Chemistry II
Beginning of the Year
Warm Up
Let's see what the sun
baked out this summer!
Easy Ones!
• What is the chart thing on the wall?
– Answer: Periodic Table
• Bonus: How is it arranged?
– Answer: By atomic number / by number of protons
Tell me what else you know about this
thing ...
Other things to know:
• Polyatomic Ions
• Naming Compounds
• Writing Compound Formulas
• Identifying Charges on Ions
• Any of these SCARE you???
Where to Start??
Our first topic is bonding… so you should
remember the following items from Pre-AP or
Chemistry I.
If these first five slides made you sick, you are
either going to have to study/review/ask for
help/wake up your brain, or reconsider your
schedule.
Periodic Trends
What do you remember about Periodic trends?
Did you get it all?
Periodic Trends
Definition: a pattern of behavior on the periodic table
• Defined for a group
• Defined for a period
Some Examples:
• Atomic Size:
• Electronegativity:
• Ionization Energy:
Periodic Trends Continued…
• Atomic Size- atomic radius
• increases down a group, decreases L-R across a period
• Electronegativity- Ability of an atom to attract
shared electrons "greed“
• Decreases down a group, Increases L-R across a period
• Ionization Energy- Energy needed to remove
electrons from the atom
• Decreases down a group, Increases L-R across a period
Next Topic: Valence Electrons
What do you remember about Valence Electrons?
Did you get it all?
Valence Electrons
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•
•
•
•
•
•
Outermost Electron(s)
Control chemical activity
Can be shared
Can be transferred
Loss of electrons = positive ion
Gain of electrons = negative ion
Involved in bonding (sharing, transfer)
Atomic Models
What do you remember about atomic models?
Did you get it all?
Atomic Models
• JJ Thomson
“Plum Pudding Model”
• Rutherford
“Gold Foil Experiment”
• Bohr
“orbits, only worked for H”
Atomic Models continued
• Current Model- Wave Mechanical Model
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•
•
•
Mathematical representation
Orbital- area of probability- expect to find electrons
s/p/d/f sublevels
Electron configurations represent mathematical
description
Electron Configurations
What do you remember about Electron Configurations?
Did you get it all?
Electron Configurations
• Description of electron arrangement
• wave mechanical model
• quantum mechanical model
• Orbital- probability zone
• Pauli Exclusion Principle: no two electrons can
have the same set of four quantum numbers
• Quantum Numbers
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•
•
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Principle Energy Level
Sublevel- s, p, d, f
Orbital
Spin
Anatomy of a Standard Electron
Configuration
2
1s
Principle Energy Level:
Tells distance from nucleus
Relative amount of energy
Number of sublevels in the
Number of
electrons in the
sublevel
Sublevel:
Tells shape of
orbital
Indicates how many
electrons
may be
s - 2 electrons
held
max.
p- 6 electrons
max.
Abbreviated Configurations
• Start with the previous noble gas in brackets
[He]
2
2s
Previous noble
gas symbol
placed in
brackets
4
2p
Continue with
electron
configuration
from noble gas
on
Orbital Diagrams
• Show the fourth quantum number- spin
1s
2s
2p
Practice Electron Configurations
• Magnesium- atomic #12
– Standard configuration
– Abbreviated configuration
– Orbital diagram
You should remember what you
learned in Chemistry I or Pre AP !
If you do not, the items you will need most right
now are:
• recognize polyatomic ions (names, formulas and charges)
• write formulas for compounds, write names for formulas
• describe basic workings/organization of periodic table
Later you will need:
• describe parts of a chemical equation :
reactant, product, coefficients
• describe basic parts of a solution: solvent,
solute, concentration (molarity)
• describe acids and bases
Assignment
• Electron Configuration Practice Worksheet
• Answer Key Page 1
• Answer Key Page 2