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Chemistry Highly Challenging Topics 221 A&R Items XI and XII Full
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Spread the Happiness. Assertion and Reason Statements Feedback: 9008271516CHEMISTRY _ FULL SYLLABUS _ CHALLENGING TOPICS
S# Correct Assertion Correct Reason
A negative ΔG indicates a spontaneous reaction ΔG < 0 signifies energy release (ΔG = ΔH - TΔS) favoring
1
at constant temperature and pressure. product formation.
Strong acids promote dehydration of alcohols Acid weakens O-H bond, facilitating H O elimination (R-OH
2
via elimination. + H → R + H O).
Uneven electron distribution creates a dipole Separation of positive and negative charges creates a
3
moment (μ). polar molecule with a dipole moment (μ).
ΔG determines reaction spontaneity at constant Negative ΔG suggests a spontaneous reaction (ΔG < 0),
4
temperature and pressure. while positive ΔG indicates non-spontaneity (ΔG > 0).
Leaving group stability affects the rate of More stable leaving groups (e.g., Br vs. OH ) depart faster
5
elimination reactions. in elimination reactions (R-X → R + X ).
Dipole moment (μ) measures a molecule's μ arises from the unequal distribution of electrical charge
6 polarity. within a molecule. Uneven electron distribution creates a
separation of positive and negative charges.
Stronger bond enthalpies (ΔHbond) lead to Stronger bonds (higher ΔHbond) require more energy to
7 higher thermal stability. break, making the molecule more resistant to
decomposition at high temperatures.
Enthalpy change (ΔH) reflects heat absorbed or ΔH signifies the system's overall energy change at
8
released in a reaction. constant pressure (ΔH < 0 indicates exothermic).
Enthalpy of reaction (ΔH ) is the difference in ΔH reflects the energy change associated with the
9 enthalpies of formation between reactants and reaction process.
products.
POAC (Point of Average Concentration) helps POAC identifies the point where the average analyte
10
determine the equivalence point in titrations. concentration equals the titrant concentration.
The modern periodic table organizes elements This organization reveals periodic trends in properties and
11 based on atomic number and electron chemical behavior.
configuration.
Optical isomers rotate plane-polarized light Their non-mirror-image structure leads to distinct
12
differently due to their asymmetry. interactions with the electric field of polarized light.
Acid strength is assessed using factors like Stronger acids readily donate protons, causing observable
13 reactivity with metals or indicators. reactions (e.g., hydrogen gas evolution with metals).
NAR (Nucleophilic Acyl Substitution) involves A nucleophile displaces a leaving group on an acyl
14
nucleophilic attack on an acyl carbonyl group. derivative.
Synergic bonding in metal carbonyls enhances Interactions between the metal and multiple CO ligands
15
overall bond strength. contribute to this increased stability.
E-Z isomers differ in the relative placement ofThe "E" configuration has similar groups on the same
16
substituent groups around a double bond. side, while "Z" has them on opposite sides.
Carbocations and carbanions prefer different Carbocations favor electron-donating groups nearby, while
17 stabilizing groups. carbanions prefer electron-withdrawing substituents for
stabilization.
Molar heat capacity (Cm) depends on the amount It's a property of a substance, not the total mass (m).
18
of substance (moles, n).
Increased temperature (T) leads to higher Faster particle movement due to higher temperature.
19
average kinetic energy of particles.
Raoult's Law predicts the partial pressure P_component relates to its mole fraction (X_component)
(P_component) of a component in an ideal and the pure component's vapor pressure (P_pure) using
20
solution. the formula: P_component = X_component * P_pure.
Balanced chemical equations determine the Stoichiometric coefficients represent mole ratios
21
mass ratio of reactants needed. convertible to mass ratios using molar masses (M).
The wave function (Ψ) in Schrödinger's equation Ψ²(r) (wave function squared) represents the probability
22 describes electron probability density (P(r)). density at a specific location (r) (P(r) = Ψ²(r)).
Zero-order reactions exhibit a constant reaction The rate-determining step is independent of reactant
23 rate regardless of reactant concentration. concentration (Rate = k).
Chlorine (Cl ) and hydrochloric acid (HCl) are They share properties like high electron affinity and
24
both halogens (Group 17 elements). forming single covalent bonds.
Back bonding strengthens metal-ligand bonds in Electron donation occurs from a metal d-orbital to an
25
coordination compounds. empty ligand p-orbital.
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, Spread the Happiness. Assertion and Reason Statements Feedback: 9008271516
CHEMISTRY _ FULL SYLLABUS _ CHALLENGING TOPICS
S# Correct Assertion Correct Reason
SHE (Standard Hydrogen Electrode) sets the Establishes a baseline (E°(SHE) = 0 V) for measuring
26 reference point for electrode potentials (E°(SHE) potentials of other electrodes (V).
= 0 V by convention).
Geometrical isomers arise from restricted Restricted rotation hinders free movement, leading to
27 rotation around double bonds or lone pairs on a distinct 3D arrangements of ligands in complexes.
central atom.
Concentration relationship: C V = C V This formula helps determine the final concentration (C )
28 (assuming constant temperature and negligible after mixing solutions of known volumes (V , V ) and
volume change). concentrations (C ).
Faraday's first law (m = QIt/F) relates deposited The mass (m) of material deposited at an electrode is
mass (m) to charge (Q) passed during directly proportional to the current (I) flowing through the
29
electrolysis. electrolyte and electrolysis time (t), with F being the
Faraday's constant (C/mol).
Enthalpy of combustion (ΔH_c) is calculated This equation considers the enthalpy changes of formation
using ΔH_c = Σ nΔH_f (products) - Σ mΔH_f (ΔH_f) for reactants (m moles) and products (n moles) to
30
(reactants) (all in kJ/mol). determine the heat of combustion (ΔH_c) per mole of
reactant.
Law of Chemical Equivalence: Reactant This ensures balanced electron transfer between reactants
31 quantities (in moles) are proportional to their based on their gram equivalents (eq), achieving a complete
gram equivalents (eq) for a complete reaction. reaction.
Arrangement of atoms determines the number of The specific arrangement of atoms within a molecule
32 isomers. dictates the number of possible isomers (different spatial
arrangements).
Nernst equation (E = E° - (RT/nF)ln(Q)) relates The potential difference (E) between an electrode and a
electrode potential (E) to the reaction quotient reference electrode (e.g., SHE) depends on the
33
(Q). concentrations of reactants and products (represented by
the dimensionless reaction quotient, Q).
Limiting reagent dictates the amount of product The completely consumed reactant (limiting reagent) limits
34 formed in a reaction. the reaction's progress, determining the maximum product
yield based on stoichiometry.
The number of structural isomers depends on The arrangement of atoms within the molecule, influenced
35 factors like functional groups and chain length. by functional groups and chain length, determines the
number of possible structural isomers.
Faraday's first law (m = QIt/F) allows calculating This formula (m = QIt/F) helps determine the mass (m) of a
36 the mass deposited during electrolysis. substance produced at an electrode based on the charge
(Q) passed, current (I), and electrolysis time (t).
Heat of combustion (ΔH_c) signifies energy ΔH_c (calculated using ΔH_f values) indicates energy
37 change (kJ/mol) during combustion. absorbed (positive ΔH_c) or released (negative ΔH_c)
during a substance's combustion process.
Law of Chemical Equivalence ensures balanced Stoichiometric ratios dictate the amount of each reactant
38 electron transfer in reactions. needed (based on gram equivalents, eq) for complete
consumption via balanced electron transfer.
Reaction with NaHSO3 depends on the specific NaHSO3 acts as a reducing agent, targeting specific
39 functional group(s) present in the organic functional groups within the organic molecule for
molecule. reactions (formula not applicable - reaction specific).
Dilution reduces solution concentration (C) (e.g., Adding solvent increases the total volume (V) of the
Molarity (M)). solution while keeping the amount of solute constant (C V
40
= C V ). This results in a decrease in solution
concentration (C).
Hydrolysis breaks down salts (WA and WB) into This reaction helps understand the behavior of ionic
41 their constituent ions (W , A , etc.) in water. compounds (WA & WB) in aqueous solutions (H O).
Buffer solutions resist changes in pH upon Buffers contain a weak acid (HA) and its conjugate base
42 addition of small amounts of acid (H ) or base (A ) or vice versa, allowing them to neutralize small pH
(OH ). shifts through the equilibrium: HA H + A .
Buffer capacity (β) of a solution depends on the A higher ratio of [A ] to [HA] (within limits) indicates a
concentration of the weak acid (HA) and its greater buffer capacity (β) to resist pH changes.
43 conjugate base (A ) according to the Henderson-
Hasselbalch equation: pH = pKa + log([A ]/[HA]).
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