Properties of Ethanol
Name of Molecule |
Ethanol |
Molecular Geometry |
Tetrahedral |
Hybridization |
sp3 |
Molecular Formula |
C2H5OH |
Molecular Weight |
46.069 g/mol |
Bond Pairs |
8 |
Lone Pairs |
2 |
Lewis structure |
in Infographic |
absolute alcohol – alcohol - cologne spirit - drinking alcohol - ethylic alcohol – EtOH - ethyl alcohol - ethyl hydrate - ethyl hydroxide – ethylol - grain alcohol – hydroxyethane - methylcarbinol
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Definitions
Molecular Geometry: Molecules have a balanced geometric shape, the bonds have a certain
length and angle as well, and the laws of quantum mechanics determine this. The
chemical equation and the structural equation of a molecule are the two most
important factors in determining its properties, especially its activity. The
structure of the molecule also plays an important role in determining polarity,
state of matter, colour, magnetism, taste, and many other properties.
Hybridization: Hybridization in chemistry is
the process of mixing, merging, or combining two or more different orbitals of
electrons in the same atom. And they are close in energy to produce new hybrid
orbitals of equal length and energy. Hybridization occurs in the same single
atom and produces orbitals that are equivalent in shape, length and energy. The
atom must be excited. The orbitals must be close in energy, such as 2s with 2p
or 4s with 3d. The number of hybrid orbitals is equal to the number of pure
orbitals involved in the hybridization. The hybrid orbitals are more prominent
outward so that their ability to overlap is stronger than that of normal
orbitals.
Molecular Formula: A chemical formula is a brief way
of expressing the number and type of atoms that make up a particular chemical
compound. It expresses each element with its chemical symbol, and writes
directly next to it the number of atoms in the molecule of this compound. If
there is more than one atom of the same element in the molecule, the number of
atoms is written to the bottom right of the element. For non-molecular
substances, the bottom number represents the descriptive formula. The chemical
formula that is used for a series of compounds that differ from each other by
fixed units is called the "general formula". This series is called a
homogeneous series, and its number is called the homogeneity symbol.
Molecular Weight: in chemistry of a substance
(sometimes called the molecular weight of a substance) is the mass of a
molecule of that substance, relative to a unit of atomic mass (u which equals
1/12 of the mass of an n-carbon-12 atom) (simply: molecular mass is the sum of
the weights atoms in a molecule). Molecular mass can be calculated as the sum
of the atomic weights of the atoms in any molecule. Molecular mass can also be
measured directly with a mass spectrometer. In mass spectrometry, the molecular
mass of small molecules (less than about 200 atoms of a given element) is
minute, ie the sum of the most abundant isotopes of that element. For larger
molecules, it is average, or it is calculated using the molecular mass of the
element or using the periodic table, where there are statistics for the
distribution of atoms represented by isotopes of the molecule.
Bond Pairs: A bond pair is a pair of electrons present in a chemical bond. As we
know, one bond is always made of two electrons paired together. Together, these
two electrons are called a bond pair. Bond pairs can be seen in covalent
compounds and coordination compounds.
Lone Pairs: A non-bonding or lone pair is a pair of electrons in an atom without
bonding or sharing with another atom. It often has a negative polarity due to
its high charge density. This pair is used to make coordination bonds. For
example, in the manufacture of hydronium, H3O +, ions are present when acids
are dissolved in water and the oxygen atom gives a lone pair to the hydrogen
ion.
Lewis structure: A Lewis structure or Lewis representation (also known as electron raster diagram, Lewis raster formula, Lewis point structure, or point electron structure) is a two-dimensional diagram used in chemistry to show the bonding between atoms of a molecule and the lone electron pairs that may be present in this molecule. It is primarily used to show the relative positions of the different atoms with respect to each other and the formations of the valence bonds that bring together the different atoms of the compound as well as the position of electrons with respect to the atoms of the molecule. The Lewis structure can be plotted for any molecule that contains a covalent bond in addition to the complexes.
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