Which of the following best helps to explain why the electron affinity of Br has a greater magnitude than that of I?
A) Br has a lower electronegativity than I does.
B) Br has a lower ionization energy than I does.
C)An added electron would go into a new shell in Br but not in I
(D) There is a greater attraction between an added electron and the nucleus in Br than in I.

Express the oxidation state numerically (e.g., +1).

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Ions

In an ion, the sum of the oxidation states is equal to the overall ionic charge. Note that the sign of the oxidation states and the number of atoms associated with each oxidation state must be considered. In OH−, for example, the oxygen atom has an oxidation state of −2 and the hydrogen atom has an oxidation state of +1, for a total of (−2)+(+1)=−1.

Part C

What is the oxidation state of an individual phosphorus atom in PO33−?

Express the oxidation state numerically (e.g., +1).

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Part D

What is the oxidation state of each individual carbon atom in C2O42−?

Express the oxidation state numerically (e.g., +1).