Recitation Activity 8
... 4. There are three possible structures (called “isomers”) for dichloroethylene, C2H2Cl2, two of which are polar and one which is not. a) Draw the three Lewis structures (use the name to help you), predict an overall shape for each and explain why one is nonpolar and the others are polar. b) Two of ...
... 4. There are three possible structures (called “isomers”) for dichloroethylene, C2H2Cl2, two of which are polar and one which is not. a) Draw the three Lewis structures (use the name to help you), predict an overall shape for each and explain why one is nonpolar and the others are polar. b) Two of ...
Fall Exam 3
... Orbital energies increase in the order 3s < 3p < 3d because orbital penetration decreases in the order 3s > 3p > 3d. Orbital energies increase in the order 3s < 3p < 3d because the Schrödinger equation predicts that orbital energy depends only on the angular momentum quantum number, l. Orbital energ ...
... Orbital energies increase in the order 3s < 3p < 3d because orbital penetration decreases in the order 3s > 3p > 3d. Orbital energies increase in the order 3s < 3p < 3d because the Schrödinger equation predicts that orbital energy depends only on the angular momentum quantum number, l. Orbital energ ...
Bonding - Inorganic Chemistry
... Single bond covalent radius: typical contribution by an atom to the length of a predominately covalent bond. E.g. covalent radius for fluorine is taken to be one half the inter-nuclear distance in the homo-nuclear diatomic F2. The Cl-Cl distance is 1.988 Å yields a covalent radius of 0.99 Å for the ...
... Single bond covalent radius: typical contribution by an atom to the length of a predominately covalent bond. E.g. covalent radius for fluorine is taken to be one half the inter-nuclear distance in the homo-nuclear diatomic F2. The Cl-Cl distance is 1.988 Å yields a covalent radius of 0.99 Å for the ...
ppt
... We took 1 s orbital and 3 p orbitals to make 4 sp3 orbitals. The sum of the atomic orbitals = the sum of the hybrid orbitals The 4 sp3 orbitals point in the 4 directions of the tetrahedral bonds ...
... We took 1 s orbital and 3 p orbitals to make 4 sp3 orbitals. The sum of the atomic orbitals = the sum of the hybrid orbitals The 4 sp3 orbitals point in the 4 directions of the tetrahedral bonds ...
Document
... 29. Which of the following statements is(are) typically true for a catalyst? (A) The concentration of the catalyst will decrease as a reaction proceeds. (B) The catalyst provides a new pathway for the reaction. (C) The catalyst speeds up the reaction. (D) two of these (E) none of these 30. Which of ...
... 29. Which of the following statements is(are) typically true for a catalyst? (A) The concentration of the catalyst will decrease as a reaction proceeds. (B) The catalyst provides a new pathway for the reaction. (C) The catalyst speeds up the reaction. (D) two of these (E) none of these 30. Which of ...
Bonding Challenge
... 1) (a) Draw the Lewis electron-dot structures for CO32-, CO2, and CO, including resonance structures where appropriate. (b) Put the three species in order of increasing C-O bond length? Explain the reason for your answer. (c) Predict the molecular shapes for the three species. ...
... 1) (a) Draw the Lewis electron-dot structures for CO32-, CO2, and CO, including resonance structures where appropriate. (b) Put the three species in order of increasing C-O bond length? Explain the reason for your answer. (c) Predict the molecular shapes for the three species. ...
Hybridization
... Lewis structures and VSEPR are useful tools for predicting the shape of a molecule or ion, but they really do not provide any information about the bonds that exist between the atoms; they do not tell us why covalent bonds form nor do they describe what happens to the atomic orbitals when the bond f ...
... Lewis structures and VSEPR are useful tools for predicting the shape of a molecule or ion, but they really do not provide any information about the bonds that exist between the atoms; they do not tell us why covalent bonds form nor do they describe what happens to the atomic orbitals when the bond f ...
2A Final Exam Review Worksheet
... Hybridization o Determine hybridization for any central atom o Draw hybridization schematics for sp, sp2, and sp3 for atoms (C as well as others) o Determine what hybrid orbitals overlap to form a bond o Determine the total number of σ and π bonds in a molecule (remember bond-line formulas) ...
... Hybridization o Determine hybridization for any central atom o Draw hybridization schematics for sp, sp2, and sp3 for atoms (C as well as others) o Determine what hybrid orbitals overlap to form a bond o Determine the total number of σ and π bonds in a molecule (remember bond-line formulas) ...
Chem 222 Intro to Inorganic Chemistry Summer 2011 Problem Set 3
... The following MO diagram results. The strength of the bonding is the same (filled versus unfilled) but the correct relative MO ordering will affect its behavior as a ligand. Also note that for exams, you would be given the filling order for any heteroatomic molecular orbitals. ...
... The following MO diagram results. The strength of the bonding is the same (filled versus unfilled) but the correct relative MO ordering will affect its behavior as a ligand. Also note that for exams, you would be given the filling order for any heteroatomic molecular orbitals. ...
Odd number electron system. In a closed shell molecule with 2
... is the same for both the electrons in a molecular orbital. The results of a HartreeFock calculation on a closed shell molecule include the molecular orbital energies with out reference to spin. In an odd number electron molecule, the unpaired electron is taken to have α spin and clearly every α spin ...
... is the same for both the electrons in a molecular orbital. The results of a HartreeFock calculation on a closed shell molecule include the molecular orbital energies with out reference to spin. In an odd number electron molecule, the unpaired electron is taken to have α spin and clearly every α spin ...
Bonding in Simple Diatomic Molecules
... We use bonding models with various degrees of complexity to understand the interaction between atoms in a molecule and explain the geometry, physical properties, and chemical reactivity of the molecules. Lewis structures and hybrid orbitals treat bonds as being completely localized between two atoms ...
... We use bonding models with various degrees of complexity to understand the interaction between atoms in a molecule and explain the geometry, physical properties, and chemical reactivity of the molecules. Lewis structures and hybrid orbitals treat bonds as being completely localized between two atoms ...
chemical bond
... covalent bonds (sharing). i.e. must be a non-metal and a non-metal Molecular compound – a chemical compound whose simplest units are molecules. ...
... covalent bonds (sharing). i.e. must be a non-metal and a non-metal Molecular compound – a chemical compound whose simplest units are molecules. ...
3: Many electrons
... The orbital approximation predicts that all terms arising from a given configuration will be degenerate. In reality, they can be split into different terms. The energy of a configuration is not obtained simply as the sum of the occupied orbital energies! Consider a (π)2 configuration (see later for ...
... The orbital approximation predicts that all terms arising from a given configuration will be degenerate. In reality, they can be split into different terms. The energy of a configuration is not obtained simply as the sum of the occupied orbital energies! Consider a (π)2 configuration (see later for ...
Bent's rule
Bent's rule describes and explains the relationship between the isovalent hybridization of central atoms in molecules and the electronegativities of substituents. The rule was stated by Henry Bent as follows: ""Atomic s character concentrates in orbitals directed toward electropositive substituents"".The chemical structure of a molecule is intimately related to its properties and reactivity. Valence bond theory proposes that molecular structures are due to covalent bonds between the atoms and that each bond consists of two overlapping and typically hybridised atomic orbitals. Traditionally, p-block elements in molecules are assumed to hybridise strictly as spn, where n is either 1, 2, or 3. In addition, the hybrid orbitals are all assumed to be equivalent (i.e. the n+1 spn orbitals have the same p character). Results from this approach are usually good, but they can be improved upon by allowing hybridised orbitals with noninteger and unequal p character. Bent's rule provides a qualitative estimate as to how these hybridised orbitals should be constructed. Bent's rule is that in a molecule, a central atom bonded to multiple groups will hybridise so that orbitals with more s character are directed towards electropositive groups, while orbitals with more p character will be directed towards groups that are more electronegative. By removing the assumption that all hybrid orbitals are equivalent spn orbitals, better predictions and explanations of properties such as molecular geometry and bond strength can be obtained.Bent's rule can be generalized to d-block elements as well. The hybridisation of a metal center is arranged so that orbitals with more s character are directed towards ligands that form bonds with more covalent character. Equivalently, orbitals with more d character are directed towards groups that form bonds of greater ionic character.