Toxic atoms,radioactive atoms,isotopes, subatomics what is a normal atom or particle?
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Toxic atoms are just elements that have properties that are bad for life.\n\nRadioactive atoms are unstable, which means they fall apart all by themselves into smaller pieces. Usually a radioactive atom will throw off one or more neutrons to become the next lower element or isotope on the periodic table.\n\nAn isotope is an element that has a different number of neutrons in it's nucleus. For example, most carbon atoms have 6 protons and 6 neutrons in the nucleus.  That is a total of 12 particles so it is called carbon 12. Carbon 14 has two extra neutrons, or 6 protons and 8 neutrons. Because the number of electrons is always the same as the number of protons, and because chemistry is all based on electron interactions, both types of carbon behave the same chemically.\n\nA subatomic particle is a particle smaller than one atom. Atoms were once thought to be the smallest possible particle of matter, but we now know that they are made up of collections of various numbers of smaller particles called protons, neutrons and electrons.\n\nA "normal" atom would probably be the most stable isotope. For example carbon 14 is radioactive and changes into carbon 12 if given enough time, so carbon 12 might be considered more "normal". But I think the term "normal" is not clear and has no real meaning in this case. Certainly many naturally occurring elements are toxic, or radioactive or both.
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atomic number represents the number of protons or electrons in an atom
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there are innumerable protons and neutrons in universe. generally protons and neutrons are in an atom.
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A more generic term for the components of an atom is "sub-atomic particles."  I think that's the answer you're looking for.
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Atoms are most stable at certain energy levels.  If an atom goes above a particular level, it will release energy to go back.  Most of the time, this occurs as electromagnetic radiation, where an electron drops to a lower shell and releases heat (infrared light), light, or more energetic radiation (like x-rays).\n\nIn the case of radioactive decay or nuclear fission, the released radiation is in the form of nuclear particles: alpha particles are helium nuclei (no electrons) and have low energy, and beta particles are electrons, which are higher energy.  Gamma rays are electromeagnetic, not particulate, so they are just photons, and have very high energy.
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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
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chemically: electrons\n\nphysically: nucleons and/or protons (alpha, beta or gamma ray for nuclear elements)
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The most fundamental particles known to exist at the moment are quarks and leptons. Quarks are the things the make up the pieces of the nucleus in an atom and leptons include things like electrons.\n\nWithin a nucleus you will have heard of Protons and Neutrons ro collectively Nucleons. Well a quark is a sub unit of one of these so called "Nucleons". There are three quarks to every nucleon. There are many types of quark and these create many types of particles, most of which are extremely shortlived. You can learn more about the world of Particle Physics in the Particle Physics Adventure.\n\nhttp://particleadventure.org/particleadventure/
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It means an element in which its atoms emit electromagnetig waves and particles Without the use of any medium. normaly radoiactive is liked to harm but since all radioactive material has harmfull efects to living organisims then it is true to link radioactivity with harm.
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I think you mean at the atomic level, but still the answer is no.\n\nOne counter example would be positronium. This is when an electron and its anti particle, a positron, "revolve" around each other.  This is very unstable with a half-life of about 10^-7 seconds. \n\nThere are other exotic atoms of this type. Any atom formed by a particle and its anti particle is called an onia.
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1)electron ...(also negative meson)\n2)the atom is the basic (many atoms make molecule and so on)\n3)polymer (the most famous are protiens)
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A substance whose atoms all have the same number of protons. Neutron numbers may vary (these are called "isotopes"). In a neutral (non-charged) atom, the number of electrons equals the number of protons.
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According to the standard model (which has proven correct MANY times) atoms are made up of neutrons and protons and are circled by electrons in their basic form. Neutrons and protons are both baryons (which are types of hadrons) and are composed of quarks. Quarks are fundamental particles (not composite) just like the electron. They are known as point particles as well.\n\nTheories are that these point particles are in fact strings (string theory) oscillating at different frequencies etc, but that is still disputed.
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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.
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Alpha, beta and gamma radiation is radioactive radiation. It is cause by unstable atoms "decaying" to become stable atoms. Alpha and beta partciles are Protons and Electrons respectively whilst gamma radiation is very very high frequency "electromagnetic radiation." \nNon radioactive radiation is sound, heat, light..
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electron\nThe electron is a lightweight fundamental subatomic particle that carries a negative electric charge. The electron is a spin-1/2 lepton, does not participate in strong interactions and has no substructure. Together with atomic nuclei, electrons make up atoms; they are responsible for chemical bonding. The flow of electricity in solid conductors is primarily due to the movement of electrons.\nhttp://en.wikipedia.org/wiki/Electron\n\nThe electron, denoted  is a fundamental particle with negative electric charge that is found arranged in quantum mechanical orbits about neutral atoms. The electron is a lepton, and therefore has lepton number 1. The antiparticle of the electron is called the positron. \n\nThe electron mass is  kg, and the electron charge , where  \nhttp://scienceworld.wolfram.com/physics/Electron.html
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CHEMISTRY I: ATOMS AND MOLECULES\nTable of Contents\nAtoms | Electrons and energy | Chemical Bonding | Chemical reactions and molecules\n\nLearning Objectives | Terms | Review Questions | Links\nAtoms | Back to Top\n\nMost of the Universe consists of matter and energy. Energy is the capacity to do work. Matter has mass and occupies space. All matter is composed of basic elements that cannot be broken down to substances with different chemical or physical properties. Elements are substances consisting of one type of atom, for example Carbon atoms make up diamond, and also graphite. Pure (24K) gold is composed of only one type of atom, gold atoms. Atoms are the smallest particle into which an element can be divided. The ancient Greek philosophers developed the concept of the atom, although they considered it the fundamental particle that could not be broken down. Since the work of Enrico Fermi and his colleagues, we now know that the atom is divisible, often releasing tremendous energies as in nuclear explosions or (in a controlled fashion in) thermonuclear power plants.\n\nSubatomic particles were discovered during the 1800s. For our purposes we will concentrate only on three of them. The proton is located in the center (or nucleus) of an atom, each atom has at least one proton. Protons have a charge of +1, and a mass of approximately 1 atomic mass unit (amu). Elements differ from each other in the number of protons they have, e.g. Hydrogen has 1 proton; Helium has 2.\n\nThe neutron also is located in the atomic nucleus (except in Hydrogen). The neutron has no charge, and a mass of slightly over 1 amu. Some scientists propose the neutron is made up of a proton and electron-like particle.\n\nThe electron is a very small particle located outside the nucleus. Because they move at speeds near the speed of light the precise location of electrons is hard to pin down. Electrons occupy orbitals, or areas where they have a high statistical probability of occurring. The charge on an electron is -1. Its mass is negligible (approximately 1800 electrons are needed to equal the mass of one proton).\n\nThe atomic number is the number of protons an atom has. It is characteristic and unique for each element. The atomic mass (also referred to as the atomic weight) is the number of protons and neutrons in an atom. Atoms of an element that have differing numbers of neutrons (but a constant atomic number) are termed isotopes. Isotopes can be used to determine the diet of ancient peoples by determining proportions of isotopes in mummified or fossilized human tissues. Biochemical pathways can be deciphered by using isotopic tracers. The age of fossils and artifacts can be determined by using radioactive isotopes, either directly on the fossil (if it is young enough) or on the rocks that surround the fossil 9for older fossils like dinosaurs). Isotopes are also the source of radiation used in medical diagnostic and treatment procedures.\n\nNote that each of these isotopes of hydrogen has only one proton. Isotopes differ from each other in the number of neutrons, not in the number of protons. Image from Purves et al., Life: The Science of Biology, 4th Edition, by Sinauer Associates (www.sinauer.com) and WH Freeman (www.whfreeman.com), used with permission.\n\nSome isotopes are radioisotopes, which spontaneously decay, releasing radioactivity. Other isotopes are stable. Examples of radioisotopes are Carbon-14 (symbol 14C), and deuterium (also known as Hydrogen-2; 2H). Stable isotopes are 12C and 1H.\n\nCarbon has three isotopes, of which carbon-12 and carbon-14 are the most well known. Image from Purves et al., Life: The Science of Biology, 4th Edition, by Sinauer Associates (www.sinauer.com) and WH Freeman (www.whfreeman.com), used with permission.\n\nThe Periodic Table of the Elements provides a great deal of information about various elements. An on-line Periodic Table is available by clicking here, or if that is busy try a mirror site.\n\nThe Periodi