Grade 11 : Chemistry - Periodic Table (Set 4)

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Grade 11 : Chemistry - Periodic Table (Set 4)— Questions & Detailed Solutions

Ionization Stage $IE_1$ $IE_2$ $IE_3$ $IE_4$
Energy (kJ/mol) 738 1451 7733 10540
The table above lists the successive ionization energies for an unknown main-group element $X$. To which group of the periodic table does element $X$ belong?

Ionization Stage	$IE_1$	$IE_2$	$IE_3$	$IE_4$
Energy (kJ/mol)	738	1451	7733	10540

(A)

Group 1

(B)

Group 2

(C)

Group 13

(D)

Group 14

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: A huge jump in ionization energy occurs between $IE_2$ (1451 kJ/mol) and $IE_3$ (7733 kJ/mol), indicating that two electrons are present in the outermost valence shell. Removing the third electron requires breaking a stable noble-gas core. Hence, element $X$ has 2 valence electrons and belongs to Group 2 (alkaline earth metals).

Isoelectronic Species Series: $N^{3-}, O^{2-}, F^-, Na^+, Mg^{2+}, Al^{3+}$
Which of the following options correctly arranges these isoelectronic species in order of INCREASING ionic radius?

(A)

$Al^{3+} < Mg^{2+} < Na^+ < F^- < O^{2-} < N^{3-}$

(B)

$N^{3-} < O^{2-} < F^- < Na^+ < Mg^{2+} < Al^{3+}$

(C)

$Na^+ < Mg^{2+} < Al^{3+} < F^- < O^{2-} < N^{3-}$

(D)

$Al^{3+} < Na^+ < Mg^{2+} < N^{3-} < O^{2-} < F^-$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: For isoelectronic species (all having 10 electrons), ionic radius decreases as the nuclear charge (atomic number $Z$) increases. Nuclear charge order: $Al(13) > Mg(12) > Na(11) > F(9) > O(8) > N(7)$. Thus, $Al^{3+}$ has the strongest nuclear pull (smallest radius) and $N^{3-}$ has the weakest nuclear pull (largest radius).

Statement I: The first ionization enthalpy of Nitrogen (1402 kJ/mol) is higher than that of Oxygen (1314 kJ/mol).
Statement II: Nitrogen has a stable half-filled $2p^3$ electronic configuration, whereas Oxygen has a $2p^4$ electronic configuration.
Analyze both statements and choose the correct conclusion:

(A)

Both Statement I and Statement II are true, and Statement II is the correct explanation for Statement I.

(B)

Both Statement I and Statement II are true, but Statement II is NOT the correct explanation for Statement I.

(C)

Statement I is true, but Statement II is false.

(D)

Statement I is false, but Statement II is true.

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Nitrogen ($1s^2 2s^2 2p^3$) possesses an extra stable half-filled $2p$ subshell, making electron removal more difficult compared to Oxygen ($1s^2 2s^2 2p^4$), where removing one electron yields a stable half-filled $2p^3$ state. Hence, Statement II correctly explains Statement I.

Oxide $Na_2O$ MgO $Al_2O_3$ $SiO_2$ $P_4O_{10}$ $SO_3$ $Cl_2O_7$
Nature Basic Basic ? Acidic Acidic Acidic Acidic
Refer to the Period 3 oxide trend table above. Which oxide acts as an amphoteric oxide?

Oxide	$Na_2O$	MgO	$Al_2O_3$	$SiO_2$	$P_4O_{10}$	$SO_3$	$Cl_2O_7$
Nature	Basic	Basic	?	Acidic	Acidic	Acidic	Acidic

(A)

$Na_2O$

(B)

MgO

(C)

$Al_2O_3$

(D)

$SO_3$

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: Oxides of elements across Period 3 change from basic ($Na_2O, MgO$) to amphoteric ($Al_2O_3$) to acidic ($SiO_2, P_4O_{10}, SO_3, Cl_2O_7$). Aluminum oxide ($Al_2O_3$) reacts with both acids and bases to yield salt and water, defining its amphoteric nature.

Across a period from left to right in the periodic table, effective nuclear charge ($Z_{eff}$) experienced by valence electrons increases primarily because:

(A)

Nuclear charge $Z$ increases by 1 unit per element while inner core shielding increases only marginally as electrons enter the same valence shell.

(B)

The number of inner shell electrons decreases across a period.

(C)

Principal quantum number $n$ increases steadily across a period.

(D)

The shielding constant $\sigma$ decreases to zero across a period.

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: According to Slater's rules, electrons added to the same principal energy shell provide partial shielding ($\sigma \approx 0.35$ per electron), whereas the nuclear charge $Z$ increases by +1 for each element. Thus, $Z_{eff} = Z - \sigma$ increases across a period.

The electron gain enthalpy ($\Delta_{eg}H$) of Fluorine (-328 kJ/mol) is less negative than that of Chlorine (-349 kJ/mol). What is the primary reason for this anomaly?

(A)

Fluorine has a higher electronegativity than Chlorine.

(B)

The small size of the $2p$ subshell in Fluorine creates strong inter-electronic repulsions for the incoming electron.

(C)

Chlorine has empty $3d$ orbitals while Fluorine does not.

(D)

Fluorine has a higher ionization enthalpy than Chlorine.

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Due to the exceptionally small compact size of the $2p$ subshell in Fluorine, adding an incoming electron experiences significant electron-electron repulsion. In Chlorine, the incoming electron enters the larger $3p$ orbital, where repulsions are much lower, releasing more energy ($\Delta_{eg}H$ more negative).

Lithium (Group 1, Period 2) displays properties similar to Magnesium (Group 2, Period 3) due to a diagonal relationship.
Which of the following features is NOT a cause of the diagonal relationship between Lithium and Magnesium?

(A)

Similar ionic radii ($Li^+ = 76\text{ pm}, Mg^{2+} = 72\text{ pm}$)

(B)

Similar charge-to-radius ratio (polarizing power)

(C)

Similar electronegativity values ($Li \approx 1.0, Mg \approx 1.2$)

(D)

Identical number of valence electrons

View Correct Answer & Detailed Solution

✓ Correct Option: (D)

Explanation: Lithium has 1 valence electron ($2s^1$), while Magnesium has 2 valence electrons ($3s^2$). Their diagonal similarity arises from nearly equal ionic radii, similar electronegativity, and comparable polarizing power, NOT identical valence electron counts.

To which block of the periodic table does Lanthanum ($Z = 57$) strictly belong based on its ground-state electron configuration $[Xe] 5d^1 6s^2$?

(A)

s-block

(B)

p-block

(C)

d-block

(D)

f-block

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: Lanthanum ($Z = 57$) has the electron configuration $[Xe] 5d^1 6s^2$. The last electron enters the $5d$ orbital (before filling of $4f$ begins with Cerium $Z=58$). Hence, Lanthanum is classified as a d-block element in Group 3.

Which element has the highest electronegativity value on the Pauling scale ($3.98 \approx 4.0$)?

(A)

Fluorine ($F$)

(B)

Oxygen ($O$)

(C)

Chlorine (Cl)

(D)

Helium (He)

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Fluorine is the most electronegative element in the periodic table with a Pauling value of 4.0, owing to its small atomic radius and high effective nuclear charge. Noble gases like Helium generally do not have assigned electronegativities on the Pauling scale.

Q10

Element $IE_1$ (kJ/mol) $IE_2$ (kJ/mol)
P 496 4562
Q 738 1451
R 578 1817
S 786 1577
Based on the ionization enthalpy data above, which element is an Alkali Metal?

Element	$IE_1$ (kJ/mol)	$IE_2$ (kJ/mol)
P	496	4562
Q	738	1451
R	578	1817
S	786	1577

(A)

Element P

(B)

Element Q

(C)

Element R

(D)

Element S

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Alkali metals (Group 1) have relatively low $IE_1$ values and extremely high $IE_2$ values due to reaching a stable noble gas configuration after losing 1 electron. Element P shows $IE_1 = 496\text{ kJ/mol}$ and a massive jump to $IE_2 = 4562\text{ kJ/mol}$ (nearly 9-fold increase), identifying it as Sodium (Na).

Q11

According to Mulliken's scale, the electronegativity ($\chi_M$) of an atom is expressed in terms of ionization enthalpy (IE) and electron affinity (EA) in eV as:

(A)

$\chi_M = IE - EA$

(B)

$\chi_M = \frac{IE + EA}{2}$

(C)

$\chi_M = \frac{IE + EA}{5.6}$

(D)

$\chi_M = \sqrt{IE \times EA}$

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: On the Mulliken scale, electronegativity is defined as the arithmetic mean of the ionization energy and electron affinity of an atom: $\chi_M = \frac{IE + EA}{2}$ (when IE and EA are measured in electron-volts, eV).

Q12

Statement I: Metallic character of elements increases as we move down a group.
Statement II: Atomic size increases down a group, leading to a decrease in ionization enthalpy and greater ease of cation formation.
Choose the correct assessment of Statements I and II:

(A)

Both Statement I and Statement II are true, and Statement II is the correct explanation of Statement I.

(B)

Both Statement I and Statement II are true, but Statement II is NOT the correct explanation of Statement I.

(C)

Statement I is true, but Statement II is false.

(D)

Statement I is false, but Statement II is true.

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: As we go down a group, additional energy shells are added, increasing atomic size and shielding. This weakens the attraction between the nucleus and outer electrons, lowering ionization enthalpy. Ease of losing electrons increases metallic character, making Statement II the direct explanation of Statement I.

Q13

What is the trend in valency of elements with respect to Hydrogen across Period 3 (from Na to Cl)?

(A)

Increases continuously from 1 to 7

(B)

Remains constant at 1 for all elements

(C)

Increases from 1 to 4 and then decreases from 4 to 1

(D)

Decreases from 7 to 1

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: Valency with respect to Hydrogen follows the number of valence electrons up to Group 14, then $(8 - \text{valence electrons})$: $NaH(1), MgH_2(2), AlH_3(3), SiH_4(4), PH_3(3), H_2S(2), HCl(1)$. Hence, it increases from 1 to 4 and then decreases to 1.

Q14

The maximum covalency of second-period elements (such as B, C, N, O, F) is strictly limited to 4 because:

(A)

They have small atomic radii.

(B)

They lack vacant d-orbitals in their valence shell ($n=2$).

(C)

They have very high electronegativity values.

(D)

They cannot form covalent bonds.

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Second period elements have only four valence orbitals available for bonding (one $2s$ and three $2p$ orbitals). Because $n=2$ has no $2d$ subshell, these elements cannot expand their octet beyond 4 covalent bonds, unlike Period 3+ elements.

Q15

Which of the following represents the correct increasing order of atomic radii for Fluorine ($F$), Oxygen ($O$), Nitrogen ($N$), and Carbon ($C$)?

(A)

$F < O < N < C$

(B)

$C < N < O < F$

(C)

$O < F < N < C$

(D)

$F < N < O < C$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Across a period from left to right, atomic size decreases due to an increase in effective nuclear charge ($Z_{eff}$). Moving from Carbon ($Z=6$) to Fluorine ($Z=9$), radii decrease in the order: $C (77\text{ pm}) > N (74\text{ pm}) > O (66\text{ pm}) > F (64\text{ pm})$. In increasing order: $F < O < N < C$.

Q16

An element $M$ has the valence electron configuration $n=4, l=1$ with 5 electrons in its $4p$ subshell ($4p^5$).
Identify the Period and Group number of element $M$ in the modern periodic table.

(A)

Period 3, Group 15

(B)

Period 4, Group 15

(C)

Period 4, Group 7

(D)

Period 4, Group 17

View Correct Answer & Detailed Solution

✓ Correct Option: (D)

Explanation: The principal quantum number $n=4$ indicates Period 4. The valence configuration is $4s^2 4p^5$. For p-block elements, Group number $= 12 + \text{number of p electrons} = 12 + 5 = 17$ (Halogens). Element $M$ is Bromine (Br).

Q17

Among the hydrides of Group 16 elements ($H_2O, H_2S, H_2Se, H_2Te$), which hydride exhibits the STRONGEST acidic character?

(A)

$H_2O$

(B)

$H_2S$

(C)

$H_2Te$

(D)

$H_2Se$

View Correct Answer & Detailed Solution

✓ Correct Option: (C)

Explanation: Down Group 16, atomic size of the central atom increases ($O < S < Se < Te$), which increases bond length and decreases $H-E$ bond dissociation enthalpy. As $H-Te$ bond is weakest, $H_2Te$ dissociates most easily to release $H^+$, making it the strongest acid in the group.

Q18

Atom H C N O F
Pauling Electronegativity 2.1 2.5 3.0 3.5 4.0
Using the electronegativity data above, which of the following covalent bonds has the HIGHEST polarity (dipole moment magnitude)?

Atom	H	C	N	O	F
Pauling Electronegativity	2.1	2.5	3.0	3.5	4.0

(A)

$H-F$

(B)

$H-O$

(C)

$C-F$

(D)

$N-H$

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Bond polarity is directly proportional to the electronegativity difference ($\Delta \chi$) between the bonded atoms.
$\Delta \chi(H-F) = 4.0 - 2.1 = 1.9$
$\Delta \chi(H-O) = 3.5 - 2.1 = 1.4$
$\Delta \chi(C-F) = 4.0 - 2.5 = 1.5$
$\Delta \chi(N-H) = 3.0 - 2.1 = 0.9$
The $H-F$ bond has the maximum difference (1.9) and hence highest polarity.

Q19

Why do Noble Gases (Group 18) have large POSITIVE electron gain enthalpies ($\Delta_{eg}H > 0$)?

(A)

They have small atomic radii and strong nuclear attraction.

(B)

They possess stable, completely filled valence octets ($ns^2 np^6$), forcing the added electron to enter a higher principal energy level ($n+1$)s.

(C)

They are non-metallic gases at room temperature.

(D)

Their effective nuclear charge is zero.

View Correct Answer & Detailed Solution

✓ Correct Option: (B)

Explanation: Noble gases have a stable closed-shell configuration ($ns^2 np^6$). Adding an extra electron requires forcing it into a higher energy shell ($(n+1)s$), which experiences heavy shielding and is energetically unfavorable. Energy must be supplied, resulting in a positive $\Delta_{eg}H$.

Q20

According to IUPAC nomenclature for superheavy elements ($Z > 100$), what is the systematic name and symbol for element with atomic number $Z = 114$?

(A)

Ununquadium (Uuq)

(B)

Ununtrium (Uut)

(C)

Ununpentium (Uup)

(D)

Unbiquadium (Ubq)

View Correct Answer & Detailed Solution

✓ Correct Option: (A)

Explanation: Using IUPAC numerical roots: 1 = 'un', 4 = 'quad'. For 114: un + un + quad + ium = Ununquadium (symbol Uuq). (Officially named Flerovium, Fl).

grade 11chemistryperiodic tableperiodic trendsionization energyelectronegativity

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Grade 11 : Chemistry - Periodic Table (Set 4)

Grade 11 : Chemistry - Periodic Table (Set 4)— Questions & Detailed Solutions

Ionization Stage$IE_1$$IE_2$$IE_3$$IE_4$Energy (kJ/mol)7381451773310540The table above lists the successive ionization energies for an unknown main-group element $X$. To which group of the periodic table does element $X$ belong?

Isoelectronic Species Series: $N^{3-}, O^{2-}, F^-, Na^+, Mg^{2+}, Al^{3+}$Which of the following options correctly arranges these isoelectronic species in order of INCREASING ionic radius?

Oxide$Na_2O$MgO$Al_2O_3$$SiO_2$$P_4O_{10}$$SO_3$$Cl_2O_7$NatureBasicBasic?AcidicAcidicAcidicAcidicRefer to the Period 3 oxide trend table above. Which oxide acts as an amphoteric oxide?

Across a period from left to right in the periodic table, effective nuclear charge ($Z_{eff}$) experienced by valence electrons increases primarily because:

The electron gain enthalpy ($\Delta_{eg}H$) of Fluorine (-328 kJ/mol) is less negative than that of Chlorine (-349 kJ/mol). What is the primary reason for this anomaly?

Lithium (Group 1, Period 2) displays properties similar to Magnesium (Group 2, Period 3) due to a diagonal relationship.Which of the following features is NOT a cause of the diagonal relationship between Lithium and Magnesium?

To which block of the periodic table does Lanthanum ($Z = 57$) strictly belong based on its ground-state electron configuration $[Xe] 5d^1 6s^2$?

Which element has the highest electronegativity value on the Pauling scale ($3.98 \approx 4.0$)?

Element$IE_1$ (kJ/mol)$IE_2$ (kJ/mol)P4964562Q7381451R5781817S7861577Based on the ionization enthalpy data above, which element is an Alkali Metal?

According to Mulliken's scale, the electronegativity ($\chi_M$) of an atom is expressed in terms of ionization enthalpy (IE) and electron affinity (EA) in eV as:

Statement I: Metallic character of elements increases as we move down a group.Statement II: Atomic size increases down a group, leading to a decrease in ionization enthalpy and greater ease of cation formation.Choose the correct assessment of Statements I and II:

What is the trend in valency of elements with respect to Hydrogen across Period 3 (from Na to Cl)?

The maximum covalency of second-period elements (such as B, C, N, O, F) is strictly limited to 4 because:

Which of the following represents the correct increasing order of atomic radii for Fluorine ($F$), Oxygen ($O$), Nitrogen ($N$), and Carbon ($C$)?

An element $M$ has the valence electron configuration $n=4, l=1$ with 5 electrons in its $4p$ subshell ($4p^5$).Identify the Period and Group number of element $M$ in the modern periodic table.

Among the hydrides of Group 16 elements ($H_2O, H_2S, H_2Se, H_2Te$), which hydride exhibits the STRONGEST acidic character?

AtomHCNOFPauling Electronegativity2.12.53.03.54.0Using the electronegativity data above, which of the following covalent bonds has the HIGHEST polarity (dipole moment magnitude)?

Why do Noble Gases (Group 18) have large POSITIVE electron gain enthalpies ($\Delta_{eg}H > 0$)?

According to IUPAC nomenclature for superheavy elements ($Z > 100$), what is the systematic name and symbol for element with atomic number $Z = 114$?

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Ionization Stage $IE_1$ $IE_2$ $IE_3$ $IE_4$
Energy (kJ/mol) 738 1451 7733 10540
The table above lists the successive ionization energies for an unknown main-group element $X$. To which group of the periodic table does element $X$ belong?

Isoelectronic Species Series: $N^{3-}, O^{2-}, F^-, Na^+, Mg^{2+}, Al^{3+}$
Which of the following options correctly arranges these isoelectronic species in order of INCREASING ionic radius?

Oxide $Na_2O$ MgO $Al_2O_3$ $SiO_2$ $P_4O_{10}$ $SO_3$ $Cl_2O_7$
Nature Basic Basic ? Acidic Acidic Acidic Acidic
Refer to the Period 3 oxide trend table above. Which oxide acts as an amphoteric oxide?

Lithium (Group 1, Period 2) displays properties similar to Magnesium (Group 2, Period 3) due to a diagonal relationship.
Which of the following features is NOT a cause of the diagonal relationship between Lithium and Magnesium?

Element $IE_1$ (kJ/mol) $IE_2$ (kJ/mol)
P 496 4562
Q 738 1451
R 578 1817
S 786 1577
Based on the ionization enthalpy data above, which element is an Alkali Metal?

Statement I: Metallic character of elements increases as we move down a group.
Statement II: Atomic size increases down a group, leading to a decrease in ionization enthalpy and greater ease of cation formation.
Choose the correct assessment of Statements I and II:

An element $M$ has the valence electron configuration $n=4, l=1$ with 5 electrons in its $4p$ subshell ($4p^5$).
Identify the Period and Group number of element $M$ in the modern periodic table.

Atom H C N O F
Pauling Electronegativity 2.1 2.5 3.0 3.5 4.0
Using the electronegativity data above, which of the following covalent bonds has the HIGHEST polarity (dipole moment magnitude)?