the nitrogen atom in an ammonia molecule has a lone pair of electrons
TRANSCRIPT
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The nitrogen atom in an ammonia molecule has a lone pair of electrons.
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The nitrogen atom in an ammonia molecule has a lone pair of electrons.
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It can make a dative covalent bond with a hydrogen ion (a proton), forming an ammonium ion.
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It can make a dative covalent bond with a hydrogen ion (a proton), forming an ammonium ion.
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Ammonia is a Brønsted–Lowry base because it can accept protons.
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The nitrogen atom in a methylamine molecule has a lone pair of electrons.
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It can make a dative covalent bond with a proton, forming a methylammonium ion.
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It can make a dative covalent bond with a proton, forming a methylammonium ion.
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Methylamine is a Brønsted–Lowry base because it can accept protons.
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Amines are Brønsted–Lowry bases because they can accept a proton.
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When amines dissolve in water, they form alkaline solutions due to the presence of hydroxide ions.
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Amines dissolve in dilute acids to form soluble ionic salts.
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Phenylamine is almost insoluble in water.
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But it dissolves in excess dilute hydrochloric acid.
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The salt phenylammonium chloride is formed in the reaction.
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Ammonia is a weak base.
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It has a pKa value of 9.25 – the higher the value, the stronger the base.
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These primary aliphatic amines have higher pKa values than ammonia.
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These primary aliphatic amines have higher pKa values than ammonia.
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These primary aliphatic amines have higher pKa values than ammonia.
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They are stronger bases than ammonia. Why?
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They are stronger bases than ammonia. Why?
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The base strength of primary amines depends upon the availability of the lone pair of electrons on the nitrogen atom, which forms a bond with an H+ ion.
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The base strength of primary amines depends upon the availability of the lone pair of electrons on the nitrogen atom, which forms a bond with an H+ ion.
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The base strength of primary amines depends upon the availability of the lone pair of electrons on the nitrogen atom, which forms a bond with an H+ ion.
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These amines contain alkyl groups.
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These amines contain alkyl groups.
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The alkyl groups are electron-releasing relative to nitrogen.
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The alkyl groups are electron-releasing relative to nitrogen.
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The alkyl groups are electron-releasing relative to nitrogen.
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They increase the availability of the lone pair of electrons on the nitrogen atom, so primary aliphatic amines are stronger bases than ammonia.
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They increase the availability of the lone pair of electrons on the nitrogen atom, so primary aliphatic amines are stronger bases than ammonia.
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Primary aromatic amines are weaker bases than ammonia.
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Ammonia has a pKa value of 9.25 but phenylamine has a pKa value of 4.62. Why?
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The answer lies in the delocalised rings of electrons in the benzene ring and the lone pair of electrons on the nitrogen atom (seen here as the shape of a p orbital).
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The answer lies in the delocalised rings of electrons in the benzene ring and the lone pair of electrons on the nitrogen atom (seen here as the shape of a p orbital).
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The answer lies in the delocalised rings of electrons in the benzene ring and the lone pair of electrons on the nitrogen atom (seen here as the shape of a p orbital).
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The answer lies in the delocalised rings of electrons in the benzene ring and the lone pair of electrons on the nitrogen atom (seen here as the shape of a p orbital).
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The answer lies in the delocalised rings of electrons in the benzene ring and the lone pair of electrons on the nitrogen atom (seen here as the shape of a p orbital).
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The answer lies in the delocalised rings of electrons in the benzene ring and the lone pair of electrons on the nitrogen atom (seen here as the shape of a p orbital).
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The lone pair of electrons on the nitrogen atom interacts with these delocalised rings of electrons. The lone pair becomes less available for bonding to an H+ ion.
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The lone pair of electrons on the nitrogen atom interacts with these delocalised rings of electrons. The lone pair becomes less available for bonding to an H+ ion.
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The lone pair of electrons on the nitrogen atom interacts with these delocalised rings of electrons. The lone pair becomes less available for bonding to an H+ ion.