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Find how ionization energy changes with ...

Find how ionization energy changes with increase in nuclear charge?

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The correct Answer is:
On moving from left to right in a period, as nuclear charge increases, the size of the atom decrease hence ionization energy increase.
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Define ionization energy?

Can you find out how ionization energy changes as we move from top to bottom in a group?

Knowledge Check

  • Ionization energy of an element is:

    A
    Equal in magnitude but opposite in sign to the electron gain enthalpy of the cation of the element
    B
    Same as electron affinity of the element .
    C
    Energy required to remove one valence electron from an isolated gaseous atom in its ground state
    D
    Equal in magnitude but opposite in sign to the electron gain enthalpy of the anion of the element

  • The ionization energy of an element depends upon nuclear charge, atomic size, penetration effect of the 'electrons, shielding effect of the inner electrons and electronic configuration (exactly half filled & completely filled configuration are extra stable). The electron affinity of an element depends upon atomic size, nuclear charge and electronic configuration. In general, ionization energy and electron affinity increases as the atomic radii decreases and nuclear charge increases across a period. In general, in a group, ionization energy and electron affinity decrease as the atomic size increases. The members of third period have higher electron affinity values than the members of second period elements have very small atomic size. Hence there is a tendency of electron electron repulsion, which results in less evolution of energy in the formation of corresponding anion. The first ionization energy of Na, Mg, Al and Si are in the order of:

    A
    `Na lt Al lt Mg lt Si`
    B
    `Na gt Mg gt Al gt Si`
    C
    `Na lt Mg lt Al gt Si`
    D
    `Na gt Mg gt Al lt Si`

  • The ionization energy of an element depends upon nuclear charge, atomic size, penetration effect of the 'electrons, shielding effect of the inner electrons and electronic configuration (exactly half filled & completely filled configuration are extra stable). The electron affinity of an element depends upon atomic size, nuclear charge and electronic configuration. In general, ionization energy and electron affinity increases as the atomic radii decreases and nuclear charge increases across a period. In general, in a group, ionization energy and electron affinity decrease as the atomic size increases. The members of third period have higher electron affinity values than the members of second period elements have very small atomic size. Hence there is a tendency of electron electron repulsion, which results in less evolution of energy in the formation of corresponding anion. Identify the least stable ion amongst the following:

    A
    `Li^-`
    B
    `Be^-`
    C
    `B^-`
    D
    `C^-`

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    Don't you think that there is a relationship between ionization energy and metallic non metallic character? Is the element with highest ionization energy metallic or non metallic?

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    The ionization energy of an element depends upon nuclear charge, atomic size, penetration effect of the 'electrons, shielding effect of the inner electrons and electronic configuration (exactly half filled & completely filled configuration are extra stable). The electron affinity of an element depends upon atomic size, nuclear charge and electronic configuration. In general, ionization energy and electron affinity increases as the atomic radii decreases and nuclear charge increases across a period. In general, in a group, ionization energy and electron affinity decrease as the atomic size increases. The members of third period have higher electron affinity values than the members of second period elements have very small atomic size. Hence there is a tendency of electron electron repulsion, which results in less evolution of energy in the formation of corresponding anion. Which one of the following statements is incorrect in relation to ionisation enthalpy?

    The ionization energy of an element depends upon nuclear charge, atomic size, penetration effect of the 'electrons, shielding effect of the inner electrons and electronic configuration (exactly half filled & completely filled configuration are extra stable). The electron affinity of an element depends upon atomic size, nuclear charge and electronic configuration. In general, ionization energy and electron affinity increases as the atomic radii decreases and nuclear charge increases across a period. In general, in a group, ionization energy and electron affinity decrease as the atomic size increases. The members of third period have higher electron affinity values than the members of second period elements have very small atomic size. Hence there is a tendency of electron electron repulsion, which results in less evolution of energy in the formation of corresponding anion. Considering the elements F, Cl, O and S, the correct order of their electron affinity values is:

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