Connect with knowledgeable individuals and find the best answers at IDNLearn.com. Our platform offers detailed and accurate responses from experts, helping you navigate any topic with confidence.
Sagot :
To solve the question of what [tex]\( X \)[/tex] represents in the given electron configuration for an atom with 14 electrons, let's follow a step-by-step process:
1. Identify Total Electrons Represented:
- The atom in question has a total of 14 electrons.
2. Analyze the Provided Configuration:
- The given partial electron configuration is [tex]\( 1s^2 2s^2 2p^6 3s^2 \)[/tex].
- We need to determine how many electrons are accounted for in this partial configuration.
3. Count the Electrons in Each Sublevel:
- [tex]\( 1s^2 \)[/tex]: This means there are 2 electrons in the 1s orbital.
- [tex]\( 2s^2 \)[/tex]: This means there are 2 electrons in the 2s orbital.
- [tex]\( 2p^6 \)[/tex]: This means there are 6 electrons in the 2p orbitals.
- [tex]\( 3s^2 \)[/tex]: This means there are 2 electrons in the 3s orbital.
4. Sum the Electrons:
- Total electrons in the provided configuration: [tex]\( 2 (1s^2) + 2 (2s^2) + 6 (2p^6) + 2 (3s^2) = 12 \)[/tex] electrons.
5. Determine Remaining Electrons:
- The atom has a total of 14 electrons, and the partial configuration accounts for 12 of them.
- Therefore, there are [tex]\( 14 - 12 = 2 \)[/tex] electrons yet to be placed in an appropriate orbital.
6. Identify Next Available Energy Level:
- The next available orbitals after [tex]\( 3s \)[/tex] are the [tex]\( 3p \)[/tex] orbitals because the [tex]\( p \)[/tex] orbitals in any given principal energy level come after the [tex]\( s \)[/tex] orbital.
7. Place the Remaining Electrons:
- The 2 remaining electrons will occupy the [tex]\( 3p \)[/tex] orbital.
8. Determine [tex]\( X \)[/tex] in the Configuration:
- Therefore, [tex]\( X = 3p^2 \)[/tex].
9. Match [tex]\( X \)[/tex] with the Given Options:
- Among the provided options:
- [tex]\( 2d^2 \)[/tex] is not possible because [tex]\( d \)[/tex] orbitals start from the 3rd principal energy level.
- [tex]\( 3s^2 \)[/tex] is already occupied in the given configuration.
- [tex]\( 3p^2 \)[/tex] matches our requirement perfectly.
- [tex]\( 4s^2 \)[/tex] would be the next level after [tex]\( 3p \)[/tex] and not appropriate here.
Therefore, [tex]\( X \)[/tex] represents [tex]\( 3p^2 \)[/tex], corresponding to the third multiple-choice option:
[tex]\[ \boxed{3p^2} \][/tex]
Thus, the correct multiple-choice option is:
[tex]\[ \boxed{3} \][/tex]
1. Identify Total Electrons Represented:
- The atom in question has a total of 14 electrons.
2. Analyze the Provided Configuration:
- The given partial electron configuration is [tex]\( 1s^2 2s^2 2p^6 3s^2 \)[/tex].
- We need to determine how many electrons are accounted for in this partial configuration.
3. Count the Electrons in Each Sublevel:
- [tex]\( 1s^2 \)[/tex]: This means there are 2 electrons in the 1s orbital.
- [tex]\( 2s^2 \)[/tex]: This means there are 2 electrons in the 2s orbital.
- [tex]\( 2p^6 \)[/tex]: This means there are 6 electrons in the 2p orbitals.
- [tex]\( 3s^2 \)[/tex]: This means there are 2 electrons in the 3s orbital.
4. Sum the Electrons:
- Total electrons in the provided configuration: [tex]\( 2 (1s^2) + 2 (2s^2) + 6 (2p^6) + 2 (3s^2) = 12 \)[/tex] electrons.
5. Determine Remaining Electrons:
- The atom has a total of 14 electrons, and the partial configuration accounts for 12 of them.
- Therefore, there are [tex]\( 14 - 12 = 2 \)[/tex] electrons yet to be placed in an appropriate orbital.
6. Identify Next Available Energy Level:
- The next available orbitals after [tex]\( 3s \)[/tex] are the [tex]\( 3p \)[/tex] orbitals because the [tex]\( p \)[/tex] orbitals in any given principal energy level come after the [tex]\( s \)[/tex] orbital.
7. Place the Remaining Electrons:
- The 2 remaining electrons will occupy the [tex]\( 3p \)[/tex] orbital.
8. Determine [tex]\( X \)[/tex] in the Configuration:
- Therefore, [tex]\( X = 3p^2 \)[/tex].
9. Match [tex]\( X \)[/tex] with the Given Options:
- Among the provided options:
- [tex]\( 2d^2 \)[/tex] is not possible because [tex]\( d \)[/tex] orbitals start from the 3rd principal energy level.
- [tex]\( 3s^2 \)[/tex] is already occupied in the given configuration.
- [tex]\( 3p^2 \)[/tex] matches our requirement perfectly.
- [tex]\( 4s^2 \)[/tex] would be the next level after [tex]\( 3p \)[/tex] and not appropriate here.
Therefore, [tex]\( X \)[/tex] represents [tex]\( 3p^2 \)[/tex], corresponding to the third multiple-choice option:
[tex]\[ \boxed{3p^2} \][/tex]
Thus, the correct multiple-choice option is:
[tex]\[ \boxed{3} \][/tex]
Thank you for using this platform to share and learn. Don't hesitate to keep asking and answering. We value every contribution you make. For dependable answers, trust IDNLearn.com. Thank you for visiting, and we look forward to assisting you again.
