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Chapter 18: Q104 E (page 1047)

What is the hybridization of iodine in\({\rm{I}}{{\rm{F}}_3}\)and \({\rm{I}}{{\rm{F}}_5}\)?

Short Answer

Expert verified

The hybridization of Iodine in \(I{F_3}\)is \(s{p^3}d\) and the \(I{F_5}\)is \(s{p^3}{d^2}\) respectively.

Step by step solution

01

Step 1:Concept of Hybridization

Hybridization is defined as an idea of mixing two atomic orbitals to give rise to a new type of hybridized orbitals which are comparable in energy.

02

The Hybridization of iodine in \(I{F_3}\).  

The \(I{F_3}\) is \(s{p^3}d\) hybridized.

03

The Hybridization of iodine in \(I{F_5}\).

The hybridization of \(I{F_5}\) is \(s{p^3}{d^2}\).

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Most popular questions from this chapter

Write balanced chemical equations for the following reactions:

(a) cadmium burned in air

(b) elemental cadmium added to a solution of hydrochloric acid

(c) cadmium hydroxide added to a solution of acetic acid, \({\rm{C}}{{\rm{H}}_3}{\rm{C}}{{\rm{O}}_2}{\rm{H}}\)

Give balanced equations for the overall reaction in the electrolysis of molten lithium chloride and for the reactions occurring at the electrodes. You may wish to review the chapter on electrochemistry for relevant examples.

Why is it necessary to keep the chlorine and sodium, resulting from the electrolysis of sodium chloride, separate during the production of sodium metal?

What is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of mercury, if the fish contains \({\bf{30}}\)parts per million of mercury by weight? (Assume that all the mercury from the fish ends up asMercury (II) chloride in the body and that a fatal dose is \({\bf{0}}.{\bf{20}}{\rm{ }}{\bf{g}}\) of\({\bf{HgC}}{{\bf{l}}_2}\).) How many pounds of fish is this?

The reaction of calcium hydride,\({\rm{Ca}}{{\rm{H}}_{\rm{2}}}\), with water can be characterized as a Lewis acid-base reaction: \({\rm{Ca}}{{\rm{H}}_{\rm{2}}}\left( {\rm{s}} \right){\rm{ + 2}}{{\rm{H}}_{\rm{2}}}{\rm{O}}\left( {\rm{l}} \right) \to {\rm{Ca}}{\left( {{\rm{OH}}} \right)_{\rm{2}}}\left( {{\rm{aq}}} \right){\rm{ + 2}}{{\rm{H}}_{\rm{2}}}\left( {\rm{g}} \right)\).

Identify the Lewis acid and the Lewis base among the reactants. The reaction is also an oxidation-reduction reaction. Identify the oxidizing agent, the reducing agent, and the changes in oxidation number that occur in the reaction.
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