Boron must give up 3 electrons in order to achieve a noble-gas electron configuration.
Noble gases
When an electron is removed from the valence shell of a noble gas, it forms a positively charged ion since the number of protons in the nucleus is greater than the number of electrons. This process requires energy and is generally not favored for noble gases due to their stability from having a full valence shell.
Noble Gas Configurations
This is the family of noble gases (group 18).
Helium has 2 valence electrons. All other noble gases have 8 valence electrons.
Noble gases
When an electron is removed from the valence shell of a noble gas, it forms a positively charged ion since the number of protons in the nucleus is greater than the number of electrons. This process requires energy and is generally not favored for noble gases due to their stability from having a full valence shell.
Noble Gas Configurations
This is the family of noble gases (group 18).
Helium has 2 valence electrons. All other noble gases have 8 valence electrons.
Noble gases have completely filled orbitals / energy levels. They generally have 8 valence electrons (helium has only 2 valence electrons) and have stable electronic configuration.
Group 18 contains eight valence electrons, namely the noble gases.
I - Alkali Metals II - Earth Alkali Metals III - Boron Group IV - Carbon Group V - Nitrogen Group VI - Chalcogenes VII - Halogenes VIII - Noble Gases
Helium has only 2 valence electrons. The rest noble gases have eight.
The noble gases are elements with their valence band completely full of electrons: for helium this is 2 electrons, for all other noble gases this is 8 electrons. Because their valence band is already full they do not normally participate in chemical reactions.
Because all noble gases have completely filled valence orbitals. Helium has 2 valence electrons whereas all other noble gases have 8 valence electrons.
There are no unpaired electrons. All electron shells are filled; this is the reason they are called the noble gases.