An element with atomic number 107 has recently been discovered. Its block, group number, period and outshell electronic configuration respectively are `:`

Options

A. s−
block, group 2, period 6,6s2
B. p−
block, group 13,period, 5,5s2,5p4
C. d−
block, group 7, period 7,7s2
D. f−
block, group 3, period 6,6s2

Explanation

To determine the block, group number, period, and outer shell electronic configuration of the element with atomic number 107, we can follow these steps:

### Step 1: Identify the nearest noble gas
The atomic number of the element is 107. The nearest noble gas before this atomic number is Radon (Rn), which has an atomic number of 86.

**Hint:** Look for the noble gas with the highest atomic number that is less than the atomic number of the element in question.

### Step 2: Calculate the number of electrons beyond the noble gas
To find the number of electrons that need to be added beyond Radon, we subtract the atomic number of Radon from 107:
\[ 107 - 86 = 21 \]
This means there are 21 electrons to distribute after Radon.

**Hint:** Subtract the atomic number of the nearest noble gas from the atomic number of the element to find the remaining electrons.

### Step 3: Determine the electronic configuration
The remaining 21 electrons will fill the orbitals according to the Aufbau principle. The filling order will be:
- 5f can hold a maximum of 14 electrons (5f14)
- 6d can hold a maximum of 10 electrons (6d5)
- 7s can hold a maximum of 2 electrons (7s2)

Thus, the electronic configuration becomes:
\[ [Rn] \, 5f^{14} \, 6d^{5} \, 7s^{2} \]

**Hint:** Use the order of filling for orbitals (Aufbau principle) to determine how the remaining electrons are distributed.

### Step 4: Identify the block
Since the last electron added is in the d orbital (6d), this element belongs to the d-block of the periodic table.

**Hint:** The block is determined by the subshell that receives the last electron.

### Step 5: Identify the group number
The element is in the 7th period (as it follows Radon, which is in the 6th period) and belongs to group 7, as the outermost electrons are in the 7s and 6d orbitals.

**Hint:** The group number can often be inferred from the outermost electron configuration.

### Step 6: Identify the period
Since Radon is in the 6th period and the next row starts with 7s, the element is in the 7th period.

**Hint:** The period corresponds to the highest principal quantum number (n) in the electron configuration.

### Final Answer
- **Block:** d-block
- **Group Number:** 7
- **Period:** 7
- **Outermost Electronic Configuration:** 7s²

Thus, the element with atomic number 107 has the following characteristics:
- Block: d-block
- Group Number: 7
- Period: 7
- Outermost Electronic Configuration: 7s²