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The element with the electronic configuration as $\left[ {{\rm{Ar}}} \right]3{d^{10}}4{s^2}4{p^3}$ represents a

A.RAMA NAGESWARARAO · Accepted Answer

## CORE INFORMATION
✓ **Answer**: C
## CONCEPT FRAMEWORK
	**Primary Concept**: Determining element type based on its electronic configuration and position in the periodic table.
	**Related Topics**: Electronic configuration, valence electrons, periodic trends, metals, non-metals, metalloids.
	**Prerequisites**: Knowledge of the Aufbau principle, Hund's rule, and the organization of the periodic table.
## SOLUTION PATHWAY
**Given Information**:
	Electronic configuration: [Ar]3d¹⁰4s²4p³
**Method & Steps**:
	1. **Identify the element's valence electrons:** The valence electrons are the electrons in the outermost shell (n=4 in this case), which are 4s²4p³. This gives a total of 5 valence electrons.
		Reasoning: The outermost shell electrons determine chemical properties and the group the element belongs to.
	2. **Determine the element's group:** The element is in the p-block (4p electrons) and has 5 valence electrons, which means it belongs to Group 15 (also known as Group 5A or the pnictogens).
		Reasoning: Elements in the same group have similar chemical properties due to the same number of valence electrons.
	3. **Identify the element's type:** Elements in Group 15 are typically non-metals or metalloids. Given that the element in question is in Period 4, it is Arsenic (As), a metalloid. Metalloids have intermediate properties between metals and non-metals.
		Reasoning: Metalloids are located along the staircase line in the periodic table and exhibit properties of both metals and non-metals.
	4. **Conclusion:** The given electronic configuration corresponds to a metalloid.
		Result: The element is a metalloid.
 ## OPTION ANALYSIS
[A] :x: Metals have a tendency to lose electrons and have fewer valence electrons (typically 1-3). This element has 5 valence electrons.
[B] :x: Non-metals tend to gain electrons and have more valence electrons (typically 5-7), however, this elements is a metalloid.
[C] ✓: Metalloids have intermediate properties and can be found in Group 15, and have both non-metal and metal properties.
[D] :x: Transition elements have partially filled d orbitals. This element has a completely filled d orbital (3d¹⁰) and its valence electrons are in the s and p orbitals.
 ## LEARNING AIDS
	**Common Mistakes**:
		1. **Misidentifying the valence shell:** Be sure to identify the outermost shell (highest n value) when determining valence electrons.
		2. **Confusing transition elements and p-block elements:** Remember that transition elements have partially filled d orbitals, not filled ones.
	**Quick Tips**:
		1. **Memorize the location of metalloids:** They are located along the staircase line in the periodic table.
		2. **Know the trends in valence electrons:** Metals generally have fewer valence electrons, non-metals have more, and metalloids are in between.

A.RAMA NAGESWARARAO · Answer

Metal

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Non-metal

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The correct Option is "Metalloid"

A.RAMA NAGESWARARAO · Answer

Transition element

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