[He] 2s2 2p1
[Kr] 5s1
Yes it is possible to write the noble gas configuration of all elements, though it is not possible to list all of them here.
[Xe] 4f14 5d2 6s2
Boron must give up 3 electrons in order to achieve a noble-gas electron configuration.
The electron configuration for a ground-state potassium atom is 1s22s22p63s23p64s1. The noble gas shorthand configuration is [Ar]4s1.
2.3!<-----wrong shorthand electron configuration for Boron (B on the periodic table) is [He] 2s2 2p1 because Shorthand means building on the last noble gas element. So put the closest Noble gas element before this one and then the new addition.
The electron configuration of boron is: [He]2s2.2p1.
[Ne]3s23p3
[Kr] 5s1
The standard electron configuration form of boron is 1s2 2s2 2p1. The noble gas form is [He] 2s2 2p1.
The atoms of the element boron (atomic number 5) have the electron configuration 1s2 2s2 2p1 *or noble-gas form [He] 2s2 2p1
Yes it is possible to write the noble gas configuration of all elements, though it is not possible to list all of them here.
[Xe] 4f14 5d2 6s2
Boron must give up 3 electrons in order to achieve a noble-gas electron configuration.
The electron configuration for a ground-state potassium atom is 1s22s22p63s23p64s1. The noble gas shorthand configuration is [Ar]4s1.
Boron gains noble gas configuration by losing 3 electrons. So it forms positive ions.
[Xe] 4f14 5d10 6s2 6p2