Describe the hybrid orbitals used by the central atom(s) and the type(s) of bonds formed in:

1 answer:

3 0

sp2 Hybridization. The valence orbitals of a central atom surrounded by three regions of electron density consist of a set of three sp2 hybrid orbitals and one unhybridized p orbital.

<h3>How do you describe hybrid orbitals?</h3>

A hybrid orbital is an orbital formed by the combination of two or more atomic orbitals. The resulting orbital has a different shape and energy than the component orbitals that form it. Hybridization is used to model molecular geometry and to explain atomic bonding.

<h3>What is the hybridization of the s atom?</h3>

The middle S atom containing the 5 valence atomic orbitals is basically hybridized to form five sp3d hybrid orbitals. In 2P-orbitals, four hybrid orbitals are overlapped and the fifth one contains a lone pair.

Learn more about hybrid orbitals here:

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Consider the reaction 2NO(g) 1 O2(g) ¡ 2NO2(g) Suppose that at a particular moment during the reaction nitric oxide (NO) is reac

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<h2>a) The rate at which $NO_2$ is formed is 0.066 M/s</h2><h2>b) The rate at which molecular oxygen $O_2$ is reacting is 0.033 M/s</h2>

Explanation:

Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.

$2NO(g)+O_2(g)\rightarrow 2NO_2(g)$

The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.

Rate in terms of disappearance of $NO$ = $-\frac{1d[NO]}{2dt}$ = 0.066 M/s