If element X is in period 5 of the Periodic Table, it typically has five electron shells. When it forms an ion, it often loses or gains electrons to achieve a stable electron configuration similar to that of the nearest noble gas, which in this case is krypton (Kr). For example, if X is a metal, it may lose electrons to form a cation with a configuration resembling Kr. Conversely, if X is a non-metal, it may gain electrons to achieve the same stable electron configuration.
No, chlorine (Cl) does not have a noble gas electronic configuration. It has the electron configuration [Ne]3s^2 3p^5, which is one electron away from achieving a stable, noble gas configuration like argon (Ar).
Sulfide, S2-
Fr is in the 1st period. It removes an electron to get noble gas configuration. Fr+ does not have valence electrons.Francium has 1 electron in its outermost energy level. It donates its outermost electron to stabilize its electron configuration. Francium(I) has no valence electrons.
Iodine accepts one electron to achieve noble gas configuration. Strontium loses two electrons to achieve noble gas configuration. Nitrogen accepts three electrons to achieve noble gas configuration. Krypton already has a noble gas configuration.
A noble gas electron configuration involves representing an element's electron configuration by using the electron configuration of the nearest noble gas preceding it in the periodic table, followed by the remaining electron configuration for that element. For example, the noble gas electron configuration for sodium (Na) is [Ne] 3s¹, where [Ne] represents the electron configuration of neon leading up to sodium.
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.
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.
No, chlorine (Cl) does not have a noble gas electronic configuration. It has the electron configuration [Ne]3s^2 3p^5, which is one electron away from achieving a stable, noble gas configuration like argon (Ar).
The noble gas configuration for potassium is [Ar] 4s^1. To form a cation, potassium would lose its one valence electron, resulting in a 1+ ion. Therefore, the ion formed when potassium achieves a noble gas electron configuration is K^+.
P3-
The ion formed when potassium achieves noble-gas electron configuration is K+ (potassium ion). This occurs when potassium loses one electron to have a full outer electron shell, similar to the nearest noble gas, argon.
The "Noble gas electron configuration," or the condensed electron configuration, for F is [He] 2s2 3p5.
Sulfide, S2-
When potassium achieves a noble gas electron configuration, it loses one electron to form the K+ ion. The K+ ion has a stable electron configuration similar to that of argon, with 18 electrons.
P-3 ion is formed with 18 electrons.
An atom of silicon needs to gain 4 electrons in its 3p sublevel to attain the noble gas electron configuration of argon, the noble gas in period 3 of the periodic table.
P3- or phosphide ion is formed. it has the same number of electrons as the noble gas, argon