(b) Electrovalent compound are polar in nature because they are formed by ions.
Chemical Bonding and Molecular Structure
11887
Ionic compounds do not have
1 Hard and brittle nature
2 High melting and boiling point
3 Directional properties
4 Soluble in polar solvents
Explanation:
Hard and brittle: Due to the presence of a strong force of attraction between the positive and negative ions ionic compounds are solids and are hard to break. They generally break into pieces when pressure is applied as they are brittle. High melting and boiling points: Due to the presence of an electrostatic force of attraction between ions, a large amount of energy is required to break the ionic bonds between the atoms. Thus, ionic compounds have high melting and boiling points. Non-Directional nature: Ionic bonds are strong electrostatic attraction forces formed between positive and negative ions. This bond is nondirectional, this means the pull of electron doesn't favour one item over another. Soluble in polar solvents: Ionic compounds are soluble in polar solvents like water. Polar water molecules have a strong attraction for charged ions and the charged ions become solvated as they dissociate into the water. Hence the ionic compounds are soluble in polar solvents. Therefore, ionic compounds do not have direction properties. Directional bonds are the ones where a specific orientation of atoms or groups is necessary.
Chemical Bonding and Molecular Structure
11888
What is the effect of more electronegative atom on the strength of ionic bond
1 Decreases
2 Increases
3 Decreases slowly
4 Remains the same
Explanation:
(b) As soon as the electronegativity increases, ionic bond strength increases.
Chemical Bonding and Molecular Structure
11889
An element \(X\) with the electronic configuration \(1{s^2},\,2{s^2}2{p^6},\,3{s^2}\) would be expected to form the chloride with the formula
1 \(XC{l_3}\)
2 \(XC{l_2}\)
3 \(XCl\)
4 \({X_2}Cl\)
Explanation:
(b) This \(X\) element is a second group element so its chloride will be \(XC{l_2}\).
Chemical Bonding and Molecular Structure
11890
Two element have electronegativity of \(1.2\) and \(3.0\). Bond formed between them would be
1 Ionic
2 Polar covalent
3 Co-ordinate
4 Metallic
Explanation:
When electronegativity difference is from \(1.7\) to \(3.0\). This bond is called as ionic bond.
(b) Electrovalent compound are polar in nature because they are formed by ions.
Chemical Bonding and Molecular Structure
11887
Ionic compounds do not have
1 Hard and brittle nature
2 High melting and boiling point
3 Directional properties
4 Soluble in polar solvents
Explanation:
Hard and brittle: Due to the presence of a strong force of attraction between the positive and negative ions ionic compounds are solids and are hard to break. They generally break into pieces when pressure is applied as they are brittle. High melting and boiling points: Due to the presence of an electrostatic force of attraction between ions, a large amount of energy is required to break the ionic bonds between the atoms. Thus, ionic compounds have high melting and boiling points. Non-Directional nature: Ionic bonds are strong electrostatic attraction forces formed between positive and negative ions. This bond is nondirectional, this means the pull of electron doesn't favour one item over another. Soluble in polar solvents: Ionic compounds are soluble in polar solvents like water. Polar water molecules have a strong attraction for charged ions and the charged ions become solvated as they dissociate into the water. Hence the ionic compounds are soluble in polar solvents. Therefore, ionic compounds do not have direction properties. Directional bonds are the ones where a specific orientation of atoms or groups is necessary.
Chemical Bonding and Molecular Structure
11888
What is the effect of more electronegative atom on the strength of ionic bond
1 Decreases
2 Increases
3 Decreases slowly
4 Remains the same
Explanation:
(b) As soon as the electronegativity increases, ionic bond strength increases.
Chemical Bonding and Molecular Structure
11889
An element \(X\) with the electronic configuration \(1{s^2},\,2{s^2}2{p^6},\,3{s^2}\) would be expected to form the chloride with the formula
1 \(XC{l_3}\)
2 \(XC{l_2}\)
3 \(XCl\)
4 \({X_2}Cl\)
Explanation:
(b) This \(X\) element is a second group element so its chloride will be \(XC{l_2}\).
Chemical Bonding and Molecular Structure
11890
Two element have electronegativity of \(1.2\) and \(3.0\). Bond formed between them would be
1 Ionic
2 Polar covalent
3 Co-ordinate
4 Metallic
Explanation:
When electronegativity difference is from \(1.7\) to \(3.0\). This bond is called as ionic bond.
(b) Electrovalent compound are polar in nature because they are formed by ions.
Chemical Bonding and Molecular Structure
11887
Ionic compounds do not have
1 Hard and brittle nature
2 High melting and boiling point
3 Directional properties
4 Soluble in polar solvents
Explanation:
Hard and brittle: Due to the presence of a strong force of attraction between the positive and negative ions ionic compounds are solids and are hard to break. They generally break into pieces when pressure is applied as they are brittle. High melting and boiling points: Due to the presence of an electrostatic force of attraction between ions, a large amount of energy is required to break the ionic bonds between the atoms. Thus, ionic compounds have high melting and boiling points. Non-Directional nature: Ionic bonds are strong electrostatic attraction forces formed between positive and negative ions. This bond is nondirectional, this means the pull of electron doesn't favour one item over another. Soluble in polar solvents: Ionic compounds are soluble in polar solvents like water. Polar water molecules have a strong attraction for charged ions and the charged ions become solvated as they dissociate into the water. Hence the ionic compounds are soluble in polar solvents. Therefore, ionic compounds do not have direction properties. Directional bonds are the ones where a specific orientation of atoms or groups is necessary.
Chemical Bonding and Molecular Structure
11888
What is the effect of more electronegative atom on the strength of ionic bond
1 Decreases
2 Increases
3 Decreases slowly
4 Remains the same
Explanation:
(b) As soon as the electronegativity increases, ionic bond strength increases.
Chemical Bonding and Molecular Structure
11889
An element \(X\) with the electronic configuration \(1{s^2},\,2{s^2}2{p^6},\,3{s^2}\) would be expected to form the chloride with the formula
1 \(XC{l_3}\)
2 \(XC{l_2}\)
3 \(XCl\)
4 \({X_2}Cl\)
Explanation:
(b) This \(X\) element is a second group element so its chloride will be \(XC{l_2}\).
Chemical Bonding and Molecular Structure
11890
Two element have electronegativity of \(1.2\) and \(3.0\). Bond formed between them would be
1 Ionic
2 Polar covalent
3 Co-ordinate
4 Metallic
Explanation:
When electronegativity difference is from \(1.7\) to \(3.0\). This bond is called as ionic bond.
(b) Electrovalent compound are polar in nature because they are formed by ions.
Chemical Bonding and Molecular Structure
11887
Ionic compounds do not have
1 Hard and brittle nature
2 High melting and boiling point
3 Directional properties
4 Soluble in polar solvents
Explanation:
Hard and brittle: Due to the presence of a strong force of attraction between the positive and negative ions ionic compounds are solids and are hard to break. They generally break into pieces when pressure is applied as they are brittle. High melting and boiling points: Due to the presence of an electrostatic force of attraction between ions, a large amount of energy is required to break the ionic bonds between the atoms. Thus, ionic compounds have high melting and boiling points. Non-Directional nature: Ionic bonds are strong electrostatic attraction forces formed between positive and negative ions. This bond is nondirectional, this means the pull of electron doesn't favour one item over another. Soluble in polar solvents: Ionic compounds are soluble in polar solvents like water. Polar water molecules have a strong attraction for charged ions and the charged ions become solvated as they dissociate into the water. Hence the ionic compounds are soluble in polar solvents. Therefore, ionic compounds do not have direction properties. Directional bonds are the ones where a specific orientation of atoms or groups is necessary.
Chemical Bonding and Molecular Structure
11888
What is the effect of more electronegative atom on the strength of ionic bond
1 Decreases
2 Increases
3 Decreases slowly
4 Remains the same
Explanation:
(b) As soon as the electronegativity increases, ionic bond strength increases.
Chemical Bonding and Molecular Structure
11889
An element \(X\) with the electronic configuration \(1{s^2},\,2{s^2}2{p^6},\,3{s^2}\) would be expected to form the chloride with the formula
1 \(XC{l_3}\)
2 \(XC{l_2}\)
3 \(XCl\)
4 \({X_2}Cl\)
Explanation:
(b) This \(X\) element is a second group element so its chloride will be \(XC{l_2}\).
Chemical Bonding and Molecular Structure
11890
Two element have electronegativity of \(1.2\) and \(3.0\). Bond formed between them would be
1 Ionic
2 Polar covalent
3 Co-ordinate
4 Metallic
Explanation:
When electronegativity difference is from \(1.7\) to \(3.0\). This bond is called as ionic bond.
(b) Electrovalent compound are polar in nature because they are formed by ions.
Chemical Bonding and Molecular Structure
11887
Ionic compounds do not have
1 Hard and brittle nature
2 High melting and boiling point
3 Directional properties
4 Soluble in polar solvents
Explanation:
Hard and brittle: Due to the presence of a strong force of attraction between the positive and negative ions ionic compounds are solids and are hard to break. They generally break into pieces when pressure is applied as they are brittle. High melting and boiling points: Due to the presence of an electrostatic force of attraction between ions, a large amount of energy is required to break the ionic bonds between the atoms. Thus, ionic compounds have high melting and boiling points. Non-Directional nature: Ionic bonds are strong electrostatic attraction forces formed between positive and negative ions. This bond is nondirectional, this means the pull of electron doesn't favour one item over another. Soluble in polar solvents: Ionic compounds are soluble in polar solvents like water. Polar water molecules have a strong attraction for charged ions and the charged ions become solvated as they dissociate into the water. Hence the ionic compounds are soluble in polar solvents. Therefore, ionic compounds do not have direction properties. Directional bonds are the ones where a specific orientation of atoms or groups is necessary.
Chemical Bonding and Molecular Structure
11888
What is the effect of more electronegative atom on the strength of ionic bond
1 Decreases
2 Increases
3 Decreases slowly
4 Remains the same
Explanation:
(b) As soon as the electronegativity increases, ionic bond strength increases.
Chemical Bonding and Molecular Structure
11889
An element \(X\) with the electronic configuration \(1{s^2},\,2{s^2}2{p^6},\,3{s^2}\) would be expected to form the chloride with the formula
1 \(XC{l_3}\)
2 \(XC{l_2}\)
3 \(XCl\)
4 \({X_2}Cl\)
Explanation:
(b) This \(X\) element is a second group element so its chloride will be \(XC{l_2}\).
Chemical Bonding and Molecular Structure
11890
Two element have electronegativity of \(1.2\) and \(3.0\). Bond formed between them would be
1 Ionic
2 Polar covalent
3 Co-ordinate
4 Metallic
Explanation:
When electronegativity difference is from \(1.7\) to \(3.0\). This bond is called as ionic bond.
