is this right about atoms?
923045
True.  Elements are characterized by the nature of their atoms; each atom has a positively charged nucleus and is surrounded by a cloud of electrons.  All atoms of a particular element have the same nuclear charge.  Under normal circumstances, atoms are in a low energy state (the "ground state") in which the shape of the electron orbitals is roughly spherical -- bearing in mind that we're talking about the shape of a fog, without definite edges.  In higher energy states, the electron orbitals can get arbitrarily large.
750008
Yes it is correct.\n\nYou can always move a term from one side of the equation to the other side of the equation as long as you change its sign. This is called transposition.
933142
Yep, all you have to do is to make sure that the atoms shown in the left hand part of the equation appear on the left hand side.  Nothing is created or lost, you just make new compounds.  Dead easy, if only languages were so easy!!!
254116
"mathematician" is correct.\n\nAny atom of a given element will have the same number of protons in its nucleus.  If the atom is neutral (i.e. has no charge), then it will have the same number of electrons as protons.\nHowever, the number of neutrons in the nucleus can vary slightly from atom to atom for a given element.  Atoms of the same element but with different numbers of neutrons in their nucleus are called isotopes.  With a greater/less number of neutrons, the over all atomic weight of the atom will varry.  By taking into account the naturally occuring percentages of each of these isotopes of a given element, we can obtain the average atomic mass of all the atoms of that element.\n\nCommon isotopes you might hear would be, "Carbon-12" or "Carbon-14", these are two different isotopes of the element Carbon.  The -# after the element name indicates the total atomic mass of the atom.  Since we know that Carbon always has 6 protons, we can easily determine the number of neutrons if we know the atomic mass.
916732
Is relative to the amount of energy and object contains.
789494
Basic Atomic Structure\n\nThe definitions of atoms and elements seems, at first glance, almost circular: an element is a substance made up of only one kind of atom, and an atom is the smallest particle of an element that retains all the chemical and physical properties of the element. In fact, these two definitions do not form a closed loop, as they would if it were stated that an element is something made up of atoms. Every item of matter that exists, except for the subatomic particles discussed in this essay, is made up of atoms. An element, on the other hand, is—as stated in its definition—made up of only one kind of atom. "Kind of atom" in this context refers to the number of protons in its nucleus.\n\nProtons are one of three basic subatomic particles, the other two being electrons and neutrons. As we shall see, there appear to be particles even smaller than these, but before approaching these "sub-subatomic" particles, it is necessary to address the three most significant components of an atom. These are distinguished from one another in terms of electric charge: protons are positively charged, electrons are negative in charge, and neutrons have no electrical charge. As with the north and south poles of magnets, positive and negative charges attract one another, whereas like charges repel. Atoms have no net charge, meaning that the protons and electrons cancel out one another.
705654
i dont see anything wrong the way u solved it(mathematically).if there was any condition or state is mentioned about that thing in time or wrt time then u have to reconsider the problem.
282194
In the early 20th century it was thought that electrons revolved around the nucleus in an atom very much like the way planets revolve around the sun in the solar system.  This led to some speculation that maybe atoms really were tiny solar systems (with teeny tiny people -- see the sf novel "The Girl in the Golden Atom" by Ray Cummings, 1923).  But the more detailed understanding of atoms that came about with quantum mechanics makes it clear that an atom is nothing like a solar system, and that electrons don't even have surfaces, let alone surfaces with teeny tiny people on them.
180604
No, the human body is a very large collection of atoms, the cells are made up of all sorts of things taht each could be divided into smaller things and that on the other hand maybe can bedivided into smaller things until you find that all that is left is atoms.
410056
ATOM..basic building block\n \n[Gr.,=uncuttable (indivisible)], basic unit of matter; more properly, the smallest unit of a chemical element having the properties of that element.  That is the definition.  Continue to read further; it really gives great detail!!!!!\n\nStructure of the Atom\n\nThe atom consists of a central, positively charged core, the nucleus, and negatively charged particles called electrons that are found in orbits around the nucleus.\n\nThe Nucleus\n\nAlmost the entire mass of the atom is concentrated in the nucleus, which occupies only a tiny fraction of the atom's volume. The nucleus of an atom consists of neutrons and protons, the neutron being an uncharged particle and the proton a positively charged one. Their masses are almost equal. Atoms containing the same number of protons but different numbers of neutrons represent different forms, or isotopes, of the same element.\n\nThe Electrons\n\nSurrounding the nucleus of an atom are its electrons; for a neutral atom, the number of electrons is equal to the atomic number. The outermost electrons of an atom determine its chemical and electrical properties. An atom may combine chemically with another atom in various ways, either by giving up or receiving electrons, thus setting up an electrical attraction between the atoms (see ion), or by sharing one or more pairs of electrons (see chemical bond). Because metals have few outermost electrons and tend to give them up easily, they are good conductors of electricity or heat (see conduction).\n\nThe electrons are often described as revolving about the nucleus as the planets revolve about the sun. This picture, however, is misleading. The quantum theory has shown that all particles in motion also have certain wave properties. For a particle the size of an electron, these properties are of considerable importance. As a result the electrons in an atom cannot be pictured as localized in space, but rather should be viewed as smeared out over the entire orbit so that they form a cloud of charge. The electron clouds around the nucleus represent regions in which the electrons are most likely to be found. The shapes of these clouds can be very complex, in marked contrast to the simple elliptical orbits of planets. Surprisingly, the sizes of all atoms are comparable, in spite of the large differences in the number of electrons they contain.\n\nAtomic Weight and Number\n\nThe atomic number of an atom is simply the number of protons in its nucleus. The atomic weight of an atom is given in most cases by the mass number of the atom, equal to the total number of protons and neutrons combined. An atom may be conveniently symbolized by its chemical symbol with the atomic number and mass number written as subscript and superscript, respectively. For example, the symbol for uranium is U (atomic number 92); the isotopes of uranium with atomic weights 235 and 238 are indicated by 23592U and 23892U.\n\nDevelopment of Atomic Theory\n\nEarly Atomic Theory\n\nThe atomic theory, which holds that matter is composed of tiny, indivisible particles in constant motion, was proposed in the 5th cent. by the Greek philosophers Leucippus and Democritus and was adopted by the Roman Lucretius. However, Aristotle did not accept the theory, and it was ignored for many centuries. Interest in the atomic theory was revived during the 18th cent. following work on the nature and behavior of gases (see gas laws).\n\nFrom Dalton to the Periodic Table\n\nModern atomic theory begins with the work of John Dalton, published in 1808. He held that all the atoms of an element are of exactly the same size and weight (see atomic weight) and are in these two respects unlike the atoms of any other element. He stated that atoms of the elements unite chemically in simple numerical ratios to form compounds. The best evidence for his theory was the experimentally verified law of simple multiple proportions, which gives a relation between the weights of two elements th
360394
A more generic term for the components of an atom is "sub-atomic particles."  I think that's the answer you're looking for.
373061
yes. in order for an atom to be stable, it must have eight valence electrons. In other words, each atom wants to have eight valence electrons. On the periodic table, you can determine what element can form a bond with any other elements. There are some elements which are an exception to the eight valence rule.
897762
Element talks about the chemical identity.  How one atom is not like another.\nAtom talks about the particular entities.\n\nElement is a general term while atom is a specific term.\nSo you can speack of the element so and so and be describing the substance and its properties for example as that element is in all the universe.
73838
Its' probably a rounding error. It would depend on which masses for the elements you use, how precise you want to be.
914809
Not for an atom but it is for an electron.
399707
Atoms consist of protons and neutrons in a nucleus, with electrons in shells round it. \nIn an uncharged/neutral atom, the number of protons and electrons are equal and this is the same as the atomic number. In the periodic table, the elements are arranged in order of increasing atomic number. \nA molecule is two or more atoms chemically bonded together.\ne.g. Ne is an atom and H20 is a molecule.
693223
Yes an atom is the same as an element.  A single atom is the smallest particle of an element.  There are 118 different elements in the periodic table. For example, a Hydrogen atom is one proton and one electron.  The next element in the periodic table is Helium, it has one proton, one neutron and one electron.  Each of these atom examples represent their own element.  So you see a single atom does represent it's own particular element, as discussed in the Hydrogen and Helium examples.