![](https://static.wixstatic.com/media/3486ea_ed23f246174046018af4c8c425c45562~mv2.png/v1/fill/w_54,h_23,al_c,q_85,usm_0.66_1.00_0.01,blur_2,enc_auto/3486ea_ed23f246174046018af4c8c425c45562~mv2.png)
(a) The charge distribution in the water molecule. (b) The water molecule in an electric field. (c) The electrostatic potential diagram of the water molecule.
![](https://static.wixstatic.com/media/3486ea_67d95a2678434c9db025fa974e867510~mv2.png/v1/fill/w_121,h_45,al_c,q_85,usm_0.66_1.00_0.01,blur_2,enc_auto/3486ea_67d95a2678434c9db025fa974e867510~mv2.png)
(a) The structure and charge distribution of the ammonia molecule. The polarity of the N-H bonds occurs because nitrogen has a greater electronegativity than hydrogen.
(b) The dipole moment of the ammonia molecule oriented in an electric field. (c) The electrostatic potential diagram for ammonia.
![](https://static.wixstatic.com/media/3486ea_edc317ccf9fa4eaf82b3ecfe844b2e97~mv2.png/v1/fill/w_62,h_22,al_c,q_85,usm_0.66_1.00_0.01,blur_2,enc_auto/3486ea_edc317ccf9fa4eaf82b3ecfe844b2e97~mv2.png)
(a) The carbon dioxide molecule. (b) The opposed bond polarities cancel out, and the carbon dioxide molecule has no dipole moment. (c) The electrostatic potential diagram for carbon dioxide.