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Class 9 Chemistry Structure Of Molecules What is a chemical bond and why do atoms form a chemical bond?


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What is a chemical bond and why do atoms form a chemical bond?

16. Which one of the following is an electron deficient molecule?(a) \mathrm{NH}_{3} (b) \mathrm{BF}_{3} (c) \mathrm{N}_{2} (d) \mathrm{O}_{2}
16. Which one of the following is an electron deficient molecule?(a)  \mathrm{NH}_{3} (b)  \mathrm{BF}_{3} (c)  \mathrm{N}_{2} (d)  \mathrm{O}_{2}

16. Which one of the following is an electron deficient molecule?(a) \mathrm{NH}_{3} (b) \mathrm{BF}_{3} (c) \mathrm{N}_{2} (d) \mathrm{O}_{2}

How can you justify that bond strength in polar covalent compounds is comparable to that of ionic compound?
How can you justify that bond strength in polar covalent compounds is comparable to that of ionic compound?

How can you justify that bond strength in polar covalent compounds is comparable to that of ionic compound?

What is octet rule? Why do atoms always struggle to attain the nearest noble gas electronic configuration?
What is octet rule? Why do atoms always struggle to attain the nearest noble gas electronic configuration?

What is octet rule? Why do atoms always struggle to attain the nearest noble gas electronic configuration?

7. A bond formed between two non-metals is expected to be:(a) covalent(b) ionic(c) coordinate covalent(d) metallic
7. A bond formed between two non-metals is expected to be:(a) covalent(b) ionic(c) coordinate covalent(d) metallic

7. A bond formed between two non-metals is expected to be:(a) covalent(b) ionic(c) coordinate covalent(d) metallic

3. Considering the electronic configuration of atoms which atom with the given atomic number will be the most stable one?(a) 6(b) 8(c) 10(d) 12
3. Considering the electronic configuration of atoms which atom with the given atomic number will be the most stable one?(a) 6(b) 8(c) 10(d) 12

3. Considering the electronic configuration of atoms which atom with the given atomic number will be the most stable one?(a) 6(b) 8(c) 10(d) 12

11. What is a triple covalent bond explain with an example?
11. What is a triple covalent bond explain with an example?

11. What is a triple covalent bond explain with an example?

Explain the types of covalent bonds with at least one example of each type.
Explain the types of covalent bonds with at least one example of each type.

Explain the types of covalent bonds with at least one example of each type.

2. Why is the bond between an electropositive and an electronegative atom ionic in nature?
2. Why is the bond between an electropositive and an electronegative atom ionic in nature?

2. Why is the bond between an electropositive and an electronegative atom ionic in nature?

Define hydrogen bonding. Explain that how these forces affect the physical properties of compounds.
Define hydrogen bonding. Explain that how these forces affect the physical properties of compounds.

Define hydrogen bonding. Explain that how these forces affect the physical properties of compounds.

3. Ionic compounds are solids. Justify.
3. Ionic compounds are solids. Justify.

3. Ionic compounds are solids. Justify.

5. Metals are good conductor of electricity. Why?
5. Metals are good conductor of electricity. Why?

5. Metals are good conductor of electricity. Why?

4. More electronegative elements can form bonds between themselves. Justify.
4. More electronegative elements can form bonds between themselves. Justify.

4. More electronegative elements can form bonds between themselves. Justify.

What is a chemical bond and why do atoms form a chemical bond?
What is a chemical bond and why do atoms form a chemical bond?
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What is a chemical bond and why do atoms form a chemical bond?

6. When an electronegative element combines with an electropositive element the type of bonding is:(a) covalent(b) ionic(c) polar covalent(d) coordinate covalent
6. When an electronegative element combines with an electropositive element the type of bonding is:(a) covalent(b) ionic(c) polar covalent(d) coordinate covalent

6. When an electronegative element combines with an electropositive element the type of bonding is:(a) covalent(b) ionic(c) polar covalent(d) coordinate covalent

1. Why do atoms react?
1. Why do atoms react?

1. Why do atoms react?

16 . Give the characteristic properties of ionic compounds.
 16 . Give the characteristic properties of ionic compounds.

16 . Give the characteristic properties of ionic compounds.

4. Octet rule is:(a) description of eight electrons(b) picture of electronic configuration(c) pattern of electronic configuration(d) attaining of eight electrons
4.    Octet rule is:(a) description of eight electrons(b) picture of electronic configuration(c) pattern of electronic configuration(d) attaining of eight electrons

4. Octet rule is:(a) description of eight electrons(b) picture of electronic configuration(c) pattern of electronic configuration(d) attaining of eight electrons

10. Ice floats on water because:(a) ice is denser than water(b) ice is crystalline in nature(c) water is denser than ice(d) water molecules move randomly
10. Ice floats on water because:(a) ice is denser than water(b) ice is crystalline in nature(c) water is denser than ice(d) water molecules move randomly

10. Ice floats on water because:(a) ice is denser than water(b) ice is crystalline in nature(c) water is denser than ice(d) water molecules move randomly

12. How many covalent bonds does \mathrm{C}_{2} \mathrm{H}_{2} molecule have?(a) two(b) three(c) four(d) five
12. How many covalent bonds does  \mathrm{C}_{2} \mathrm{H}_{2}  molecule have?(a) two(b) three(c) four(d) five
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12. How many covalent bonds does \mathrm{C}_{2} \mathrm{H}_{2} molecule have?(a) two(b) three(c) four(d) five

What are intermolecular forces? Compare these forces with chemical bond forces with reference to \mathrm{HC} 1 molecule?
What are intermolecular forces? Compare these forces with chemical bond forces with reference to  \mathrm{HC} 1  molecule?
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What are intermolecular forces? Compare these forces with chemical bond forces with reference to \mathrm{HC} 1 molecule?

5. Transfer of electrons between atoms results in:(a) metallic bonding(b) ionic bonding(c) covalent bonding(d) coordinate covalent bonding
5. Transfer of electrons between atoms results in:(a) metallic bonding(b) ionic bonding(c) covalent bonding(d) coordinate covalent bonding
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5. Transfer of electrons between atoms results in:(a) metallic bonding(b) ionic bonding(c) covalent bonding(d) coordinate covalent bonding

17. Identify which pair has polar covalent bonds.(a) \mathrm{O}_{2} and \mathrm{Cl}_{2} (b) \mathrm{H}_{2} \mathrm{O} and \mathrm{N}_{2} (c) \mathrm{H}_{2} \mathrm{O} and { }_{2} \mathrm{H}_{2} (d) \mathrm{H}_{2} \mathrm{O} and \mathrm{Hcl}
17. Identify which pair has polar covalent bonds.(a)  \mathrm{O}_{2}  and  \mathrm{Cl}_{2} (b)  \mathrm{H}_{2} \mathrm{O}  and  \mathrm{N}_{2} (c)  \mathrm{H}_{2} \mathrm{O}  and  { }_{2} \mathrm{H}_{2} (d)  \mathrm{H}_{2} \mathrm{O}  and  \mathrm{Hcl}
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17. Identify which pair has polar covalent bonds.(a) \mathrm{O}_{2} and \mathrm{Cl}_{2} (b) \mathrm{H}_{2} \mathrm{O} and \mathrm{N}_{2} (c) \mathrm{H}_{2} \mathrm{O} and { }_{2} \mathrm{H}_{2} (d) \mathrm{H}_{2} \mathrm{O} and \mathrm{Hcl}

10. Why HC1 has dipole-dipole forces of attraction?
10. Why HC1 has dipole-dipole forces of attraction?
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10. Why HC1 has dipole-dipole forces of attraction?

8. Differentiate between lone pair and bond pair of electrons.
8. Differentiate between lone pair and bond pair of electrons.
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8. Differentiate between lone pair and bond pair of electrons.

13. Why a covalent bond becomes polar?
13. Why a covalent bond becomes polar?
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13. Why a covalent bond becomes polar?

7. What type of covalent bond is formed in nitrogen molecule.
7. What type of covalent bond is formed in nitrogen molecule.
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7. What type of covalent bond is formed in nitrogen molecule.

What is metallic bond? Explain the metallic bonding with the help of a diagram.
What is metallic bond? Explain the metallic bonding with the help of a diagram.
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What is metallic bond? Explain the metallic bonding with the help of a diagram.

8. A bond pair in covalent molecules usually has:(a) one electron(b) two electrons(c) three electrons(d) four electrons
8. A bond pair in covalent molecules usually has:(a) one electron(b) two electrons(c) three electrons(d) four electrons
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8. A bond pair in covalent molecules usually has:(a) one electron(b) two electrons(c) three electrons(d) four electrons

12. What is difference between polar and non-polar covalent bonds explain with one example of each?
12. What is difference between polar and non-polar covalent bonds explain with one example of each?
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12. What is difference between polar and non-polar covalent bonds explain with one example of each?

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