Regents Chemistry
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Transcript Regents Chemistry
Regents Chemistry
• Agenda
– Start Chapter 12 - Chemical Bonding
– Bonding worksheet
– HW: Finish worksheet
What is bonding?
• Bonding is the “glue” that hold two or more
elements together
• This “glue” is most likely formed as a result
of a chemical reaction
• Bonding and molecular structure play a
central role in determining the course of
chemical reactions
What is a bond?
• A bond can be thought of as a force that
holds groups of two or more atoms
together and makes them function as a
unit
• Example : water
O
H
H
Bonds require energy to break
and release energy when made
Bonds and Energy
• BREAKING BONDS requires energy
– You Must Heat Wood to get it to react with
oxygen (ENDOTHERMIC)
• MAKING BONDS releases energy
– Once the bonds are broken, they form new
products and this process releases heat
(EXOTHERMIC)
Types of bonds
• Ionic bonds - typically formed between
metals and nonmetals
• Covalent bonds - typically formed between
nonmetals
• Metallic bonds - formed between metals
Ionic Bonds
• Ionic substances are formed when an
atom that loses electrons relatively easily
reacts with an atom that “wants” electrons
• We call these substances ionic
compounds and result when a metal
reacts with a nonmetal
• Ionic bonds are strong
Ionic Bonds
• Na and Cl
– Na is a metal and likes to lose one electron
– Cl is a nonmetal and likes to gain one electron
– the final ionic compounds is NaCl
Na+ + Cl-
NaCl
The electrostatic interaction
keeps them together!
Ionic Bonds
• Na looses an electron and chlorine gains
it!
Na
Cl
• They do this to achieve an octet!
Covalent Bonds
• Covalent Bonds
– exist between nonmetals bonded together
– form when atoms of nonmetals share
electrons
– electrons can be shared equally or unequally
Covalent Bonds Con’t
• Covalent bonds that have elements that
share electrons equally are simply said to
have a covalent type of bond
• Covalent bonds that share electrons
unequally are said to have a polar
covalent type of bond
• The unequal sharing results in a bond
polarity
H
+
F-
Metallic Bonds
• Metallic bonds exist between metals
• Occur when two metals, usually the same
metal, are bonded together
Regents Chemistry
• Electronegativity
How can we tell really tell which
type of bond we have?
• Electronegativity – is the relative ability
of an atom in a molecule to attract
shared electrons to itself
• This tells us what type of bond we have;
– Covalent, polar covalent or ionic
• Electronegativity values are determined
by measuring the polarities of bonds
between various elements to determine
a specific value for each element
Electronegativity
• Electronegativity values for each element
are obtained by using the Periodic Table
• In fact, there is a general trend in
electronegativity we observe in the
Periodic Table
• Electronegativity values increase across
and up the Periodic Table
– See table on pg. 332
Electronegativity
• We take the difference between the
electronegativity values to determine
exactly what type of bond exists, in
essence the polarity of the bond
See table 12.1
Determining Bond Polarity
• If the difference between the
electronegativity values is:
– 0.0 – 0.5: covalent bond (equal sharing)
– 0.6 – 1.6: polar covalent bond (unequal
sharing)
– 1.7 – up: ionic bond (transferring electrons)
Examples
• Use your Reference Tables to determine
the difference in electronegativity values
and the type of bond for each of the
following:
– H-H
– H-Cl
– H-O
– H-S
• H-F
• NaCl
• O2
• KBr
Worksheet
Regents Chemistry
• Intro to valence electrons
Electrons in an atom
• Electrons surround the nucleus of an atom
in specific energy levels or shells
• Each level can hold only a certain amount
of electrons
• It is an atoms ability to the lose, gain or
share electrons from its outer shell that
determine its reactivity
The outer shell
• The outer shell in an atom contains the
valence electrons
• Valence electrons can be lost, gained or
shared to have eight electrons in the outer
shell
• Each group on the table tells the number of
valence electrons
Periodic Table
• Groups 1, 2, 13, 14, 15, 16, 17, 18 have
1,2,3,4,5,6,7,8 valence electrons,
respectively
• We will not consider the transition metals
• See periodic table
Sharing to reach the Octet Rule
• The octet rule states that an atom cannot
have more than 8 electrons in its outer
shell
• Valence electrons are lost, gained or
shared with other atoms to attain 8
electrons in the outer shell
• Eight valence electrons means a filled and
happy shell - like the noble gases
Nonmetals share
• Nonmetals share electrons to reach eight
valence electrons
• Single, double and triple bonds can be
formed by sharing electrons
Metals + non-metals =
lose/gain e• metals and nonmetals interact by losing
and gaining electrons to reach 8 electrons
(filled outer shell)
• The oxidation states on the periodic table
represent this desire to move electrons
• ex: K+ want to lose 1 electron to reach
noble gas configuration of eight electrons
Lewis structures: your
assignment
• The reading and problems focus on
drawing Lewis structures
• Lewis structures are a means to represent
bond formation between atoms
• Covalent bonded compounds have
different Lewis structures than Ionic
bonded compounds
Example of a Lewis Structure
C
H
H
H C H
H
CH4
Covalent bonds
Regents Chemistry
• Lewis Structures
Lewis Structures
The Lewis Structure is a representation of a
molecule that shows how the valence
electrons are arranged among the atoms in
a molecule
We used dots around the elemental symbol
to represent the valence electrons
C
Single Lewis Structure - Practice
Draw four lone electrons first (if necessary)
them pair them up
Draw Lewis Structures for the following
atoms
Na
Be
Al
Br
Lewis Structures for Ionic
Compounds
For Lewis Structures of ionic bonds the
atoms are not joined but draw next to each
other
example:
KBr
+
K [
Potassium loses an
electron to achieve
the noble gas configuration
of Argon
Br ]
Bromine gains an
electron to achieve
the noble gas configuration
of Krypton
Lewis Structures – Covalent Bonds
Hydrogen forms stable molecules when it shares
two electrons
Two electrons fill Hydrogen’s valence shell
Helium does not form bonds because its valence
shell is already filled; it is a noble gas
Second row non-metals Carbon through Fluorine
from stable molecules when surrounded by eight
electrons – the Octet Rule
Lewis Structures – Covalent Bonds
Valence electrons in covalent bonds can
either be bonding pairs, if involved directly
in the bond or lone pairs if not involved in
the bond
Writing Lewis Structures - Rules
Obtain the total sum of the valence electrons from
all of the atoms
Use one pair of electrons to form a bond between
each pair of bound atoms. For convenience, a line
(instead of a pair of dots) can be used to indicate
each pair of bonding electrons
Arrange the electrons to satisfy the duet rule for
hydrogen and the octet rule for second row
non metals
Lewis Structures – Covalent Bonds
Examples
PH
3
H
l
H– P –H
••
Step 1) 8 total valence e- total
Step 2) Draw one pair of
electrons per bond
8-6 = 2 left
Step 3) Arrange the remaining
electrons according to
octet rule
H
H P H
Lewis Structures – Covalent Bond
Practice Examples
HBr
..
H:Br:
··
CF4
Worksheet
Regents Chemistry
– Ionic Lewis Structures
– Multiple bonds in Lewis Structures
– Polyatomic ion Lewis Structures and
Resonance
Lewis Structures for Ionic
Compounds
For Lewis Structures of ionic bonds the atoms
are not joined but draw next to each other
example:
KBr
+
K [
Br ]
Potassium loses an
electron to achieve
the noble gas configuration
of Argon
Bromine gains an
electron to achieve
the noble gas configuration
of Krypton
Examples of Ionic Lewis
Structures
Draw Lewis Structures for the following:
NaCl
LiBr
KI
Multiple Bonds and Lewis
Structures…review first
We have seen how to draw Lewis Structures
for molecules with single bonds
• For example
NH3
1. Sum the total
valence e2. Subtract number
of bonding e3. Place remaining
valence e-
8 total valence e3 bonds x 2e- = 6 bonding
2 e- left over
H N H
H
Multiple Bonds
Between atoms of the same element
Example
• Oxygen
O O
O=O
Just
O = O
Also a Lewis Structure
is called a structural model
Example of Multiple Bonds
Nitrogen
N N
N
N
We now meet the octet rule!
Multiple Bonds
Between atoms of different elements
CO2
O
C
O
O = C = O
We must use double bonds to meet the octet rule!
Lewis Structures for Polyatomic
Ions and Resonance Structures
Read pg. 344 (bottom) to 349 and answer
questions a-g in example
12.4 (pg. 347) and a-i in the Self Check
exercise 12.4 (pg. 348)