Nature of the bond in Beryllium Chloride?
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The Be2+ cation is smaller in size (being above the rest of the group 2 elements) and hence has high charge density. This enables it to easily polarise the comparatively larger Cl- anion, which results in a covalent characteristic of the compound. As explained clearly in the previous answer, dative bonding occurs in the compound and BeCl2 usually occurs as a dimer i.e Be2Cl4 (polymeric type) based on the linear molecular structure of BeCl2.\n\nPolarisation occurs between a small cation with high charge density and a larger anion. Since the size of the cations of the group 2 elements increases down the group (more atomic radius), charge density around the cation decreases and hence their ability to polarise the Cl- also decreases, resulting in an ionic compound.
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Element = Sodiuim.  It still retains its properties even at the atomic level.\n\nCompound = NaCl (Table Salt).  It consists of two chemically bonded elements.\n\nMixture = sand and sugar.  No chemical bonding occurs.
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NaCl can conduct electricty well becuase its valence electrons can move between the atoms easily
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http://www.chemicalelements.com/elements/be.html\n\nthis website may help you!!!!!! ( hope you get an A)
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Atomic radii decrease as one moves from left to right across a period and while moving up a group. The atomic radius is the distance between the nucleus and the valence electrons.\n\nElectron affinity, ionization energy, and electronegativity increase as one moves from left to right across a period and while moving up a group. \n\nElectron affinity is the ease with which an atom can accept an electron. The halogens (F, Cl, I, etc.) have the highest electron affinity, with F having the highest of all elements. The alkaline metals (Li, Na, K, etc.) have the lowest electron affinity, with Fr having the lowest of all elements.\n\nIonization energy is the energy needed to remove an electron from an atom. All atoms want to form a stable octet. Since alkaline metals only have one valence electron, it takes very little energy to remove an electron from them. In contrast, it takes a lot of energy to remove an electron from a halogen.\n\nElectronegativity is the strength of the attraction an atom has for an electron in a chemical bond. Halogens are the most electronegative, while the alkaline earths are the least. The electronegativity of two elements can inform you of what type of chemical bond they will form. If Na (low EN) and Cl (high EN) form a bond, Cl will rip the lone valence electron away from Na, forming an ionic bond. If C and O form a bond, the atoms will share electrons because their EN's are very close. Since O is more EN, it will have a slight negative charge, and the bond will be a polar covalent bond. If C and C form a bond, both have the same EN, and they will form a non polar covalent bond.
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Its a salt of beryllium and is toxic and is mainly used to extract the beyllium from it and hence is an mineral. Beryllium is used in aerospace and defense industry as light weight structural material. Beryllium is used in nuclear weapons for similar reasons. \n\n\nBeryllium is used as an alloying agent in the production of beryllium-copper because of its ability to absorb large amounts of heat. Beryllium-copper alloys are used in a wide variety of applications because of their electrical and thermal conductivity, high strength and hardness, nonmagnetic properties, along with good corrosion and fatigue resistance. These applications include the making of spot-welding electrodes, springs, non-sparking tools and electrical contacts.\n\n\nThin sheets of beryllium foil are used with X-ray detection diagnostics to filter out visible light and allow only X-rays to be detected.\n\n\nBecause it has a low thermal neutron absorption cross section, the nuclear power industry uses this metal in nuclear reactors as a neutron reflector and moderator
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Quick answer is that HCl is a covalent compound and LiCl is an ionic compound.
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a) Tetrahedral shape. bond angle : 109.5\nNo lone pair on central carbon\n\nb) Linear shape. Bond angle: 180\nNo lone pair on central Be\n\nc) Trigonal pyramdial shape. Bond angle less than 109.5\na lone pair on Cl. 2 oxgen double-bonded and 1 oxygen single-bonded to Cl. 0 formal charge on Cl and the O=Cl. Formal charge on Cl-O is -1.
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Any two elements from different sides of the periodic table. More specifically, one from the metal category and one from the nonmetal category.\n\nEDIT: brwneyes, sodium chloride is one example of an ionic bond, not the only kind of ionic bond.
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Sterostructure is its three-dimensional structure in space. The central P atom has 5 bonding pairs and no lone pairs, so the Cl atoms will be arranged in a trigonal bipyramidal shape, with 90 degrees between the axial and equatorial bonds, and 120 degrees between the equatorial bonds themselves.
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Metallic bonding is the bonding within metals. It involves the delocalized sharing of free electrons between a lattice of metal atoms. Thus, metallic bonds may be compared to molten salts.\n\ne.g. Iron (Fe)... Why is it so strong? Of course, metallic bonding.\n\nMetal atoms typically contain a small amount of electrons in their valence shell compared to their period or energy level. These become delocalised and form a Sea of Electrons surrounding a giant lattice of positive ions.\n\nMetals seem to have higher boiling and melting points which might suggest stronger bonds between the atoms.\n\nMetallic bonding, as with covalent bonding is non-polar, in that there is no (for pure elemental metals) or very little (for alloys) electronegativity difference among the atoms participating in the bonding interaction, and the electrons involved in that interaction are delocalized across the crystalline structure of the metal.\n\nThe metallic bond accounts for many physical characteristics of metals, such as strength, malleability, ductility, conduction of heat and electricity, and luster. See also chemical bond.\n\nMetallic bonding is the electrostatic attraction between the metal atoms or ions and the delocalised electrons. This is why atoms or layers are allowed to slide past each other, resulting in the characteristic properties of malleability and ductility.\n\nMetallic bond are different from chemical bonds. Ionic and covalent bonds are chemical bonds.\n\nCovalent bonding is a common type of bonding, in which the electronegativity difference between the bonded atoms is small or non-existent. In the latter case, the bond is sometimes referred as purely covalent. See sigma bonds and pi bonds for current LCAO-explanation of non-polar bonds.\ne.g. CH4 (methane)\n\nIonic bonding is type of electrostatic bond between atoms which have an electronegativity difference of over 1.6 (this limit is a convention). These form in a solution between two ions after the excess of the solvent is removed.\ne.g. NaCl (common salt)\n\n<BEST ANSWER>\n============================================================\nHey, I tried to draw the structures of NaCl and methane molecules but this Yahoo! made it impossible. I hope you know the structurel.
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Determining structure of molecules.\nIonic structures- The Alkali metal halides are ionic compounds e.g NaCl. Na has a positive charge whereas Cl has a negative charge.\n\nMolecular solids- are held by weak bonds called Van Der waals forces. \n\nMacromolecular structures or giant molecular- have covalent bonds between atoms, these bind all the atoms into a giant molecule e.g Diamond
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NaCl IS NOT TWO ATOMS (sodium and chlorine) BONDED TOGETHER!\n\nNaCl is what is known in chemistry as an ionic salt.  That means that a very positively charged Na+ ion met up with a very negatively charged Cl- ion, and because opposite charges attract, they got close to each other in what is known as an ionic bond, which isn't really a bond, just two particles hanging out together.
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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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Nickel(III) Bromide and Beryllium Nitrate
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Halogens, in their elemental state, are covalent. In their elemental state, they are not compounds, because they are not combined with other elements. But F2, Cl2, Br2, I2, and At2 are covalently bonded.
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The most polar bond will be the one between atoms that have the biggest difference in electronegativity\n\nF is the most electronegative element there is.\nC has similar electonegativity to S.\nCl and Br are quite close to each other\nSo the biggest difference in electronegativity is between the C and F, thus the most polar bond is C-F in CF4\n\nThe molecular dipole moment depends on the sum of the dipole moments of all the bonds in each molecule.\nCS2 is linear and the dipole moments are cancelling out each other so the total dipole moment is 0\nBr-Cl has only one polar bond (Cl is more electronegative) so it has a dipole moment\nSCl2 has 2 polar bonds and 2 lone pairs in the central atom (S). So the arrangement of the electron groups is tetrahedral and since there are only 2 bonds, there is a net dipole moment\nCF4 the molecule is tetrahedral but has 4 identical polar bonds so the dipole moments cancel out each other and the molecule has no dipole moment\nC2H2 is linear with the dipole moments of the polar C-H bonds canceling out each other (the molecule is H-Ctriple bondC-H) so the dipole moment is 0