CBSE Questions for Class 11 Medical Chemistry Classification Of Elements And Periodicity In Properties Quiz 5 - MCQExams.com

State the electronic configuration for Boron [p=5, n=6].
  • 2, 3
  • 5, 10 
  • 5, 12 
  • 5, 11 
Name the following with reference to the elements of the modern periodic table.

The alkali metal in period 2 
  • H
  • Li
  • Rb
  • Cs
Which element  is considered radioactive among the options given below?
  • Sodium
  • Gold
  • Thorium
  • Neon
What is the electronic configuration of nitrogen [Atomic number=7, Atomic mass=14]?
  • $$2, 3$$
  • $$2, 5$$
  • $$2, 2$$
  • $$7$$
Refer to changes in properties of elements  on moving left to right across a period of the periodic table. For each property, choose the letter corresponding to the correct answer from A, B, C and D

The ionization potential _______ .
  • goes up and down
  • decreases
  • increases
  • remains the same
Electronic configuration of Mg is:
  • $$1s^2 2s^1p^5 3s^23d^2$$
  • $$1s^2 2s^2p^6 3s^2$$
  • $$1s^2 2s^2p^7 3s^1$$
  • $$1s^2 2s^2p^6 3s^2p^2$$
What is the electronic configuration of silicon [Atomic no.=14, Mass number=28]?
  • $$2, 8, 1$$
  • $$2, 8, 2$$
  • $$2, 8, 3$$
  • $$2, 8, 4$$
What is the electronic configuration of oxygen [Atomic no.=8, Atomic mass=16]?
  • $$2, 3$$
  • $$2, 4$$
  • $$2, 5$$
  • $$2, 6$$
Ionisation potential of elements on moving down a group:
  • increases
  • decreases
  • constant
  • none of these
The electronic configuration, $$1s^2, 2s^22p^6, 3s^23p^6, 3d^9$$ represents a
  • Metal atoms
  • non metals atom
  • non-metallic anionic
  • metallic cation
What is the electronic configuration of carbon [Atomic mass=12, Atomic number=6]?
  • $$2, 3$$
  • $$2, 5$$
  • $$2, 6$$
  • $$2, 4$$
Which is the metallic element?
  • $$Y$$
  • $$X$$
  • Both $$A$$ and $$B$$
  • None of the above
Atom with ____atomic radii and ___ionisation potential tends to gain electrons
  • large , high
  • large , low
  • small , low
  • small , high
Compare the properties of a typical metal and a non-metal on the basis of the following.

Electronic configuration :
  • Metal have 1, 2, 3, 4 valence electrons while non metals have 5, 6, 7, 8 valence electrons.
  • Metal have 1, 2 valence electrons while non metals have 4, 5, 6, 7, 8 valence electrons.
  • Metal have 1, 2, 3 valence electrons while non metals have 6, 7, 8 valence electrons.
  • Metal have 1, 2, 3 valence electrons while non metals have 4, 5, 6, 7 valence electrons.
Compare the properties of metals and non-metals with respect to electronic configuration.
  • Metals have 1,2 valence electrons while non metals have 3,5,6 or 7 valence electrons
  • Metals have 1 or 3 valence electrons while non metals have 2,5 valence electrons
  • Metals have 2 or 3 valence electrons while non metals have 1,5,6 or 7 valence electrons
  • Metals have 1,2 or 3 valence electrons while non metals have 4,5,6 or 7 valence electrons
Which element has an electronic configuration of 2, 8, 8 ?
  • He
  • Ne
  • Ar
  • Kr
The formula of the hydroxide of the element having electronic configuration 2, 8, 2 is :
  • $$MgOH$$
  • $$Mg(OH)_3$$
  • $$Mg_2(OH)_3$$
  • $$Mg(OH)_2$$
The character of the hydroxide of the element $$Al$$:
  • acidic
  • basic
  • neutral
  • amphoteric
Increase in nuclear charge of an atom decreases the tendency of the atom to loose electrons.
  • True
  • False
Arrange the following elements in order of their increasing ionization energies $$O, S, Se, Te, Po$$.
  • $$Se,Te, S, Po, O$$
  • $$O,S,Se,Te, Po$$
  • $$Po, Te,Se,S,O$$
  • $$Te, O,S,Po,Se$$
Which of the following statements are correctly matched?
  • $$d$$-block element : electronic configuration is $$n{s}^{1-2}(n-1){d}^{1-10}$$
  • $$p$$-block element : electronic configuration is $$n{s}^{1-2}n{d}^{1-6}$$
  • $$s$$-block element : electronic configuration is $$n{s}^{1-2}$$
  • $$Ce$$: $$f$$-block's first member
What is the electronic arrangement of G ?
  • 2, 2, 5
  • 2, 4, 3
  • 2, 7
  • 2, 5, 2
Ionization energy is influenced by:
  • size of an atom
  • charge on a nucleus
  • electrons present in the inner shells
  • None of the above
Electronic configuration of element T is 2, 8, 7. Under which category this element belongs to?
  • Alkali metal
  • Alkaline metal
  • Noble gases
  • Non-metal
Match column I with column II and select the correct answer using the codes given below:
           Column I                                 Column II
(A)  $$_{ 6 }^{ 14 }{ C }$$ and $$_{ 6 }^{ 13 }{ C }$$           (p)  Different number of neutrons
(B)  $$_{ 20 }^{ 40 }{ C a}$$ and $$_{ 18 }^{ 40 }{ Ar }$$       (q)  Different number of protons and neutrons
(C)  $$K \left(19\right)$$                    (r)  Non-metal
(D)  Chlorine $$\left(17\right)$$         (s)  Metal                                
  • A - (p); B - (q); C - (r); D - (s)
  • A - (q); B - (p); C - (s); D - (r)
  • A - (p); B - (q); C - (s); D - (r)
  • A - (p); B - (s); C - (q); D - (r)
In the Periodic Table, the Ionization potential in a group _____ from top to bottom.
  • increases
  • decreases
  • does not change
  • can not be predicted
The electronic configuration of chlorine atom is :
  • $$1s^22s^2p^63s^3p^5$$
  • $$1s^22s^3p^63s^3p^4$$
  • $$1s^22s^2p^63s^2p^5$$
  • $$1s^22s^2p^63s^2p^6$$
The electronic configurations of three elements X, Y and Z are $$2, 8$$; $$2, 8, 7$$; and $$2, 8, 2$$ respectively. Which of the following is correct?
  • $$X$$ is a metal
  • $$Y$$ is a metal
  • $$Z$$ is a non-metal
  • $$Y$$ is a non-metal and $$Z$$ is a metal
Select the correct I.E. order for the following species.
  • $$Cl\,>\,Br$$
  • $$Br^-\,>\,Cl^-$$
  • $$Cl\,>\,Cl^-$$
  • $$Br\,>\,Br^-$$
Ionization energy depends upon :
  • principal quantum number
  • azimuthal quantum number
  • magnetic quantum number
  • spin quantum number
For which set of elements, "diagonal relationship" exists?
  • $$B, Si$$
  • $$Li, Mg$$
  • $$B, Mg$$
  • $$Be, Al$$
In group Ia of alkali metals, the ionization potential decreases down the group. Therefore, lithium is a:
  • good reducing agent
  • poor reducing agent
  • good oxidising agent
  • poor oxidising agent
The chemistry of lithium is very similar to that of magnesium even though they are placed in different groups. Its reason is that:
  • both are found together in nature
  • both have nearly the same size
  • both have similar electronic configurations
  • the ratio of their charge to size is nearly the same
Which of the following has the lowest ionization enthalpy?
  • $$4s^1$$
  • $$3d^2$$
  • $$3p^6$$
  • $$2p^6$$
Aluminium is diagonally related to :
  • $$Li$$
  • $$Si$$
  • $$Be$$
  • $$B$$
Identify the least stable ion amongst the following :
  • $$Li^-$$
  • $$Be^-$$
  • $$B^-$$
  • $$C^-$$
Compound of a metal $$'M'$$ is $$M_{2}O_{3}$$.The formula of its nitride will be -
  • $$M_{3}N$$
  • $$MN$$
  • $$M_{3}N_{2}$$
  • $$M_{2}N_{3}$$
I.P. of sodium is 5.14 eV then I.P. of potassium will be :
  • equal to sodium
  • 5.68 eV
  • 4.34 eV
  • 10.28 eV
A large difference between the third and fourth ionization energies indicates the presence of :
  • 4 valence electrons in an atom.
  • 5 valence electrons in an atom
  • 3 valence electrons in an atom
  • 8 valence electrons in an atom.
Which of the following decreases in going down the halogen group?
  • Ionic radius
  • Atomic radius
  • Ionisation potential
  • Boiling point
As we go down in the electro-chemical series of metals, the reactivity ______ .
  • decreases and then increases
  • increases and then decreases
  • decreases
  • increases
Which is most acidic oxide ?
  • $$Cl_2O$$
  • $$Cl_2O_3$$
  • $$Cl_2O_6$$
  • $$Cl_2O_7$$
The correct order of ionization energies of $$\displaystyle F^{-},Cl^{-}F$$ and $$Cl$$ is:
  • $$\displaystyle Cl< F< Cl^{-}< F^{-}$$
  • $$\displaystyle Cl^{-}< F^{-}< Cl< F$$
  • $$\displaystyle F^{-}< Cl^{-}< Cl< F$$
  • $$\displaystyle Cl^{-}< Cl< F^{-}< F$$
Fluorine is the most reactive among all the halogens, because of its:
  • small size
  • low dissociation energy of F - F bond
  • large size
  • high dissociation energy of F - F bond
Which of the following is mismatched with reference to third period?
  • Largest size ___ Argon
  • Strongest oxidant ____ chlorine
  • IP of phosphorus ____ greater than nitrogen
  • IP of phosphorus ______ greater than sulphur
IP is influenced by :
  • size of atom
  • effective nuclear charge
  • electrons present in inner shell
  • all
With reference to ionisation potential which one of the following set is correct?
  • $$Li > K > B$$
  • $$B > Li > K$$
  • $$Cs > Li > K$$
  • $$Cs < Li < K$$
Which of the following statement is correct?
  • Ionization energy may be negative for some elements.
  • Second electron gain enthalpy always remains positive for all the elements.
  • Negative value of electron gain enthalpy of Fluorine is minimum in its group.
  • Ionization energy of Ga is slightly lower than Al.
As one moves down the group from top to bottom, which one among the following will not be observed?
  • Increase in Ionization energy
  • Decrease in electron affinity
  • Decrease in electronegativity
  • Increase in atomic radii
Which of the following is the increasing order of electron affinity of halogens ?

  • $$I < Br < Cl < F$$
  • $$I < Br < F < Cl$$
  • $$F < Cl < Br < I$$
  • $$Br < F< I < Cl$$
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