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- https://chem.libretexts.org/Courses/University_of_California_Irvine/UCI%3A_General_Chemistry_1A_(OpenChem)/116Review_Lecture_-_Constructive_and_Destructive_Interference(OpenChem)
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Coordination_Chemistry/Structure_and_Nomenclature_of_Coordination_Compounds/Isomers/Stereoisomers_of_Complex_Metal_ComplexesStereoisomers are isomers that have the same molecular formula and ligands, but differ in the arrangement of those ligands in 3D space.
- https://chem.libretexts.org/Bookshelves/General_Chemistry/ChemPRIME_(Moore_et_al.)/07%3A_Further_Aspects_of_Covalent_Bonding/7.05%3A_Multiple_Bonds_and_Molecular_ShapesAlso, because of the “fatness” of the double bond, squeezing the C—H bond pairs together, we expect the H―C―H angle to be slightly less than 120°. Experimentally it is found to have the value of 117°....Also, because of the “fatness” of the double bond, squeezing the C—H bond pairs together, we expect the H―C―H angle to be slightly less than 120°. Experimentally it is found to have the value of 117°. The complete lewis diagram shows central "N" sharing two pairs of electrons with one "O" and one pairs of electrons with "C" "L". There are two lone pairs on the oxygen, three lone pairs on the chlorine, and one lone pair on the nitrogen.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Molecular_Geometry/Trigonal_Bipyramidal_Molecular_GeometryAX 5 Shape: trigonal bipyramidal Steric Number: Lone Pairs: Polar/NonPolar: sp 3 d PCl 5 , SbF 5 NOTES: This molecule is made up of 5 sp 3 d hybrid orbitals. Three orbitals are arranged around the equ...AX 5 Shape: trigonal bipyramidal Steric Number: Lone Pairs: Polar/NonPolar: sp 3 d PCl 5 , SbF 5 NOTES: This molecule is made up of 5 sp 3 d hybrid orbitals. Three orbitals are arranged around the equator of the molecule with bond angles of 120 o . Two orbitals are arranged along the vertical axis at 90 o from the equatorial orbitals. The shape of the orbitals is trigonal bipyramidal. Since there is an atom at the end of each orbital, the shape of the molecule is also trigonal bipyramidal.
- https://chem.libretexts.org/Bookshelves/Inorganic_Chemistry/Supplemental_Modules_and_Websites_(Inorganic_Chemistry)/Molecular_Geometry/Trigonal_Planar_______Molecular_GeometryAX 3 Shape: trigonal planar Steric Number: Lone Pairs: Polar/NonPolar: NonPolar Hybridization: sp 2 Examples: BF 3 , CO 3 2 - NOTES: This molecule is made up of 3 equally spaced sp 2 hybrid orbitals a...AX 3 Shape: trigonal planar Steric Number: Lone Pairs: Polar/NonPolar: NonPolar Hybridization: sp 2 Examples: BF 3 , CO 3 2 - NOTES: This molecule is made up of 3 equally spaced sp 2 hybrid orbitals arranged at 120 o angles. The shape of the orbitals is planar triangular. Since there is an atom at the end of each orbital, the shape of the molecule is also planar triangular. Contributors and Attributions Charles Ophardt, Professor Emeritus, Elmhurst College; Virtual Chembook
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/09%3A_Covalent_Bonding/9.15%3A_Molecular_Shapes_-_Lone_Pair(s)_on_Central_AtomThis page explains the impact of lone pairs of electrons on molecular geometry, noting that they alter electron domain arrangements. It highlights examples like ammonia (NH3), which has a tr...This page explains the impact of lone pairs of electrons on molecular geometry, noting that they alter electron domain arrangements. It highlights examples like ammonia (NH3), which has a trigonal pyramidal shape due to one lone pair, and water (H2O), which has a bent shape with two lone pairs. Additionally, it discusses sulfur tetrafluoride (SF4) which displays a distorted tetrahedral geometry.
- https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/09%3A_Covalent_Bonding/9.22%3A_Hybrid_Orbitals_-_spThis page explains sp3 hybridization in chemistry, detailing how carbon achieves four equivalent bonds in methane (CH4 despite having only two unpaired electrons. It emphasizes the form...This page explains sp3 hybridization in chemistry, detailing how carbon achieves four equivalent bonds in methane (CH4 despite having only two unpaired electrons. It emphasizes the formation of hybrid orbitals through the mixing of atomic orbitals to create tetrahedral geometry, which enables carbon to form four covalent bonds, enhancing the stability of its compounds.
- https://chem.libretexts.org/Courses/University_of_Florida/CHM2047%3A_One-Semester_General_Chemistry_(Kleiman)/05%3A_Molecular_Structure_and_Geometry/5.04%3A_VSEPR_Geometry/5.4.01%3A_5.4.1-Limitations_of_VSPERThe VSEPR model also fails to predict the structure of certain compounds because it does not take relative sizes of the substituents and stereochemically inactive lone pairs into account. As a result,...The VSEPR model also fails to predict the structure of certain compounds because it does not take relative sizes of the substituents and stereochemically inactive lone pairs into account. As a result, VSEPR does not give correct geometries for these transitional metal complex compounds.. For example, [SeCl 6 ] 2- , [TeCl 6 ] 2- ,and [BrF 6 ] - are predicted to adopt pentagonal bipyramidal geometries according to VSEPR since the central atom can have seven electron pairs.
- https://chem.libretexts.org/Courses/University_of_North_Texas/UNT%3A_CHEM_1410_-_General_Chemistry_for_Science_Majors_I/Text/07%3A_Further_Aspects_of_Covalent_Bonding/7.03%3A_The_Shapes_of_MoleculesThe location in three-dimensional space of the nucleus of each atom in a molecule defines the molecular shape or molecular geometry. Molecular shapes are important in determining macroscopic propertie...The location in three-dimensional space of the nucleus of each atom in a molecule defines the molecular shape or molecular geometry. Molecular shapes are important in determining macroscopic properties such as melting and boiling points, and in predicting the ways in which one molecule can react with another. We will concentrate on several rules based on Lewis diagrams which will allow you to predict molecular shapes.
- https://chem.libretexts.org/Courses/Prince_Georges_Community_College/CHEM_2000%3A_Chemistry_for_Engineers_(Sinex)/Unit_2%3A__Molecular_Structure/Chapter_5%3A_Molecular_Geometry/Chapter_5.1%3A_Predicting_the_Geometry_of_MoleculesFrom the BP and LP interactions we can predict both the relative positions of the atoms and the angles between the bonds, called the bond angles The angle between bonds.. Using this information, we ca...From the BP and LP interactions we can predict both the relative positions of the atoms and the angles between the bonds, called the bond angles The angle between bonds.. Using this information, we can describe the molecular geometry The arrangement of the bonded atoms in a molecule or a polyatomic ion in space., the arrangement of the bonded atoms in a molecule or polyatomic ion.
- https://chem.libretexts.org/Courses/Northern_Alberta_Institute_of_Technology/CHEM1130_Principles_in_Chemistry_I/3%3A_Chemical_Bonding._Solubility/3.6%3A_Predicting_the_Geometry_of_MoleculesFrom the BP and LP interactions we can predict both the relative positions of the atoms and the angles between the bonds, called the bond angles The angle between bonds.. Using this information, we ca...From the BP and LP interactions we can predict both the relative positions of the atoms and the angles between the bonds, called the bond angles The angle between bonds.. Using this information, we can describe the molecular geometry The arrangement of the bonded atoms in a molecule or a polyatomic ion in space., the arrangement of the bonded atoms in a molecule or polyatomic ion.
