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3 years ago

Why isn't hydrogen considered an alkali metal ?

2 answers:

7 0

Hydrogen is a non-metal, it is one of the two elements on the periodic table that only need two valence electrons to be stable. Hydrogen doesn't share many properties with the other Alkali Metals. It has a much higher electronegativity, doesn't form ionic bonds, doesn't react with the same things that the other elements in group one do (like water.) The only reason hydrogen is place there is because it has one valence electrons like all the other alkali metals and there is not where else to place hydrogen, because it doesn't really fit in with any group.

Maurinko [17]3 years ago

4 0

Hydrogen isn't classified as an alkali metal because it exhibits several properties that are not found in the alkali metal group, including the tendency to be found as a diatomic molecule, a tendency to form weak bonds with other bound hydrogen atoms nearby, weak electromagnetism, a low activity series placement, and the tendency to be found as a gas. Because of all this, it's impossible to classify it with any group, although it does seem to be closest to nonmetals.

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Answer:

The standard potential, E cell, for this galvanic cell is 0.5670V

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2 years ago

Calculate for the following electrochemical cell at 25°C, Pt H2(g) (1.0 atm) H (0.010 M || Ag (0.020 M) Ag if E (H) - +0.000 V a

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Solution :

The values of standard reduction electrode potential of the cell are:

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From the cell representation we conclude that, the hydrogen (H) undergoes oxidation by loss of electrons and thus act as anode. Silver (Ag) undergoes reduction by gain of electrons and thus act as cathode.

The half reaction will be:

Reaction at anode (oxidation) : $H_2\rightarrow 2H^{+}+2e^-$

Reaction at cathode (reduction) : $Ag^{+}+1e^-\rightarrow Ag$

The balanced cell reaction will be,

$H_2+2Ag^{+}\rightarrow 2H^{+}+2Ag$

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$E^o_{cell}=E^o_{cathode}-E^o_{anode}$

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Therefore, the standard cell potential will be +0.799 V

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3 years ago

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Answer:

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3 years ago

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