What happens is that Beryllium is on the 2A group of the periodic tale, meanwhile Sulphur is on the 6A group. It's like two friends. One of them has 2 bucks, and the other one has 6. If they want to have the most amount of money by bringing eack dollar one by one, what is easier, ¿That the guy with six bucks takes one by one his 6 dollars to the other one or that the one with 2 just makes a double journey?. Imagine that the guy with 6 bucks is Sulphur and the other one is Beryllium. This is called electronegativity. The more on the left (your left) elements are, the more electronegatiuvity they have.
Beryllium loses 2 electrons as it has 2 valency and as it's electronic configuration is 2,2; so it shud either gain 6 e- or lose 2 e- and as losing 2 e- wud require less of energy as compared to gaining 6 e-, it loses 2 e-.
The same happens in the case of S. it's e- configuration is 2,8,6 it can either gain 2 e- or lose 6 e-; as gaining 2e- would require less of energy, it does so.
snother fact is that all elements whichlose e- are metals andgain are non-metals. Those who share are metalloids. But still there are some exceptions like Hydrogen, Carbon etc.
Beryllium has less electrons on it's outer shell than sulfur does and the more electrons on the outer shell the tighter the hold on electrons. So since beryllium has a looser hold on it outer shell electrons (because it has less) it loses its electrons. However if beryllium was forming ionic bonds say Hydrogen, Hydrogen would lose electrons while Beryllium gains.
Beryllium will lose electrons. It loses two valence electrons. Beryllium is an element that has an atomic number of 4, and is a classified as a metal.
Because of it's low valence, losing electrons takes the least amount of energy when trying to fill the outer energy level.
The elements classed as metals (left side of Periodic Table) have less of an attraction for their outer electrons than the classic oxidizers (O F S Cl Br).
I HAVE NO IDEA WHAT YOUR TALKING ABOUT
sorry if this was an interruption....
because nonmetals gain electrons in ionic bonds and metals lose electrons in ionic bonds(oxidize).
silicon prefers to share electrons forming covalent bonds
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My best guess is that Be is "tricked" into thinking that it's valence shell is now full since it's two valence electrons are now being "shared/hogged" by the much more electronegative Fluorine. I would guess that this is a highly polar covalent bond!?! 8-) Where is the senior chemistry teacher (RAM) around when I need her? Cheers, "Lurch" from the club club.
Beryllium generally forms covalent bonds. Beryllium is in the 2nd group and 2nd period so it is a very small cation. Smaller cation favors formation of covalent bonds. source(s):Fajan's Rule
because nonmetals gain electrons in ionic bonds and metals lose electrons in ionic bonds(oxidize).
Beryllium is a metal and while Sulphur is a non-metal. Hence when forming an ionic bond, Beryllium being a metal looses the electron and sulphur being a non-metal gains the electrons.
Beryllium would tend to lose its two electrons when forming a bond because it is easier to lose its two valence electrons rather than gain an additional five in order to obtain a full outer shell.
Sharing of electrons. Generally this involves pirs of electrons forming bonds.
Valence electrons.
No. Beryllium has only two valence electrons and forms ionic bonds with chlorine, not covalent bonds. Beryllium atoms form 2+ ions, and chlorine atoms form 1- ions in order to form the ionic compound beryllium chloride, BeCl2.
In covalent bonds, the atoms share their electrons.
silicon prefers to share electrons forming covalent bonds
Electrons
In most compounds, valence electrons are involved in forming bonds.
polar bonds
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