Chemistry Anomalies Quiz

Identify the incorrect statement among the following:

• Gallium (Ga) has a lower melting point than expected due to its d10 electron configuration, affecting metallic bonding strength.

• Aluminium (Al) exhibits a higher oxidation state more readily than thallium (Tl), aligning with the general expectations for group 13 elements.

• Bismuth (Bi) exhibits more stable +5 oxidation state compounds due to inert pair effect.

Identify the incorrect statement among the following:

• The acidity of hydrides increases from NH3 to BiH3 in group 15, showcasing a trend where heavier elements form more acidic hydrides.

• Water (H2O) is less acidic than hydrogen sulfide (H2S), illustrating the trend of increasing acidity with heavier chalcogens.

• Ammonia (NH3) is more acidic than phosphine (PH3), an anomaly in the trend of acidity within group 15 hydrides.

Identify the incorrect statement among the following:

• Iodine (I2) sublimates at room temperature, an unusual property for a non-metal and indicative of its weak van der Waals forces.

• Xenon's ability to form compounds with fluorine and oxygen challenges the notion of complete noble gas inertness, due to its relatively large atomic size.

• The melting point of neon (Ne) is lower than that of helium (He), contrary to trends of increasing melting points with larger atomic radii in noble gases. This is due to super fluidity exhibited by Helium.

Identify the incorrect statement among the following:

• Oxygen (O2) demonstrates paramagnetism due to the presence of unpaired electrons, an unexpected behavior not observed in any other non-metallic diatomic molecules.

• Fluorine (F2) exhibits lower bond dissociation energy compared to other halogens, due to its small atomic size and high electronegativity.

• Xenon (Xe) forms fluorides like XeF2, an unexpected behavior as noble gases are traditionally considered inert and non-reactive.

Identify the incorrect statement among the following:

• The electron affinity of chlorine (Cl) is higher than that of fluorine (F), an anomaly due to fluorine's small size and electron repulsion.

• Silicon (Si) forms stronger Si-O bonds than Si-Si bonds, attributed to oxygen's higher electronegativity and smaller size.

• Fluorine's bond dissociation energy is anomalously higher than other group elements, expected due to its high electronegativity and bond strength in F2 molecules.

Identify the incorrect statement among the following:

• Nitrogen's ability to be stable in the atmosphere is unique among nonmetals, facilitated by the strong N≡N triple bond.

• The reactivity of oxygen towards organic compounds is more than sulfur's, contradicting the trend of increasing reactivity with heavier group 16 elements.

• Fluorine's reactivity towards organic compounds is mitigated by its high ionization energy, deviating from the expected high reactivity of halogens.

Identify the incorrect statement among the following:

• Thallium (Tl) exhibits a +1 oxidation state more frequently than +3, deviating from the expected group trend due to the inert pair effect.

• Lead (Pb) shows higher reactivity in water compared to tin (Sn), in line with the general increase in reactivity seen across the group.

• Aluminum (Al) reacts with water to release hydrogen gas, a reactivity trend that is consistent with the expected behavior of group 13 elements.

Identify the incorrect statement among the following:

• The relativistic effect significantly contracts the atomic radii of gold (Au), a phenomenon less pronounced in lighter p-block elements.

• Anomalous electron affinity values in the p-block are attributed to electron-electron repulsions in compact orbitals of period 2 elements.

• Boron's (B) unique ability to form stable covalent compounds, unlike its group counterparts, is due to its inability to form complete octets.

Identify the incorrect statement among the following:

• Carbon (C) exhibits an anomaly in its group by forming pi bonds due to p-orbital overlap, a property not seen in silicon (Si) to the same extent.

• The anomalous high melting point of diamond, an allotrope of carbon, is due to uniform bonding through sp3 hybrid orbitals forming covalent lattice, a property rarely seen in other elements.

• Nitrogen (N) shows a unique ability to form pπ-pπ multiple bonds with itself, an anomaly that only phosphorus (P) can replicate due to similar electron configurations.