From simple queries to complex problems, IDNLearn.com provides reliable answers. Our experts provide timely and accurate responses to help you navigate any topic or issue with confidence.
Sagot :
Certainly! Let's determine the electron configuration for a fluorine (F) atom step-by-step.
1. Determine the Atomic Number:
- Fluorine has an atomic number of 9. This means a neutral fluorine atom has 9 electrons.
2. Electron Configuration:
- Electrons fill atomic orbitals following the Aufbau principle, which states that electrons occupy the lowest energy orbitals first. Additionally, we use the Pauli exclusion principle and Hund's rule.
3. Filling the Orbitals:
- The sequence of orbital energy levels is typically: [tex]\(1s, 2s, 2p, 3s, 3p, \ldots\)[/tex]
- Electrons fill the [tex]\(1s\)[/tex] orbital first:
[tex]\[ 1s^2 \quad (\text{2 electrons in 1s orbital}) \][/tex]
- Next, electrons fill the [tex]\(2s\)[/tex] orbital:
[tex]\[ 2s^2 \quad (\text{2 electrons in 2s orbital}) \][/tex]
- Finally, the remaining electrons fill the [tex]\(2p\)[/tex] orbitals. Since fluorine has 9 electrons in total, we already accounted for 4 electrons (2 in [tex]\(1s\)[/tex] and 2 in [tex]\(2s\)[/tex]), leaving 5 electrons to fill the [tex]\(2p\)[/tex] orbitals:
[tex]\[ 2p^5 \quad (\text{5 electrons in 2p orbitals}) \][/tex]
4. Constructing the Full Configuration:
- Combining all the filled orbitals, the electron configuration for fluorine (F) is:
[tex]\[ 1s^2 2s^2 2p^5 \][/tex]
5. Verification with Given Choices:
- Now let's match this configuration to the given options:
- [tex]\(1s^2 2s^2 2p^4\)[/tex] is incorrect because it accounts for only 8 electrons.
- [tex]\(1s^2 2s^2 2p^6 3s^1\)[/tex] is incorrect because it exceeds 9 electrons (11 electrons total).
- [tex]\(1s^2 2s^2 2p^5\)[/tex] matches our determined configuration and sums to 9 electrons.
- [tex]\(1s^2 2s^2 2p^6 3s^2\)[/tex] is also incorrect as it exceeds 9 electrons (12 electrons total).
Therefore, the correct electron configuration is:
[tex]\[ \boxed{1s^2 2s^2 2p^5} \][/tex]
And the correct option from the given choices is:
[tex]\[ \boxed{3} \][/tex]
So, the electron configuration for fluorine, F, is [tex]\(1s^2 2s^2 2p^5\)[/tex], which corresponds to option 3.
1. Determine the Atomic Number:
- Fluorine has an atomic number of 9. This means a neutral fluorine atom has 9 electrons.
2. Electron Configuration:
- Electrons fill atomic orbitals following the Aufbau principle, which states that electrons occupy the lowest energy orbitals first. Additionally, we use the Pauli exclusion principle and Hund's rule.
3. Filling the Orbitals:
- The sequence of orbital energy levels is typically: [tex]\(1s, 2s, 2p, 3s, 3p, \ldots\)[/tex]
- Electrons fill the [tex]\(1s\)[/tex] orbital first:
[tex]\[ 1s^2 \quad (\text{2 electrons in 1s orbital}) \][/tex]
- Next, electrons fill the [tex]\(2s\)[/tex] orbital:
[tex]\[ 2s^2 \quad (\text{2 electrons in 2s orbital}) \][/tex]
- Finally, the remaining electrons fill the [tex]\(2p\)[/tex] orbitals. Since fluorine has 9 electrons in total, we already accounted for 4 electrons (2 in [tex]\(1s\)[/tex] and 2 in [tex]\(2s\)[/tex]), leaving 5 electrons to fill the [tex]\(2p\)[/tex] orbitals:
[tex]\[ 2p^5 \quad (\text{5 electrons in 2p orbitals}) \][/tex]
4. Constructing the Full Configuration:
- Combining all the filled orbitals, the electron configuration for fluorine (F) is:
[tex]\[ 1s^2 2s^2 2p^5 \][/tex]
5. Verification with Given Choices:
- Now let's match this configuration to the given options:
- [tex]\(1s^2 2s^2 2p^4\)[/tex] is incorrect because it accounts for only 8 electrons.
- [tex]\(1s^2 2s^2 2p^6 3s^1\)[/tex] is incorrect because it exceeds 9 electrons (11 electrons total).
- [tex]\(1s^2 2s^2 2p^5\)[/tex] matches our determined configuration and sums to 9 electrons.
- [tex]\(1s^2 2s^2 2p^6 3s^2\)[/tex] is also incorrect as it exceeds 9 electrons (12 electrons total).
Therefore, the correct electron configuration is:
[tex]\[ \boxed{1s^2 2s^2 2p^5} \][/tex]
And the correct option from the given choices is:
[tex]\[ \boxed{3} \][/tex]
So, the electron configuration for fluorine, F, is [tex]\(1s^2 2s^2 2p^5\)[/tex], which corresponds to option 3.
Your participation is crucial to us. Keep sharing your knowledge and experiences. Let's create a learning environment that is both enjoyable and beneficial. IDNLearn.com is committed to providing the best answers. Thank you for visiting, and see you next time for more solutions.
