atoms in stable compounds almost always have a noble gas electron configuration or when representative metals and nonmetals react, thay transferelectrons in such a way that both th cation and the anion have noble gas electron configuration.
The most likely charge on an ion formed by an element with a valence electron configuration of ns1 is +1. This is because elements with ns1 configuration tend to lose one electron to achieve a stable noble gas configuration, which results in a +1 charge.
The electron configuration of neon determines its effective nuclear charge. Neon has a full outer electron shell, which means it has a high effective nuclear charge because the positive charge of the nucleus is not shielded by inner electrons.
The -2 charge ion with the same electron configuration as krypton is the oxide ion (O2-). Krypton has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6. The oxide ion gains two electrons to achieve a full valence shell, resulting in an electron configuration of 1s2 2s2 2p6.
The ion charge for sodium is +1. This means that sodium loses one electron to achieve a stable electron configuration.
Potassium forms a +1 charge, meaning it typically loses one electron to achieve a stable electron configuration.
Chlorine's charge after accepting an electron is -1, as it gains one negative charge when it accepts an electron to achieve a stable electron configuration.
The most likely charge on an ion formed by an element with a valence electron configuration of ns1 is +1. This is because elements with ns1 configuration tend to lose one electron to achieve a stable noble gas configuration, which results in a +1 charge.
Electron is a subatomic particle. This is negative elementary electric charge.
The electron configuration for a nitrogen anion with a charge of -2 (N²⁻) involves adding two additional electrons to the neutral nitrogen atom. The neutral nitrogen atom has an electron configuration of 1s² 2s² 2p³. Therefore, the electron configuration for the N²⁻ ion is 1s² 2s² 2p⁵.
The charge of chlorine is -1. It typically gains one electron to achieve a stable octet electron configuration.
The electron configuration of neon determines its effective nuclear charge. Neon has a full outer electron shell, which means it has a high effective nuclear charge because the positive charge of the nucleus is not shielded by inner electrons.
The -2 charge ion with the same electron configuration as krypton is the oxide ion (O2-). Krypton has the electron configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6. The oxide ion gains two electrons to achieve a full valence shell, resulting in an electron configuration of 1s2 2s2 2p6.
Potassium forms a +1 charge, meaning it typically loses one electron to achieve a stable electron configuration.
The ion charge for sodium is +1. This means that sodium loses one electron to achieve a stable electron configuration.
Lithium does not have a '0' charge. Its electron configuration is 2,1. This means there is one valence electron in its outer shell. Losing this electron will make Lithium have a full shell (2 only) which all atoms try to achieve, therefore Li has a +1 charge because it loses an electron to gain noble gas configuration.
Iodide (I⁻) has a negative charge of -1. This occurs because it gains an extra electron, resulting in a net negative charge. As a halogen, iodide readily accepts an electron to achieve a stable electron configuration.
The most common charge of sodium is +1, as it typically loses one electron to achieve a stable electron configuration.