What about DNA, a molecule, an atom...
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Self-awareness is something that can't really be defined, and is debated often by philosophers.\n\nHowever, the way most people define self-awareness is when you can identify and think about yourself, and act in a way that shows this.  The only truly self-aware species is the human species, but there is some evidence that non-human primates are aware about some things, but not others (for a good example see Gordon Gallup Jr.'s mirror test for self-awareness)\n\nMicrobes are usually unicellular, and only have the most essential mechanisms for them to survive.  From our experience with the biological world, self-aware species (or species that come close to it) have an extremely complex central nervous system (the brain, brainstem, etc).  Thus, microbes are not aware at all.\n\nThe microbe's smaller components, such as ribosomes, endoplasmic reticulum, DNA, etc. are also not aware, by the same definition.
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Yes. DNA is a polynucleotide, and the bases referred to are actually the paired up ATCG. I think the person who answered this question thought that you were referring to the sides of the molecule, i.e. the ribose-sugar backbone, also comonly called the 'rails'.
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The fundamental physical and functional unit of heredity. A gene is an ordered sequence of nucleotides located in a particular position on a particular chromosome that encodes a specific functional product (ie, a protein or RNA molecule).
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DNA, perhaps?  Deoxyribonucleic acid, that is.
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The atomic number of an element is equal to the number of electrons it has. Do you mean something more than that?
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Yes, all organisms(living things) have DNA.
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You have one correct idea listed.  It is the smallest particle of a single element.  Atoms, however, are not "uncuttable" as there are much more fundamental particles, like electrons.  Neither would I call atoms "the building blocks of all matter" as there are more fundamental particles out there.  An atom is simply the smallest unit of a single element.
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http://faculty.clintoncc.suny.edu/faculty/Michael.Gregory/files/Bio%20101/Bio%20101%20Lectures/DNA/dna.htm
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Are you talking about Adenine, Thiamine, Cytosine, and Guanine?\nAmino Acids.
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purines: adenine, guanine\npyrimidines: thymine, cytosine, uracil\n\nin the dna, complementary base pairing occurs in adenine=thymine and guanine=cytosine. \n\nbut in the rna, uracil is the one present instead of thymine. therefore, the complementary base pairing in the rna occurs in adenine=uracil and guanine=cytosine.
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Element:\n\nA substance composed of atoms having an identical number of protons in each nucleus. Elements cannot be reduced to simpler substances by normal chemical means.
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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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Two words: Deoxyribonucleic and Acid.
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molecules. i would say that the best and most simple answer to this question is on one the the most basic levels in life. Life is possible because of these reactions that take place everyday such as the main source of life, water. It is brought together by oxygen and hydrogen.
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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
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organ: brain\nmolecule: DNA
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One question at a time please!\n\nCarbon forms Covalent bonds.\n\n1 molecule of Carbon can form 4 bonds.\n\nLipids are formed from Carbon, Hydrogen, and Oxygen and consist of fatty acids, and esters, and glycerols.\n\nOkay, Organic vs. Inorganic Here are some of the most educated opinions on that subject that I have ever encountered:\n\n Ask A Scientist\nChemistry Archive  \n\nhttp://www.newton.dep.anl.gov/askasci/chem99/chem99286.htm\n\n--------------------------------------------------------------------------------\n\nOrganic / Inorganic\n\nQuestion:\nI teach sophomores an introductory biology course.  When I cover the biochemistry section the terms organic and inorganic come up.\nI am not satisfied with the simplistic statement that organic chemicals are ones that contain carbon since it does not account for carbon dioxide being an inorganic. Is there a definition of 'organic chemical' which accounts for all\nor most molecules?\n doug happ\n \nAnswer 1:\n   Given the existence of hemoglobin, "zinc fingers" in some enzymes, and buckyballs, I'd guess not.\n christopher grayce\n\nAnswer 2:\nConsidering the number of carbon containing molecules that ARE considered to be organic relative to the number that are NOT, the rule that an organic molecule is one that contains carbon,  works VERY well. The "exceptions" might serve as a lead-in to a discussion of the use of rules, such as classifying molecules as organic or inorganic, as a contrived convenience.  They are helpful for most cases.  In the cases\nwhere the rules don't work well we have to be able to turn to other tools, such as an understanding of chemical bonds or molecular orbitals so we can concentrate on the characteristic of interest -- which is very rarely\nwhether the molecule is organic or more often things like reactivity. You're at the leading edge of helping these students think for themselves\nin a field where they probably feel unsure of themselves! It sounds like you have some inquiring students there and some active\ndiscussions.  May you have many more!\nGreg\n\nAnswer 3:  An interesting question.\nI believe that "organic" vs. "inorganic" originally stemmed from the ancient idea that compounds could be divided into two categories; those isolated from plants and animals (organic) and those extracted from minerals and ore (inorganic)\n[source: Bodner and Pardue, Chemistry: An Experimental Science, 1993].\n \nAs a working definition, now we think of organic chemistry as primarily being the chemistry of carbon-containing compounds. Most carbon-containing compounds have one or more of the\nfollowing: H,N,O,S,P. Some authors describe organic chemistry as the study of compounds that contain carbon and hydrogen. By this definition, CO2 would be "inorganic." But I would\nlike to stress that in fact there is no general agreement on such semantics, and I'd bet that a lot of chemists consider CO2 to be "organic" because it contains C and O.\nTopper