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K+ and Cl- ions are isoelectronic. Which of the statements is not correct?
- a)Both K+ and Cl- ions contain 18 electrons
- b)Both K+ and Cl- ions have same configuration
- c)K+ ion is bigger than Cl- ion in ionic size
- d)Cl- ion is bigger than K+ ion in size
Correct answer is option 'C'. Can you explain this answer?
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K+and Cl- ions are isoelectronic. Which of the statements is not corre...
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K+and Cl- ions are isoelectronic. Which of the statements is not corre...
Explanation:
To understand why statement (c) is incorrect, we need to analyze the electronic configurations and sizes of K+ and Cl- ions.
Electronic Configurations:
K (Potassium) has an atomic number of 19, therefore it has 19 electrons. The electron configuration of K is 1s2 2s2 2p6 3s2 3p6 4s1.
Cl (Chlorine) has an atomic number of 17, therefore it has 17 electrons. The electron configuration of Cl is 1s2 2s2 2p6 3s2 3p5.
When K loses one electron to form K+, it loses its outermost 4s1 electron and its electron configuration becomes 1s2 2s2 2p6 3s2 3p6, which is the same as the noble gas configuration of Argon (Ar).
Cl gains one electron to form Cl-, and its electron configuration becomes 1s2 2s2 2p6 3s2 3p6, which is the same as the noble gas configuration of Argon (Ar).
Therefore, both K+ and Cl- ions have the same electron configuration, which is the configuration of the noble gas Argon. Hence, statement (b) is correct.
Size of Ions:
When an atom loses electrons to become a cation (positive ion), it loses its outermost electrons, resulting in a smaller size compared to the parent atom. In the case of K+, it loses the 4s1 electron, resulting in a smaller size compared to the neutral K atom. Therefore, Cl- is bigger than K+ in size. Hence, statement (d) is correct.
Conclusion:
Based on the analysis of electronic configurations and sizes of K+ and Cl- ions, we can conclude that statement (c) is incorrect. K+ ion is smaller than Cl- ion in size, and both ions have the same electron configuration.
To understand why statement (c) is incorrect, we need to analyze the electronic configurations and sizes of K+ and Cl- ions.
Electronic Configurations:
K (Potassium) has an atomic number of 19, therefore it has 19 electrons. The electron configuration of K is 1s2 2s2 2p6 3s2 3p6 4s1.
Cl (Chlorine) has an atomic number of 17, therefore it has 17 electrons. The electron configuration of Cl is 1s2 2s2 2p6 3s2 3p5.
When K loses one electron to form K+, it loses its outermost 4s1 electron and its electron configuration becomes 1s2 2s2 2p6 3s2 3p6, which is the same as the noble gas configuration of Argon (Ar).
Cl gains one electron to form Cl-, and its electron configuration becomes 1s2 2s2 2p6 3s2 3p6, which is the same as the noble gas configuration of Argon (Ar).
Therefore, both K+ and Cl- ions have the same electron configuration, which is the configuration of the noble gas Argon. Hence, statement (b) is correct.
Size of Ions:
When an atom loses electrons to become a cation (positive ion), it loses its outermost electrons, resulting in a smaller size compared to the parent atom. In the case of K+, it loses the 4s1 electron, resulting in a smaller size compared to the neutral K atom. Therefore, Cl- is bigger than K+ in size. Hence, statement (d) is correct.
Conclusion:
Based on the analysis of electronic configurations and sizes of K+ and Cl- ions, we can conclude that statement (c) is incorrect. K+ ion is smaller than Cl- ion in size, and both ions have the same electron configuration.
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K+and Cl- ions are isoelectronic. Which of the statements is not corre...
Yes cation is smaller than anion
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K+and Cl- ions are isoelectronic. Which of the statements is not correct?a)Both K+ and Cl-ions contain 18 electronsb)Both K+and Cl- ions have same configurationc)K+ion is bigger than Cl-ion in ionic sized)Cl-ion is bigger than K+ion in sizeCorrect answer is option 'C'. Can you explain this answer?
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