Question

What correlation, if any, exists for the Period 2 elements between group number and the number of covalent bonds the element typically forms? How is the correlation different for elements in Periods 3 to 6?

Answer 1

The number of valence electrons shared by elements in a group is constant. The number of occupied electron shells is the same for elements in the same period.

How is the correlation different for elements in Periods 3 to 6?

Triple bonds are stronger than double bonds because it takes more energy to totally break all three of them than to entirely break only two. They are shorter between like atoms than double bonds.

Similar to single bonds, double bonds between similar atoms are more powerful and compact. However, bonds of the same order between several atoms exhibit a wide range of bond energies.

• As we move down the periodic table, the strength of bonds between hydrogen and atoms in the same column decreases. Thus, an H-F bond is more powerful than an H-I bond, H-C is more powerful than H-Si, H-N is more powerful than H-P, and H-O is more powerful than H-S.
• As one of the atoms gets bigger, the area of space where electrons are shared by two atoms is correspondingly smaller.
• As we descend a column, bonds between like atoms typically weaken (important exceptions are noted later). The single bond C-C is stronger than the single bond Si-Si, which is stronger than the single bond Ge-Ge, and so on. As two bonded atoms get bigger, the space between them filled by bonding electrons grows proportionately smaller.
• Single bonds between the period 2 atoms of groups 15, 16, and 17 (i.e., N, O, and F) are notable exceptions because they are unusually weak in comparison to single bonds between their larger congeners.
• Due to potent repulsive interactions between lone pairs of electrons on nearby atoms, it is possible that the N-N, O-O, and F-F single bonds are weaker than could be anticipated. As a result, the halogens' bond energies are on the rise.

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