What is the basic theme of organisation in the periodic table?

Which important property did Mendeleev use to classify the elements in his periodic table and did he stick to that?

What is the basic difference in approach between the Mendeleev’s Periodic Law and the Modern Periodic Law?

On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements.

In terms of period and group where would you locate the element with Z =114?

Write the atomic number of the element present in the third period and seventeenth group of the periodic table.

Which element do you think would have been namedby (I) Lawrence BerkeleyLaboratory (II) Seaborg’s group?

Why do elements in the same group have similar physical and chemical properties?

What does atomic radius and ionic radius really mean to you?

How does atomic radius vary in a period and in a group? How do you explain the variation?

What do you understand by isoelectronic species? Name a species that will be isoelectronic with each of the following atoms or ions. (I) F^– (II) Ar (III) Mg²⁺ (IV) Rb+

Consider the following species: N^3–, O^2–, F^–, Na⁺, Mg²⁺ and Al³⁺ (I) What is common inthem? (II) Arrange them in the order of increasing ionicradii.

Explain why cations are smaller and anions larger in radii than their parent atoms?

What is the significance of the terms - ‘isolated gaseous atom’ and ‘ground state’ while defining the ionization enthalpy and electron gain enthalpy?Hint: Requirements for comparison purposes.

Energy of an electron in the ground state of the hydrogen atom is –2.18 × 10^–18 J. Calculate the ionization enthalpy of atomic hydrogen in terms of J mol^–1.

Among the second period elements the actual ionization enthalpies are in the order Li < B < Be < C < O < N < F < Ne. Explain why (I) Be has higher ?_iH thanB (II) O has lower ?_iH than N andF?

How would you explain the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?

What are the various factors due to which the ionization enthalpy of the main group elements tends to decrease down a group?

The first ionization enthalpy values (in kJmol^–1) of group 13 elements are : B Al Ga In Tl 801 577 579 558 589 How would you explain this deviation from the general trend?

Which of the following pairs of elements would have a more negative electron gain enthalpy?(i) O or F (ii) F or Cl

Would you expect the second electron gain enthalpy of O as positive, more negative or less negative than the first? Justify your answer.

Whatisthebasicdifferencebetweenthetermselectrongainenthalpyand electronegativity?

How would you react to the statement that the electronegativity of N on Pauling scale is3.0 in all the nitrogen compounds?

Describe the theory associated with the radius of an atom as it (I) gains anelectron (II) loses an electron

Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.

What are the major differences between metals and non-metals?

Use the periodic table to answer the following questions. (I) Identify an element with five electrons in the outersubshell. (II) Identify an element that would tend to lose twoelectrons. (III) Identify an element that would tend to gain twoelectrons. (IV) Identify the group having metal, non-metal, liquid as well as gas at the room temperature.

The increasing order of reactivity among group 1 elements is Li < Na < K < Rb CI > Br > I. Explain.

Write the general outer electronic configuration of s-, p-, d- and f- block elements.

Assign the position of the element having outer electronic configuration (i) ns²np⁴ for n = 3 (ii) (n - 1)d²ns² for n = 4, and (iii) (n - 2) f⁷ (n - 1)d¹ns² for n = 6, in the periodic table.

The first (?_iH1) and the second (?_iH) ionization enthalpies (in kJ mol^–1) and the (?_egH) electron gain enthalpy (in kJ mol^–1) of a few elements are given below: Elements ?_iH ?_iH ?_egH I 520 7300 –60 II 419 3051 –48 III 1681 3374 –328 IV 1008 1846 –295 V 2372 5251 +48 VI 738 1451 –40 Which of the above elements is likely to be : (I) the least reactiveelement. (II) the most reactivemetal. (III) the most reactivenon-metal. (IV) the least reactivenon-metal. (V) the metal which can form a stable binary halide of the formula MX₂,(X=halogen). (VI) the metal which can form a predominantly stable covalent halide of the formula MX (X=halogen)?

Predict the formula of the stable binary compounds that would be formed by the combination of the following pairs of elements. (a) Lithiumandoxygen(b) Magnesium andnitrogen (c) Aluminiumandiodine(d) Silicon and oxygen (e) Phosphorusandfluorine(f) Element 71 andfluorine

In the modern periodic table, the period indicates the value of: (I) Atomicnumber (II) Atomicmass (III) Principal quantumnumber (IV) Azimuthal quantum number.

Which of the following statements related to the modern periodic table is incorrect? (I) The p-block has 6 columns, because a maximum of 6 electrons can occupy all the orbitals in ap-shell. (II) The d-block has 8 columns, because a maximum of 8 electrons can occupy all the orbitals in ad-subshell. (III) Each block contains a number of columns equal to the number of electrons that can occupy that subshell. (IV) The block indicates value of azimuthal quantum number (l ) for the last subshell that received electrons in building up the electronicconfiguration.

Anything that influences the valence electrons will affect the chemistry of the element. Which one of the following factors does not affect the valence shell? (I) Valence principal quantum number(n) (II) Nuclear charge(Z) (III) Nuclearmass (IV) Number of core electrons.

The size of isoelectronic species — F^–, Ne and Na⁺ is affected by (I) Nuclear charge (Z) (II) Valence principal quantum number(n) (III) Electron-electron interaction in the outerorbitals (IV) None of the factors because their size is the same.

Which one of the following statements is incorrect in relation to ionization enthalpy? (I) Ionization enthalpy increases for each successiveelectron. (II) The greatest increase in ionization enthalpy is experienced on removal of electron from core noble gasconfiguration. (III) End of valence electrons is marked by a big jump in ionizationenthalpy. (IV) Removal of electron from orbitals bearing lower n value is easier than from orbital having higher nvalue.

Considering the elements B, Al, Mg, and K, the correct order of their metallic character is: (a) B > Al > Mg> K(b) Al > Mg > B >K(c) Mg > Al > K > B (d) K > Mg > Al > B

Considering the elements B, C, N, F, and Si, the correct order of their non-metallic character is: (a) B > C > Si > N> Fb) Si > C > B > N >F(c) F > N > C > B > Si d) F > N > C > Si > B

Considering the elements F, Cl, O and N, the correct order of their chemical reactivity in terms of oxidizing property is: (a) F > Cl > O>N(b) F > O > Cl >N(c) Cl > F > O > N (d) O > F > N > Cl