State three differences and three similarities between group 1 and group 2.
Answers
Answer:
Ionic radius increases down the group reducing the polarizing power of the cation.group 2 metal are less stable than group 1 because they have a smaller ionic radius .
The polarizing power and polarizability which enhances the formation of covalent bonds is favoured by the following factors:
Small cation: the high polarizing power stems from the greater concentration of positive charge on a small area. This explains why LiBr is more covalent than KBr.
Large anion: the high polarizability stems from the larger size where the outer electrons are more loosely held and can be more easily distorted by the cation. This explains why for the common halides, iodides, are the most covalent in nature .
Explanation:
Ionic radius increases down the group reducing the polarizing power of the cation.group 2 metal are less stable than group 1 because they have a smaller ionic radius .
The polarizing power and polarizability which enhances the formation of covalent bonds is favoured by the following factors:
Small cation: the high polarizing power stems from the greater concentration of positive charge on a small area. This explains why LiBr is more covalent than KBr.
Large anion: the high polarizability stems from the larger size where the outer electrons are more loosely held and can be more easily distorted by the cation. This explains why for the common halides, iodides, are the most covalent in nature .
Answer:
Answer:
Ionic radius increases down the group reducing the polarizing power of the cation.group 2 metal are less stable than group 1 because they have a smaller ionic radius .
The polarizing power and polarizability which enhances the formation of covalent bonds is favoured by the following factors:
Small cation: the high polarizing power stems from the greater concentration of positive charge on a small area. This explains why LiBr is more covalent than KBr.
Large anion: the high polarizability stems from the larger size where the outer electrons are more loosely held and can be more easily distorted by the cation. This explains why for the common halides, iodides, are the most covalent in nature .
Explanation:
Ionic radius increases down the group reducing the polarizing power of the cation.group 2 metal are less stable than group 1 because they have a smaller ionic radius .
The polarizing power and polarizability which enhances the formation of covalent bonds is favoured by the following factors:
Small cation: the high polarizing power stems from the greater concentration of positive charge on a small area. This explains why LiBr is more covalent than KBr.
Large anion: the high polarizability stems from the larger size where the outer electrons are more loosely held and can be more easily distorted by the cation. This explains why for the common halides, iodides, are the most covalent in nature .