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Which is not similar characteristic(s) about the electronic configuration of Be, Mg, Ca:
- a)All the atoms have a pair of s-electrons in their outermost energy level
- b)All the atoms contain a pair of p-electrons in their outermost energy level
- c)All are alkaline earth metals
- d)All are of second group of the periodic table
Correct answer is option 'B'. Can you explain this answer?
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Which is not similar characteristic(s) about the electronic configurat...
Bcz these three compounds have outer most electron i s orbital so the ans is B Is correct
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Which is not similar characteristic(s) about the electronic configurat...
Explanation:
The electronic configuration of an atom refers to the distribution of electrons in its energy levels or shells. It provides important information about the chemical behavior and properties of an element.
Be (Beryllium):
- Atomic number: 4
- Electronic configuration: 1s² 2s²
- Beryllium belongs to the alkaline earth metals group (Group 2) in the periodic table.
Mg (Magnesium):
- Atomic number: 12
- Electronic configuration: 1s² 2s² 2p⁶ 3s²
- Magnesium also belongs to the alkaline earth metals group (Group 2) in the periodic table.
Ca (Calcium):
- Atomic number: 20
- Electronic configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
- Calcium is also a member of the alkaline earth metals group (Group 2) in the periodic table.
Characteristics of the electronic configuration:
All the atoms have a pair of s-electrons in their outermost energy level:
- This is true for all three elements (Be, Mg, Ca). In their respective electronic configurations, the outermost energy level is the s-subshell, which contains two electrons.
All the atoms contain a pair of p-electrons in their outermost energy level:
- This statement is not true for any of the elements. None of the elements (Be, Mg, Ca) have p-electrons in their outermost energy level. In their electronic configurations, the p-subshell is either completely filled (Mg and Ca) or not occupied at all (Be).
All are alkaline earth metals:
- This statement is true for all three elements (Be, Mg, Ca). They all belong to the alkaline earth metals group (Group 2) in the periodic table.
All are of the second group of the periodic table:
- This statement is also true for all three elements (Be, Mg, Ca). They all belong to Group 2, which is the second group of the periodic table.
Conclusion:
The characteristic that is not similar among Be, Mg, and Ca is that they do not all contain a pair of p-electrons in their outermost energy level. While Be and Ca have completely filled p-subshells, Mg does not have any p-electrons in its outermost energy level.
The electronic configuration of an atom refers to the distribution of electrons in its energy levels or shells. It provides important information about the chemical behavior and properties of an element.
Be (Beryllium):
- Atomic number: 4
- Electronic configuration: 1s² 2s²
- Beryllium belongs to the alkaline earth metals group (Group 2) in the periodic table.
Mg (Magnesium):
- Atomic number: 12
- Electronic configuration: 1s² 2s² 2p⁶ 3s²
- Magnesium also belongs to the alkaline earth metals group (Group 2) in the periodic table.
Ca (Calcium):
- Atomic number: 20
- Electronic configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s²
- Calcium is also a member of the alkaline earth metals group (Group 2) in the periodic table.
Characteristics of the electronic configuration:
All the atoms have a pair of s-electrons in their outermost energy level:
- This is true for all three elements (Be, Mg, Ca). In their respective electronic configurations, the outermost energy level is the s-subshell, which contains two electrons.
All the atoms contain a pair of p-electrons in their outermost energy level:
- This statement is not true for any of the elements. None of the elements (Be, Mg, Ca) have p-electrons in their outermost energy level. In their electronic configurations, the p-subshell is either completely filled (Mg and Ca) or not occupied at all (Be).
All are alkaline earth metals:
- This statement is true for all three elements (Be, Mg, Ca). They all belong to the alkaline earth metals group (Group 2) in the periodic table.
All are of the second group of the periodic table:
- This statement is also true for all three elements (Be, Mg, Ca). They all belong to Group 2, which is the second group of the periodic table.
Conclusion:
The characteristic that is not similar among Be, Mg, and Ca is that they do not all contain a pair of p-electrons in their outermost energy level. While Be and Ca have completely filled p-subshells, Mg does not have any p-electrons in its outermost energy level.
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Which is not similar characteristic(s) about the electronic configuration of Be, Mg, Ca:a)All the atoms have a pair of s-electrons in their outermost energy levelb)All the atoms contain a pair of p-electrons in their outermost energy levelc)All are alkaline earth metalsd)All are of second group of the periodic tableCorrect answer is option 'B'. Can you explain this answer?
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