Back to chemistry after 2 months and got stuck in the beginning! That's why I don't like it. Anyways, come to the question please.

Following are the words from my textbook (Don't ask the name ;-)

$$\ce {Na -> Na^+ + e^-}\quad\Delta{H}=+495 \frac{KJ}{mol}$$

 

$$\ce {Cl + e^- -> Cl^-}\quad\Delta{H}=-348 \frac{KJ}{mol}$$

 

$$\ce {Na^+ + Cl^- -> NaCl}\quad\Delta{H}=-786 \frac{KJ}{mol}$$

 

We conclude that it is essential for the formation of ions and ionic bond that the sum of energies released in second and third reactions must be larger than what is required in the first step.

 

The great attractive forces (bonds) reduce the energy of the system greatly as it emits 786 KJ of energy.

a. Why should it happen? i.e. sum must be greater et cetera.

b. How does attractive forces tend to reduce the energy?

Back to chemistry after 2 months and got stuck in the beginning! That's why I don't like it. Anyways, come to the question please.

Following are the words from my textbook (Don't ask the name ;-)

$$\ce {Na -> Na^+ + e^-}\quad\Delta{H}=+495 \frac{KJ}{mol}$$

$$\ce {Cl + e^- -> Cl^-}\quad\Delta{H}=-348 \frac{KJ}{mol}$$

$$\ce {Na^+ + Cl^- -> NaCl}\quad\Delta{H}=-786 \frac{KJ}{mol}$$

We conclude that it is essential for the formation of ions and ionic bond that the sum of energies released in second and third reactions must be larger than what is required in the first step.

The great attractive forces (bonds) reduce the energy of the system greatly as it emits 786 KJ of energy.

a. Why should it happen? i.e. sum must be greater et cetera.

b. How does attractive forces tend to reduce the energy?

Back to chemistry after 2 months and got stuck in the beginning! That's why I don't like it. Anyways, come to the question please.

Following are the words from my textbook (Don't ask the name ;-)

$$\ce {Na -> Na^+ + e^-}\quad\Delta{H}=+495 \frac{KJ}{mol}$$

$$\ce {Cl + e^- -> Cl^-}\quad\Delta{H}=-348 \frac{KJ}{mol}$$

$$\ce {Na^+ + Cl^- -> NaCl}\quad\Delta{H}=-786 \frac{KJ}{mol}$$

We conclude that it is essential for the formation of ions and ionic bond that the sum of energies released in second and third reactions must be larger than what is required in the first step.

Why should it happen? Do Anybody know what do they want to say?

Back to chemistry after 2 months and got stuck in the beginning! That's why I don't like it. Anyways, come to the question please.

Following are the words from my textbook (Don't ask the name ;-)

$$\ce {Na -> Na^+ + e^-}\quad\Delta{H}=+495 \frac{KJ}{mol}$$

$$\ce {Cl + e^- -> Cl^-}\quad\Delta{H}=-348 \frac{KJ}{mol}$$

$$\ce {Na^+ + Cl^- -> NaCl}\quad\Delta{H}=-786 \frac{KJ}{mol}$$

We conclude that it is essential for the formation of ions and ionic bond that the sum of energies released in second and third reactions must be larger than what is required in the first step.

The great attractive forces (bonds) reduce the energy of the system greatly as it emits 786 KJ of energy.

a. Why should it happen? i.e. sum must be greater et cetera.

b. How does attractive forces tend to reduce the energy?