The absolute rate constants for the reactions of (CH3)(2)N radicals with NO and NO2 were determined in the gas phase and at room temperature by using the very low pressure reactor (VLPR) technique. The rates were k((CH3)2N+NO) = (8.53 +/- 1.42) X 10(-14) cm(3) molecule(-1) s(-1) and k((CH3)2N+NO2) = (9.08 +/- 1.36) X 10(-13) cm(3) molecule(-1) s(-1). The reaction with NO2 proceeds via two competitive pathways : the recombination pathway (CH3)(2)N + NO2 --> (CH3)(2)NNO2, with a rate constant k(2a) = (3.18 +/- 0.48) X 10(-13) cm(3) molecule(-1) s(-1), and the oxidation pathway (CH3)(2)N + NO2--> (CH3)(2)NONO* --> (CH3)(2)NO + NO, with a rate constant k(2b) = (6.36 +/- 0.74) x 10(-13) cm(3) molecule(-1) s(-1). The oxidation pathway is ca. 2.2 times faster than the recombination one, and the ratio k(2a)/k(2b) = 0.45 +/- 0.15. Conventional transition state theory analysis indicates that the involved transition states are loose, with the N...N or N...O bond lengths equal to ca. 2.5 Angstrom.