Home
Class 11
CHEMISTRY
Effective nuclear charge (Z(eff)) for a ...

Effective nuclear charge `(Z_(eff))` for a nucleus of an atom is defined as

A

shielding of the outermost shell electrons from the nucleus by the innermost shell electrons

B

the net positive charge experienced by electron from the nucleus

C

the attractive force experienced by the nucleus from electron

D

screening of positive charge on nucleus by innermost shell electrons.

Text Solution

Verified by Experts

The correct Answer is:
B
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • STRUCTURE OF ATOM

    NCERT FINGERTIPS|Exercise Higher Order Thinking Skills|11 Videos

  • STRUCTURE OF ATOM

    NCERT FINGERTIPS|Exercise NCERT Exemplar|15 Videos

  • STRUCTURE OF ATOM

    NCERT FINGERTIPS|Exercise Towards Quantum Mechanical Model Of The Town|10 Videos

  • STATES OF MATTER

    NCERT FINGERTIPS|Exercise Assertion And Reason|15 Videos

  • THE P-BLOCK ELEMENTS

    NCERT FINGERTIPS|Exercise Assertion And Reason|15 Videos

Similar Questions

Explore conceptually related problems

Tell the relation between effective nuclear charge (Z_(eff)) atomic number (Z) and shielding constant (sigma) . Explain it qualitatively.

Arrange s, p and d sub-shells of a shell in the increasing order of effective nuclear charge (Z_("eff")) experienced by the electron present in them.

Knowledge Check

  • Effective nuclear charge depends upon

    A
    the shielding effect
    B
    the atomic number
    C
    the charge on the nucleus
    D
    both the nuclear charge and the shielding effect.

  • Effective nuclear charge (Z_(eff)) is the net attractive force on electrons under consideration and is equal to: Z_(eff) = Z - sigma (nuclear charge - screening constant). Z_(eff) or sigma is calculated by Slater's formula, as given. If one electrons is present in the outermst orbit, there will be no screening in that orbital. Each electrons contribute, 0.35 (total electrons minus one electron) present in the outermost shell. A contribution of 0.85 for each electrons is taken in the (n - 1)th shell. Which of the following statement is wrong?

    A
    `IE_(1)` of `Ga gt Al`, due ot imperfect shielding of `3d`-orbitals in `Ga`.
    B
    `IE_(1)` of `Ga lt Al`, due ot perfect shielding of `3d`-orbitals in `Ga`.
    C
    The atomic size of `Ga` and `Al` are almost same because of poor shielding effect of electrons in `d`-orbitals as the effective nuclear charge increases in `Ga`.
    D
    `IE_(1)` of group `16` elements is less than that of group `15` elements.

  • Effective nuclear charge (Z_(eff)) is the net attractive force on electrons under consideration and is equal to: Z_(eff) = Z - sigma (nuclear charge - screening constant). Z_(eff) or sigma is calculated by Slater's formula, as given. If one electrons is present in the outermst orbit, there will be no screening in that orbital. Each electrons contribute, 0.35 (total electrons minus one electron) present in the outermost shell. A contribution of 0.85 for each electrons is taken in the (n - 1)th shell. Which of the following statement is wrong?

    A
    The number of lobes in `f`-orbitals are `8`.
    B
    `IE_(1)` of elements increases along the period.
    C
    `IE_(1)` of the group `3` elements is more than that of the group `2` elements.
    D
    `IE_(1), IE_(2)` and `IE_(3)` of an elemnt are `9.5, 18.5` and `154.4 eV`. Predict that the element has either two `s`-electrons or two `p`-electrons in the valence shell.

    • Similar Questions

    Explore conceptually related problems

    Arrange s,p and d subshells of a shell in the increasing order of effective nuclear charge (Z_(eff)) experienced by the electron present in them.

    Effective nuclear charge (Z_(eff)) is the net attractive force on electrons under consideration and is equal to: Z_(eff) = Z - sigma (nuclear charge - screening constant). Z_(eff) or sigma is calculated by Slater's formula, as given. If one electrons is present in the outermst orbit, there will be no screening in that orbital. Each electrons contribute, 0.35 (total electrons minus one electron) present in the outermost shell. A contribution of 0.85 for each electrons is taken in the (n - 1)th shell. The screening constant (sigma) for 4s electron of Mn (Z = 25) will be

    J.C. Slater proposed an empirical constant that represents the cumulative extent to which the other electrons of an atom shield (or screen) any particular electron from the nuclear charge. Thus, slater's screening contant sigma is as : Z^(**)=Z-sigma Here, Z is the atomic number of the atom, and hence is equal to the actual number of protons in the atom. the parameter Z^(**) is the effective nuclear charge, which according to is smaller than Z, since the electron in question is screened (shielded) from Z by an amount sigma . Conversely, an electron that is well shielded from the nuclear charge Z experiences a small effective nuclear charge Z^(**) . The value of sigma for any one electron in a given electron configuration (i.e., in the presence of the other electrons of the atom in question) is calculated using a set of empirical rules developed by slater. according to these rules, the value of sigma for the electron in question is the cumulative total provided by the various other electrons of the atom. Q. According to Slater's rule, order of effective nuclear charge (Z^(**)) for last electron in case of Li, Na and K.

    J.C. Slater proposed an empirical constant that represents the cumulative extent to which the other electrons of an atom shield (or screen) any particular electron from the nuclear charge. Thus, slater's screening contant sigma is as : Z^(**)=Z-sigma Here, Z is the atomic number of the atom, and hence is equal to the actual number of protons in the atom. the parameter Z^(**) is the effective nuclear charge, which according to is smaller than Z, since the electron in question is screened (shielded) from Z by an amount sigma . Conversely, an electron that is well shielded from the nuclear charge Z experiences a small effective nuclear charge Z^(**) . The value of sigma for any one electron in a given electron configuration (i.e., in the presence of the other electrons of the atom in question) is calculated using a set of empirical rules developed by slater. according to these rules, the value of sigma for the electron in question is the cumulative total provided by the various other electrons of the atom. Q. According to Slater's rule, order of effective nuclear charge (Z^(**)) for last electron in case of Li, Na and K.

    The effective nuclear charge (Z_("eff")) takes into account the interelectronic repulsion in multielectron atoms. Slater's rule helps us in evaluating Z_("eff") for various species. Apply Slater's rules to answer the following questions. Z_("eff") for 3d electron of Zn=x Z_("eff") for 3d electron of Zn^(2+( = y Z_("eff") for 4s electron Zn = z Choose the correct option(s)

    Home
    Profile