* not completed

. The halogens have high electron affinity because:

They can accommodate only one electron in their valence shell; therefore the energy required for this process is low. correct incorrect

The incoming electron can occupy an orbital of an incomplete valence shell and thus experience strong nuclear attraction. correct incorrect

The nuclear attraction to the electrons in their atoms is high and tends to draw new electrons in. correct incorrect

* not completed

. Find the correct statement:

The Group 17 elements form hydrides that behave as acids in aqueous solutions correct incorrect

The Group 17 elements form very stable oxides commonly found in the laboratory correct incorrect

The Group 17 elements occur in oxidation states from -1 to +7. correct incorrect

* not completed

. Why are aqueous fluoride solutions not used in the production of fluorine by electrolysis?

because fluorides are insoluble in water correct incorrect

because water is oxidized at a much lower potential than F^– and because any F₂ produced would react rapidly with the water correct incorrect

because the electrolysis of water solutions of fluorides would require a prohibitively large amount of water and energy correct incorrect

* not completed

. Fluorine atoms are small and their electrons are tightly gripped by the nucleus. Therefore, molecular fluorine compounds have:

high polarizabilities and strong dispersion interactions correct incorrect

low polarizabilities and strong dispersion interactions correct incorrect

low polarizabilities and weak dispersion interactions correct incorrect

* not completed

. What is the molecular geometry of ClF₃ as predicted by VSEPR?

T-shaped correct incorrect

trigonal bipyramidal correct incorrect

trigonal planar correct incorrect

* not completed

. When I₂ is added to a solution containing I^–, a deep brown colour develops. How can that phenomenon be explained?

I^– is oxidized to I₂. correct incorrect

I₂ is dissolved in the water. correct incorrect

Polyiodides, such as I₃^– and I₅^–, are formed. correct incorrect

* not completed

. Perchlorate is a very weak Brønsted base and a weak Lewis base and is used as a weakly coordinating ion that can be easily displaced from a complex by other ligands. When using the perchlorate ion in this situation, care must be taken because:

The perchlorate ion is a powerful oxidizing agent that can explode unexpectedly and unpredictably. correct incorrect

The perchlorate ion is a powerful oxidizing agent that rapidly oxidizes the ligands before complexes are formed for further study. correct incorrect

The perchlorate ion is a powerful oxidizing agent that rapidly oxidizes the metal acceptors before complexes are formed for further study. correct incorrect

* not completed

. In basic solutions chlorine, bromine, and iodine undergo ___________, with the formation of +1 (XO^–) and ______ species:

comproprionation; +3 (XO₂^–) correct incorrect

reduction; O₂ correct incorrect

disproportionation; –1 (X^–) correct incorrect

* not completed

. The oxidation of molecules and ions by halogen oxoanions increases in the order:

ClO₂^– < ClO₃^– < ClO₄^– correct incorrect

ClO₄^– < BrO₄^– < IO₄^– correct incorrect

IO₃^– < IO₄^– correct incorrect

* not completed

. Which transition metal fluoride is used in the production of fluorocarbons?

FeF₃ correct incorrect

CoF₃ correct incorrect

NiF₂ correct incorrect