Chemistry 101 Camp

In chemistry, a molecular geometry is the geometric configuration of the atoms that constitute a molecule. It is the arrangement of the atoms around one another in three-dimensional space along with the bond lengths and bond angles between the atoms. The molecule's molecular geometry can be deduced from the chemical structure of the molecule and the physical laws that govern the movement of molecules. From the molecular geometry, the properties of the molecule (such as bond length, bond angle, shape, and torsion) can be deduced.

In chemistry, shape is the three-dimensional arrangement of atoms in a molecule. The position of each atom is defined by the coordinates of its center, but the arrangement of the atoms in space may not be the same as the arrangement in space of the atoms of which it is composed. For example, water is composed of two hydrogen atoms bonded to a single oxygen atom, with the oxygen atom at the center of the H-O-H bond. In this case, the molecule is said to be in the "bent" shape, because the three atoms are not coplanar.

VSEPR is an acronym for valence shell electron pair repulsion theory. This theory is used to predict the molecular geometry of covalent molecules and ions.

In chemistry and physics, the molecular geometry describes the geometric arrangement of the atoms that form a molecule. It is determined by the nature of the chemical bonds between the atoms. These constraints result in the molecule adopting a regular geometric form, like a polyhedron or a sphere. The molecular geometry can be determined by various spectroscopic methods and diffraction methods.

In chemistry and physics, an expanded octet is a molecule with an electron configuration that is less than eight electrons from the noble gases. The first expanded octet configurations were discovered by Hückel in the 1930s, and the term was coined by Mulliken in the 1940s. The general concept of an expanded valence shell was developed by Mulliken in the 1930s and 1940s.

In chemistry, geometry describes the spatial arrangement of the atoms that constitute a molecule, as well as the bonds between atoms. Geometric molecular-orbital theory (GMO) is a computational method for calculating the molecular orbitals of large molecules. The method is based on the Hartree–Fock method, but extended to larger systems. The method is based on the assumption that the electrons in the molecule are localized.

The shape of a molecule is described by its electron density distribution, which is derived from the quantum mechanical wave function of the molecule. The wave function, in turn, determines the molecule's chemical, physical, and biochemical properties. The shape of a molecule may be described in terms of various types of geometries. For example, the molecule can be roughly spherical (as in a gas molecule), be planar (as in a molecule with sp-hybridized atoms), or have a complex structure (as in a protein).

In chemistry, covalent bonding is a type of chemical bonding that is characterized by the sharing of electron pairs between atoms. The number of shared pairs of electrons is equal to the number of electrons each atom contributes, or two electrons per shared pair. The term covalent bond dates from 1939.

In chemistry, hybridization is the concept of mixing atomic orbitals into new hybrid orbitals suitable for the pairing of nuclei. Hybrid orbitals are very useful in the explanation of molecular geometry and atomic bonding properties.

In chemistry, a hypervalent molecule is a molecule that has more than the maximum number of valence electrons that are allowed by the octet rule. The term hypervalent is used to describe molecules that have more than the canonical number of electrons (8) in their valence shell. The concept of hypervalent molecules was introduced by Ira Remsen and co-workers in 1952. Hypervalent molecules are also called "hypercoordinate" or "exceedingly nucleophilic" molecules.

In chemistry, a sigma bond (? bond) is a type of chemical bond that is formed between two atoms when the pair of electrons in the bond is shared equally between them.

In chemistry, a multiple bond is a chemical bond between two atoms involving more than two electrons. The most common multiple bonds are found between pairs of atoms of the same element, where two atoms share two electrons, giving each atom a total of eight electrons in its outer shell. A multiple bond between two atoms of the same element is often called a double bond. Multiple bonds are also possible between pairs of atoms of different elements, for example in the molecule carbon dioxide, where one carbon atom and one oxygen atom share two electrons.

In chemistry, a multiple bond is a chemical bond between two atoms involving more than two pairs of electrons. The most common multiple bonds are between one atom and two atoms, but others include three atoms, four atoms, and even more atoms. Multiple bonds are also possible between two atoms and between more than two atoms.

In chemistry, a molecular orbital (MO) is a mathematical function describing the wave-like behavior of an electron in a molecule. This function can be used to calculate chemical and physical properties such as the probability of finding an electron in any specific region. The term orbital was introduced by Robert S. Mulliken in 1932 as an abbreviation for one-electron orbital wave function. At an elementary level, it is used to represent the region of space in which the function has a significant amplitude. Molecular orbitals are usually constructed by combining atomic orbitals or hybrid orbitals from each atom of the molecule, or other molecular orbitals from groups of atoms. They can be quantized to describe the electron configurations of molecules and ions. Quantum mechanics can be used to predict the location of an electron in a molecule, based on the orbitals' quantized configurations.

In chemistry, a diatomic molecule is a molecule composed of two atoms. In other words, a molecule with this bonding number is a molecule with two atoms bonded together. The most common diatomic molecules are the diatomic elements, all of which are composed of two atoms. Examples include molecular nitrogen (N), molecular oxygen (O), and the diatomic halogens (Xe, Rn, and Fr). The prefix "di" is from the Greek ??, meaning "two".

In chemistry, a chemical bond is an attraction between atoms that enables the formation of chemical compounds. A chemical bond is usually depicted as a line connecting two chemical elements. A bond is an electrostatic force of attraction between atoms that enables the formation of chemical compounds. A bond is depicted as a line connecting two atoms. The bond strength is directly proportional to the bond length (the distance between the nuclei of the bonded atoms), and inversely proportional to the bond energy. This bond energy is the potential energy stored in the electrostatic force of attraction between the atomic nuclei.

In chemistry, bonding is the way in which atoms covalently or ionically associate through chemical bonds. A bond is an attraction between atoms that enables the formation of chemical compounds. The bond strength is the force required to break the bond.

In chemistry, a bond is a lasting attraction between atoms that enables the formation of chemical compounds. The bond may result from the electrostatic force of attraction between oppositely charged atoms, ionic bonding between atoms with positive and negative charges, or the sharing of electrons as in covalent bonding. The strength of chemical bonds varies considerably; the most covalent are those of single and double carbon-carbon bonds, while the most ionic are those of oxygen (O–O, O–H, O–S and O–Cl) and the most metallic are the bonds of sodium (Na–Na).

In chemistry, a chemical bond is a lasting attraction between atoms that enables the formation of chemical compounds. Atoms with a bond (also called a covalent bond) are held together by a force that is greater than the force that would be between two individual atoms. The bond is the fundamental cause of the chemical properties of the atoms. The term bond can also be applied to covalent bonds between molecules.

A homonuclear diatomic molecule is a molecule of one atom of each type, joined by covalent chemical bonds. The most abundant homonuclear diatomic molecules are the diatomic elements, which are composed of only one type of atom.

In chemistry, a molecular geometry is the geometric configuration of the atoms that constitute a molecule. It is the arrangement of the atoms around one another in three-dimensional space along with the bond lengths and bond angles between the atoms. The molecule's molecular geometry can be deduced from the chemical structure of the molecule and the physical laws that govern the movement of molecules. From the molecular geometry, the properties of the molecule (such as bond length, bond angle, shape, and torsion) can be deduced.

In chemistry, a molecular geometry is the geometric configuration of the atoms that constitute a molecule. It is the arrangement of the atoms around one another in three-dimensional space along with the bond lengths and bond angles between the atoms. The molecule's molecular geometry can be deduced from the chemical structure of the molecule and the physical laws that govern the movement of molecules. From the molecular geometry, the properties of the molecule (such as bond length, bond angle, shape, and torsion) can be deduced.

In chemistry, a molecular geometry is the geometric configuration of the atoms that constitute a molecule. It is the arrangement of the atoms around one another in three-dimensional space along with the bond lengths and bond angles between the atoms. The molecule's molecular geometry can be deduced from the chemical structure of the molecule and the physical laws that govern the movement of molecules. From the molecular geometry, the properties of the molecule (such as bond length, bond angle, shape, and torsion) can be deduced.

In chemistry, a molecular geometry is the geometric configuration of the atoms that constitute a molecule. It is the arrangement of the atoms around one another in three-dimensional space along with the bond lengths and bond angles between the atoms. The molecule's molecular geometry can be deduced from the chemical structure of the molecule and the physical laws that govern the movement of molecules. From the molecular geometry, the properties of the molecule (such as bond length, bond angle, shape, and torsion) can be deduced.