Predict the relative strength of each of the following groups
OH-,Cl-,No3-,CH3Coo and NH3
Based on their ability to donate or accept protons (H+ ions) or electrons, we can rank the relative strength of each of the following groups as follows:
1. NH3 (Ammonia): NH3 can act as a weak base, accepting a proton to form NH4+. It has a lone pair of electrons that can donate and readily react with acids. Therefore, NH3 is the strongest group out of the given options.
2. OH- (Hydroxide ion): OH- can act as a strong base, readily accepting protons to form H2O. It has a lone pair of electrons that can donate and react with acids. Therefore, OH- is stronger than Cl- and No3- but weaker than NH3.
3. No3- (Nitrate ion): No3- does not have a lone pair of electrons to donate or accept protons. It is primarily an anion and does not typically react as a base or an acid. Therefore, No3- is weaker than OH- but stronger than Cl- and CH3COO-.
4. CH3COO- (Acetate ion): CH3COO- does not have a lone pair of electrons to donate or accept protons. It is primarily an anion and does not typically react as a base or an acid. Therefore, CH3COO- is weaker than NH3, OH-, and No3-, but stronger than Cl-.
5. Cl- (Chloride ion): Cl- does not have a lone pair of electrons to donate or accept protons. It is primarily an anion and does not typically react as a base or an acid. Therefore, Cl- is the weakest group out of the given options.
To predict the relative strength of each group, we need to evaluate their respective acid-base properties. Here is the ranking, from strongest to weakest, of the given groups in terms of their basicity:
1. OH- (hydroxide ion): Hydroxide ions are strong bases due to the availability of a lone pair of electrons on the oxygen atom. This makes them capable of accepting a hydrogen ion (proton) from an acid, hence making them very strong bases.
2. NH3 (ammonia): Ammonia is a weaker base compared to hydroxide ions, but still a moderately strong base. It contains a lone pair of electrons on the nitrogen atom, allowing it to accept a hydrogen ion from an acid. However, it is not as strong as hydroxide ions.
3. CH3COO- (acetate ion): The acetate ion is a weak base. It is derived from acetic acid, which is a weak acid. While it can still act as a base and accept a hydrogen ion, it is less basic compared to hydroxide and ammonia.
4. Cl- (chloride ion): Chloride ions, derived from hydrochloric acid, are not basic at all. They do not possess any lone pairs of electrons that can accept a hydrogen ion, making them very weak as bases.
5. NO3- (nitrate ion): Nitrate ions are not basic either. They do not have any available lone pairs of electrons to accept protons, so they are not basic in nature. Instead, they act as weak conjugate bases of nitric acid.
To summarize, the ranking from strongest to weakest basicity is: OH- > NH3 > CH3COO- > Cl- > NO3-.
To predict the relative strength of each of the given groups, we need to determine their relative abilities to donate or accept protons (H+ ions).
1. OH-: The hydroxide ion is a strong base since it easily accepts a proton, forming water (H2O). Therefore, OH- is a strong group.
2. Cl-: Chloride ion is a weak base since it has a limited ability to accept protons. Therefore, Cl- is a weak group.
3. NO3-: The nitrate ion is not reactive towards protons and does not easily accept or donate them. Therefore, NO3- is considered a neutral group.
4. CH3COO-: The acetate ion is a weak base that can accept protons but has limited ability. Therefore, CH3COO- is a weak group.
5. NH3: Ammonia is a weak base since it can accept a proton, forming ammonium (NH4+). Therefore, NH3 is considered a weak group.
Therefore, from strongest to weakest, the relative strength of the given groups is as follows:
OH- > NH3 > CH3COO- > Cl- > NO3-