octet rule sentence in Hindi
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- The nitrate ion ( NO 3 " ), for instance, must form a double bond between nitrogen and one of the oxygen's to satisfy the octet rule for nitrogen.
- The octet rule is a heuristic ( very simplified rule-of-thumb ) which helps get the right answer without having to go through the in-depth mathematics necessary to understand the full implications of quantum theory.
- When figuring out the most stable form of a molecule, does requirement for octet rule always trump everything else, no matter what kind of atoms are involved ? talk ) 03 : 07, 17 January 2008 ( UTC)
- In the methane diagram shown here, the carbon atom has a valence of four and is, therefore, surrounded by eight electrons ( the octet rule ), four from the carbon itself and four from the hydrogens bonded to it.
- For example, in PCl 5, if it is supposed that there are five true covalent bonds in which five distinct electron pairs are shared, then the phosphorus would be surrounded by 10 valence electrons in violation of the octet rule.
- The rules which govern stability of electron configuration are extremely complicated, so a lot of simple versions such as the " octet rule " exist; however these are at best " approximate " and talk ) 16 : 31, 2 January 2008 ( UTC)
- Still haven't figure out how PEP explains the octet rule . ( And no, it's not homework I don't have homework . )-- 71.162.233.206 03 : 18, 9 April 2007 ( UTC)
- To form five bonds, the one s, three p and one d orbitals combine to form five sp 3 d hybrid orbitals which each share an electron pair with a halogen atom, for a total of 10 shared electrons, two more than the octet rule predicts.
- In this model the availability of empty d orbitals is used to explain the fact that third-row atoms such as phosphorus and sulfur can form more than four covalent bonds, whereas second-row atoms such as nitrogen and oxygen are strictly limited by the octet rule.
- According to the octet rule, the atoms immediately before and after neon in the periodic table ( i . e . C, N, O, F, Na, Mg and Al ), tend to attain a similar configuration by gaining, losing, or sharing electrons.
- A trick is to count up valence electrons, then count up the number of electrons needed to complete the octet rule ( or with hydrogen just 2 electrons ), then take the difference of these two numbers and the answer is the number of electrons that make up the bonds.
- The "'octet rule "'is a chemical rule of thumb that reflects observation that atoms of main-group elements tend to combine in such a way that each atom has eight electrons in its valence shell, giving it the same electronic configuration as a noble gas.
- Or does the fact that the iodine is " crowded " provide an exception to the octet rule ? ( Too bad astatine isn't stable enough to see if we could get AtF8 . . . damn you radioactivity . ) talk ) 05 : 06, 2 September 2009 ( UTC)
- They can be thought of as abbreviated Lewis structures observing the following conventions : ( 1 ) carbon atoms are indicated as the terminus of a line segment or meeting point of line segments; ( 2 ) hydrogen atoms connected to carbon are omitted, with the presumption that each carbons atom is bonded to the number of hydrogen atoms that would bring its valence to 4 ( or as close to satisfying the octet rule as other electronic details allow ).
- For example, in the sulfur hexafluoride molecule ( SF 6 ), Pauling considered that the sulfur forms 6 true two-electron bonds using so-called sp 3 d 2 quantum-mechanical calculations on this and similar molecules have shown that the role of d orbitals in the bonding is minimal, and that the SF 6 molecule should be described as having 6 polar covalent ( partly ionic ) bonds made from only four orbitals on sulfur ( one s and three p ) in accordance with the octet rule, together with six orbitals on the fluorines.
- Because the way I see it, the total sum of the enthalpy of K + and the kinetic energy of the electron is definitely greater that the enthalpy of K, but maybe the enthalpy of the ion itself ( without the kinetic energy of the electron ) is less than K . Because when you think about it in a simple non-thermodynamic point of view, potassium ( or any alkaline metal for that matter ) is definitely unstable in its atomic form, and is definitely happier in its ionic form because of the octet rule, so you could say that K + is more stable than K, right?
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