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question_answer1)
\[N{{a}^{+}},\ M{{g}^{2+}},A{{l}^{3+}}\] and \[S{{i}^{4+}}\] are isoelectronic. The order of their ionic size is
A)
\[N{{a}^{+}}>\ M{{g}^{2+}}<A{{l}^{3+}}<S{{i}^{4+}}\] done
clear
B)
\[N{{a}^{+}}<\ M{{g}^{2+}}>A{{l}^{3+}}>S{{i}^{4+}}\] done
clear
C)
\[N{{a}^{+}}>\ M{{g}^{2+}}>A{{l}^{3+}}>S{{i}^{4+}}\] done
clear
D)
\[N{{a}^{+}}<\ M{{g}^{2+}}>A{{l}^{3+}}<S{{i}^{4+}}\] done
clear
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question_answer2)
Consider the following changes \[A\to {{A}^{+}}+{{e}^{-}}:{{E}_{1}}\] and \[{{A}^{+}}\to {{A}^{2+}}+{{e}^{-}}:{{E}_{2}}\]. |
The energy required to pull out the two electrons are \[{{E}_{1}}\] and \[{{E}_{2}}\] respectively. The correct relationship between two energies would be |
A)
\[{{E}_{1}}<{{E}_{2}}\] done
clear
B)
\[{{E}_{1}}={{E}_{2}}\] done
clear
C)
\[{{E}_{1}}>{{E}_{2}}\] done
clear
D)
\[{{E}_{1}}\ge {{E}_{2}}\] done
clear
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question_answer3)
The elements with zero electron affinity are
A)
Boron and Carbon done
clear
B)
Beryllium and Helium done
clear
C)
Lithium and Sodium done
clear
D)
Fluorine and Chlorine done
clear
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question_answer4)
Ionization energies of atoms A and B are 400 and \[300\text{ }k\text{ }cal\text{ }mo{{l}^{-1}}\] respectively. The electron affinities of these atoms are 80.0 and \[85.0\text{ }k\text{ }cal\,mo{{l}^{-1}}\] respectively. Then which is the correct statement regarding electronegativity\[\chi \]?
A)
\[{{\chi }_{A}}<{{\chi }_{B}}\] done
clear
B)
\[{{\chi }_{A}}>{{\chi }_{B}}\] done
clear
C)
\[{{\chi }_{A}}={{\chi }_{B}}\] done
clear
D)
none of these done
clear
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question_answer5)
The set of three elements having successive atomic numbers and having the ionization energies of 2372, 520 and \[890\text{ }kJ\] per mol is
A)
H, He, Li done
clear
B)
He, Li, Be done
clear
C)
Li, Be, B done
clear
D)
B, C, N done
clear
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question_answer6)
Similarity in chemical properties of the atoms of elements in a group of the Periodic table is most closely related to:
A)
atomic numbers done
clear
B)
atomic masses done
clear
C)
number of principal energy levels done
clear
D)
number of valence electrons done
clear
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question_answer7)
In the long form of the periodic table, the valence shell electronic configuration of \[5{{s}^{2}}5{{p}^{4}}\] corresponds to the element present in:
A)
Group 16 and period 6 done
clear
B)
Group 17 and period 6 done
clear
C)
Group 16 and period 5 done
clear
D)
Group 17 and period 5 done
clear
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question_answer8)
Consider the following ionization enthalpies of two elements 'A' and 'B'.
| Elements 1st | Lionization 2nd | Enthalpy (KJ/mol) |
A | 899 | 1757 | 14847 |
B | 737 | 1450 | 7731 |
Which of the following statements is correct?
A)
Both 'A' and 'B' belong to group-1 where 'B' comes below 'A'. done
clear
B)
Both 'A' and 'B' belong to group-1 where 'A' comes below 'B. done
clear
C)
Both 'A' and 'B' belong to group-2 where 'B' comes below 'A'. done
clear
D)
Both 'A' and 'B' belong to group-2 where 'A' comes below 'B'. done
clear
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question_answer9)
Sum of first three ionization energies of Al is \[53.0\text{ }eV\text{ }ato{{m}^{-1}}\] and the sum of first two ionization energies of Na is \[52.2\text{ }eV\text{ }ato{{m}^{-1}}.\] Out of Al(III) and Na(II)
A)
Na (II) is more stable than Al (III) done
clear
B)
Al (III) is more stable than Na (II) done
clear
C)
Both are equally stable done
clear
D)
Both are equally unstable done
clear
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question_answer10)
Which pair of elements belongs to same group?
A)
Elements with atomic no. 17 and 38 done
clear
B)
Elements with atomic no. 20 and 40 done
clear
C)
Elements with atomic no. 17 and 53 done
clear
D)
Elements with atomic no. 11 and 33 done
clear
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question_answer11)
In a given energy level, the order of penetration effect of different orbitals is
A)
\[f<d<p<s\] done
clear
B)
\[s=p=d=f\] done
clear
C)
\[s<p<d<f\] done
clear
D)
\[p>s>d>f\] done
clear
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question_answer12)
Consider the following changes:
(1) \[M\left( s \right)\xrightarrow{{}}M\left( g \right)\] |
(2) \[M(s)\xrightarrow{{}}{{M}^{2+}}(g)+2{{e}^{-}}\] |
(3) \[M(g)\xrightarrow{{}}{{M}^{+}}(g)+{{e}^{-}}\] |
(4) \[{{M}^{+}}(g)\xrightarrow{{}}{{M}^{2+}}(g)+{{e}^{-}}\] |
(5) \[M\left( g \right)\xrightarrow{{}}{{M}^{2+}}\left( g \right)+2{{e}^{-}}\] |
The second ionization energy of M could be calculated from the energy values associated with: |
A)
\[1+3+4\] done
clear
B)
\[~2-1+3\] done
clear
C)
\[1+5\] done
clear
D)
\[5-3\] done
clear
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question_answer13)
The correct order of decreasing electronegativity values among the elements I-beryllium, II-oxygen, III-nitrogen and IV-magnesium is
A)
\[II>III>I>IV\] done
clear
B)
\[III>IV>II>I\] done
clear
C)
\[I>II>III>IV\] done
clear
D)
\[I>II>IV>III\] done
clear
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question_answer14)
What is the order of ionisation energies of the coinage metal
A)
\[Cu>Ag<Au\] done
clear
B)
\[Cu>Ag>Au\] done
clear
C)
\[Cu<Ag<Au\] done
clear
D)
\[Au>Ag<Cu\] done
clear
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question_answer15)
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:
A)
Q: Alkaline earth metal done
clear
B)
P: Alkali metals done
clear
C)
R: s-block element done
clear
D)
They belong to same period done
clear
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question_answer16)
What is the correct order of electronegativity?
A)
\[{{M}^{-}}<{{M}^{2-}}<\text{ }{{M}^{3-}}<{{M}^{4-}}\] done
clear
B)
\[{{M}^{-}}>{{M}^{2}}^{-}>{{M}^{3}}^{-}>{{M}^{4}}^{-}\] done
clear
C)
\[{{M}^{-}}<{{M}^{2-}}>{{M}^{3-}}<{{M}^{4-}}\] done
clear
D)
\[{{M}^{4-}}<{{M}^{2-}}<{{M}^{3-}}<{{M}^{-}}\] done
clear
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question_answer17)
The chemistry of lithium is very similar to that of magnesium even though they are placed in different groups. Its reason is:
A)
Both are found together in nature done
clear
B)
Both have nearly the same size done
clear
C)
Both have similar electronic configuration done
clear
D)
The ratio of their charge and size (i.e. charge density) is nearly the same done
clear
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question_answer18)
Which of the following sequence correctly represents the decreasing acidic nature of oxides?
A)
\[L{{i}_{2}}O>BeO>{{B}_{2}}{{O}_{3}}>C{{O}_{2}}>{{N}_{2}}{{O}_{3}}\] done
clear
B)
\[{{N}_{2}}{{O}_{3}}>C{{O}_{2}}>{{B}_{2}}{{O}_{3}}>BeO>L{{i}_{2}}O\] done
clear
C)
\[C{{O}_{2}}>{{N}_{2}}{{O}_{3}}>{{B}_{2}}{{O}_{3}}>BeO>L{{i}_{2}}O\] done
clear
D)
\[{{B}_{2}}{{O}_{3}}>C{{O}_{2}}>{{N}_{2}}{{O}_{3}}>L{{i}_{2}}O>BeO\] done
clear
View Solution play_arrow
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question_answer19)
Correct order of first IP among following elements Be, B, C, N, O is
A)
\[B<Be<C<O<N\] done
clear
B)
\[B<Be<C<N<O\] done
clear
C)
\[Be<B<C<N<O\] done
clear
D)
\[Be<B<C<O<N\] done
clear
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question_answer20)
In which of the following process highest energy is absorbed?
A)
\[Cu\to C{{u}^{+}}\] done
clear
B)
\[Br\to B{{r}^{-}}\] done
clear
C)
\[~I\to {{I}^{-}}\] done
clear
D)
\[Li\to L{{i}^{-}}\] done
clear
View Solution play_arrow
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question_answer21)
The correct order of acidic strength:
A)
\[C{{l}_{2}}{{O}_{7}}>S{{O}_{2}}>{{P}_{4}}{{O}_{10}}\] done
clear
B)
\[{{K}_{2}}O>CaO>MgO\] done
clear
C)
\[C{{O}_{2}}>{{N}_{2}}{{O}_{5}}>S{{O}_{3}}\] done
clear
D)
\[N{{a}_{2}}O>MgO>A{{l}_{2}}{{O}_{3}}\] done
clear
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question_answer22)
An element of atomic weight 40 has 2, 8, 8, 2 as the electronic configuration. Which one of the following statements regarding this element is not correct?
A)
it belongs to II group of the periodic table done
clear
B)
it has 20 neutrons done
clear
C)
the formula of its oxide is \[M{{O}_{2}}\] done
clear
D)
it belongs to 4th period of the periodic table done
clear
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question_answer23)
Which of the following series correctly represents relations between the elements from X to Y?
A)
\[{}_{3}Li\to {}_{19}K\] Ionization enthalpy increases done
clear
B)
\[{}_{9}F\to {}_{35}Br\] Electron gain enthalpy (negative sign) increases done
clear
C)
\[{}_{6}C\to {}_{32}Ge\] Atomic radii increases done
clear
D)
\[~{}_{18}Ar\to {}_{54}Xe\] Noble character increases done
clear
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question_answer24)
Which of the following arrangements represents the increasing order (smallest to largest) of ionic radii of the given species\[{{O}^{2-}},{{S}^{2-}},{{N}^{3-}},{{P}^{3-}}\]?
A)
\[{{O}^{2-}}<{{N}^{3-}}<{{S}^{2-}}<{{P}^{3-}}\] done
clear
B)
\[{{O}^{2-}}<{{P}^{3-}}<{{N}^{3-}}<{{S}^{2-}}\] done
clear
C)
\[{{N}^{3}}<{{O}^{2-}}<{{P}^{3-}}<{{S}^{2-}}\] done
clear
D)
\[{{N}^{3-}}<{{S}^{2-}}<{{O}^{2-}}<{{P}^{3-}}\] done
clear
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question_answer25)
Which one of the following has largest ionic radius?
A)
\[L{{i}^{+}}\] done
clear
B)
\[O_{2}^{2-}\] done
clear
C)
\[{{B}^{3+}}\] done
clear
D)
\[~{{F}^{-}}\] done
clear
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question_answer26)
Elements X, Y and Z have atomic numbers 19, 37 and 55 respectively. Which of the following statements is true about them?
A)
Their ionization potential would increase with increasing atomic number done
clear
B)
'Y' would have an ionisation potential between those of 'X' and 'Z' done
clear
C)
'Z' would have the highest ionization potential done
clear
D)
'Y' would have the highest ionization potential. done
clear
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question_answer27)
An element X occurs in short period having configuration \[n{{s}^{2}}n{{p}^{1}}\]. The formula and nature of its oxide is
A)
\[X{{O}_{3}}\], basic done
clear
B)
\[X{{O}_{3}}\] acidic done
clear
C)
\[{{X}_{2}}{{O}_{3}},\] amphoteric done
clear
D)
\[{{X}_{2}}{{O}_{3}}\]basic done
clear
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question_answer28)
The decreasing order of the ionization potential of the following elements is
A)
\[Ne>Cl>P>S>Al>Mg\] done
clear
B)
\[Ne>Cl>P>S>Mg>Al\] done
clear
C)
\[Ne>Cl>S>P>Mg>Al\] done
clear
D)
\[Ne>Cl>S>P>Al>Mg\] done
clear
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question_answer29)
The incorrect statement among the following is
A)
the first ionization potential of Al is less than the first ionization potential of Mg done
clear
B)
the second ionization potential of Mg is greater than the second ionization potential of Na done
clear
C)
the first ionization potential of Na is less than the first ionization potential of Mg done
clear
D)
the third ionization potential of Mg is greater than the third ionization potential of Al. done
clear
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question_answer30)
The screening effect of inner electrons of the nucleus causes
A)
decrease in the ionization energy done
clear
B)
increase in the ionization energy done
clear
C)
no effect on the ionization energy done
clear
D)
increases the attraction of the nucleus for the electrons done
clear
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question_answer31)
The order of increasing sizes of atomic radii among the elements O, S, Se and As is:
A)
\[As<S<O<Se\] done
clear
B)
\[Se<S<As<O\] done
clear
C)
\[O<S<As<Se\] done
clear
D)
\[O<S<Se<As\] done
clear
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question_answer32)
Which is the correct order of second ionization potential of \[C,\text{ }N,\text{ O}\] and F in the following?
A)
\[O>N>F>C\] done
clear
B)
\[O>F>N>C\] done
clear
C)
\[F>O>N>C\] done
clear
D)
\[C>N>O>F\] done
clear
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question_answer33)
The first \[({{\Delta }_{i}}{{H}_{1}})\] and second \[({{\Delta }_{i}}{{H}_{2}})\] ionization enthalpies (in \[kJ\text{ }mo{{l}^{-1}}\]) and the electron gain enthalpy \[({{\Delta }_{eg}}H)\] (in \[kg\,\,mo{{l}^{-1}}\]) of the elements I, II, III, IV and V are given below.
Element |
\[{{\Delta }_{i}}{{H}_{1}}\] |
\[{{\Delta }_{i}}{{H}_{2}}\] |
\[{{\Delta }_{eg}}H\] |
I |
520 |
7300 |
\[-\,60\] |
II |
419 |
3051 |
\[-\,48\] |
III |
1681 |
3374 |
\[-\,328\] |
IV |
1008 |
1846 |
\[-\,295\] |
V |
2372 |
5251 |
+48 |
The most reactive metal and the least reactive non-metal of these are respectively
A)
I and V done
clear
B)
V and II done
clear
C)
II and V done
clear
D)
IV and V done
clear
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question_answer34)
Aqueous solutions of two compounds \[{{M}_{1}}-O-H\] and \[{{M}_{2}}-O-H\] are prepared in two different beakers. If, the electronegativity of \[{{M}_{1}}=3.4,\]\[{{M}_{2}}=1.2,\,\,O=3.5\] and \[H=2.1\] then the nature of two solutions will be respectively:
A)
acidic, basic done
clear
B)
acidic, acidic done
clear
C)
basic, acidic done
clear
D)
basic, basic done
clear
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question_answer35)
An element having electronic configuration \[1{{s}^{2}}2{{s}^{2}}2{{p}^{6}}3{{s}^{2}}3{{p}^{6}}4{{s}^{1}}\] forms
A)
Acidic oxide done
clear
B)
Basic oxide done
clear
C)
Amphoteric oxide done
clear
D)
Neutral oxide done
clear
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question_answer36)
The van der Waal and covalent radii of fluorine atom respectively from the following figure are.
A)
219 pm, 72 pm done
clear
B)
75 pm, 72 pm done
clear
C)
147 pm, 72 pm done
clear
D)
147 pm, 144 pm done
clear
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question_answer37)
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:
A)
Maximum electronegativity: Y done
clear
B)
Maximum catenation property: X done
clear
C)
Maximum electron affinity: Z done
clear
D)
Y exhibits variable covalency done
clear
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question_answer38)
The electron affinity of chlorine is 3.7 eV. 1 g of chlorine is completely converted to \[C{{l}^{-}}\]ion in a gaseous state.\[\left( 1\text{ }eV=23.06\,Kcal\text{ }mo{{l}^{-1}} \right)\]. Energy released in the process is
A)
4.8 kcal done
clear
B)
7.2 kcal done
clear
C)
8.2 kcal done
clear
D)
2.4 kcal done
clear
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question_answer39)
In which of the following arrangements, the sequence is not strictly according to the property written against it?
A)
\[C{{O}_{2}}<Si{{O}_{2}}<Sn{{O}_{2}}<Pb{{O}_{2}}\]: increasing oxidising power done
clear
B)
\[N{{H}_{3}}<P{{H}_{3}}<As{{H}_{3}}<Sb{{H}_{3}}:\] increasing basic strength done
clear
C)
\[HF<HCl<HBr<HI:\] increasing acid strength done
clear
D)
\[B<C<O<N:\] increasing first ionisation enthalpy. done
clear
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question_answer40)
Which among the following elements has the highest first ionization enthalpy?
A)
Nitrogen done
clear
B)
Boron done
clear
C)
Carbon done
clear
D)
Oxygen done
clear
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question_answer41)
Which of the following is not the correct order for the stated property?
A)
\[Ba>Sr>\]Mg; atomic radius done
clear
B)
\[F>O>N:\] first ionization enthalpy done
clear
C)
\[Cl>F>I;\] electron affinity done
clear
D)
\[O>Se>Te;\] electronegativity done
clear
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question_answer42)
The increasing order of electron affinity of N, P and As is
A)
N<P<As done
clear
B)
As <P<N done
clear
C)
As<N<P done
clear
D)
As<N>P done
clear
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question_answer43)
Which of the following ionisation energy values for calcium show a sudden increase?
A)
Third done
clear
B)
Second done
clear
C)
First done
clear
D)
Fourth done
clear
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question_answer44)
The electronegativity follows the order
A)
\[F>O>Cl>Br\] done
clear
B)
\[~F>Cl>Br>O\] done
clear
C)
\[~O>F>Cl>Br\] done
clear
D)
\[~Cl>F>O>Br\] done
clear
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question_answer45)
The first ionisation potential of aluminium is smaller than that of magnesium because
A)
Atomic size of Al > Atomic size of Mg. done
clear
B)
Atomic size of Al < Atomic size of Mg. done
clear
C)
Al has one electron in p - orbital done
clear
D)
None of these done
clear
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question_answer46)
Which one of the following statements is incorrect in relation to ionisation enthalpy?
A)
Ionisation enthalpy increases for each successive electron. done
clear
B)
The greatest increase in ionisation enthalpy is experienced on removal of electron from core noble gas configuration. done
clear
C)
End of valence electrons is marked by a big jump in ionisation enthalpy. done
clear
D)
Removal of electron from orbitals bearing lower n value is easier than from orbital having higher n value. done
clear
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question_answer47)
Highest electron affinity is shown by
A)
\[{{O}^{-}}\] done
clear
B)
\[{{F}^{-}}\] done
clear
C)
\[C{{l}_{2}}\] done
clear
D)
\[~{{F}_{2}}\] done
clear
View Solution play_arrow
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question_answer48)
Which of the following order is wrong?
A)
\[N{{H}_{3}}<P{{H}_{3}}<As{{H}_{3}}-Acidic\] done
clear
B)
\[Li<Be<B<C-I{{E}_{1}}\] done
clear
C)
\[A{{l}_{2}}{{O}_{3}}<MgO<N{{a}_{2}}O<{{K}_{2}}O-Basic\] done
clear
D)
\[L{{i}^{+}}<N{{a}^{+}}<{{K}^{+}}<C{{s}^{+}}-\]Ionic radius done
clear
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question_answer49)
The electronic configuration of an element is. The atomic number and the group number of the element 'X' which is just below the above element in the periodic table are respectively
A)
23 and 5 done
clear
B)
23 and 15 done
clear
C)
33 and 15 done
clear
D)
33 and 5 done
clear
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question_answer50)
Consider the following information about element P and Q:
|
Period number |
Group number |
P |
2 |
15 |
Q |
3 |
2 |
A)
QP done
clear
B)
\[{{Q}_{2}}{{P}_{3}}\] done
clear
C)
\[{{Q}_{3}}{{P}_{2}}\] done
clear
D)
\[{{Q}_{2}}P\] done
clear
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question_answer51)
Which one of the following statements is incorrect?
A)
Greater the nuclear charge, greater is the electron affinity done
clear
B)
Nitrogen has zero electron affinity done
clear
C)
Electron affinity decreases from fluorine to iodine in 17th group done
clear
D)
Chlorine has highest electron affinity done
clear
View Solution play_arrow
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question_answer52)
Which of the following statements is wrong?
A)
van der Waal's radius of iodine is more than its covalent radius done
clear
B)
All isoelectronic ions belong to same period of the periodic table done
clear
C)
\[I.E{{.}_{1}}\]of N is higher than that of O while\[I.E{{.}_{2}}\] of O is higher than that of N done
clear
D)
The electron gain enthalpy of N is almost zero while that of P is \[74.3\text{ }kJ\text{ }mo{{l}^{-1}}\] done
clear
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question_answer53)
Electron affinity is positive for
A)
\[O(g)+{{e}^{-}}\to {{O}^{-}}(g)\] done
clear
B)
\[S(g)+{{e}^{-}}\to {{S}^{-}}(g)\] done
clear
C)
\[{{O}^{+}}(g)+{{e}^{~}}^{-}\to O(g)\] done
clear
D)
\[{{O}^{-}}(g)+{{e}^{-}}\to {{O}^{2-}}(g)\] done
clear
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question_answer54)
Which one of the following ionic species has the greatest proton affinity to form stable compound?
A)
\[C{{l}^{-}}\] done
clear
B)
\[{{F}^{-}}~\] done
clear
C)
\[~{{I}^{-}}\] done
clear
D)
\[~B{{r}^{-}}\] done
clear
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question_answer55)
Which property decreases from left to right across the periodic table and increases from top to bottom?
(i) Atomic radius |
(ii) Electronegativity. |
(iii) Ionisation energy |
(iv) Metallic character |
A)
(i) only done
clear
B)
(i), (ii) and (iii) done
clear
C)
(i), (iii) and (iv) done
clear
D)
(i) and (iv) done
clear
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question_answer56)
The basic character of \[MgO,\text{ }BaO,\text{ }N{{a}_{2}}O\] and \[FeO\]follow the order
A)
\[MgO<FeO<BaO<N{{a}_{2}}O\] done
clear
B)
\[FeO<MgO<N{{a}_{2}}O<BaO\] done
clear
C)
\[FeO<MgO<BaO<N{{a}_{2}}O\] done
clear
D)
\[N{{a}_{2}}O<MgO<FeO<BaO\] done
clear
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question_answer57)
If the ionization enthalpy and electron gain enthalpy of an element are 275 and\[86\text{ }kcal\text{ }mo{{l}^{-1}}\] respectively, then the electronegativity of the element on the Pauling scale is:
A)
2.8 done
clear
B)
0.0 done
clear
C)
4.0 done
clear
D)
2.6 done
clear
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question_answer58)
Which transition involves maximum amount of energy?
A)
\[{{M}^{-}}\left( g \right)\xrightarrow{{}}M\left( g \right)+{{e}^{-}}\] done
clear
B)
\[{{M}^{-}}\left( g \right)\xrightarrow{{}}{{M}^{+}}\left( g \right)+2{{e}^{-}}\] done
clear
C)
\[{{M}^{+}}\left( g \right)\xrightarrow{{}}{{M}^{2+}}\left( g \right)+{{e}^{-}}\] done
clear
D)
\[{{M}^{2+}}\left( g \right)\xrightarrow{{}}{{M}^{3+}}\left( g \right)+{{e}^{-}}\] done
clear
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question_answer59)
Which ionisation potential (IP) in the following equations involves the greatest amount of energy?
A)
\[Na\to N{{a}^{+}}+{{e}^{-}}\] done
clear
B)
\[{{K}^{+}}\to {{K}^{2+}}+{{e}^{-}}\] done
clear
C)
\[{{C}^{2+}}\to {{C}^{3+}}+{{e}^{-}}\] done
clear
D)
\[C{{a}^{+}}\to C{{a}^{2+}}+{{e}^{-}}\] done
clear
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question_answer60)
Consider the following ionisation reactions: |
I.E.\[\left( kJ\text{ }mo{{l}^{-1}} \right)\] I.E. \[\left( kJ\text{ }mo{{l}^{-1}} \right)\] |
\[A(g)\to {{A}^{+}}(g)+{{e}^{-}},\,\,{{A}_{1}}\,\,A(g)~\to {{A}^{+}}(g)+{{e}^{-}},\,\,{{A}_{1}}\] |
\[{{B}^{+}}(g)\to {{B}^{2+}}(g)+{{e}^{-}},\,\,{{B}_{2}}C(g)\to {{C}^{+}}(g)+{{e}^{-}},\,\,{{C}_{1}}\] |
\[{{C}^{+}}(g)\to {{C}^{2+}}(g)+{{e}^{-}},\,\,{{C}_{1}}\,{{C}^{2+}}(g)\to {{C}^{3+}}(g)+{{e}^{-}},\,\,{{C}_{3}}\] |
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:
A)
\[{{C}_{3}}>{{B}_{2}}>{{A}_{1}}\] done
clear
B)
\[{{B}_{1}}>{{A}_{1}}>{{C}_{1}}\] done
clear
C)
\[{{C}_{3}}>{{C}_{2}}>{{B}_{2}}\] done
clear
D)
\[{{B}_{2}}>{{C}_{3}}>{{A}_{1}}\] done
clear
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