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In alkali metals down the group basicity increase so why NAOH is more basic than KOH?
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Natalie Feldman
In alkali metals down the group basicity increase so why NAOH is more basic than KOH?
How do the elements of group 2A differ from alkali metals?
The chief differences are: They are harder and denser; they are less reactive (though still very reactive in absolute terms); they show a +2 valence instead of +1.
How do the elements of group 2A differ from alkali metals?
The chief differences are: They are harder and denser; they are less reactive (though still very reactive in absolute terms); they show a +2 valence instead of +1.
Technically there is no basicity for bases it is acidity.
I think you mean basic character.
Basic character increases down the group because many metallic characters like electropositivity, increases down the group.
Atomic radius too increases down the group making electronic transfer easier.
Ionisation enthalpy decreases down the group having favouring effect.
As a combined effect, going down the group first makes preparing the base itself easier and also gives us a more polar molecule of the base so it is easier for the base to dissociate and be more basic in nature.
Technically there is no basicity for bases it is acidity.
I think you mean basic character.
Basic character increases down the group because many metallic characters like electropositivity, increases down the group.
Atomic radius too increases down the group making electronic transfer easier.
Ionisation enthalpy decreases down the group having favouring effect.
As a combined effect, going down the group first makes preparing the base itself easier and also gives us a more polar molecule of the base so it is easier for the base to dissociate and be more basic in nature.
When the group 1 metals react with water they form hydrogen, the metal cations and hydroxide ions. The production of OH- ions increases the ph thus creating alkaline conditions which is what I assume they derive their name from.
When the group 1 metals react with water they form hydrogen, the metal cations and hydroxide ions. The production of OH- ions increases the ph thus creating alkaline conditions which is what I assume they derive their name from.
Of faijans rule as OH- is smaller ions and Li is too small which makes it more covalent therefore it cant produce oH- completely which tends to make it less basic also its polarising power is more. Whereas in KOh due to a big size diffrence and less polarizing powerit forms ionic bond more comfortabily and is most basic.
I think it is most simple reason u can remember…
And don’t forget to upvote .so i can get that u got it
Of faijans rule as OH- is smaller ions and Li is too small which makes it more covalent therefore it cant produce oH- completely which tends to make it less basic also its polarising power is more. Whereas in KOh due to a big size diffrence and less polarizing powerit forms ionic bond more comfortabily and is most basic.
I think it is most simple reason u can remember…
And don’t forget to upvote .so i can get that u got it
The alkali metals are so called because upon reaction with water they generate free hydroxide; therefore high pH solution. I have no idea what is meant by the “three types of alkali”
The alkali metals are so called because upon reaction with water they generate free hydroxide; therefore high pH solution. I have no idea what is meant by the “three types of alkali”
(and covers LiOH, NaOH, KOH, RbOH, and CsOH). Bottom line is that the order of basicity is:
CsOH > RbOH > KOH > NaOH > LiOH
A rationale for this order is based on the relative electronegativity of the cations. The order of basicity appears to be inversely related to the electronegativity. Thus the more electropositive the more the cation may associate with the OH-, making it less available to act as a base.
(and covers LiOH, NaOH, KOH, RbOH, and CsOH). Bottom line is that the order of basicity is:
CsOH > RbOH > KOH > NaOH > LiOH
A rationale for this order is based on the relative electronegativity of the cations. The order of basicity appears to be inversely related to the electronegativity. Thus the more electropositive the more the cation may associate with the OH-, making it less available to act as a base.
How do the elements of group 2A differ from alkali metals?
The chief differences are:
They are harder and denser; they are less reactive (though still very reactive in absolute terms); they show a +2 valence instead of +1.
How do the elements of group 2A differ from alkali metals?
The chief differences are:
They are harder and denser; they are less reactive (though still very reactive in absolute terms); they show a +2 valence instead of +1.
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It's depending upon hydration enthalpy if hydration enthalpy is greater than lattice enthalpy nitrates soluble in water.
If not substance don't soluble in water.
It's depending upon hydration enthalpy if hydration enthalpy is greater than lattice enthalpy nitrates soluble in water.
If not substance don't soluble in water.
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Ammonia. It’s composed of two nonmetals, hydrogen and nitrogen.
Ammonia. It’s composed of two nonmetals, hydrogen and nitrogen.
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Technically there is no basicity for bases it is acidity.
I think you mean basic character.
Basic character increases down the group because many metallic characters like electropositivity, increases down the group.
Atomic radius too increases down the group making electronic transfer easier.
Ionisation enthalpy decreases down the group having favouring effect.
As a combined effect, going down the group first makes preparing the base itself easier and also gives us a more polar molecule of the base so it is easier for the base to dissociate and be more basic in nature.
Technically there is no basicity for bases it is acidity.
I think you mean basic character.
Basic character increases down the group because many metallic characters like electropositivity, increases down the group.
Atomic radius too increases down the group making electronic transfer easier.
Ionisation enthalpy decreases down the group having favouring effect.
As a combined effect, going down the group first makes preparing the base itself easier and also gives us a more polar molecule of the base so it is easier for the base to dissociate and be more basic in nature.
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When the group 1 metals react with water they form hydrogen, the metal cations and hydroxide ions. The production of OH- ions increases the ph thus creating alkaline conditions which is what I assume they derive their name from.
When the group 1 metals react with water they form hydrogen, the metal cations and hydroxide ions. The production of OH- ions increases the ph thus creating alkaline conditions which is what I assume they derive their name from.
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Most basic is koh and least is LIOH its bcoz
Of faijans rule as OH- is smaller ions and Li is too small which makes it more covalent therefore it cant produce oH- completely which tends to make it less basic also its polarising power is more. Whereas in KOh due to a big size diffrence and less polarizing powerit forms ionic bond more comfortabily and is most basic.
I think it is most simple reason u can remember…
And don’t forget to upvote .so i can get that u got it
Most basic is koh and least is LIOH its bcoz
Of faijans rule as OH- is smaller ions and Li is too small which makes it more covalent therefore it cant produce oH- completely which tends to make it less basic also its polarising power is more. Whereas in KOh due to a big size diffrence and less polarizing powerit forms ionic bond more comfortabily and is most basic.
I think it is most simple reason u can remember…
And don’t forget to upvote .so i can get that u got it
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The alkali metals are so called because upon reaction with water they generate free hydroxide; therefore high pH solution. I have no idea what is meant by the “three types of alkali”
The alkali metals are so called because upon reaction with water they generate free hydroxide; therefore high pH solution. I have no idea what is meant by the “three types of alkali”
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It isn’t.
A nice summary of what is known about these bases and the rest of the alkali metal hydroxides can be found at:
Is LiOH a weaker base than NaOH?
(and covers LiOH, NaOH, KOH, RbOH, and CsOH). Bottom line is that the order of basicity is:
CsOH > RbOH > KOH > NaOH > LiOH
A rationale for this order is based on the relative electronegativity of the cations. The order of basicity appears to be inversely related to the electronegativity. Thus the more electropositive the more the cation may associate with the OH-, making it less available to act as a base.
It isn’t.
A nice summary of what is known about these bases and the rest of the alkali metal hydroxides can be found at:
Is LiOH a weaker base than NaOH?
(and covers LiOH, NaOH, KOH, RbOH, and CsOH). Bottom line is that the order of basicity is:
CsOH > RbOH > KOH > NaOH > LiOH
A rationale for this order is based on the relative electronegativity of the cations. The order of basicity appears to be inversely related to the electronegativity. Thus the more electropositive the more the cation may associate with the OH-, making it less available to act as a base.
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They both do and can do serious damage.
They both do and can do serious damage.
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In bulk form and at ordinary temperatures and pressures, osmium metal does resist attack by all acids and alkalis, including potassium hydroxide.
However, in finely powdered form, osmium reacts with oxygen at elevated temperatures (200–300°C) to produce osmium tetroxide (OsO[math]_{4}[/math]).
Osmium tetroxide is water soluble and will react with strong bases such as potassium hydroxide to form osmates;-
2KOH + OsO[math]_{4}[/math] → 2K[math]^{+}[/math] + OsO[math]_{4}[/math](OH)[math]^{-2}_{2}[/math]
Osmium is not amphoteric.
In bulk form and at ordinary temperatures and pressures, osmium metal does resist attack by all acids and alkalis, including potassium hydroxide.
However, in finely powdered form, osmium reacts with oxygen at elevated temperatures (200–300°C) to produce osmium tetroxide (OsO[math]_{4}[/math]).
Osmium tetroxide is water soluble and will react with strong bases such as potassium hydroxide to form osmates;-
2KOH + OsO[math]_{4}[/math] → 2K[math]^{+}[/math] + OsO[math]_{4}[/math](OH)[math]^{-2}_{2}[/math]
Osmium is not amphoteric.
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The alkali metals have a high electropositivity meaning that they readily lose their single valence electron in order to obey the octet rule
The alkali metals have a high electropositivity meaning that they readily lose their single valence electron in order to obey the octet rule
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