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It would look something like this
.. .. ..
: F ----Br -----F:
.. .. ..
There are 21 valence electrons in neutral BrF2, so there will be one unpaired. Draw each F having a shared pair, giving each F 8 electrons. The central Br atom will have 9 electrons.
If the charge is BrF2 there will only be 8 electrons around Br, if the charge is BrF2- then there will 10. BrF2+ is well known.
To draw the Lewis dot structure for BrF2, start by placing the least electronegative element (Br) in the center. Add the two fluorine (F) atoms around the bromine atom, each bonded by a single bond to Br. Finally, add lone pairs to the fluorine atoms to complete the octet rule for each atom. This will result in a structure where Br is surrounded by two F atoms, each with three lone pairs.
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How do you draw a Lewis structure for Be2 plus?
To draw a Lewis structure for Be2+, start by writing the symbol for beryllium. Since Be2+ has a 2+ charge, it has lost two electrons. Place the two electrons as individual dots around the beryllium symbol, as there is no other atom bonded to it. The Lewis structure for Be2+ is simply Be with two dots around it.
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1 Source: My online chemistry book.
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Two equivalent Lewis structures are necessary to describe the bonding in NH4+ because nitrogen in the ammonium ion has a full octet and can form a single coordinate covalent bond with each of the four hydrogen atoms, resulting in two resonance structures.
How do you draw a Lewis structure for Be2 plus?
To draw a Lewis structure for Be2+, start by writing the symbol for beryllium. Since Be2+ has a 2+ charge, it has lost two electrons. Place the two electrons as individual dots around the beryllium symbol, as there is no other atom bonded to it. The Lewis structure for Be2+ is simply Be with two dots around it.
How many equivalent Lewis structures are necessary to describe the bonding in PCl4 plus?
1 Source: My online chemistry book.
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