The Electronic Configuration of an Element 'X' is 2,8,2. To which group and period of the modern periodic table does 'X' belong. State it's valency and justify your answer in each case?

Question

Answer

Element Name - Magnesium.

Group Number - 2.

Period - 3.

Valency - 2.

Answer

The electronic configuration is
K L M
2 8 2
So the total is 12.
Magnesium has the atomic number 12.
So it belongs to
Group ---> 2
Period ---> 3
Valency ---> 2( because its outermost shell contain 2 electrons).

Answer

X is MagnesiumGroup is 2Period is 3Valency is 2 vo no of electron present in outermost shell Is 2..

Answer

Element X=magnesium which vlency is 2

Answer

Group-2
period-3

Answer

The electronic configuration of an element 'X' is 2,8,2. To determine which group and period of the modern periodic table 'X' belongs to, we need to analyze the electronic configuration and understand the periodic trends.

Electronic Configuration:
The electronic configuration of 'X' is 2,8,2. This configuration tells us that the element 'X' has 2 electrons in the first energy level (1s), 8 electrons in the second energy level (2s and 2p), and 2 electrons in the third energy level (3s).

Group and Period:
To identify the group of element 'X', we look at the number of valence electrons. Valence electrons are the outermost electrons in an atom, and they determine the chemical properties and reactivity of an element.

In this case, 'X' has 2 valence electrons in the outermost energy level (3s). The group number corresponds to the number of valence electrons. Therefore, 'X' belongs to Group 2 of the periodic table.

To determine the period of element 'X', we count the total number of energy levels. In this case, 'X' has 3 energy levels, so it belongs to Period 3.

Valency:
Valency is the combining capacity of an element, and it is determined by the number of valence electrons. The valency of an element can be predicted by its group number.

In this case, since 'X' belongs to Group 2, it has 2 valence electrons. Elements in Group 2 tend to lose these 2 valence electrons to achieve a stable electron configuration, resulting in a valency of +2. Therefore, the valency of element 'X' is +2.

Justification:
The justification for 'X' belonging to Group 2 and Period 3 is based on the electronic configuration and the periodic trends. Elements in the same group have similar chemical properties due to the same number of valence electrons, while elements in the same period have the same number of energy levels.

The electronic configuration of 'X' shows that it has 2 valence electrons in the outermost energy level, which corresponds to Group 2. Additionally, the element has 3 energy levels, indicating its position in Period 3.

The valency of +2 is justified by the tendency of Group 2 elements to lose 2 valence electrons and achieve a stable electron configuration. This loss of electrons results in a positive charge of +2, making 'X' highly reactive with elements that can accept these 2 electrons.

In conclusion, based on the electronic configuration, element 'X' belongs to Group 2 and Period 3 of the modern periodic table. Its valency is +2, as it tends to lose 2 valence electrons to achieve stability.

Similar Class 10 Doubts

An element belongs to 3rd period and second group of the periodic table

Write the number of periods and groups present in the modern periodic table. State the changes in valency and metallic character of elements as we move from left to right in a period. Also state the changes, if any, in the valency and atomic size of elements as we go down a group ?

How does the electronic configuration of an atom of an element relate to its position in the modern periodic table? Explain with one example.

Choose from the following Ca, li, na, ne

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