Outer electronic configuration of an element is 4s13d10. The element is expected to be

Options

A. a metal
B. a non-metal
C. an element of 10th group
D. liquid at `2981^@ C`

Answer

To determine the element with the outer electronic configuration of 4s¹3d¹⁰, we can follow these steps:

### Step 1: Identify the outer electronic configuration
The outer electronic configuration given is 4s¹3d¹⁰. This indicates that there is 1 electron in the 4s subshell and 10 electrons in the 3d subshell.

### Step 2: Determine the total number of electrons
To find the atomic number of the element, we need to consider the filled inner shells. The configuration can be broken down as follows:
- The 3d subshell can hold a maximum of 10 electrons (which it does here).
- The 4s subshell has 1 electron.

### Step 3: Fill in the inner shells
The electron configuration preceding the outer shells is:
- 1s² (2 electrons)
- 2s² (2 electrons)
- 2p⁶ (6 electrons)
- 3s² (2 electrons)
- 3p⁶ (6 electrons)

So, the total number of electrons in the filled inner shells is:
2 (from 1s) + 2 (from 2s) + 6 (from 2p) + 2 (from 3s) + 6 (from 3p) = 18 electrons.

### Step 4: Calculate the total atomic number
Now, adding the electrons from the outer configuration:
- 18 (inner shells) + 1 (from 4s) + 10 (from 3d) = 29 electrons.

### Step 5: Identify the element
The atomic number 29 corresponds to Copper (Cu). Therefore, the element with the outer electronic configuration of 4s¹3d¹⁰ is Copper.

### Step 6: Determine the group and block
Copper is located in the d-block of the periodic table, specifically in group 11. It is classified as a transition metal.

### Final Answer
The element is Copper (Cu).

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