Chemistry and Biology of Non-canonical Nucleic Acids. Naoki Sugimoto

Chemistry and Biology of Non-canonical Nucleic Acids

3.1 Potential hydrogen bonding sites in bases of the nucleosides. Hydrogen bonding donor sites are labeled with red arrows, and hydrogen bonding accepter sites are labeled with blue arrows.

Schematic illustration of the (a) Hydrogen bond formation in base pairs in a DNA duplex. The hydrogen bonds are shown in dashed lines. (b) Duplex structures of DNAs are depicted in tube and ball-and-stick models, respectively. Stacking interactions are shown in arrows.

Figure 3.2 (a) Hydrogen bond formation in base pairs in a DNA duplex. The hydrogen bonds are shown in dashed lines. (b) Duplex structures of DNAs are depicted in tube and ball-and-stick models, respectively. Stacking interactions are shown in arrows.

3.2.2 Stacking Interactions

The π–π stacking interactions refer to the interactions between aromatic rings containing π orbitals in bases of nucleic acids. The individual bases make strong stacking interactions with neighboring bases, which are major contributors to duplex stability (Figure 3.2b). The stacking interactions are much more prevalent in duplexes than in single strands. Base-stacking interactions are London dispersion force interactions and depend on the aromaticity of the bases and their dipole moments. The degree of stabilization afforded by base stacking depends on the DNA sequence. Nearest-neighbor base-stacking interactions are important determinants of duplex stability. The values of free energy change at 37 °C (−Δ upper G 37 Superscript ring ) due to stacking interactions during duplex formation are 0.4–1.6 kcal mol⁻¹ [3].

Moreover, the stacking interactions increase with increasing salt concentration, as high salt concentrations mask the destabilizing charge repulsion between the two negatively charged phosphodiester backbones. The DNA duplex stability increases with increasing salt concentration.

3.2.3 Conformational Entropy

The conformations of nucleotides depend on the torsion angles for rotation around each bonding shown in Figure 3.3. There are seven torsion angles (α, β, γ, δ, ε, ζ, χ) per nucleotide that must be specified to characterize the conformation of ordered structures for the nucleic acids. The duplex formation is favorable for enthalpy. However, the loss of conformational entropy is induced by reduction of degrees of freedom for nucleotides.

Schematic illustration of the torsion angles in a polyribonucleotide chain.

Figure 3.3 Torsion angles in a polyribonucleotide chain.

3.3 Thermodynamic Analysis for the Formation of Duplex

In the case of canonical duplex structures, the base stacking decreases the transition dipole moment of bases, which makes UV absorbance at 260 nm of duplex smaller than that of single-stranded state. Heating of nucleic acids causes the strands to be denatured by disrupting the ordered stacking of the bases and breaking hydrogen bonds. The process can be conveniently monitored by an increase in UV absorbance as the duplex unwinds to single strands owing to hyperchromicity.

The example in Figure 3.4a shows a melting curve (UV absorption as a function of temperature). Slow heating of duplex causes the unwinding of the ordered helical structure into the two single-stranded constituents. The unwinding can be seen as a sigmoidal curve of increasing UV absorption. The midpoint corresponding to the precise melting temperature (T_m) of the duplex is indicated.

Methods to obtain the thermodynamic parameters of enthalpy (ΔH^°), entropy (ΔS^°), and free energy changes at 25 °C (Δ upper G 25 Superscript ring ) for the formation of a nucleic acid structure are described below; DNA duplex formation is taken as an example. Data are typically analyzed with a two-state model, which assumes that each strand is either completely paired or unpaired. The equilibrium for the duplex formation is represented as either a self-complementary or non-self-complementary association as follows [4]:

(3.1) 2 upper A right-arrow over left-arrow normal upper A 2

(3.2) normal upper B plus normal upper C left-arrow over right-arrow normal upper B dot normal upper C

where A, B, and C indicate the single strands of DNA and A₂ and B·C indicate the double-stranded DNA.

Graphs depict the UV melting curves of the self-complementary duplex at 5 μM strand concentration with (a) Tm value and (b) upper and lower baselines. Upper and lower baselines can be represented as Eds = mdsT + bds and Ess = mssT + bss, respectively, where Eds and Ess indicate the absorbance for the double-stranded and single-stranded DNA, respectively. The mds and bds or mss and bss represent the slope and intercept of the upper baseline or lower baseline for the UV melting curve, respectively.

Figure 3.4 UV melting curves of the self-complementary duplex (5′-ATGCGCAT-3′) at 5 μM strand concentration with (a) T_m value and (b) upper and lower baselines. Upper and lower baselines can be represented as ε_ds = m_dsT + b_ds and ε_ss = m_ssT + b_ss, respectively, where ε_ds and ε_ss indicate the absorbance for the double-stranded and single-stranded DNA, respectively. The m_ds and b_ds or m_ss and b_ss represent the slope and intercept of the upper baseline or lower baseline for the UV melting curve, respectively.

The equilibrium for an intramolecular transition, for example, a hairpin, is represented as

(3.3) normal upper D Subscript s s Baseline right-arrow over left-arrow normal upper D Subscript normal f

where D_ss and D_f indicate the single-stranded (unfolded) and folded DNA structures, respectively.

For self-complementary (Eq. 3.1) or non-self-complementary equilibria (Eq. 3.2) with equal concentrations of B and C, the observed equilibrium constant K_obs is given by

(3.4) upper K Subscript o b s Baseline equals left-parenthesis alpha slash 2 right-parenthesis slash left-parenthesis upper C Subscript normal t Baseline slash s right-parenthesis left-parenthesis 1 minus alpha right-parenthesis squared

where C_t is the total strand concentration,

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