7.2 Covalent Bonding
Electron sharing between atoms, electronegativity differences, and where a bond falls on the scale from pure covalent to polar to ionic.
6 exercises
7.2 Exercise 1
Why is it incorrect to speak of a molecule of solid NaCl?
7.2 Exercise 3
Predict which of the following compounds are ionic and which are covalent, based on the location of their constituent atoms in the periodic table:
(a) Cl2CO
(b) MnO
(c) NCl3
(d) CoBr2
(e) K2S
(f) CO
(g) CaF2
(h) HI
(i) CaO
(j) IBr
(k) CO2
7.2 Exercise 5
From its position in the periodic table, determine which atom in each pair is more electronegative:
(a) Br or Cl
(b) N or O
(c) S or O
(d) P or S
(e) Si or N
(f) Ba or P
(g) N or K
7.2 Exercise 7
From their positions in the periodic table, arrange the atoms in each of the following series in order of increasing electronegativity:
(a) C, F, H, N, O
(b) Br, Cl, F, H, I
(c) F, H, O, P, S
(d) Al, H, Na, O, P
(e) Ba, H, N, O, As
7.2 Exercise 9
Which atoms can bond to sulfur so as to produce a positive partial charge on the sulfur atom?
7.2 Exercise 11
Identify the more polar bond in each of the following pairs of bonds:
(a) HF or HCl
(b) NO or CO
(c) SH or OH
(d) PCl or SCl
(e) CH or NH
(f) SO or PO
(g) CN or NN
Adapted from General Chemistry © 2019 Rice University. Licensed under CC BY 4.0. Sources: Chemistry 2e, Chemistry: Atoms First 2e. Imported at revision 32c7196.