W2 General Chemistry Flashcards
are forces of attraction that exist
between a positive ion and a negative
ion or between molecules.
Chemical Bonds
- an atom other than hydrogen tends to
form bonds until it is surrounded by
eight electrons.
Octet Rule
According to ______ * atoms combine to achieve a more stable
electron configuration.
GLIBERT LEWIS
Maximum stability results when an atom is _______ with a noble gas
isoelectronic
3 Types of Interatomic Bond
*Ionic bond
* Covalent bond
* Metallic bond
Ionic bond aka ____
Electrovalent Bond
formed by the transfer of electrons
from an atom of low ionization
energy (alkali and alkaline earth
metal) to a more electronegative
element (halogen and oxygen)
IONIC BOND
bond in which two electrons are
shared between atoms
Covalent Bond
–formed when
electrons are shared equally
between two atoms with the same
or almost the same
electronegativity
Covalent compounds
Non-bonding pairs are called ____
LONE PAIRS
pairs of valence electrons that
are not involve in covalent bond formation
LONE PAIRS
This is formed from sharing of electrons
between two atoms with different
electronegativity.
Polar Covalent Bond
the ability of an atom to attract toward itself
the electrons in a chemical bond.
ELECTRONEGATIVITY
property that helps us distinguish a nonpolar
covalent bond from a polar covalent bond
ELECTRONEGATIVITY
A bond formed wherein one
furnishes both the bonding pair of
electrons.
Coordinate Covalent Bond
consists of group of cations held in
a fixed position in the metal and
the valence electrons which are
free to move about among the
different electron clouds.
Metallic Bond
attractive
forces between molecules
Intermolecular forces
Very weak forces of
attraction between non-polar molecules
Van der Waals
is an attractive force
that exists between the hydrogen of one
molecule and the more electronegative
portion of another molecule
Hydrogen Bond
is an attractive force
between polar molecules
Dipole Bond
The use of two or more Lewis Structures to represent a particular molecule.
Resonance
– is one of the two or
more Lewis Structures for a single molecule
that cannot be represented accurately by only one Lewis Structure.
Resonance Structure
Two polar molecules align so that
OPPOSITE CHARGES are matched
(electrostatic attraction)
DIPOLE-DIPOLE
A dipole can induce (cause) a temporary dipole to form in a non-
polar molecule
The molecules then line up to
match opposite charges
Dipole-Induced Dipole
A temporary dipole forms in a non-
polar molecule which leads to a temporary dipole to form in
ANOTHER non-polar molecule
Dispersion Forces
is the ONLY
intermolecular attraction that
occurs between non-polar
molecules
Dispersion
simply shows the
exact number of each type of atom present. It tells you nothing
about the bonding within the compound
MOLECULAR FORMULA
gives the simplest
possible whole number ratio of the different types of atom within
the compound
EMPIRICAL FORMULA
formula that shows the simplest whole number ration
EMPIRICAL FORMULA
is also text-based here each carbon
atom is listed separately with atoms attached to it following an exception is cyclic parts of molecules example benzene where
the carbons are grouped
CONDENSED FORMULA
a displayed formula shows all of the atoms and all of the bonds present in an organic compound the bonds are represented as
lines
DISPLAYED FORMULA
Similar to displayed formula not all bonds are shown although all atoms are still indicated using subscript numbers. Carbon- hydrogen bonds are often simplified
STRUCTURAL FORMULA
formula which shows how the molecules are bonded to one another in a molecule
STRUCTURAL FORMULA
most hydrogen atoms are omitted and lines and or vertices represent carbons. Functional groups and atoms other than carbon or hydrogen are still shown. Easiest to draw
and commonly used
SKELETEAL FORMULA
