BrCl Lewis dot structure

Answer 1

maybe...

Cl:Br

(hard to draw... but additional 6 dots around each... Cl and Br)

Br valence electrons=7

Cl valence electrons =7

total= 14 e-

- 2 e- ( bond between Cl and Br)

= 12 e-

- 6 e- ( 6 dots around Cl to fill octet)

= 6 e-

- 6 e- ( 6dots around Br to fill octet)

= 0 e-

Fomal charges= (number of e- in valence shell of isolated atom)-(number of bonds to the atom+number of unshared e-)

Formal charge Br= 7 - (1+6)= 0

Formal charge Cl= 7- (1+6)=0

Since Formal charge is 0 this is the preferred Lewis structure for the molecule (least amount of energy used... and molecules like it when they are using the lowest amount energy)

Answer 2

A Lewis dot diagram needs to account for all the valence electrons in the elements. Boron has 3 and chlorine has 7, which means that the diagram needs to show 24 electrons. Electrons are shown either in bonds (a solid line representing two electrons) or as dots that represent bonding electrons, usually in pairs.

Thus the boron atom would be shown in the central position, with the chlorine atoms situated at 90 degree angles to it, joined by a dash. Each element is represented by its chemical symbol.

Though most elements form 4 bonds and need to be surrounded by 8 electrons to be stable (having a completed octet), boron is an exception and can only form 3 bonds. Thus, being joined to 3 chlorines, its electron requirements have been fulfilled.

The three bonds have taken care of 6 of the valence electrons. The remaining 18 are placed around the chlorine atoms in pairs to complete each chlorine's octet, represented by drawing a pair of dots on the three sides of the Cl symbol that are not bonded to B.

It works out that there are just enough electrons to surround each chlorine with three pairs. These 6 electrons, plus the bond with boron, give each chlorine a completed octet.

Answer 3

.. ..

: Cl - Be - Cl : .. ..