Samacheer Kalvi solutions for Chemistry - Volume 1 and 2 [English] Class 11 TN Board chapter 3 - Periodic Classification Of Elements [Latest edition]

What would be the IUPAC name for an element with the atomic number 222?

The electronic configuration of the elements A and B are 1s², 2s², 2p⁶, 3s² and 1s², 2s², 2p⁵ respectively. The formula of the ionic compound that can be formed between these elements is

The group of elements in which the differentiating electron enters the anti penultimate shell of atoms are called ________.

In which of the following options the order of arrangement does not agree with the variation of the property indicated against it?

Which of the following elements will have the highest electronegativity?

Various successive ionisation enthalpies (in kJ mol^-1) of an element are given below.

The element is

In the third period the first ionization potential is of the order.

Identify the wrong statement.

Which one of the following arrangements represent the correct order of least negative to most negative electron gain enthalpy

The correct order of electron gain enthalpy with negative sign of F, Cl, Br and I having atomic number 9, 17, 35 and 53 respectively is

Which one of the following is the least electronegative element?

The element with positive electron gain enthalpy is

The correct order of decreasing electronegativity values among the elements X, Y, Z and A with atomic numbers 4, 8, 7 and 12 respectively

Assertion: Helium has the highest value of ionisation energy among all the elements known

Reason: Helium has the highest value of electron affinity among all the elements known

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?

IE₁ and IE₂ of Mg are 179 and 348 kcal mol⁻¹ respectively. The energy required for the reaction \[\ce{Mg -> Mg^2+ + 2e^-}\] is

In a given shell the order of screening effect is

Which of the following orders of ionic radii is correct?

The First ionisation potential of Na, Mg and Si are 496, 737 and 786 kJ mol^-1 respectively. The ionisation potential of Al will be closer to

Which one of the following is true about metallic character when we move from left to right in a period and top to bottom in a group?

How does electron affinity change when we move from left to right in a period in the periodic table?

Which of the following pairs of elements exhibit diagonal relationship?

Define modern periodic law.

What are isoelectronic ions? Give examples.

What is the effective nuclear charge?

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"

Magnesium loses electrons successively to form Mg⁺, Mg²⁺ and Mg³⁺ ions. Which step will have the highest ionisation energy and why?

Define electronegativity.

How would you explain the fact that the second ionisation potential is always higher than the first ionisation potential?

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.

The electronic configuration of atom is one of the important factor which affects the value of ionisation potential and electron gain enthalpy. Explain

In what period and group will an element with Z = 118 will be present?

Justify that the fifth period of the periodic table should have 18 elements on the basis of quantum numbers.

Elements a, b, c and d have the following electronic configurations:

• a: 1s², 2s², 2p⁶
• b: 1s², 2s², 2p⁶, 3s², 3p¹
• c: 1s², 2s², 2p⁶, 3s², 3p⁶
• d: 1s², 2s², 2p¹

Which elements among these will belong to the same group of the periodic table

Give the general electronic configuration of lanthanides and actinides?

Why do halogens act as oxidising agents?

Mention any two anomalous properties of second period elements.

Explain the Pauling method for the determination of ionic radius.

Explain the periodic trend of ionisation potential.

Explain the diagonal relationship.

Why the first ionisation enthalpy of sodium is lower than that of magnesium while its second ionisation enthalpy is higher than that of magnesium?

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.

Ionisation potential of N is greater than that of O

Explain the following, give an appropriate reason.

First ionisation potential of the C-atom is greater than that of the B atom, whereas the reverse is true is for the second ionisation potential.

Explain the following, give an appropriate reason.

The electron affinity values of Be and Mg are almost zero and those of N (0.02 eV) and P (0.80 eV) are very low.

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.

What is the screening effect?

Briefly give the basis for Pauling's scale of electronegativity.

State the trends in the variation of electronegativity in groups and periods.