Periodic Table Groups
1. Color-code the following groups on your periodic table:
-alkali group -alkaline group - transitional group -halogen group
-noble gases
-inner transitional group
2. Add the staircase (separates metals/non-metals.)
3. Place an asterisk by each metalloid.
4. Non-metals groups: Which group is most reactive and which is most
stable? Explain how you know this.
5. Metal groups: Which group is most reactive and which is most
stable? Explain how you know this.
6. Give an example of two elements that will form an ionic bond to reach
stability.
7. Give an example of two elements that will form a covalent bond to
reach stability.
8. What does each period on the periodic table symbolize for an atom?
9. What period and group is Bromine in?
10. a. What is electronegativity?
b. What is the trend in electronegativity across a period and down a
group on the periodic table.
Chem II-Block: 9.2.14
Infinite Campus:
• Scientific Skills and Matter Exam (53pts.) Avg.= 73%
Objectives:
• Periodic Table Organization and Trends
• Classify and Name Compounds (Nomenclature)
Homework:
• Review polyatomic ions (quiz Thurs.)
• Classifying compounds by their electronegativity
differences.
Bell Ringer: Periodic Table Check-up
• Use your homework (Periodic Table
Group)qts. and color-coded periodic table to
answer qts.
Periodic Table Groups-homework(9.2)
1. Color-code the following groups on your periodic table:
-alkali group -alkaline group - transitional group -halogen group
-noble gases
-inner transitional group
2. Add the staircase (separates metals/non-metals.)
3. Place an asterisk by each metalloid.
4. Non-metals groups: Which group is most reactive and which is most
stable? Explain how you know this.
5. Metal groups: Which group is most reactive and which is most
stable? Explain how you know this.
6. Give an example of two elements that will form an ionic bond to reach
stability.
7. Give an example of two elements that will form a covalent bond to
reach stability.
8. What does each period on the periodic table symbolize for an atom?
9. What period and group is Bromine in?
10. a. What is electronegativity?
b. What is the trend in electronegativity across a period and down a
group on the periodic table.
Periodic Table
Periodic Table Check-Up
Periodic Table
Chem II-Block: 9.3.14
Objectives:
• Periodic Table Organization and Trends
• Classify and Name Compounds (Nomenclature)
Homework:
• Chemical Nomenclature Quiz-Thursday
• Classifying compounds by their electronegativity
differences.
Periodic Table Check-Up
• Assess peers work, make changes where
necessary.
Periodic Table Applications
1. Pick a representative element and a transitional
element from your periodic table and answer
the following qts. for each:
a. What group is it in?
b. Using electron configuration, validate the
number of valence electrons it has.
c. Would it participate in ionic and/or covalent
bonding? Explain your answer.
2. Of the two elements you chose, which do you
predict would have a greater electronegativity?
Explain your answer.
Periodic Table Applications
1. Pick a representative element and a transitional
element from your periodic table and answer
the following qts. for each:
a. What group is it in?
b. Using electron configuration, validate the
number of valence electrons it has.
c. Would it participate in ionic and/or covalent
bonding? Explain your answer.
2. Of the two elements you chose, which do you
predict would have a greater electronegativity?
Explain your answer.
Chemical Nomenclature
Electronegativity
• Electronegativity: The degree of attraction
one atom has towards another atom’s valence
electron in a compound.
O
H
H
Electronegativity and Chemical Bonding
•Do metals or non-metals have a greater electronegativity value?
Chemical Nomenclature
• Review with peers and place problems on
Activ board we need to address:
•
•
•
•
•
•
•
•
•
•
Covalent Compounds Nomenclature:
Prefixes
One
Two
Three
Four
Five
Six
Seven
Eight
Nine
Ten
Homework: Polar vs. Non-Polar
• Distinguish between polar and non-polar
compounds with a Venn diagram.
• Classify each compound from the bell ringer as
either ionic, polar, or non-polar by calculating
their electronegativity differences.
Electronegativity Values
webassign.net
Chemical Bonding :
Electronegativity Difference
Chem II-Block: 9.4.14
Due:
• Chemical Nomenclature Packet
• Polar vs. Non-Polar Bonds Wksht.
Objectives:
• Classify and Name Compounds (Nomenclature)
• Predict chemical bonding using electronegativity
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Classify geometries of covalent compounds. (VSEPR
theory)
Homework:
• Classification of compounds and chemical
nomenclature quiz-tomorrow.
Chemical Nomenclature
Gallery Walk
• Watch roman numerals and prefixes.
Think about when you need them and
when you don’t.
• Drop charges when expressing final
answer for chemical formulas.
Types of Chemical Bonding
Covalent Bonding
Ionic Bonding
Chemical
Bonding
Chem II-Block: 9.5.14
Infinite Campus:
• Chemical Nomenclature Gallery Walk (10pts.)
Objectives:
• Chemical Compounds: classify/nomenclature-quiz
• Predict chemical bonding using electronegativity.
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Identify geometries of covalent compounds. (VSEPR
theory)
• Classify covalent compounds as either polar or nonpolar.
• Identify types of intermolecular forces.
.
Electronegativity and Bonding
Complete the table below.
Chemical Bond
Electronegativity
Difference
(Use
electronegativity
Periodic table)
Type of Bond
Ionic Bonding (Lewis Dot Transfer)
Metal
(Lewis Dot)
Al
Non-metal
(Lewis Dot)
S
Ionic Bonding
(Lewis Dot Transfer)
Molecular Structures: Lewis Dot Sharing
Molecules
CS2
CO2
N2
Lewis Dot Sharing
Molecular
Name
Polar or NonPolar Bonds
Chem II-Block: 9.8.14
Infinite Campus:
• Chemical Nomenclature Quiz (26pts.)’
• Density Lab Report (25pts.)
Objectives:
• Chemical Compounds: classify/nomenclature-quiz
• Predict chemical bonding using electronegativity.
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Identify geometries of covalent compounds. (VSEPR
theory)
• Classify covalent compounds as either polar or nonpolar.
• Identify types of intermolecular forces.
Bell Ringer: Chemical Bonding
Chemical Formula
CO2
CF4
Mg3N2
N2
FeO
Classify
Compound
Lewis Dot
Structures
Chemical
Name
Chem II-Block: 9.9.14
Objectives:
• Chemical Compounds: classify/nomenclature-quiz
• Predict chemical bonding using electronegativity.
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Identify geometries of covalent compounds. (VSEPR
theory)
• Classify covalent compounds as either polar or nonpolar.
• Identify types of intermolecular forces.
.
Nomenclature Quiz
Density Lab Report
Strengths:
• Organization of data tables
• Graphing data (hand-graph, calculator)
• Analyzing group and class’s data
Weaknesses:
• Organization of lab report (headings)
• Analysis section should be in paragraph form
• Graph titles should be specific to experiment.
• Use line of best fit to interpret data
VSEPR Theory
(Valence Shell Electron Pair Repulsion)
liakatas.org
Bell Ringer: Chemical Bonding
Chemical Formula
Lewis Dot
Structure
Molecular Structure
Molecular
Geometry
Chemical Compounds Structure:
Ionic Compounds
7.2
Crystalline Lattice
• The orderly arrangement of ions produces
beautiful crystalline structure.
Covalent Compounds: Crystal Lattice
• Attraction between each molecule (covalent
compounds).
• What is that force called between
molecules?
o
o
C
C
o
o
C
http://iscience.ru/wp-content/uploads/2008/12/sugarmolecule-02.jpg
C
http://www.michigansugar.com/images/ag/production/th_me
d_crystals.jpg
Bell Ringer: Chemical Bonding
Chemical Formula
Lewis Dot
Structure
Molecular Structure
Molecular
Geometry
Molecular Geometry
• Shape of the molecule in 3-D space.
• VSEPR Theory:
-(Valence Shell Electron Pair Repulsion)
-How bonds and lone pairs are arranged
around atoms to minimize electron
repulsion.
VSEPR Theory
(Valence Shell Electron Pair Repulsion)
liakatas.org
Molecular Geometry
Molecules
Molecular
Structure
Molecular
Geometry Name;
Bond Angle
CBr4
PH3
SiS2
Using the VESPR hand-out classify the geometries and
bond angles for each molecule from your homework/bell ringer
Covalent Compound Questions
1. What does the VSEPR acronym stand for?
2. How is VSEPR theory applied to covalent
compounds? Explain for full credit.
3. What are molecular orbitals?
Covalent Compound Questions
1. What does the VSEPR acronym stand for?
2. How is VSEPR theory applied to covalent
compounds? Explain for full credit.
3. What are molecular orbitals?
Chem II Homework: due 9.8.14
• Using the VESPR hand-out classify the
molecular geometry and bond angle of
each of your molecules from your packet.
• Distinguish between sigma and pi bonds
within a molecule. Give an example of a
molecule that has both a sigma and pi bond.
•
• Identify, define, and give an example of the
three classes of intermolecular forces that
exist between molecules in the solid and
liquid state.
Chem II-Block: 9.11.14
Objectives:
• Chemical Compounds: classify/nomenclature-quiz
• Predict chemical bonding using electronegativity.
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Identify geometries of covalent compounds. (VSEPR
theory)
• Classify covalent compounds as either polar or nonpolar.
• Classify the type of bonds between atoms. (sigma/pi)
• Identify types of intermolecular forces.
.
Bell Ringer: Chemical Bonding
Chemical Formula
Lewis Dot
Structure
Molecular Structure
Molecular
Geometry
VSEPR Theory
(Valence Shell Electron Pair Repulsion)
liakatas.org
Drawing Molecular Structures
1.Draw Lewis Dot Structure for each element.
2.Calculate the total number of ve- for the
molecule .
3.Share unpaired ve- with atoms. (covalent
bonds)
4.Place lone pairs around appropriate atoms.
5.If an atom is not stable, then lone pairs can be
used to reach maximum stability.
6.There are some exceptions to Octet Rule
• Elements with d-orbitals
• Molecules with an odd number of ve- (total)
Molecular Structures Lab
Molecular Orbitals
• When ve- are shared between two atoms in
a molecule, their atomic orbitals overlap.
• The overlap of atomic orbitals between two
atoms create molecular orbitals.
• Each molecular orbital is also called a
bonding orbital because it represents the
sharing of two ve- between two atoms.
• Two types of bonding orbitals: Sigma and Pi
Molecular Orbitals
wikis.lawrence.edu
Bonding Orbitals
chemistryland.com
Molecular Geometry
• Using the VESPR hand-out and the
molecular model kit, classify each of these
molecules.
Molecules
Molecular
Structure
Molecular
Geometry Name;
Bond Angle
Type of Bonds
(Sigma/Pi)
NCl3
Trigonal pyramidal
sigma
CBr4
Tetrahedral
sigma
CH4
Tetrahedral
sigma
PF3
Trigonal pyramidal
sigma
In addition: CO , SiCl , SBr , N , C H
2
4
2 2 2 2
Homework
1. Draw the molecular structure of the following
molecules:
a. SiCl4
b. SBr2
c.
d. *BF3
*d. SO3 *(bonus)
b. Determine the molecular geometry (shape) of the
molecules above including bond angles.
2. a. Illustrate the difference between sigma an pi of
bonding orbitals.
b. Classify the bonding orbitals in the following
molecules.
-CH4 tetrahderal; sigma bonds
- N2 linear; sigma and 2 pi bonds
- C2H2 linear; 3 sigma and 1 pi bond
Chem II-Block: 9.12.14
Due:
• Polar vs. Non-Polar Molecules: (CH4 and CCl4)
• Intermolecular Forces between molecules.
Objectives:
• Chemical Compounds: classification/nomenclature.
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Assess type of bonds(sigma/pi) and polarity of bonds.
• Identify geometries of molecules. (VSEPR theory).
• Classify molecules as either polar or non-polar.
• Predict the type of intermolecular forces that exist
between molecules in the solid and liquid state.
.
Polar Molecules
• Polar molecules: One end of the molecule
is partially positive and the other end is
partially negative.
• Also called dipole molecules.
• Draw the following molecular structures:
CH4 and CF4
Polar or Non-Polar Molecules?
P
3dchem.com
Assess type of bonds (sigma/pi) andF
polarity of bonds.
F
en.wikipedia.org
ieshermanosbilingual.blogspot.com
F
Polar vs. Non-Polar Molecules
Polar Molecules
Non-Polar Molecules
Polar vs. Non-Polar Molecules
• Classify your molecules as either polar or
non-polar molecules.
Chem II-Block: 9.16.14
Infinite Campus:
Molecule Lab (16pts)
Objectives:
• Chemical Compounds: classification/nomenclature.
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Assess type of bonds(sigma/pi) and polarity of bonds.
• Identify geometries of molecules. (VSEPR theory).
• Classify molecules as either polar or non-polar.
• Predict the type of intermolecular forces that exist
between molecules in the solid and liquid state.
.
Intramolecular Forces
.
Intermolecular Forces
Types of Intermolecular Forces
• Identify and define the types of intermolecular
forces that can exist between molecules in the
liquid and solid state.
• Give an example of a molecule that applies
each type of intermolecular force when in the
solid and liquid state.
Intermolecular Forces
itl.chem.ufl.edu
Types of Intermolecular Forces
1.Dipole Forces :
Prentice Hall: Chemistry
Types of Intermolecular Forces
1.Dipole Forces :
• Attraction b/w polar molecules
• Partial charges oppositely
attract
Prentice Hall: Chemistry
Types of Intermolecular Forces
Hydrogen Bonds :
http://employees.csbsju.edu/hjakubowski/classes/Chem%20
and%20Society/IMF_Solutions/olIMF_solutions.htm
Types of Intermolecular Forces
Hydrogen Bonds :
• Very strong dipole force.
Pre-resquiste for H bonding to occur:
• H must be covalently bonded to a very
electronegative element (N, O, F).
Types of Intermolecular Forces
• 3. London Dispersion Forces:
I
I
elmhurst.edu
Chem II-Block: 9.17.14
Objectives:
• Chemical Compounds: classification/nomenclature.
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Assess type of bonds(sigma/pi) and polarity of bonds.
• Identify geometries of molecules. (VSEPR theory).
• Classify molecules as either polar or non-polar.
• Predict the type of intermolecular forces that exist
between molecules in the solid and liquid state.
Homework: Test on Friday-will not meet tomorrow.
.
Types of Intermolecular Forces
• 3. London Dispersion Forces:
• Caused by randomn motion of electrons in an atom.
• Occur in non-polar and polar molecules.
• Temporary and dynamic dipole forces between
atoms.
• Use the data below to explain
what influences the strength of
dispersion forces?
*States of Matter: Diatomic Molecules
solid
I2
liquid
Br2
*At Room Tempearatue
gases
F2; Cl2
elmhurst.edu
Intermolecular Forces
Molecular
Formula
CS2
NH3
OCl2
Polar or Nonpolar
Molecule
Intermolecular
Forces
Molecular
Name
Gallery Walk: Chemical Bonding
Review