The electron configuration of vanadium (V), which has an atomic number of 23, is written as ( \text{[Ar]} 3d^3 4s^2 ). This indicates that vanadium has two electrons in the 4s subshell and three electrons in the 3d subshell, following the argon core. The arrangement reflects the filling of the 3d and 4s orbitals according to the Aufbau principle.
the correct electronic confrigration of phosperous is 2,8,5
Other elements can acquire a noble gas configuration by either gaining or losing electrons. Elements on the left side of the periodic table, such as alkali metals, tend to lose electrons to achieve a noble gas configuration. Elements on the right side of the periodic table, such as halogens, tend to gain electrons to achieve a noble gas configuration. Elements in the middle of the periodic table may gain or lose electrons to acquire a noble gas configuration, depending on the specific element and its properties.
Because emission spectrum are the result of the electron configuration of the element and no two elements have exactly the same electron configuration.
All the elements in their normal state are reactive and unstable. In order to attain stability i.e. a state of minimum energy, they tend to form ions by loosing or gaining electrons. By doing so, they achieve stable electronic configuration or noble gas configuration. However, some elements do not form ions. Instead of that, two such atoms share electrons with each other and achieve this noble gas configuration. At the end, the main reason for attaining a noble gas configuration is to attain max. stability and min. energy.
Looks like copper.
The nitrogen family, group 15, is characterized by an s2p3 configuration.
Only group 18 elements have noble gas configuration. All other elements lack a noble gas electronic configuration.
the correct electronic confrigration of phosperous is 2,8,5
Magnesium
Vanadium ( V) has that configuration. Its atomic number is 23.
Electron configuration is a term applied to chemical elements not to compounds.
The configuration of various elements
The configuration of various elements
By acquiring noble gas configuration elements become stable .
Other elements can acquire a noble gas configuration by either gaining or losing electrons. Elements on the left side of the periodic table, such as alkali metals, tend to lose electrons to achieve a noble gas configuration. Elements on the right side of the periodic table, such as halogens, tend to gain electrons to achieve a noble gas configuration. Elements in the middle of the periodic table may gain or lose electrons to acquire a noble gas configuration, depending on the specific element and its properties.
Because emission spectrum are the result of the electron configuration of the element and no two elements have exactly the same electron configuration.
"V" stands for Vanadium.