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There are many types of rules for electron configuration. Look at the Aufbau principle and Hund's rules.
- In each orbital there is a maximum of two electrons.
- In a "s" orbital, there are two electrons.
- In a "p" orbital, there are three sub-orbitals, each containing two electrons. (Thus containing 6 electrons)
- In a "d" orbital, there are five sub-orbitals, each containing two electrons. (Thus containing 10 electrons)
- In a "f" orbital, there are seven sub-orbitals, each containing two electrons. (Thus containing 14 electrons)
Look at the Aufbau diagram linked below.
The coefficient represents the orbital. Do not use mathematics to try to solve the configurations.
1s2 2s2 2p6 : Neon's Electron Configuration
The letter following the coefficient describes which type of orbital it is, being s, p, d, or f.
The superscript denotes the number of electrons it contains. If you add 2, 2, and 6, you would get 10, Neon's atomic number.
Electron configurations become stable when they are neutrally charged.
i.e Li: 1s2 2s1
This is a stable electron configuration. However, if you lose that one electron,
Li: 1s2
It become a positively charged ion, called a cation.
What else can I help you with?
What have stable electron configurations?
any time there are as many electrons and protons and they fill each orbital optimally.
What are stable electron configurations most likely to contain?
Stable electron configurations are most likely to contain filled energy levels or filled subshells. These configurations generally follow the octet rule or duet rule, depending on the element. Additionally, stable electron configurations may contain configurations with a full valence shell of electrons.
How many energy levels do the most stable electron configurations have?
6
What is a pseudo-noble gas?
Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.
How do elements achieve stable electron configurations between two atoms?
protons
What are stable electron configurations are likely to contain?
completely filled valence shells
When comparing the electron configurations of neon and fluorine what must happen for fluorine to become stable?
For fluorine to become stable, it needs to gain one electron to attain a full valence shell, similar to the electron configuration of neon. Fluorine has seven valence electrons in its outer shell, so gaining one electron would fill its outer shell and make it stable with a full octet like neon.
Do Helium Xenon and Neon have stable electron configurations?
Yes, helium, xenon, and neon all have stable electron configurations. Helium has a full outer electron shell with 2 electrons, xenon has a full outer shell with 8 electrons, and neon has a full outer shell with 8 electrons as well.
The elements Li and F combine to form an ionic compound The electron configurations in this compound are the same as the electron configurations of atoms in which group?
The electron configurations of LiF will be the same as the electron configurations of atoms in Group 18 (noble gases) because Li will lose its single electron to attain a stable octet similar to the noble gases, while F will gain an electron to achieve a complete valence shell.
A sodium atom has an electron configuration of 1s22s22p63s1 If the sodium atom becomes ionized its new electron configuration will be the same as which element?
If a sodium atom loses an electron to become a Na+ ion, its electron configuration will be the same as neon (1s22s22p6). Both sodium and neon have stable electron configurations.
What is inert gas configuration?
Inert gas configurations refer to the electron configurations of noble gases, which have a full outer electron shell. These configurations are very stable and unreactive due to their complete outer energy level. Other elements may strive to attain such configurations through chemical bonding to achieve greater stability.
What does chlorine need to become stable?
A chlorine atom needs one additional electron in order to become stable.
