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TUTORIAL INSTRUCTIONS:
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MAKE NOTES AS NECESSARY
(ELEMENTS versus COMPOUNDS)
In a sample of the
element hydrogen all the
particles are hydrogen atoms
but in the compound carbon
monoxide the particles
contain both carbon and
oxygen atoms.
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(IONIC versus COVALENT BONDS)
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In the compound sodium
chloride one electron has
been transferred from each
sodium atom to each
chlorine atom, producing
positively charged sodium
cations and negatively
charged chloride anions.
(IONIC versus COVALENT BONDS)
However, in the
compound hydrogen
chloride, the hydrogen
atom and the chlorine atom
each supply one electron to
produce an electron pair
which they share.
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MAKE NOTES AS NECESSARY
(IONIC versus COVALENT BONDS)
In sodium chloride (ionic)
sodium has a positive
charge and chlorine has a
negative charge. In
hydrogen chloride (covalent)
hydrogen and chloride
share a pair of electrons.
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MAKE NOTES AS NECESSARY
(IONIC versus MOLECULAR COMPOUNDS)
A sample of sodium
chloride contains
+
alternating Na and Cl
ions; a sample of
hydrogen chloride
contains discrete HCl
molecules;
(IONIC versus MOLECULAR COMPOUNDS)
a sample of hydrogen
contains discrete H2
molecules; a sample of
chlorine contains
discrete Cl2 molecules.
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MAKE NOTES AS NECESSARY
(SINGLE COVALENT BOND)
The bond is
represented by a
single line drawn
between H and Cl.
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(DOUBLE COVALENT BOND)
The bond is
represented by
two parallel lines
between two Os.
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(TRIPLE COVALENT BOND)
The bond is
represented by
three parallel lines
between C and N.
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IA
IIA
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(LEWIS THEORY OF BONDING)
IIIA
IVA VA VIA VIIA VIIIA
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(LEWIS THEORY OF BONDING)
Note, however, that
hydrogen is a
nonmetal although
it has one valence
electron.
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(LEWIS THEORY OF BONDING)
Sodium is in Group
IA and has one valence
electron. It transfers one
electron to chlorine
which is in Group VIIA
and has seven valence
electrons.
(LEWIS THEORY OF BONDING)
As a result, sodium atoms
become positively charged
sodium cations and
chlorine atoms become
negatively charged chloride
anions so that they both
obey the Octet rule.
(LEWIS THEORY OF BONDING)
Hydrogen is in Group
IA and has one valence
electron. Chlorine is in
Group VIIA and has seven
valence electrons. Each will
supply one electron for
sharing and in this way
obey the Octet rule.
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(NONPOLAR versus POLAR COVALENT BONDS)
The covalent bonds in the
hydrogen molecule and in
the chlorine molecule are
nonpolar because in both
cases the atoms in the
bond are identical, and so
there is equal sharing of
electrons;
(NONPOLAR versus POLAR COVALENT BONDS)
hydrogen chloride,
however, is polar
because the atoms
differ in
electronegativity.
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(NONPOLAR versus POLAR MOLECULES)
Although the two
oxygen-oxygen bonds
in O3 are asymmetrically
arranged, the molecule is
nonpolar.
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(NONPOLAR versus POLAR MOLECULES)
BF3 is nonpolar
because the three
fluorine atoms are
symmetrically
arranged around the
central boron.
(NONPOLAR versus POLAR MOLECULES)
Similarly, SF6 is
nonpolar because
the S-F bonds are
symmetrically
arranged.
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(NONPOLAR versus POLAR MOLECULES)
Water is polar
because the two
hydrogen atoms
are asymmetrically
arranged around the
central oxygen.
(NONPOLAR versus POLAR MOLECULES)
ICl3 is polar
because the three
I-Cl atoms are
asymmetrically
arranged.
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(OCTET RULE DISOBEYED)
BeH2 has four
electrons around the
central beryllium and
BH3 has six electrons
around the central
boron.
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MAKE NOTES AS NECESSARY
(OCTET RULE DISOBEYED)
1
2
3
4
5
6
7
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(OCTET RULE DISOBEYED)
PI5 has ten electrons
around the central
phosphorus (Group VA)
and XeCl4 has twelve
electrons around the
central xenon (Group
VIIIA.)
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MAKE NOTES AS NECESSARY
(VALENCE BOND THEORY OF BONDING)
s and p
orbitals.
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(HYBRID ORBITALS)
One s orbital and one p
orbital together form two
linearly arranged sp
hybrid orbitals.
In BeH2, the central Be
bonds with sp orbitals.
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(HYBRID ORBITALS)
One s orbital and two p
orbitals together form three
2
sp hybrid orbitals in a
trigonal planar arrangement;
In BF3, the central B bonds
2
with sp orbitals.
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(HYBRID ORBITALS)
One s orbital and three p
orbitals together form four
3
tetrahedrally-arranged sp
hybrid orbitals.
In CH4, the central C
3
bonds with sp orbitals.
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(HYBRID ORBITALS)
One d orbital, one s
orbital and three p orbitals
3
together form five dsp
hybrid orbitals in trigonal
bipyramid arrangement.
In PI5, the central P
3
bonds with dsp orbitals.
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(HYBRID ORBITALS)
Two d orbitals, one s
orbital and three p orbitals
together form six
octahedrally-arranged
2
3
d sp hybrid orbitals.
In SF6, the central S bonds
2
3
with d sp orbitals.
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MAKE NOTES AS NECESSARY
(MOLECULAR GEOMETRY)
A region of high
electron density may
be a single bond, a
double bond, a triple
bond or a nonbonding
electron pair.
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MAKE NOTES AS NECESSARY
(ELECTRONIC and MOLECULAR GEOMETRY)
In BeH2 there are two pairs of
valence electrons around the
central Be (Group IIA) and so the
electronic geometry is linear.
Both electron pairs are involved in
bonding and so the shape, or
molecular geometry, is also
linear.
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(ELECTRONIC and MOLECULAR GEOMETRY)
In BF3 there are three pairs of
valence electrons around the
central B (Group IIIA) and so the
electronic geometry is trigonal
planar. All the electron pairs are
involved in bonding and so the
shape, or molecular geometry,
is also trigonal planar.
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(ELECTRONIC and MOLECULAR GEOMETRY)
In CH4 there are four pairs of
valence electrons around the
central C (Group IVA) and so the
electronic geometry is
tetrahedral. All the electron pairs
are involved in bonding and so the
shape, or molecular geometry, is
also tetrahedral.
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(ELECTRONIC and MOLECULAR GEOMETRY)
In PI5 there are five pairs of
valence electrons around the
central P (Group VA) and so the
electronic geometry is trigonal
bipyramid. All the electron pairs
are involved in bonding and so the
shape, or molecular geometry,
is also trigonal bipyramid.
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(ELECTRONIC and MOLECULAR GEOMETRY)
In SF6 there are six pairs of
valence electrons around the
central S (Group VIA) and so the
electronic geometry is
octahedral. All the electron pairs
are involved in bonding and so the
shape, or molecular geometry,
is also octahedral.
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MAKE NOTES AS NECESSARY
(ELECTRONIC and MOLECULAR GEOMETRY)
O3 has three sp2 hybrid
orbitals around the central O,
giving it trigonal planar
electronic geometry. One of
these orbitals is nonbonding
and so its molecular
geometry is angular, or
bent.
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(ELECTRONIC and MOLECULAR GEOMETRY)
3
sp
NH3 has four
hybrid
orbitals around the central
N, giving it tetrahedral
electronic geometry. One of
these orbitals is nonbonding
and so its molecular
geometry is trigonal
pyramid.
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(ELECTRONIC and MOLECULAR GEOMETRY)
3
sp
H2O has four
hybrid
orbitals around the central
O, giving it tetrahedral
electronic geometry. Two of
these orbitals are
nonbonding and so its
molecular geometry is bent,
or angular.
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OH
(ELECTRONIC and MOLECULAR GEOMETRY)
3
sp
has four
hybrid
orbitals around the central
O, giving it tetrahedral
electronic geometry. Its
molecular geometry is
linear because there are
only two atoms in the
molecule.
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(ELECTRONIC and MOLECULAR GEOMETRY)
3
dsp
SF4 has five
hybrid
orbitals around the central
S, giving it trigonal
bipyramid electronic
geometry. One of these
orbitals is nonbonding and
so its molecular geometry
is see-saw.
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(ELECTRONIC and MOLECULAR GEOMETRY)
3
dsp
ICl3 has five
hybrid
orbitals around the central I
(Group VIIA), giving it
trigonal bipyramid
electronic geometry. Two of
these orbitals are nonbonding
and so its molecular geometry
is see-saw.
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(ELECTRONIC and MOLECULAR GEOMETRY)
3
dsp
XeH2 has five
hybrid
orbitals around the central
Xe, giving it trigonal
bipyramid electronic
geometry. Three of these
orbitals are nonbonding and
so its molecular geometry is
linear.
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(ELECTRONIC and MOLECULAR GEOMETRY)
2
3
d sp
BrF5 has six
hybrid
orbitals around the central
Br, giving it octahedral
electronic geometry. One of
these orbitals is nonbonding
and so its molecular
geometry is square
pyramid.
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(ELECTRONIC and MOLECULAR GEOMETRY)
2
3
d sp
XeCl4 has six
hybrid orbitals around the
central Xe, giving it
octahedral electronic
geometry. Two of these
orbitals are nonbonding and
so its molecular geometry is
square planar.
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VALENCE BOND THEORY
SUMMARIZATION TABLE
No. of
electron
pairs
Hybrid- Electronic
ization geometry
No. of
lone
pairs
No. of
bonds
Molecular
geometry
Example
and polarity
2
sp
linear
0
2
linear
BeH2
nonpolar
3
sp2
trigonal
planar
0
3
trigonal
planar
BF3
nonpolar
1
2
angular
O3
nonpolar
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VALENCE BOND THEORY SUMMARIZATION TABLE
(cont’d)
No. of
electron
pairs
Hybrid- Electronic
ization geometry
4
sp3
No. of
lone
pairs
No. of Molecular
bonds geometry
tetrahedral 0
4
1
3
2
2
Example
and polarity
tetrahedral CH4
nonpolar
NH3
trigonal
polar
pyramid
angular or H2O
bent
polar
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VALENCE BOND THEORY SUMMARIZATION TABLE
(cont’d)
No. of
Hybridi- Electronic
electron zation
geometry
pairs
5
dsp3
No. of
lone
pairs
No. of Molecular
bonds geometry
trigonal
0
bipyramid
5
1
4
2
3
3
2
Example
and polarity
trigonal
PCl5
bipyramid nonpolar
see-saw
SF4
polar
T-shaped ICl3
polar
linear
XeF2
nonpolar
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VALENCE BOND THEORY SUMMARIZATION TABLE
(cont’d)
No. of
Hybridi- Electronic
electron zation
geometry
pairs
6
d2sp3
octahedral
[END OF TUTORIAL]
No. of
lone
pairs
No. of Molecular
bonds geometry
0
6
1
5
2
4
Example
and polarity
octahedral SF6
polar
square
BrF3
pyramid
nonpolar
square
XeF4
planar
polar
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