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The amount of enthalpy required to remov...

The amount of enthalpy required to remove the most loosely bound electron from an isolated gaseous atom to form a positive ion is known as

A

ionization enthalpy

B

electron affinity

C

lattice enthalpy

D

electrolysis.

Text Solution

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The correct Answer is:
To solve the question, we need to identify the term that describes the amount of energy required to remove the most loosely bound electron from an isolated gaseous atom to form a positive ion. ### Step-by-Step Solution: 1. **Understanding the Concept**: - We are looking for a specific term that relates to the removal of an electron from an atom. This process involves energy, as removing an electron requires overcoming the attraction between the negatively charged electron and the positively charged nucleus. 2. **Identifying the Options**: - The question provides four options: A. Ionization enthalpy B. Electron affinity C. Lattice enthalpy D. Electrolysis process 3. **Analyzing Each Option**: - **A. Ionization enthalpy**: This is defined as the amount of energy required to remove the most loosely bound electron from an isolated gaseous atom, forming a positive ion. This matches our requirement. - **B. Electron affinity**: This refers to the energy change that occurs when an electron is added to a neutral atom, which is not what we are looking for. - **C. Lattice enthalpy**: This is the energy required to separate one mole of a solid ionic compound into its gaseous ions. This is also not relevant to our question. - **D. Electrolysis process**: This is a method of using a direct electric current to drive a chemical reaction, which does not pertain to the removal of an electron from an atom. 4. **Conclusion**: - Since option A, "Ionization enthalpy," directly corresponds to the definition provided in the question, we can conclude that the correct answer is **A. Ionization enthalpy**. ### Final Answer: The amount of enthalpy required to remove the most loosely bound electron from an isolated gaseous atom to form a positive ion is known as **Ionization enthalpy**. ---
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The amount of energy required to remove the most loosely bound electron from an isolated gaseous atom is called as first ionization energy (IE_(1)) . Similarly the amount of energies required to knock out second, third etc. electrons from the isolated and IE_(3)gt IE_(2)gt IE_(1) . (i) Nuclear charge (ii) Atomic size (iii) penetration effect of the electrons (iv) shielding effect of the inner electrons and (b) electronic configurations (exactly half filled and completely filled configurations are extra stable) are the important factors which affect the ionisation energies. Similarly, the amount of energy released when a neutral isolated gaseous atom accepts an extra electron to from gaseous anion is called electron affinity. (X(g)+e^(-)(g)rarr X^(-)(g)+ energy A positive elecrton affinity idicates that the ion X^(-) has a lower more negative energy than the neutral atom X. The second electron affinity for the addition of a second electron to an initially neutral atom is negative because the electron replusion outweights the nuclear attraction, e.g., O(g)+e^(-)overset("Exothermic")rarr O^(-)(g),E_(a)=+141 kJ mol^(-) ....(i) O^(-)(g)+e^(-)overset("Excothermic")rarr, E_(a)=-780 kJ mol^(-) ...(ii) The electron affinity of an element depends upon (i) atomic size (ii) nuclear charge and (iii) electronic configuration. In general, in a group, ionisation energy and electron affinity decrease as the atomic size increases. The members of third period have some higher (e.g., S and Cl) electron affinity values than the members of second period (e.g., O and F) because second period elements have very small atomic size. Hence, there is tendency of electron-electron repulsion, which resultss in less evolution of energy in the formation of correcsponding anion. Which one of the following statements is incorrect in relation to ionisation enthalpy?

The amount of energy required to remove the most loosely bound electron from an isolated gaseous atom is called as first ionization energy (IE_(1)) . Similarly the amount of energies required to knock out second, third etc. electrons from the isolated and IE_(3)gt IE_(2)gt IE_(1) . (i) Nuclear charge (ii) Atomic size (iii) penetration effect of the electrons (iv) shielding effect of the inner electrons and (b) electronic configurations (exactly half filled and completely filled configurations are extra stable) are the important factors which affect the ionisation energies. Similarly, the amount of energy released when a neutral isolated gaseous atom accepts an extra electron to from gaseous anion is called electron affinity. (X(g)+e^(-)(g)rarr X^(-)(g)+ energy A positive elecrton affinity idicates that the ion X^(-) has a lower more negative energy than the neutral atom X. The second electron affinity for the addition of a second electron to an initially neutral atom is negative because the electron replusion outweights the nuclear attraction, e.g., O(g)+e^(-)overset("Exothermic")rarr O^(-)(g),E_(a)=+141 kJ mol^(-) ....(i) O^(-)(g)+e^(-)overset("Excothermic")rarr, E_(a)=-780 kJ mol^(-) ...(ii) The electron affinity of an element depends upon (i) atomic size (ii) nuclear charge and (iii) electronic configuration. In general, in a group, ionisation energy and electron affinity decrease as the atomic size increases. The members of third period have some higher (e.g., S and Cl) electron affinity values than the members of second period (e.g., O and F) because second period elements have very small atomic size. Hence, there is tendency of electron-electron repulsion, which resultss in less evolution of energy in the formation of correcsponding anion. Identify the least stable ion amongst the following:

The amount of energy required to remove the most loosely bound electron from an isolated gaseous atom is called as first ionization energy (IE_(1)) . Similarly the amount of energies required to knock out second, third etc. electrons from the isolated and IE_(3)gt IE_(2)gt IE_(1) . (i) Nuclear charge (ii) Atomic size (iii) penetration effect of the electrons (iv) shielding effect of the inner electrons and (b) electronic configurations (exactly half filled and completely filled configurations are extra stable) are the important factors which affect the ionisation energies. Similarly, the amount of energy released when a neutral isolated gaseous atom accepts an extra electron to from gaseous anion is called electron affinity. (X(g)+e^(-)(g)rarr X^(-)(g)+ energy A positive elecrton affinity idicates that the ion X^(-) has a lower more negative energy than the neutral atom X. The second electron affinity for the addition of a second electron to an initially neutral atom is negative because the electron replusion outweights the nuclear attraction, e.g., O(g)+e^(-)overset("Exothermic")rarr O^(-)(g),E_(a)=+141 kJ mol^(-) ....(i) O^(-)(g)+e^(-)overset("Excothermic")rarr, E_(a)=-780 kJ mol^(-) ...(ii) The electron affinity of an element depends upon (i) atomic size (ii) nuclear charge and (iii) electronic configuration. In general, in a group, ionisation energy and electron affinity decrease as the atomic size increases. The members of third period have some higher (e.g., S and Cl) electron affinity values than the members of second period (e.g., O and F) because second period elements have very small atomic size. Hence, there is tendency of electron-electron repulsion, which resultss in less evolution of energy in the formation of correcsponding anion. The first ionisation energy of Na, Mg,AI and Si are in the order of:

Highest amount of energy will be required for the removal of electron from