Name: Assessment of Boron Doped Diamond Electrode Quality and Application to In Situ Modification of Local pH by Water Electrolysis (Video) | JoVE Journal
Uploaded: 2016-01-06T13:00:01.000+00:00
Duration: 13 min 9 s
Description: Learn standardized electrochemical assessment of boron doped diamond electrode quality through solvent window, capacitance, and non-diamond carbon analysis. This method enables reliable in situ local pH control for accurate electrochemical measurements.

ai_agent_IP

ai_agent

maintenance

instantTrialDurationMinutes

isBiopharma

enableNewMyJoveSectionDesign

educationFeatures

seoMetaApi

ai_copilot_institution_blacklist

ai_chat_institution_blacklist

freeAccessWindow

ssoRoleCapture

scheduledMaintenanceBanner

joveLabsFeatures

disable_autoplay_for_bots

extended_trial_duration

5 minutes

We would like to thank Dr. Jonathan Newland for the photograph in Figure 4B and for processing optical microscope images for the video, Miss Jennifer Webb for advice and visuals on contact angle measurements, Miss Sze-yin Tan for the solvent window data in Figure 2B, Dr Maxim Joseph for advice on Raman spectroscopy, and also members of the Warwick Electrochemistry and Interfaces Group who have helped to develop the protocols described herein. We would also like to thank Max Joseph, Lingcong Meng, Zoe Ayres and Roy Meyler for their part in filming the protocol.

NOTE: BDD electrodes are most commonly grown using chemical vapor deposition techniques, attached to a growth substrate. They leave the growth chamber H-terminated (hydrophobic). If grown thick enough the BDD can be removed from the substrate and is termed freestanding. The freestanding BDD growth surface is often polished to significantly reduce surface roughness. Cleaning the BDD in acid results in an oxygen (O)-terminated surface.
1. Acid Cleaning BDD
<ol>
	<li>Place a beaker of concentrated sulfuric acid (H2SO4; ~ 2 ml or deep enough to cover the diamond) on a hot plate at RT and insert the BDD.</li>
	<li>Add potassium nitrate (KNO3) until it no longer dissolves (~ 0.5 g in 2 ml), then cover with a watch glass and heat to ~ 300 &#176;C, the solution will turn brown as it heats and the potassium nitrate will dissolve. 
	CAUTION! Care should be taken when handling hot acid; rubber gloves, safety glasses and lab coat should be worn and this process should be conducted in a fume hood.</li>
	<li>Leave to heat for at least 30 min or until there is no longer any brown color to the solution, then turn off the hot plate and leave the solution to cool to RT.</li>
	<li>Carefully dispose of the acid by diluting in RT water and rinse the BDD with distilled water.</li>
	<li>Measure the surface contact angle, see section 1.2. Hydrophobic (H-terminated)20,21 electrodes have reported contact angles in the range 60-90&#176;3, which significantly reduces as the surface is rendered hydrophilic through O-termination.</li>
	<li>(optional alternative method) For very thin film electrodes (attached to the growth substrate and to avoid film delamination using the above treatment), wash once with 2-propanol and twice with deionized water in an ultrasonic bath. Then, adopt one of the following three cleaning procedures (1) anodically polarize the diamond for 30 min at 10 mA cm-2 in 1 M perchloric acid at 40 &#176;C22; or (2) anodically polarize the diamond for 20 min at 10 mA cm-2 in 1 M nitric acid, then subsequently cathodically polarize at 10 mA cm-2 for a further 20 min in the same solution23 or; (3) cycle the diamond between 2 V in 0.1 M H2SO4 until a stable electrochemical signal is achieved7. Follow this with step 1.4.</li>
</ol>
2. Contact Angle Measurement
<ol>
	<li>Place the diamond on the sample stage of a contact angle analyzer, ensuring it is flat. Place a 1 ml syringe in the positioner above the sample stage, secure a needle on the end. Fill the syringe with deionized water.</li>
	<li>Use the z-controller to lower the syringe to the sample, use the x- and y- controllers and the camera/illuminator to align the syringe above the center of the diamond.</li>
	<li>Using the analyzer software dispense repeat 1 &#181;l volumes of water out of the syringe until a droplet forms at the tip of the needle, visible on the camera image (never more than 10 &#181;l). Lower the needle to deposit the droplet on to the surface and adjust the illumination for maximum contrast.</li>
	<li>Collect an image and apply drop shape analysis software, using the conic section method. Click &#34;find baseline&#34; in the software, and then click &#34;computation&#34; followed by &#34;tangent&#34;. 
	NOTE: this procedure detects the baseline and fits a conic equation to the (elliptical) drop shape; a contact angle, &#952;, is drawn between the baseline and the tangent at the three-phase contact point.</li>
</ol>
3. BDD Material Characterization
<ol>
	<li>Raman Analysis for sp2/sp3 content
	<ol>
		<li>Carry out Raman (see reference14 for a guide to Practical Raman Spectroscopy) in several different areas of the BDD electrode,24 use of a 514.5 nm or 532 nm laser, which emphasizes sp2 content, is advocated.</li>
		<li>Turn on the micro-Raman spectrometer and allow ~30 min for the CCD Detector to cool down. Check the appropriate lens, diffraction grating and filters are in place for use with the laser of choice.</li>
		<li>Calibrate the system using a silicon (Si) calibration sample. Place the Si substrate in the instrument chamber and focus optically on the sample with the microscope. Shut the door to the chamber. Switch to laser view and check the laser spot is well defined and circular. Calibrate using the software, click &#34;tools&#34; followed by &#34;calibration&#34; then &#34;quick calibration&#34; then &#34;ok&#34;.</li>
		<li>Remove the Si substrate from the chamber and replace with the BDD electrode. Optically focus the microscope on the area of interest, switch to laser view and open the shutter to check that the laser is focused. Close the shutter.</li>
		<li>Take a Raman measurement using the software; click &#34;measurement&#34; then &#34;new&#34; then &#34;spectral acquisition.&#34; set the measurement wavenumber range to cover the features of interest, for BDD this is 200 - 1,800 cm-1; set the scan acquisition time (&#60;10 sec); set the laser power to 100% (for BDD) and; set the number of accumulations (repeat scans) to five (for BDD). If the resulting spectrum is very noisy more accumulations may be necessary. Press run and save the resulting spectrum for analysis. Take a picture of the area Raman was performed in using the live video. Save the image as a reference.</li>
		<li>Observe the peak ~ 1,332 cm-1 in the spectrum which indicates sp3 diamond (Figure 1); the broader the peak the more defects present3,25.</li>
		<li>Observe any NDC &#8212; indicated by a broad G peak centered at 1,575 cm-1 26, in the spectra (Figure 1A and 1B), originating from the stretching of paired sp2 sites; the greater the peak intensity the more NDC present. 
		NOTE: the &#960; bonds formed by sp2 C are more polarizable than sp3 &#963; bonds and are resonantly enhanced by visible lasers, leading to broader, more dominant, G peaks25. Note that the exact method used to perform analyses may vary between different instruments and software.</li>
	</ol>
	</li>
</ol>
4. Electrochemical Characterization
<ol>
	<li>Preparing ohmic contacts
	<ol>
		<li>Freestanding BDD
		<ol>
			<li>Using standard techniques sputter (or evaporate)the backside of the BDD with titanium (Ti)/gold (Au) 10 nm/300 nm, using a sputterer/evaporator at pressures below 1 &#215; 10-5 mBar. If a three target source is available, more ideally is Ti 10 nm / platinum (Pt) 10 nm / Au 300 nm to avoid diffusion of Ti into the Au.</li>
			<li>Anneal for 5 hr at 400 &#176;C (atmospheric pressure) enabling the Ti to form titanium carbide, crucial for formation of an ohmic contact27. 
			NOTE: if the back surface of the BDD is highly polished (~ nm roughness) then it is preferably to roughen the surface prior to sputter deposition to ensure a more robust coating. This can be achieved by, for example, low power laser micromachining the surface (removing &#60; 30 &#956;m material).</li>
		</ol>
		</li>
		<li>Thin film diamond grown on a conducting substrate
		<ol>
			<li>Sputter/evaporate as above, but to the top face, using a shadow mask gently place on the top surface to avoid top contacting the entire electrode. 
			OR</li>
			<li>Scratch the back of the conducting substrate using a diamond tipped pen. Then coat the scratched area with conducting Ag paste or a similar conductive paint by painting on a thin layer with a small paintbrush. Finally, electrically connect by attaching copper wires with conductive epoxy. 
			NOTE: there are a variety of ways to prepare the BDD after electrical contact as described in reference 4, e.g. if the BDD can be machined into smaller structures, seal in glass or epoxy, or if still attached to the wafer clamp/attach an electrochemical cell to the top surface.</li>
		</ol>
		</li>
	</ol>
	</li>
	<li>Capacitance Measurements
	<ol>
		<li>Prepare a 20 ml of 0.1 M KNO3 solution by weighing 0.20 g in doubly distilled water (this water quality is recommended throughout, resistivity 18.2 M cm). Clean the electrode prior to use either by alumina polishing or by electrochemically cycling in dilute acid (see section 1 NOTE)16,23,28.</li>
		<li>Using a potentiostat run cyclic voltammograms (CVs) at 0.1 V sec-1 between -0.1 V and 0.1 V, starting at 0 V, with the BDD as the working electrode versus a common reference electrode, e.g. silver/silver chloride (Ag/AgCl) or a saturated calomel electrode (SCE), and a Pt counter electrode. Analyze the second CV. 
		NOTE: Figure 2A shows a typical capacitance curve recorded with a freestanding metallic doped BDD electrode.</li>
		<li>Measure the total current magnitude at 0 V from the recorded capacitance curve and divide by 2, this value is &#34;i&#34;. Determine the capacitance, C, using the value for i, with equation 1, normalize with respect to electrode area (accounting for surface roughness if appropriate) and quote in &#181;F cm-2. High quality, &#34;metal-like&#34; BDD has a capacitance &#60;&#60; 10 &#181;F cm-2. Use any data plotting software to present and analyze the data. 
		i = C(Vt-1)&#160;&#160; (eq. 1); 
		where i is current (A) and (V t-1) is the potential scan rate.</li>
	</ol>
	</li>
	<li>Solvent Window
	<ol>
		<li>Clean the electrode as in step 4.2.1. Using a potentiostat run a CV in 0.1 M KNO3 at 0.1 V sec-1 from 0 V to -2 V then between -2 V and +2 V and back to 0 V with the BDD as the working electrode vs. a common reference electrode and Pt counter electrode. Repeat. Analyze the second CV, an example CV is shown in Figure 2B.</li>
		<li>Convert current to current density (mA cm-2), taking surface roughness into account, and quote the solvent window as the potential window defined by current limits of &#177;0.4 mA cm-2 in both directions.7,29 Use any data plotting software to present and analyze the data.</li>
		<li>Observe the evidence of NDC (sp2 carbon) in the solvent window; the oxygen reduction reaction is favored on NDC that is clearly evident in the reductive window. Oxidation of sp2 containing groups also results in characteristic peaks just before water electrolysis in the anodic window (Figure 2B). 
		NOTE: high quality &#34;metallic&#34; BDD electrodes have solvent windows &#62;&#62; 3 V, do not support the oxygen reduction reaction (ORR) in 0.1 M KNO3 (or ORR is strongly kinetically retarded) and show negligible NDC oxidation signatures.</li>
	</ol>
	</li>
	<li>Redox Electrochemistry
	<ol>
		<li>Clean the electrode as in step 4.2.1.</li>
		<li>Using a potentiostat record CVs in 1 mM ruthenium hexaamine (Ru(NH3)63+) and 0.1 M KNO3 between +0.2 V and -0.8 V versus SCE, for scan rates in the range 0.05 V sec-1- 0.2 V sec-1. 
		NOTE: This couple shows fast electron transfer and is electroactive in a region which challenges p-type semiconducting BDD. sp2 containing BDD will also show ORR in this region, the signal for the latter is more evident as the concentration of Ru(NH3)63+ is decreased.</li>
		<li>Measure the voltage separation between the anodic and cathodic peak current (&#916;Ep) from the recorded CV, and the temperature as described20. For &#34;metal-like&#34; ohmically contacted oxygen-terminated BDD at 298 K, &#916;Ep &#60; 70 mV30,31. Larger &#916;Ep values are symptomatic of a poor ohmic contact or a lower boron content, as shown in Figure 2C for BDD electrodes of dopant densities in the range 9.2 &#215; 1016 to 3 &#215; 1020 B atoms cm-3.</li>
		<li>Measure the peak current of the forward scan, ip, and correlate with that expected from the Randles Sevcik equation 2 (quoted at 298 K)3,30, assuming the electrode is disk-shaped in geometry and large enough (diameter 1 mm) that linear diffusion dominates. Use any data plotting software to present and analyze the data. 
		ip = 2.69 &#215; 105 n3/2 AD1/2 cv1/2&#160;&#160; (eq 2) 
		where n is the number of electrons transferred, A is area (cm2), D is diffusion coefficient (cm2 sec-1), c is concentration (mol cm-3) and v is scan rate (V sec-1).</li>
	</ol>
	</li>
</ol>
5. pH Generation: Preparation of pH Sensitive Electrode and pH Generation
<ol>
	<li>Iridium Oxide (pH sensitive) Solution Preparation
	<ol>
		<li>Prepare a 20 ml 0.1 M KNO3 solution as in section 5.4.1. Add 5 drops of phenolphthalein indicator solution using a Pasteur pipette and stir (this is sufficient to see a response by eye, but for a more intense color, add more drops). Place the BDD working electrode and Pt counter electrode in solution.</li>
		<li>Adjust pH of the solution to 10.5 by addition of anhydrous potassium chloride salt, stirring continuously. Leave covered and stirring for 48 hr at RT to stabilize, at this stage the solution will gradually go from yellow-green to blue-purple. Store in a refrigerator at 3 &#176;C.</li>
	</ol>
	</li>
	<li>pH Sensitive Iridium Oxide Film Deposition
	<ol>
		<li>Using a potentiostat run a CV in the iridium oxide solution between 0 V and +1 V versus SCE to determine the potential at which the maximum current is recorded. This is the deposition potential, Edep as shown in Figure 3A, typically lying between ~+0.6 V &#8211; +0.85 V; it can vary depending on a number of factors such as temperature, electrode material etc.32,33</li>
		<li>Using chronoamperometry with a potentiostat, step the potential from 0 V (&#34;initial E&#34; and &#34;Low E&#34; in the software), where no electrolysis occurs to Edep (&#34;High E&#34; in the software), for a time period of 0.2 sec per step, repeat 100x.</li>
		<li>Run a CV between 0 V and +1 V in 0.1 M H2SO4 for the IrOx deposited electrode. The characteristic CV shape is shown in Figure 3B. A current density in the range ~ 0.6 mA cm-2 - 0.7 mA cm-2 for the first anodic peak (corresponding to an average film thickness of ~ 8 nm for 0.7 mA cm-2), indicates a stable pH sensitive film34,35.</li>
		<li>If the current density is less than 0.6 mA cm-2 repeat steps 5.2.2 - 5.2.4 until this value is reached. Leave the electrode in pH 7 buffer solution for 24 hr to hydrate as the response of the IrOx film is hydration-dependant33.</li>
	</ol>
	</li>
	<li>IrOx Film pH Characterization
	<ol>
		<li>Prepare a series of buffer solutions which cover the pH range of interest (pH 2 - pH 12), these can be made in house (e.g. Carmody36) or purchased commercially.</li>
		<li>Rinse the electrode with distilled water. Place the IrOx electrode and reference electrode in the buffer solution of lowest pH. Using a potentiostat record the open circuit potential (OCP) over 30 sec, with three repeats. Remove the electrode from the solution, rinse and place in the next buffer.</li>
		<li>Repeat step 5.3.2 for each buffer, then repeat the series at least twice. Plot pH vs. OCP, the calibration plot for the film response. An IrOx film exhibits a slope with a gradient between 59 - 80 mV per decade37. 
		NOTE: Figure 3C shows an example calibration plot for a successful IrOx pH sensor on BDD.</li>
	</ol>
	</li>
	<li>Using a pH generator and measurement system 
	NOTE: this assumes use of a dual electrode system where one electrode is coated with the IrOx film (e.g. disc) and the second (e.g. BDD ring) will generate H+ or OH- galvanostatically from water electrolysis.
	<ol>
		<li>Prepare a 20 ml 0.1 M KNO3 solution by adding deionized water to the salt. Connect the IrOx coated electrode as the working electrode in a two electrode system, with the second electrode a stable reference electrode e.g. SCE. Measure the OCP using a potentiostat, to establish the starting pH.</li>
		<li>Connect the generator electrode to a suitable two electrode galvanostatic system with a counter electrode, e.g. Pt foil, and repeat step 5.4.1, but after a defined period of time apply a current to the generator electrode. 
		NOTE: we find currents in the range 0 to &#177; 50 &#956;A are suitable with our BDD electrodes; larger currents result in appreciable gas evolution. The magnitude and direction of the current depends on the desired result; a positive current will result in a shift to more acidic pH and a negative current to more alkaline pH, the larger the current the greater the pH change.</li>
		<li>Using the potentiostat, record the change in OCP in response to the galvanostatic current, wait until the response stabilizes. Then place the IrOx electrode in pH 7 buffer for 10 min to re-equilibrate the IrOx film.</li>
		<li>Repeat steps 5.4.2 to 5.4.3 with different applied currents, until all the data required has been collected. Plot the data using the calibration curve obtained in section 5.3 to convert OCP to pH, an example data set is shown in Figure 4A. Remove the IrOx film using alumina polishing or pulsing in 0.1 M H2SO4 from +2 V to -2 V for 0.2 sec, &#215;100. Apply to the measurement system of interest.</li>
	</ol>
	</li>
	<li>Visual assessment of local pH generation
	<ol>
		<li>Prepare a 20 ml 0.1 M KNO3 solution as in section 5.4.1. Add 5 drops of phenolphthalein indicator solution using a Pasteur pipette and stir (this is sufficient to see a response by eye, but for a more intense color, add more drops). Place the BDD working electrode and Pt counter electrode in solution.</li>
		<li>Apply a negative current to the working electrode using a galvanostat as in step 5.4.2 (e.g. ~ -0.6 mA cm-2) such that the solution changes color from colorless to pink. This now locally generates a solution which is at pH &#8805; 10.5.</li>
		<li>Repeat step 5.5.1 with 5 drops of methyl red solution instead of phenolphthalein and stir. Apply a sufficiently positive current (e.g. ~ 6.6 mA cm-2) such that the solution changes color from yellow to red. This now locally generates a solution which is at pH &#8804; 4.238.</li>
	</ol>
	</li>
</ol>

The authors declare that they have no competing financial interests.

Starting with an O-terminated surface is advocated because the H-terminated surface is electrochemically unstable, especially at high anodic potentials7,40,41. Changing surface termination can affect the electron transfer kinetics of inner sphere couples, such as water electrolysis (used herein to change the local solution pH). Furthermore, if the BDD contains significant NDC at grain boundaries it is also possible that upon application of the extreme anodic/cathodic potentials advocated in this article for pH...

Choice of electrode material is of great importance when conducting any electroanalytical study. In recent years, sp3 carbon (diamond) doped with sufficient boron to render the material &#34;metal-like&#34; has become a popular choice for a wide range of electroanalytical applications due to its excellent electrochemical (and thermal and mechanical) properties1,2,3. These include corrosion resistance under extreme solution, temperature and pressure conditions4 ultra-wide solvent windows, low background currents, and reduced fouling, in comparison to other commonly used electrode materials5-7,3. However, increasing non-diamond-carbon (NDC: sp2) content results in a decreasing solvent window, increasing background currents7,8, changes in both structural integrity and sensitivity towards different inner sphere redox species, e.g. oxygen9-12.
Note for some applications, NDC presence is seen as advantageous13. Furthermore, if the material does not contain sufficient boron it will behave as a p-type semi-conductor and show reduced sensitivity to redox species in the reductive potential window, where the material is most depleted of charge carriers7. Finally, the surface chemistry of boron doped diamond (BDD) can also play a role in the observed electrochemical response. This is especially true for inner sphere species which are sensitive to surface chemistry and lower doped diamond where a hydrogen (H-)-terminated surface may make a semi-conducting BDD electrode appear &#34;metal-like&#34;7.
To take advantage of the superior properties of BDD, it is often essential the material is sufficiently doped and contains as little NDC as possible. Dependent on the method adopted to grow the BDD, the properties can vary14,15. This paper first suggests a materials and an electrochemical characterization protocol guide for assessing BDD electrode suitability prior to use (i.e. sufficient boron, minimal NDC) and then describes one application based on locally changing pH electrochemically using the protocol-verified electrode. This process takes advantage of the surface resilience of NDC-free BDD towards corrosion or dissolution under application of extreme applied potentials (or currents) for long periods of time. In particular the use of a BDD electrode to generate stable proton (H+) or hydroxide (OH-) fluxes due to electrolysis (oxidation or reduction respectively) of water in close proximity to a second (sensor)16,17 is described herein.
In this way it is possible to control the pH environment of the sensor in a systematic way, e.g. for pH titration experiments, or to fix the pH at a value where the electrochemical process is most sensitive. The latter is especially useful for applications where the sensor is placed at the source, e.g. river, lake, sea and the pH of the system is not optimal for the electrochemical measurement of interest. Two recent examples include: (i) generation of a localized low pH, in a pH neutral solution, for the electrodeposition and stripping of mercury17; note BDD is a favored material for electrodeposition of metals due to the extended cathodic window9,18,19. (ii) Quantification of the electrochemically detectable form of hydrogen sulfide, present at high pH, by locally increasing the pH from neutral to strongly alkaline16.

<table><tbody><tr><td>Pt Wire</td><td></td><td></td><td>Counter Electrode</td></tr><tr><td>Saturated Calomel Electrode</td><td>IJ Cambria Scientific Ltd.</td><td>2056</td><td>Reference Electrode (alternatively use Ag|AgCl)</td></tr><tr><td>BDD Electrode</td><td></td><td></td><td>Working Electrode</td></tr><tr><td>Iridium Tetrachloride</td><td>VWR International Ltd</td><td>12184.01</td><td></td></tr><tr><td>Hydrogen Peroxide</td><td>Sigma-Aldrich</td><td>H1009</td><td>(30% w/w) Corrosive</td></tr><tr><td>Oxalic Acid&amp;nbsp;</td><td>Sigma-Aldrich</td><td>241172</td><td>Harmful, Irritant</td></tr><tr><td>Anhydrous Potassium Chloride</td><td>Sigma-Aldrich</td><td>451029</td><td></td></tr><tr><td>Sulphuric Acid</td><td>VWR International Ltd</td><td>102765G</td><td>(98%) Corrosive</td></tr><tr><td>Potassium Nitrate</td><td>Sigma-Aldrich</td><td>221295</td><td></td></tr><tr><td>Hexaamine Ruthenium Chloride</td><td>Strem Chemicals Inc.</td><td>44-0620</td><td>Irritant</td></tr><tr><td>Perchloric Acid</td><td>Sigma-Aldrich</td><td>311421</td><td>Oxidising, Corrosive</td></tr><tr><td>2-Propanol</td><td>Sigma-Aldrich</td><td>24137</td><td>Flammable</td></tr><tr><td>Nitric Acid</td><td>Sigma-Aldrich</td><td>695033</td><td>Oxidising, Corrosive</td></tr><tr><td>Sputter/ Evapourator</td><td></td><td></td><td>With Ti &amp;amp; Au targets</td></tr><tr><td>Raman</td><td></td><td></td><td>514.5 nm laser</td></tr><tr><td>Annealing Oven</td><td></td><td></td><td>Capable of 400 &amp;deg;C</td></tr><tr><td>Ag paste</td><td>Sigma-Aldrich</td><td>735825</td><td>or other conductive paint</td></tr><tr><td>Potentiostat</td><td></td><td></td><td></td></tr><tr><td>pH Buffer solutions</td><td>Sigma-Aldrich</td><td>38740-38752</td><td>Fixanal buffer concentrates</td></tr><tr><td>Phenolphthalein Indicator</td><td>VWR International Ltd</td><td>210893Q</td><td></td></tr><tr><td>Methyl Red Indicator</td><td>Sigma-Aldrich</td><td>32654</td><td></td></tr></tbody></table>

assessment of boron doped diamond electrode quality and application to in situ modification of local ph by water electrolysis

Assessment of Boron Doped Diamond Electrode Quality and Application to In Situ Modification of Local pH by Water Electrolysis

Boron doped diamond (BDD) electrodes have shown considerable promise as an electrode material where many of their reported properties such as extended solvent window, low background currents, corrosion resistance, etc., arise from the catalytically inert nature of the surface. However, if during the growth process, non-diamond-carbon (NDC) becomes incorporated into the electrode matrix, the electrochemical properties will change as the surface becomes more catalytically active. As such it is important that the electrochemist is aware of the quality and resulting key electrochemical properties of the BDD electrode prior to use. This paper describes a series of characterization steps, including Raman microscopy, capacitance, solvent window and redox electrochemistry, to ascertain whether the BDD electrode contains negligible NDC i.e. negligible sp2 carbon. One application is highlighted which takes advantage of the catalytically inert and corrosion resistant nature of an NDC-free surface i.e. stable and quantifiable local proton and hydroxide production due to water electrolysis at a BDD electrode. An approach to measuring the local pH change induced by water electrolysis using iridium oxide coated BDD electrodes is also described in detail.

Raman spectra and electrochemical characteristics were obtained for representative BDD macrodisc electrodes with different dopant densities, and both significant and negligible levels of NDC, Figures 1 and 2. Figures 1A and B show typical Raman data for NDC-containing thin film microcrystalline BDD and larger grain freestanding BDD, doped above the metallic threshold, respectively. The presence of NDC is identifiable by t...

A protocol is described for the characterization of the key electrochemical parameters of a boron doped diamond (BDD) electrode and subsequent application for in situ pH generation experiments.

Boron doped diamond (BDD) electrodes have shown considerable promise as an electrode material where many of their reported properties such as extended ...

The goal of this video is to illustrate a standardized method for the electro-chemical assessment of diamond quality through solvent window, capacitance, reversability, and non-diamond carbon presence. Quality checked diamond electrodes are used to electro-chemically control the local pH of the measurement environment. The diamond electrode assessment method can help researchers in the field compare and contrast their results with others, as well as choose the appropriate diamond electrode for a given application.The main advantages of the work presented are both a standardized assessment approach to diamond electrode quality, and a reliable quantitative methodology for changing local pH. Generally, individuals new to this method will struggle, because electro-chemical characterization of diamond quality does not often take place across the research field, leading to contrasting data. Demonstrating the procedures alongside Tania will be Max Joseph, post-doc from my laboratory, as well as the PhD students Lincong Meng, Roy Meyler, and Zoe Ayres.Several types of boron doped diamond, or BDD, are available for electro-chemical use. Typical examples include free-standing all diamond substrates, and thin film supported on a non-diamond growth substrate. The thin film substrate-supported BDD should not be acid cleaned to avoid disintegration.To begin, place a beaker of concentrated sulfuric acid on a hot plate at room temperature, and insert the BDD. Add potassium nitrate until it no longer dissolves. Then, cover with a watch glass and heat to approximately 300 degrees Celsius.The solution will turn brown as it heats, and the potassium nitrate will dissolve. Leave the solution to heat for at least 30 minutes or until there is no longer any brown color to the solution. Then, turn off the hot plate and leave the solution to cool to room temperature.Hydrophobic hydrogen terminated electrodes have reported contact angles of 60 to 90 degrees, which significantly reduces as the surface is rendered hydrophilic through oxygen termination. Place the diamond on the sample stage of a contact angle analyzer, ensuring it is flat. Place a one milliliter syringe in the positioner above the sample stage, and secure a needle on the end.Fill the syringe with de-ionized water. Use the Z controller to lower the syringe to the sample. Then, use the X and Y controllers and the camera illuminator to align the syringe above the center of the diamond.Using the analyzer software, dispense repeat one microliter volumes of water out of the syringe until a droplet forms at the tip of the needle, as visible on the camera image. Lower the needle to deposit the droplet onto the surface, and adjust the illumination for maximum contrast. Collect an image and apply the drop shape analysis software using the Conic section method.Click find baseline'in the software, and then click computation'followed by tangent. To perform raman analysis for sp2 sp3 content, turn on the micro raman spectrometer and allow approximately 30 minutes for the ccd detector to cool down. Check that the appropriate lens, defraction grading, and filters are in place for use with the laser of choice.To calibrate the system using a silicon calibration sample, first place the silicon substrate in the instrument chamber. Focus optically on the sample with the microscope. After shutting the door to the chamber, switch to laser view and check that the laser spot is well-defined and circular.Calibrate using the software by clicking tools'followed by calibration, quick calibration, and then, okay. Remove the silicon substrate from the chamber and replace it with the BDD electrode. Optically focus the microscope on the area of interest.Switch to laser view and open the shutter to check that the laser is focused. Close the shutter. Take a raman measurement using the software.Click measurement, then new, then spectral acquisition. Set the measurement wave number range to cover the features of interest. Set the scan acquisition time to less than 10 seconds, the laser power to 100 percent, and the number of accumulations to five.Press run'and save the resulting spectrum for analysis. Take a picture of the area raman was performed in using the live video. Save the image as a reference.Observe the peak at approximately 1, 332 inverse centimeters in the spectrum, which indicates sp3 diamond. The broader the peak, the more defects are present. Observe any non-diamond carbon, or NDC, as indicated by a broad g peak centered at 1, 575 inverse centimeters in the spectrum, originating from the stretching of paired sp2 sites.The greater the peak intensity, the more NDC present. Clean the electrode prior to use either by aluminum polishing or by electro-chemically cycling in dilute acid. Using a potentiostat, run cyclic voltammograms, or Cvs, at 0.1 volts per second between negative 0.1 volt and 0.1 volt, starting at zero volts.Use the BDD as the working electrode, versus a platinum counter electrode and a common reference electrode. Analyze the second CV.Measure the total current magnitude at zero volts from the recorded capacitance curve, and divide by two. This value is I.Determine the capacitance C using the value for I as described in the text protocol.Using a potentiostat, run a CV in 0.1 molar potassium nitrate at 0.1 volts per second from zero volts to negative two volts, and then between negative two volts and positive two volts, and back to zero volts. Use the BDD as the working electrode, versus a common reference electrode and platinum counter electrode. After repeating once, analyze the second CV.Convert the current to current density, taking surface roughness into account.Quote the solvent window as the potentially window, defined by current limits of plus or minus 0.4 milliamps per centimeter squared in both directions. Observe the evidence of NDC in the solvent window. The oxygen reduction reaction is favored on NDC that is clearly evident in the reductive window.Using a potentiostat, record Cvs in one millimolar ruthenium hexamine and 0.1 molar potassium nitrate between positive 0.2 volts and negative 0.8 volts versus SCE. Use scan rates in the range of 0.05 volts per second to 0.2 volts per second. Measure the peak current of the forward scan IP and correlate with that expected from the Randles-Sevcik equation.Assuming that the electrode is disc-shaped in geometry and large enough that linear diffusion dominates. Using a potentiostat, run a CV in the iridium oxide solution between zero volts and positive one volt versus SCE to determine the potential at which the maximum current is recorded. This is the deposition potential, EDep, typically lying between approximately positive 0.6 volts and positive 0.85 volts.It can vary depending on temperature and electrode material. Using chronoamperometry with a potentiostat, step the potential from zero volts, where no electrolysis occurs, to EDep for a time period of 0.2 seconds per step. Shown here is the electrode surface before and after deposition, displaying film formation.Next, run a CV between zero volts and positive one volt in 0.1 molar sulfuric acid for the iridium oxide deposited electrode. The characteristic CV shape is shown here. Add five drops of phenolphthalein indicator solution to a 20 milliliter 0.1 molar potassium nitrate solution using a Pasteur pipette, and stir.Place the BDD working electrode and platinum counter in solution. Apply a sufficiently negative current to the working electrode using a galvanostat such that the solution local to the electrode changes color from colorless to pink. Repeat with five drops of methyl red solution, instead of phenolphthalein, and stir.Apply a sufficiently positive current such that the solution local to the electrode changes color from yellow to red. Shown here is typical raman data recorded with a 514 nanometer laser on NDC containing diamond. A high-quality boron doped diamond would only show the sharp sp3 peak at around 1, 332 inverse centimeters.A high-quality NDC free boron doped diamond electrode typically exhibits a wide, featureless solvent window. The capacitance curve should return a capacitance of much less than 10 microfarads per centimeter squared, as shown. A CV recorded with a typical outer sphere redox mediator at a sufficiently doped boron doped diamond shows a close to 59 millivolt separation between the anodic and cathodic current peaks.Using various geometries of dual boron doped diamond electrodes in either stationary or convective systems, it is possible to generate both acidic and alkaline local pH changes via electrolysis of water on one electrode as seen in these typical, experimentally-measured pH versus time profiles. After watching this video, you should have a good understanding of how to characterize diamond electrodes, and be able to choose the right electrodes for the appropriate application.

assessment-boron-doped-diamond-electrode-quality-application-to-situ

Research

JoVE Journal

Chemistry

We present a unique platform for characterizing electrode surfaces in solid oxide fuel cells (SOFCs) that allows simultaneous performance of multiple characterization techniques (e.g. in situ Raman spectroscopy and scanning probe microscopy alongside electrochemical measurements). Complementary information from these analyses may help to advance toward a more profound understanding of electrode reaction and degradation mechanisms, providing insights into rational design of better materials for...

Probing and Mapping Electrode Surfaces in Solid Oxide Fuel Cells

A procedure for performing reductive electropolymerization of vinyl-containing compounds onto glassy carbon and fluorine doped tin-oxide coated electrodes is presented. Recommendations on electrochemical cell configurations and troubleshooting procedures are included. Although not explicitly described here, oxidative electropolymerization of pyrrole-containing compounds follows similar procedures to vinyl-based reductive electropolymerization.

Reductive Electropolymerization of a Vinyl-containing Poly-pyridyl Complex on Glassy Carbon and Fluorine-doped Tin Oxide Electrodes

A method for electrochemically etching field emission tips is presented. Etching parameters are characterized and the operation of the tips in field emission mode is investigated.

Electrochemical Etching and Characterization of Sharp Field Emission Points for Electron Impact Ionization

We present a procedure for real-time imaging and elemental composition analysis of boehmite particles in deionized water by in situ liquid Scanning Electron Microscopy.

In Situ Characterization of Boehmite Particles in Water Using Liquid SEM

This protocol describes the measurement of the electromotive force of alkaline-earth elements in liquid metal alloys at high temperatures (723-1,123 K) to determine their thermodynamic properties, including activity, partial molar entropy, partial molar enthalpy, and phase transition temperatures, over a wide composition range.

Determination of Thermodynamic Properties of Alkaline Earth-liquid Metal Alloys Using the Electromotive Force Technique

The incorporation of reference electrodes in a Li-ion battery provides valuable information to elucidate degradation mechanisms at high voltages. In this article, we present a cell design that accommodates multiple reference electrodes, along with the assembly steps to assure maximum accuracy of the data obtained in electrochemical measurements.

In Situ Lithiated Reference Electrode: Four Electrode Design for In-operando Impedance Spectroscopy

Here we present a protocol of whole-cell electrochemical experiments to study the contribution of proton transport to the rate of extracellular electron transport via the outer-membrane cytochromes complex in Shewanella oneidensis MR-1.

Electrochemical Detection of Deuterium Kinetic Isotope Effect on Extracellular Electron Transport in Shewanella oneidensis MR-1

This protocol demonstrates a method for electrochemical roughening of thin-film platinum electrodes without preferential dissolution at grain boundaries. The electrochemical techniques of cyclic voltammetry and impedance spectroscopy are demonstrated to characterize these electrode surfaces.

Electrochemical Roughening of Thin-Film Platinum Macro and Microelectrodes

We describe aqueous and organic solvent systems for the electropolymerization of poly(3,4-ethylenedioxythiophene) to create thin layers on the surface of gold microelectrodes, which are used for sensing low molecular weight analytes.

Electrochemical Preparation of Poly(3,4-Ethylenedioxythiophene) Layers on Gold Microelectrodes for Uric Acid-Sensing Applications

Here we present a protocol for characterizing mediated extracellular electron transfer (EET) in lactic acid bacteria using a three-electrode, two-chamber bioelectrochemical system. We illustrate this method with Lactiplantibacillus plantarum and the redox mediator 1,4-dihydroxy-2-naphthoic acid and provide a thorough description of the electrochemical techniques used to evaluate mediated EET.

Characterizing Mediated Extracellular Electron Transfer in Lactic Acid Bacteria with a Three-Electrode, Two-Chamber Bioelectrochemical System

Learn standardized electrochemical assessment of boron doped diamond electrode quality through solvent window, capacitance, and non-diamond carbon analysis. This method enables reliable in situ local pH control for accurate electrochemical measurements.

Assessment of Boron Doped Diamond Electrode Quality and Application to In Situ Modification of Local pH by Water Electrolysis

Explore More Videos