CBSE Questions for Class 11 Medical Chemistry Classification Of Elements And Periodicity In Properties Quiz 2 - MCQExams.com

In $$CuX_2$$, X belongs to which group?
  • group IA
  • group IIA
  • group IIIA
  • group VIA
  • group VIIA
Which of the following has the lowest ionization energy?
  • $$Li$$
  • $$Na$$
  • $$K$$
  • $$Rb$$
  • $$Cs$$
Which element reacts most explosively in water?
  • $$K$$
  • $$Ca$$
  • $$Br$$
  • $$Kr$$
  • $$Zn$$
Arrange the elements in order of their reactivity?
B, Al, Ga, In
  • B < Al < Ga < In
  • In < Ga < Al < B
  • Ga < In < Al < B
  • None of the above
Which statement describes positive ions?
  • Positive ions have more electrons than neutrons
  • Positive ions have more protons than neutrons
  • Positive ions have more electrons than protons
  • Positive ions have more protons than electrons
The electronic configuration of the two outermost shells of an atom is $$3s^23p^63d^54s^2$$. What is this atom?
  • Manganese
  • Phosphorus
  • Strontium
  • Vanadium
Electronic configuration of  $$H^{ - }$$  is:
  • $$1 s ^ { 0 }$$
  • $$1 s ^ { 1 }$$
  • $$1 s ^ { 2 }$$
  • $$1 s ^ { 1 }$$ $$2 s ^ { 1 }$$
Which of the following gas does not have an octet or eight electrons in the outer shell
  • $$Ne$$
  • $$Ar$$
  • $$Rn$$
  • $$He$$
An element 'X' with atomic number 114 has recently been discovered. Its IUPAC name is:
  • Eka-Iead
  • Ununfortium
  • Ununquadium
  • Bohrium
Configuration of the final elements of $$3d, 4d, 5d$$ series respectively are:
  • $$3d^{5}4s^{2}, 4d^{10}5s^{2}, 5d^{10}6s^{2}$$
  • $$3d^{10}4s^{2}, 4d^{10}5s^{2},5d^{10}6s^{2}$$
  • $$3d^{10}4s^{2}, 4d^{10}5s^{2}s5d^{10}6s^{1}$$
  • $$3d^{9}4s^{2},4d^{10}5s^{2},5d^{10}6s^{1}$$
General outermost electronic configuration of the elements situated above and below $$X$$ (Atomic number $$=50$$) would be:
  • $$ns^{2}np^{2}$$
  • $$Ns^{2}np^{3}$$
  • $$ns^{2}np^{4}$$
  • $$ns^{2}np^{5}$$
The first ionisation potential is maximum for :
  • lithium
  • uranium
  • iron
  • hydrogen
The positions of four elements A, B, C and D in the modern periodic table are shown below. Which element is most likely to form an acidic oxide?


2046588_336af298c62946b79ee145f6ad0283a8.PNG
  • A
  • B
  • C
  • D
The properties of _________ were predicted by Mendeleev before their isolation.
  • Co and Ni
  • I and Te
  • Sc, Ga and Ge
  • Cl, Ar and K
In Mendeleev table, the triad of VIII group is :
  • Ru, Rh, Pd
  • Cu, Ag, Au
  • N, O, F
  • Tl, Pb, Bi
Which of the following electronic configurations is characteristic of alkali metals?
  • $$(n-1)p^{6},ns^{2},np^{1} $$
  • $$ ( n- 1 )s^{2}p^{6}d^{10},ns^{1} $$
  • $$( n-1)p^{6},ns^{1}$$
  • $$ns^{2},np^{6},nd^{1}$$
Mendeleev corrected the atomic weight of :
  • $$Be$$
  • $$N$$
  • $$O$$
  • $$Cl$$
Identify the property which does not reflect the periodicity of the elements.
  • Bonding behaviour
  • Electronegativity
  • Ionization potential
  • Neutron-proton ratio
A pair of atomic numbers which belong to s-block are:
  • 7, 15
  • 6, 12
  • 9, 17
  • 3, 12
The correct order of the second ionisation potential of carbon, nitrogen, oxygen and fluorine is :
  • $$C>N>O>F$$
  • $$O>N>F>C$$
  • $$O>F>N>C$$
  • $$F>O>N>C$$
Number of short periods in Mendeleev's periodic table is :
  • $$2$$
  • $$3$$
  • $$4$$
  • $$1$$
The ionization energy of nitrogen is more than that of oxygen because :
  • of the extra stability of half-filled p orbitals in nitrogen
  • of the smaller size of nitrogen
  • the former contains less number of electrons
  • the former is less electronegative
Considering the chemical properties, atomic weight of $$Be$$ was corrected based on:
  • electronic configuration
  • valency
  • atomic number
  • both B and C
Ionisation potential of boron is less than that of beryllium. This is because :
  • B has $$ 1s^{2} 2s^{2} 2p^{1}$$ configuration
  • B has small atomic size
  • B has higher nuclear charge
  • B has more number of shells
Which has least ionization potential?
  • $$Li$$
  • $$Cs$$
  • $$Cl$$
  • $$I$$
The ionization potential of elements in any group decreases from top to bottom. This is due to :
  • increase in the size of an atom
  • increase in the atomic number
  • increase in the screening effect
  • both increase in the size of an atom and increase in the screening effect
The I.P. of sodium is 5.14 eV. The I.P. of potassium could be :
  • same as that of sodium
  • 5.68 eV
  • 4.34 eV
  • 10.28 eV
The electron configuration of elements A, B and C are $$ [He] 2s^{1},\ [Ne]3s^{1}$$ and $$[Ar] 4s^{1}$$ respectively. Which one of the following order is correct for the first ionization potentials $$(in\ KJ\ mol^{1})$$ of A, B and C? 
  • A > B > C
  • C > B > A
  • B > C > A
  • C > A > C
The high ionistion potential of magnesium compared with aluminium is due to :
  • filled orbitals in magnesium
  • high nuclear charge in magnesium
  • low radius of magnesium atom
  • low effective nuclear charge in magnesium
The ionisation potential is very low for :
  • $$Be$$
  • $$Mg$$
  • $$B$$
  • $$Al$$
Elements X, Y, and Z have atomic numbers $$19, 37$$, and $$55$$ respectively. Which of the following statements are true about them? 
  • Their ionization potential would increase with increasing atomic number
  • Y would have an ionization potential between those of X and Z
  • Z would have the highest ionization potential
  • Y would have the highest ionization potential
The $$IP_{1}$$ value of potassium is less than the $$IP_{1}$$ value of sodium. This is due to :
  • large size of potassium atom
  • small size of potassium atom
  • low density of potassium
  • univalent nature of potassium
The set representing the correct order of first ionisation potential is :
  • $$K>Na>Li$$
  • $$Be>Mg>Ca$$
  • $$B>C>N$$
  • $$Ge>Si>C$$
The incorrect statement among the following is :
  • the first ionisation potential of $$ Al$$ is less than the first ionisation potential of $$Mg$$
  • the second ionisation potential of $$Mg$$ is greater than the second ionisation potential of $$Na$$
  • the first ionisation potential of $$Na$$ is less than the first ionisation potential of $$Mg$$
  • the third ionisation of potential of $$Mg$$ is greatest
Beryllium shows diagonal relationship with aluminium. Which of the following similarity is incorrect? 
  • $$Be_{2}C$$ like$$ Al_{4}C_{3}$$ yields methane on hydrolysis
  • $$Be$$, like $$Al$$ is rendered passive by $$HNO_{3}$$
  • Be$$ (OH)_{2}$$ like $$Al(OH)_{3}$$ is basic
  • $$Be$$ forms beryllates and $$Al$$ forms aluminate
The decreasing order of the second ionization potential of $$K, \ Ca$$ and $$Ba$$ is :
  • $$K > Ca > Ba$$
  • $$Ca > Ba > K$$
  • $$Ba > K > Ca$$
  • $$K > Ba > Ca$$
Diagonal relationship is quite pronounced in the elements of:
  • $$ 2^{nd}$$ and $$3^{rd}$$ periods
  • $$ 1^{st}$$ and $$2^{nd}$$ periods
  • II and III groups
  • $$3^{rd}$$ and $$4^{th}$$ periods
The decreasing order of electron affinity of halogens is :
  • $$F > Cl > Br > I$$
  • $$F < Cl < Br < I$$
  • $$F < Cl > Br < I$$
  • $$Cl > F > Br > I$$
Boron is diagonally related to:
  • boron
  • aluminium
  • magnesium
  • silicon
Among the following four elements, the ionisation potential of which one is the highest?
  • Oxygen
  • Argon
  • Barium
  • Caesium
Boron and silicon resemble chemically. This is due to the equal value of their:
  • electron affinity
  • atomic volume
  • ions polarizing power
  • nuclear charge
Diagonal relationship is shown by
  • $$B - S$$
  • $$Li - Mg$$
  • $$Mg - Ca$$
  • $$S - Se$$
Which of the following will have high ionization potential?
  • $$Al^{3+}$$
  • $$F^{-}$$
  • $$Na^{+}$$
  • $$O^{2-}$$
If the ionization potential of calcium is five units then that of magnesium may be :
  • 6 Units
  • 5 Units
  • 4 Units
  • 2 Units
$$Al$$ has lower ionization potential than that of $$Mg$$ because :
  • $$Al$$ atom is bigger than $$Mg$$ atom
  • $$Mg$$ atom is bigger than $$Al$$ atom
  • all electrons in $$Mg$$ are paired, but those of $$Al$$ are not
  • all belongs to a higher group
The first I.P. values in electron volts of nitrogen and oxygen atoms are respectively given by :
  • $$14.6, \ 13.6$$
  • $$13.6,\ 14.6$$
  • $$13.6,\ 13.6$$
  • $$14.6,\ 14.6$$
As you go down in a group, the alkali metals become:
  • brighter
  • hotter
  • more reactive
  • less reactive
The following are some statements about diagonal relationship.
i) It is due to nearly same size, electronegativity and same polarising power
ii) $$Li$$ has similar properties with $$H_{2}$$
iii) $$BeO$$, $$Al_{2}O$$ are amphoteric in nature
iv) All $$d$$-block elements are stable
  • Only (i) correct
  • Only (ii) correct
  • Only (iii) correct
  • Only (iv) is correct
The ionization potential$$ (I_{1})$$ of nitrogen ($$Z=7$$) is more than oxygen ($$Z=8$$). This is explained by :
  • Hunds rule
  • Excitation rule
  • Pauli principle
  • Aufbau principle
The correct order of ionization energies is :
  • $$Zn < Cd < Hg $$
  • $$Hg < Cd < Zn$$
  • $$ Ar > Ne > He$$
  • $$Cs < Rb < Na$$
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