A Geometric isomerism
B Optical isomerism
C Linkage isomerism
D Ionization isomerism
Explanation: NO2- is an ambidentate ligand that can bind through N or O. This gives rise to linkage isomerism: -NO2 (nitro) vs -ONO (nitrito).
Explanation: BF3 has three bonding pairs and no lone pairs on boron, requiring sp2 hybridization and trigonal planar geometry.
A KMnO4
B H2O2
C Na
D Cl2
Explanation: Sodium (Na) is a strong reducing agent because it readily loses its valence electron to form Na+, getting oxidized in the process.
A Tetrahedral
B Square planar
C See-saw
D Square pyramidal
Explanation: XeF4 has sp3d2 hybridization with 4 bonding pairs and 2 lone pairs. The lone pairs are trans to each other, giving square planar geometry.
A CH3CH2OH
B CH3CH(OH)CH3
C CH3CH(OH)COOH
D CH3COCH3
Explanation: CH3CH(OH)COOH (lactic acid) has a chiral carbon bonded to four different groups (-H, -OH, -CH3, -COOH), exhibiting optical isomerism.
A 3.74
B 4.74
C 5.74
D 7.00
Explanation: pH = pKa + log([salt]/[acid]). When [salt] = [acid], pH = pKa = -log(1.8 x 10^-5) = 4.74.
Explanation: In hydrogen (single electron system), energy depends only on n. 3s has n=3, which is higher than n=2 (2s, 2p) and n=1 (1s).
A KMnO2
B KMnO3
C KMnO4
D K2MnO4
Explanation: Potassium permanganate has the formula KMnO4, where Mn is in the +7 oxidation state and is a powerful oxidizing agent.
A Sodium
B Iron
C Silicon
D Chlorine
Explanation: Iron (Fe, Z=26) has partially filled 3d orbitals ([Ar] 3d6 4s2), placing it in the d-block of the periodic table.
A 0.5 mole
B 1 mole
C 2 moles
D 1.5 moles
Explanation: CaCO3 decomposes as: CaCO3 -> CaO + CO2. One mole of CaCO3 produces exactly one mole of CO2.
A [Ar] 3d9 4s2
B [Ar] 3d10 4s1
C [Ar] 3d8 4s2 4p1
D [Ar] 3d10 4s2
Explanation: Copper is an exception to the expected configuration. One 4s electron is promoted to 3d to achieve a fully filled 3d10 subshell for extra stability.
A H-H
B O-O
C H-Cl
D Na-Cl
Explanation: H-Cl has an electronegativity difference of 0.9, resulting in unequal electron sharing (polar covalent bond). Na-Cl is ionic, and H-H and O-O are nonpolar.
Explanation: Magnesium (Mg) loses its two valence electrons to achieve a stable neon-like configuration, forming Mg2+ with a +2 charge.
A CH3OH
B CH3OCH3
C CH3COOH
D CH3CHO
Explanation: CH3OCH3 (dimethyl ether) has an oxygen atom bonded between two alkyl groups (R-O-R\'), which defines the ether functional group.
A Positive
B Negative
C Zero
D Variable
Explanation: By convention, the standard enthalpy of formation of any element in its most stable standard state is defined as zero.
Explanation: Benzene (C6H6) has 6 C-H sigma bonds + 6 C-C sigma bonds in the ring = 12 sigma bonds, plus 3 delocalized pi bonds.
A Acetic acid
B Ammonia
C Sodium chloride
D Ethanol
Explanation: NaCl completely dissociates into Na+ and Cl- ions in water, making it a strong electrolyte. The others are weak electrolytes or nonelectrolytes.
Explanation: In KMnO4: +1(K) + Mn + 4(-2)(O) = 0, so Mn = +7.
A Plasma
B Bose-Einstein condensate
C Photonic state
D Fermionic condensate
Explanation: Plasma, Bose-Einstein condensate, and fermionic condensate are recognized states of matter. \'Photonic state\' is not a recognized state of matter.
A Ethyl chloride
B Ethyl ethanoate
C Diethyl ether
D Acetaldehyde
Explanation: Ethanol reacts with ethanoic acid in an esterification reaction to form ethyl ethanoate (an ester) and water.