Named after the Greek word for “bright,” Beryllium is a metal with an atomic number of 4. It has 2 valence electrons, which makes it a member of group 2 in the periodic table. How many valence electrons does beryllium have? Why does beryllium have 2 valence electrons? Does Beryllium have 4 Valance Electrons? How do you find the Valence Electrons of Beryllium?
There are a number of reasons why beryllium only has two valence electrons. The first is that it needs to have eight protons in its nucleus, and the second reason is that if beryllium had four valance electrons then it would not be stable enough to exist on earth. It must also maintain an outer electron shell with full occupancy due to the octet rule. This means they need their orbitals filled until all energy levels are maxed out before adding more electrons into the orbital energy level.
Beryllium has two valence electrons because it needs to have eight protons in its nucleus, and if beryllium had four then it would not be stable enough. It must also maintain an outer electron shell with full occupancy due to the octet rule. This means they need their orbitals filled until all energy levels are maxed out before adding more electrons into the orbital level.
The Octet Rule:
Beryllium must also maintain an outer shell of fully occupied orbitals which is called the octet rule; this means that within each subshell (each different column), there should only be a maximum of eight electrons total. If you add one more without removing another, many things can happen including instability in the atom and different chemical reactions.
The Electron Shell: If you look at the electron shell, it is made up of many orbitals that are all filled with electrons except for one orbital which can hold eight more before adding another would be considered unstable or a violation of the octet rule. The only way to fill these without violating any rules is by using two valence electrons from beryllium’s four in order to complete its outer electron shell. You will see this difference if you compare how many valance electrons each element has after viewing their periodic table entry. How many valence electrons does beryllium have?
How do you find the valence electrons of beryllium?
Beryllium has four total, but only two are used for its outer shell. Berylliums low atomic number is what contributes to it having just two valance electrons in order to complete its electron shells and stay stable. The octet rule states that an atom will try to fill up its orbitals with eight rather than ten or more which would make them unstable. Even though this makes a difference when looking at other periodic table entries of elements, it plays no role here because these atoms all follow the same rules.
Beryllium has a bond order of two, which means that it can be considered to have four valence electrons. This is because beryllium outer dots are not used for bonding and so they do not count towards its total electron shell’s number of bonds. The octet rule states that an atom will try to fill up its orbitals with eight rather than ten or more which would make them unstable. With this in mind, the only way to ensure stability is by filling all of the bits on your periodic table entry first before going on to anything else.
No matter what other atoms you look at on the periodic table, each one will follow the same rules as discussed here meaning there are exceptions like hydrogen having one electron in its outermost shell.
Beryllium has two valence electrons and so it will need to form bonds with other atoms, such as helium or carbon, which have the same number of valence electrons. In order for beryllium to be stable meaning that there is no risk of becoming unstable if left alone (ie not bonded) then the atom needs four more orbitals than what it already has before bonding can take place.
In other words, beryllium will need to have six electrons in its outermost shell before it can bond with another atom and be stable. This is why beryllium has a full set of four orbitals plus two more orbital which are being used for bonding purposes.