Periodic Table & Periodicity PYQs Set 4 (PDF)

Set 4 of 11 · Questions 91-120 of 322

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NEET Chemistry · Periodic Table & Periodicity · Set 4 (Q91-120)

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91.
Which one of the following statements for D.I. Mendeleeff, is incorrect?
1. (1) $He authored the textbook - Principles of Chemistry.$
2. (2) $At the time, he proposed Periodic Table of elements structure of atom was known.$
3. (3) $Element with atomic number 101 is named after him.$
4. (4) $He invented accurate barometer.$
92.
Which of the following represents the correct trend for the mentioned property?(A) $F > P > S > B -$ First Ionization Energy(B) $Cl > F > S > P -$ Electron Affinity(C) $K > Al > Mg > B -$ Metallic character(D) $K_{2} O > Na_{2} O > MgO > Al_{2} O_{3} -$ Basic character
Choose the correct answer from the options given below :
1. (1) $(B) and (C) only$
2. (2) $(A), (B) and (D) only$
3. (3) $(A) and (B) only$
4. (4) $(A), (B), (C) and (D)$
93.
The ionic radii of $O^{2 -}, F^{-}, N a^{+}$ and $M g^{2 +}$ are in order
1. (1) $F^{-} > O^{2 -} > N a^{+} > M g^{2 +}$
2. (2) $M g^{2 +} > N a^{+} > F^{-} > O^{2 -}$
3. (3) $O^{2 -} > F^{-} > M g^{2 +} > N a^{+}$
4. (4) $O^{2 -} > F^{-} > N a^{+} > M g^{2 +}$
94.
Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements?
1.Nitrogen $(N)$
2.Phosphorus ( $P$ )
3.Chlorine $(Cl)$
4.Fluorine $(F)$
1. (1) $P < N < F < Cl$
2. (2) $N < P < F < Cl$
3. (3) $Cl < F < P < N$
4. (4) $F < Cl < N < P$
95.
Given below are two statements :
Statement $I$ : The metallic radius of $Na$ is $1.86 A^{\circ}$ and the ionic radius of $Na^{+}$ is lesser than $1.86 A^{\circ}$ .
Statement II : Ions are always smaller in size than the corresponding elements.
In the light of the above statements, choose the correct answer from the options given below :
1. (1) $Both Statement I and Statement II are false$
2. (2) $Statement I is incorrect but Statement II is true$
3. (3) $Both Statement I and Statement II are true$
4. (4) $Statement I is correct but Statement II is false$
96.
$Match List - I with List - II (Atomic number) (Block of periodic table)$
$LIST-I$ $LIST-II$
$(A) 37 I. p-block$ $III. f-block$
$(B)78 II. d-block$ $(D) 65 IV. s-block$
$(C) 52$
$Choose the correct answer from the options given below:$
1. (1) $A-II,B-IV,C-I,D-III$
2. (2) $A-I, B-III, C-IV, D-II$
3. (3) $A-IV,B-III,C-II,D-I$
4. (4) $A-IV,B-II,C-I,D-III$
97.
Assertion (A) : Mg2+ and Al3+ are isoelectronic but the magnitude of ionic radius of Al3+ is less than that in Mg2+.
Reason (R) : The effective nuclear charge on the outermost electrons in Al3+ is greater than that in Mg2+.The correct option among the following is
1. (1) $A is true, R is true and R is the correct explanation for A .$
2. (2) $A is true, R is true but R is not the correct explanation for A .$
3. (3) $A is true but R is false.$
4. (4) $A is false but R is true.$
98.
First ionisation enthalpy values of first four group 15 elements are given below. Choose the
correct value for the element that is a main component of apatite family:
1. (1) $1402 kJ mol^{- 1}$
2. (2) $834 kJ mol^{- 1}$
3. (3) $1012 kJ mol^{- 1}$
4. (4) $947 kJ mol^{- 1}$
99.
Assertion (A): First ionisation enthalpy of oxygen is less than that of nitrogenReason (R): Atoms with half-filled or completely filled orbitals are less stable
The correct option among the following is
1. (1) $(A) and (R) are true. (R) is the correct explanation of (A)$
2. (2) $(A) and (R) are true, but (R) is not correct explanation of (A)$
3. (3) $(A) is true but (R) is false$
4. (4) $(A) is false but (R) is true$
100.
The type of oxide formed by the element among $Li, Na, Be, Mg, B$ and Al that has the least
atomic radius is:
1. (1) $A_{2} O$
2. (2) $A_{2} O_{3}$
3. (3) $AO_{2}$
4. (4) $AO$
101.
The successive 5 ionisation energies of an element are $800, 2427, 3658, 25024$ and
$32824 kJ / mol$ , respectively. By using the above values predict the group in which the above element is present:
1. (1) $Group 13$
2. (2) $Group 14$
3. (3) $Group 2$
4. (4) $Group 4$
102.
Among the following, the pair of elements having same electronegativity values are
I. $H$ and $P$
II. $Be$ and $Al$
III. $N$ and $Cl$
IV. $C$ and $P$
1. (1) $I, II and III$
2. (2) $II, III and IV$
3. (3) $I, III and IV$
4. (4) $I, II, III and IV$
103.
In the following, the element with the highest ionisation energy is
1. (1) $| Ne | 3 s^{2} 3 p^{1}$
2. (2) $[Ne] 3 s^{2} 3 p^{2}$
3. (3) $[Ne] 3 s^{2} 3 p^{3}$
4. (4) $[Ne] 3 s^{2} 3 p^{4}$
104.
The number of following pairs of elements which exhibit diagonal relationship is:
$1. B & Si 2. Be & Al$
3. $Li & Mg$ 4. $Al & S$
1. (1) $2$
2. (2) $1$
3. (3) $3$
4. (4) $4$
105.
Given below are two statements: one is labelled as Assertion A and the other is labelled as Reason R. Assertion A : The energy required to form $M g^{2 +}$ from Mg is much higher than that required to produce $M g^{+}$ Reason R: $M g^{2 +}$ is small ion and carry more charge than $M g^{+}$
In the light of the above statements, choose the correct answer from the options given below.
1. (1) $Both A and R are true but R is NOT the correct explanation of A$
2. (2) $A is true but R is false$
3. (3) $A is false but R is true$
4. (4) $Both A and R are true and R is the correct explanation of A$
106.
Element "E" belongs to the period 4 and group 16 of the periodic table. The valence shell electron configuration of the element, which is just above $^{‘} E^{’}$ in the group is
1. (1) $3 s^{2} . 3 p^{4}$
2. (2) $3 d^{10} . 4 s^{2}, 4 p^{4}$
3. (3) $4 d^{10} . 5 s^{2}, 5 p^{4}$
4. (4) $2 s^{2}, p4$
107.
In which of the following arrangements the order is NOT according to the property indicated against it?
1. (1) $A l^{3 +} < M g^{2 +} < N a^{+} < F^{-} - increasing ionic size$
2. (2) $B < C < N < O - increasing first ionization enthalpy$
3. (3) $I < Br < F < Cl - increasing electron gain enthalpy (with negative sign)$
4. (4) $Li < Na < K < Rb - increasing metallic radius$
108.
Given below are two statements:
Statement (I) : The oxidation state of an element in a particular compound is the charge acquired by its atom on the basis of electron gain enthalpy consideration from other atoms in the molecule.
Statement (II) : $p π - p π$ bond formation is more prevalent in second period elements over other periods.
In the light of the above statements, choose the most appropriate answer from the options given below :
1. (1) $Both Statement I and Statement II are correct$
2. (2) $Both Statement I and Statement II are incorrect$
3. (3) $Statement I is incorrect but Statement II is correct$
4. (4) $Statement I is correct but Statement II is incorrect$
109.
Choose the smallest ion from the following.
1. (1) $Mg^{2 +}$
2. (2) $S^{2 -}$
3. (3) $Na^{+}$
4. (4) $Cl^{-}$
110.
Arrange the following in increasing order of ionic radii
$O^{2 -}, Na^{+}, F^{-}, Mg^{2 +}$
1. (1) $Mg^{2 +} < Na^{+} < F^{-} < O^{2 -}$
2. (2) $Mg^{2 +} < F^{-} < Na^{+} < O^{2 -}$
3. (3) $O^{2 -} < F^{-} < Na^{+} < Mg^{2 +}$
4. (4) $O^{2 -} < Mg^{2 +} < F^{-} < Na^{+}$
111.
Given that ionisation potential and electron gain enthalpy of chlorine are $13 eV$ and $4 eV$ respectively. The electronegativity of chlorine on Mulliken scale, approximately equals to
1. (1) $8.5 eV$
2. (2) $6.0 eV$
3. (3) $3.0 eV$
4. (4) $1.5 eV$
112.
Number of elements from the following that CANNOT form compounds with valencies which match with their respective group valencies is_____ B, C, N, S, O, F, P, Al, Si
1. (1) $7$
2. (2) $3$
3. (3) $5$
4. (4) $6$
113.
Given below are two statements : one is labelled as Assertion A and the other is labelled as Reason R:
Assertion A: The first ionisation enthalpy decreases across a period.
Reason R: The increasing nuclear charge outweighs the shielding across the period.
In the light of the above statements, choose the most appropriate from the options given below:
1. (1) $Both A and R are true and R is the correct explanation of A$
2. (2) $A is true but R is false$
3. (3) $A is false but R is true$
4. (4) $Both A and R are true but R is NOT the correct explanation of A$
114.
Which one of the following is correct order of the size of iodine species?
1. (1) $I^{+} > I^{-} > I$
2. (2) $I^{-} > I > I^{+}$
3. (3) $I > I^{-} > I^{+}$
4. (4) $I > I^{+} > I^{-}$
115.
The property/properties that show irregularity in first four elements of group-17 is/are
(A) Covalent radius(B) Electron affinity(C) Ionic radius(D) First ionization energy
Choose the correct answer from the options given below:
1. (1) $A, B, C and D$
2. (2) $A and C only$
3. (3) $B only$
4. (4) $B and D only$
116.
Assertion (A) : Na+and Mg2+ ions are isoelectronic but the ionic radius of Na+is greater than that of Mg2+.Reason $(R)$ : The effective nuclear charge of Na+ion is less than that of Mg2+ ion.
1. (1) $Both (A) and (R) are correct but (R) is not the correct explanation of (A).$
2. (2) $Both (A) and (R) are correct and (R) is correct explanation of (A) .$
3. (3) $(A) is not correct but (R) is correct.$
4. (4) $(A) is correct but (R) is not correct.$
117.
Identify the pair of elements with the highest and lowest electronegativity respectively
1. (1) $K and Rb$
2. (2) $I and F$
3. (3) $F and Fr$
4. (4) $Fr and Li$
118.
In which group of the periodic table the element with $Z = 120$ be placed?
1. (1) $2$
2. (2) $1$
3. (3) $14$
4. (4) $15$
119.
In the periodic table from left to right in a period, the atomic volume
1. (1) $decreases$
2. (2) $increases$
3. (3) $remains same$
4. (4) $first decrease then increases.$
120.
In which of the following, the elements $Al, B, Mg$ and $K$ are correctly arranged in the increasing order of their metallic character?
1. (1) $B < Al < Mg < K$
2. (2) $B < Mg < Al < K$
3. (3) $Al < Mg < K < B$
4. (4) $B < Mg < K < Al$