The first ionization enthalpy values (in kJ mol –1 ) of group 13 elements are : B Al Ga In Tl 801 577 579 558 589 The explanation for the deviation from the general trend can be -

Ga has higher ionization enthalpy than Al.

Ga has lower ionization enthalpy than Al.

Al has higher ionization enthalpy than Ga.

Ga has a lesser valence electron than Al.

Chemistry - Classification Elements Periodicity Properties - Quiz-8

Electronic configuration of four elements A, B, C and D are given below :

A. $1 s^{2} 2 s^{2} 2 p^{6}$

B. $1 s^{2} 2 s^{2} 2 p^{4}$

C. $1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$

D. $1 s^{2} 2 s^{2} 2 p^{5}$

The correct order of increasing tendency to gain electron is :

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A < C < B < D
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A < B < C < D
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D < B < C < A
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D < A < B < C

Which of the following oxides is most acidic in nature?

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${Na}_{2} O$
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MgO
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${SiO}_{2}$
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${Cl}_{2} O_{7}$

Match the element in column I with that in column II.
Column-I Column-II

(a) Copper (i) Non-metal

(b) Fluorine (ii) Transition metal

(d) Cerium (iv) Metalloid

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(a)-(ii), (b)-(iv), (c)-(i), (d)-(iii)
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(a)-(ii), (b)-(i), (c)-(iv), (d)-(iii)
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(a)-(iv), (b)-(iii), (c)-(i), (d)-(ii)
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(a)-(i), (b)-(ii), (c)-(iii), (d)-(iv)

Among the elements Ca, Mg, P and Cl, the order of increasing atomic radii is -

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Cl < P < Mg < Ca
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P < Cl < Ca < Mg
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Ca < Mg < P < Cl
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Mg < Ca < Cl < P

What is the value of electron gain enthalpy of Na⁺ if IE₁ of Na = 5.1 eV?

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+ 10.2 eV
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–5.1 eV
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–10.2 eV
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+ 2.55 eV

The formula for the oxide formed by Eka-aluminum is:

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${EO}_{4}$
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$E_{2} O_{3}$
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$E_{3} O_{2}$
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EO

In which of the following molecule,the internuclear distance will be maximum :

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CsI
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CsF
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LiF
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LiI

The first ionization potential of Be and B will be-

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8.8 and 8.8
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6.6 and 6.6
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6.6 and 8.8
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8.8. and 6.6

An electronic configuration that has maximum difference between II and III ionization potential is - :

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$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1}$
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$1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}$
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$1 s^{2} 2 s^{2} 2 p^{6}$
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$1 s^{2} 2 s^{2} 2 p^{5}$

Incorrect order among the following is : -

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NH₃ < PH₃ < AsH₃ – Acidic
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Li < Be < B < C – I^st I.P.
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Al₂O₃ < MgO < Na₂O < K₂O - Basic
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Li⁺ < Na⁺ < K⁺ < Cs⁺ - Ionic radius

An atom has electronic configuration 1s²2s²2p⁶3s²3p⁶3d³4s², you will place it in which group : -

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Fifteenth
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Second
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Third
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Fifth

Correct order of $I^{s t}$ IP among following elements Be, B, C, N, O is : -

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B < Be < C < O < N
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B < Be < C < N < O
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Be < B < C < N < O
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Be < B < C < O < N

The basic theme of the periodic table is

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To classify the elements in a period according to their properties.
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To classify the elements in a group according to their ionization enthalpy.
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To classify the elements in periods and groups according to their properties.
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To classify the elements in periods and groups according to their lustre.

Property used by Mendeleev to classify the elements was -

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Brightness
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Atomic weight or mass
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Number of isotopes
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Lustre

The basic difference between Mendeleev’s Periodic Law (A) and Modern Periodic Law (B) is

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A is based on atomic weights while B is based on atomic numbers.
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B is based on atomic weights while A is based on atomic numbers.
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A is based on the number of isotopes while B is based on atomic numbers.
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A is based on physical properties while B is based on chemical properties.

The number of elements in the 6th period of the periodic table is-

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32
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36
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35
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33

The period and group number of the element with Z =114 are

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8th period and 16th group
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7th period and 14th group
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14th period and 7th group
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7th group and 14th period

The atomic number of the element present in the 3rd period and 17th group of the periodic table would be -

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18
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23
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24
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17

The similarity in physical and chemical properties in a group of periodic table is due to the -

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Same atomic number
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Same number of valence electrons.
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Same atomic mass
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Same number of isotopes

The ionic radius indicates the distance between the nucleus and

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outermost shell of an atom
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outermost shell of an ion
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outermost shell of the cation only
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outermost shell of the anion only

The trend of atomic radius in a period and a group is :

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Generally decreases from right to left across a period and increases down a group.
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Generally increases from left to right across a period and decreases down a group.
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Generally decreases from left to right across a period and increases down a group.
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Generally remains same from left to right across a period and increases down a group.

Anions are larger in radii than their parent atoms because -

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An anion has a fewer number of electrons than its parent atom
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An anion has the same number of electrons as its parent atom.
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An anion has a higher effective nuclear charge.
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An anion has more electrons than its parent atom

The energy of an electron in the ground state of the hydrogen atom is $- 2.18 \times 10^{- 18} J$ . The ionization enthalpy of atomic hydrogen in terms of J ${mol}^{- 1}$ is -

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2.81 × 10⁶J mol $^{- 1}$
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1.31 × 10⁶J mol $^{- 1}$
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2.31 × 10⁶J mol $^{- 1}$
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1.81 × 10⁶J mol $^{- 1}$

The explanation for the fact that the first ionization enthalpy of sodium is lower than that of magnesium but its second ionization enthalpy is higher than that of magnesium would be -

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pressure and volume
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lustre and brightness
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atomic size and effective nuclear charge
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availability in nature

The ionization enthalpy of the main group elements tends to decrease down a group due to,

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Increase in the atomic size of elements and increase in the shielding effect
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Decrease in the atomic size of elements and increase in the shielding effect
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Increase in the atomic size of elements and decrease in the shielding effect
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Decrease in the atomic size of elements and decrease in the shielding effect

The first ionization enthalpy values (in kJ mol^–1) of group 13 elements are :

B	Al	Ga	In	Tl
801	577	579	558	589

The explanation for the deviation from the general trend can be -

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Ga has lower ionization enthalpy than Al.
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Ga has higher ionization enthalpy than Al.
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Al has higher ionization enthalpy than Ga.
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Ga has a lesser valence electron than Al.

An element with higher negative electron gain enthalpy in the given pair is-

(i) O or F (ii) F or Cl

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O, Cl
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F, F
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O, F
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F, Cl

The relationship between 1^st and 2 ^nd electron gain enthalpy of oxygen atom (O) would be -

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Both values of electron gain enthalpy are negative.
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The 1^st electron gain enthalpy of (O) is negative while 2 ^nd is positive.
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Both values of electron gain enthalpies are positive.
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The 1^st electron gain enthalpy of (O) is positive while 2 ^nd is negative.

The basic difference between the terms electron gain enthalpy (E_a) and electronegativity (E_N) is -

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E_ais the tendency to lose electrons while E_N is the tendency to repel the shared pairs of electrons.
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E_a is the tendency to gain neutrons while E_N is the tendency to attract the shared pairs of electrons.
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E_ais the tendency to donate electrons while E_N is the tendency to attract the shared pairs of molecules.
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E_a is the tendency to gain electrons while E_N is the tendency to attract the shared pairs of electrons.

The statement that "the electronegativity of N on the Pauling scale is 3.0 in all the nitrogen compounds" is incorrect because -

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Electronegativity of an element is a variable property.
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Pauling scale is not used to measure electronegativity.
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The electronegativity of N on the Pauling scale is 12.0
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None of the above.

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Practice Chemistry Quiz Questions and Answers

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Practice Chemistry Quiz Questions and Answers

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