Describe the electron arrangement that makes an atom stable.?
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An atom is stable when it has a full valence (outer) electron shell.  For the first row on the periodic table, the outer (and only) shell can hold up to 2 electrons.  For the next two rows, the atoms' outer shells can hold up to 8 electrons.  The next two can hold up to 18.\n\nAtoms like sodium, in column 1 of the periodic table, have one electron in its valence shell.  It is very reactive, since it wants to get rid of this extra electron so that its outer shell can be full.\n\nAtoms like chlorine, in the second last column, have one electron missing from their valence shells.  They are also very reactive, since they want to accept an electron to fill the outer shell.\n\nNoble gases are almost totally unreactive, since they have the unique property of having full outer shells without having to give away or accept any electrons.
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For Al .. \n\nElectron configuration : [Ne] 3s2 3p1 ... so after losing 3 electrons its stable and need high energy to destabilize it ..\n\nwhile for As [Ar] 3d10 4s2 4p3 .. \nfor Ga [Ar] 3d10 4s2 4p1\nfor Se [Ar] 3d10 4s2 4p4\nfor S [Ne] 3s2 3p4\n\n4th ionization energy in kJ/mol :\n\nAl  11577 \nGa 6180 \nAs 4837 \nS 4556\nSe 4144
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1.ATOMIC NUMBER\n2.ELECTRON\n3.SHELL\n4.ORBIT
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a nucleus, containing protons and neutrons  and around that nucleus, there are electrons. [Although it more correct to speak of electron clouds, as they are not really localized. ]
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to explain how two electrons can be near each other
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Well if it's stable, there will be the same amount of protons as electrons. If it has a charge add or subtract. \n(If you have a plus charge, that means there's 1 more proton than electron... if you have a -2 there are two more electrons than protons etc.)
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b. electrons\n\nI really hope you are trying to answer these first before you put them on here because although we are all certainly willing to help you, you are not going to gain anything from just having the answers given to you.  You really need to try and learn this stuff.
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By Hund's rule of multiplicity, the more or most stable state of electronic configuration is such that all the electrons are at most UNPAIRED before Pairing up. \n\nIn Chromium, there is an option for the electrons to "scatter" in five separate unpaired d orbitals first before being "forced" to pair up. Moreover, the electron in the 4s  level is unpaired as well. The stabilizing effect of these unpaired spins makes up for a lot more than the stabilizing effect of the paired 4s2 electrons.
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alright. Electron configurations. I had the exact same problem three weeks ago. I was SO confused. But i got it in the end.\n\nLet me explain.\nThere are two types of electron configurations. One is the simple electron shell configuration. Let's say 2-8-16 and the other is called spdf notation like 1s2 2s2(i can' t type the two after the s like an exponent so bear with me)\n\nNow the first one is simple. Shell notation. An atoms outer shells are divided into shells that each have a maximum limit for the number of electrons that they can contain. the first can hold 2, the second 8 and so on. They all follow a rule. It is always 2 time the shell number squared. lets say level 1. Square it. You get 1. Multiply it by 2. You get 2. Therefore 2 is the maximum # that level one can hold. You said 15. So fill each level so that each contains the max. It would be 2-8-5. (The last one is five so that the all ad up to 15). Got it?\n\nNext, we have spdf notation. This takes a lot of time to explain so i'll just give you a site to go to. \n\nhttp://www.fordhamprep.org/gcurran/sho/sho/lessons/lesson36.htm\n\nGood luck!
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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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alkaline earth metals are elements of group 2 in periodic table, so they have 2 electrons in outermost orbit. so to become stable they will try to loose 2 electrons to have stable electronic configuration. so they all have +2 oxidation states.\n\ni hope this will help you out
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A suspecious student for perfection?\n\nGood question.\n\nGenerally H is shown on top of 1st group but H has three positions:\n\n1. Top of 1st Group: Because there is only one electron is the outer most shell. H can also form +1 ions.\n\n2. Top of 7th Group: Because one electron is short to complete the outer most shell. H can also form -1 ions.\n\n3. At top of 4th Group: Because 4th group and H have half filled outer most shell. H mostly forms covalent compounds.
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Two in the first shell. 10 in the second shell. 10 in the third shell. 5 in the 4th shell for neutral Manganese. Mn 2+ is missing 2 electrons, so it would only have 3 in the outer shell. The rest will stay the same.\n\nHere's a cool interactive periodic table that may help you with your homework. \n\nhttp://www.webelements.com/\n\nYou can click on the the element you are interested in, then in the column on the left you can go to electronic properties and it will show you how the electrons are distributed. You can add or remove electrons to configure the electron arrangement of various ions of the substance you are interested in.
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Electron is simply the smallest and ligthest subatomic particle inside every atoms. as you know, atom consists of protons (positively charged), neutrons (no charge) and electrons (negatively charged). you can imagine atoms to be like a planet which has meteors orbiting around it. the planet represent the nucleus which consists of the protons and the neutrons. and the meteors around are representing the electrons. due to its light weight, electrons move around in an incredible speed around the nucleus. however, electrons do not escaped from the nucleus because they are bounded by forces which keep them in tracks. you can check it out in www.wikipedia.com if you need more info on electrons :D . GL for ur science fair anw.
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Yes, then it is a called a cation.  The element still contains its protons and therefore gives the ion a positive charge.  \n\nHowever, the electron configuration of the element determines what ions you can make as the stability will drastically fall with the more electrons removed
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proton and neutron, the electrons are on the outer shell
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The valency is determined by how many electrons the atom is using to bond with another atom to form a compound. The electrons in the outermost orbit generally forms the bonds. For materials having multiple electrons in the outermost orbit the element can have different valencies. Whatever happens tends to lower the the total energy of the system to make it stable.