Examples of electron shell in the following topics:
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- These orbits form electron shells or energy levels, which are a way of visualizing the number of electrons in the various shells.
- Electrons fill orbit shells in a consistent order.
- The innermost shell has a maximum of two electrons, but the next two electron shells can each have a maximum of eight electrons.
- As shown, helium has a complete outer electron shell, with two electrons filling its first and only shell.
- In this model, electrons exist within principal shells.
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- The second electron shell may contain eight electrons.
- Lithium (Li) contains three electrons that occupy the first and second shells.
- Larger elements have additional orbitals, making up the third electron shell.
- Principal shell 3n has s, p, and d subshells and can hold 18 electrons.
- Principal shell 4n has s, p, d, and f orbitals and can hold 32 electrons.
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- The electrons in the partially filled outermost shell (or shells) determine the chemical properties of the atom; it is called the valence shell.
- The electron shell configurations of the first 18 elements in the periodic table.
- The number of outer-shell electrons is represented by the right-most digit in the group numbers.
- Each box includes representations of the electron shell structure for the element.
- Position in the periodic table based on electron shell configuration.
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- This results in a full outermost electron shell and makes them energetically more stable.
- As illustrated, sodium (Na) only has one electron in its outer electron shell.
- It takes less energy for sodium to donate that one electron than it does to accept seven more electrons to fill the outer shell .
- In this example, sodium will donate its one electron to empty its shell, and chlorine will accept that electron to fill its shell.
- In this example, sodium loses one electron to empty its shell and chlorine accepts that electron to fill its shell.
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- However, when more electrons are involved, each electron (in the $n$-shell) feels not only the electromagnetic attraction from the positive nucleus, but also repulsion forces from other electrons in shells from '1' to '$n$'.
- This causes the net force on electrons in the outer electron shells to be significantly smaller in magnitude.
- Therefore, these electrons are not as strongly bonded to the nucleus as electrons closer to the nucleus.
- The shielding theory also explains why valence shell electrons are more easily removed from the atom.
- Each has 10 electrons, and the number of nonvalence electrons is two (10 total electrons minus eight valence electrons), but the effective nuclear charge varies because each has a different number of protons:
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- The more electron shells there are, the greater the shielding effect experienced by the outermost electrons.
- However, when more electrons are involved, each electron (in the n-shell) feels not only the electromagnetic attraction from the positive nucleus but also repulsion forces from other electrons in shells from 1 to n-1.
- The shielding effect explains why valence shell electrons are more easily removed from the atom.
- The valence shell is shell 2 and contains 8 valence electrons.
- Once again, the electron configuration is the same as in the previous examples and the number of nonvalence electrons is 2 (by losing one electron, the valence shell becomes the n=2 shell).
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- Here, electrons are arranged in energy levels, or shells, around the nucleus of an atom.
- An atom's electron shell can accommodate 2n2 electrons, where n is the energy level.
- For example, the first shell can accommodate 2 x (1)2 or 2 electrons.
- The second shell can accommodate 2 x (2)2, or 8, electrons.
- An element's electron configuration is the arrangement of the electrons in the shells.
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- Electron shell #1 has the lowest energy and its s-orbital is the first to be filled.
- In the third period of the table, the atoms all have a neon-like core of 10 electrons, and shell #3 is occupied progressively with eight electrons, starting with the 3s-orbital.
- The highest occupied electron shell is called the valence shell, and the electrons occupying this shell are called valence electrons.
- The other members of group 8 have a characteristic valence shell electron octet (ns2 + npx2 + npy2 + npz2).
- These atoms have only one electron in the valence shell, and on losing this electron arrive at the lower shell valence octet.
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- Monatomic ions are formed by the addition or removal of electrons from an atom's valence shell.
- For example, Group 1 element sodium (Na) has a single electron in its valence shell, with full shells of 2 and 8 electrons beneath.
- Removal of this one electron leaves sodium stable: Its outermost shell now contains eight electrons, giving sodium the electron configuration of neon.
- Sodium could gain electrons, but it would require seven more to achieve a full valence shell.
- On the other hand, a chlorine atom (Cl) has seven electrons in its valence shell, which is one short of a stable, full shell with 8 electrons.
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- The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.
- The electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals.
- Electron configurations describe electrons as each moving independently in an orbital, in an average field created by all other orbitals.
- However, the electronic wave function is usually dominated by a very small number of configurations and therefore the notion of electronic configuration remains essential for multi-electron systems.
- The outermost electron shell is often referred to as the valence shell and (to a first approximation) determines the chemical properties.