introduction to bonding topic #13 essential question: what are all the differences and similarities...
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Introduction to BondingTopic #13
Essential Question: What are all the differences and similarities between covalent bonds and ionic bonds?
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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
OH H
Bonds require energy to break and release energy when made
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Types of bonds
• Ionic bonds - typically formed between metals and nonmetals
• Covalent bonds - typically formed between nonmetals
• Metallic bonds - formed between metals
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Ionic Bonds
• Ionic bonding results from the transfer of electrons. Then, the opposite charges attract each other.
• Ionic bonds are strong
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Ionic Bonds
• Na and Cl– Na is a metal and likes to lose one electron
and form a +1 ion.– Cl is a nonmetal and likes to gain one electron
and form a -1 ion.
– the final ionic compounds is NaCl
Na+ Cl-+ NaClThe electrostatic interaction keeps them together!
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Ionic Bonds
•They do this
to achieve an
octet!
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Covalent Bonds
• Covalent Bonds– exist between nonmetals bonded together– form when atoms of nonmetals share
electrons– electrons can be shared equally or unequally
– The unequal sharing results in polar molecules
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Metallic Bonds
• Metallic bonds exist between metals
• Occur when two metals, usually the same metal, are bonded together
• “sea of electrons”• “delocalized electrons”
• ttp://www.youtube.com/watch?v=XAnTCYZPJsE&feature=bf_next&list=PLBFE28832E577A62B
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Regents Chemistry
• Electronegativity
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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
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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
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• 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
Electronegativity
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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)
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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
• KBrWorksheet
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Regents Chemistry
• Intro to valence electrons
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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
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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
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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
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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
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Nonmetals share
• Nonmetals share electrons to reach eight valence electrons
• Single, double and triple bonds can be formed by sharing electrons
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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
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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
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Example of a Lewis Structure
CH H
H
HC
H
CH4 Covalent bonds
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Regents Chemistry
• Lewis Structures
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Lewis StructuresLewis Structures The Lewis Structure is a The Lewis Structure is a
representation of a molecule that representation of a molecule that shows how the valence electrons shows how the valence electrons are arranged among the atoms in are arranged among the atoms in a moleculea molecule
We used dots around the We used dots around the elemental symbol to represent the elemental symbol to represent the valence electronsvalence electronsC
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Single Lewis Structure - Single Lewis Structure - PracticePractice Draw four lone electrons first (if Draw four lone electrons first (if
necessary) them pair them upnecessary) them pair them up Draw Lewis Structures for the Draw Lewis Structures for the
following atomsfollowing atoms
Na Be Al Br
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Lewis Structures for Ionic Lewis Structures for Ionic CompoundsCompounds
For Lewis Structures of ionic bonds For Lewis Structures of ionic bonds the atoms are not joined but draw the atoms are not joined but draw next to each othernext to each other
[ Br ]K+ -Bromine gains anelectron to achievethe noble gas configurationof Krypton
Potassium loses anelectron to achievethe noble gas configurationof Argon
example:KBr
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Lewis Structures – Covalent Lewis Structures – Covalent BondsBonds
Hydrogen forms stable molecules when Hydrogen forms stable molecules when it shares two electronsit shares two electrons
Two electrons fill Hydrogen’s valence Two electrons fill Hydrogen’s valence shellshell
Helium does not form bonds because its Helium does not form bonds because its valence shell is already filled; it is a valence shell is already filled; it is a noble gasnoble gas
Second row non-metals Carbon through Second row non-metals Carbon through Fluorine from stable molecules when Fluorine from stable molecules when surrounded by eight electrons – surrounded by eight electrons – the the Octet RuleOctet Rule
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Lewis Structures – Covalent Lewis Structures – Covalent BondsBonds
Valence electrons in covalent Valence electrons in covalent bonds can either be bonds can either be bonding pairsbonding pairs, , if involved directly in the bond or if involved directly in the bond or lone pairslone pairs if not involved in the if not involved in the bondbond
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Writing Lewis Structures - Writing Lewis Structures - RulesRules Obtain the total sum of the valence Obtain the total sum of the valence
electrons from all of the atomselectrons from all of the atoms Use one pair of electrons to form a bond Use one pair of electrons to form a bond
between each pair of bound atoms. For between each pair of bound atoms. For convenience, a line (instead of a pair of convenience, a line (instead of a pair of dots) dots) cancan be used to indicate each pair be used to indicate each pair of bonding electronsof bonding electrons
Arrange the electrons to satisfy the duet Arrange the electrons to satisfy the duet rule for hydrogen and the octet rule for rule for hydrogen and the octet rule for second row second row
non metalsnon metals
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Lewis Structures – Covalent Lewis Structures – Covalent BondsBonds
ExamplesExamples
PH3
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 H lH– P –H ••
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Lewis Structures – Covalent Lewis Structures – Covalent Bond Practice ExamplesBond Practice Examples
HBr ..
H:Br:
··
CF4
Worksheet
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Regents Chemistry
– Ionic Lewis Structures– Multiple bonds in Lewis Structures– Polyatomic ion Lewis Structures and
Resonance
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Lewis Structures for Ionic Lewis Structures for Ionic CompoundsCompounds
For Lewis Structures of ionic bonds For Lewis Structures of ionic bonds the atoms are not joined but draw the atoms are not joined but draw next to each othernext to each other
[ Br ]K+ -Bromine gains anelectron to achievethe noble gas configurationof Krypton
Potassium loses anelectron to achievethe noble gas configurationof Argon
example:KBr
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Examples of Ionic Lewis Examples of Ionic Lewis StructuresStructures
Draw Lewis Structures for the Draw Lewis Structures for the following:following:
NaClNaCl
LiBrLiBr
KIKI
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Multiple Bonds and Lewis Multiple Bonds and Lewis Structures…Structures…review firstreview first
We have seen how to draw Lewis We have seen how to draw Lewis Structures for molecules with Structures for molecules with single bondssingle bonds• For exampleFor example
NH3NH31. Sum the total valence e-
2. Subtract number of bonding e-3. Place remaining valence e-
8 total valence e-3 bonds x 2e- = 6 bonding2 e- left over
H
H HN
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Multiple BondsMultiple Bonds
Between atoms of the same Between atoms of the same elementelement
ExampleExample• OxygenOxygen
O OO O
O = OAlso a Lewis Structure
Just O = O is called a structural model
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Example of Multiple BondsExample of Multiple Bonds
NitrogenNitrogen
N N
N N
We now meet the octet rule!
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Multiple BondsMultiple Bonds
Between atoms of different Between atoms of different elementselements
COCO22 C OO
O = C = O
We must use double bonds to meet the octet rule!
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Lewis Structures for Lewis Structures for Polyatomic Ions and Polyatomic Ions and
Resonance StructuresResonance Structures Read pg. 344 (bottom) to 349 and Read pg. 344 (bottom) to 349 and
answer questions a-g in example answer questions a-g in example
12.4 (pg. 347) and a-i in the Self 12.4 (pg. 347) and a-i in the Self Check exercise 12.4 (pg. 348)Check exercise 12.4 (pg. 348)