Question

Ti4+ salts are colourless where cr3+ salts are coloured

Answer 1

here is your answer ------
electronic configuration of Ti4+ is fully filled while Cr3+ has d4 configuration ,so there is non paired electron in Titanium 4 positive and there are four unpaired electron in Cr 3 positive
that's why Titanium 4 positives is colourless and chromium 3 positive is coloured

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Answer 2

Answer : $Ti^{4+}$ salts are colorless where $Cr^{3+}$ salts are colored due to the number of unpaired electrons present in $Cr^{3+}$.

Explanation :

The element is titanium with symbol (Ti).

Atomic number of titanium is, 22

Number of electrons in titanium = 22

The electronic configuration of titanium will be,

$1s^22s^23s^23p^64s^23d^2$

The electronic configuration of $Ti^{4+}$ will be,

$1s^22s^23s^23p^6$

As we know that the more the number of unpaired electrons present in the ion, the element will shows color due to the transition of the electrons from ground state to the excited state.

In case of $Ti^{4+}$, there is no unpaired electrons that means the shells are fully filled. So, they will not show any color. That's why $Ti^{4+}$ are colorless.

The element is chromium with symbol (Cr).

Atomic number of chromium is, 26

Number of electrons in chromium = 26

The electronic configuration of chromium will be,

$1s^22s^23s^23p^64s^13d^5$

The electronic configuration of $Cr^{3+}$ will be,

$1s^22s^23s^23p^63d^3$

In case of $Cr^{3+}$, there are 3 unpaired electrons present in d-shell. So, they will show color. That's why $Cr^{3+}$ salts are colored.

Hence, the $Ti^{4+}$ salts are colorless where $Cr^{3+}$ salts are colored due to the number of unpaired electrons present in $Cr^{3+}$.