HBrO3 is a stronger acid than HBrO2 , because bromine in the former acid is in +5 oxidation state compared to the later in which it is in +3 oxidation state.
HBrO3 is a stronger acid than HBrO2 , because bromine in the former acid is in +5 oxidation state compared to the later in which it is in +3 oxidation state.
HBrO2(aq) is bromous acid and HIO2(aq) is iodous acid.
Like many of the oxyacids, the molecules of HBrO2 (hydrogen bromite) and HIO2 (hydrogen iodite) are unlikely to exist in nature as they would likely decompose into oxides and water vapour when trying to isolate them from their respective acid solutions.
HBrO2(aq) is bromous acid and HIO2(aq) is iodous acid.
Like many of the oxyacids, the molecules of HBrO2 (hydrogen bromite) and HIO2 (hydrogen iodite) are unlikely to exist in nature as they would likely decompose into oxides and water vapour when trying to isolate them from their respective acid solutions.
CH3CCL2COOH because the chlorine is closer to the COOH-group withdraws electrons by inductive effect, so the H+ will be released more easy, so a stronger acid.
CH3CCL2COOH because the chlorine is closer to the COOH-group withdraws electrons by inductive effect, so the H+ will be released more easy, so a stronger acid.
In both acid the oxidation number of chlorine and bromine are same ,that is +3 . But chlorine atom is more electronegative than bromine atom . So the electron of O - H bond strongly attract Cl atom towards itself than bromine atom .As a result the O -H bond in HClO2 is more polar than O -H bond in HBrO2 . Hence HClO2 released proton easily than HBrO2 . Consequently , HClO2 is more stroger acid than HBrO2 .
In both acid the oxidation number of chlorine and bromine are same ,that is +3 . But chlorine atom is more electronegative than bromine atom . So the electron of O - H bond strongly attract Cl atom towards itself than bromine atom .As a result the O -H bond in HClO2 is more polar than O -H bond in HBrO2 . Hence HClO2 released proton easily than HBrO2 . Consequently , HClO2 is more stroger acid than HBrO2 .
A good general rule is that with other elements unchanged, more O atoms results in a stronger acid.
It might be helpful to think about acids that you know are strong as as compared with similar acids with fewer O atoms, such as HNO3 and HNO2 or H2SO4 and H2SO3.
A good general rule is that with other elements unchanged, more O atoms results in a stronger acid.
It might be helpful to think about acids that you know are strong as as compared with similar acids with fewer O atoms, such as HNO3 and HNO2 or H2SO4 and H2SO3.
HBrO3 is a stronger acid than HBrO2 , because bromine in the former acid is in +5 oxidation state compared to the later in which it is in +3 oxidation state.
HBrO3 is a stronger acid than HBrO2 , because bromine in the former acid is in +5 oxidation state compared to the later in which it is in +3 oxidation state.
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HBrO2(aq) is bromous acid and HIO2(aq) is iodous acid.
Like many of the oxyacids, the molecules of HBrO2 (hydrogen bromite) and HIO2 (hydrogen iodite) are unlikely to exist in nature as they would likely decompose into oxides and water vapour when trying to isolate them from their respective acid solutions.
HBrO2(aq) is bromous acid and HIO2(aq) is iodous acid.
Like many of the oxyacids, the molecules of HBrO2 (hydrogen bromite) and HIO2 (hydrogen iodite) are unlikely to exist in nature as they would likely decompose into oxides and water vapour when trying to isolate them from their respective acid solutions.
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CH3CCL2COOH because the chlorine is closer to the COOH-group withdraws electrons by inductive effect, so the H+ will be released more easy, so a stronger acid.
CH3CCL2COOH because the chlorine is closer to the COOH-group withdraws electrons by inductive effect, so the H+ will be released more easy, so a stronger acid.
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In both acid the oxidation number of chlorine and bromine are same ,that is +3 . But chlorine atom is more electronegative than bromine atom . So the electron of O - H bond strongly attract Cl atom towards itself than bromine atom .As a result the O -H bond in HClO2 is more polar than O -H bond in HBrO2 . Hence HClO2 released proton easily than HBrO2 . Consequently , HClO2 is more stroger acid than HBrO2 .
In both acid the oxidation number of chlorine and bromine are same ,that is +3 . But chlorine atom is more electronegative than bromine atom . So the electron of O - H bond strongly attract Cl atom towards itself than bromine atom .As a result the O -H bond in HClO2 is more polar than O -H bond in HBrO2 . Hence HClO2 released proton easily than HBrO2 . Consequently , HClO2 is more stroger acid than HBrO2 .
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A good general rule is that with other elements unchanged, more O atoms results in a stronger acid.
It might be helpful to think about acids that you know are strong as as compared with similar acids with fewer O atoms, such as HNO3 and HNO2 or H2SO4 and H2SO3.
A good general rule is that with other elements unchanged, more O atoms results in a stronger acid.
It might be helpful to think about acids that you know are strong as as compared with similar acids with fewer O atoms, such as HNO3 and HNO2 or H2SO4 and H2SO3.
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“Stronger or weaker” by themselves have no meaning at all.
[math]mathrm{H_2^+}[/math] is less stable than [math]mathrm{H_2}[/math] because it has both a net electrical charge and a weaker bond.
The bond is weaker because in [math]mathrm{H_2^+}[/math] it is a one-electron bond, while in [math]mathrm{H_2}[/math] it is a two-electron bond.
“Stronger or weaker” by themselves have no meaning at all.
[math]mathrm{H_2^+}[/math] is less stable than [math]mathrm{H_2}[/math] because it has both a net electrical charge and a weaker bond.
The bond is weaker because in [math]mathrm{H_2^+}[/math] it is a one-electron bond, while in [math]mathrm{H_2}[/math] it is a two-electron bond.
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Stronger as what? Acetone is generally a better solvent for a greater variety of solutes.
Stronger as what? Acetone is generally a better solvent for a greater variety of solutes.
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