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- The most stable configuration is when the entire shell is full (noble gas configuration). Next best is when a specific orbital (s, p, d, f, etc.) is completely full, even if the shell is not complete. Next best after that is when a specific orbital is exactly half full.
- All atoms would like to attain electron configurations like noble gases, i.e., have completed outer shells. Atoms can form stable electron configurations like noble gases by losing electrons, gaining electrons and sharing electrons. For a stable configuration each atom must fill its outer energy level. In the case of noble gases there will be eight electrons in the valence (outer most) shell (with the exception of He which has two electrons). Atoms that have 1, 2 or 3 electrons in their outer levels will tend to lose them in interactions with atoms that have 5, 6 or 7 electrons in their outer levels. Atoms that have 5, 6 or 7 electrons in their outer levels will tend to gain electrons from atoms with 1, 2 or 3 electrons in their outer levels. Atoms that have 4 electrons in the outer most energy level will tend neither to totally lose nor totally gain electrons during interactions and thus they tend to share electrons.
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∙ 9y ago
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∙ 9y agoIn chemistry, the noble gases (neon, argon, krypton xenon radon) with an outer electron shell containing 8 electrons, 2 in s orbitals and 6 in p orbitals are considered to be the most stable, as the noble gases are relatively un-reactive.
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∙ 13y agoA full valence shell (8-electron rule) is the most stable configuration of an atom.
Therefore the noble gases like Helium and Neon are inert and very stable since they have 8 electrons in their valence shell (i.e. their outer shell)
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∙ 9y agoElectron configurations where n equals the energy level, ns2 np6 have the greatest stability.
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∙ 15y agoamongst other factor is when its valence shell is filled.
for highschool students this means 8 valence electrons
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∙ 11y agoThe noble gas configuration is known as the most stable configuration that an atom can achieve. In other words, the valence shell with ns2 np6 electron configuration.
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∙ 14y agoNOBEL GASES without a doubt
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∙ 13y agoElements in group 13
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∙ 9y agoThe noble gasses.
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What is the ground state electron configuration for silicon and what is the actual ground state electron configuration for copper?
The expected ground-state electron configuration of copper is ; however, the actual configuration is because a full dsubshell is particularly stable. There are 18 other anomalous elements for which the actual electron configuration is not what would be expected.
How do ionic compound obtain a stable electron configuration?
They achieve stable configuration by sharing their electrons in their outermost shell.
What does oxygen need to do in order to to achieve a stable electron configuration?
Oxygen atoms need to share or gain two electrons in order to achieve a stable electron configuration.
What has a pseudo-noble-gas electron configuration?
The pseudo noble-gas electron configuration has the outer three orbitals filled, the s, p and d- s2p6d10 (18 electrons total) and so is fairly stable. Elements that attain this electron configuration are at the right side of the transition metals (d-block). Br-, I-, Se2-
What is the correct electron configuration for Cu?
The electron configuration of copper is: [Ar]4s13d10. It isn't 4s23d9 because Cu is able to obtain a more stable electron configuration when it takes an electron from the 4s and adds it to 3d. A half filled 4s and a completely filled 3d is more stable.
What group of elements have stable electron confoguration?
The group of elements that have a stable electron configuration are the noble gases.
What is important about the electron configuration of the noble gases?
By acquiring noble gas configuration elements become stable .
How many valance electrons do most elements need to have a stable electron configuration?
8 valance electron
What is the ground state electron configuration for silicon and what is the actual ground state electron configuration for copper?
The expected ground-state electron configuration of copper is ; however, the actual configuration is because a full dsubshell is particularly stable. There are 18 other anomalous elements for which the actual electron configuration is not what would be expected.
What is the most reactive group of elements?
It is in Group 17 that you will find the most reactive elements. These elements all lack only one electron from having that "magic" electron configuration of the inert gases. That makes these elements very "hungry" to get that "last electron" so their electron structures become more stable.
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.
What is the formula of the ion formed when sodium achieves a stable electron configuration?
Na+ is the formula of the ion formed when sodium achieves a stable electron configuration.
What symbol would represent a chlorine ion that has ionized to have a stable electron configuration?
What symbol would represent a chlorine ion that has ionized to have a stable electron configuration?
How do ionic compound obtain a stable electron configuration?
They achieve stable configuration by sharing their electrons in their outermost shell.
What does oxygen need to do in order to to achieve a stable electron configuration?
Oxygen atoms need to share or gain two electrons in order to achieve a stable electron configuration.
What is a stable electron configueration?
A stable electron configuration refers to an atom in which the outer electron shell is full. Outermost electron shells hold a maximum of 2, 8, 8, 18,...(etc.) electrons. With an outer shell of 2 electrons, the periodic table shows that helium has a stable electron configuration. The next stable configuration of an element has 10 (2 + 8) electrons. This is neon. Neon is followed by argon, with 18 (2 + 8 + 8) electrons. Krypton, with 36 (2 + 8 + 8 + 18) electrons is next. The remaining stable configurations follow a similar pattern, based on the maximum number of electrons able to fit into the outermost ring. These elements are extremely stable and rarely react with other elements. They are referred to as the noble gases or inert elements. Atoms of other elements may bond with each other or different elements to form molecules having full outermost shells of electrons.
Do ions have the same electron configuration as noble gases?
The stable ions of all the elements except the Transition metals, Actinide, and Lanthanide series (that is the d and f block elements) form stable ions that are isoelectronic to a nobel gas by gaining or losing electrons in order to achieve an s2 p6 stable octet. For example, sodium will lose one electron to have the same electron configuration as neon, while nitrogen will gain three electrons to become isoelectronic to neon.
