Nickel–zinc battery: Difference between revisions

Nickel–zinc battery
	Nickel–zinc cells in AA and AAA sizes
Specific energy	100 W·h/kg
Energy density	280 W·h/L
Specific power	> 3000 W/kg
Energy/consumer-price	2–3Wh/US$
Nominal cell voltage	1.65 V

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A nickel–zinc battery (Ni–Zn battery or NiZn battery) is a type of rechargeable battery similar to nickel–cadmium batteries, but with a higher voltage of 1.6 V.

Larger nickel–zinc battery systems have been known for over 100 years. Since 2000, development of a stabilized zinc electrode system has made this technology viable and competitive with other commercially available rechargeable battery systems. Unlike some other technologies, trickle charging is not recommended.

History

In 1901 Thomas Alva Edison was awarded U.S. patent 684,204 for a rechargeable nickel–zinc battery system.^[1]

The battery was later developed by the Irish chemist Dr. James J. Drumm (1897–1974),^[2] and installed in four two-car Drumm railcar sets between 1932 and 1949 for use on the Dublin–Bray railway line. Although successful, they were withdrawn when the batteries wore out. Early nickel–zinc batteries provided only a small number of discharge–recharge cycles. In the 1960s nickel–zinc batteries were investigated as an alternative to silver–zinc batteries for military applications, and in the 1970s were again of interest for electric vehicles.^[3] Evercel Inc. developed and patented several improvements in nickel–zinc batteries, but withdrew from that area in 2004.^[4]

Applications

Nickel–zinc batteries have a charge–discharge curve similar to 1.2 V NiCd or NiMH cells, but with a higher 1.6 V nominal voltage.^[5]

Nickel–zinc batteries perform well in high-drain applications, and may have the potential to replace lead–acid batteries because of their higher energy-to-mass ratio and higher power-to-mass ratio – as little as 25% of the mass for the same power.^[6] Nickel–zinc batteries are less expensive than nickel–cadmium batteries^[6] and are expected to be priced somewhere between nickel–cadmium and lead–acid types. Nickel–zinc may be used as a substitute for nickel–cadmium. The European Parliament has supported bans on cadmium-based batteries;^[1] nickel–zinc is a good alternative for power tools and other applications. A disadvantage is increased self-discharge rate after about 30–50 cycles, so that batteries do not hold their charge as long as when new. Where this is not a problem nickel–zinc is a good choice for applications requiring high power and high voltage.^[7]

Battery life

Compared with cadmium hydroxide, the tendency of the soluble zinc hydroxide ion (zincate) to dissolve into solution and not fully migrate back to the cathode during recharging has, in the past, presented challenges for the commercial viability of the nickel–zinc battery.^[1]^[3] Another common issue with zinc rechargeable batteries is electrode shape change and dendrites (or "whiskers"), which may reduce the cell discharging performance or, eventually, short out the cell, resulting in a low cycle life.

Recent advances have enabled this problem to be greatly reduced. These advances include improvements in electrode separator materials, inclusion of zinc material stabilizers, and electrolyte improvements (e.g. by using phosphates). PowerGenix has developed 1.6 V batteries with claimed battery cycle life comparable to NiCd batteries.^[8]

Battery cycle life is most commonly specified at a discharge depth of 80 percent of rated capacity and assuming a one-hour discharge current rate. As the discharge current or the depth of discharge is reduced, the number of charge-discharge cycles for a battery increases. When comparing Ni–Zn to other battery technologies, cycle life comparisons may vary depending on the discharge rate and depth of discharge used.

Advantages

Nickel–zinc cells have an open circuit voltage of 1.85 volts when fully charged,^[9] and a nominal voltage of 1.65 V. This makes Ni–Zn particularly suitable for electronic products that require the 1.5 V of alkaline primary cells rather than the 1.2 V of most rechargeable cells (most circuits tolerate the slightly higher voltage), and will not function correctly beyond, typically, the endpoint voltage of an alkaline cell. The output voltage of a 1.2 V rechargeable cell will drop to this point before it has fully delivered its charge.^{[citation needed]}

For use in multi-cell batteries, the higher voltage of Ni–Zn cells requires fewer cells than NiCd and NiMH for the same voltage. They have low internal impedance (typically 5 milliohms), which allows for high battery discharge rates, up to 50C. (C is battery capacity in Ah, divided by one hour.)^{[citation needed]}

Newer cells which are more powerful and have a life of up to 800 cycles can be an alternative to Li-ion batteries for electric vehicles.

Nickel–zinc batteries do not use mercury, lead, or cadmium, or metal hydrides, all of which can be difficult to recycle.^[10] Both nickel and zinc are commonly occurring elements in nature, and can be fully recycled. NiZn cells use no flammable active materials or organic electrolytes, and later designs use polymeric separators which reduce the dendrites problem.

Properly designed NiZn cells can have very high power density and good low-temperature discharging performance, and can be discharged to almost 100% and recharged without problems. As of 2017^[update] they were available in sizes up to F, and 50Ah/prismatic cell.

Zinc is a cheap and abundant metal, the 24th most abundant element in the Earth's crust, and is not dangerous to health. Common oxidation is +2, so charge and discharge move two electrons instead of one as in NiMH batteries.

Charging

Chargers for nickel–zinc batteries must be capable of charging a battery with a fully charged voltage of 1.85 V per cell, higher than the 1.4 V of NiMH. NiZn technology is well suited for fast recharge cycling, as optimum charge rates of C or C/2 are preferred.^[11]

Known charging regimes include a constant current of C or C/2 to cell voltage = 1.9 V. One manufacturer^[12] recommends charging at a constant current of C/4 to C until cell voltage reaches 1.9V, then continuing to charge at a constant voltage of 1.9V until charge current declines to C/40.

Maximum charge time was stated in 2009 to be about three hours.^[11] Once charged, continuous trickle charging is not recommended, as recombination is not provided for, and excess hydrogen will eventually vent, adversely affecting battery cycle life.^{[citation needed]} Some chargers for NiZn batteries state that they do not trickle charge after the battery is fully charged, but shut off.^[13]

Chemistry

(−) electrode: Zn + 4 OH⁻ ⇌ Zn(OH)₄²⁻ + 2e⁻ (E⁰ = −1.2 V/SHE )

Electrolyte: KOH

Zn(OH)₄²⁻ ⇌ Zn(OH)₂ + 2OH⁻

Zn(OH)₂ ⇌ ZnO + H₂O

(+) electrode: 2 NiO(OH) + 2 H₂O + 2 e⁻ ⇌ 2 Ni(OH)₂ + 2 OH⁻ (E⁰ = +0.50 V/SHE)

Overall reaction: Zn + 2 NiO(OH) + H₂O ⇌ ZnO + 2 Ni(OH)₂

Parasitic reaction: Zn + 2 H₂O → Zn(OH)₂ + H₂

References

^ ^a ^b ^c "Building A Better Battery", Kerry A. Dolan, Forbes.com, Forbes magazine, 11 May 2009, Retrieved 2011-02-12, Forbes-44.
^ "Famous Irish Chemists: James J. Drumm". Ul.ie. Archived from the original on 22 July 2012. Retrieved 1 July 2012.
^ ^a ^b David Linden (ed)., Handbook of Batteries, McGraw Hill, 2002, ISBN 0-07-135978-8, chapter 31.
^ Evercel financial statement 2007 Archived 7 March 2016 at the Wayback Machine, Evercel.com, page 9, Retrieved 23 November 2010.
^ Battery-meter-problem, NiZn discharge curves and camera voltage cutoffs, PentaxForums.com
^ ^a ^b "Nickel Zinc". EnerSys.com. EnerSys. Retrieved 13 July 2015.
^ Thomas, Justin (16 March 2012). "A Review of NiZn Batteries". MetaEfficient.com. inSync Theme. Retrieved 10 August 2020.
^ "A Brief History of Battery Developments", PowerGenix.com, 2010, Retrieved 12 February 2011. Archived 25 February 2011 at the Wayback Machine
^ [1] New NiZn batteries offer lightning-fast recycle
^ "Safety Data Sheet: Nickel Zinc Battery (Cell) Sizes: Sub-C and Prismatic". ZincFive. 24 May 2019. Retrieved 10 August 2020.
^ ^a ^b "PowerGenix NiZn Quick Charger". Powergenix.com. 2009. Archived from the original on 23 April 2016.
^ "Nickel-Zinc Charging Instructions". Zincfive. Retrieved 5 June 2019.
^ "UPStealth NEMA Battery Panel". ZincFive (formerly PowerGenix). 2017. Archived from the original on 2 February 2017.{{cite web}}: CS1 maint: unfit URL (link)

[PGen-1] "Building A Better Battery", Kerry A. Dolan, Forbes.com, Forbes magazine, 11 May 2009, Retrieved 2011-02-12, Forbes-44.

[2] "Famous Irish Chemists: James J. Drumm". Ul.ie. Archived from the original on 22 July 2012. Retrieved 1 July 2012.

[Linden2002-3] David Linden (ed)., Handbook of Batteries, McGraw Hill, 2002, ISBN 0-07-135978-8, chapter 31.

[4] Evercel financial statement 2007 Archived 7 March 2016 at the Wayback Machine, Evercel.com, page 9, Retrieved 23 November 2010.

[5] Battery-meter-problem, NiZn discharge curves and camera voltage cutoffs, PentaxForums.com

[EnerSys-6] "Nickel Zinc". EnerSys.com. EnerSys. Retrieved 13 July 2015.

[7] Thomas, Justin (16 March 2012). "A Review of NiZn Batteries". MetaEfficient.com. inSync Theme. Retrieved 10 August 2020.

[8] "A Brief History of Battery Developments", PowerGenix.com, 2010, Retrieved 12 February 2011. Archived 25 February 2011 at the Wayback Machine

[9] [1] New NiZn batteries offer lightning-fast recycle

[ZincFiveSDS-10] "Safety Data Sheet: Nickel Zinc Battery (Cell) Sizes: Sub-C and Prismatic". ZincFive. 24 May 2019. Retrieved 10 August 2020.

[PowerGenix-11] "PowerGenix NiZn Quick Charger". Powergenix.com. 2009. Archived from the original on 23 April 2016.

[12] "Nickel-Zinc Charging Instructions". Zincfive. Retrieved 5 June 2019.

[13] "UPStealth NEMA Battery Panel". ZincFive (formerly PowerGenix). 2017. Archived from the original on 2 February 2017.{{cite web}}: CS1 maint: unfit URL (link)

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@@ Line 1: / Line 1: @@
+{{Short description|Type of rechargeable battery}}
-{{Expert-portal|Energy|date=November 2008}}
+{{Use dmy dates|date=June 2021}}
+{{Infobox battery
+| image   = File:Akku NiZn AAA AA by NicoJenner.jpg
+| caption = Nickel–zinc cells in AA and AAA sizes
+| EtoW    = 100 [[Watt-hour|W·h]]/kg
+| EtoS    = 280 W·h/L
+| PtoW    = > 3000 W/[[kilogram|kg]]
+| CtoDE   =
+| SDR     =
+| CD      =
+| NomV    = 1.65 V
+| EtoCP   = 2–3[[Watt hour|Wh]]/US$}}
+A '''nickel–zinc battery''' ('''Ni–Zn battery''' or '''NiZn battery''') is a type of [[rechargeable battery]] similar to [[Nickel–cadmium battery|nickel–cadmium batteries]], but with a higher voltage of 1.6&nbsp;V.
-{| align=right
-| {{Batteries|EtoW=80 [[Watt-hour|W·h]]/kg|EtoS=250 W·h/L|PtoW=> 1700 W/[[kilogram|kg]]
-|CtoDE=|SDR=|CD=200-500|NomV=1.7 V|EtoCP=2-3[[Watt hour|Wh]]/[[USD|US$]]}}
-|}
-The '''nickel-zinc battery''' (sometimes abbreviated '''NiZn''') is a type of [[rechargeable battery]] commonly used in cordless power tools, cordless telephone, digital cameras, battery operated lawn and garden tools, professional photography, electric bike and light [[electric vehicle]] sectors.
-While nickel-zinc battery systems have been around for over 100 years, recent technological breakthroughs have made this technology viable and competitive with other commercially available rechargeable battery systems.
+Larger [[nickel]]–[[zinc]] battery systems have been known for over 100 years. Since 2000, development of a stabilized zinc [[electrode]] system has made this technology viable and competitive with other commercially available rechargeable battery systems. Unlike some other technologies, [[trickle charging]] is not recommended.<!--sourced in body-->
 == History ==
+In 1901 [[Thomas Alva Edison]] was awarded {{US patent|684204}} for a rechargeable nickel–zinc battery system.<ref name="PGen">
-Developed by an [[Irish people|Irish]] chemist, Dr. James J. Drumm (1897-1974)<ref>[http://www.ul.ie/~childsp/CinA/Issue46/fam_chem.html Famous Irish Chemists: James J. Drumm]</ref> and installed in four 2-car [[Railcar#Battery-electric|Drumm Railcar]] sets between 1932 and 1948 for use on the [[Harcourt Street railway line|Dublin-Bray]] line.  Although successful they were then withdrawn when the batteries wore out. Early nickel-zinc batteries were plagued by limited number of discharge cycles.
+   "Building A Better Battery", Kerry A. Dolan, Forbes.com,
+   ''[[Forbes]]'' magazine, 11 May 2009, Retrieved 2011-02-12,
+   [https://www.forbes.com/forbes/2009/0511/044-energy-clean-tech-building-better-battery.html Forbes-44].
+</ref>
+The battery was later developed by the Irish chemist [[James J. Drumm|Dr. James J. Drumm]] (1897–1974),<ref>{{cite web |url=http://www.ul.ie/~childsp/CinA/Issue46/fam_chem.html |title=Famous Irish Chemists: James J. Drumm |website=Ul.ie |access-date=2012-07-01 |archive-url=https://web.archive.org/web/20120722084845/http://www3.ul.ie/~childsp/CinA/Issue46/fam_chem.html |archive-date=22 July 2012 |url-status=dead }}</ref> and installed in four two-car [[Railcar#Battery-electric|Drumm railcar]] sets between 1932 and 1949 for use on the [[Harcourt Street railway line|Dublin–Bray]] railway line. Although successful, they were withdrawn when the batteries wore out. Early nickel–zinc batteries provided only a small number of discharge–recharge cycles. In the 1960s nickel–zinc batteries were investigated as an alternative to silver–zinc batteries for military applications, and in the 1970s were again of interest for electric vehicles.<ref name="Linden2002" /> ''Evercel Inc.'' developed and patented several improvements in nickel–zinc batteries, but withdrew from that area in 2004.<ref>[http://www.evercel.com/EvercelFinancialStatement.pdf Evercel financial statement 2007] {{Webarchive|url=https://web.archive.org/web/20160307055429/http://www.evercel.com/evercelfinancialstatement.pdf |date=7 March 2016 }}, Evercel.com, page 9, Retrieved 23 November 2010.</ref>
-[[Thomas Edison]] was awarded a U.S. Patent for a recharged Nickel Zinc battery system in 1901 (U.S. Patent 684, 204).
 == Applications ==
+Nickel–zinc batteries have a charge–discharge curve similar to 1.2&nbsp;V [[Nickel–cadmium battery|NiCd]] or [[Nickel–metal hydride battery|NiMH]] cells, but with a higher 1.6&nbsp;V nominal voltage.<ref>[http://www.pentaxforums.com/forums/pentax-dslr-discussion/45346-k200d-battery-meter-problem-2.html Battery-meter-problem], NiZn discharge curves and camera voltage cutoffs, PentaxForums.com</ref>
-Presently this battery technology has limited consumer availability with only AA cells offered for the digital camera market in some camera stores (Ritz Camera).  Nickel-zinc is considered as the next generation batteries used for high drain applications, and is expected to replace [[lead-acid batteries]] because of their higher energy to mass ratio and higher power to mass ratio (up to 75% lighter for the same power), and are relatively cheap compared to [[nickel-cadmium batteries]] (expected to be priced somewhere in between NiCd and lead-acids, but have twice the energy storing capacity). NiZn can now be considered the industrial substitute for nickel-cadmium.  The European Parliament has supported bans on cadmium based batteries and nickel-zinc offers the European power tool industry the most attractive alternative.
+Nickel–zinc batteries perform well in high-drain applications, and may have the potential to replace [[Lead–acid battery|lead–acid batteries]] because of their higher energy-to-mass ratio and higher power-to-mass ratio&nbsp;– as little as 25% of the mass for the same power.<ref name="EnerSys">{{cite web|title=Nickel Zinc|url=http://www.enersys.com/Nickel_Zinc.aspx|website=EnerSys.com|publisher=[[EnerSys]]|access-date=13 July 2015}}</ref> Nickel–zinc batteries are less expensive than [[Nickel–cadmium battery|nickel–cadmium batteries]]<ref name="EnerSys" /> and are expected to be priced somewhere between nickel–cadmium and lead–acid types. Nickel–zinc may be used as a substitute for nickel–cadmium. The European Parliament has supported bans on cadmium-based batteries;<ref name="PGen" /> nickel–zinc is a good alternative for power tools and other applications. A disadvantage is increased self-discharge rate after about 30–50 cycles, so that batteries do not hold their charge as long as when new. Where this is not a problem nickel–zinc is a good choice for applications requiring high power and high voltage.<ref>{{cite web |url=http://www.metaefficient.com/rechargeable-batteries/nizn-batteries.html |title=A Review of NiZn Batteries |website=MetaEfficient.com |publisher=inSync Theme |first=Justin |last=Thomas |date=16 March 2012 |access-date=10 August 2020}}</ref>
+== Battery life ==
-== Electrochemistry ==
+Compared with cadmium hydroxide, the tendency of the soluble zinc hydroxide ion ([[zincate]]) to dissolve into solution and not fully migrate back to the cathode during recharging has, in the past, presented challenges for the commercial viability of the nickel–zinc battery.<ref name="PGen" /><ref name="Linden2002">David Linden (ed)., ''Handbook of Batteries'', McGraw Hill, 2002, {{ISBN|0-07-135978-8}}, chapter 31.</ref> Another common issue with zinc rechargeable batteries is electrode shape change and [[Dendrite (crystal)|dendrites]] (or "[[Whisker (metallurgy)|whiskers]]"), which may reduce the cell discharging performance or, eventually, short out the cell, resulting in a low cycle life.
-Charge Reaction:   2Ni(OH)<sub>2</sub>(s) + Zn(OH)<sub>2</sub>(s) ↔ 2Ni(OH)<sub>3</sub>(s) + Zn(s)
+Recent advances have enabled this problem to be greatly reduced. These advances include improvements in electrode separator materials, inclusion of zinc material stabilizers, and electrolyte improvements (e.g. by using [[phosphate]]s). [[PowerGenix]] has developed 1.6&nbsp;V batteries with claimed battery cycle life comparable to NiCd batteries.<ref>[http://www.powergenix.com/?q=battery-technology-history "A Brief History of Battery Developments"], PowerGenix.com, 2010, Retrieved 12 February 2011. {{Webarchive|url=https://web.archive.org/web/20110225142342/http://www.powergenix.com/?q=battery-technology-history |date=25 February 2011 }}</ref>
-Note that the stoichiometry above is different than below, but the reactions are identical.  Technically, water is consumed and generated on the charge and discharge cycles.
+Battery cycle life is most commonly specified at a discharge depth of 80 percent of rated capacity and assuming a one-hour discharge current rate. As the discharge current or the depth of discharge is reduced, the number of charge-discharge cycles for a battery increases. When comparing Ni–Zn to other battery technologies, cycle life comparisons may vary depending on the discharge rate and depth of discharge used.
-Discharge Reaction: H<sub>2</sub>O + Zn + 2NiOOH ↔ ZnO +2Ni(OH)<sub>2</sub>
+== Advantages ==
-Electrochemical open circuit voltage potential: ~1.73V
+Nickel–zinc cells have an open circuit voltage of 1.85 volts when fully charged,<ref>[http://strobist.blogspot.com/2010/01/new-nizn-batteries-offer-lightning-fast.html] New NiZn batteries offer lightning-fast recycle</ref> and a nominal voltage of 1.65&nbsp;V. This makes Ni–Zn particularly suitable for electronic products that require the 1.5&nbsp;V of alkaline primary cells rather than the 1.2&nbsp;V of most rechargeable cells (most circuits tolerate the slightly higher voltage), and will not function correctly beyond, typically, the endpoint voltage of an alkaline cell. The output voltage of a 1.2&nbsp;V rechargeable cell will drop to this point before it has fully delivered its charge.{{citation needed|reason=I do not dispute this, and my experience seems to support it, but it needs reliable sources|date=October 2017}}
+For use in multi-cell batteries, the higher voltage of Ni–Zn cells requires fewer cells than NiCd and NiMH for the same voltage. They have low internal [[Electrical impedance|impedance]] (typically 5 [[milliohm]]s), which allows for high battery discharge rates, up to 50''C''. (''C'' is battery capacity in Ah, divided by one hour.){{citation needed|date=January 2015}}
-== Technological Advantage ==
+Newer cells which are more powerful and have a life of up to 800 cycles can be an alternative to Li-ion batteries for electric vehicles.
-Higher performances than other alkaline batteries.
+Nickel–zinc batteries do not use mercury, lead, or cadmium, or [[metal hydride]]s, all of which can be difficult to recycle.<ref name=ZincFiveSDS>{{cite web |url= https://www.zincfive.com/subc-prismatic-material-safety-data-sheet |title= Safety Data Sheet: Nickel Zinc Battery (Cell) Sizes: Sub-C and Prismatic |work= [[ZincFive]] |date= 24 May 2019 |access-date= 10 August 2020}}</ref> Both nickel and zinc are commonly occurring elements in nature, and can be fully recycled. NiZn cells use no flammable active materials or organic electrolytes, and later designs use polymeric separators which reduce the dendrites problem.
-No use of heavy metals (mercury, lead or cadmium).
+Properly designed NiZn cells can have very high power density and good low-temperature discharging performance, and can be discharged to almost 100% and recharged without problems. {{As of|2017}} they were available in sizes up to F, and 50Ah/prismatic cell.
-No use of metal hydrides (rare earth metals) that are difficult to recycle.
+Zinc is a cheap and abundant metal, the 24th most abundant element in the Earth's crust, and is not dangerous to health.
-No flammable active material or organic electrolyte.
+Common oxidation is +2, so charge and discharge move two electrons instead of one as in NiMH batteries.
+==Charging==
-Simple recycling process, similar to the one in use for primary alkaline batteries.  Zinc and nickel can be fully recycled.
+Chargers for nickel–zinc batteries must be capable of charging a battery with a fully charged voltage of 1.85&nbsp;V per cell, higher than the 1.4&nbsp;V of NiMH. NiZn technology is well suited for fast recharge cycling, as optimum charge rates of [[battery charger#C-rate|C]] or C/2 are preferred.<ref name="PowerGenix"/>
+Known charging regimes include a constant current of C or C/2 to cell voltage = 1.9&nbsp;V. One manufacturer<ref>{{cite web |title=Nickel-Zinc Charging Instructions |url=https://www.zincfive.com/charging |website=Zincfive |access-date=5 June 2019}}</ref> recommends charging at a constant current of C/4 to C until cell voltage reaches 1.9V, then continuing to charge at a constant voltage of 1.9V until charge current declines to C/40.
-.6V cell voltage vs. 1.2V for NiCd and NiMH rechargeable cells.
+Maximum charge time was stated in 2009 to be about three hours.<ref name="PowerGenix">{{cite web |url=http://www.powergenix.com/?q=products/nizn-quick-charger |title=PowerGenix NiZn Quick Charger |website=Powergenix.com |date=2009 |archive-date=23 April 2016 |archive-url=https://web.archive.org/web/20160423172044/http://powergenix.com/?q=products%2Fnizn-quick-charger |url-status=dead }}</ref> Once charged, continuous trickle charging is not recommended, as recombination is not provided for, and excess [[hydrogen]] will eventually vent, adversely affecting battery cycle life.{{Citation needed|date=January 2017}} Some chargers for NiZn batteries state that they do not trickle charge after the battery is fully charged, but shut off.<ref>{{cite web |url=http://www.zincfive.com/upstealth-nema-battery-panel/|url-status=unfit|archive-url=https://web.archive.org/web/20170202030815/http://www.zincfive.com/upstealth-nema-battery-panel/|archive-date=2 February 2017|title=UPStealth NEMA Battery Panel|year=2017|website=ZincFive (formerly PowerGenix)}}</ref>
-Fewer cells required (compared to NiCd and NiMH)to achieve battery pack voltage reducing pack weight, size and improving pack reliability.
+==Chemistry==
-Both [[nickel]] and [[zinc]] are commonly occurring elements in nature and are not hazardous.
+:(−) electrode: 		 Zn + 4 OH<sup>−</sup> {{eqm}} Zn(OH)<sub>4</sub><sup>2−</sup> + 2e<sup>−</sup> (E<sup>0</sup> = −1.2 V/SHE )
-Nickel-zinc batteries when used with aqueous electrolytes may provide a "green" battery.
+:Electrolyte: KOH
+::Zn(OH)<sub>4</sub><sup>2−</sup> {{eqm}} Zn(OH)<sub>2</sub> + 2OH<sup>−</sup>
+::Zn(OH)<sub>2</sub> {{eqm}} ZnO + H<sub>2</sub>O
+:(+) electrode: 	      2 NiO(OH) + 2 H<sub>2</sub>O + 2 e<sup>−</sup> {{eqm}}  2 Ni(OH)<sub>2</sub> + 2 OH<sup>−</sup> (E<sup>0</sup> = +0.50 V/SHE)
+:'''Overall reaction: 	   Zn + 2 NiO(OH) + H<sub>2</sub>O  {{eqm}} ZnO + 2 Ni(OH)<sub>2</sub>'''
+:Parasitic reaction: 	  Zn + 2 H<sub>2</sub>O → Zn(OH)<sub>2</sub> + H<sub>2</sub>
+==See also==
+* [[Comparison of battery types]]
+* [[List of battery sizes]]
+* [[List of battery types]]
+* [[Nickel–cadmium battery]]
+* [[Zinc–air battery]]
 ==References==
+{{Reflist|30em}}
-<references />
+{{Galvanic cells}}
-== External links ==
-*[http://www.powergenix.com/technology2.htm Powergenix] - Developer and Manufacturer of nickel zinc batteries
-*[http://www.scps-group.com] - SCPS - Developer of industrial NiZn batteries
-*[http://www.xellerion.com] - Branch of Evionyx who has all infos on NiZn battery
-*[http://www.evionyx.com eVionyx] - Developer and manufacturer of "flooded" prismatic NiZN battery
-*[http://www.alibaba.com/catalog/11420911/eVionyx_NiZn_Battery_Xell_18.html eVionyx Taiwan] - Taiwan manufacturer of eVionyx products
+{{DEFAULTSORT:Nickel-zinc battery}}
+[[Category:Nickel]]
 [[Category:Rechargeable batteries]]
+[[Category:Zinc]]
-[[fr:Accumulateur nickel-zinc]]
-[[ru:Никель-цинковый аккумулятор]]

v t e Electrochemical cells
Types	Galvanic cell Concentration cell Electric battery Flow battery Trough battery Fuel cell Thermogalvanic cell Voltaic pile
Primary cell (non-rechargeable)	Alkaline Aluminium–air Bunsen Chromic acid Clark Daniell Dry Edison–Lalande Grove Leclanché Lithium metal Lithium organic Lithium–air Mercury Metal–air electrochemical Nickel oxyhydroxide Silicon–air Silver oxide Weston Zamboni Zinc–air Zinc–carbon
Secondary cell (rechargeable)	Automotive Lead–acid gel–VRLA Lithium–air Lithium ion Dual carbon Lithium–iron–phosphate Lithium–polymer Lithium–sulfur Lithium–titanate Metal–air Molten salt Nanopore Nanowire Nickel–cadmium Nickel–hydrogen Nickel–iron Nickel–lithium Nickel–metal hydride Nickel–zinc Polysulfide–bromide Potassium ion Rechargeable alkaline Silver–cadmium Silver–zinc Sodium ion Sodium–sulfur Solid state Vanadium redox Zinc–bromine Zinc–cerium
Other cell	Atomic battery Fuel cell Solar cell
Cell parts	Anode Binder Catalyst Cathode Electrode Electrolyte Half-cell Ions Salt bridge Semipermeable membrane