forgot the options so it will kinna be hard for me to find these when its due tomorrow and its 1.38 a.m. and I have school tomorrow !!lol. HELP please. Thanks, here are the questions...\n\n1.)The negatively charged subatomic particle located outside the nucleus of an atom is called the ________.\n2.)Bonding that occurs when there is a transfer of electrons is called _________.\n3.) Substances produced when atoms of elements chemically combine with each other are called _______.\n4.) In a(an) _________reaction, a complex substance breaks down into two or more simpler substances.\n\nTHX FOR YOUR TIME. YOU MIGHT NOT WANNA JUST GIVE ME JUST ANYTHING CAUSE IM BASING MY BEST ANSWER ON IF ITS RIGHT CAUSE IM GOING TO CHECK THESE IF POSSIBLE.
121334
1. electron\n2. ionic\n3. molecules of compounds\n4. decomposition (not sure)
300852
first of all, two elements combine to form molecules...not new elements, unless you are talking fusion, and that will involve radiation, not voltage (electric potential).\n\nsecond of all, there is no question here, unless you are asking if what you wrote makes sense.  If that is the question, then no, it does not make perfect sense.
349774
Because there will always be interactions between all the elements in a compund except for a bridging ligand, we can asusme that we need to take into account the charge on each atom. \n\na element in group 2 is always +2\na element in group 4 is +2,3,4\nOxygen is is -2\n\nknowing we have a neutral charge we can immedialty eliminate C and as we know that we must use all of our atoms the only answer that makes sense is D
255915
From elementary chemistry it is known that the atomic structure of any element is made up of a positively charged nucleus surrounded by electrons revolving around it. An element’s atomic number indicates the number of positively charged protons in the nucleus. The atomic weight of an atom indicates how many protons and neutrons in the nucleus. To determine the number of neutrons in an atom, the atomic number is simply subtracted from the atomic weight.\n\nAtoms like to have a balanced electrical charge. Therefore, they usually have negatively charged electrons surrounding the nucleus in numbers equal to the number of protons. It is also known that electrons are present with different energies and it is convenient to consider these electrons surrounding the nucleus in energy “shells.” For example, magnesium, with an atomic number of 12, has two electrons in the inner shell, eight in the second shell and two in the outer shell.\n\nAll chemical bonds involve electrons. Atoms will stay close together if they have a shared interest in one or more electrons. Atoms are at their most stable when they have no partially-filled electron shells. If an atom has only a few electrons in a shell, it will tend to lose them to empty the shell. These elements are metals. When metal atoms bond, a metallic bond occurs. When an atom has a nearly full electron shell, it will try to find electrons from another atom so that it can fill its outer shell. These elements are usually described as nonmetals. The bond between two nonmetal atoms is usually a covalent bond. Where metal and nonmetal atom come together an ionic bond occurs.\n\nhttp://www.tech.farmingdale.edu/depts/met/met205/atomicbonds.html\n\nhttp://web.jjay.cuny.edu/~acarpi/NSC/5-bonds.htm
139808
I'm going to explain it really simplified, without the theory behind it, but:\n\nIf an atom has two bonds attached to it, it's an sp.\nIf an atom has three bonds attached to it, it's an sp2.\nFour bonds, sp3.\nFive bonds, sp3d.\nSix bonds, sp3d2.\n\nMake sure you count double and triple bonds toward the bond number.\n\nJust remember that on the test. The reasoning behind it has to do with the number of orbitals that are mixed together. An sp3 is a mix of one s orbital and 3 p orbitals, forming 4 orbitals that are between s and p in energy. An sp3d2 is a mix of one s, 3 p's, and 2 d orbitals, forming 6 orbitals, all of the same energy.\n\n\nHope this helped.
382850
no too sure since its been a while since iv done this, but its a simple enough molecule, C2Br4  2Br to each carbon and a double bond between the carbons, its a linear moleule, not sure about the electronegativity of the elements as my notes r all packed away but the Br atoms should sit slightly of veritcal from each other toward the outside of the molecule. and im sure that the two halves sit at 90 degrees to each other, not sure if u call it this but if u do then 2 Br attached to one carbon will sit along the x- axis of the molecule and the two Br attached to the other carbon will sit along the Z-axis, ask ur tutor or teacher if this is correct as im not 100% sure\n\ntetrahedral only applies to CBr4, thats because the 4 Br are comin off the same carbon, because there are 2 carbons it changes it all together\n   (ignore the full stops, needed them to position the atoms decently)\n\nBr&#92; ........ /Br\n.......C=C\nBr/ ........ &#92;Br\n\nThis is not perfect but imagine the top Br on the left aiming toward you at 45 degrees and the top one on the right aiming away at 45 degrees, hope this helps
29133
Some atoms do not loose their electrons easily.  These can either share electrons (like carbon usually does) or snatch electrons from other atoms to become negative ions (like Fluorine does).  Most metallic elements easily loose electrons to become positive ions (like sodium Na - e- = Na+).
488160
1. Not sure\n2. Electrons in their outer shell\n3. Shells of electrons?\n4. Metalloids
435711
Indeed; this has to do with atomic orbital structure. Atoms try to fill their outermost electron shell with electrons. All atoms will release energy when they accept an electron (this energy is called its electron affinity) and absorb energy when they free an electron (called the ionization potential). Atoms that are a few electrons short of filling their last shell (such as O, F, Cl and most of Group IIIA-VIIA on the periodic table) "will do anything" to fill this last shell, and will release a great amount of energy in the diatomic form (O2). Thus two single O atoms are not stable very long, they would immediately react to form O2 which is far more stable. O is so unstable it would even react with O2 to form O3 if it can't find another O atom.\n\nThe fact that some atoms "exist only" in diatomic form in nature does not mean it is impossible to single out an O atom. If you bombard O2 atoms with light that has a higher energy than the bond, you will break it. And, for a brief period of time, will have to single O atoms which will very quickly react with one another, or with another molecule to achieve stability.\n\nHope that helps; good luck with your studies.
484080
A: they are the only electrons used by atoms to bond. they belong to the shell, so it does not take so much energy to get them away from the nucleus.\nB: for example: N +N = N2, the both have 5 valence electrons, so, by sharing electrons they can achieve an octet (they have a chemical interaction through their valence electrons   :N:::N:)\nC: In a same period, atom increase 1 (in Z) by moving →. Interaction between protons and electrons are much more important than electron-electron. Because neutral atoms have the same number of protons than electrons, then, nonmetal usually have smaller radius, because protons attract much harder the electrons than the own electron repulse with each others. When they become ions the situation is different: nonmetal are usually larger (because they attract electrons; they are anions, and metals release them. So, metals decrease the repulsive forces between electrons, and at the same time they can get more interaction proton-electron, the opposite thing happens with non-metals: they are only adding repulsive forces by taking in electrons, which decrease the effective nuclear charge).\nD: valence electrons are the outermost electrons, they belong to the shell, so they have the highest energy levels.\nE: Li, because it goes: Li>K>Ba>Ca>Na>Zn>Cr>fe>Co>Ni>\nSn>Pb>Cu>Ag>Hg>Pt>Au.\nF: the O is usually O2- ion when bonds because it is easier for the O atom to taking in 2 electrons and complete an octet (O is in group 6A: it has 6 valence electrons) 6+2=8, just like Ne.\nG: Nitrate: since N works with 5+ valence in this ion and you have 3 O (2- each= 6-) the ion is negative and usually bonds forming salts with metals, like AgNO3\nH: the are cation: by loosing electrons they achieve an octet. Their are solid (except for Hg, Ga), shiny, silver, they can do layers and thin strings... some of them (transition) are magnetic (they have unpaired electron that don't cancel with another electron their magnetic momentum (that is what gives them spin +-1/2))...\nNoble gas: elements of group 8A, they have an octet so it is not strictly necessary for them to bond in order to get stability.\nJ: usually elements like F, Cl, O, N. They are quite electronegative and they are usually involved in many reactions.
147468
As above, chemical bonds hold atoms together, making molecules.  Molecules make up the vast majority of the stuff everything is made of.  Knowing all we can know about chemical bonds enables us to break existing bonds and make new ones.  That's how we make different kinds of things (from new drugs to artificial diamonds).  It's what makes chemistry soooo cool.  \n\nThere are 4 kinds of bonds (covalent, ionic, metallic, and hydrogen), but I've never heard of 4 kinds of hydrogen bonds.  Hydrogen bonds, strictly speaking, are different from the other three and are the attractive force between a polar hydrogen atom in one molecue and an exposed, unshared pair of electrons on another atom (like oxygen or nitrogen) on another molecule.
504480
the minus means that you have to add an electron somewhere. So you could add it to the middle N and then you would have single bonds to both side N's. Then there would be 4 electrons left on all of the N's
340858
This is kinda hard to draw on here...\n......_\nK--Br|\n......_\n\nThe lines around Br represent 2 electrons, and the -- represents a bond...ignore the periods
538785
Huge order. Let's see how far it can be served.\n\n1. Monoatomic negative ions: take the element name (sometimes shortened) and add "-ide" (as in hydride, nitride, oxide, sulphide, phosphide, chloride...)\nPositive ions: element-name, charge (if several charges are possible), ion (sodium ion, iron II ion...)\n\n2. Polyatomic ions:\nComplexes with various ligands list the ligands and the central ion/atom.\nOxygen as ligands has its own nomenclature, depending on oxidation state. E.g. Sulphate, sulphite, perchlorate, chlorate, chlorite, hypochlorite...\n\n3. Binary molecular compounds: Halogen, oxygen and sulphur compounds usually have the correspondent "-ide" as if you had ionic compounds. Usually the more electropositive element is used as center.\n\n4. Acids: Oxygen acids have a similar nomenclature to oxygen ions.
31100
people have this picture in their head of what an atomic electron is like - it's a little ball and it whizzes around the nucleus really fast.  but it's not really like that.  \n\nyou have to divorce from your mind the notion that the electron has a single, fixed, localized position.  instead the electron is "spread out" over space, like a big smear in three dimensions.  a lot of chemistry teachers like to fudge this bit by saying that the electron spends "more time" in areas with higher electron-cloud density, but that's not really correct.  if it were, i could see where your confusion might come from - if it was spending some time on one side of the nucleus, it must spend some time getting back to the other side.\n\nthe truth is, in quantum mechanics an electron is "delocalized".  this means that it has no real, fixed position - instead it is spread out over a region or regions of space, and in fact those regions of space need not be connected.  the electron is quite literally in both places at once, not in one place or the other.\n\nthis is a rather small effect in atomic electrons, but if you consider a conducting metal like copper, the "free electrons" that carry electricity are extremely delocalized.  every single electron is basically spread out over the entire piece of copper.  it's kind of hard to picture, but that's why quantum mechanics is hard.\n\nhope this helps.  feel free to email if you'd like to discussit more.
207300
when a solid is formed with hydrogen the way it is formed is by covalent/ionic bonding.  \nBecause there would be no electron covalent bonds would not be able to be formed.  also because every thing would be positivly charged it would not be possible for ionic bonds to form.  \n\nthe definition of a plasma is exactly what you are looking at.  It is the fourth state of matter, namely it is when the electrons are dissasociated from the nucli.  No matter what tempature you had it would remain a plasma.  even if it was cooled to abolute zero and pressurised with electrostatic feilds it would still remain in a gas like form for there is no way for it to solidify.  The repultion of the electric feilds would be far to great to over come the neuclear forces that would be needed to make an isotope of heleium with no nutrons.  \n\none might imagine that if you did cool it and compress it a whole bunch it would maintain some shape, but then quantum mechanics take over and the protons would be switching possitions constantly.  \n\nalso the possitive charge of the proton star would be incredible, remeber that it takes only one in a thousand electron to make a substance very highly electricly charged... we are talk a thousand times more than that it is impossible to even imagine what the effects would be
303552
Don't listen to him.  They are both a form of atom bonding using the electrons in the outer shell of the atom.  The atoms bond to make themselves stable.  Covalent bonding occurs when atoms will share electrons to become stable like all hydrocarbons.  Ionic bonding is very similar, these types of bonds usually occur between metals and non metals and need to either lose or gain electrons to become stable.\n\nTry this site for a better explanation.\n\nhttp://en.wikipedia.org/wiki/Ionic_bonding\n\nhttp://en.wikipedia.org/wiki/Covalent_bonds