because the number of electrons in the outer orbital determines how and what the element bonds with.

Valence Electrons:

To figure out how many valence electrons an atom has we must follow the steps below:

• Write out the electron configuration

• Identify the outermost energy level

o This is the highest number in front of the orbital name

• Add up how many electrons are in that energy level (Add together the superscripts)

Example:

Sulfur (S): # of electrons __________

Electron Configuration: ___________________________________

The outermost energy level: ____________

Electrons found in energy level: ______________

Valence Electrons: ____________

Florine (F): # of electrons __________

Electron Configuration: ___________________________________

The outermost energy level: ____________

Electrons found in energy level: ______________

Valence Electrons: ____________

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