In which of the following compounds does the transition-metal have the highest oxidation number? in which of the following compounds does the transition-metal have the highest oxidation number? rb3[moo3f3] k4[mn(cn)6] na[ag(cn)2] k2[ptcl6] [co(nh3)4cl2]

The transition-metal have the highest oxidation number is Mo in Rb₃[MoO₃F₃]

Explanation:

Transition metals are metals that are found in the middle of the periodic table.

For the compounds:

Rb₃[MoO₃F₃]: Rb is an alkali metal that has a charge of +1. that means [MoO₃F₃] is -3. The oxyfluoride O₃F₃ has a charge of -9. That means the Mo is +6

K₄[Mn(CN)₆]: Potassium is +1, thus, the [Mn(CN)₆] is -4, As the CN is -1 and there are 6, the Mn is +2

Na[Ag(CN)₂]: As Na is +1, the [Ag(CN)₂] is -1. As CN are -1, the Ag is +1

K₂[PtCl₆]: Potassium is +1, the [PtCl₆] is -2, As the Cl are -1, the Pt is +4

[Co(NH₃)₄Cl₂]: The NH₃ are neutral, The Cl are -1, that means the Co is +2.

The transition-metal have the highest oxidation number is Mo +6

I hope it helps!

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