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Q3: week 4 – 2/27  –  3/3

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 ___________________________________________________                                                                                Jump to:  Monday Homework   

2/27 – Monday – “B” Day –  

Main focus: 

 
a)  To identify metallic bonding and the properties of metallic solids
b)  To identify the differences in the properties of Ionic, Covalent, and Metalllic solids

 

Period  8:

1.  To review the Bonding Test

2.  Metallic Bonding  lesson.

3. Complete the Bodacious Bonding Bonanza worksheet together. 

Bodacious bonding with properties chart.pdf
View Download

 

Metallic Video: a great presentation

Today’s Lesson on Metallic Bonds and properties:

 

 
Bonding Presentation : 
          

 

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2/27 – Monday’s Homework: – 

1. Please complete today’s worksheet and review with the key below:

Bodacoius bonding with properties chart key.pdf
View Download

2. Complete the Form below.

                               

 
Bonding Form 9: Ionic, Covalent, metallic solid properties.
          

 

 

 

_______________________________________________________                                                                       Jump to:  Tuesday Homework 2/28 – Tuesday “A” Day 

 

 Main focus:

a)  To identify the chemical formulas of chemicals that either have ionic, covalent, or  metallic bonding.

b) To identify the intra and intermolecular attractions.
   
c) To differentiate between LDF’s, dipole – dipole, and H bonding Intermolecular Forces of  attraction
   

Period  9:

1. Review the homework form 9 with key.

2.   Intermolecular attractions lesson:

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TODAY’s NOTES: 

Network solids are the RARE CASE when some molecular compounds make continuous covalent bonds in their crystals.  Diamond and Graphite are examples.  Most molecular solids are held by IMF. *Graphite is the only Network solid that conducts due to the delocalization of electrons throughout its crystal.  

 

IMF = Intermolecular Forces – ATTRACTIVE forces that hold molecules together
 
Molecular solids have the lowest melting points because when you give them heat you are separating molecules HELD TOGETHER BY ATTRACTIVE FORCES (IMF) that are only a fraction of the BOND Energy of Covalent, Ionic, or Metallic BONDs!  It takes less energy to separate molecules held together by attractive forces than it does to separate atoms or ions (breaking bonds).
 
Since we are breaking only attractive forces AND NOT BONDS heating this solid would be a PHYSICAL Change as the chemical formulas (of the individual molecules) would not change!
 
All phase changes (ex. melting, freezing) of molecular compounds are always physical changes!!!!
 
                                                      H2O (s)  —-> H2O (l)  —-> H2O (g) 
 
                                                               Ice     —->  water    —->  steam (can’t see it!!)
 
We are only separating the attractive forces between the molecules and thus the chemical formula does not change.
 
In our copper Iodine lab earlier in the year why did the Iodine sublime?
                                                                        
                                                                                                                                 I2 (s)  ——>   I2 (g) 
 
Because Iodine is a molecular solid with a low melting (sublimation) point due to the weak attractive keeping iodine as a solid.                        
 What caused the atmospheric Oxygen become a liquid? What forces are at play? 

 

                What held the molecules of polyvinyl chloride together in SLIME (Holiday Cross Linked polymers)?

 

Intermolecular Molecular Attractions: (IMF’s)

Today’s Lesson on Intermolecular Forces.


 

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2/28 – Tuesday’s Homework: – 

Please complete the form below based on the notes taken today.

 

              

 
 IMF Form 1: 
          

 

 

_________________________________________________                                                                      Jump to:  Wednesday Homework 

3/1 – Wednesday – B Day – 

Main focus: 

 

a) To Identify the type of molecular attractions (IMF’s) in the cross-linked polymer.

b) To identify the orientation of water molecules when they dissolve ionic compounds.

 
 
Period  8:
 
1.  Review last nights form. 
 
2.  Continue with the Intermolecular attractions presentation-
  

Period  9:   

1. Lab 13 –  Intermolecular attractions lab

LAB 13 – Regents IMF’s Lab .pdf
View Download

DNA keep are important genetic information intact by H bonding:

Molecule Ion Attractions – Ion Dipole: (animation)

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3/1 –  Wednesday – “B” Day homework: –
 
1. Please complete the questions for today’s Lab.
 

___________________________________________________                                                                        Jump to:  Thursday Homework

3/2 – Thursday “A” Day – 

Main focus:   
 

a) To identify the solvent and solute in a homogeneous mixture.

b) To draw the molecules – ion attractions for an aqueous solution with the correct orientation.

c) To identify if an Ionic compound (salt) is soluble or Insoluble based on Table I                                                                       

 

Period  9:   

1.  Take Notes on Solubility and Table I

Solubility Intro Notes – Table F.pdf

Solubility Intro Notes – Table F.pdf                                                                                                                                View Download

2.  Complete the back of todays worksheet.

 

TODAY’s NOTES:

Molecule Ion Attractions – (ION – Dipole) are the attractions a positive or negative ion has for a polar molecule (water) THAT will Dissolve the ion from its crystal of ions and create a solution (aq) = homogeneous mixture! 

IONIC BONDs (electrovalent)- Ionic solids → Salts (Crystals of ions): 

Occurs between ions and these ions are produces by a REDOX REACTION that occurs due to a transfer of electrons.

Almost every case of ionic bonding occurs between a metal and nonmetal because

THE DIFFERENCE BETWEEN ELECTRONEGATIVITY IS LARGE ( ≥ 1.7) 

and thus a transfer of electrons occurs!

 

Covalent BONDs – Molecular solids → Molecules of finite particles: 

  Occurs between Nonmetals and they occur due to the sharing of electrons.

  Almost every case of covalent bonding occurs between a nonmetal and nonmetal because

THE DIFFERENCE BETWEEN ELECTRONEGATIVITY IS SMALL ( 0 – < 1.7) 

and thus electrons are shared!

Nonpolar Covalent Bond = electrons shared equally: Difference of electronegativity = 0 – 0.4.

Polar Covalent Covalent Bond = electrons shared unequally: Difference of electronegativity = > 0.4 to <1.7

 

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3/2 –  Thursday – “A” Day homework: 
 
1.  Please complete the back of the today’s worksheet and review with the key below:
 

Solubility Notes backside KEY.pdf                                                                                                                                 View Download

 
2. Complete the Form below. You have 3 submissions.
 
_______________________________________________________________________________________
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Solubility Form 1: 
          

 

 

____________________________________________________.                                                                         Jump to:  Friday Homework

3/3 – Friday – “B” Day 

Main focus: 

a) To determine if ionic solids are soluble or insoluble using Table F.

b) To determine the solvent and solute in a solution

c) To determine if a solute will dissolve in polar or nonpolar solvent.

                                                 

Period  8:   

 1.  Review the Solubility form 1

Solubility worksheet.pdf                                                                                                                                         View Download

 2.  Take another form.

Period  9:   

1. Lab 13 – 

 

 
Solubility Form 1B: 
          

 

 

3/3 –  Friday Homework: –
 

No homework.                                           

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