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Ionisation energy is the amount of energ...

Ionisation energy is the amount of energy required to remove the outermost `e^(-)` from a gaseous atom. It's unit is kJ/mole or kcal/mole.
Successive ionisation energy - It is the amount of energy required to remove electron successively from a gaseous ion. These are termed as `IE_(2), IE_(3), IE_(4)` etc. the difference in the values of `IE_(1), IE_(2) " and " IE_(3)` helps to determine electronic configuration of the element.

Which element forms stable unipositive ion ?

A

A

B

B

C

C

D

D

Text Solution

Verified by Experts

The correct Answer is:
B
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Ionisation energy is the amount of energy required to remove the outermost e^(-) from a gaseous atom. It's unit is kJ/mole or kcal/mole. Successive ionisation energy - It is the amount of energy required to remove electron successively from a gaseous ion. These are termed as IE_(2), IE_(3), IE_(4) etc. the difference in the values of IE_(1), IE_(2) " and " IE_(3) helps to determine electronic configuration of the element. Which element is a noble gas ?

Ionisation energy is the amount of energy required to remove the outermost e^(-) from a gaseous atom. It's unit is kJ/mole or kcal/mole. Successive ionisation energy - It is the amount of energy required to remove electron successively from a gaseous ion. These are termed as IE_(2), IE_(3), IE_(4) etc. the difference in the values of IE_(1), IE_(2) " and " IE_(3) helps to determine electronic configuration of the element. Which of the following is a non-metal ?

Knowledge Check

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

    A
    s-subshell
    B
    p-subshell
    C
    d-subshell
    D
    f-subshell

  • If 13.6 eV energy is required to ionise the hydrogen atom, then energy required to remove an electron from n=3 is :

    A
    9 eV
    B
    6.8 eV
    C
    3.4 eV
    D
    1.5 eV

  • The value of IE_(1), IE_(2), IE_(3) and IE_(4) of an atom are respectively 7.5 eV, 25.6 eV, 48.6 eV and 170.6 eV . The electronic configuration of the atom will be

    A
    `1s^(2), 2s^(2)2p^(6), 3s^(1)`
    B
    `1s^(2)2s^(2)2p^(6)3s^(2) 3p^(1)`
    C
    `1s^(2), 2s^(2)2p^(6)3s^(2)3p^(3)`
    D
    `1s^(2), 2s^(2)2p^(6)3s^(2)`

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    With the help of Bohr 's model , calculate the second ionisation energy of helium (energy required to remove the electron from He^(o+)

    How much energy is required to ionise a hydrogen atom if the electron occupies n=5 orbit ? Compare your answer with the ionisation energy of hydrogen atom (energy required to remove the electron from n=1 orbit).

    The energy required to dislodge electron from excited isolated H-atom, IE_1 =13.6 eV is

    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:

    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?

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