HOME WORK - 02/11/2019 - CHEMISTRY - NIOS - 313
Senior Secondary Course

Module II: Atomic Structure and Chemical Bonding - HW-03-02

Chapter Name - PERIODIC TABLE AND PERIODICITY IN PROPERTIES - 3
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Q1. Classify the elements of group 14, 15 and 16 into metals, non-metals and metalloids.

Q2. Compare the metallic character of aluminium and potassium.

Q3. Name the group number for the following type of clements
(i) Alkaline earth metals
(ii) Alkali metals
(iii) Transition metals
(iv) Halogens
(v) Noble gases.

Q4. Name five man made elements

Q5. Write the names of the elements with atomic numbers 105, 109, 112, 115 according to IUPAC nomenclature.

Q6. Arrange the following in the order of increasing size Na+, Al3+, O2–, F–

Q7. How does the size of atoms vary from left to right in a period and on descending a group in the periodic table?

Q8. What is the correlation between atomic size and ionization enthalpy.

Q9. Which species, in each pair is expected to have higher ionization enthalpy.
(i) 3Li, 11Na (ii) 7N, 15P
(iii) 20Ca, 12Mg (iv) 13Al, 14Si
(v) 17Cl, 18Ar (vi) 18Ar, 19K
(vii) 13Al, 14C

Q10. Account for the fact that there is a decrease in first ionization enthalpy from Be to B and Mg to Al.

Q11. Why is the ionization enthalpy of the noble gases highest in their respective periods?

Q12. Name the most electronegative element.

Q13. Define modern periodic law.

Q14. Refer the periodic table given in Table 3.2 and answer the following questions.
(i) The elements placed in group number 18 are called ...............
(ii) Alkali and alkaline earth metals are collectively called ............... block metals.
(iii) The general configuration for halogens is ...............
(iv) Name a p-block element which is a gas other than a noble gas or a hologen.
(v) Name the groups that comprise the ‘s’ block of elements.
(vi) Element number 118 has not yet been established, to which block, will it belong?
(vii) How many elements should be there in total if all the 7s, 7p, 6d and 5f, blocks are to be full?

Q15. Describe the variation of electron affinity and ionization enthalpy in the periodic table.

Q16. Define the following:
(a) Electron gain enthalpy (b) Ionization enthalpy
(c) Ionic radius (d) Electronegativity.

Q17. What is electronegativity? How is it related to the type of bond formed?

Q18. Why is the electron gain enthalpy of Cl more in negative value as compared to that of F?