For example, a chemical bond between Titanium and Aluminum.  Both of them donate electrons. so how can they form bonding together...like TiAl, TiAl3, etc.???
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Intermetallic bonding is definitely confusing....\n\nFirst to review titanium chemically....All 'transition' metals are called as such because the the electrons in their outer-most shells keep shifting from one orbital to another and never stay put. This is why transition metals form compounds with variable oxidation states/valencies, as they don't always donate a fixed number of electrons, unlike group 1 and 2 elements which always donate 1 and 2 electrons respectively. So if a transition metal like titanium is to combine with another metal, then the resulting compound would not have a fixed formula, as you justified by mentioning TiAl and TiAl3.\n\nWhen 2 metals are to combine, both of them would donate electrons and since neither of the 2 metals would accept them, the donated electrons form an electron cloud around the atoms. Imagine it as 2 positive charges (nuclei of both metallic atoms) surrounded by a negatively charged cloud. The electron cloud is held in place by the attractive force of the nuclei for the electrons. \nIf 2 non-transition metals combine, the electron cloud formed would contain the fixed number of electrons that each metal would donate. If 2 transition metals combine or a transition metal combines with a non-transition metal, the electron cloud would vary in the number of electrons in it. \n\nConsider the electronic configuration of Ti and Al: \n1s2, 2s2, 2p6, 3s2, 3p6, 3d2, 4s2. [titanium]\n1s2, 2s2, 2p6, 3s2, 3p1 [aluminum]\nTitanium would donate 4 electrons from 4s2 and 3d2 to achieve noble gas configuration of argon. As stated at the beginning, the electrons in 3p and 3d orbitals would keep shifting to and fro, so it may happen that at one point, 2 electrons from 3s orbital shift to 3d, and the like. So each time titanium has to bond with aluminum, it may donate 4 or more than 4 electrons.\nIf at one point, 1 titanium atom donates 4 electrons from 4s2 and 3d2 and 4 aluminum atoms donate 1 each from 3p1, then both will have a complete orbital (for Al) and a complete shell (for Ti) left. So with 1 Ti atom and 4 Al atoms, the compound formed will be TiCl4. Other compound like TiAl will be formed according to the number of atoms (of both metals), and the number of electrons they donate.
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1. Covalent Bonds\n2. Ionic Bonds\n3. Hydrogen Bonds
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when bonding takes place by sharing of electrons then it is said to be covalent bond. now it can be possible in two ways.\n\nfor eg if two hydrogen are combining to form a bond then they both will share one electon each and the force applied from there nucleus will be same so the elecron pair will remain nearly equal with both the hydrogen.so you can say that it remains exactly at centre from both the nucleus\n\nbut if you consider HCl. here also both hydrogen and chlorine are going to share one elctron each when bond formation takes place. but as electronegativity of chlorine is quite high(ie its attraction from nucleus is quite high) compared to that of hydrogen so eventhough they both have shared one electron each but still electron pair will remain towards chlorine.\n\ni hope this will help you out
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d) bond to carbon\n\nThis nonmetal has the interesting chemical property of being able to bond with itself and a wide variety of other elements, forming nearly ten million known compounds.
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only Sodium Chloride is not.\n\nsimple answer:\ncovalent bonds are between non-metals\nionic bonds are between a metal and a non-metal\n\nthis is because of the large difference in electronegativity between metals and non-metals.\n\nonly sodium chloride has a metal.  the rest are all made only of non-metals and thus covalently bonded.
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what you need to do, get a SI data book, and look up their natural state. not bonded with anything else, and possibly itself.\n\nPhophorus - white: molecular (P4). red: Chain. Black: Layer\nIodine - molecular (I2)\nMagnesium - hexagonal closest-packing\nNeon - cubic closest-packing\nArsenic -grey: 3d structure - Layer formation. yellow: molecular As4\nSulfur- molecular S8\nBoron - complicated structure.\nSelenium - grey: chain, Red: molecular: Se8\nGallium - Complicated\nCesium - body-centred cubic\nOxxygen - O2, O3 molecular
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Forget the potassium ions - they don't do anything. The aluminium metal dissolves in the potassium hydroxide solution, forming aluminate ions and hydrogen gas.\n\nThe ionic equation is:\n\n2Al + 2OH- + 6H2O ---> 2[Al(OH)4]- + 3H2\n\nTo explain how to get this equation, you need the ideas of half equations, and oxidation and reduction.\n\nFor example, Al + 4OH- ---> [Al(OH)4]- + 3e-\n\nand 4H2O + 4e- ----> 2H2 + 4OH-\n\nNow combine them, getting the number of electrons equal, and cancelling down some hydroxide ions.\n\nIf it's any consolation, this exercise would be beyond most A-level pupils in the UK.
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Ionic compounds try to achieve the same thing...only instead of atoms sharing electrons with other atoms (co-valent) in a chemical bond, Ionic compounds achieve lowest energy configurations by receiving, or giving up, electrons.  For example, the sodium atom has one electron in it's valence "shell" and will give it up (becoming positively charged in the process) in order to have the same electronic configuration as the previous noble gas (neon) and becomes the sodium cation.\nFluorine, having seven electrons in it's valence shell would rather accept and electron (to have the neon electron configuration) and becomes the negatively charged fluoride anion.
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Force holding atoms in a molecule together as a specific, separate entity (as opposed to, e.g., colloidal aggregates; see bonding).\n\nIn covalent bonds, two atoms share one or more pairs of valence electrons to give each atom the stability found in a noble gas. In single bonds (e.g., H-H in molecular hydrogen), one electron pair is shared; in double bonds (e.g., O=O in molecular oxygen or H2C=CH2 in ethylene), two; in triple bonds (e.g., HCºCH in acetylene), three. In coordinate covalent bonds, additional electron pairs are shared with another atom, usually forming a functional group, such as sulfate (SO4) or phosphate (PO4). The number of bonds and the atoms participating in each (including any additional paired electrons) give molecules their configuration; the slight negative and positive charges at the opposite ends of a covalent bond are the reason most molecules have some polarity (see electrophile; nucleophile). Carbon in organic compounds can have as many as four single bonds, each pointing to one vertex of a tetrahedron; as a result, certain molecules exist in mirror-image forms (see optical activity). Double bonds are rigid, leading to the possibility of geometric isomers (see isomerism). Some types of bonds, such as the amide linkages that join the amino acids in peptides and proteins (peptide bonds), are apparently single but have some double-bond characteristics because of the electronic structure of the participating atoms. The configurations of enzymes and their substrates, determined by their covalent bonds (particularly the peptide bonds) and hydrogen bonds, are crucial to the reactions they participate in, which are fundamental to all life
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This is based on the electons in the outer shell of the atom you are drawing. From the periodic table you can see how many electrons are in the outer shell e.g. Na has 1, Cl has 7, to create a complete shell (8) they combine to form NaCl. \n\nIf you wanted to draw all of the electrons then you would draw the first shell with 2, which completes the first row of the periodic table, then the second with 8, then the third with 1 (for Na). For Cl you would draw the first shell with 2, which completes the first row of the periodic table, then the second with 8, then the third with 7. \n\nIf you wanted to show the bond between them then you would draw the shells with the final circles combining and two electrons touching the circles.\n\nI did a search and found the website below, there are probably better ones out there but this gives a pictorial representation of some of what I say
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If the metal not in the compound is higher on the activity series than the metal in the compound then a reaction will occur and the metals will switch spots. If the metal not in the compound isn't higher on the activity series than the metal in the compound then no reaction will take place. You got to be joking if you think I'm going to be doing 20 problems for you. The only way to learn these is to do them on your own. Just so you know in #6 a reaction will not occur.\n\nHere is an activity series:\nhttp://en.wikipedia.org/wiki/Reactivity_series\n\nREACH doesn't know how to do these, don't listen to his answer.
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You get the first answered.\nCovalent bonds are strong and don't disassociate into ions, as ionic bonds do. Watch.\nNaCl common salt, sodium and chlorine, put in solution.\n\nNa+  and Cl- they disassociate and you can follow the path of electricity Electron jumps from sodium to be accepted by chlorine. That is electron flow; conduction of electricity.
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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
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Let's see, this may be a bit difficult to explain, but since no one else has so far, I figured I'd give it a shot.\n\nI don't have a periodic table in front of me, so I'll do my best to explain.  There is a double bond between N and one of the O's because of something called "in-bonds."  You determine the number of "in-bonds," or bonds in between elements by subtracting the number of valence electrons that you have all together from the number that you need for everything to be stable.  In this case, forget about H for the time being, and you have N03.  Each element needs 8 electrons to fill its valence shell right?  Multiply 8 by 4, since there are 4 elements, and you get 32.  However, you only have 24 electrons to go 'round.  The difference is 8, there for you can have a total of 8 electrons, or 4 individual bonds in between the elements.  It doesn't matter which O gets to share the double bond with N, as they are all the same.\n\nThe double bond was used in HNO3 and not NF3 because I believe you had enough electrons to go around, therefore there were no "in-bonds."\n\nI hope this helps to clear up your questions.
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In brief:  a model of metallic bonding in which cations are considered to be fixed points within a mobile 'sea' of electrons. \n\nAnother view could be from this definition: (Electron Sea Model) : The metallic bond consists of a series of metals atoms that have all donated their valence electrons to an electron cloud that permeates the structure. This electron cloud is frequently referred to as an electron sea. It might help to visualize the electron sea model as if it were a box of marbles that are surrounded by water. The marbles represent the metal atoms and the water represents the electron sea.\n\nIf you want to look at Electron sea diagrams, go to this URL:\n\nhttp://bouman.chem.georgetown.edu/statesofmatter/stelectron.htm
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Chemical bonds could be ionic, covalent or metallic.\nMolecular bonds implies covalent only.
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im highly sceptical on that, because the bond angle of carbon is different from other chemicals, but if one was to be formed, i would imagine silicone or germanium would form it, although, silicone forms stronger bonds, which cant bend that easily, I THINK... not perticularly true... just an assumption on my part