The common positive oxidation states for an element with atomic number 24, are
(a) + 2 to + 6
(b) +

Q: Why isn't the configuration $4s^2 3d^4$?

A half-filled $3d^5$ subshell is significantly more stable due to exchange energy and symmetrical electron distribution, so one electron shifts from the $4s$ orbital to the $3d$ orbital.

Q: Does Chromium ever show a +1 oxidation state?

Yes, but it is extremely rare and only found in specific coordination complexes. It is not considered a "common" oxidation state.

Q: Why is +3 the most stable state for Chromium in aqueous solution?

The $Cr^{3+}$ ion has a $3d^3$ configuration, which corresponds to an exactly half-filled $t_{2g}$ level in an octahedral crystal field, making it highly stable.

Q: Can Chromium show a +7 oxidation state?

No, Chromium only has 6 valence electrons (five in $3d$ and one in $4s$), so the maximum number of electrons it can lose is 6.

Q: Why are transition metals able to show variable oxidation states?

The energy difference between the $(n-1)d$ and $ns$ orbitals is very small, allowing electrons from both subshells to participate in bonding.

Question

The common positive oxidation states for an element with atomic number 24, are

Options:

(A) + 2 to + 6

(B) + 1 and + 3 to + 6

(C) + 1 and + 3

(D) + 1 to + 6

Sigma Percentile · Accepted Answer

### The Identity of Element 24

Imagine you are exploring the periodic table, specifically the vibrant world of the $3d$ transition series. The question points us to an element with an atomic number of $24$.

If we count through the series—Scandium, Titanium, Vanadium—we land exactly on **Chromium ($Cr$)**.

Identifying the element is our crucial first step, as the chemical behavior of transition metals is deeply tied to their specific electronic configurations.

### The Exceptional Electronic Configuration

To understand the oxidation states of Chromium, we must dive into its electronic structure.

Normally, following the Aufbau principle, we would expect the configuration to be $[Ar] 4s^2 3d^4$. However, nature loves stability.

A half-filled $d$-subshell is exceptionally stable due to symmetrical electron distribution and maximum exchange energy. Therefore, one electron from the $4s$ orbital jumps to the $3d$ orbital.

This gives Chromium its famous exceptional configuration: **$[Ar] 3d^5 4s^1$**.

### Counting the Valence Electrons

Now, let's look closely at the valence shell.

We have five unpaired electrons residing in the $3d$ subshell and one unpaired electron in the $4s$ subshell.

When we add these up, we find that Chromium has a total of **$6$ valence electrons** available to participate in chemical bonding.

### The Range of Oxidation States

Because Chromium possesses $6$ valence electrons, it can theoretically lose any number of these electrons to form bonds with other elements.

This implies that Chromium can exhibit a wide spectrum of oxidation states, ranging all the way from $+1$ up to $+6$.

However, not all of these states are equally stable or frequently encountered in chemical reactions.

### Pinpointing the Common States

Here is where we must be careful. The question specifically asks for the **common** positive oxidation states.

While the $+1$ state is possible, it is extremely rare and only found in a handful of specialized coordination complexes. It is certainly not considered "common."

The most stable and frequently observed oxidation states for Chromium are $+2$, $+3$, and $+6$.

Therefore, the common range of positive oxidation states is universally accepted as **$+2$ to $+6$**. This perfectly matches our first option, making it the correct answer!

Animated Solution for Chemistry - d and f-Block Elements: The common positive oxidation states for an element with atomic number 24, are

Select Answer:

Visualized Solution

$Z = 24$

$Electronic Configuration$

$Valence Electrons$

$Possible States$

$Common States$

$Stability Insights$

The Sigma Insight: d-block Elements

The Identity of Element 24

The Exceptional Electronic Configuration

Counting the Valence Electrons

The Range of Oxidation States

Pinpointing the Common States

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