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प्रश्न
Identify the wrong statement.
विकल्प
Amongst the isoelectronic species, smaller the positive charge on cation, smaller is the ionic radius.
Amongst isoelectric species greater the negative charge on the anion, larger is the ionic radius.
Atomic radius of the elements increases as one moves down the first group of the periodic table.
Atomic radius of the elements decreases as one moves across from left to right in the 2nd period of the periodic table.
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उत्तर
Amongst the isoelectronic species, smaller the positive charge on cation, smaller is the ionic radius.
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संबंधित प्रश्न
Which of the following elements will have the highest electronegativity?
Various successive ionisation enthalpies (in kJ mol-1) of an element are given below.
| IE1 | IE2 | IE3 | IE4 | IE5 |
| 577.5 | 1,810 | 2,750 | 11,580 | 14,820 |
The element is
In the third period the first ionization potential is of the order.
The correct order of decreasing electronegativity values among the elements X, Y, Z and A with atomic numbers 4, 8, 7 and 12 respectively
The electronic configuration of the atom having maximum difference in first and second ionisation energies is
Which of the following is the second most electronegative element?
Is the definition given below for ionisation enthalpy is correct?
"Ionisation enthalpy is defined as the energy required to remove the most loosely bound electron from the valence shell of an atom"
Energy of an electron in the ground state of the hydrogen atom is −2.18 × 10−18 J. Calculate the ionisation enthalpy of atomic hydrogen in terms of kJ mol−1.
By using Pauling's method calculate the ionic radii of K+ and Cl− ions in the potassium chloride crystal. Given that `"d"_("K"^+) - "Cl"^-` = 3.14 Å
Explain the following, give an appropriate reason.
The formation of \[\ce{F^-_{(g)}}\] from \[\ce{F_{(g)}}\] is exothermic while that of \[\ce{O^2-_{(g)}}\] from \[\ce{O_{(g)}}\] is endothermic.
