As
you look over the representative-element structure
table (page 6) again, you can see the gradual diagonal change
in properties from lower left to upper right: bcp and then cp metals,
an intermediate zone of metallic and nonmetallic allotropes, and
finally the covalently bonded discrete molecules of nonmetals. As
the number of bonds formed between like atoms in Groups IVA, VA,
and VIA changes from four, to three, to two, the metallic allotrope
changes from packed atoms, to stacked layers or sheets, to helical
chains; and the nonmetallic allotrope changes from a three-dimensional
diamond lattice, to
tetrahedra, to rings of eight atoms. Only the smallest atoms can
form diatomic gases having multiple bonds, but singly bonded diatomic
molecules are the rule for the halogens, in Group VIIA.
As we have seen before, the melting point, or the temperature needed
to break a solid apart into fluid atoms or molecules, is a convenient
measure of the forces between these atoms or molecules. Melting
points for the representative elements are plotted on the three-dimensional
graph, with the periodic table as the base and temperature along
the vertical axis. Along the left edge, the alkali metals in Group
IA, having one electron per atom and an open bcp structure, are
soft and low-melting. The hardness of the metal and its melting
point increase in Group IIA, in which twice as many electrons are
available. Al, Ga, and In are lower melting because of the imperfections
and openness of their metal structures. Within one group, the heavier
metals are softer and lower melting because their atoms are farther
apart.