1 electron in the s orbital
it has 1
the alkali metals have 1 electron in their outer most shell. in order to obtain a full outer shell they have to lose this electron. so when they react with another metal they lose this electron and the outer most shell.
The electron configuration of rutherfordium is: [Rn] 5f14 6d2 7s2.
1 electron in the s orbital
it has one electron in its outer energy level like all alkali metals
The electron configuration of copper is 1s22s22p63s23p63d104s1.
The alkali metals exist in group one of the Periodic Table; as such, they are in the s-block. The electron configuration for each alkali metal ends in ns1. When represented in an Aufbau diagram, the outer shell electron has an "up" spin. Because of their single outer shell electron, alkali metals react well with halogens.
The alkali metals exist in group one of the Periodic Table; as such, they are in the s-block. The electron configuration for each alkali metal ends in ns1. When represented in an Aufbau diagram, the outer shell electron has an "up" spin. Because of their single outer shell electron, alkali metals react well with halogens.
alkali metal
The electron outside the shell donate its electron to the one inside the shell
I assume you are talking about the Alkali metal group which in fact would readily loose their outer electron to form a 1+ cation (have a full valence electron shell).
the alkali metals have 1 electron in their outer most shell. in order to obtain a full outer shell they have to lose this electron. so when they react with another metal they lose this electron and the outer most shell.
The electron configuration of rutherfordium is: [Rn] 5f14 6d2 7s2.
1 electron in the s orbital
it has one electron in its outer energy level like all alkali metals
halogens
It is classed with group 1 because, like the alkali metals it has only 1 outer shell electron.
The oute (valence) shell of the alkali metals contains just one electron