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Why is transfer of electron from 2s subshell to 1s subshell not possible?
Wiki User
∙ 14y ago
For a 2s subshell to be present, the 1s subshell must first be full, which means no more electrons can be moved into the 1s subshell.
Wiki User
∙ 14y ago
Transfer of an electron from a higher energy orbit (2s) to a lower energy orbit (1s) is not possible because it would violate the energy conservation principle. Electrons naturally occupy the lowest available energy levels in an atom, following the Aufbau principle. This means electrons will only move to higher energy levels if they absorb energy, not by transferring between lower and higher energy levels.
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How can you tell the difference between 1s subshell and 3s subshell?
The principal quantum number (n) distinguishes between different subshells. For example, the 1s subshell has an n value of 1, while the 3s subshell has an n value of 3. The higher the n value, the higher the energy level of the subshell.
Why is the 2s subshell of heigher energy than the 1s subshell?
The 2s subshell has a higher energy level than the 1s subshell due to the presence of more nodes in the 2s orbital, which increases its energy. Additionally, the 2s orbital has a larger principal quantum number (n) than the 1s orbital, leading to greater distance from the nucleus and therefore higher energy.
Which sum gives the total number of electrons in electron configuration?
The total number of electrons in an electron configuration is given by the sum of the individual electron counts for each subshell (i.e. s, p, d, f). For example, in the electron configuration for oxygen (1s^2 2s^2 2p^4), the total number of electrons is 8, which is the sum of 2 (s subshell), 2 (s subshell), and 4 (p subshell) electrons.
How many electrons can the first electron cloud hold?
Your question is a bit vague, but if you are enquiring about the first electron shell in an atom, it holds a maximum of two electrons.
What atom is represented in the following orbital diagram 1s2s2p?
The atom represented in the orbital diagram 1s2s2p is carbon (C). This notation indicates the electron configuration of carbon, where the 1s subshell is filled with 2 electrons, followed by 2 electrons in the 2s subshell and 2 electrons in the 2p subshell.
How can you tell the difference between 1s subshell and 3s subshell?
The principal quantum number (n) distinguishes between different subshells. For example, the 1s subshell has an n value of 1, while the 3s subshell has an n value of 3. The higher the n value, the higher the energy level of the subshell.
What is the subshell of the K shell?
The K shell is the first shell in an atom and has only one subshell, which is the 1s subshell. This subshell can hold up to 2 electrons.
How many total electrons does an atom possess if it has the first two electron orbitals completed?
An atom with the first two electron orbitals completed would have 10 total electrons. The first electron orbital can hold up to 2 electrons (2 in the s subshell), and the second electron orbital can hold up to 8 electrons (2 in the s subshell and 6 in the p subshell).
Why is the 2s subshell of heigher energy than the 1s subshell?
The 2s subshell has a higher energy level than the 1s subshell due to the presence of more nodes in the 2s orbital, which increases its energy. Additionally, the 2s orbital has a larger principal quantum number (n) than the 1s orbital, leading to greater distance from the nucleus and therefore higher energy.
Which sum gives the total number of electrons in electron configuration?
The total number of electrons in an electron configuration is given by the sum of the individual electron counts for each subshell (i.e. s, p, d, f). For example, in the electron configuration for oxygen (1s^2 2s^2 2p^4), the total number of electrons is 8, which is the sum of 2 (s subshell), 2 (s subshell), and 4 (p subshell) electrons.
How many electrons can the first electron cloud hold?
Your question is a bit vague, but if you are enquiring about the first electron shell in an atom, it holds a maximum of two electrons.
Write the electron configuration diagram that shows the transfer of electrons that takes place to form the compound sodium fluoride and include the electron configuration of the ions formed?
For the formation of sodium fluoride, sodium (Na) will transfer one electron to fluorine (F) to achieve a stable electron configuration. The electron configuration for sodium is [Ne] 3s^1, and for fluorine, it is [He] 2s^2 2p^5. After transfer, sodium forms the Na+ cation with an electron configuration of [Ne], and fluorine forms the F- anion with an electron configuration of [He] 2s^2 2p^6.
What atom is represented in the following orbital diagram 1s2s2p?
The atom represented in the orbital diagram 1s2s2p is carbon (C). This notation indicates the electron configuration of carbon, where the 1s subshell is filled with 2 electrons, followed by 2 electrons in the 2s subshell and 2 electrons in the 2p subshell.
What is the electron configuration of h?
The electron configuration of hydrogen (H) is 1s¹, meaning it has one electron in the 1s orbital.
What electron configuration is correct for a sodium ion?
The correct electron configuration for a sodium ion (Na+) is 1s2 2s2 2p6. Sodium loses one electron to form a +1 ion, resulting in a filled 1s orbital and a filled 2s2 2p6 subshell.
Why electrons pairing start with only 2p orbital in P subshell?
Electrons pair in the 2p orbital first because each orbital can hold a maximum of 2 electrons, and pairing allows for greater stability due to electron-electron repulsion being minimized. Additionally, electron pairing in the 2p orbital follows Hund's rule, which states that electrons fill degenerate orbitals singly before pairing up.
Why are electrons in the 1s subshell much closer to the nucleus in Ar than in He?
Electrons in the 1s subshell are closer to the nucleus in Ar than in He due to the greater nuclear charge in argon (Ar) compared to helium (He). Ar has more protons in its nucleus, creating a stronger attraction for the electrons in the 1s subshell, pulling them closer to the nucleus.
