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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 cannot forms a large number of ionic compounds by losing an 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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Verified Answer
Which of the following statements are not true for hydrogen?a)It can l...
The electronic configuration of the Hydrogen atom is 1s1.
It has one electron in the outermost shell. It exists as a diatomic molecule (H2) by sharing its' electron with other hydrogen atom.
It cannot form ionic compounds because it cannot donate its' electron and can only form covalent compounds by sharing the electron. It cannot lose an electron to form a cation because the hydrogen atom cannot exist after losing an electron.
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Which of the following statements are not true for hydrogen?a)It can l...
Explanation:
Statement a: It can lose an electron to form a cation which can freely exist
This statement is not true for hydrogen.
Explanation:
- Hydrogen is the first element in the periodic table and has one electron in its only shell.
- In its ground state, hydrogen atom has one electron in its 1s orbital.
- To lose an electron and form a cation, an atom must have more than one electron in its outermost shell.
- Since hydrogen has only one electron, it cannot lose an electron to form a cation with a complete outer shell.
- Therefore, hydrogen does not form cations that can freely exist.
Statement b: It cannot forms a large number of ionic compounds by losing an electron.
This statement is true for hydrogen.
Explanation:
- Hydrogen does not readily form ionic compounds by losing an electron.
- It is more likely to form covalent compounds by sharing electrons with other atoms.
- Hydrogen typically forms covalent bonds with other elements, such as in water (H2O) and methane (CH4).
Statement c: It has one electron in the outermost shell.
This statement is true for hydrogen.
Explanation:
- Hydrogen has one electron in its only shell, which is the 1s orbital.
- The 1s orbital is the outermost shell for hydrogen, as it does not have any more shells beyond this.
Statement d: It exists as diatomic molecule.
This statement is true for hydrogen.
Explanation:
- Hydrogen exists as a diatomic molecule, meaning it forms a covalent bond with another hydrogen atom to form H2.
- This is because each hydrogen atom wants to have a full outer shell, which consists of two electrons.
- By sharing one electron each, the two hydrogen atoms can achieve a stable electron configuration and form a diatomic molecule.
Statement a: It can lose an electron to form a cation which can freely exist
This statement is not true for hydrogen.
Explanation:
- Hydrogen is the first element in the periodic table and has one electron in its only shell.
- In its ground state, hydrogen atom has one electron in its 1s orbital.
- To lose an electron and form a cation, an atom must have more than one electron in its outermost shell.
- Since hydrogen has only one electron, it cannot lose an electron to form a cation with a complete outer shell.
- Therefore, hydrogen does not form cations that can freely exist.
Statement b: It cannot forms a large number of ionic compounds by losing an electron.
This statement is true for hydrogen.
Explanation:
- Hydrogen does not readily form ionic compounds by losing an electron.
- It is more likely to form covalent compounds by sharing electrons with other atoms.
- Hydrogen typically forms covalent bonds with other elements, such as in water (H2O) and methane (CH4).
Statement c: It has one electron in the outermost shell.
This statement is true for hydrogen.
Explanation:
- Hydrogen has one electron in its only shell, which is the 1s orbital.
- The 1s orbital is the outermost shell for hydrogen, as it does not have any more shells beyond this.
Statement d: It exists as diatomic molecule.
This statement is true for hydrogen.
Explanation:
- Hydrogen exists as a diatomic molecule, meaning it forms a covalent bond with another hydrogen atom to form H2.
- This is because each hydrogen atom wants to have a full outer shell, which consists of two electrons.
- By sharing one electron each, the two hydrogen atoms can achieve a stable electron configuration and form a diatomic molecule.
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Community Answer
Which of the following statements are not true for hydrogen?a)It can l...
The electronic configuration of the Hydrogen atom is 1s1.
It has one electron in the outermost shell. It exists as a diatomic molecule (H2) by sharing its' electron with other hydrogen atom.
It cannot form ionic compounds because it cannot donate its' electron and can only form covalent compounds by sharing the electron. It cannot lose an electron to form a cation because the hydrogen atom cannot exist after losing an electron.
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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 cannot forms a large number of ionic compounds by losing anelectrons.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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