In the graph you can observe the trends of boiling points for various families of compounds. For the red, blue and green trends, devise an explanation for the significant decrease in boiling points from periods 2 to 3.
A)
B)
The intramolecular attractions between Hand the other element are much
stronger in period 3 as opposed to period 2.
The compounds from period 2 exhibit a very strong dipole force known as
hydrogen bonding whereas the compounds in period 3 exhibit weaker
dipole forces
The hydrogen bonding in period 2 is lighter in strength than the
compounds in period 3, respectively. These results in a tighter bond
requiring more thermal energy to break
The intermolecular forces between compounds in period 2 are stronger
than in period 3. This results in less thermal energy being required to break
the bonds in period 2 compounds.
D)

the answer is na (sodium)

answer : (a) volume of the gas = 8.67 ×   l

                (b) second virial coefficient b = -1.21226 l/mole

solution :   given,     t = 300k

                                p = 20atm

                                z = 0.86

                                n = 8.2 mmoles = 8.2 × moles

                                r =   0.082 l atm/k/mol

        find,     (a) volume of gas   and (b) second virial coefficient b at 300k.

formula used :            

                          and            

(a)            

                    = \times 0.082\times 300}{20}[/tex]

                    = 8.67 ×   l

(b)      

                    = (0.00867-1) × 8.659

                    = - 8.5839 l/mole