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-Period: 9.11.14
Infinite Campus:
• Scientific Skills and Matter Exam (48pts.)
Objectives:
• Periodic Table Organization and Trends
• Chemical classification and nomenclature
Homework:
• Chemical Nomenclature Packet(ionic/covalent)
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.
Periodic Table: Organization and Bonding
Bell Ringer: Periodic Table Check-up
1. Give an example of an element from each group
below: alkali, halogen, transitional, noble gas, and
alkaline-earth.
2. Which element from qts. 1 is a metal and is
considered to be the most reactive. Explain your
answer.
3. Which element from qts. one is a non-metal and
considered the most reactive? Explain your answer.
4. Which element from qts. one is the most stable.
Explain your answer.
5. Give an example of two elements that would form:
a. a covalent bond
b. an ionic bond
6. What is electronegativity and how is it related to
chemical bonding?
Bell Ringer: Periodic Table Check-up
1. Give an example of an element from each group
below: alkali, halogen, transitional, noble gas, and
alkaline-earth.
2. Which element from qts. 1 is a metal and is
considered to be the most reactive. Explain your
answer.
3. Which element from qts. one is a non-metal and
considered the most reactive? Explain your answer.
4. Which element from qts. one is the most stable.
Explain your answer.
5. Give an example of two elements that would form:
a. a covalent bond
b. an ionic bond
6. What is electronegativity and how is it related to
chemical bonding?
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.
Chemical Nomenclature
• Naming and deriving the formula of
compounds .
Chem II-Period: 9.12.14
Graded:
• Periodic Table Bell Ringer
Objectives:
• Chemical classification and nomenclature
• Relationship between chemical bonding and
organization of periodic table.
Homework:
• Chemical Nomenclature Packet(ionic/covalent)
• Chemical Bonding Study Guide
Chemical Nomenclature
Chem II-Period: 9.16.14
Due:
• Chemical Nomenclature Packet (ionic/covalent)
Objectives:
• Chemical classification and
nomenclature(Acids/Bases)
• Relationship between chemical bonding and
organization of periodic table.
Chemical Nomenclature
Chem II-Period: 9.17.14
Due:
• Chemical Nomenclature Packet (ionic/covalent)
Objectives:
• Chemical classification and
nomenclature(Acids/Bases)
• Relationship between chemical bonding and
organization of periodic table.
Homework:
• Electronegativity Values and Chemical Bonding
packet-Due Friday! (ppts. on my webpage)
Chemical Nomenclature
Nomenclature Gallery Walk
Classify: Ionic or Covalent
Chemical Formula
Chemical Name
Chem II-Period: 9.19.14
Infinite Campus:
• Chemical Nomenclature Lab (10pts.)
Objectives:
• Chemical classification and nomenclature.
• Relationship between chemical bonding and
electronegativity.
Homework:
• Chemical Classification and Nomenclature-Quiz
Chem II-Period: 9.22.14
Objectives:
• Chemical classification and nomenclature.
• Relationship between chemical bonding and
electronegativity.
• Drawing Chemical Structures-Lewis Dot Structures
Homework:
• Chemical Classification and Nomenclature-Quiz
• Chemical Bonding/Structures Packet
Chemical Nomenclature Bell Ringer
Complete the table below for each compound.
Chemical Name
Classification
(ionic, covalent, acid, base)
Chemical Formula
manganese (II) sulfate
phosphorous trichloride
carbonic acid
BrCl5
Sr(OH)2
H3P
Chemical Nomenclature Quiz: A
Complete the table below for each compound.
Chemical Name
Classification
(ionic, covalent, acid, base)
Chemical Formula
Phosphoric acid
copper (I) sulfate
Phosphorous
tetrachloride
Al(NO2)3
H2S
SO
Chemical Nomenclature Quiz:B
Complete the table below for each compound.
Chemical Name
Classification
(ionic, covalent, acid, base)
Chemical Formula
dinitrogen
pentasulfide
iron (III) acetate
hydrofluoric acid
H(NO3)
Ba(NO3)2
SiCl4
Chemical Bonding and Electronegativity
Electronegativity
• Electronegativity: The degree of attraction
one atom has towards another atom’s valence
electron in a compound.
• Determines the type of chemical bonds in a
compound. (ionic, non-polar, and polar)
O
H
H
Electronegativity Values
webassign.net
Chemical Bonding :
Electronegativity Difference
•
The eletronegativity (EN) difference is calculated by subtracting the
electronegativity values of each atom within a single bond.
Electronegativity Values
• According to the eletronegativity table below, would metals
or non-metals
have a greater electronegativity value?
• Explain how electronegativity values determine the type of
ion (cation/anion) that a metal and non-metal would form in
an ionic compound.
webassign.net
Electronegativity Values
webassign.net
Covalent Compounds: Polar vs.Non-Polar Bonds
Chemical Bonding :
Electronegativity Difference
•
The eletronegativity (EN) difference is calculated by subtracting the
electronegativity values of each atom within a single bond.
Chem II-Period: 9.23.14
Due: Chemical Bonding Table Worksheet
Objectives:
• Chemical classification and nomenclature(quiz).
• Relationship between chemical bonding and
electronegativity.
• Drawing Chemical Structures-Lewis Dot Structures
Homework:
• Chemical Bonding/Structures Packet
Chemical Bonding and Electronegativity
Chemical Formula
Classify
Compound
Chemical Name
Bonds:
Ionic,
Polar,
Non-polar
(EN
difference)
CO2
C---O
CI4
C----I
MgF2
Mg---F
N2
N----N
FeO
Fe---O
Chem II-Period: 9.24.14
Infinite Campus:
Chemical Cmpds. Quiz (12pts.)
Due:
Electronegativity and Chemical Bonds
Objectives:
• Relationship between chemical bonding and
electronegativity.
• Drawing Chemical Structures-Lewis Dot Structures
Homework:
• Chemical Bonding/Structures Packet
Chem II-Period: 9.25.14
Infinite Campus:
Chemical Cmpds. Quiz (12pts.)
Due:
Electronegativity and Chemical Bonds
Objectives:
• Relationship between chemical bonding and
electronegativity.
• Drawing Chemical Structures-Lewis Dot Structures
Homework:
• Chemical Bonding/Structures Packet
Chemical Compounds Quiz
Chemical Bonding : Electronegativity Difference
Modifications to electronegativity difference table?
Covalent Compounds: Polar vs.Non-Polar Bonds
Ionic Bonding (Lewis Dot Transfer)
Metal
(Lewis Dot)
Mg
Non-metal
(Lewis Dot)
F
Ionic Bonding
(Lewis Dot Transfer)
Molecular Structures: Lewis Dot Sharing
Molecules
CS2
CO2
N2
Lewis Dot Sharing
Molecular
Name
Polar or NonPolar Bonds
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)
VSEPR Theory
(Valence Shell Electron Pair Repulsion)
liakatas.org
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.
Chem II-Period: 9.29.14
Objectives:
• Chemical Compounds: classify/nomenclature-quiz
• Predict chemical bonding using electronegativity.
• Illustrate ionic and covalent bonding using Lewis Dot
Structures.
• Identify and model geometries of covalent
compounds. (VSEPR theory)
• Classify the type of bond between atoms in a
molecule (sigma/pi).
• Classify molecules as either polar or non-polar.
• Predict the types of intermolecular forces that exist
between molecules.
Homework: Chemical Bonding Study Guide-test Fri.
Molecular Structure Lab
Purpose:
• Model the geometrical shape of molecules
using the VSEPR diagram.
• Additional Molecules:
• CH2Cl2
• CO
• (NH4)+
• PCl5
• BF3
Chem II-Period: 9.30.14
Due:
• Molecluar Structure Lab (pre-lab, L-D structures)
Objectives:
• Identify and model geometries of covalent
compounds. (VSEPR theory)
• Classify the type of bond between atoms in a
molecule (sigma/pi).
• Classify molecules as either polar or non-polar.
• Predict the types of intermolecular forces that exist
between molecules.
Homework: Chemical Bonding Study Guide-test Fri.
.
Molecular Structure Lab
Purpose:
• Model the geometrical shape of molecules
using the VSEPR diagram.
• Additional Molecules:
• CH2Cl2
• CO
• (NH4)+
• PCl5
• BF3
Molecular Structures
Chem II-Period: 10.01.14
Due:
• Molecluar Structure Lab (classify bonds and polarity
of molecule).
Objectives:
• Identify and model geometries of covalent
compounds. (VSEPR theory)
• Classify the type of bond between atoms in a
molecule (sigma/pi).
• Classify molecules as either polar or non-polar.
• Predict the types of intermolecular forces that exist
between molecules.
Homework: Chemical Bonding Study Guide-test Fri.
Molecular Structures
Exceptions:
• Sometimes lone pairs are used in bonding
(coordinate bonds)
• There are exceptions to the octet rule:
(S, P, B, H, He)
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
Bonding Orbitals
chemistryland.com
Molecular Orbitals
wikis.lawrence.edu
Polar Molecules
• What are polar molecules?
Polar Molecules
• Polar molecules: One end of the molecule
is partially positive and the other end is
partially negative.
• Also called dipole molecules.
• Which molecules did you predict from the
lab were polar molecules?
Polar Molecules
Polar or Non-Polar Molecules?
P
3dchem.com
F
F
F
en.wikipedia.org
ieshermanosbilingual.blogspot.com
Chem II-Period: 10.02.14
Due:
• Molecular Structure Lab (classify bonds and polarity
of molecule).
Objectives:
• Identify and model geometries of covalent
compounds. (VSEPR theory)
• Classify the type of bond between atoms in a
molecule (sigma/pi).
• Classify molecules as either polar or non-polar.
• Predict the types of intermolecular forces that exist
between molecules.
Homework: Chemical Bonding Study Guide-test Fri.
Molecular Structures
Molecules
SiH4
CF4
NBr3
CS2
Molecular
Structure
Geometry/
Bond
Angle
Sigma/Pi
Bonds
Polar/Non Polar/Non-Polar
Polar
Bonds
Molecule
Molecular Structures
Molecules
SiH4
CF4
NBr3
CS2
Molecular
Structure
Geometry/
Bond
Angle
Sigma/Pi
Bonds
Polar/Non Polar/Non-Polar
Polar
Bonds
Molecule
Intermolecular Forces: Classes
• 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
Forces between molecules in the solid, liquid,
and gaseous state.
itl.chem.ufl.edu
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 :
• Very strong dipole force.
Pre-resquiste for H bonding to occur:
• H must be covalently bonded to a very
electronegative element (N, O, F).
Prentice Hall: Chemistry
Types of Intermolecular Forces
3. London Dispersion Forces:
Caused by randomn motion of electrons
Occur in non-polar and polar molecules.
Temporary dipole forces.
I
I
•
•
•
•
elmhurst.edu
Intermolecular Forces
Rank the intermolecular forces from weakest to
strongest?
itl.chem.ufl.edu
Intermolecular Forces
Molecular Formula
Polar or Nonpolar Molecule
Intermolecular Forces
CS2
Non-polar molecule because
the bonds are non-polar;
symmetrical.
Van der Waals or London
Dispersion forces
because the molecule is
non-polar.
Polar molecule because bonds
are polar, central atoms has
lone pairs, and the geometry is
asymetrical.
Hydrogen Bonding, strong
dipole forces because
hydrogen is bonded to a
very electronegative
element, N.
Polar molecule because bonds
are polar and the central atom
has to sets of lone pairs. Also
the molecule is asymetrical.
Dipole Bonding, because
the molecule is polar,
meaning there is a partial
charges that exist in the
molecule.
NH3
OCl2