Regarding the resemblance of hydrogen with halogens, the incorrect statement is
It is a diatomic molecule
It forms hydrides with more electropositive metals
Hydride ion is stable with Helium configuration
It is a strong oxidizing agent like halogens

How would you account for the following ? (i)The lower oxidation state becomes more stable with increasing atomic number in Group 13. (ii)Hydrogen fluoride is much less volatile than hydrogen chloride. (iii)Interhalogen compounds are strong oxidising agents.

The elements of group 1 describe, more clearly than any other group of elements, the effects of increasing the size of atoms or ions on the physical and chemical properties.The chemical and physical properties the elements are closely related to their electronic structures and sizes.These metals are highly electropositive and thus form very strong bases, and have quite stable oxo-salts, In the manufacturing of sodium hydroxide chlorine and sodium carbonate, the sodium chloride is used as starting material. Which is not correctly matched ? (1)Basic strength of oxides , Cs_2OltRb_2OltK_2OltNa_2OltLi_2O (2)Stability of peroxides , Na_2O_2 lt K_2O_2 lt Rb_2O_2 lt Cs_2O_2 (3)Stability of bicarbonates , LiHCO_3 lt NaHCO_3 lt KHCO_3 lt RbHCO_3lt CsHCO_3 (4)Melting point , NaF < NaCl < NaBr < Nal

The elements of group 1 describe, more clearly then only group of elements, the effects of increasing the size of atoms or ions on the physical and chemical properties.The chemical and physical properties of the elements are closely related to their electronic structures and sizes.These metals are highly electropositive and thus form very strong bases, and have quite stable oxo-salts.In the manufacturing of sodium hydroxide, chlorine and sodium carbonate, the sodium chloride is used as starting material. Which of the following has the highest solubility in water ?

The small size and high charge of Al^(3+) ion gives it a high charge density which is responsible for its tendency to show (a) covalency in its compounds in the gaseous state (b) high hydration energy which stabilizes its compounds in solution, and (c) high lattice energy of its compounds in the solid state. Thus aluminium can forms both covalent and ionic bond. Like halides of boron, halides of aluminium do not show back bonding because of increase in size of aluminium. Actually aluminium atoms complete their octets by forming dimers. Thus chloride and bromide of aluminium exist as dimers, both in the vapour state and in polar-solvents like benzene while the corresponding boron halides exists as monomer. In boron trihalides the extent of back bonding decreases with increases with increase in size of halogens and thus lewis acid character increases. All BX_(3) are hydrolysed by water but BF_(3) shows a different behaviour. Which of the following reaction is incorrect ?

The small size and high charge of Al^(3+) ion gives it a high charge density which is responsible for its tendency to show (a) covalency in its compounds in the gaseous state (b) high hydration energy which stabilizes its compounds in solution, and (c) high lattice energy of its compounds in the solid state. Thus aluminium can forms both covalent and ionic bond. Like halides of boron, halides of aluminium do not show back bonding because of increase in size of aluminium. Actually aluminium atoms complete their octets by forming dimers. Thus chloride and bromide of aluminium exist as dimers, both in the vapour state and in polar-solvents like benzene while the corresponding boron halides exists as monomer. In boron trihalides the extent of back bonding decreases with increases with increase in size of halogens and thus lewis acid character increases. All BX_(3) are hydrolysed by water but BF_(3) shows a different behaviour. Which of the following statements about anhydrous aluminium chloride is correct ?