boron has very small atomic radius.the hypothetical B3+ ion has very small size and hence high charge densities.This value is so high that B3+ ion does not exist.All thecompounds of boron are therefor covalent.Boron has 4 valencce electro n and this gives it a great electron accepting power that is its compound behave as strong lewis acid
Cl- This is the symbol of a chlorine ion that gains one electron
The reaction between ammonia and boron trifluoride, BF3If you have recently read the page on covalent bonding, you may remember boron trifluoride as a compound which doesn't have a noble gas structure around the boron atom. The boron only has 3 pairs of electrons in its bonding level, whereas there would be room for 4 pairs. BF3 is described as being electron deficient.The lone pair on the nitrogen of an ammonia molecule can be used to overcome that deficiency, and a compound is formed involving a co-ordinate bond.Using lines to represent the bonds, this could be drawn more simply as:The second diagram shows another way that you might find co-ordinate bonds drawn. The nitrogen end of the bond has become positive because the electron pair has moved away from the nitrogen towards the boron - which has therefore become negative. We shan't use this method again - it's more confusing than just using an arrow.
When a fluorine atom gains an electron, it forms a negative ion.
No. Potassium (K) has only one valence electron, so it would only form a 1+ ion, not the 2+ ion needed for KF2. So instead it forms KF.
Magnesium forms divalent cations and chlorine forms monovalent anions; therefore, the binary compound of magnesium and chloride has the formula MgCl2.
boron
Many elements can combine with Boron although not many compound with Boron in are found on Earth naturally. Here are some more common examples: Barium (Ba) - Forms Barium Borate Calcium (Ca) - Forms Calcium Borate Lithium (Li) - Forms Lithium Borate
Potassium lose an electron (iodine gain this electron) to form potassium iodide, KI.
Boron has an electronic configuration of 1s22s22p1 (it has 5 electrons). In order to reach the stable electron configuration of a noble gas with a completely filled valence shell, boron atom has to lose 3 electrons to obtain a stable duplet structure (i.e. 2 electrons in its first electron shell). After losing 3 electrons, the boron atom forms a B3+ ion, or a so-called tripositive ion.
Cl-
ionic bond
Boron forms electron poor hydrides that can exist in many different shapes and formulas because of the hydrogen bridges it can form.
Cl- This is the symbol of a chlorine ion that gains one electron
Cl- This is the symbol of a chlorine ion that gains one electron
xe forms chemical compound among inert gass because :Low ionization EnthalpyMore negative electron gain enthalpyamong all the other inert gases.
The reaction between ammonia and boron trifluoride, BF3If you have recently read the page on covalent bonding, you may remember boron trifluoride as a compound which doesn't have a noble gas structure around the boron atom. The boron only has 3 pairs of electrons in its bonding level, whereas there would be room for 4 pairs. BF3 is described as being electron deficient.The lone pair on the nitrogen of an ammonia molecule can be used to overcome that deficiency, and a compound is formed involving a co-ordinate bond.Using lines to represent the bonds, this could be drawn more simply as:The second diagram shows another way that you might find co-ordinate bonds drawn. The nitrogen end of the bond has become positive because the electron pair has moved away from the nitrogen towards the boron - which has therefore become negative. We shan't use this method again - it's more confusing than just using an arrow.
Strontium.