Sodium has the lowest oxidation potential in alkali metals. Hence it is the weakest reducing agent among alkali metals. Low ionization energy should be present for the element to act as a reducing agent. Alkali metals have low ionization energy thus making them a strong reducing agent.
So, the correct option is (B): Na.
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The Correct Answer is (B)
The weakest reducing agent is copper. It can be used in:
The Correct Answer is (B)
Group 1 elements of the periodic table are known as Alkali metals. They are strong reducing agents. This is due to the single valence electron in the valence shell. The elements can easily lose their valence electron to acquire the noble gas configuration.
Reason for the alkali metal to act as a strong reducing agent.
Reducing agents: The elements that themselves get oxidized are called reducing agents. Due to the smaller nuclear charge and low ionization potential, they have a tendency to lose the electron easily. Thus making alkali metals strong reducing agents. As we go down from Li to Cs, the ionization potential decreases, and therefore the reducing power decreases. On the other hand, the hydration enthalpy of Sodium is the lowest thus making it the weakest reducing agent. Hydration enthalpy is the amount of energy released when one mole of ions is hydrated.
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Related Concepts | ||
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Redox reaction | Valence shell | Atom |
Atomic mass of elements | Protons | Electrons |
Given below are two statements.
In the light of the above statements, choose the correct answer from the options given below:
Given below are two statements:
Statement I: Nitrogen forms oxides with +1 to +5 oxidation states due to the formation of $\mathrm{p} \pi-\mathrm{p} \pi$ bond with oxygen.
Statement II: Nitrogen does not form halides with +5 oxidation state due to the absence of d-orbital in it.
In the light of the above statements, choose the correct answer from the options given below:
Given below are the pairs of group 13 elements showing their relation in terms of atomic radius. $(\mathrm{B}<\mathrm{Al}),(\mathrm{Al}<\mathrm{Ga}),(\mathrm{Ga}<\mathrm{In})$ and $(\mathrm{In}<\mathrm{Tl})$ Identify the elements present in the incorrect pair and in that pair find out the element (X) that has higher ionic radius $\left(\mathrm{M}^{3+}\right)$ than the other one. The atomic number of the element (X) is
Match List-I with List-II: List-I