Which of the following cation(s) will turn blue in oxidizing flame ?

C o^{2 +}

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C r^{3 +}

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N i^{2 +}

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C u^{2 +}

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Solution

The correct options are
A $C o^{2 +}$
D $C u^{2 +}$
Option (A),(D) are correct.
$C o^{2 +}$ and $C u^{2 +}$ will turn blue in oxidizing flame.
$C o^{2 +}$ turns blue in reducing flame while $C u^{2 +}$ turns brown red in reducing flame.

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H_{2} S

{C u}^{2 +}

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N i^{2 +}

M^{2 +}

Z n^{2 +} > S c^{2 +} = C u^{2 +} > T i^{2 +} = N i^{2 +} > V^{2 +} = C o^{2 +} > C r^{2 +} = F e^{2 +} > M n^{2 +}

M n^{2 +}, C o^{2 +}, Z n^{2 +} & N i^{2 +}

Write down the number of 3d electrons in each of the following ions:

Ti²⁺, V²⁺, Cr³⁺, Mn²⁺, Fe²⁺, Fe³⁺, CO²⁺, Ni²⁺ and Cu²⁺.

Indicate how would you expect the five 3d orbitals to be occupied for these hydrated ions (octahedral).

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