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Question 1 A) Use the periodic table to answer the question. An illustration shows the periodic table of elements. The elements...Question
Question 4
A)
Use the periodic table to answer the question.
An illustration shows the periodic table of elements. The elements in the periodic table are arranged in groups (columns numbered 1 through 18) and periods (rows numbered 1 through 7) such that the atomic number increases along a period from left to right. The elements are divided into the following categories: · Alkali metals · Alkaline earth metals · Transition metals · Post-transition metals · Lanthanides · Actinides · Metalloids · Nonmetals · Noble gases · Unknown The elements are also classified on the basis of their physical states as follows: · Solid · Liquid · Gas · Unknown The element sulfur is enlarged with the following properties. · Chemical symbol: S · Name: Sulfur · Atomic Number: 16 · Atomic mass: 32.06 · Common oxidation states: 6, 4, 2, negative 2 · Electronegativity: 2.58 · Ionization energies: 999.589 · Electron configuration: [Ne] 3s2 3p4
Based on patterns in the periodic table, which ion has a stable valence electron configuration?
(1 point)
Responses
potassium (K) with a 1+
charge
potassium (K) with a 1 raised to the plus power charge
fluorine (F) with a 1+
charge
fluorine (F) with a 1 raised to the plus power charge
magnesium (Mg) with a 1−
charge
magnesium (Mg) with a 1 raised to the negative power charge
sulfur (S) with a 1−
charge
sulfur (S) with a 1 raised to the negative power charge
A)
Use the periodic table to answer the question.
An illustration shows the periodic table of elements. The elements in the periodic table are arranged in groups (columns numbered 1 through 18) and periods (rows numbered 1 through 7) such that the atomic number increases along a period from left to right. The elements are divided into the following categories: · Alkali metals · Alkaline earth metals · Transition metals · Post-transition metals · Lanthanides · Actinides · Metalloids · Nonmetals · Noble gases · Unknown The elements are also classified on the basis of their physical states as follows: · Solid · Liquid · Gas · Unknown The element sulfur is enlarged with the following properties. · Chemical symbol: S · Name: Sulfur · Atomic Number: 16 · Atomic mass: 32.06 · Common oxidation states: 6, 4, 2, negative 2 · Electronegativity: 2.58 · Ionization energies: 999.589 · Electron configuration: [Ne] 3s2 3p4
Based on patterns in the periodic table, which ion has a stable valence electron configuration?
(1 point)
Responses
potassium (K) with a 1+
charge
potassium (K) with a 1 raised to the plus power charge
fluorine (F) with a 1+
charge
fluorine (F) with a 1 raised to the plus power charge
magnesium (Mg) with a 1−
charge
magnesium (Mg) with a 1 raised to the negative power charge
sulfur (S) with a 1−
charge
sulfur (S) with a 1 raised to the negative power charge
Answers
There are no human answers yet.
Answered by
GPT-4o mini
To determine which ion has a stable valence electron configuration, we should refer to the concept of achieving a full outer shell of electrons, which is typically associated with having eight electrons in the outer shell (an octet) for main group elements.
1. **Potassium (K)**: Potassium has an atomic number of 19 and has the electron configuration of [Ar] 4s¹. When it loses one electron to form a \( K^+ \) ion, it achieves the electron configuration of Argon, which has a complete outer shell.
2. **Fluorine (F)**: Fluorine has an atomic number of 9 and an electron configuration of [He] 2s² 2p⁵. When it gains one electron to form a \( F^- \) ion, it achieves the electron configuration of Neon, which also has a complete outer shell.
3. **Magnesium (Mg)**: Magnesium has an atomic number of 12, with an electron configuration of [Ne] 3s². When it loses two electrons to form a \( Mg^{2+} \) ion, it achieves the electron configuration of Neon, which is stable.
4. **Sulfur (S)**: Sulfur has an atomic number of 16, with an electron configuration of [Ne] 3s² 3p⁴. When it gains two electrons to form a \( S^{2-} \) ion, it achieves the electron configuration of Argon, which is also stable.
Among the provided options, both potassium (K) with a \( 1+ \) charge and fluorine (F) with a \( 1- \) charge form ions with stable configurations. However, the question requires the identification of a single correct answer based on the context of achieving stable configuration via gaining or losing electrons.
The best final answer to the question, particularly focusing on the options you provided, is:
- **Fluorine (F) with a 1− charge.**
Fluorine achieves a stable configuration by gaining one electron (gaining an electron makes it a \( F^- \) ion), reaching a noble gas configuration (Neon), thereby satisfying the conditions for stability in the periodic table context.
1. **Potassium (K)**: Potassium has an atomic number of 19 and has the electron configuration of [Ar] 4s¹. When it loses one electron to form a \( K^+ \) ion, it achieves the electron configuration of Argon, which has a complete outer shell.
2. **Fluorine (F)**: Fluorine has an atomic number of 9 and an electron configuration of [He] 2s² 2p⁵. When it gains one electron to form a \( F^- \) ion, it achieves the electron configuration of Neon, which also has a complete outer shell.
3. **Magnesium (Mg)**: Magnesium has an atomic number of 12, with an electron configuration of [Ne] 3s². When it loses two electrons to form a \( Mg^{2+} \) ion, it achieves the electron configuration of Neon, which is stable.
4. **Sulfur (S)**: Sulfur has an atomic number of 16, with an electron configuration of [Ne] 3s² 3p⁴. When it gains two electrons to form a \( S^{2-} \) ion, it achieves the electron configuration of Argon, which is also stable.
Among the provided options, both potassium (K) with a \( 1+ \) charge and fluorine (F) with a \( 1- \) charge form ions with stable configurations. However, the question requires the identification of a single correct answer based on the context of achieving stable configuration via gaining or losing electrons.
The best final answer to the question, particularly focusing on the options you provided, is:
- **Fluorine (F) with a 1− charge.**
Fluorine achieves a stable configuration by gaining one electron (gaining an electron makes it a \( F^- \) ion), reaching a noble gas configuration (Neon), thereby satisfying the conditions for stability in the periodic table context.
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