The Periodic Table is an organized arrangement of elements based on their atomic number, electron configuration, and recurring chemical properties. Initially proposed by Dmitri Mendeleev, it has been refined over time to align with modern atomic theory.
The periodic table is a systematic arrangement of elements, grouping those with similar properties together.
The periodic table consists of 18 vertical columns known as groups. Elements in the same group form a family and are often named after the first element in the group. Some groups also have specific names, including:
All other groups are generally named after their first element.
The horizontal rows in the periodic table are called periods. There are seven periods in the long-form periodic table:
In multi-electron atoms, the outermost (valence) electrons experience both:
This reduces the effective nuclear attraction on valence electrons, a phenomenon called the shielding or screening effect.
The effective nuclear charge (Zeff) is the net positive charge experienced by an electron. It is calculated using the formula:
Zeff = Z − 𝛔
Where:
Across a period (left to right), the effective nuclear charge increases, due to greater nuclear attraction.
Ionization Energy
Electron Affinity
Electronegativity= Ionization Potential+Electron Affinity2
Pauling’s Scale: The most commonly used scale, based on bond energy differences.
ΔE=(Actual Bond Energy)−(EA−A * EB−B)
The relationship between Pauling and Mulliken electronegativity values is:
𝜒(Pauling) = 0.34×𝜒(Mulliken) − 0.2
Atomic Volume
Density
Melting and Boiling Points
Oxidation State (Oxidation Number, O.N.)
Magnetic Properties
Q.1 Given below are two statements :
Statement (I) : The 4f and 5f - series of elements are placed separately in the Periodic table to preserve the principle of classification.
Statement (II) :S-block elements can be found in pure form in nature. In the light of the above statements, choose the most appropriate answer from the options given below :
(1) Statement I is false but Statement II is true
(2) Both Statement I and Statement II are true
(3) Statement I is true but Statement II is false
(4) Both Statement I and Statement II are false
Ans. (3)
Sol. s-block elements are highly reactive and found in combined state.
Q.2 The correct order of first ionization enthalpy values of the following elements is :
(A) O
(B) N
(C) Be
(D) F
(E) B
Choose the correct answer from the options given below :
(1) B < D < C < E < A (2) E < C < A < B < D
(3) C < E < A < B < D (4) A < B < D < C < E
Ans. (2)
Sol. Correct order of Ist IE
Li < B < Be < C < O < N < F < Ne
↓ ↓ ↓ ↓ ↓
E < C < A < B < D
Q.3 The transition metal having highest 3rd ionisation enthalpy is :
(1) Cr
(2) Mn
(3) V
(4) Fe
Ans. (2)
Sol. 3rd Ionisation energy : [NCERT Data]
V : 2833 KJ/mol
Cr : 2990 KJ/mol Mn : 3260 KJ/mol Fe : 2962 KJ/mol
Alternative
Mn : 3d5 4s2 Fe : 3d6 4s2 Cr : 3d5 4s1 V : 3d3 4s2
So Mn has the highest 3rd IE among all the given elements due to d5 configuration.
Q.4 Given below are two statements :
Statement (I) : Both metal and non-metal exist in p and d-block elements.
Statement (II) : Non-metals have higher ionisation enthalpy and higher electronegativity than the metals.
In the light of the above statements, choose the most appropriate answer from the option given below:
(1) Both Statement I and Statement II are false
(2) Statement I is false but Statement II is true
(3) Statement I is true but Statement II is false
(4) Both Statement I and Statement II are true
[2024]
Ans. (2)
Sol. I. In p-Block both metals and non metals are present but in d-Block only metals are present.
II. EN and IE of non metals are greater than that of metals
I - False, II-True
Q.5 It is observed that characteristic X-ray spectra of elements show regularity. When frequency to the power 'n' i.e. vn of X-rays emitted is plotted against atomic number 'Z', the following graph is obtained.
The value of 'n' is
(1) 1
(2) 2
(3) 12
(4) 3
Ans. (3)
Sol. According to Henry Moseley √v ∝ z – b
So n = 12
Q.6 For electron gain enthalpies of the elements denoted as DegH, the incorrect option is :
(1) ΔegH (Cl) < ΔegH (F)
(2) ΔegH (Se) < ΔegH (S)
(3) ΔegH (I) < ΔegH (At)
(4) ΔegH (Te) < ΔegH (Po)
Ans. (2)
Sol.
(1) ΔegH (Cl) < Δeg H (F)
(–345) (– 328) Correct
(2) ΔegH (Se) < ΔegH (S)
(–195) (– 200) Incorrect
(3) ΔeggH (I) < ΔegH (At)
(–295) (– 270) Correct
(4) ΔegH (Te) < ΔegH (Po)
(–190) (– 183) Correct
Q.7 Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R
Assertion A: 5f electrons can participate in bonding to a far greater extent than 4f electrons
Reason R: 5f orbitals are not as buried as 4f orbitals
In the light of the above statements, choose the correct answer from the options given below
(1) Both A and R are true but R is NOT the correct explanation of A
(2) Both A and R are true and R is the correct explanation of A
(3) A is false but R is true
(4) A is true but R is false
[2023]
Ans. (2)
Sol. 5f orbital not buried as 4f orbitals so e– present in 5f orbital experience less nuclear attraction than e– present in 4f orbital. Hence electrons of 5f orbital can take part in bonding to a far greater extent.
Q.8 Outermost electronic configurations of four elements A, B, C, D are given below:
The correct order of first ionization enthalpy for them is:
(1) (A) < (B) < (C) < (D)
(2) (B) < (A) < (D) < (C)
(3) (B) < (D) < (A) < (C)
(4) (B) < (A) < (C) < (D)
Ans. (3)
(A) 3s2→ Mg
(B) 3s23p1→ Al
(C) 3s23p3 → P
(D) 3s23p4→ S
Ans. (3) C > D > A > B.
P > S > Mg > Al
Q.9 The first ionization enthalpy of Na, Mg and Si, respectively, are: 496, 737 and 786 mo1-1. The first ionization enthalpy (kJ mol-1) of Al is:
(1) 487 (2) 768 (3) 577 (4) 856
Ans. (3)
Sol. I.E. : Na < Al < Mg < Si
∴ 496 < IE (Al) < 737
i.e. IE(Al) = 577 kJ mol-1
Q.10 In which of the following pairs, electron gain enthalpies of constituent elements are nearly the same or identical ?
(A) Rb and Cs (B) Na and K (C) Ar and Kr (D) I and At
Choose the correct answer from the options given below :
(1) (A) and (B) only (2) (B) and (C) only
(3) (A) and (C) only (4) (C) and (D) only
Ans. (3)
Sol. Rb & Cs have nearly the same electron gain enthalpy electron gain enthalpy = – 46 kj/ml.
Ar & Kr have the same . Value is ΔHeq + 96 kj/ml
Q.11. Match List -I with List - II
Choose the most appropriate answer from the options given below -
(1) (a) → (ii), (b) → (iii), (c)→ (iv), (d) → (i)
(2) (a) → (i), (b) → (iv), (c) → (iii), (d) → (ii)
(3) (a) → (i), (b) → (iii), (c) → (iv), (d) → (ii)
(4) (a) → (iv), (b) → (i), (c) → (ii), (d) → (iii)
Ans. (1)
Sol. (a) 1s22s2 → Be
(b) 1s22s22p4 → O
(c) 1s22s22p3→ N
(d) 1s22s22p1 → B
The ionization enthalpy order is
B < Be < O < N
Be has more IE compared to B due to extra stability & N has more IE compared to oxygen due to extra stability
Hence, N → 1402 kJ/mol
O → 1314 kJ/mol
B → 801 k
Be → 899 kJ/mol
Q.12. The ionic radii of F– and O2– respectively are 1.33 Å and 1.4 Å, while the covalent radius of N is 0.74 Å. The correct statement for the ionic radius of N3– from the following is :
(1) It is smaller than F– and N
(2) It is bigger than O2– and
(3) It is bigger than F– and N, but smaller than of O2–
(4) It is smaller than O2– and F–, but bigger than of N
Ans. (2)
Sol. F–, O2– and N3– all are isoelectronic species in which N3– have the least number of protons due to which its size increases as least nuclear attraction is experienced by the outer shell electrons.
Size order N3– > O2– > F–
Q.13 The correct order of conductivity of ions in water is :
(1) Na+ > K+ > Rb+ > Cs+
(2) Cs+ > Rb+ > K+ > Na+
(3) K+ > Na+ > Cs+ > Rb+
(4) Rb+ > Na+ > K+ > Li+
Ans.(2)
Sol.
∴ Correct option is Na+ > K+ > Rb+ > Cs+.
OR
Sol.
As the size of gaseous ions decreases, it gets more hydrated in water and hence, the size of aqueous ions increases. When this bulky ion moves in solution, it experiences greater resistance and hence lower conductivity.
Size of gaseous ion : Cs+ > Rb+ > K+ > Na+
Size of aqueous ion : Cs+ < Rb+ < K+ < Na+
Conductivity : Cs+ > Rb+ > K+ > Na+
(Session 2025 - 26)