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.
Transcript
Periodic Table Groups1. 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: 9.11.14Infinite Campus:•Scientific Skills and Matter Exam (48pts.)
Objectives:•Periodic Table Organization and Trends•Chemical classification and nomenclature
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
Chemical Name Classification (ionic, covalent, acid, base)
Chemical Formula
manganese (II) sulfate
phosphorous trichloride
carbonic acid
BrCl5
Sr(OH)2
H3P
Complete the table below for each compound.
Chemical Nomenclature Quiz: A
Chemical Name Classification (ionic, covalent, acid, base)
Chemical Formula
Phosphoric acid
copper (I) sulfate
Phosphorous tetrachloride
Al(NO2)3
H2S
SO
Complete the table below for each compound.
Chemical Nomenclature Quiz:B
Chemical Name Classification (ionic, covalent, acid, base)
Chemical Formula
dinitrogen pentasulfide
iron (III) acetate
hydrofluoric acid
H(NO3)
Ba(NO3)2
SiCl4
Complete the table below for each compound.
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)
• The eletronegativity (EN) difference is calculated by subtracting the electronegativity values of each atom within a single bond.
Electronegativity Values
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• 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.
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: 9.23.14Due: 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 ClassifyCompound
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: 9.24.14Infinite 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: 9.25.14Infinite 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)
Non-metal(Lewis Dot)
Ionic Bonding(Lewis Dot Transfer)
Mg F
Molecular Structures: Lewis Dot Sharing
Molecules Lewis Dot Sharing Molecular Name
Polar or Non- Polar Bonds
CS2
CO2
N2
Drawing Molecular Structures1.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)
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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: 9.29.14Objectives:•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.
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: 10.01.14Due: •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?
ieshermanosbilingual.blogspot.com
en.wikipedia.org
3dchem.com
P
F
F
F
Chem II-Period: 10.02.14Due: •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 Molecular
Structure Geometry/Bond Angle
Sigma/PiBonds
Polar/Non-Polar Bonds
Polar/Non-PolarMolecule
SiH4
CF4
NBr3
CS2
Molecular Structures Molecules Molecular
Structure Geometry/Bond Angle
Sigma/PiBonds
Polar/Non-Polar Bonds
Polar/Non-PolarMolecule
SiH4
CF4
NBr3
CS2
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
itl.chem.ufl.edu
Forces between molecules in the solid, liquid, and gaseous state.
Types of Intermolecular Forces
1.Dipole Forces :
• Attraction b/w polar molecules
• Partial charges oppositely
attract
Prentice Hall: Chemistry
Types of Intermolecular ForcesHydrogen 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.
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I
I
Intermolecular Forces
itl.chem.ufl.edu
Rank the intermolecular forces from weakest to strongest?
Intermolecular ForcesMolecular 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.
NH3
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.
OCl2
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.
