whata the period block and group in which elements with the following electron configuration is located?

a) [Ne] 3s^23p^4
b) [Kr] 4d^105s^25p^2
c) [Xe] 4f^145d^106s^26p^5

a) [Ne] 3s^2, 3p^4 shows (2+4)=6 valence electrons. That is Group VI (O, S, etc.) in the "p-block" (last 6 columns)

b) [Kr] 4d^10, 5s^2, 5p^2 shows (2+2)=4 valence electrons, Group IV (C, Si, etc.) in the "p-block"

(c) [Xe] 4f^14, 5d^10, 6s^2, 6p^5, 7 valence electrons. I will let you figure out the group and block.

for c is it grou VII and p-block?

Let's break down the electron configurations and identify the period, block, and group for each element.

a) [Ne] 3s²3p⁴
To determine the period, we count the number of energy levels, which is 3. Therefore, the element is located in the 3rd period.
The block can be determined based on the last subshell before the configuration. In this case, the last subshell is 3p. So, the element is located in the p-block.
To determine the group, we look at the number of valence electrons, which is 6. Since oxygen (O) also has 6 valence electrons and is located in group 16, this element, with the same number of valence electrons, will also be found in group 16.

b) [Kr] 4d¹⁰5s²5p²
This electron configuration belongs to the element located in the 5th period since there are 5 energy levels.
The block for this element can be determined based on the last subshell, which is 5p, indicating that it is in the p-block.
For the group, we look at the number of valence electrons, which is 2 in this case. The element with 2 valence electrons in the p-block is oxygen (O), which is in group 16.

c) [Xe] 4f¹⁴5d¹⁰6s²6p⁵
This element is in the 6th period since there are 6 energy levels.
The block can be determined from the last subshell before the configuration, which is 6p. Therefore, the element is in the p-block.
To determine the group, we focus on the number of valence electrons, which is 5. Fluorine (F) also has 5 valence electrons and is found in group 17. Thus, this element will also be in group 17.

To find the period, block, and group of an element based on its electron configuration, we need to understand the periodic table.

1. Period: The period of an element corresponds to its energy levels or shells. Each new period starts when a new energy level is filled by electrons. The period is determined by the highest principal quantum number (n) in the electron configuration.

2. Block: The block of an element refers to the type of orbital (s, p, d, f) where the last electron enters. It provides information about the shape and orientation of the electron cloud. The blocks are labeled in the periodic table as s, p, d, and f.

3. Group: The group or family of an element gives us information about the number of valence electrons and the chemical behavior. Elements in the same group have similar properties, as they have the same number of valence electrons.

Now let's determine the period, block, and group for each electron configuration:

a) [Ne] 3s²3p⁴
For this electron configuration, the highest principal quantum number is 3. Hence, the element is in the third period.

The last electron enters the p orbital, so it belongs to the p-block elements.

To determine the group, we need to know the number of valence electrons. In this case, there are 6 valence electrons (2 from the 3s orbital and 4 from the 3p orbital). Based on this, the element is in Group 16 (also known as Group VIA or Group 6A).

b) [Kr] 4d¹⁰5s²5p²
The highest principal quantum number is 4, indicating that the element is in the fourth period.

The last electron enters the p orbital. So, it belongs to the p-block elements.

Counting the number of valence electrons, we find that there are 4 (2 from the 5s orbital and 2 from the 5p orbital), which places the element in Group 14 (also known as Group IVA or Group 4A).

c) [Xe] 4f¹⁴5d¹⁰6s²6p⁵
The highest principal quantum number is 6, indicating that the element is in the sixth period.

The last electron enters the p orbital. So, it belongs to the p-block elements.

Counting the number of valence electrons, we find there are 7 (2 from the 6s orbital and 5 from the 6p orbital), which places the element in Group 17 (also known as Group VIIA or Group 7A).

In summary:
a) [Ne] 3s²3p⁴ is in the 3rd period, p-block, and Group 16.
b) [Kr] 4d¹⁰5s²5p² is in the 4th period, p-block, and Group 14.
c) [Xe] 4f¹⁴5d¹⁰6s²6p⁵ is in the 6th period, p-block, and Group 17.