In the long or modern form of the periodic table, the element in the periodic table have been divided into four blocks, `s-p-d`-and `f`-. Each period begins with the filling of new energy shell. Two series of `f`-block elements are placed at the bottom of the periodic table.
The element with `Z=113` has been discovered. Its block, group number, period and ourershell electronic configuration are

Options

A. `s`-block, group `2`, period `7,7s^(2)`
B. `p`-block, group `13`, period `7,7s^(2)7p^(1)`
C. `p`-block, group, 13`, period 6,6s^(2)6p^(1)`
D. `d`-block, group `12`,period `6,5d^(10), 6s^(2)`

Explanation

To determine the block, group number, period, and outer shell electronic configuration of the element with atomic number \( Z = 113 \), we can follow these steps:

### Step 1: Write the electronic configuration
The electronic configuration for the element with \( Z = 113 \) can be derived by filling the orbitals according to the Aufbau principle. The complete electronic configuration is:
\[ \text{Rn} \, 5f^{14} \, 6d^{10} \, 7s^2 \, 7p^1 \]

### Step 2: Identify the block
In the electronic configuration, the last electron enters the \( p \) subshell (7p). Therefore, this element belongs to the **p-block** of the periodic table.

### Step 3: Determine the group number
For p-block elements, the group number can be determined by the number of electrons in the outermost \( p \) subshell. Since there is 1 electron in the \( 7p \) subshell, the group number is:
\[ 13 \]
Thus, the element belongs to **Group 13**.

### Step 4: Identify the period
The highest principal quantum number in the electronic configuration is 7 (from \( 7s^2 \) and \( 7p^1 \)). Therefore, the element is in **Period 7**.

### Step 5: Summarize the findings
- **Block**: p-block
- **Group Number**: 13
- **Period**: 7
- **Outer Shell Electronic Configuration**: \( 7s^2 \, 7p^1 \)

### Final Answer:
- Block: p-block
- Group Number: 13
- Period: 7
- Outer Shell Electronic Configuration: \( 7s^2 \, 7p^1 \)

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