Chemistry - Classification Elements Periodicity Properties - Quiz-5

The graph that represents the relationship between atomic number (Z) and magnetic moment of d-block elements among the following is-

[Outer electronic configuration : $(n - 1) d^{x} n s^{1 o r 2}]$

If the IUPAC name of an element is "unununium",then the correct statement regarding the element is

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It is an inner transition element .
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It belongs to the 8th period in the periodic table .
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It is a transition element .
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It is a non-transition element.

The following property/ies decrease from left to right across the periodic table and increase from top to bottom:

(i) Atomic radius (ii) Electronegativity (iii) Ionisation energy (iv) Metallic character

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(i) only
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(i), (ii), and (iii)
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(i), (iii), and (iv)
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(i), and (iv)

Consider the following information about element P and Q :

Period number Group number

P 2 15

Q 3 2

Then formula of the compound formed by P and Q element is :

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PQ
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$P_{3} Q_{2}$
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$Q_{3} P_{2}$
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$P Q_{2}$

Incorrect order of radius is :

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1
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(1) $S r^{2 +} < {Rb}^{+} < {Br}^{‐} < {Se}^{2 -}$ (2) $Co > Ni > Cu > Zn$
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(3) $Co > {Co}^{2 +} > {Co}^{3 +} > {Co}^{4 +}$ (4) $A s^{3 -} > S e^{2 -} > C s^{+} > B a^{2} +$
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4

The radius of which ion is closest to that of $L i^{+}$ ion ?

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$N a^{+}$
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$B e^{2 +}$
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$M g^{2 +}$
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$A l^{3 +}$

The correct order of ${IE}_{2}$ is:

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Ne>F>O>N
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O>F>Ne>N
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Ne>O>F>N
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O>Ne>F>N

Which of the following transformation least energy is required?

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${F^{-}}_{(g)} \to F_{(g)} + e^{-}$
(2) ${P^{-}}_{(g)} \to P_{(g)} + e^{-}$
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2
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${S^{-}}_{(g)} \to S_{(g)} + e^{-}$
(4) $C {l^{-}}_{(g)} \to C l_{(g)} + e^{-}$
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Which of the following represents correct order of electron affinity?

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Cl>F>S>O
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F>O>S>Cl
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F>Cl>S>O
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Cl>S>O>F

Correct expression of "Allred and Rochow's" scale is:

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() Electronegativity = $0.744 \frac{Z_{e f f .}}{r^{2}} + 0.359$
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() Electronegativity = $0.359 \frac{r^{2}}{Z_{e f f .}} + 0.744$
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() Electronegativity = $0.359 \frac{Z_{e f f .}}{r} + 0.744$
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() Electronegativity = $0.359 \frac{Z_{e f f .}}{r^{2}} + 0.744$

The process that requires absorption of energy is:

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$N \to N^{-}$
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$F \to F^{-}$
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$C l \to C l^{-}$
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$H \to H^{-}$

Which of the following compound is most acidic?

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$C l_{2} O_{7}$
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$P_{4} O_{10}$
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$S O_{3}$
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$B_{2} O_{3}$

If P and T are second period p-block elements then which of the following graph show correct relation between valence electrons in $P_{2}$ to $T_{2}$ (corresponding molecules) and their bond order is :

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()
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()
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()
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()

Consider the following four elements, which are represented according to long form of periodic table.

Here W, Y and Z are left, up and right elements with respect to the element 'X' and 'X' belongs to 16th group and 3rd period.Then according to given information the incorrect statement regarding given elements is:

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Maximum electronegativity :Y
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Maximum catenation property :X
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Maximum electron affinity :Z
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Y exhibits variable covalency

The ground state electronic configurations of the elements, U,V,W,X,and Y (these symbols do not have any chemical significance) are as follows:

$U 1 s^{2} 2 s^{2} 2 p^{3} V 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1} W 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2} X 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{5} 4 s^{2} Y 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6}$

Determine which sequence of elements satisfy the following statements :

(i) Element forms a carbonate that is not decomposed by heating

(ii) Element is most likely to form coloured ionic compounds

(iii) Element has a largest atomic radius

(iv) Element forms an only acidic oxide

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V W Y U
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V X Y W
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V W Y X
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V X W U

Which one will show variable oxidation state?

(I) $[K r] 5 s^{1}$ (II) $[R n] 5 f^{14} 6 d^{1} 7 s^{2}$
(III) $[A r] 3 d^{10} 4 s^{2} 4 p^{5}$ (IV) $[A r] 3 d^{6} 4 s^{2}$

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In alkaline earth metals, the properties, from the following, that will increase from Be to Ba are-

(i) Atomic radius (ii) Ionisation energy (iii) Nuclear charge

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(i) and (ii)
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(i) and (iii)
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(ii) and (iii)
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(i), (ii), and (iii)

Incorrect order of ionic size is :

(a) $L a^{3 +} > G d^{3 +} > E u^{3 +} > L u^{3 +}$ (b) $V^{2 +} > V^{3 +} > V^{4 +} > V^{5 +}$

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Aqueous solutions of two compounds $M_{1} - O - H a n d M_{2} - O - H$ are prepared in two different beakers. If, the electronegativity of $M_{1} = 3.4, M_{2} = 1.2, O = 3.5 a n d H = 2.1,$ then the nature of two solutions will be respectively:

(a) acidic, basic (b) acidic, acidic

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First three ionisation energies (in kJ/mol) of three representative elements are given below:

Element $I E_{1}$ $I E_{2}$ $I E_{3}$

P 495.8 4562 6910
Q 737.7 1451 7733
R 577.5 1817 2745

Then incorrect option is :

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Q: Alkaline earth metal.
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P: Alkali metal.
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R: s-block element.
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All three: P,Q & R belong to the same period.

If the ionization enthalpy and electron gain enthalpy of an element are 275 and 86 kcal $m o l^{- 1}$ respectively, then the electronegativity of the element on the Pauling scale is:

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2.8
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0.0
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4.0
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2.6

The incorrect statement is:

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The second ionisation energy of Se is greater than that of second ionisation energy of As
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The first ionisation energy of $C^{2 +}$ ion is greater than that of first ionisation energy of $N^{2 +}$ ion
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The third ionisation energy of F is greater than that of third ionisation energy of O
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Helogens have highest I.E. in respective period

Consider the following ionisation reactions :

I.E. (kJ $m o l^{- 1}$ )

$A_{(g)} \to A_{(g)}^{+} + e^{-}, A_{1} B_{(g)}^{+} \to B_{(g)}^{2 +} + e^{-}, B_{2} C_{(g)}^{+} \to C_{(g)}^{2 +} + e^{-}, C_{2} B_{(g)} \to B_{(g)}^{+} + e^{-}, B_{1} C_{(g)} \to C_{(g)}^{+} + e^{-}, C_{1} C_{(g)}^{2 +} \to C_{(g)}^{3 +} + e^{-}, C_{3}$

If monovalent positive ion of A, divalent positive ion of B and trivalent positive ion of C have zero electron. Then incorrect order of corresponding I.E. is :

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$C_{3} > C_{2} > B_{2}$
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$B_{1} > A_{1} > C_{1}$
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$C_{3} > C_{2} > B_{2}$
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$B_{2} > C_{3} > A_{1}$

The incorrect match among the following options is :

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$[Ar] 3 d^{5} 4 s^{1} \to 4^{th} period, 6^{th} group$
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$[Kr] 4 d^{10} \to 5^{th} period, 12^{th} group$
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$[Rn] 6 d^{2} 7 s^{2} \to 7^{th} period, 3^{th} group$
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$[Xe] 4 f^{14} 5 d^{2} 6 s^{2} \to 6^{th} period, 4^{th} group$

Which of the following order is correct for the property mentioned in brackets?

$(a) S^{2 -} > C l^{-} > K^{+} > C a^{2 +}$ (Ionisation energy)

$(b) C < N < F < O$ (2nd Ionisation energy)

$(c) B > A l > G a > I n > T l$ (Electronegativity)

$(d) N a^{+} > L i^{+} > M g^{2 +} > B e^{2 +} > A l^{3 +}$ (Ionic radius)

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${IP}_{1}$ and ${IP}_{2}$ for Mg are 178 and 348 Kcal ${mol}^{- 1}$ respectively. The energy required for the reaction, $Mg \to {Mg}^{2 +} + 2 e^{-}$ is :

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+170 Kcal ${mol}^{- 1}$
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+526 Kcal ${mol}^{- 1}$
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-170 Kcal ${mol}^{- 1}$
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-526 Kcal ${mol}^{- 1}$

Incorrect statement about characteristics regarding halogens is :

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Ionization energy decreases with increase in atomic number.
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Electronegativity decreases with increase in atomic number.
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Electron affinity decreases with increase in atomic number.
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Enthalpy of fusion increases with increase in atomic number.

The process requiring the absorption of energy is :

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$F \to F^{-}$
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$H \to H^{-}$
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$C l \to C l^{-}$
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$O \to O^{2 -}$

Consider the following statements:

(I) Rutherford name was associated with the development of periodic table.

(II) A metal M having electronic configuration $1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{6}, 3 d^{10}, 4 s^{1}$ is d-block element.

(III) Diamond is an element.

(IV) The electronic configuration of the most electronegative elements is $1 s^{2}, 2 s^{2}, 2 p^{5},$

and select the correct one from the given codes.

(A) I, II, IV (B) I, II, III, IV

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Which of the following has the highest electron affinity?

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F^–
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O^–
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O
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Na

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Practice Chemistry Quiz Questions and Answers

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Practice Chemistry Quiz Questions and Answers

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