Αποτελέσματα Αναζήτησης
Give an example. For each of the following compounds, draw a Lewis Structure, determine the AXE formula, steric number, electronic geometry, molecular geometry, bond angles, and hybridizations.
Analyze the structure of dichlorodifluoromethane, or CCl2F2 by 1) drawing the Lewis structure, 2) performing a geometry optimization using Maestro, and 3) measuring the bond lengths and bond angles listed below. Use the same DFT method as the last example (B3LYP-D3/6-31G**). Lewis-Dot Structure of. CCl2F2.
Use one toothpick for single bonds, two toothpicks for double bonds, and three toothpicks for triple bonds. c. Use your protractor to get the bond angles as close as possible – it’s hard to do with playdough and toothpicks, that’s ok!
1) How are ionic bonds and covalent bonds different? Ionic bonds result from the transfer of electrons from one atom to another; Covalent bonds result from two atoms sharing electrons. 2) Describe the relationship between the length of a bond and the strength of that bond.
Example: Sodium has 11 electrons. This gives sodium the following configuration: Na = 1s22s22p63s1. It has 3 energy levels and 4 orbitals holding the 11 electrons. Spin. Within an orbital, electrons pair up with opposite spin so that the atom is as stable as possible. Electrons in the same orbital must have opposite spins.
Ammonia and boron trifluoride react to form a compound NH3BF3 which contains a dative covalent bond. Each of the molecules, NH3 and BF3, has a different feature of its electronic structure that allows this to happen. Use these two different features to explain how a dative covalent bond is formed. (2
Molecules and ions possess two types of electron pairs: Bonding pairs (the two shared electrons in a covalent bond) Lone pairs (two electrons in a pair not involved in bonding – also known as non-bonding pairs). These electron pairs will repel each other as far as possible.
