The electron configuration of a Copper(II)ion is [Ar]4s0 3d9.
The electron configuration for a potassium ion (K+) is [Ar] 4s1. Potassium loses one electron to form the +1 ion, resulting in a noble gas configuration like argon.
The ions of elements nitrogen (N3-), oxygen (O2-), and fluorine (F-) will have the same electron configuration as a sodium ion (Na+), which is the same as the electron configuration of the noble gas neon.
The electronic configuration for the sodium ion, Na+ is 1s2 2s2 2p6 or [Ne]
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^+.
The ion charge for sodium is +1. This means that sodium loses one electron to achieve a stable electron configuration.
The electron configuration of Cu+1 is [Ar] 3d10 4s1. When copper loses one electron to become a +1 ion, it loses the 4s electron first, followed by one of the 3d electrons to attain a stable electron configuration.
The electron configuration for a potassium ion (K+) is [Ar] 4s1. Potassium loses one electron to form the +1 ion, resulting in a noble gas configuration like argon.
The ions of elements nitrogen (N3-), oxygen (O2-), and fluorine (F-) will have the same electron configuration as a sodium ion (Na+), which is the same as the electron configuration of the noble gas neon.
The electronic configuration for the sodium ion, Na+ is 1s2 2s2 2p6 or [Ne]
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^+.
The ion charge for sodium is +1. This means that sodium loses one 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.
Copper has an electron configuration of [Ar] 3d10 4s1, with a fully filled d orbital. This stability allows for unpaired electrons, making copper paramagnetic. When it forms a 1+ ion, it loses the 4s electron, resulting in a filled 3d orbital, leading to no unpaired electrons and making it diamagnetic.
When fluorine forms an ion, it gains one electron to achieve a stable electron configuration, becoming a fluoride ion with a charge of -1.
Bromine can form a -1 ion by gaining one electron to achieve a stable electron configuration. This allows bromine to attain a full outer electron shell, similar to the electron configuration of a noble gas, making it more stable.
The electron configuration of a fluorine atom is 1s2 2s2 2p5. When fluorine gains an electron to form a fluoride ion, its electron configuration becomes 1s2 2s2 2p6, which is the same as that of a noble gas (neon). This gives the fluoride ion a stable, filled outer electron shell.
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.