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Work Session 8: Electron configuration and Chemical Periodicity 1. What are the values of n and l for electrons in the following orbitals? 5s 4d 3p 6p 6f 7f 2. There are three 2p orbitals. Sketch

How to fill out 8 electron configuration

How to fill out 8 electron configuration:

1. Start by determining the atomic number of the element you are working with. This can be found on the periodic table.
2. Next, write down the electron configuration of the previous noble gas. For example, if you are filling out the electron configuration for oxygen (atomic number 8), you would start with the electron configuration of the noble gas neon (atomic number 10): [Ne].
3. Then, continue filling in the electron shells, starting with the first energy level (1s) and moving up. Each energy level has a specific number of subshells and orbitals, which can be determined by the periodic table.
4. In the case of oxygen (atomic number 8), the electron configuration would proceed as follows: 1s^2 2s^2 2p^4. This indicates that the first energy level (1s) contains 2 electrons, the second energy level (2s) contains 2 electrons, and the second energy level (2p) contains 4 electrons.
5. Finally, ensure that the total number of electrons matches the atomic number of the element.

Who needs 8 electron configuration:

1. Elements in the group 18 of the periodic table, also known as the noble gases, already have a full electron configuration with 8 electrons in their outermost energy level. This stability makes them highly unreactive and, therefore, they do not typically form chemical bonds with other elements.
2. Other elements that are not part of the noble gases may also strive to achieve an electron configuration with 8 electrons in their outermost energy level. This is known as the octet rule and is a characteristic of many stable, non-noble gas elements.
3. Compounds formed between elements with 8 electron configurations and those that do not have 8 electrons in their outermost energy level often involve the transfer or sharing of electrons to meet the octet rule. These interactions are the foundation of chemical bonding and are essential in the formation of compounds with specific properties.

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