Boiling point (\u00b0C)<\/strong><\/td>\n-188<\/td>\n | -35<\/td>\n | 59<\/td>\n | 184<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n 2. General physical properties of Group 17 elements \n<\/strong> \n(a) Physical states and colours<\/strong> \nTable shows the physical states and colours of various halogens.<\/p>\n\n\n\nHalogen<\/strong><\/td>\nPhysical state and colour<\/strong><\/td>\n<\/tr>\n\nFluorine<\/td>\n | Pale yellow gas<\/td>\n<\/tr>\n | \nChlorine<\/td>\n | Greenish-yellow gas<\/td>\n<\/tr>\n | \nBromine<\/td>\n | Reddish-brown liquid<\/td>\n<\/tr>\n | \nIodine<\/td>\n | Purplish-black solid<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n The colours of the halogens become darker<\/strong> when going down Group 17. \n(b)\u00a0<\/strong>All halogens have low melting<\/strong> and boiling points.<\/strong> \nThis can be explained as below:<\/p>\n\n- The halogen molecules are held together by weak van der Waals forces of attraction.<\/strong><\/li>\n
- Hence, small amount of heat energy<\/strong> is needed to overcome it during melting or boiling.<\/li>\n<\/ul>\n
All halogens have low densities.<\/strong> \nAll halogens do not conduct electricity.<\/strong> \nAll halogens are weak conductors of heat.<\/strong><\/p>\n3. Trend of change in the physical properties<\/strong><\/p>\nHowever, some of the physical properties mentioned above vary gradually when going down Group 17, as shown in Table.<\/p>\n \n\n\nGroup 17 elements<\/strong><\/td>\nTrend of change in the physical properties<\/strong><\/td>\n<\/tr>\n\n<\/td>\n | The atomic radius (atomic size)<\/strong> of the halogens increases gradually<\/strong> down the group.<\/p>\n Reason:<\/strong> \nThe number of shells<\/strong> occupied with electrons increases<\/strong> down the group.<\/td>\nAlthough halogens have low melting and boiling points<\/strong>, the melting and boiling points increase<\/strong> down the group.<\/p>\n Reason:<\/strong> \nThe molecular size<\/strong> of the halogens increases<\/strong> down the group. \nHence, the forces of attraction between the halogen molecules become stronger<\/strong> down the group. \nConsequently, more heat energy<\/strong> is required to overcome the stronger forces of attraction during melting or boiling.<\/td>\nAlthough halogens have low densities,<\/strong> the density of the halogens increases gradually<\/strong> down the group.<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\nChemical properties\u00a0<\/strong>of Group 17 elements<\/strong><\/h3>\n1. Table shows the electron arrangements of halogens.<\/p>\n \n\n\nElement<\/strong><\/td>\nElectron arrangement<\/strong><\/td>\n<\/tr>\n\nFluorine<\/td>\n | 2.7<\/td>\n<\/tr>\n | \nChlorine<\/td>\n | 2.8.7<\/td>\n<\/tr>\n | \nBromine<\/td>\n | 2.8.18.7<\/td>\n<\/tr>\n | \nIodine<\/td>\n | 2.8.18.18.7<\/td>\n<\/tr>\n | \nAstatine<\/td>\n | 2.8.18.32.18.7<\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n 2. Similar chemical properties<\/strong><\/p>\n\n- All halogens exhibit similar<\/strong> chemical properties.<\/li>\n
- This is because all the atoms of halogens have 7 valence electrons.<\/strong><\/li>\n<\/ul>\n
3. Reactivity<\/strong><\/p>\n\n- Although halogens exhibit similar chemical properties, they differ in reactivity.<\/li>\n
- The reactivity<\/strong> of halogens decreases<\/strong> when going down Group 17.
\n<\/li>\n- The reactivity of a halogen is measured by how easily its atom accepts one electron<\/strong> to achieve a stable noble gas electron arrangement<\/strong> (octet electron arrangement).
\n<\/li>\n- The easier the atom of a halogen gains one electron, the more reactive is the halogen,<\/li>\n<\/ul>\n
Explanation:<\/strong> \nThe decrease<\/strong> in the reactivity down Group 17 can be explained as follows.<\/p>\n\n- All halogens have seven valence electrons.<\/strong><\/li>\n
- Each halogen atom will gain one electron<\/strong> to achieve a stable octet electron arrangement.<\/strong> Hence, an ion with a charge of -1 is formed.
\n<\/li>\n- When going down Group 17, the atomic size<\/strong> of halogens increases.<\/strong><\/li>\n
- The outermost occupied shell becomes further away<\/strong> from the nucleus and is screened by more inner shells<\/strong> containing electrons.
\n<\/li>\n- This means that the effective nuclear charge<\/strong> exerted on the outer valence shell decreases<\/strong> when going down the group.<\/li>\n
- Hence, the attractive forces<\/strong> exerted by the nucleus<\/strong> to attract one more electron<\/strong> into the valence shell decreases when going down the group.<\/li>\n
- This causes the reactivity<\/strong> of halogens to decrease<\/strong> down the group.<\/li>\n<\/ul>\n
4. As oxidising agents<\/strong><\/p>\n\n- Oxidising agents are good electron acceptors in chemical reactions.<\/li>\n
- Halogens are good oxidising agents<\/strong> because the atoms of each halogen can easily accept one electron<\/strong> to achieve a stable octet electron arrangement.<\/li>\n
- The strength<\/strong> of the halogens as oxidising agents decreases<\/strong> when going down Group 17.
\n \nThis is because the strength<\/strong> of the nucleus of a halogen atom to attract one more electron<\/strong> into the valence shell (outermost shell) decreases<\/strong> when going down the group.<\/li>\n<\/ul>\n5. Electronegativity<\/strong><\/p>\nHalogens are very electronegative. | | | | | | | | | | | |