october 2 , 2013 when the bell rings voices are at zero, working on the do now
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October 2 , 2013 When the bell rings voices are at zero, working on the DO NOW Pick up daily handouts Pick up turned back docs Turn in your TEST CORRECTIONS and any late work, any progress reports. DO NOT TURN ANYTHING IN UNLESS STATED ABOVE HAVE OUT YOUR REFERENCE TABLE - PowerPoint PPT PresentationTRANSCRIPT
October 2, 2013-When the bell rings voices are at zero, working on the DO NOW -Pick up daily handouts -Pick up turned back docs-Turn in your TEST CORRECTIONS and any late work, any progress reports. -DO NOT TURN ANYTHING IN UNLESS STATED ABOVE-HAVE OUT YOUR REFERENCE TABLE -Start on the Do Now in your Do Now form-PICK UP 1 WHITE BOARD AND 1 MARKER – DO NOT USE THEM YET – LEAVE YOUR MARKER CAPPEDDO NOW 10/2/13Finish your anticipation guide (after reading – use what we learned yesterday and anything in the provided reading) WRITE “ANTICIPATION GUIDE” in your DO NOW FORM
Homework
Formula Practice Worksheet
Notebook Check Friday 10/4/13
Electron Configuration/Lewis Structure Notes (periodic table colored in)
Ionic Formula Writing Handout (today)
Upcoming Dates
• 10/2/2013 Bonding Quiz • 10/4/2013 Mid-Quarter Test • 10/4/2013 Take home test Periodic
Trends
Tutoring
• Saturday 12pm-1pm • University City Regional Library • 301 East W.T. Harris Boulevard• Charlotte, NC 28262
Objectives SWBAT
- Explain how covalent bonding in compounds determines its characteristics - Determine that a bond is predominately covalent by the location of the atoms on the Periodic Table - Write covalent formulas - Predict ionic charge based on valence electrons
IonsIons
Cation: A positive ionMg2+, NH4
+
Anion: A negative ionCl-, SO4
2-
Predicting Ionic Charges
Group 1:Lose 1 electron to form 1+ ions
H+ Li+ Na+ K+
Predicting Ionic Charges
Group 2:Loses 2 electrons to form 2+ ions
Be2+ Mg2+ Ca2+ Sr2+ Ba2+
Predicting Ionic Charges
Group 13: Loses 3 electrons to form 3+ ions
B3+ Al3+ Ga3+
Predicting Ionic Charges
Group 14: Lose 4 electrons or gain 4 electrons?
Neither! Group 13 elements rarely form ions.
Predicting Ionic Charges
Group 15: Gains 3 electrons to form 3- ions
N3-
P3-
As3-
NitridePhosphide
Arsenide
Predicting Ionic Charges
Group 16: Gains 2 electrons to form 2- ions
O2-
S2-
Se2-
Oxide
SulfideSelenide
Predicting Ionic Charges
Group 17: Gains 1 electron to form 1- ions
F1-
Cl1-
Br1-
Fluoride
Chloride
Bromide
I1- Iodide
Predicting Ionic Charges
Group 18: Stable Noble gases do not form ions!
Predicting Ionic Charges
Groups 3 - 12:
Many transition elements have more than one possible oxidation state.Iron(II) = Fe2+ Iron(III) = Fe3+
Predicting Ionic Charges
Groups 3 - 12:
Some transition elements have only one possible oxidation state.
Zinc = Zn2+ Silver = Ag+
Writing Ionic Compound Formulas
Example: Barium nitrate
1. Write the formulas for the cation and anion, including CHARGES!
Ba2+ NO3-
2. Check to see if charges are balanced.
3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion.
Not balanced!
( ) 2
Writing Ionic Compound Formulas
Example: Ammonium sulfate
1. Write the formulas for the cation and anion, including CHARGES!
NH4+ SO4
2-
2. Check to see if charges are balanced.
3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion.
Not balanced!
( )2
Writing Ionic Compound Formulas
Example: Iron(III) chloride
1. Write the formulas for the cation and anion, including CHARGES!
Fe3+ Cl-
2. Check to see if charges are balanced.
3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion.
Not balanced!
3
Writing Ionic Compound Formulas
Example: Aluminum sulfide
1. Write the formulas for the cation and anion, including CHARGES!
Al3+ S2-
2. Check to see if charges are balanced.
3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion.
Not balanced!
2 3
Writing Ionic Compound Formulas
Example: Magnesium carbonate
1. Write the formulas for the cation and anion, including CHARGES!
Mg2+ CO32-
2. Check to see if charges are balanced.
They are balanced!
Writing Ionic Compound Formulas
Example: Zinc hydroxide
1. Write the formulas for the cation and anion, including CHARGES!
Zn2+ OH-
2. Check to see if charges are balanced.
3. Balance charges , if necessary, using subscripts. Use parentheses if you need more than one of a polyatomic ion.
Not balanced!
( )2
Writing Ionic Compound Formulas
Example: Aluminum phosphate
1. Write the formulas for the cation and anion, including CHARGES!
Al3+ PO43-
2. Check to see if charges are balanced.
They ARE balanced!
Naming Ionic CompoundsNaming Ionic Compounds
Cation first, then anion
Monatomic cation = name of the element
Ca2+ = calcium ion
Monatomic anion = root + -ideCl- = chloride
CaCl2 = calcium chloride
Naming Ionic Compounds(continued)
Naming Ionic Compounds(continued)
some metal forms more than one cation
use Roman numeral in name
PbCl2
Pb2+ is cation
PbCl2 = lead(II) chloride
Metals with multiple oxidation states
Objectives SWBAT
- Explain how ionic bonding in compounds determines its characteristics - Determine that a bond is predominately ionic by the location of the atoms on the Periodic Table - Write ionic formulas - Predict ionic charge based on valence electrons
Exit Ticket
1. In an ionic bond , ions come together due to ___________________
2. Write the Ionic Formula Compound for the following 1. Barium Nitrate
3. Name the Following Ionic Compound 1. CaCl2
Made of StarDust Video
CovalentBonding
Bonding models for methane, CH4. Models are NOT reality. Each has its own strengths and limitations.
The Octet Rule and Covalent Compounds
Covalent compounds tend to form so that each atom, by sharing electrons, has an octet of electrons in its highest occupied energy level.
Covalent compounds involve atoms of nonmetals only.
The term “molecule” is used exclusively for covalent bonding
The Octet Rule: The Diatomic Fluorine Molecule
F
F
1s
1s 2s
2s 2p
2p
Each has seven
valence electrons
F F
The Octet Rule: The Diatomic Oxygen Molecule
O
O
1s
1s 2s
2s 2p
2p
Each has six valence
electrons
O O
The Octet Rule: The Diatomic Nitrogen Molecule
N
N
1s
1s 2s
2s 2p
2p
Each has five valence
electrons
N N
Lewis structures show how valence electrons are arranged among atoms in a molecule.
Lewis structures Reflect the central idea that stability of a compound relates to noble gas electron configuration.
Shared electrons pairs are covalent bonds and can be represented by two dots (:) or by a single line ( - )
Lewis Structures
The HONC RuleHydrogen (and Halogens) form one covalent bond
Oxygen (and sulfur) form two covalent bonds
One double bond, or two single bonds
Nitrogen (and phosphorus) form three covalent bonds
One triple bond, or three single bonds, or one double bond and a single bond
Carbon (and silicon) form four covalent bonds.
Two double bonds, or four single bonds, or a triple and a single, or a double and two singles
CH
H
H
Cl
..
.. .. ..
Completing a Lewis Structure -CH3Cl
Add up available valence electrons: C = 4, H = (3)(1), Cl = 7 Total = 14
Join peripheral atoms
to the central atom with electron pairs. Complete octets on
atoms other than hydrogen with remaining electrons
Make carbon the central atom (it wants the most bonds, 4)
..
.. ..
Bond Length and Bond EnergyBond Length
(pm)Energy
(kJ/mol)
C - C 154 346
C=C 134 612
CC 120 835
C - N 147 305
C=N 132 615
CN 116 887
C - O 143 358
C=O 120 799
CO 113 1072
N - N 145 180
N=N 125 418
NN 110 942
ResonanceOccurs when more than one valid
Lewis structure can be written for a particular molecule.
These are resonance structures. The actual structure is an average of the resonance structures.
Resonance in Benzene, C6H6
Practice
QUIZ
• Ionic and metallic bonding