Atoms of the element sodium (atomic number 11) have the electron configuration 1s22s22p63s1
with the noble gas form [Ne]3s1
The noble gas electron configuration of a sodium ion is the same as that of neon, which is 1s² 2s² 2p⁶. This configuration represents the arrangement of electrons in the nearest noble gas element to sodium (Ne) before it loses one electron to become a sodium ion (Na+).
When phosphorus achieves a noble gas configuration, it gains three electrons to become the phosphide ion (P³⁻). This allows it to achieve the stable electron configuration of a noble gas, similar to argon.
No, the electron configuration for an ion is not always the same as that of its nearest noble gas. When an atom loses or gains electrons to form an ion, its electron configuration changes. For example, a sodium ion (Na⁺) has the electron configuration of [Ne], which is the same as neon, but a chloride ion (Cl⁻) also has the same configuration as argon ([Ar]). Thus, while some ions can have configurations similar to noble gases, this is not universally true for all ions.
Oxide ion (O²⁻) has the electron configuration of a noble gas neon (Ne), which is 1s² 2s² 2p⁶.
Argon has the same electron configuration as a sodium ion. Sodium ion has lost 1 electron from its outer shell, making its electronic configuration 2, 8. Argon's electronic configuration is also 2, 8 in its outer shell.
The ion formed when sodium achieves a noble-gas electronic configuration is Na+. This means that sodium has lost one electron to achieve the same electron configuration as neon, a noble gas, which has a stable electron configuration.
Sodium ion (Na+) and neon will have the same number of electrons
Both a neon atom and a sodium ion have 10 electrons. Neon is a noble gas with a full valence shell, while a sodium ion has lost one electron to achieve a stable electron configuration.
The noble gas electron configuration of a sodium ion is the same as that of neon, which is 1s² 2s² 2p⁶. This configuration represents the arrangement of electrons in the nearest noble gas element to sodium (Ne) before it loses one electron to become a sodium ion (Na+).
The most likely electron configuration for a sodium ion (Na+) in its ground state is 1s2 2s2 2p6. This configuration represents the electronic structure of a sodium atom that has lost one electron to become a sodium ion, achieving a stable octet configuration similar to that of a noble gas.
When phosphorus achieves a noble gas configuration, it gains three electrons to become the phosphide ion (P³⁻). This allows it to achieve the stable electron configuration of a noble gas, similar to argon.
No, the electron configuration for an ion is not always the same as that of its nearest noble gas. When an atom loses or gains electrons to form an ion, its electron configuration changes. For example, a sodium ion (Na⁺) has the electron configuration of [Ne], which is the same as neon, but a chloride ion (Cl⁻) also has the same configuration as argon ([Ar]). Thus, while some ions can have configurations similar to noble gases, this is not universally true for all ions.
Oxide ion (O²⁻) has the electron configuration of a noble gas neon (Ne), which is 1s² 2s² 2p⁶.
The calcium ion formed when it achieves a noble-gas electron configuration is Ca2+, as it loses two electrons to have the same electron configuration as argon, a noble gas.
Argon has the same electron configuration as a sodium ion. Sodium ion has lost 1 electron from its outer shell, making its electronic configuration 2, 8. Argon's electronic configuration is also 2, 8 in its outer shell.
That is correct. A noble gas (or at least all the noble gas elements heavier than helium) has an electron configuration of 8 electrons in its outer shell, and the sodium and chlorine ions in sodium chloride also have 8 electrons in their outer shell, just like a noble gas atom.
Sodium looses one electron to achieve noble gas electronic configuration.The formula of ion formed is Na+