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Cesium-adsorption mechanisms of woody charcoal discussed on the basis of its functional groups and nanostructure


The present study examined the Cs+-adsorption behavior of Japanese oak (Quercus serrata Thunb.) charcoal (OC) samples carbonized at 300, 500, and 700 °C to clarify the adsorption mechanisms from aqueous solution. Adsorption isotherms indicated that the Cs+-adsorption ability of OC depended strongly on carbonization temperature (CT) and suggested that the ability reached a maximum within the CT range from 300 to 700 °C. Infrared-photoacoustic (IR-PA) and Raman spectra of OC samples were obtained to investigate the functional groups and nanostructure in OC. Raman signals exhibited graphite precursor production even in OC synthesized at 300 °C. IR-PA spectral bands provided positive evidence that OC carbonized at 300 or 500 °C contained sufficient OH groups, and some of which were free from hydrogen bonding. Detecting free OH groups was the most important outcome in this study as it allowed exploration of the OC nanostructure. The experimental data indicated that the primary attraction to Cs+ is due to the surface OH groups in OC, therefore offering an approach to synthesizing woody charcoal with a high Cs+-adsorption performance.


The nuclear power plant accident caused by the Great East Japan Earthquake (2011) has raised several important and serious issues and led to many countries considering shutting down of their nuclear power plants. It is, however, unlikely that all power plant systems on Earth employing uranium nuclear fission will be brought to a standstill in the near future. Thus, it is essential to take rapid and appropriate measures to prevent nuclear pollutants from spreading, although the effective safeguard against the leakage of radioactive substances from nuclear power reactors is the top priority. Cs-134 and Cs-137 are the most troublesome radioisotopes with respect to decontamination and have been the most difficult to remove from contaminated areas in Fukushima Prefecture. This situation would recur as a result of future nuclear power plant accident; hence, high-performance and economical adsorptive materials for Cs+ are urgently required.

Many researchers have studied Cs+ adsorption by inorganic substances, such as synthesized zeolites and Prussian-blue-type complexes. In contrast, only a few studies have reported char made from plant biomass as a Cs+ adsorptive [1,2,3,4] other than ours [5,6,7,8,9,10] despite 8 years passing from the Fukushima accident, because the Cs+-adsorption ability of ordinary biochar is inferior to that of inorganic adsorptives. However, woody charcoal is inexpensive and can be mass-produced easily, and its remarkable advantage is considerable volume reduction by combustion.

We have previously investigated the Cs+-adsorption behavior of commercial charcoals used in Japan from aqueous solutions. These studies suggested that the content of acidic functional groups, such as hydroxy (OH) or carboxy groups, included in the charcoal is a governing factor determining the ability to adsorb Cs+ from aqueous solution [10]. The functional groups and nanostructures in woody charcoal were partially elucidated [11, 12], but the structure has not been completely determined because of their complicated nature.

Our objective is to examine the mechanisms involved in Cs+ adsorption from aqueous solution onto charcoal surfaces in terms of surface functional groups and nanostructure in more detail. In this paper, Japanese oak (Quercus serrata Thunb.) charcoal (OC) samples were characterized using infrared-photoacoustic (IR-PA) and Raman spectroscopy.

Infrared (IR) spectroscopy is a helpful tool for identifying functional groups in wood. Although ordinary IR techniques do not always provide a fine spectrum for black or dark samples such as charcoal and degraded wood due to non-resonant absorption, IR-PA technique is suitable for obtaining the IR spectra of such samples. For example, this technique was used to such samples, revealing that it is a useful method for determining chemical changes in functional groups [12,13,14]. It is well known that Raman signals provide information about sp2 bonding in carbon materials. We discuss the nature of the chemical attraction between Cs+ and charcoal surfaces based on the spectroscopic characterization.



Special-grade cesium chloride anhydride and microcrystalline cellulose powder were obtained commercially from FUJIFILM Wako Pure Chemical Co.

Carbonization of Japanese oak wood and cellulose

Japanese oak trees growing wild in Akita Prefecture in Japan were cut down, and their stems were cut into round slices with a thickness of 5 cm. The slices were dried indoors at ambient temperature for over 3 months. After removing bark and heartwood, the sapwood blocks were ground into powder using a cutting mill. The Japanese oak sapwood and cellulose powders were carbonized under a N2 flow (150 mL/min) in a quartz tube kiln (Isuzu Seisakusho Ltd., Japan). The furnace temperature was programmed to increase from room temperature to 105 °C at 10 °C/min, remain at 105 °C for 1 h, to subsequently increase to 300, 500, or 700 °C at 10 °C/min, and finally remain at the desired temperatures (carbonization temperature, CT) to yield charcoal. Japanese oak charcoal (OC) samples synthesized at 300, 500, and 700 °C are denoted OC300, OC500, and OC700, respectively. In the same way, cellulose charcoal (CC) samples synthesized at 300, 500, and 700 °C are similarly denoted CC300, CC500, and CC700, respectively. Moreover, the holding time (HT) at the CT is appended to the sample name; for example, OC carbonized at 500 °C for 2.0 h is referred to as OC500-2. OC powder (40–80 mesh) was used as an adsorbent for Cs+. The OC and CC samples were stored in a capped glass tube in air.

Aqueous CsCl solution

After drying at 100 °C for 1 day, CsCl powder was weighed and dissolved in water. The solution was prepared using water deionized through a column packed with ion-exchange resins. The initial concentration was 2.50 × 10−5 mol/L (Cs+ 3.32 mg/L).

Raman spectra of OC and CC

Raman spectra were obtained using a Raman spectrometer (inVia Raman Microscope, Renishaw PLC, UK) with 532-nm laser excitation (1.5–15 mW). Back-scattered Raman signals were collected through a microscope (100× objective lens) with a spectral resolution of approximately 3 cm−1, and the exposure time was 50 s. The sample powder was thinly and evenly spread on a glass plate. Wavenumber calibration was carried out using the 520 cm−1 line for a silicon wafer and the 1332 cm−1 line for diamond.

IR-PA spectra of OC and CC

IR-PA spectra were recorded using a JIR7000W spectrometer (JEOL Ltd., Japan) coupled with an IR-PA spectroscopy module (IR-PAS 1000). The spectra were obtained from 300 accumulations with a spectral resolution of ca. 4 cm−1. A thin cell made of Al (diameter 5 mm) was filled with the sample powder. OC and CC samples were exposed to air for several days and measured without drying. Photoacoustic signals were collected upon purging a cell bench with He gas. The moving-mirror velocity was set to 1.6 mm/s for all measurements. Carbon black was used as a reference. Wavenumber calibration was carried out based on the 1028, 1601, and 3060 cm−1 lines for polystyrene. The original band intensities were not altered mathematically, although baseline corrections were conducted as required.

Cs+ adsorption from aqueous CsCl solution to OC powder

The OC samples were dried at 105 °C for 3 h before mass measurements. Aqueous CsCl solution (50 mL) containing OC adsorbent (0.10, 0.20, 0.40, 0.80, or 1.60 g) in a capped Erlenmeyer flask was shaken using an orbital shaker at 23 ± 2 °C for 24 h and then removed by filtration through a nylon-membrane microfilter (Millex-HN filters, SLHN033NS, Millipore Ireland, Ltd., Ireland). The pH of the filtrate was measured with a pH meter. The Cs+ concentration in the filtrate was determined using an inductively coupled plasma mass spectrometry (ICP-MS) (Agilent 7700x, Agilent Technologies, Ltd., US) with an internal standard method (standard isotope 115In). The ICP-MS measurements were repeated three times for each sample solution. Relative standard deviations were all within 3.0%. The process of calculating the Cs+ concentration on the charcoal was described previously [6,7,8, 10].

Results and discussion

Mass reduction of OC by carbonization

Table 1 summarizes the mass reduction rates for the OC samples. The OC300 required over 1.0 h of HT until its weight was constant. The mass reduction of OC500 was likely to be nearly completed within 1.0 h, and the mass of OC700 became essentially constant before 0.5 h. Thus, the changes in mass reduction given in Table 1 suggest that the pyrolysis of Japanese oak sapwood progressed adequately within 2.0 h of HT in the carbonizing device, even at a CT of 300 °C.

Table 1 OC mass reduction rate

Cs+-adsorption isotherms from aqueous solution onto OC

Figure 1 depicts the adsorption isotherms of OC300-2, OC500-2, and OC700-2. The isotherms indicate that the Cs+-adsorption ability of OC follows the order: OC700-2 < OC300-2 < OC500-2. Therefore, it is likely that the adsorption ability increases with CT from 300 °C up to a certain optimum temperature and then decreases to at least 700 °C. The change in Cs+-adsorption ability with CT can be expected to provide insights into the functional groups and nanostructures of OC, although the optimum temperature may fluctuate with carbonization conditions. The results shown in Fig. 1 are not incompatible with the previous work on the Cs+-adsorption ability of commercial charcoals [10].

Fig. 1

Isotherms of Cs+-adsorption from aqueous CsCl solution onto OC300-2 (filled triangles), OC500-2 (filled squares), and OC700-2 (filled circles)

Raman spectra of OC and CC

Figure 2 shows Raman spectra of OC and CC from 1800 to 1000 cm−1. OC and CC samples carbonized at the same CT showed no remarkable changes in the Raman spectral shape with increasing HT when HT was longer than 1.0 h.

Fig. 2

Raman spectra in the 1800–1000 cm−1 region for a OC300-2 (red solid line), b CC300-2 (blue solid line), c OC500-2 (red solid line), d CC500-2 (blue solid line), e OC700-2 (red solid line), and f CC700-2 (blue solid line)

All the OC samples exhibit clear broad D and G bands, characteristic of graphite-like structures. The peak position of G band is nearly independent of CT, whereas that of D band clearly shifts to lower wavenumber with the increase in CT. The widths of the D and G bands for OC700-2 appear narrower than those for OC300-2 and OC500-2. These spectral changes are in good agreement with Raman data for Japanese cedar charcoal reported previously [15, 16].

The D- and G-band shapes for CC500-2 and CC700-2 are very similar to those for OC500-2 and OC700-2, respectively. The Raman scattering intensity for CC300-2 is extremely weak, and the D band is not easily detectable, although the G band appears similar to that for OC300-2. The Raman spectral differences between OC300-2 and CC300-2 suggest that an uncarbonized portion of CC300-2 was large compared with that of OC300-2. In other words, it seems likely that all of carbonization reactions of hemicellulose and/or lignin were almost completed even below 300 °C [17, 18]. The narrowing of the D and G bands suggests that the stereoregularity of graphite precursors produced by carbonization is enhanced with increasing CT.

IR-PA spectra of OC and CC

The IR-PA spectra also showed no remarkable changes in shape with increasing HT when HT was above 1.0 h. Figure 3 shows IR-PA spectra in the 4000–2500 cm−1 range for OC300-2, OC500-2, OC700-2, and raw Japanese oak sapwood.

Fig. 3

IR-PA spectra in the 4000–2500 cm−1 region for a raw Japanese oak sapwood (green solid line), b OC300-2 (red solid line), c OC500-2 (brown solid line), and d OC700-2 (black solid line). All spectra are displayed with the same vertical axis scale

As shown in Fig. 3a, a band assigned to C–H stretching vibrational modes of CH3–, –CH2–, and > CH– groups appears around 2900 cm−1. It was difficult to quantitatively evaluate the band intensities in the IR-PA spectra because of no appropriate internal standard band. However, it can be reasonably assumed that the band around 2900 cm−1 becomes weaker as CT increases and disappears at 700 °C, since all the spectra shown in Fig. 3 are displayed at the same vertical scale and their band intensities are not altered mathematically. Furthermore, a new band at about 3050 cm−1 appears at 500 °C, which is attributed to sp2 C–H stretching vibrations [13, 19].

A strong and extremely broad peak assigned to O–H stretching vibrations appears between 3700 and 3100 cm−1 in the raw wood spectrum, and this broadening is caused by hydrogen bonding. This band also diminishes with increasing CT and is undetectable at 700 °C. Additionally, it seems that the peak top of this band shifts to higher wavenumber with the increase in CT. In general, the stronger the hydrogen bonding is, the lower the wavenumber of the O–H stretching vibrational mode becomes. Therefore, this shift suggests that the effects of hydrogen bonding on OH groups are comprehensively weakened with increasing CT.

It is interesting to note that a band at about 3650 cm−1 is clearly detected in the O–H stretching vibration region (Fig. 3b, c). The band appears as a shoulder in the OC300-2 spectrum and a well-resolved peak in the OC500-2 spectrum. It is attributed to O–H stretching vibrations of alcoholic and/or phenolic OH groups free from hydrogen bonding [20]. Few reports are available on detecting free OH groups in the solid state by IR or Raman spectroscopy without deconvolution processing. The direct detection of free OH groups is the most important outcome in this study and provides useful information on the OC nanostructures.

Figure 4 illustrates a simplified model of the nanostructures in OC300 and OC500. As shown in Fig. 4a, raw Japanese oak wood contains numerous OH groups. Almost all the OH groups form hydrogen bonds with neighboring functional groups having O atoms or water molecules. Water evaporation and pyrolysis of wood constituents occur with heating. Hence, pyrolysis leads to a decrease in the amount of OH groups and causes non-uniform contraction of wood cell walls. Consequently, many pores with free OH groups on their surfaces are formed in OC300-2 and OC500-2, as illustrated in Fig. 4b and/or c. The pores may be more appropriately called crevices or crevasses on the molecular level, since no activation treatments were applied to any of the OC samples. It is known that water is generated by pyrolysis of wood components [18, 21]. The water molecules may be trapped in the pores and form hydrogen bonds with surface OH groups. If external water molecules can move into a pore, OH groups will form hydrogen bonds with them, as shown in the left side of Fig. 4c’. Otherwise, the OH groups will remain free from hydrogen bonds, as shown in Fig. 4b’ and the right side of Fig. 4c’, even when the OC samples are kept in air for a long time.

Fig. 4

Schematic of changes in OC300 or OC500 nanostructures. a raw Japanese oak wood, b, c freshly synthesized OC300 or OC500, and b’ and c’ OC300 or OC500 kept in air for a long period after synthesis. Small blue filled circles: OH groups in bulk of solid, small blue open circles: free OH groups on surface, small red open circles: hydrogen-bonded OH groups on surface, large light-blue filled circles: water molecules moved from outside, and large purple filled circles: water molecules produced by pyrolysis of wood constituents

Figure 5 depicts the 2000–800 cm−1 region of the IR-PA spectra shown in Fig. 3. As shown in the bottom spectrum, OC700-2 also exhibits no IR bands in this region, suggesting that organic functional groups derived from raw wood are completely thermally decomposed up to 700 °C as with Japanese cedar charcoal [13].

Fig. 5

IR-PA spectra in the 2000–800 cm−1 region for a raw Japanese oak sapwood (green solid line), b OC300-2 (red solid line), c OC500-2 (brown solid line), and d OC700-2 (black solid line). All spectra are displayed with the same vertical axis scale

The spectral changes with CT in the range of 1800–1550 cm−1 are remarkably interesting and contain potential information about the OC nanostructures. The IR bands appearing at 1740 and 1652 cm−1 in the IR spectrum of raw wood (Fig. 5a) are assigned to C=O in carboxy group, and ethylenic C=C in coniferyl alcohol and/or C=O in coniferyl aldehyde, respectively [22]. The band at 1594 cm−1 is attributed to aromatic six-membered rings.

As seen in Fig. 5b, OC300-2 exhibits no peaks at 1740 and 1652 cm−1; however, a broad new band appears at 1710 cm−1. A band near 1594 cm−1 is also observed, but this is broader than that in Fig. 5a. The resolution among IR bands in the OC300-2 spectrum is poor, although bands at about 1459, 1424, 1370, and 1157 cm−1 are observable as peaks or shoulders. Peaks at about 1710 and 1594 cm−1 are clearly detected in the OC500-2 spectrum (Fig. 5c), but other bands in the 1500–1100 cm−1 region are indistinguishable from one another despite their strong intensities. The bands at 1710 and 1594 cm−1 (Fig. 5b, c) indicate that OC300-2 and OC500-2 contain C=O groups and aromatic six-membered rings [12]. It is, however, anticipated from the relative intensity and width of the bands that the C=O groups and aromatic rings were not derived from the raw wood, but were formed during the carbonization process.

Figure 6 shows IR-PA spectra of OC and CC samples from 4000 to 800 cm−1. As cellulose is a major constituent of wood, the overall spectral shape for cellulose (Fig. 6b) is similar to that of Japanese oak wood (Fig. 6a). However, the spectral shape between 1800 and 1550 cm−1 is quite different from that of Japanese oak wood because of the absence of C=O and phenyl groups. In contrast, as shown in Fig. 6d, f, CC300-2 and CC500-2 exhibit strong broad bands at about 1710 and 1594 cm−1, similar to those for OC300-2 and OC500-2. As was referred to Fig. 5, the IR-PA spectra of CC provide strong evidence that the two bands are not due to residual functional groups derived from raw wood, but are instead mainly due to functional groups formed by heat treatment. The bands at 1710 and 1594 cm−1 observed for OC300-2, CC300-2, OC500-2, and CC500-2 are attributed to C=O groups and aromatic rings, respectively, and the latter band suggests that precursors of graphite were formed in the charcoal samples. This is supported by the appearance of a band at 3050 cm−1 due to C–H bonds of sp2 C in the CC500-2 spectrum, as is similar to OC500-2 spectrum shown in Fig. 3.

Fig. 6

IR-PA spectra in the 4000–800 cm−1 region for a raw Japanese oak sapwood, b cellulose powder, c OC300-2, d CC300-2, e OC500-2, and f CC500-2. Light green belt: wavenumber region from 1800 to 1700 cm−1. All spectra are displayed with the same vertical axis scale

These IR-PA results are consistent with the Raman spectra shown in Fig. 2. Moreover, the shape of the broad band (3700–3100 cm−1) for the CC samples is very similar to that of the corresponding OC samples; CC300-2 and CC500-2 also exhibit a shoulder and a peak at about 3650 cm−1, respectively. Hence, it can be assumed that similar nanostructural changes illustrated in Fig. 4 occurred in the CC samples.

Mechanisms for Cs+ adsorption onto OC from aqueous solution

We describe here comprehensive mechanisms for Cs+ adsorption onto OC samples. The IR-PA spectra of OC samples showed that the functional groups derived from raw Japanese oak wood decreased with increasing CT and were thoroughly decomposed up to 700 °C. Furthermore, the spectra indicated that almost all the carboxy groups were decomposed up to 300 °C. In contrast, it was evident from the IR-PA spectra of OC500-2 that a considerable portion of the OH groups remained even at 500 °C, although their amount decreased with the increase in CT. Thus, it can be assumed that the OH groups are the primary acidic functional groups in OC300 and OC500.

It has been expected that acidic functional groups would play an important role in the capture of Cs+ by commercial woody charcoals [9, 10]. By releasing a proton (H+), acidic functional groups can obtain a negative charge in aqueous solution. Since Cs+ is a cation, it is electrostatically attracted to negatively charged functional groups.

Based on the investigation into IR-PA spectra of OC, we reach the conclusion that almost all the acidic functional groups in OC300 and OC500 are OH groups. As described above, the Cs+-adsorption ability followed the order OC700 < OC300 < OC500, inferring that the ability reaches a maximum at a certain CT, CTM, (300 °C < CTM < 700 °C) and then decreases with a further increase in CT. Accordingly, the dependence of the Cs+-adsorption ability on CT cannot be explained only by changes in the total amount of OH groups per unit weight in OC samples. On the other hand, it is inferred from other studies [23,24,25] that the specific area of charcoal determined by N2-adsorption increases monotonously with increasing CT up to 600 °C when no activation processes are applied to the charcoal.

Consequently, the nanostructure and acidic functional groups presumably change as illustrated in Fig. 7. The specific area of OC300 is still small (i.e., OC300 contains few pores), although most of the OH groups remain, and thus, the percentage of the OH groups able to directly make contact with Cs+ (the surface OH groups) is considerably low (Fig. 7a). The total number of OH groups in OC500 is lower than that in OC300 owing to the pyrolysis progression. However, the number of surface OH groups is higher because of an increase in surface area (Fig. 7b). The Cs+-adsorption ability of OC700 decreases evidently, because almost all the OH groups are broken down thermally.

Fig. 7

Changes in OH groups and pores of OC with CT for a OC300, b OC500, and c OC700. Blue filled circles: OH groups in bulk of solid, red filled circles: OH groups on surface

This explanation raises the issue of why the Cs+-adsorption ability of OC700 was not negligible despite no O–H stretching vibrations being detected by IR-PA spectroscopy. This indicates that Cs+ adsorption to OC700 is due to factors other than OH groups.

The Raman and IR-PA spectra suggest that the graphite precursors having π-electrons are sufficiently contained in OC700. However, it is very difficult for hydrated Cs+ to be intercalated between the stacks in terms of the space of graphite layers [26] and the diameter of hydrated Cs+ [27, 28], if the stacks of graphitic carbon in OC700 grow considerably. Meanwhile, it is known that the cation–π interaction occurs in simple aromatics [29]. Therefore, the surface π-electrons in OC700 are likely to be able to capture Cs+, because the interactions are comparable to typical hydrogen bonds [30, 31]. Accordingly, it is assumed that the Cs+-adsorption ability in OC700 is caused largely by the interaction between Cs+ and the surface π-electrons, although the contribution from the π-electrons to Cs+-adsorption performance is likely to be much smaller than that from an OH group. Moreover, this interaction may explain why the Cs+-adsorption ability of commercial charcoal carbonized above 1000 °C is not negligibly low despite no OH groups [10].

In conclusion, the Cs+-adsorption ability of charcoal depends mainly on the number of surface OH groups per unit weight of charcoal. The present study demonstrates that a new carbonization technique that preserves OH groups as far as possible and maximally extends the surface area is essential for producing high-performance charcoal for Cs+ adsorption.

Since surface OH groups play the most important role in capturing Cs+, an investigation into chemical species formed from Cs+ and surface OH groups is required to achieve a deeper understanding of the Cs+-adsorption mechanism in charcoal. Figure 8 illustrates presumable models of the interactions between Cs+ and surface OH groups (i.e., surface complexes). In general, ions interacting with a solid surface are classified into two types [32, 33]. The first involves ions binding directly to the surface without intervening solvent molecules. Chemical species containing such ions are referred to as inner-sphere complexes (Fig. 8a–c). The second involves ions that indirectly interact with the surface via solvated molecules (e.g., water, methanol, or ethanol); complexes containing such ions are known as outer-sphere complexes (Fig. 8d, e). This concept was recently applied to Cs+ adsorption by soils [34].

Fig. 8

Structures of surface Cs+ complexes for ac inner-sphere complexes, d, e outer-sphere complexes. Black wavy line: surface of charcoal, red hashed line: ionic bond, green hashed line: coordinate or hydrogen bond, green H2O: coordinated water molecule, blue OH: non-ionized OH group on surface, red O: ionized OH group on surface

Among these surface complexes, we focus on an inner-sphere complex illustrated in Fig. 8c and an outer-sphere complex shown in Fig. 8e. In the former complex, Cs+ is coordinated by a neutral OH through a surface O atom. The latter complex has a water molecule coordinating to Cs+, which forms a hydrogen bond with a neutral OH. Thus, electrically neutral OH groups capture Cs+ in both complexes. The binding between Cs+ and the neutral OH group is probably the key to clarifying the Cs+-adsorption mechanism.

In general, point of zero charge (PZC) has been regarded as an important criterion for evaluating adsorption performance of adsorptive in aqueous solution when adsorbate has an electric charge. Hence, we have measured the PZC of the charcoal studied in the previous works and reported that the Cs+-adsorption ability of charcoal is considerably reduced when the pH of the aqueous solution approaches the PZC [5,6,7,8,9,10]. However, the ability did not completely disappear even when the pH of the aqueous solution decreased to slightly below the PZC; that is, the charcoal surface was charged to be slightly positive [8]. If the Cs+-adsorption ability depends only upon electrostatic attraction, the adsorption ability should be negligible when the pH falls below the PZC. Consequently, further investigation into the surface complexes is necessary for whole clarification of the Cs+-adsorption mechanisms.

More detailed studies using appropriate instrumental analyses are needed to further examine the Cs+ complexes, especially those shown in Fig. 8c, e. Furthermore, we are advancing preparations for determining the surface OH group concentration and pore structure in order to more deeply discuss the Cs+-adsorption mechanisms.


The adsorption isotherms presented here demonstrated that the Cs+-adsorption ability of OC strongly depends on CT and reaches a maximum within a temperature range from 300 °C to 700 °C. A noteworthy outcome of the present work is the IR-PA spectra of OC and CC samples. They confirmed that a considerable amount of residual OH groups exist on the surfaces of OC and CC synthesized at 300 °C and 500 °C.

The surface OH groups are therefore essential to the attraction to Cs+ in woody charcoal. Controlling of OH group decomposition and extension of specific surface area during carbonization process are essential to synthesizing woody charcoal with high performance in Cs+ adsorption.

Availability of data and materials

Not applicable



Japanese oak charcoal (for instance, OC carbonized at 500 °C for 2.0 h is referred to as OC500-2)


cellulose charcoal (for instance, CC carbonized at 700 °C for 1.0 h is referred to as CC700-1)




carbonization temperature


holding time


inductively coupled plasma mass spectrometry


mass reduction


point of zero charge


  1. 1.

    Narita E, Sasaki A, Aisawa S, Hirahara H (2013) Development of charcoals from corn wastes for prevention of environmental pollution. Wood Carbonization Res 9:59–67 (in Japanese)

  2. 2.

    Caccin M, Giacobbo F, Da Ros M, Mariani M, Besozzi L (2013) Adsorption of uranium, cesium and strontium onto coconut shell activated carbon. J Radioanal Nucl Chem 297:9–18

  3. 3.

    Khandaker S, Kuba T, Kamida S, Uchikawa Y (2017) Adsorption of cesium from aqueous solution by raw and concentrated nitric acid-modified bamboo. J Environ Chem Eng 5:1456–1464

  4. 4.

    Khandaker S, Toyohara Y, Kuba T (2018) Adsorptive removal of cesium from aqueous solution using oxidized bamboo charcoal. Water Res Ind 19:35–46

  5. 5.

    Yamauchi S, Kurimoto Y, Yatagai M (2013) Cesium ion adsorption on oak charcoal in aqueous solutions. Wood Carbonization Res 10:35–6742 (in Japanese)

  6. 6.

    Yamauchi S, Yamagishi T, Kirikoshi K, Yatagai M (2014) Cesium adsorption from aqueous solutions onto Japanese oak charcoal I: effects of the presence of group 1 and 2 metal ions. J Wood Sci 60:473–479

  7. 7.

    Yamauchi S, Yamagishi T, Kirikoshi K, Yatagai M (2015) Cesium adsorption from aqueous solutions onto Japanese oak charcoal II: effects of metal ions eluted from the charcoal. J Wood Sci 61:185–191

  8. 8.

    Yamauchi S, Yamagishi T, Kirikoshi K, Yatagai M (2016) Cesium adsorption from aqueous solutions onto Japanese oak charcoal III: effects of water-extraction treatment. J Wood Sci 62:562–566

  9. 9.

    Yamagishi T, Kurimoto Y, Yamauchi S (2017) A method for visualizing cesium adsorbed on wood charcoal using SEM-EDX. Wood Sci Technol 51:413–429

  10. 10.

    Yamauchi S, Yamagishi T, Kirikoshi K, Yatagai M (2017) Factors governing cesium adsorption of charcoals in aqueous solution. J Wood Sci 63:183–191

  11. 11.

    Honma S, Sano Y, Kubota M, Uehara K, Komazawa K (2000) Chemical structure and ammonia adsorption ability of todomatsu (Abies sachalinensis) wood carbonized in nitrogen and air atmospheres. Mokuzai Gakkaishi 46:348–354 (in Japanese)

  12. 12.

    Ishimaru K, Hata T, Bronsveld P, Meier D, Imamura Y (2007) Spectroscopic analysis of carbonization behavior of wood cellulose and lignin. J Mater Sci 42:122–129

  13. 13.

    Yamauchi S (2003) Infrared photoacoustic spectra of Japanese cedar (Cryptomeria japonica D. Don) wood and bark heat-treated at temperature ranging from 200 °C to 1100 °C. Eurasian J For Res 6:75–78

  14. 14.

    Yamauchi S, Kurimoto Y, Sakai Y (2017) Mössbauer characterization of iron in ancient buried trees excavated from the foothills of Mt, Chokai. J Nucl Radiochem Sci 17:23–298

  15. 15.

    Yamauchi S, Kikuchi Y, Kurimoto Y (2000) Raman spectral changes of sugi bark during thermal degradation and carbonization. Mater Sci Int 6:227–228

  16. 16.

    Yamauchi S, Kurimoto Y (2003) Raman spectroscopic study on pyrolyzed wood and bark of Japanese cedar: temperature dependence of Raman parameters. J Wood Sci 49:235–240

  17. 17.

    Fujii T, Mochidzuki K, Kobayashi S, Sakoda A (2011) Quick and simple analysis of lignocellulose ingredients by thermogravimetric analysis. J Jpn Soc Mater Cyc Was Mgt 22:293–297 (in Japanese)

  18. 18.

    Kawamoto H (2015) Reactions and molecular mechanisms of cellulose pyrolysis. Mokuzai Gakkaishi 61:1–24 (in Japanese)

  19. 19.

    Yoo KR, Ahn SJ, Kim K (1993) In-situ reflection FT-IR spectroscopic study of pyrolysis of lignite. Spectrosc Lett 26:1733–1744

  20. 20.

    Bellamy LJ (1975) The infra-red spectra of complex molecules. Chapman and Hall Ltd, London, pp 107–128

  21. 21.

    Shafizadeh F (1982) Introduction to pyrolysis of biomass. J Anal Appl Pyrolysis 3:283–305

  22. 22.

    Agarwal UP, Ralph SA (1997) FT-Raman investigation of milled wood lignins: softwood, hardwood, and chemically modified black spruce lignins. J Wood Chem Tech 31:324–344

  23. 23.

    Abe I, Iwasaki S, Iwata Y, Kominami H, Kera Y (1998) Relationship between method and adsorption property of charcoal. Tanso 185:277–284 (in Japanese)

  24. 24.

    Kitamura T, Matsumoto S, Katayama H (1999) The effect of carbonizing conditions on the properties of charcoal absorbent from cryptomeria. Mokuzai Gakkaishi 45:171–177 (in Japanese)

  25. 25.

    Pulido-Novicio L, Hata T, Kurimoto Y, Doi S, Ishihara S, Imamura Y (2001) Adsorption capacities and related characteristic of wood charcoal carbonized using a one-step or two-step process. J Wood Sci 47:48–57

  26. 26.

    Girifalco LA, Lad RA (1956) Energy of cohesion, compressibility, and the potential energy functions of the graphite system. J Chem Phys 25:693–696

  27. 27.

    Ohtaki H, Radnai T (1993) Structure and dynamics of hydrated ions. Chem Rev 93:1157–1204

  28. 28.

    Persson I (2010) Hydrated metal ions in aqueous solution: how regular are their structures? Pure Appl Chem 82:1901–1917

  29. 29.

    Ma JC, Dougherty DA (1997) The cation-π interaction. Chem Rev 97:1303–1324

  30. 30.

    Mecozzi S, Jr West A P, Dougherty DA (1996) Cation-π interactions in sample aromatics: electrostatics provide a predictive tool. J Am Chem Soc 118:2307–2308

  31. 31.

    Amicangelo JC, Armentrout PB (2000) Absolute binding energies of alkali-metal cation complexes with benzene determined by threshold collision-induced dissociation experiments and ab initio theory. J Phys Chem A 104:11420–11432

  32. 32.

    Sposito G (1989) The chemistry of soils. Oxford University Press, London, pp 127–147

  33. 33.

    Motschi H (1986) Aspects of the molecular structure in surface complexes; spectroscopic investigations. In: Stumm W (ed) Aqueous surface chemistry. John Wiley & Sons, New York, pp 11–125

  34. 34.

    Mukai H, Tamura K, Kikuchi R, Takahashi Y, Yaita T, Kogure T (2018) Cesium desorption behavior of weathered biotite in Fukushima considering the actual radioactive contamination of soils. J Environ Radioact 190–191:81–89

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TY and SY designed this study and wrote the initial draft of the manuscript. TY prepared the charcoals used in this study and performed the experiments for Cs+ adsorption. SY and YK contributed to measurements and interpretation of Raman and IR-PA spectra. KN improved a carbonization apparatus and devised an appropriate method of preparing charcoal. All authors have contributed to data collection and interpretation and critically reviewed the manuscript. All authors read and approved the final manuscript.

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Correspondence to Shigeru Yamauchi.

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Yamagishi, T., Nishikiori, K., Kurimoto, Y. et al. Cesium-adsorption mechanisms of woody charcoal discussed on the basis of its functional groups and nanostructure. J Wood Sci 65, 26 (2019).

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  • Cesium
  • Charcoal
  • Adsorption
  • Nanostructure
  • Hydroxy group
  • Hydrogen bond
  • Surface complex