CBSE Questions for Class 11 Medical Chemistry Classification Of Elements And Periodicity In Properties Quiz 12 - MCQExams.com

Which of the following statements is not correct for the element having electronic structure $$2,8,8,2$$?
  • Its valency is $$2$$
  • It is in fourth period
  • It is in group $$II$$
  • Its atom forms negative ion
Which of the following elements will have highest ionization energy ?
  • $$1s^2 2s^2 2p^6 3s^1 $$
  • $$1s^2 2s^2 2p^6 3s^2 3p^3 $$
  • $$1s^2 2s^2 2p^6 3s^2 3p^4 $$
  • $$1s^2 2s^2 2p^6 3s^1 $$
Identify the incorrect match.
NameIUPAC Official Name
a)Unniluniumi)Mendelevium
b)Unniltriumii)Lawrencium
c)Unnilhexiumiii)Seaborgium
d)Unununniumiv)Darmstadtium
  • (b), (ii)
  • (c), (iii)
  • (d), (iv)
  • (a), (i)
State True or False:
The first ionization energy of N is lower than that of oxygen.
  • True
  • False
In group 1 of alkali metals , the ionization potential decreases down the group. therefore , lithium is powerful reducing agents.
  • True
  • False
Which of the following has maximum ionization potential ?
  • Be
  • K
  • Na
  • Mg
The first ionization energy $$(kJ\,mol^{-1})$$ for H, Li, F, Na has one of the following values : $$1681, 520, 1312, 495$$.Which of these values corresponds to that of hydrogen?
  • $$1681$$
  • $$1312$$
  • $$520$$
  • $$495$$
In which of the following cases, the former change would require lesser energy than the latter?
  • $$Be^{+}\left ( g \right )\rightarrow Be^{2+}\left ( g \right )+e^{-}; Be \left ( g \right )\rightarrow Be^{+}\left ( g \right )+e^{-}$$
  • $$Na\left ( g \right )\rightarrow Na^{+}\left ( g \right )+e^{-}; Cl^{-}\left ( g \right )\rightarrow Cl\left ( g \right )+e^{-}$$
  • $$Ag\left ( g \right )\rightarrow Ag^{+}\left ( g \right )+e^{-};Au\left ( g \right )\rightarrow Au^{+}\left ( g \right )+e^{-}$$
  • $$O^{-}\left ( g \right )\rightarrow O\left ( g \right )+e^{-};S^{-}\left ( g \right )\rightarrow S\left ( g \right )+e^{-}$$
Beryllium and aluminium exhibit many properties which are similar. But, the two elements differ in:
  • maximum covalency in compounds
  • forming polymeric hydrides
  • forming covalent halides
  • exhibiting amphoteric nature in their oxides
Among $$Al_2O_3, SiO_2, P_2O_3$$ and $$SO_2$$ the correct order of acid strength is:
  • $$Al_2O_3 < SiO_2 < SO_2 < P_2O_3$$
  • $$SiO_2 < SO_2 < Al_2O_3 < P_2O_3$$
  • $$SO_2 < P_2O_3 < SiO_2 < Al_2O_3$$
  • $$Al_2O_3 < SiO_2 < P_2O_3 < SO_2$$
IP values and EA values of elements A, B, C and D are given in a tabular form. Identify the strongest oxidizing agent and reducing agent among them.
IP ValueEA Value
A450140
B225700
C300400
D7001035
  • B, D
  • B, A
  • D, A
  • D, B
Pick the correct order of ionization potential values of elements.

(a) C < O < N < F < Ne

(b) He > Ne > Ar > Kr > Xe

(c) Li > Na > K > Rb > Cs

(d) Be < Mg < Ca < Sr < Ba

(e) Na > Mg > Al > Si > P 
  • a, c and e
  • b, c and d
  • a, b and c
  • b, d and c
Suppose a gas mixture of $$F, Cl, Br$$ and $$I$$ is irradiated with photons of frequency appropriate to ionize $$Cl.$$ What ion(s) will be present in the mixture ?
  • $$F^+$$ only
  • $$Cl^+$$ only
  • $$F^+,\,Cl^+,\,Br^+$$ only
  • $$Cl^+,\,Be^+,\,I^+$$ only
Which of the following statement(s) is(are) correct?
  • The electron affinity for sulphur is more exothermic than that for oxygen
  • Successive ionization energies of an atom always increase
  • First ionization energy of $$As$$ is greater than that of $$Se$$
  • Chlorine has larger atomic size as well as electron affinity than that of fluorine
Consider the following statements.

$$S_1$$: Fluorine does not form any polyhalide as it has low F - F bond energy
$$S_2$$: The chlorine has the most negative electron gain enthalpy.
$$S_3$$: The first ionization potential of N and 0 atoms are 14.6 and 13.6 eV respectively.

Which of the above statements are correct?
  • $$S_1, S_2$$ and $$S_3$$
  • $$S_1$$ and $$S_2$$
  • $$S_1$$ and $$S_3$$
  • $$S_2$$ and $$S_3$$
Ionization energy of $${He}^{+}$$ is $$19.6 \times {10}^{-18} J {atom}^{-1}$$. The energy of the first stationary state $$\left(n=1\right)$$ of $${Li}^{2+}$$ is:
  • $$-2.2 \times {10}^{-15} J {atom}^{-1}$$
  • $$8.82 \times {10}^{-17} J {atom}^{-1}$$
  • $$4.41 \times {10}^{-16} J {atom}^{-1}$$
  • $$-4.41 \times {10}^{-17} J {atom}^{-1}$$
Ionisation energy in group $$1A$$ varies in the decreasing order as:
  • $$Li > Na > K > Cs$$
  • $$Na > Li > K > Cs$$
  • $$Li > Cs > K > Na$$
  • $$K > Cs> Na > Li$$
The ionisation enthalpy of $$He^{+}$$ ion is $$19.60\times 10^{-18}J\ atom^{-1}$$. The ionisation enthalpy of $$Li^{2+}$$ ion will be:
  • $$84.2\times 10^{-18}J atom^{-1}$$
  • $$44.10\times 10^{-18}J atom^{-1}$$
  • $$63.20\times 10^{-18}J atom^{-1}$$
  • $$21.20\times 10^{-18}J atom^{-1}$$
  • $$2.17\times 10^{-19}J atom^{-1}$$
Which has maximum ionisation potential?
  • $$N$$
  • $$O$$
  • $$O^{+}$$
  • $$Na$$
Considering the trend for ionization energy on the periodic table, which of the following elements has the highest ionization energy?
  • Boron
  • Oxygen
  • Nitrogen
  • Fluorine
Arrange the following elements in terms of increasing first ionization energy:
$$Ga,\ Ba,\ Ru,\ F,\ N$$
  • $$Ba < Ru < Ga < N < F$$
  • $$Ga<Ba<Ru<F<N$$
  • $$Ru<Ba<Ga<N<F$$
  • None of the above
The table above shows the first five ionization energies for a second-period element. Which identifies the element and provides the best explanation?
Ionization Energy $$(kJ/mol)$$
First$$801$$
Second$$2,430$$
Third$$3,660$$
Fourth$$25,000$$
Fifth$$32,820$$
  • Boron, because it has five electrons.
  • Boron, because is has three valence electrons.
  • Nitrogen, because it has five valence electrons.
  • Nitrogen, because it has three electrons in a $$2p$$ sublevel.
The most electropositive element is:
  • $$Na$$
  • $$Al$$
  • $$F$$
  • $$K$$
A swimmer coming out from a pool is covered with a film of water weighing about 18 g. Calculate the internal energy of vaporisation at $$100^0\ C$$.

[ ∆ vap H for water at 373 K = 40.66 kJ mol -1 ]
  • $$37.55 kJmol^{-1}$$
  • $$3.67kJmol^{−1}$$
  • $$30.67 kJmol^{-1}$$
  • $$3.567kJmol^{−1}$$
    35.67kJmol−
The first ($$\Delta H_{1}$$) and second ($$\Delta  H_{2}$$) ionisation enthalpies (in $$kJ mol^{-1}$$) and the electron gain enthalpy ($$\Delta_{eg}H$$) (in $$kJ mol^{-1}$$) of the elements I, II, III, IV and V are given below:

Element$$\Delta_{1}H_{1}$$$$\Delta_{1}H_{2}$$$$\Delta_{eg}H$$
I5207300-60
II4193051-48
II16813374-328
IV10081846-295
V23725251+48
The most reactive metal and the least reactive non-metal of  these are respectively.
  • I and V
  • V and II
  • II and V
  • IV and V
An element X has electronic configuration 2, 8,It forms ionic compounds with ions like nitrate, sulphate and phosphate. What will be the formulae of these compounds?
  • $${X}_{2}{NO}_{3}, {X}_{2}{SO}_{4},{X}_{2}{({PO}_{4})}_{3}$$
  • $${X}_{2}{NO}_{3}, {X}_{}{SO}_{4},{X}_{2}{({PO}_{4})}_{3}$$
  • $${X}_{}{NO}_{3}, {X}_{}{SO}_{4},{X}_{}{({PO}_{4})}_{3}$$
  • $${X}{({NO}_{3})}_{2}, {X}_{}{SO}_{4},{X}_{3}{({PO}_{4})}_{2}$$
If the configuration of $$Y^{+}$$ & $$X^{-}$$ is $$2s^{2}\ 2p^{6}$$ then
  • $$IP$$ of $$X=IP$$ of $$Y$$
  • $$EA$$ of $$X>EA$$ of $$Y$$
  • $$IP$$ of $$X^{-}=IP$$ of $$Y^{+}$$
  • $$IP$$ of $$X^{-}>IP$$ of $$Y^{+}$$
In which of the following options order of arrangement does not match with the variation of property indicated against it?
  • $$Al^{3+} < Mg^{2+} < Na^{+} < F^{-}$$ (increasing ionic size)
  • $$B < C < N < O$$ (increasing first ionisation enthalpy)
  • $$I < Br < F < Cl$$ (increasing electron gain enthalpy)
  • $$Li < Na < K < Rb$$ (increasing metallic radius)
The decreasing order of the ionization potential of the following elements is:
  • $$Ne > Cl > P > S > Al > Mg$$
  • $$Ne > Cl > P > S > Mg > Al$$
  • $$Ne > Cl > S > P > Mg > Al$$
  • $$Ne > Cl > S > P > Al > Mg$$
Which of the following statement is correct?
  • IP of $$X_{(g)} >$$ E.A. of $$X_{(g)}$$
  • IP of $$X_{(g)} >$$ IP of $$X^-{_{(g)}}$$
  • IP of $$X^+_{(g)} > $$ IP of $$X_{(g)}$$
  • All are correct
Generally, the first ionisation energy increases along a period, but there are some exceptions. From the given sets which is not an exception: 
  • N and O
  • Na and Mg
  • Mg and AI
  • Be and B
Supposing the energy of the fourth shell for the hydrogen atom is -$$50$$ a.u. (arbitrary unit). What would be its ionization potential?
  • $$50$$
  • $$800$$
  • $$15.4$$
  • $$20.8$$
In $$Cr$$, $$21^{st}$$ electron will enter in which orbital?
  • $$d_{xy}$$
  • $$d_{yz}$$
  • $$d_{zx}$$
  • Any of the above
The electronic configuration of an element is $$1s^22s^22p^63s^23p^3$$ . The atomic number of the element, which is just below the above element in the periodic table is__
  • 32
  • 33
  • 35
  • 30
The $$I{ P }_{ 2 },I{ P }_{ 3 },I{ P }_{ 4 }\ and\quad I{ P }_{ 5 }$$ of an element are 7.1, 14.3 , 34.5, 46.8, 162.2 eV respectively .The element is likely to be:
  • Na
  • Si
  • F
  • Ca
The second ionization energy is maximum for:
  • boron
  • beryllium
  • magnesium
  • aluminium
All alkali metal superoxides contain the $$ [O_{2}]^-$$ ion. They are:
  • Paramagnetic
  • Coloured compounds
  • Oxidizing agents
  • All of these
The enthalpy of formation of gaseous $$N_2O$$ and $$NO$$ at 298 K are 82 and 90 $$kJ\ mol^{-1}$$. The enthalpy of reaction:
$$N_2O(g)+\cfrac {1}{2}O_2\longrightarrow 2NO(g)$$ is
  • -8 kJ
  • 98kJ
  • -74 kJ
  • +8 kJ
In which pair do both atoms have one electron only in an "s" orbital in their ground states?
  • $$Ca, Sc$$
  • $$Cu,Be$$
  • $$H,He$$
  • $$Li,Cr$$
Which pair of elements has the same characteristic chemical properties?
  • $$Z=13, Z=22$$
  • $$Z=3, Z=11$$
  • $$Z=4, Z=24$$
  • $$Z=2, Z=4$$
In which of the following pairs, the first member has higher first ionization energy ?
  • $$N, O$$
  • $$Cl,  Ar$$
  • $$Al, Ga$$
  • $$B, Be$$
The set representing the correct order of first ionization potential is:
  • $$K> Na> Li$$
  • $$Ge> Si> C$$
  • $$Be> Mg> Ca$$
  • $$B> N> C$$
Match the atomic numbers 19, 15, 8, 4 and 2 with each of the following:                                           
  • 19: A metal of valency one.
  • 15: A solid non-metal of period 3
  • 8: A rare gas
  • 2: A gaseous element with valency 2.
  • 4: An element of group 2.
Two moles of $$N _ { 2 }$$ and two moles of $$\mathrm { H } _ { 2 }$$ are taken in a closed vessel of 5 litres capacity and suitable conditions are provided for the reaction. When the equilibrium is reached, it is found that a half mole of $$N _ { 2 }$$is used up. The equilibrium concentration of $$N H _ { 3 }$$ is:
  • 0.3 M
  • 0.4 M
  • 0.2 M
  • 0.1 M
If each orbital can hold a maximum of three electrons, the number of elements in $$9 ^ { \text { th } }$$ period of periodic table (long form) are
  • $$48$$
  • $$162$$
  • $$50$$
  • $$75$$
Which one of the following is a correct electronic composition of sodium?
  • $$2,8$$
  • $$8,2,1$$
  • $$2,1,8$$
  • $$2,8,1$$

Which members of each of the following pairs of atoms has higher first ionisation enthalpy and why?
  • $$Na : K$$
  • $$Ar:Cl$$
  • $$B: Be$$
  • $$O: N$$
Sodium forms $$Na^{ + }$$ and not $$Na^{ 2+ }$$ because :
  • sodium contains only one electron in outermost shell.
  • first ionization potential is small and the difference in first and second ionization potentials is very large.
  • radius of $$Na^{ + }$$ is much smaller than of $$Na^{2 + }$$.
  • None of the above.
The first four ionization potentials (eV) are given for two elements $$X$$ and $$Y$$.Identify them.
X8.29625.14937.92259.298
Y5.31847.2971.6598.88
  • $$B, Na$$
  • $$Na, Be$$
  • $$Be, B$$
  • $$Na, Mg$$
For the highlighted element in its $$X^{2-}$$ form identify the CORRECT electronic configuration.
1591420_f644bdd1593a484d99d6ada8808b7bd9.JPG
  • $$[Kr] 5s^2 4d^{10} 5p^4$$
  • $$[Kr] 5s^2 5p^4$$
  • $$[Kr] 5s^2 4d^{10} 5p^6$$
  • $$[Kr] 5s^2 5p^6$$
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