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

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+


Group 2:Loses 2 electrons to form 2+ ions

Be2+ Mg2+ Ca2+ Sr2+ Ba2+


Group 13: Loses 3 electrons to form 3+ ions

B3+ Al3+ Ga3+


Group 14: Lose 4 electrons or gain 4 electrons?

Neither! Group 13 elements rarely form ions.


Group 15: Gains 3 electrons to form 3- ions

N3-

P3-

As3-

NitridePhosphide

Arsenide


Group 16: Gains 2 electrons to form 2- ions

O2-

S2-

Se2-

Oxide

SulfideSelenide


Group 17: Gains 1 electron to form 1- ions

F1-

Cl1-

Br1-

Fluoride

Chloride

Bromide

I1- Iodide


Group 18: Stable Noble gases do not form ions!


Groups 3 - 12:

Many transition elements have more than one possible oxidation state.Iron(II) = Fe2+ Iron(III) = Fe3+


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


Example: Ammonium sulfate


NH4+ SO4

2-



Not balanced!

( )2


Example: Iron(III) chloride


Fe3+ Cl-



Not balanced!

3


Example: Aluminum sulfide


Al3+ S2-



Not balanced!

2 3


Example: Magnesium carbonate


Mg2+ CO32-


They are balanced!


Example: Zinc hydroxide


Zn2+ OH-



Not balanced!

( )2


Example: Aluminum phosphate


Al3+ PO43-


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

Documents

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