Rounding out the year with nickel and zinc
To complete our celebration of the 150th anniversary of Dmitri Mendeleev’s periodic table, we look at nickel and zinc, two metallic elements with chemical symbols Ni and Zn and atomic numbers 28 and 30, respectively.
This ribbon diagram shows the 3D structure of the enzyme urease in coordination with two nickel ions depicted in green.E. Jabri et al/Wikimedia Commons
Nickel can exist in oxidation states ranging from -2 to +4. The most abundant — Ni+2 — combines with common anions such as sulfate, sulfide, carbonate, nitrate and hydroxide. In contrast, zinc predominates in the oxidation +2 almost exclusively, acting as a strong reducing agent. Zinc forms binary compounds with most nonmetal and metalloid elements with the exception of noble gases.
Nickel is produced with iron in the final stages of nuclear reactions during violent explosions deep inside supergiant stars. As a result, these two elements are mixed abundantly in the interior of meteorites. The astrophysical origin of zinc is not entirely understood, but it might have involved the asymmetric explosion of the universe’s earliest supernova.
Nickel makes up only 0.008% of the Earth’s crust and occurs often as an alloy with iron in the planet’s core. It also exists in minerals in combination with sulfur and arsenic. Zinc is the 24th most common element in the Earth’s crust, where it is found primarily as zinc sulfide and as a binary alloy with metals including aluminum, gold, iron, lead, silver and nickel. Mineral weathering disperses small amounts of zinc into soil, seawater and the atmosphere.
Both nickel and zinc are essential for life and are present in many organisms. Nickel is recognized and transported into the cell by a variety of mechanisms: nonspecific influx across membrane proteins in bacteria and yeast, high-affinity uptake via transporters and permeases in certain bacteria, and incorporation through channels that preferentially carry other divalent cations — such as magnesium and calcium — in fungi and humans. Inside cells, nickel is inserted into the active site of many enzymes such as hydrogenase, nickel superoxide dismutase, carbon monoxide dehydrogenase, cis-trans isomerase and urease. Toxic excess intracellular free nickel is neutralized by binding to negatively charged molecules such as polyphosphate and sequestration of nickel-containing complexes into vacuoles.
The nickel-containing protein urease is important in the pathophysiology of liver cirrhosis, peptic ulcers and urinary stones. Urease is produced by bacteria that infect the gastrointestinal and urinary tracts, including Helicobacter pylori and Proteus mirabilis. It breaks down urea and produces ammonia, which increases the pH of the surrounding environment from neutral to basic and becomes toxic in the liver, the stomach lining, the kidneys and the blood stream.
Cells transport, use and sequester zinc much as they do other divalent metals. Photosynthetic bacteria of the genus Acidiphilium contain a purple chlorophyll pigment that uses zinc as cofactor instead of the more common magnesium. Zinc-dependent phospholipases C in Clostridia, Bacillus or Listeria species may contribute to toxicity by breaking down host cell membranes. The coordination of one or more zinc ions by particular amino acids forms a zinc-finger motif that stabilizes the 3D structure of many proteins that bind DNA, such as nucleases and transcription factors.
A year of (bio)chemical elements
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