Question
Find the oxidation numbers of the transition metal in each of the following compounds:$\mathrm{CoSO}_{4} \quad$ b $\mathrm{Ta}_{2} \mathrm{O}_{5}$$\mathrm{Cu}_{2}(\mathrm{OH})_{3} \mathrm{Cl}$
Step 1
Step 1: The oxidation number of an atom in a compound is the charge it would have if all the bonds to atoms of different elements were 100% ionic. Show more…
Show all steps
Your feedback will help us improve your experience
Aadit Sharma and 76 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Find the oxidation numbers of the transition metal in each of the following compounds: a. $\mathrm{CoSO}_{4}$ b. $\mathrm{Ta}_{2} \mathrm{O}_{5}$ c. $\mathrm{Cu}_{2}(\mathrm{OH})_{3} \mathrm{Cl}$
Find the oxidation numbers of the transition metal in each of the following compounds: a $\mathrm{CdI}_{2}$ $\mathrm{CrO}_{3}$ c) $\mathrm{PtCl}_{2}\left(\mathrm{NH}_{3}\right)_{2} \quad$ d $\mathrm{Cu}(\mathrm{OH})_{2}$
Determine the oxidation state (oxidation number) of the transition metal in each compound. $$ \begin{array}{ll} \text { (a) } \mathrm{V}_{2} \mathrm{O}_{5} & \text { (b) } \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7} \\ \text { (c) } \mathrm{MnO}_{2} & \text { (d) } \mathrm{OsO}_{4} \end{array} $$
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD