Ch 6 Section 1 Flashcards
A chemical bond is a mutual electrical attraction between the
Nuclei of valence electrons of different atoms that binds the atoms together
Most atoms are at relatively high
Potential energy
Nature favors arrangements in which potential energy is
Minimized
Most atoms are less stable existing by
Themselves than when they are combined
By bonding with each other atoms decrease in
Potential energy creating more stable arrangements of matter
When atoms bind their valence electrons are
Redistributed in ways that make the atoms more stable
The way electrons are redistributed determined the
Type of bonding
Main group metals tend to lose electrons to
Form positive ions
Nonmetals tend to gain electrons to form
Negative ions
Ionic bonding: chemical bonding that results from the
Electrical attraction between cations and anions
In purely ionic bonding atoms completely
Give up electrons to other atoms
Atoms joined by covalent bonding
Share electrons
Covalent bonding results from the
Sharing of electron pairs between two atoms
In a purely covalent bond the shared electrons are
Owned equally by the two bonded atoms
The degree to which bonding between atoms of two elements is ionic or covalent can be estimated by calculating the
Difference in the elements’ electronegativities
Between 0 to 0.3 in electronegativity difference: the hind is
Nonpolar covalent
Between 0.3 and 1.7 in electronegativity difference: vine is
Polar covalent.
Between 1.7 and 3.3 in electronegativity difference: bond is
Ionic
Bonding between two atoms of the same element is
Completely covalent
Nonpolar covalent bond: a covalent bond in which the bonding electrons are shared
Equally by bonded atoms, resulting in a balanced distribution of electrical charge
In bonds with significantly different electronegativities the electrons are more strongly
Attracted by the more electronegative atom
Polar bonds have an
Uneven distribution of charge
A polar covalent bond: a covalent bond in wh in the bonded atoms have an
Unequal attention for the shared electrons
Atoms seldom exist as
Independent particles in nature