Chapter 9, Problem 9.71QP

(a)

Interpretation Introduction

Interpretation:

The energy change in the given process is whether ionization, electron affinity, bond enthalpy or standard enthalpy of formation has to be ascertained.

Concept Introduction:

Ionization energy is defined as the energy required to remove the valence electron of an atom when it is in gaseous state.  In periodic table ionization energy of elements decreases down the column or group and increases across the row or period as it is inversely proportional to the atomic size.

Electron affinity is defined as the energy released when an electron is added (gained by an atom) to the atom in its gaseous state forming negative ion.  In periodic table electron affinity of elements decreases down the column or group and increases across the row or period as it is inversely proportional to the atomic size.

Bond enthalpy is the energy required to break one mole of a bond or energy released when one mole of bond is formed between two certain atoms.

Standard enthalpy of formation is defined as the change in enthalpy under standard conditions when one mole of compound is formed from elements in pure state and standard conditions of pressure and temperature ($298K,1atm$ ).

(b)

Interpretation Introduction

Interpretation:

The energy change in the given process is whether ionization, electron affinity, bond enthalpy or standard enthalpy of formation has to be ascertained.

Concept Introduction:

Ionization energy is defined as the energy required to remove the valence electron of an atom when it is in gaseous state.  In periodic table ionization energy of elements decreases down the column or group and increases across the row or period as it is inversely proportional to the atomic size.

Electron affinity is defined as the energy released when an electron is added (gained by an atom) to the atom in its gaseous state forming negative ion.  In periodic table electron affinity of elements decreases down the column or group and increases across the row or period as it is inversely proportional to the atomic size.

Bond enthalpy is the energy required to break one mole of a bond or energy released when one mole of bond is formed between two certain atoms.

Standard enthalpy of formation is defined as the change in enthalpy under standard conditions when one mole of compound is formed from elements in pure state and standard conditions of pressure and temperature ($298K,1atm$ ).

(c)

Interpretation Introduction

Interpretation:

The energy change in the given process is whether ionization, electron affinity, bond enthalpy or standard enthalpy of formation has to be ascertained.

Concept Introduction:

Ionization energy is defined as the energy required to remove the valence electron of an atom when it is in gaseous state.  In periodic table ionization energy of elements decreases down the column or group and increases across the row or period as it is inversely proportional to the atomic size.

Electron affinity is defined as the energy released when an electron is added (gained by an atom) to the atom in its gaseous state forming negative ion.  In periodic table electron affinity of elements decreases down the column or group and increases across the row or period as it is inversely proportional to the atomic size.

Bond enthalpy is the energy required to break one mole of a bond or energy released when one mole of bond is formed between two certain atoms.

Standard enthalpy of formation is defined as the change in enthalpy under standard conditions when one mole of compound is formed from elements in pure state and standard conditions of pressure and temperature ($298K,1atm$ ).

(d)

Interpretation Introduction

Interpretation:

The energy change in the given process is whether ionization, electron affinity, bond enthalpy or standard enthalpy of formation has to be ascertained.

Concept Introduction:

Ionization energy is defined as the energy required to remove the valence electron of an atom when it is in gaseous state.  In periodic table ionization energy of elements decreases down the column or group and increases across the row or period as it is inversely proportional to the atomic size.

Electron affinity is defined as the energy released when an electron is added (gained by an atom) to the atom in its gaseous state forming negative ion.  In periodic table electron affinity of elements decreases down the column or group and increases across the row or period as it is inversely proportional to the atomic size.

Bond enthalpy is the energy required to break one mole of a bond or energy released when one mole of bond is formed between two certain atoms.

Standard enthalpy of formation is defined as the change in enthalpy under standard conditions when one mole of compound is formed from elements in pure state and standard conditions of pressure and temperature ($298K,1atm$ ).