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An atom is classified
chemically by the number of protons in its nucleus. Atoms that have the same
number of protons in their nuclei have the same chemical behavior. Atoms that
have the same number of protons are grouped together and constitute a chemical
element. At one time chemists used
various symbols, similar to shorthand, for the atoms of the different elements.
These symbols were very cumbersome and were replaced by abbreviations of the
names of the elements. Each element has been assigned a specific one or two
letter symbol based on the first letter of its chemical name. Because there are
several elements with the same first letter, it is often necessary to add the
second letter to the symbol. In some cases the symbol comes from an
abbreviation for the old latin name of the element. For example, Fe stands for
iron (ferrum) and Cu for copper (cuprum). The first letter of the chemical
symbol is always capitalized. If the symbol has two letters, the second letter
is always lowercase. Atomic Number The number of protons in
the nucleus plays such an important role in identifying the atom that it is
given a special name, the atomic
number. The symbol Z is often used for
atomic number (or number of protons). Hydrogen has an atomic number of 1 and
lawrencium has an atomic number of 103. The atomic number is also equal to the
number of electrons. Atomic Mass Number The sum of the total
number of protons, Z, and the total number of neutrons, N, is called the atomic mass number. The symbol is A. Not all atoms of the same element
have the same atomic mass number, because, although the Z is the same, the N
and thus the A are different. Atoms of the same element with different atomic
mass numbers are called isotopes. <%CUT%> Atomic Weight In Table 1, the masses of
atomic particles are given in atomic mass units (amu). These units represent a
relative scale in which the mass of the isotope carbon-12 is used as the
standard and all others are related to it. Specifically, 1 amu is defined as
1/12 the mass of the carbon-12 atom. Since the mass of a proton or a neutron is
approximately 1 amu, the mass of a particular atom will be approximately equal
to its atomic mass number, Z. The atomic weight of an
element is generally more useful than isotopic masses. The atomic weight of an element is defined as the weighted average of the masses of all of
its natural occurring isotopes. The atomic weight of the elements are listed in
Table 2. The elements that have their atomic weights in parentheses are
unstable. For these elements, the atomic weight of the longest living isotope
is used rather than the average of the masses of all occurring isotopes.
Molecules Molecules are groups or clusters of atoms held together by means of chemical bonding. There are two types of molecule; molecules of an element and molecules of a compound.
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