We
report reactions of gas-phase free silver cluster cations, Ag
n
+ (n = 3–18),
with nitric oxide molecules, which was studied by kinetics measurements
using an ion trap. Ag
n
O(NO2)
m−1
+ and Ag
n
(NO2)
m
+ were observed as major products after multiple reactions.
The reaction pathway to form these product ions was identified by
fitting the data to rate equations for n ≤
15, except for inert n = 3 and 5. Two different reaction
mechanisms were found for the formation of these products depending
on cluster size; pseudo-first-order rate constants of each step of
elementary reactions were obtained. First, as found for n = 4, 6, and 9, Ag
n
O+ is formed
by a reaction with two NO molecules, which is followed by a release
of neutral N2O. A further reaction of Ag
n
O+ with another NO molecule produces Ag
n
NO2
+. Ag
n
(NO2)
m
+ (m ≥ 1) is thus successively formed via an intermediate,
Ag
n
O(NO2)
m−1
+. This is analogous to the reaction of
NO on silver surfaces to produce NO2. Second, both Ag
n
NO2
+ and Ag
n
O+ are formed concurrently, as found for n = 7, 8, 10, 11, 12, and 15; Ag
n
O+ does not act as an intermediate for Ag
n
NO2
+. Ag
n
O(NO2)
m−1
+ and Ag
n
(NO2)
m
+ (m ≥ 2) are
formed by successive addition of NO2 to Ag
n
O+ and Ag
n
NO2
+, respectively. It is speculated that the
successive addition of NO2 proceeds via disproportionation,
i.e., three NO molecules are converted to NO2 and N2O. The reaction pathways of n = 13 and 14
are explained equally well by the two mechanisms. The overall reaction
rate coefficients exhibit an odd–even alternation; the higher
reactivity for even values of n is due to an odd
number of valence electrons.