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Chlorine can be $sp^3d^3$ hybridized. If so, it can form $\ce{ClH_7}$ and then chlorine, being more electronegative, will have (-7) as its oxidation number. But we know that the oxidation number of $\... 1answer 208 views ### Why do the chalcogens (Y) form YX4, YX6 but not YH4, YH6? [duplicate] What is it about hydrogen that makes it different from the halides? What makes it only form di- and not tetra- or hexa- hydrides of the chalcogens? 8answers 134k views ### Can an atom have more than 8 valence electrons? If not, why is 8 the limit? According to some chemistry textbooks, the maximum number of valence electrons for an atom is 8, but the reason for this is not explained. So, can an atom have more than 8 valence electrons? If ... 3answers 3k views ### Why is it wrong to use the concept of hybridization for transition metal complexes? I have asked a lot of questions on coordination chemistry here before and I have gone through a lot others here as well. Students, including me, attempt to answer those questions using the concept of ... 1answer 3k views ### What is the molecular structure of xenon hexafluoride? Xenon hexafluoride,$\ce{XeF6}$, can be obtained by reaction of xenon with excess fluorine gas. What is the gas-phase structure of the molecule? What experimental evidence is there to support it, ... 3answers 8k views ### Hybridization of nitrogen in trisilylamine, (SiH3)3N? I want to know the hybridization of the central atom in$\ce{(SiH3)3N}$. I think it should be$\mathrm{sp^3}$, because$\ce{N}$is attached to three silicon atoms and one lone pair. But actually it ... 1answer 16k views ### What is Drago's rule? Does it really exist? My textbooks states the Drago's rule in inorganic chemistry as follows: The more electronegative atom prefers the orbital having more p character, and lone-pairs or less electronegative elements ... 2answers 2k views ### How are the hybrid orbitals of sulfur hexafluoride shaped? On the fluorine end the fluoride atoms are simply completing a$3p$orbital. On the sulfur end one could posit a hybrid of one$3s$orbital, two$3p$orbitals and a three inner$2p$orbitals. However,... 1answer 2k views ### Why only two atoms share an electron and not three? In a covalent bond between two atoms, an electron from one of the either atom is shared by overlapping of their orbitals. So, Why can't three atoms share an electron and overlap their orbitals? 1answer 5k views ### Why does potassium form peroxides but sodium does not? As we go down the periodic table, Group 1 alkali metals hold their single outer valence electron more loosely, and so reactivity increases. Below potassium (Na, Li), we can store the metal in oil with ... 1answer 2k views ### Why can't NH5 form? In ammonia a nitrogen atom forms 3 covalent bonds with hydrogen atoms and has one lone pair which can be used in a dative covalent bond with another hydrogen atom to form an ammonium ion. Instead of ... 1answer 2k views ### What does reaction exothermicity say about the stability of molecules If a reaction is exothermic it means that the energy state of the products is lower than that of the reactants so this will be the state that 'nature' will naturally strive for. Often you see that ... 1answer 191 views ### Does >2e contribution of an atomic orbital (AO) to a hybrid AO of a molecule violate Pauli exclusion? This question is inspired by On the Role of d Orbital Hybridization in the Chemistry Curriculum J. Chem. Educ., 2007, 84 (5), p 783. The article calculates 6 bonding sulfur atomic orbitals in SF6 as ... 1answer 627 views ### Why is there no non-bonding molecular orbital in the overlap between H1s and Be2s in BeH2 I've only recently started learning about this and I'm stating to get confused. (The orbital in the middle belongs to Be) So you have a + (+) + which gives a sigma bonding orbital and a + (-) + which ... 0answers 528 views ### Why does AsH5 not exist? Why does$\ce{AsH5}$not exist? Is it because the s-orbital of H doesn't and can't overlap with the d-orbital of As after As makes$\rm sp^{3}d\$ hybridization?Theoretically the bond can occur because ...

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