Question: what is the number of elements that make up most of the human body?
About the article "Biochemistry", section "Starting materials: the chemical elements of life".

Candidate passages:
Book 1 is made up of six theses which give a general description of medicine in general, the cosmic elements that make up the cosmos and the human body, the mutual interaction of elements (temperaments), fluids of the body (humours), human anatomy, and physiology. 
Around two dozen of the 92 naturally occurring chemical elements are essential to various kinds of biological life.
Most rare elements on Earth are not needed by life (exceptions being selenium and iodine), while a few common ones (aluminum and titanium) are not used.
Most organisms share element needs, but there are a few differences between plants and animals.
For example ocean algae use bromine but land plants and animals seem to need none.
All animals require sodium, but some plants do not.
Plants need boron and silicon, but animals may not (or may need ultra-small amounts).
Just six elements—carbon, hydrogen, nitrogen, oxygen, calcium, and phosphorus—make up almost 99% of the mass of a human body (see composition of the human body for a complete list).
In addition to the six major elements that compose most of the human body, humans require smaller amounts of possibly 18 more.
In human.
In the first human genome draft the fraction of LINE elements of the human genome was given as 21% and their copy number as 850,000.
The non-autonomous SINE elements which depend on L1 elements for their proliferation make up 13% of the human genome and have a copy number of around 1.5 million. 
Body percussion is used extensively in music education, because of its accessibility—the human body is the original musical instrument and the only instrument that every student possesses.
Using the body in this manner gives students a direct experience of musical elements, such as beat, rhythm, and metre and helps a student internalise rhythmic skills.
Certain approaches to music education, including Orff, Kodály and Bapne make particular use of body percussion. 
The following graph (note log scale) shows the abundance of elements in our solar system.
The table shows the twelve most common elements in our galaxy (estimated spectroscopically), as measured in parts per million, by mass.
Nearby galaxies that have evolved along similar lines have a corresponding enrichment of elements heavier than hydrogen and helium.
The more distant galaxies are being viewed as they appeared in the past, so their abundances of elements appear closer to the primordial mixture.
As physical laws and processes appear common throughout the visible universe, however, scientist expect that these galaxies evolved elements in similar abundance.
The abundance of elements in the Solar System is in keeping with their origin from nucleosynthesis in the Big Bang and a number of progenitor supernova stars.
Very abundant hydrogen and helium are products of the Big Bang, but the next three elements are rare since they had little time to form in the Big Bang and are not made in stars (they are, however, produced in small quantities by the breakup of heavier elements in interstellar dust, as a result of impact by cosmic rays).
Beginning with carbon, elements are produced in stars by buildup from alpha particles (helium nuclei), resulting in an alternatingly larger abundance of elements with even atomic numbers (these are also more stable).
In general, such elements up to iron are made in large stars in the process of becoming supernovas.
Iron-56 is particularly common, since it is the most stable element that can easily be made from alpha particles (being a product of decay of radioactive nickel-56, ultimately made from 14 helium nuclei).
Elements heavier than iron are made in energy-absorbing processes in large stars, and their abundance in the universe (and on Earth) generally decreases with their atomic number.
The abundance of the chemical elements on Earth varies from air to crust to ocean, and in various types of life.
The abundance of elements in Earth's crust differs from that in the universe (and also in the Sun and heavy planets like Jupiter) mainly in selective loss of the very lightest elements (hydrogen and helium) and also volatile neon, carbon, nitrogen and sulfur, as a result of solar heating in the early formation of the solar system.
Aluminum is also far more common in the Earth and Earth's crust than in the universe and solar system, but the composition of Earth's mantle (which has more magnesium and iron in place of aluminum) more closely mirrors that of the universe, save for the noted loss of volatile elements.
The composition of the human body, by contrast, more closely follows the composition of seawater—save that the human body has additional stores of carbon and nitrogen necessary to form the proteins and nucleic acids characteristic of living organisms.
Certain kinds of organisms require particular additional elements, for example the magnesium in chlorophyll in green plants, the calcium in mollusc shells, or the iron in the hemoglobin in vertebrate animals' red blood cells.