Elements A, B, C and D Iwoe atomic numbers 12,19, 29, and 36 respectively. On the basis of electronic configuration, write to which group of the periodic table each element belongs.
Electronic configuration of A (Z = 12)
=1s2 2s2 2p6 3s2
period = 3, Element's name = Mg block = s, Group = II Electronic configuration of B (Z = 19)
Element’s name = K (potassium)
=1s2 2s2 2p6 3s2 3p6 4s1 n = 4, period = 4 Block = s, Group = I Electronic configuration of C (Z = 29)
=1s2 2s2 2p6 3s2 3p6 3d10 4s1 n – 4, period = 4 Block = d Electronic configuration of D (Z = 36)
=1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 period = 4 Block = p-Block group = 18
Ionisation enthalpies of elements of second period are given below:
Ionisation enthalpy/kJ mol-1: 520, 899, 801, 1086, 1402, 1314, 1681, 2080. Match the correct enthalpy with the elements and complete the graph given in figure. Also write symbols of elements with their atomic number.
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
Discuss the main characteristics of four blocks of elements in the periodic table? Give their general electronic configuration.
What is the basic difference in approach between Mendeleev’s Periodic Law and the Modem Periodic Law?
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?
Show by a chemical reaction with water that Na20 is a basic oxide and Cl207 is an acidic oxide.
Consider the isoelectronic species, Na+, Mg2+, F and O2-. The correct order of increasing length of their radii is
The first ionization enthalpies of Na, Mg, A1 and Si are in the order
(a) Na < Mg > A1 < Si
(b) Na>Mg>Al>Si
(c) Na < Mg < A1 < Si
(d) Na > Mg > A1 < Si
Among the elements B, Al, C and Si,
(a) which element has the highest first ionization enthalpy
(b) which element has the most metallic character?
Justify your answer in each case.
Choose the correct order of atomic radii of fluorine and neon (in pm) out of the options given below and justify your answer.
(i) 72,160 (b) 160,160 (c) 72,72 (d) 160,72
Illustrate by taking examples of transition elements and non-transition elements that oxidation states of elements are largely based on electronic configuration.
On the basis of quantum numbers, justify that the sixth period of the periodic table should have 32 elements.
How do atomic radius vary in a period and in a group? How do you explain the variation?
Among the second period elements, the actual ionization enthalpies are in the order: Li
(i) Be has higher ∆iH1than B ?
(ii) O has lower ∆iH1 than N and F?
In the modem periodic table, the period indicates the value of
(a)atomic number (b) mass number (c) principal quantum number (d) azimuthal quantum number?
Discuss the main features of long form of the periodic table. What are the advantages of long . form of periodic table?
Those elements impart colour to the flame on heating in it, the atoms of which require low energy for the ionization (i.e., absorb energy in the visible region of spectrum). The elements of which of the following groups will impart colour to the flame?
(a) 2 (b) 13 (c) 1 (d) 17
Identify the group and valency of the element having atomic number 119. Also predict the outermost electronic configuration and write the general formula of its oxide.
Write the atomic number of the element present in the third period and seventeenth group of the periodic table.
Would you expect the second electron gain enthalpy of O as positive, more negative or less negative than the first? Justify your answer.
Assign the position of the element having outer electronic configuration,
(i) ns2 np4 for n = 3 (ii) (n – 1) d2 ns2 for n = 4 and (iii) (n – 2) f7 (n – 1) d1 ns2 for n = 6 in the periodic table?
Name different blocks of elements in the periodic table. Give general electronic configuration of each block.
Define electron gain enthalpy. What are its units? Discuss the factors which influence the electron gain enthalpy.
Electronic configurations of four elements A, B, C and D are given below:
(A) 1s2 2s12p6
(B) 1 s2 2s2 2p4
(C) 1s2 2s2 2p6 3s1
(D) Is2 2s2 2p5
Which of the following is the correct order of increasing tendency to gain electron?
(a) A < C < B < D
(b) A < B < C < D
(c) D < B < C < A
(d) D < A< B < C
What do you understand by exothermic reaction and endothermic reaction? Give one example of each type.
The increasing order of reactivity among group 1 elements is Li < Na < K < Rb < Cs whereas that of group 17 is F > Cl > Br > I. Explain?
Explain why chlorine can be converted into chloride ion more easily as compared to fluoride ion from fluorine ?
What is the cause of periodicity in properties of the elements? Explain with two examples.
Which of the following elements can show covalency greater than 4?
(a) Be (b) P (c) S (d) B
Which of the following statements are correct?
(a) Helium has the highest first ionization enthalpy in the periodic table.
(b) Chlorine has less negative electron gain enthalpy than fluorine.
(c) Mercury and bromine are liquids at room temperature.
(d) In any period, atomic radius of alkali metal is the highest.
Which of the following sets contain only isoelectronic ions?
(a) Zn2+, Ca2+, Ga3+, Al3+
(b) K+, Ca2+, Sc3+, Cl–
(c) P3-, S2- Cl–,K+
(d) Ti4+, Ar, Cl3+, V5+
How would you explain the fact that first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium?
Explain the deviation in ionization enthalpy of some elements from the general trend by using the given figure.
Explain the following:
(a) Electronegativity of elements increases on moving from left to right in the periodic table.
(b) Ionisation enthalpy decreases in a group from top to bottom.
