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Which of the following statements are not true for hydrogen?
- a)It can lose an electron to form a cation which can freely exist
- b)It forms a large number of ionic compounds by losing two electrons.
- c)It has one electron in the outermost shell.
- d)It exists as diatomic molecule.
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
Which of the following statements are not true for hydrogen?a)It can l...
It can lose an electron to form a cation which cannot freely exist.Generally, it does not form ionic compounds by losing an electron but forms a large number of covalent compounds by sharing electron.
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Which of the following statements are not true for hydrogen?a)It can l...
Explanation:
Hydrogen is the first element in the periodic table and has unique properties that distinguish it from other elements. Let's analyze each statement to determine which one is not true for hydrogen.
a) It can lose an electron to form a cation which can freely exist:
This statement is not true for hydrogen. Hydrogen is located in Group 1A of the periodic table, which means it has one valence electron in its outermost shell. In order to achieve a stable electron configuration, hydrogen tends to gain an electron to form a hydride ion (H-), rather than losing an electron to form a cation. The hydride ion is not stable on its own and requires a suitable counterion to form stable ionic compounds.
b) It forms a large number of ionic compounds by losing two electrons:
This statement is not true for hydrogen. As mentioned earlier, hydrogen tends to gain an electron to form an anion rather than losing two electrons. Losing two electrons would require a significant amount of energy, which is not favorable for hydrogen.
c) It has one electron in the outermost shell:
This statement is true for hydrogen. Hydrogen has one electron in its 1s orbital, which is its outermost shell.
d) It exists as a diatomic molecule:
This statement is true for hydrogen. In its elemental form, hydrogen exists as a diatomic molecule (H2). Each hydrogen atom shares its single electron with the other, forming a stable covalent bond.
Therefore, the correct answer is Option A - "It can lose an electron to form a cation which can freely exist." Hydrogen tends to gain an electron to achieve stability rather than losing an electron to form a cation.
Hydrogen is the first element in the periodic table and has unique properties that distinguish it from other elements. Let's analyze each statement to determine which one is not true for hydrogen.
a) It can lose an electron to form a cation which can freely exist:
This statement is not true for hydrogen. Hydrogen is located in Group 1A of the periodic table, which means it has one valence electron in its outermost shell. In order to achieve a stable electron configuration, hydrogen tends to gain an electron to form a hydride ion (H-), rather than losing an electron to form a cation. The hydride ion is not stable on its own and requires a suitable counterion to form stable ionic compounds.
b) It forms a large number of ionic compounds by losing two electrons:
This statement is not true for hydrogen. As mentioned earlier, hydrogen tends to gain an electron to form an anion rather than losing two electrons. Losing two electrons would require a significant amount of energy, which is not favorable for hydrogen.
c) It has one electron in the outermost shell:
This statement is true for hydrogen. Hydrogen has one electron in its 1s orbital, which is its outermost shell.
d) It exists as a diatomic molecule:
This statement is true for hydrogen. In its elemental form, hydrogen exists as a diatomic molecule (H2). Each hydrogen atom shares its single electron with the other, forming a stable covalent bond.
Therefore, the correct answer is Option A - "It can lose an electron to form a cation which can freely exist." Hydrogen tends to gain an electron to achieve stability rather than losing an electron to form a cation.
Community Answer
Which of the following statements are not true for hydrogen?a)It can l...
How can hydrogen form large no. of compd by losing 2 e whereas it have only 1 e
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Which of the following statements are not true for hydrogen?a)It can lose an electron to form a cation which can freely existb)It forms a large number of ionic compounds by losing two electrons.c)It has one electron in the outermost shell.d)It exists as diatomic molecule.Correct answer is option 'A'. Can you explain this answer?
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