Chemistry - Classification Elements Periodicity Properties - Quiz-9

The correct statement about radius is

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Radius increases during cation and anion formation.
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Radius increases during anion formation and decreases during cation formation.
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Radius decreases in cation as well as anion.
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Radius decreases during anion formation and increases during cation formation.

The values of first ionization enthalpies for two isotopes would be -

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Same.
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Different .
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Same values but positive for first and negative for the second.
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Same values but negative for first and positive for the second.

The general outer electronicconfiguration of s, p, d and f-block elements respectively would be

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ns^1-2, nd²np^1-6, (n-1)d^1-10np^0-2, (n-2)f^1-14(n-1)d^0-10ns²
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ns^1-2, ns²np^1-6, (n-1)f^1-10ns^0-2, (n-2)g^1-14(n-1)d^0-1ns²
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ns^1-2, ns²np^1-6, (n-1)d^1-10ns^1-2, (n-2)f^1-14(n-1)d^0-1ns²
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np^1-2, nd²np^1-6, (n-1)d^1-10ns^0-2, (n-2)f^1-14(n-1)d^0-10ns²

The position of elements with an outer electronic configuration as $(n - 2) f^{7} (n - 1) d^{1} n s^{2}, n = 6$

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6^th period and 10^th group.
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7^th period and 3^rd group.
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6^th period and 3^rd group.
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7^th period and 9^th group.

1st (∆H₁) and 2nd (∆H₂) Ionization Enthalpies (in kJ mol^–1) and the (∆_egH) Electron Gain Enthalpy (in kJ mol^–1) of a few elements are given below:

Elements	ΔH₁	ΔH₂	Δ_egH
I	520	7300	-60
II	419	3051	-48
III	1681	3374	-328
IV	1008	1846	-295
V	2372	5251	+48
VI	738	1451	-40

The most reactive element is -

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VI
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III
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I
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II

The formula of the stable binary compounds that would be formed by an element having atomic number 71 and fluorine-

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LuF₆
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LuF₂
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LuF₃
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LuF₄

The factor that does not affect the valence electron is

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Azimuthal quantum number
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Nuclear charge (Z)
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Nuclear mass
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Number of core electrons

The size of isoelectronic species: F^–, Ne and Na⁺, is affected by :

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Nuclear charge (Z)
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Valence principal quantum number (n)
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Electron-electron interaction in the outer orbitals
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None of the above factors because their size is the same

The incorrect statement about ionization enthalpy is -

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Ionization enthalpy increases for each successive electron.
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Noble gases have the highest ionization enthalpy.
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A big jump in ionization enthalpy indicates a stable configuration.
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Ionization enthalpy of oxygen is higher than that of nitrogen.

The ionic radii vary in-

(a) Inverse proportion to the effective nuclear charge.

(b) Inverse proportion to the square of effective nuclear charge.

(d) Direct proportion to the square of screening effect.

Choose the correct option :

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(a), (c)
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(b), (c)
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(c), (d)
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(b), (d)

Match the following isoelectronic species in column I and column II :

Column I	Column II
i. $F^{-}$	a. ${Br}^{-}$
ii. Ar	b. ${Si}^{2 +}$
iii. $Mg$	c. $O^{2 -}$
iv. ${Rb}^{+}$	d. $S^{2 -}$

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i = b, ii = c, iii = a, iv = d
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i = c, ii = b, iii = a, iv = d
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i = c, ii = d, iii = b, iv = a
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i = b, ii = c, iii = d, iv = a

The correct order of ionization energy of W, X,Y and Z is -

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W >X> Y> Z
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W <X < Y> Z
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W <X> Y< Z
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W >X> Y< Z

Consider the following curve:

X represents group with highest atomic radius. The element that belongs to Y group can be :

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Na
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Mg
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Br
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Si

In the following graph of variation of ionization energy with atomic number, X, Y, and Z represent elements.

The group number of X, Y, and Z elements is:

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1^st group
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15^th group
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17^th group
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18^th group

The graph between ionization energy and atomic number for the first group elements is shown below

The element represented by Y in the graph above is -

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Cs
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Rb
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Ca
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K

Abnormally high ionization enthalpy of B as depicted in the graph below can be due to :

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Completely filled 2p subshell.
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Completely filled 2s subshell.
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Completely filled 3d subshell.
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Completely filled 4f subshell.

The correct graph depicting ionization energies for 2^nd period elements is-

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None of the above.

Correct statement among the following regarding P, S, Cl, F is -

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F has most negative electron gain enthalpy, and S has least negative electron gain enthalpy.
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Cl has most negative electron gain enthalpy, and S has least negative electron gain enthalpy.
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Cl has most negative electron gain enthalpy, and P has least negative electron gain enthalpy.
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F has most negative electron gain enthalpy, and P has least negative electron gain enthalpy.

The formula of a compound that is formed by the aluminium and sulphur is-

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AlS₂
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Al₂S₃
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Al₃S₂
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Al₃S₄

An incorrect properties of p-block elements among the following is -

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Include both metals and non-metals.
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Form mainly covalent bonds with other elements.
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The ionisation enthalpies are relatively lesser than s-block elements.
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Some of the p-block elements show variable or more than one oxidation states.

The correct order of atomic radii of fluorine and neon (in pm) is respectively-

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72, 72
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160, 160
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72, 160
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160, 72

Oxygen has lower ionisation enthalpy than nitrogen due to -

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Half filled p subshell of oxygen atom.
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Half filled p subshell of nitrogen atom.
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Complete filled p subshell of oxygen atom.
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Complete filled p subshell of nitrogen atom.

Factor among the following that doesnot affect the ionization enthalpy of an element is -

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Effective nuclear charge
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2 . Atomic radius
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Half filled and completely filled sub shell
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Atomic number

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Practice Chemistry Quiz Questions and Answers

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Practice Chemistry Quiz Questions and Answers

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