Silver nanodots were used as probes 15 h after the chemical reduction of AZD3965 nmr the mixture. Results and discussion Upon the reduction

of silver ions with borohydride in the presence of single-stranded DNA molecules, a red emission species usually appears. It shifts gradually to the blue emission species, which is considered to be a multistep, intermediate-involved process. Reactive oxygen species expedite the spectral shift by quenching the red emission and facilitating the formation of the blue [22]. The peak shift depends on the concentration of oxidizing agents, which suggests that the remaining borohydride used as a reducing agent for silver nanodot preparation may weaken the oxidizing capacity of oxidants. The amount of borohydride was optimized to produce maximum blue emitters. The mixture of ssDNA and silver ions was reduced with a varied volume of aqueous sodium borohydride solution, followed by the addition of an oxidizing agent. An emission PLX-4720 molecular weight intensity check details at 340 nm excitation was recorded. The solution with 20 μL of sodium borohydride, corresponding to a Ag+/NaBH4 ratio of 6:5, yielded the maximum production of blue emitters, slightly lower than the regular NaBH4 dose (Figure 1). Too little sodium borohydride led to poor nanodot generation, whereas too much sodium borohydride weakened the oxidizing capacity of hydrogen peroxide.

Figure 1 The influence of sodium borohydride concentration on the formation of blue emitters. To a C24-Ag solution (50 μM, 1 mL), varied volumes of aqueous sodium borohydride solutions (1 mg/mL) pentoxifylline were added. The solutions were left overnight at room temperature to achieve stable red emissions, and then hydrogen peroxide was added with a final concentration of 5 mM. An emission intensity of 340 nm excitation was

recorded 5 h later. The numbers indicate the volume of aqueous sodium borohydride solution in microliters. The photoresponses of a 24mer polycytosine-protected silver nanodot (red emitter, λ em = 625 nm) upon the addition of sodium hypochlorite (NaOCl) are illustrated in Figure 2, in which the generation of the blue was much faster than the chemical bleaching of the red, with a pseudo-first-order rate constant of 2.5 × 10−1 s−1 (the blue) versus 2.1 × 10−4 s−1 (the red). As the concentration of hypochlorite was increased, the difference narrowed between the reaction rates of bleaching and the growth of the nanodots (Figure 2). It is possible that the minor part, but not the major part, of the oxidized species from the red emitter, such as silver ions, contributed to the creation of the blue emitter in this case. The higher the concentration of the hypochlorite, the greater the oxidation of the red emitter. Figure 2 Reaction kinetics between red silver nanodots and sodium hypochlorite. (a) Upon the addition of NaClO (50 μM), the red emission was quenched slowly (right), but the blue emission increased fast (left).