Explanation:
Chemical compound, any substance composed of identical molecules consisting of atoms of two or more chemical elements. ... The fundamental principle of the science of chemistry is that the atoms of different elements can combine with one another to form chemical compounds.
The Mohs scale is for natural minerals<span>. For manufactured products other measures of hardness are better. ... There are ten </span>minerals<span> in Mohs scale, talc, gypsum, calcite, fluorite, apatite, orthoclase, quartz, topaz, corundum, and for last and</span>hardest<span>, diamond.
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The net ionic equation of the reaction is:
- Pb²⁺ (aq) +2 I⁻ (aq) → PbI2(s)
<h3>What are net ionic equations?</h3>
Net ionic equations are equations where ions which remain in solution known as spectator ions are not shown in the equation. Only ions involved in formation of product are shown.
In the given equation, sodium and nitrate ions are spectator ions.
The net ionic equation of the given reaction is as follows:
- Pb²⁺ (aq) +2 I⁻ (aq) → PbI2(s)
In conclusion, spectator ions are not shown in net ionic equation.
Learn more about net ionic equations at: brainly.com/question/19705645
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The Bohr model was a one-dimensional model that used one quantum number to describe the distribution of electrons in the atom. The only information that was important was the size of the orbit, which was described by the n quantum number. Schr�dinger's model allowed the electron to occupy three-dimensional space. It therefore required three coordinates, or three quantum numbers, to describe the orbitals in which electrons can be found.
The three coordinates that come from Schr�dinger's wave equations are the principal (n), angular (l), and magnetic (m) quantum numbers. These quantum numbers describe the size, shape, and orientation in space of the orbitals on an atom.
The principal quantum number (n) describes the size of the orbital. Orbitals for which n = 2 are larger than those for which n = 1, for example. Because they have opposite electrical charges, electrons are attracted to the nucleus of the atom. Energy must therefore be absorbed to excite an electron from an orbital in which the electron is close to the nucleus (n = 1) into an orbital in which it is further from the nucleus (n = 2). The principal quantum number therefore indirectly describes the energy of an orbital.
The angular quantum number (l) describes the shape of the orbital. Orbitals have shapes that are best described as spherical (l = 0), polar (l = 1), or cloverleaf (l = 2). They can even take on more complex shapes as the value of the angular quantum number becomes larger.
