Periodic Table & Periodicity PYQs Set 10 (PDF)

Set 10 of 11 · Questions 271-300 of 322

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NEET Chemistry · Periodic Table & Periodicity · Set 10 (Q271-300)

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271.
The general formula of the compound formed when a metal (M) of group-1 reacts with non metal (x) of group-16 is
1. (1) $MX_{6}$
2. (2) $M_{2} X_{3}$
3. (3) $MX_{2}$
4. (4) $M_{2} X$
272.
The incorrect decreasing order of atomic radii is
1. (1) $Si > P > Cl > F$
2. (2) $Be > Mg > Al > Si$
3. (3) $Al > B > N > F$
4. (4) $Mg > Al > C > O$
273.
The absolute value of the electron gain enthalpy of halogens satisfies:
1. (1) $I >Br > Cl > F$
2. (2) $Cl > Br > F > I$
3. (3) $Cl > F > Br > I$
4. (4) $F > Cl > Br > I$
274.
$Match List-I with List-II (Electronic Configuration of Element) ∆_{i} H in kJ mo l^{- 1}$
$List I$ $List II$
$(1)1s²2s²$ $(i)801$
$(2) 1 s^{2} 2 s^{2} 2 p^{4}$ $(ii)899$
$(3) 1 s^{2} 2 s^{2} 2 p^{3}$ $(iii)1314$
$(4) 1 s^{2} 2 s^{2} 2 p^{1}$ $(iv)1402$
1. (1) $(1)-(ii), (b)-(iii), (c)-(iv), (d)-(i)$
2. (2) $(1)-(iv), (b)-(i), (c)-(ii), (d)-(iii)$
3. (3) $(1)-(i), (b)-(iv), (c)-(iii), (d)-(ii)$
4. (4) $(1)-(i), (b)-(iii), (c)-(iv), (d)-(ii)$
275.
The correct order of electron gain enthalpy is:
1. (1) $S > Se >Te> O$
2. (2) $O > S > Se >Te$
3. (3) $S > O > Se >Te$
4. (4) $Te> Se > S > O$
276.
The correct order of electronegativity of carbon in various hybridisation states is
1. (1) $sp < s p^{2} < s p^{3}$
2. (2) $sp > s p^{2} > s p^{3}$
3. (3) $s p^{2} > sp < s p^{3}$
4. (4) $sp = s p^{2} < s p^{3}$
277.
The atomic number of the element unnilennium is
1. (1) $109$
2. (2) $119$
3. (3) $102$
4. (4) $108$
278.
The outer electron configuration of Gd (Atomic No: 64) is:
1. (1) $4 f^{3} 5 d^{5} 6 s^{2}$
2. (2) $4 f^{8} 5 d^{0} 6 s^{2}$
3. (3) $4 f^{4} 5 d^{4} 6 s^{2}$
4. (4) $4 f^{7} 5 d^{1} 6 s^{2}$
279.
The third ionization enthalpy is minimum for:
1. (1) $Mn$
2. (2) $Co$
3. (3) $Fe$
4. (4) $Ni$
280.
Metals generally melt at very high temperature. Amongst the following, the metal with the highest melting point will be
1. (1) $Hg$
2. (2) $Ag$
3. (3) $Ga$
4. (4) $Cs$
281.
When the first electron gain enthalpy ( $D_{e g}$ H) of oxygen is –141 kJ/mol, its second electron gain enthalpy is:
1. (1) $almost the same as that of the first$
2. (2) $negative, but less negative than the first$
3. (3) $a more negative value than the first$
4. (4) $a positive value$
282.
In the periodic table metals usually used as catalysts belong to
1. (1) $f-block$
2. (2) $d -block$
3. (3) $p-block$
4. (4) $s-block.$
283.
Identify the wrong statement in the following :
1. (1) $Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the ionic radius.$
2. (2) $Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius.$
3. (3) $Atomic radius of the elements increases as one moves down the first group of the periodic table.$
4. (4) $Atomic radius of the elements decreases as one moves across from left to right in the 2nd period of the periodic table$
284.
For the properties mentioned, the correct trend for the different species is in
1. (1) $strength as Lewis acid - BCl_{3} > AlCl_{3} > GaCl_{3}$
2. (2) $inert pair effect - Al > Ga > In$
3. (3) $oxidising property - Al^{3 +} > In^{3 +} > Tl^{3 +}$
4. (4) $first ionization enthalpy - B > Al > TI$
285.
Which of the following statements are correct?
(A) The process of adding an electron to a neutral gaseous atom is always exothermic.(B) The process of removing an electron from an isolated gaseous atom is always endothermic.(C) The $1^{st}$ ionization energy of boron is less than that of beryllium.(D) The electronegativity of C is 2.5 in $CH_{4}$ and $CCl_{4}$ (E) Li is the most electropositive among elements of group I.
Choose the correct answer from the options given below:
1. (1) $A, C and D Only$
2. (2) $B and C Only$
3. (3) $B and D Only$
4. (4) $B, C and E Only$
286.
The electronic configurations of Eu (Atomic No. 63) Gd (Atomic No. 64) and Tb (Atomic No. 65) are :
1. (1) $[Xe]4f76s2, [Xe]4f75d16s2 and [Xe]4f96s2$
2. (2) $[Xe]4f76s2, [Xe]4f8 6s2 and [Xe]4f8 5d16s2$
3. (3) $[Xe]4f6 5d16s2, [Xe]4f7 5d16s2 and [Xe]4f9 5d16s2$
4. (4) $[Xe]4f6 5d16s2, [Xe]4f7 5d16s2 and [Xe]4f8 5d16s2$
287.
Consider the following elements.

Which of the following is/are true about $A^{’}, B^{’}, C^{’}$ and $D^{’}$ ?
A. Order of atomic radii: $B^{’} < A^{’} < D^{’} < C^{’}$
B. Order of metallic character: $B^{’} < A^{’} < D^{’} < C^{’}$
C. Size of the element: $D^{’} < C^{’} < B^{’} < A^{’}$
D. Order of ionic radii : $B^{’ +} < A^{’ +} < D^{’ +} < C^{’ +}$
Choose the correct answer from the options given below :
1. (1) $A only$
2. (2) $A, B and D only$
3. (3) $A and B only$
4. (4) $B, C and D only$
288.
For the second period elements the correct increasing order of first ionization enthalpy is :
1. (1) $Li < Be < B < C < O < N < F < Ne$
2. (2) $Li < Be < B < C < N < O < F < Ne$
3. (3) $Li < B < Be < C < O < N < F < Ne$
4. (4) $Li < B < Be < C < N < O < F < Ne$
289.
Match List - I with List - II :
$List - I (A) NaOH (B) Be (OH)_{2} (C) Ca (OH)_{2} (D) B (OH)_{3} (E) Al (OH)_{3} List - II (i) Acidic (ii) Basic (iii) Amphoteric$
Choose the most appropriate answer from the options given below
1. (1) $(A)-(ii),(B)-(ii), (C)-(iii), (D)-(ii), (E)-(iii)$
2. (2) $(A)-(ii), (B)-(iii), (C)-(ii), (D)-(i), (E)-(iii)$
3. (3) $(A)-(ii), (B)-(ii), (C)-(iii), (D)-(i), (E)-(iii)$
4. (4) $(A)-(ii), (B)-(i), (C)-(ii), (D)-(iii), (E)-(iii)$
290.
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. (1) $E < C < A < B < D$
2. (2) $C < E < A < B < D$
3. (3) $B < D < C < E < A$
4. (4) $A < B < D < C < E$
291.
Identify the correct statement.
1. (1) $Lead forms compounds in +2 oxidation state due to inert pair effect$
2. (2) $All halogens show only negative oxidation state$
3. (3) $Catenation property increases from boron to oxygen$
4. (4) $Oxidation state of oxygen is -1 in ozonides$
292.
Ionic radii of:
1. (1) $T i^{4 +} < M n^{7 +}$
2. (2) $^{35} C l^{-} <^{37} C l^{-}$
3. (3) $K^{+} > C l^{-}$
4. (4) $P^{3 +} > P^{5 +}$
293.
$N d^{2 +}$ =_______
1. (1) $4 f^{2} 6 s^{2}$
2. (2) $4 f^{4}$
3. (3) $4 f^{3}$
4. (4) $4 f^{4} 6 s^{2}$
294.
The first ionization enthalpy of the following elements are in the order:
1. (1) $C < N < Si < P$
2. (2) $P < Si < C <N$
3. (3) $P < Si < N < C$
4. (4) $Si < P < C <N$
295.
Atomic radius of $Ag$ is similar to
1. (1) $Cu$
2. (2) $Hg$
3. (3) $Au$
4. (4) $Ni$
296.
$H^{+}$ ion always get associated with other atoms or molecules. This is because
1. (1) $Ionisation enthalpy of hydrogen resembles that of alkali metals.$
2. (2) $Its reactivity is similar to halogens.$
3. (3) $It resembles both alkali metals and halogens.$
4. (4) $Loss of an electron from hydrogen atom results in a nucleus of very small size as compared to other atoms or ions$
297.
Consider the following statements :
I. The radius of an anion is larger than that of the parent atom.
II. The ionization energy generally increases with increasing atomic number in a period.
III. The electronegativity of an element is the tendency of an isolated atom no attract an electron.
Which of the above statements is/are correct?
1. (1) $I alone$
2. (2) $II alone$
3. (3) $I and II$
4. (4) $II and III$
298.
Match the following.
$List I A. Rubidium B. Platinum C. Eka-silicon D. Polonium List II (1) Germanium (2) Radioactive chalcogen (3) s-block element (4) Atomic number 78$
A B C D
1. (1) $4 3 2 1$
2. (2) $3 4 1 2$
3. (3) $2 1 4 3$
4. (4) $4 3 1 2$
299.
What is the atomic number of the element with symbol Uus?
1. (1) $117$
2. (2) $116$
3. (3) $115$
4. (4) $114$
300.
Similarity in chemical properties of the atoms of elements in a group of the periodic table is most closely related to:
1. (1) $atomic numbers$
2. (2) $atomic masses$
3. (3) $number of principal energy levels$
4. (4) $number of valence electrons$