An excited ozone molecule, o3*, in the atmosphere can undergo one of the following reactions, o3* ? o3 (1) fluorescence o3* ? o + o2 (2) decomposition o3* + m ? o3 + m (3) deactivation, where m is an inert molecule, the rate constant for the fluorescence reaction is k1, the rate constant for the decomposition reaction is k2, and the rate constant for the deactivation reaction is k3. write a simplified expression for the fraction, x, of ozone molecules undergoing deactivation in terms of the rate constants. (use the following as necessary: k1, k2, k3, co for [o3*], and cm for [m].)

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vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

- lead + phosphoric acid = hydrogen + lead(ii) phosphate

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.