MCQ Questions for Class 11 Medical Chemistry Classification Of Elements And Periodicity In Properties Quiz 13

An element Y has the proton number 18 .The next element of the periodic table is an element Z.
Which statement is correct?

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Element Z has 1 more electron in its outer shell than element Y.
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Element Z has 1 more electron shell than element Y.
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Element Z is in the same group of the periodic table as element Y.
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Element Z is in the same period of the periodic table as element Y.

The IUPAC name of the element having atomic number 109 is

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Unniloctium
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Unnilquadium
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Unnilennium
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Ununseptium

The electronic configuration of an element is

$1{ s }^{ 2 }2{ s }^{ 2 }2{ p }^{ 6 }3{ s }^{ 2 }3{ p }^{ 6 }3{ d }^{ 5 }4{ s }^{ 1 }.$ This represents its:

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excited state
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ground state
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cationic form
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none

The correct order of second I. E. of C, N, O and F are in the order :

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F > O > N > C
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C > N > O > F
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O > N > F > C
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O > F > N > C

Which of the following is not correct increasing order of ionisation energy

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$Cl^{-} < Ar < K^{+}$
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Au < Ag < Cu
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Cs < Rb < K
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K < Ca < Sc

Explanation

Ionization energy of gold is more than copper and silver because of poor shielding of 4f electrons nucleus has more attraction on s-orbital electrons.

so correct order is

$Au > Cu> Ag$

The elements with the lowest number that has a ground state electronic configuration of

$\left( {n - 1} \right){d^6}n{s^2}$ is located in the :

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fifth period
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sixth period
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fourth period
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third period

Explanation

For d, minimum orbital is

$3d$ , which is in the fourth period {Option C}

Group I elements of the periodic table are known as:

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Alkali metals
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Alkaline earth metals
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Inert gases
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None of these

Which of the following atoms has the highest first ionisation energy?

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$Na$
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$K$
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$Cs$
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$Rb$

Which of the following has maximum ionization potential?

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$Al$
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$P$
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$Si$
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$Mg$

General electronic configuration of outermost and penultimate shell is

$(n-1) s^2(n - 1)p^6(n - 1)d^x ns^2$ . If

$n = 4$ and

$x = 5$ , then the number of protons in the nucleus will be:

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$> 25$
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$< 24$
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$25$
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$30$

Which one of the following is not a monoatomic element ?

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Copper
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Helium
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Iodine
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Barium

Select the correct order of first ionization potential :

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$N > O_2$
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$O_2 > N$
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$O_2 = N$
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None of these

Which of the following is incorrect ?

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Among $Cl, Ar$ and $K,K$ has the smallest ionization potential
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Among $CH_4 ,NH_3$ and $HF, HF$ has the highest boiling point
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Among $Cl_2, Br_2$ and $I_2 , Br_ 2$ has the lowest boiling point
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Among $HOl$ and $HOBr$ and $HOCl, HOl$ is the weakest

Sodium has, as compared to potassium:

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less electronegativity
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more ionisation potential
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larger atomic radius
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lower melting point

Explanation

Element

$Na$

$K$

$IE_1$

$496$

$419$

$IE_2$

$4562$

$3051$

sodium has higher

$I.E$ because of smaller atomic size.

Option B is correct.

An element having electronic configuration

$1s^{2}, 2s^{2}, 2p^{6}, 3s^{2},3p^{6}, 4s^{1}$ will form:

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Acidic oxide
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Basic oxide
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Amphoteric oxide
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Neutral oxide

The ionisation enthalpy of isotopes of an element will be:

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same
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different
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dependent on atomic masses
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dependent on the number of neutrons present in the nucleus

The set representing the correct order of first ionisation enthalpy is :

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K > Na > Li
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Be > Mg > Ca
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B > C > N
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Ge > Si > C

In which of the following arrangements, the order is not according to the property indicated against it?

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$Al^{3+} < Mg^{2+} < Na^+ < F^-$ increasing ionic size
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B < C < N < O increasing first ionisation enthalpy
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I < Br < F < Cl increasing electron gain enthalpy (with negative sign)
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Li < Na < K < Rb increasing metallic radius

Explanation

First

$IE$ of N will be maximum as it has a half filled orbital providing it extra stability.

Potassium forms

$K^+$ ion but it does not form

$K^{2+}$ because of

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Very low value of $(I.E.)_1$ and $(I.E.)_2$
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Very high value of $(I.E.)_1$ and $(I.E.)_2$
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Low value of $(I.E.)_1$ and low value of $(I.E.)_2$
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Low value of $(I.E.)_1$ and high value of $(I.E.)_2$

Explanation

$K \xrightarrow {I.E._1} K^+ \xrightarrow {I.E._2} K^{2+}$

$I.E._2 > > I.E._1$

$\therefore$ Potassium gets ionized only once after which it attains inert gas configuration.

$K^+ = 1s^2, 2s^2 2p^6, 3s^23p^6$

In the following, the element with the highest ionisation energy is :

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$[Ne] 3s^2 3p^1$
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$[Ne] 3s^23p^3$
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$[Ne] 3s^2 3p^2$
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$[Ne]3s^2 3p^4$

Explanation

$[Ne]3s^23p^3$ is a symmetrical configuration or half-filled stability thus, this atom has extra stability. So, this element will have the highest ionisation energy.

For the process

$A_{(g)} + e^- \longrightarrow A_{(g)}; \quad \Delta H = x$
and

$A^- _{(g)} \longrightarrow A_{(g)} + e^-; \quad \Delta H = y$

Select correct alternate:

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Ionization energy of $A^-_{(g)}$ is $y.$
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Electron affinity of $A_{(g)}$ is $x.$
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Electron affinity of $A_{(g)}$ is $-y.$
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All are correct statements

In which of the following arrangements, the order is NOT according to the property indicated against it?

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$Li < Na < K < Rb$ : increasing metallic radius
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$I < Br < F < Cl$ : increasing electron gain enthalpy
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$B < C < N < O$ : increasing first ionization enthalpy
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$Al^{3+} < Mg^{2+} < Na^+< F^-:$ increasing ionic size

Explanation

Ionisation energy of

$N$ is greater than

$O$ due to its half-filled 2p - subshell.

So, the correct order is:

$B < C < O < N$ : increasing first ionization enthalpy.

The element with atomic number 3 to 10 belong to the second period. Identify the most electropositive and most electronegative element in this period.

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$F, Li$
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$Li, F$
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$Li, Ne$
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$Ne, Li$

Assign the position of the element having outer electronic configuration,
(A)

$ns^2np^2\,(n =6)$
(B)

$(n - 1)d^2ns^2\,(n=4)$
(C)

$(n-2)f^7(n-1)d^{1}ns^2\,(n=6)$
Which of the following statement(s) is/are correct?

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The element A belongs to $3^{rd}$ periods and $16^{th}$ groups.
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The element ‘A belongs to $6^{th}$ periods and $14^{th}$ groups.
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The element 'C’ belongs to $6^{th}$ period and is a lanthanide element
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All A, B, C elements are metals

Explanation

The ground state electron configuration of A is $[Xe]\; 4f^{14}.\;5d^{10}.\;6s^2\;6p^2$ .

Group: 14, Period : 6

The electronic configuration of B is $[Ar]\;3d^2\;4s^2$ .

Group : 4, Period : 4

The electronic configuration of C is $[Xe]\; 4f^7 \;5d^1\; 6s^2$

Group :Lanthanide, Period : 6

Which of the following atomic species has maximum ionization energy?

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$O^-$
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$S^-$
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$Se^-$
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$Te^-$

Which of the following pairs of elements have the same number of electrons in their outermost shell?

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Mn, Fe
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Na, Sr
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As, Bi
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Se, Te

Explanation

$As: 4s^2\;4p^3$

$Bi: 6s^2\;6p^3$

$Se: 4s^2\;4p^4$

$Te: 5s^2\;5p^3$

Hence option C and D are correct

An element of the

$4th$ period which has maximum number of unpaired electrons is :

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$_{20} Ca$
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$_{24}Cr$
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$_{30}Zn$
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$_{33} As$

The first ionization potential of

$Mg , Al , P$ and

$S$ follows the order:

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$Mg < Al < P < S$
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$Al < Mg < P < S$
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$Al < Mg < S < P$
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$Mg < Al < S < P$

Explanation

Because of extra stability of exactly half-filled electronic configuration of P its

$IE_{1}$ is higher than that of S. Further the

$IE_{1}$ of Mg is higher than that of Al because in case of Mg , electron is to be removed from a

$3s$ - orbital while in case of Al, the electron is to be removed from a

$3p$ orbital. Thus option (c), i.e.,

$Al < Mg < S < P$ is correct.

Hence option C is correct

The first ionization enthalpies of the given elements are in the order of:

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$C < N < Si < P$
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$N < Si < C < P$
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$Si < P < C < N$
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$P < Si < N < C$

If there were 10 periods in the periodic table and each orbital could have maximum 4 electrons, then how many maximum number of elements would be present in period 9?

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100
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125
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150
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90

The first ionization energies of

$Na , Mg , Al$ and

$Si$ are in the order :

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$Na < Mg > Al < Si$
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$Na > Mg > Al < Si$
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$Na > Mg > Al > Si$
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$Na < Mg < Al < Si$

The highly metallic element will have the configuration of :

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$2 , 8 , 7$
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$2 , 8 , 8 , 5$
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$2 , 8 , 8 , 1$
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$2 , 8 , 2$

CBSE Questions for Class 11 Medical Chemistry Classification Of Elements And Periodicity In Properties Quiz 13 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

CBSE Questions for Class 11 Medical Chemistry Classification Of Elements And Periodicity In Properties Quiz 13 - MCQExams.com

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Practice Class 11 Medical Chemistry Quiz Questions and Answers

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