Question

draw the lewis structure for n₂br₂ molecule. be sure to include all lone pair electrons and nonzero formal charges. click and drag to start drawing a structure.

Explanation:

Step1: Determine valence electrons

N has 5 valence electrons and Br has 7 valence electrons. For \(N_2Br_2\), total valence electrons = \(2\times5 + 2\times7= 24\).

Step2: Arrange atoms

Arrange the two N atoms in the middle and one Br on each side (\(Br - N - N - Br\)).

Step3: Form single - bonds

Connect the atoms with single - bonds (\(Br - N - N - Br\)). Each single - bond uses 2 electrons, so 6 electrons are used so far, leaving \(24 - 6=18\) electrons.

Step4: Add lone - pairs

Add lone - pairs to satisfy the octet rule. Each Br needs 3 lone - pairs (6 electrons per Br) and each N needs 1 lone - pair (2 electrons per N).

Step5: Check formal charges

The formal charge on an atom is given by \(FC = V - N_{bonding}-N_{non - bonding}\), where \(V\) is the number of valence electrons of the atom in isolation, \(N_{bonding}\) is the number of bonding electrons, and \(N_{non - bonding}\) is the number of non - bonding electrons. For \(N_2Br_2\) in the structure with single bonds between all atoms and appropriate lone - pairs, the formal charges on all atoms are zero. The Lewis structure has the following form:
Br has 3 lone - pairs and is single - bonded to N. N has 1 lone - pair and is single - bonded to another N and a Br. The other N and Br are arranged symmetrically.

Answer:

The Lewis structure has two N atoms in the middle with a single bond between them. Each N is single - bonded to a Br atom. Each Br has 3 lone - pairs of electrons and each N has 1 lone - pair of electrons, with all atoms having a formal charge of zero.