CBSE Questions for Class 11 Medical Chemistry Classification Of Elements And Periodicity In Properties Quiz 9 - MCQExams.com

Select the group where $$EN$$ increases down the group.
  • $$Zn, Cd, Hg$$
  • $$F, Cl, Br$$
  • $$Li, Na, K$$
  • $$Ca, Sr, Ba$$
What is the correct order of ionisation energy?
  • B > Al < Ga > In < Tl
  • B < Al > Ga > In > Tl
  • B > Al > Ga > In >Tl
  • B > Al < Ga < In < Tl
Which of the following gases is most predominating in the Sun?
  • Hydrogen
  • Nitrogen
  • Ozone
  • Helium
In hydrogen atom the energy difference between the states $$n=2$$ and $$n=3$$ is $$EeV$$. The ionisation potential of $$H$$ atom is:
  • $$3.2E$$
  • $$5.6E$$
  • $$7.2E$$
  • $$13.2E$$
The first ionisation enthalpy of the elements are in the order of:
  • $$C < Si <N < P$$
  • $$N < Si < C < P$$
  • $$Si < N < C < P$$
  • none of the above
Which is correct increasing order of their tendency of the given elements to form $$M^{3-}$$ ion?
  • $$Bi > Sb > As > P > N$$
  • $$Bi < Sb < As < P < N$$
  • $$N < P < Sb < Bi < As$$$
  • $$Bi > Sb \sim N \sim P > As$$
Match the column:- 
(A)$${ 1s }^{ 2 }{ 2s }^{ 2 }{ 2p }^{ 6 }{ 3s }^{ 2 }3p^{ 4 } $$(P)s-block , II A, 2nd period
(B)$$[Rn]6d^27s^2$$(Q)d -block, II B, 4th period
(C)$$ { 1s }^{ 2 }{ 2s }^{ 2 }{ 2p }^{ 6 }{ 3s }^{ 2 }{ 3p }^{ 6 }{ 3d }^{ 10 }{ 4s }^{ 2 }$$(R) f-block , III B, 7th period
(D)$$1s^22s^2 $$(S)p-block VI A, 3rd period
  • $$ A-Q, B-P, C-S, D-R $$
  • $$A-R, B-P , C-S , D-Q $$
  • $$A-S, B-R, C-Q,D-P $$
  • None of the above
The first ionization enthalpies for three elements are 1314, 1680, and 2080 kJ$$ mol^{-1}$$, respectively. The correct sequence of the element is ______.
  • O,F and Ne
  • F,O and Ne
  • Ne,F and O
  • F,Ne and O
Choose the correct answer form the alternatives given. $$Ca^{2+}$$ is isoelectronic with:
  • $$Na$$
  • $$4Mg^{2+}$$
  • $$Ba^{2+}$$
  • $$Ar$$
The main reason for showing anomalous properties of the first member of a group in s or p-block is :
  • maximum chemical reactivity
  • maximum electronegativity and different configurations
  • small size, large charge/radius ratio
  • tendency to form multiple bonds
Two elements $$X$$ and $$Y$$ contain only one electron in the outer level. Element $$X$$ is reactive and loses electron easily while element $$Y$$ is relatively unreactive and non-corrosive. The elements $$X$$ and $$Y$$ respectively are:
  • $$Cs$$ and $$Li$$
  • $$Rb$$ and $$Na$$
  • $$Li$$ and $$Cu$$
  • $$Ag$$ and $$Au$$
Which of the following elements will have highest ionisation energy?
  • $$1s^{2}2s^{2}2p^{6}3s^{1}$$
  • $$1s^{2}2s^{2}2p^{6}3s^{2}3p^{3}$$
  • $$1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}$$
  • $$1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}$$
Which of the following is not a periodic property for the elements?
  • Electronegativity
  • Atomic size
  • Occurrence in nature
  • Ionization energy
The electronic states $$X$$ and $$Y$$ of an atom are depeicted below:
$$X : 1s^{2} 2s^{2} 2p^{6} 3s^{1}$$
$$Y: 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{1}$$
Which of the following statements is not correct?
  • $$X$$ represents an alkali metal.
  • Energy is required to change $$X$$ into $$Y$$
  • $$Y$$ represents ground state of the element.
  • Less energy is required to remove an electron from $$X$$ than from $$Y$$
Beryllium has higher ionization enthalpy than boron. This can be explained as :
  • beryllium has higher size than boron hence its ionisation enthalpy is higher
  • penetration of $$2p- $$electrons to the nucleus is more than the $$2s-$$electrons
  • it is easier to remove an electron from $$2p-$$orbital as compared to $$2s-$$orbital due to more penetration of $$s-$$electrons
  • ionisation energy increases in a period
Which of the following can most easily form unipositive gaseous ion?
  • $$1s^{2} 2s^{2} 2p^{6} 3s^{2}$$
  • $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{1}$$
  • $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{2}$$
  • $$1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{3}$$
An energy of $$24.6\ eV$$ is required to remove one of the electrons from a neutral helium atom. The energy $$(in\ eV)$$ required to remove both the electrons from a neutral helium atom is:
  • $$2$$
  • $$49.2$$
  • $$51.8$$
  • $$79.0$$
The first ionisation energies of the elements of the first transition series ($$Ti$$ to $$Cu$$):
  • increases as the atomic number increases
  • decreases as the atomic number increases
  • do not show any change as the addition of electrons takes place in the inner $$(n - 1) d-$$orbitals
  • increases from $$Ti$$ to $$Mn$$ and then decreases from $$Mn$$ to $$Cu$$
The highest ionization energy is exhibited by:
  • halogens
  • alkaline earth metals
  • transition metals
  • noble gas
Who is father of the Periodic Table of Elements?
  • Johann Baeyer
  • Dmitri Mendeleev
  • Alfred Nobel
  • Johannes Van der Waals
Which of the following is not correctly matched with the given example?
  • An element of first transition series which has highest second ionization enthalpy-$$Cu$$
  • An element of first transition series with highest third ionisation enthalpy-$$Zn$$
  • An element of first transition series with lowest enthalpy of atomisation-$$Zn$$
  • Last element of third transition series-$$Cd$$
The first ionization energy for $$Li$$ is $$5.4$$ eV and electron affinity of $$Cl$$ is $$3.61$$ eV. The $$\Delta H$$ (in kJ/mol) for the reaction $$Li(g)+Cl(g)\rightarrow Li^+(g)+Cl^-(g)$$ is:
(If the resulting ions do not combine with each other)
  • $$70$$
  • $$100$$
  • $$172$$
  • $$270$$
Which reference to concept of ionization potential, which one of the following sets are correct
  • $$U > K > Cs$$
  • $$B > U > K$$
  • $$Cs > U > B$$
  • $$Cs > U > K$$
In each of the following pairs,state which atom/ion has higher ionization enthalpy and more negative electron gain enthalpy?
  • $$I, { I }^{ - }$$
  • $$Br, { Br }^{ - }$$
  • $$Li, { Li }^{ - }$$
  • $$Br, I$$
The successive ionization energies for element X is given below
$$IE_1$$   :   $$250 kJ mol^{-1}$$
$$IE_2$$   :   $$820 kJ mol^{-1}$$
$$IE_3$$   :   $$1100 kJ mol^{-1}$$
$$IE_4$$   :   $$1400 kJ mol^{-1}$$
Find out the number of valence electrons for the element X.
  • $$3$$
  • $$4$$
  • $$2$$
  • $$1$$

General electronic configuration of outermost and penultimate shell is $$\left( {n - 1} \right)\,\,{s^2}\,\,\left( {n - 1} \right){p^{6\,\,}}\left( {n - 1} \right)\,{d^x}\,\,n{s^2}$$. If $$n = 4$$ and $$x = 5$$   then number of protons in the nuleus will be :-
  • $$ > \,\,25$$
  • $$ < \,\,24$$
  • $$25$$
  • $$30$$
The number of electrons having $$n + s = 2.5$$ in sulphide ion is:
  • $$3$$
  • $$4$$
  • $$6$$
  • $$2$$
Ionic potential $$\left( \phi  \right) $$ of electropositive element will be highest in which of the following compound:
  • $$CsCl$$
  • $$Mg{ CI }_{ 2 }$$
  • $$AI{ F }_{ 3 }$$
  • $${ SF }_{ 6 }$$
Strong electropositive property shown by the following:
  • $$Mg$$
  • $$P$$
  • $$Si$$
  • $$Cl$$
Which compound is mainly responsible for the depletion of ozone layer?
  • $$CO_2$$
  • $$CH_4$$
  • $$CH_3OH$$
  • $$CF_2Cl_2$$
Elements of which of the following group $$\left ( s \right )$$ of periodic table do not from hydrides.
  • group 7,8,9
  • group 13
  • group 15,16,17
  • group 14
Which of the following sulphates has the highest solubility in water?
  • $$Mg{SO}_{4}$$
  • $$Ba{SO}_{4}$$
  • $$Ca{SO}_{4}$$
  • $$Be{SO}_{4}$$
Which of the following pair has electron deficient compounds?
  • $$B_2H_6, \ AlCl_3$$
  • $$C_2H_6, \ Al_2Cl_6$$
  • $$SF_2, \ Cl_2O$$
  • $$NaBH_4, \ ICl$$
Correct order of the tendency of metals to loss of electrons. 
  • $$Zn > Cu > Ag$$
  • $$Zn < Cu < Ag$$
  • $$Zn > Cu < Ag$$
  • $$Cu > Zn > Ag$$
Which of the following match is correct?
  • last natural element- Uub
  • General electronic configuration of IA group - $${ ns }^{ 2 }$$
  • inert gas lies in $${ 2 }^{ nd }$$ - $${ 6 }^{ th }$$ period
  • Typical elements - $${ 3 }^{ rd }$$ period elements
Which of the following group bear maximum number of elements?
  • $$ 3^{rd} $$ group
  • $$ 2^{nd} $$ group
  • $$ 18^{th} $$ group
  • $$ 13^{th} $$ group
Which of the following sequence regarding ionisation potential of coinage metal is correct?
  • $$Cu>Ag>Au$$
  • $$Cu<Ag<Au$$
  • $$Cu>Ag<Au$$
  • $$Ag>Cu<Au$$
The one electron species having ionization energy of 54.4 eV is
  • $$H$$
  • $$He^+$$
  • $$B^{4+}$$
  • $$Li^{2+}$$
  • $$Be^{2+}$$
Strongest reducing agent is:
  • K
  • Mg
  • Both
  • None
The elements with atomic number 117 and 120 are yet to be discovered. In which group would you place these elements when discovered?
  • 17, 2
  • 16, 4
  • 15, 3
  • 18, 2
Which of the following metal oxides is most basic?
  • $$ZnO$$
  • $$Al_2O_3$$
  • $$As_2O_3$$
  • $$K_2O$$
$$1s^2,2s^2,2p^6,3s^1$$ shows configuration of:
  • $$Al^{3+}$$ in ground state
  • $$Ne$$ in excited state
  • $$Mg^+$$ in excited state
  • None of these
Name the element which has a total of three shells with five electrons in its valence shells:
  • Nitogen
  • Phosphorus
  • Arsenic
  • Anitmony
  • Bismuth
Which of the following elements never show positive oxidation number?
  • O
  • Fe
  • Ga
  • F
The electronic configuration of an element is $$1s^22s^22p^63s^23p^63d^{10}4s^1$$. What is the atomic number of the next element of the same group?
  • $$20$$
  • $$119$$
  • $$30$$
  • $$47$$
Nuclides have:
  • specific atomic number
  • same numbers of proton
  • same numbers of neutrons
  • specific atomic number and mass number
Element having highest I.P. value is:
  • Ne
  • He
  • Be
  • N
In general, the properties that decrease and increase down a group in the periodic table, respectively, are:
  • electronegativity and electron gain enthalpy.
  • electronegativity and atomic radius.
  • atomic radius and electronegativity
  • electron gain enthalpy and electronegativity
The element with $$Z = 120$$ (not yet discovered) will be an/ a:
  • transition metal
  • inner-transition metal
  • alkaline earth metal
  • alkali metal
Which of the following is affected by the stable electron configuration of an atom ?
I. Electronegativity
II. Ionisation enthalpy
III. Electron gain enthalpy

  • Only I
  • Only II
  • Both II & III
  • All the above
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