Including Naming Note We likely wont make it to covalent nomenclature this is the one students find FAR easier than ionic Please refer to the videos and naming hand out for help with this and as always office hours discussions and ID: 321035
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Slide1
Ionic and Covalent BondingIncluding Naming
Note: We likely won’t make it to covalent nomenclature, this is the one students find FAR easier than ionic. Please refer to the videos and naming hand out for help with this, and as always office hours, discussions, and
facebook
for extra help. If you don’t remember it from high school/1P. Slide2
Types of Bonds
Ionic:
Covalent:
Metallic:
“trades” electrons
Metal and a
non-metal(oversimplified definition)
“shares” electronsnon-metals(oversimplified definition)
delocalized electronsmetalselectrically conductivecollective description of many bonds
NaCl
CO
AgSlide3
For the Following Choose the Ionic Compounds (based on previous definition)
NaCl
CH
3
Cl
MgCl2
SO2Na2SO3Slide4
For the binary ionic compounds in the last slide, decide which has more covalent character.
Reminder note from videos (see slides included FYI):
Summary of slides:
The more polarizing power and polarizability lead to a bond with more covalent character.
Small highly charged
cations
have more polarizing power.Large highly negatively charged cations have more polarizability.
NaClMgCl2
For cations which have more polarizability?Slide5
Polarizing Power Polarizability and Covalent Character
Polarizability: Anion
More electrons that are further from the nucleus
Nucleus has less pull on far off electrons. The more energy shells the more polarizability
A more negative charge, higher
electron:proton
ratio, more polarizabilityPolarizing power: CationLess electrons closer to the nucleus
Nucleus has larger effect on electrons if they are closer to the nucleus. Less electron shells equal more polarizing powerA more positive charge, higher proton:electron ratio, higher polarizing power
NaC
l
MgI
2Slide6
Polarizing Power Polarizability
and Covalent Character
More polarizability/polarizing power of the anion/
cation
leads to a
bond with more covalent character
NaCl
MgI
2Slide7
Charge
Ion 1
Charge
Ion 2
Internuclear
radius
Lattice Energies
Note: This isn’t and won’t be covered in the videos.
You won’t need to do lattice energy problems any more complex than shown in the next couple of slides.
We will not be calculating the numbers, this equation will be for illustration purposes only.
If
internuclear
distance increases what happens to energy?
If charge increases what happens to energy?Slide8
Ionic Bond Formation
A) Explain why the lattice energy of silver bromide (903 kJ/
mol
) is greater than that of silver iodide (887 kJ/
mol), given that they have a similar arrangement of ions .
Hint: How does the charge of Br- and I
- compare?Hint: How does the size of Br- and I- compare?
Hint: If two charges are closer together, how is the force required to hold them together affected?Slide9
Naming: Ionic
Name the Compounds we identified as ionic on the first problem.
NaCl
MgCl
2
Na
2
SO
3Slide10
Naming: Covalent
Name the Compounds below.
SO
2
NO
PCl
5