Chemistry Group 15 Quiz

Electronegativity generally decreases down Group 15.

Phosphorus has an electronegativity of 2.1 eV (electron volts).

Melting and boiling points generally increase down Group 15.

Nitrogen exhibits unique properties compared to other elements in Group 15 due to its small size and high electronegativity.

Nitrogen exists as a gas at room temperature.

Group 15 elements react with hydrogen to form hydrides of the type EH₃.

Ammonia forms hydrogen bonds due to nitrogen's high electronegativity.

NH₃ has a higher boiling point than PH₃ because of stronger hydrogen bonding in NH₃.

PH3 reacts with HCl to form phosphonium chloride (PH4Cl).

PH3 reacts with water to form phosphonium hydroxide (PH4OH).

PH3 reacts with nitric acid (HNO3) to form phosphonium nitrate (PH4NO3).

Phosphorus (P4) reacts with chlorine (Cl2) to produce phosphorus trichloride (PCl3).

Phosphorus (P4) and thionyl chloride (SOCl2) react to form phosphorus trichloride (PCl3), sulfur dioxide (SO2), and disulfur dichloride (S2Cl2).

PCl3 reacts with water to form phosphorous acid (H3PO3) and hydrochloric acid (HCl).

PCl3 reacts with oxygen to produce phosphorus oxychloride (POCl3).

Phosphorus (P4) reacts with excess chlorine (Cl2) to produce phosphorus pentachloride (PCl5).

PCl5 reacts with water to form phosphoric acid (H3PO4) and hydrochloric acid (HCl).

PCl5 reacts with sulfur dioxide (SO2) to form thionyl chloride (SOCl2) and phosphorus oxychloride (POCl3).

Heating PCl5 results in the formation of PCl3 and chlorine gas (Cl2).

Elements in Group 16 of the periodic table are called the oxygen family.

Burning sulphur in air or reacting FeS2 with oxygen produces sulphur dioxide.

Colorless gas with a pungent smell, soluble in water, boiling point 263K.

SO2 reacts with water to form sulphurous acid (H2SO3).

SO2 reacts with oxygen to form sulphur trioxide (SO3).

SO2 reacts with chlorine to produce Sulphoryl Chloride (SO2Cl2).

A process for manufacturing sulphuric acid, involving reactions of sulphur, oxygen, and V2O5.

Colorless oily liquid, freezing point 283K, boiling point 611K, specific gravity 1.83.

Copper reacts with H2SO4 to form copper sulphate and hydrogen gas.

Zinc reacts with H2SO4 to form zinc sulphate and hydrogen gas.

Elements of Group 17 in the periodic table.

Nitric acid (HNO3) reacts with carbon (C) to produce carbon dioxide (CO2), water (H2O), and nitrogen dioxide (NO2).

Nitric acid (HNO3) reacts with sulfur (S) to form sulphuric acid (H2SO4), nitrogen dioxide (NO2), and water (H2O).

Nitric acid (HNO3) reacts with phosphorous (P) to form phosphoric acid (H3PO4), nitrogen dioxide (NO2), and water (H2O).

Nitric acid (HNO3) reacts with iodine (I2) to form iodic acid (HIO3), nitrogen dioxide (NO2), and water (H2O).

Zinc (Zn) reacts with dilute nitric acid (HNO3) to produce zinc nitrate (Zn(NO3)2), water (H2O), and nitrous oxide (N2O).

Copper (Cu) reacts with dilute nitric acid (HNO3) to produce copper nitrate (Cu(NO3)2), water (H2O), and nitrogen monoxide (NO).

Copper (Cu) reacts with concentrated nitric acid (HNO3) to produce copper nitrate (Cu(NO3)2,) nitrogen dioxide (NO2), and water (H2O).

Zinc (Zn) reacts with concentrated nitric acid (HNO3) to produce zinc nitrate (Zn(NO3)2), nitrogen dioxide (NO2), and water (H2O).

A highly reactive, waxy solid form of phosphorus, found as P4, soluble in carbon disulfide.

A less reactive form of phosphorus, obtained by heating white phosphorus, insoluble in water.

A form of phosphorus created by high-pressure heating of red phosphorus.

A weak acid with the formula H3PO2. It mainly contains P-H bonds.

A weak acid with the formula H3PO3. It has P-H bonds.

A weak polyprotic acid with the formula H3PO4. It contains P-OH bonds.

A cyclic polymer of phosphoric acid with the formula (HPO3)3. Contains multiple P atoms in a ring.

Phosphorous reacts with sodium hydroxide and water to produce phosphine (PH3).

A colorless, poisonous gas that is soluble in water, with a rotten fish odour.

Phosphorus reacts with halogens like chlorine, fluorine, bromine, to form phosphorus trihalides (PX3) and phosphorus pentahalides (PX5).

Halogens react with water to produce hydrogen halide and oxygen.

Halogens react with metals to form metal halides.

Interhalogen compounds are formed when halogens of different sizes combine.

Group 18 elements are also known as noble gases or inert gases.

Group 18 elements have a full outer electron shell (ns²np⁶).

Generally, the oxidation state of group 18 elements is zero.

Examples of group 18 elements include helium, neon, argon, krypton, xenon, and radon.

Group 18 elements are all gases at room temperature.

The most common oxidation state of Group 17 elements is +7 and -1.

The general electronic configuration of Group 17 elements is ns²np⁵.

Fluorine (F) is a gas at room temperature.

Chlorine (Cl) is a liquid at room temperature.

Bromine (Br) is a liquid at room temperature.

Iodine (I) is a solid at room temperature.

Halogen reactivity decreases down the group.

Atomic size generally increases down the group in Group 17.

Ionization energy generally decreases down the group in Group 17.

Metallic character decreases down the group in Group 17.

Electronegativity generally decreases down the group in Group 17.

Halogens react with hydrogen to form hydrogen halides.

HI is a stronger acid than HF due to bond strength differences.

Reactivity of halogens decreases as you go down the group.