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Warm Up
What are the three types of bonds? Determine the type of bond, and how
many of each element are present in: Na2O CO2
CuZn
Objectives
Draw the Lewis structures of ionic and covalent structures.
Lewis Structures
Combining of the dot diagrams to show bonding and to predict shape.
Every Element wants 8 electrons. 2 Types- covalent and ionic.
Ionic Lewis Structures
Step 1: Draw the Lewis dot diagrams for each element.
Step 2: Draw an arrow from the metals electrons to the empty spaces around the nonmetal.
Step 3: Redraw the Lewis dot diagrams showing the movement of electrons AND charges.
Example
Draw the Lewis structure for: NaCl
Example
Draw the Lewis structure for: LiF
Example
Draw the Lewis structure for: MgCl2
Example
Draw the Lewis structure for: Na2O
You Try
Draw the Lewis structure for: KI BeI2 SrF2
Covalent Lewis Structures
Show the sharing of electrons. Show bonds as Show the lone pairs as
Steps for Lewis Structures
Step 1: Add up total number of valence electrons.Step 2: Draw a skeleton by connecting each element with a line. (Carbon or the solo element goes in the middle)
★Hydrogen and the Halogens CANNOT be in the center.
Step 3: Distribute the electrons as PAIRS. Start from the outside and move inward. Step 4: Check Ya Self! Count and adjust electrons till each element has 8. (except Hydrogen)
Examples
Draw the lewis structures for the following:
CF4
Examples
Draw the lewis structures for the following:
H2O
Examples
Draw the lewis structures for the following:
PH3
Examples
Draw the lewis structures for the following:
O2
You Try
Draw the lewis structures for the following:
NH3
F2O CO2
Warm Up
What elements and how many are present in: CO2
PH3
MgBr2
Draw the Lewis structures for: KCl CaF2
Objectives
Draw the Lewis structures for covalent molecules
Predict the shape of a molecule given the formula.
Objectives
Distinguish between a polar and non-polar covalent bond.
Draw Lewis structures of compounds.
Review
Ionic Bond Between a metal and non-metal
Covalent Bond Between a non-metal and another non-
metal Two types: Polar and Non-polar covalent
Metallic Bond Between a metal and a metal
Electronegativity
The attraction an element has to electrons.
Scale of 0-4 Can be used to determine the type of
bond. 0-0.4 = Nonpolar covalent
0.41-1.7 = Polar CovalentGreater than 1.7 is ionic
Example
Identify the following bonds as polar or non-polar covalent:
H bonded to O H bonded to C C bonded to F C bonded to N
Warm Up
What are the three types of bonds? What is electronegativity? Determine the type of bond in:
Na2O CO2
CuZn
Objectives
Determine the type and number of atoms in a compound based on the formula.
Draw Lewis structures of ionic and covalent compounds.
What is a Chemical Formula? Tells you the elements in the compound.
Notated by the atomic symbol of the element.
Tells you the number of each element. Shown by the subscript number. No number
means 1. Note it is always a whole number!
Example
What type of elements and how many are in:
MgCl2
Example
What type of elements and how many are in:
NH3
Example
What type of elements and how many are in:
CF4
Example
Identify each element and amount of each element in the following compounds:
H2O CH4
NaCl Li2O
Lewis Structures
Combining of the dot diagrams to show bonding and to predict shape.
Every Element wants 8 electrons. 2 Types- covalent and ionic.
Ionic Lewis Structures
Step 1: Draw the lewis dot diagrams for each element.
Step 2: Draw an arrow from the metals electrons to the empty spaces around the nonmetal.
Step 3: Redraw the lewis dot diagrams showing the movement of electrons AND charges.
Example
Draw the Lewis structure for: NaCl
Example
Draw the Lewis structure for: LiF
Example
Draw the Lewis structure for: MgCl2
Example
Draw the Lewis structure for: Na2O
You Try
Draw the Lewis structure for: KI BeI2 SrF2
Warm Up
What elements and how many are present in: CO2
PH3
MgBr2
Draw the Lewis structures for: KCl CaF2
Objectives
Draw the Lewis structures for covalent molecules
Predict the shape of a molecule given the formula.
Steps for Lewis Structures
Step 1: Add up total number of valence electrons.Step 2: Draw a skeleton by connecting each element with a line. (Carbon, the solo element, or the most electronegative element goes in the middle)★Hydrogen and the Halogens CANNOT be in the center.Step 3: Distribute the electrons as PAIRS. Start from the outside and move inward. Step 4: Count and adjust electrons till each element has 8. (except Hydrogen)
Examples
Draw the lewis structures for the following:
CF4
Examples
Draw the lewis structures for the following:
H2O
Examples
Draw the lewis structures for the following:
PH3
Examples
Draw the lewis structures for the following:
O2
You Try
Draw the lewis structures for the following:
NH3
F2O CO2
Exit Card
Identify the type of bond as polar or non-polar:
CCl4 CH4
Identify the elements and their amounts of the compounds above.
Draw the Lewis structures for: NH3
CF4
Day 2
Warm Up
Classify the following bonds as ionic, polar covalent, or non-polar covalent.
F2
MgI2
NH3
Draw the Lewis structures for the following: F2
MgI2
NH3
Objectives
Predict the shape of a molecule based on the VSEPR theory.
VSEPR
Stands for “Valence shell Electron pair Repulsion”
V-Valence S-Shell E-Electron P-Pair R-Repulsion Basically Electrons don’t like each other
very much!
Steps for predicting shapes
Step 1: Draw the Lewis structures for the compound
Step 2: Draw a box around the central atom/element
Step 3: Predict the shape based on the following.
5 Shapes
Four single bonds-Tetrahedral 3 single bonds and 1 lone pair-Trigonal
Pyramidal 2 single, 1 double-Trigonal planar 2 bonds (any type) and lone pairs-Bent 2 bonds no lone pairs OR just 2 atoms-
Linear
Example
Predict the shape of the following: SO3
Example
Predict the shape of the following: H2O
Example
Predict the shape of the following: NH3
You Try
Predict the shape of the following PF3
MgCl2
SiO2
Exit Card
What does VSEPR stand for? List the five different shapes of
molecules. Predict the shape of the following: H2S O3 CCl4
Warm Up
What does VSEPR stand for? List the 6 different shapes of molecules. Predict the shape of the following: H2S O3 CCl4
Objectives
Predict the polarity of a molecule based on the structure of a molecule.
(Honors) Determine the intermolecular forces between two molecules
Polar and nonpolar…again
Molecules have an overall polarity in addition to polar and nonpolar bonds.
Polar molecules have unequal distribution of electrons.
while Nonpolar molecules have an equal
distribution of electrons.
How do you know if a molecule is polar?
First determine the shape of the molecule in question.
Then Predict the polarity of the molecule based on its shape. Bent, and trigonal pyramidal molecules are
ALWAYS polar. Tetrahedral, trigonal planar, and linear are
ALWAYS nonpolar.
How do you know if a molecule is polar?
Bent, and trigonal pyramidal molecules are ALWAYS polar.
Tetrahedral, trigonal planar, and linear are usually nonpolar. But can be polar, IF and ONLY IF there are 3 or more different elements. Ex. CH4 vs. CH2F2
Examples
Determine if the following molecules are polar or non-polar.
SiBr4
Examples
Determine if the following molecules are polar or non-polar.
OI2
Examples
Determine if the following molecules are polar or non-polar.
O3
Examples
Determine if the following molecules are polar or non-polar.
CO2
Examples
Determine if the following molecules are polar or non-polar.
S3O
Examples
Determine if the following molecules are polar or non-polar.
CSeF2
You Try
Determine if the following molecules are polar or non-polar.
NF3
SO2
H2S
Warm Up
Determine if the following molecules are polar or non-polar.
NF3
SiO2
H2S
Objectives
(Honors) Determine the intermolecular forces between two molecules.
Predict the properties of a molecule or compound
May the Forces be with You
Intramolecular forces- Intermolecular forces- the attractions between molecules that account for properties such as BP, MP, viscosity, surface tension, and solubility.
Types of Intermolecular Forces
Three types:
London Dispersion
Also called induced dipole Between non-polar molecules Very very weak
Dipole-Dipole
Between polar molecules Two oppositely charges ends.(one +
and one -)
Hydrogen Bonding
NOT a bond. Between hydrogen of one molecule
and fluorine, oxygen, or nitrogen of ANOTHER molecule.
Extremely strong.
Ranking Intermolecular Forces
The stronger the IM the higher the Bp and Mp.
Hydrogen Bonds >>> Dipole >> London
Example
Rank the following in order of increasing boiling point.
PH3
CH4
CO2
H2O
Example
Which will have a higher Mp? Why? NH3 or PH3
Example
Water boils at 100C and H2S boils at -60C, briefly explain why these two molecules have vastly different boiling points despite having similar structures and polarities.
You Try
Rank the following in order of increasing boiling point.
SBr2
NH3
SiO2
You Try
Rank the following in order of increasing boiling point.
F2O Cl2 Br2O
Properties of Ionic Substances Hard Brittle A solid at room temperature Very very high melting and boiling Points Soluble in water Conduct electricity when dissolved in
water or as a liquid.
Properties of Metals
Shiny Solid at room temperature. Very high melting and high boiling points Insoluble in water Conduct electricity Malleable and ductile
Properties of Polar Molecules
Typically a liquid at room temperature. Low melting points and boiling points Soluble in water Not a of conductor electricity
Properties of Non-polar molecules Typically a gas at room temperature. Very low melting and boiling points Insoluble in water Not a conductor of electricity.
Steps for determining properties. Step 1: Draw the Lewis structures of all
compounds involved. Step 2: Predict the shape of all
compounds Step 3: Based on the shape determine
the polarity of the compound Step 4: Once the polarity is determined
look up the properties for that type of compound.
Example
Which of the following will conduct electricity?
NaCl CO2
ZnCu H2O
Example
Which of the following will be a liquid at room temperature?
NaCl CO2
ZnCu H2O
Example
Which of the following will be a gas at room temperature?
NaCl CO2
ZnCu H2O
You Try
Predict the state of matter for each of the following at room temperature.
MgBr2
O3
SO3
HgZn
Exit Card
Determine if the molecule is polar or non-polar and predict the state of matter at room temperature:
NH3
HCl O2
CHF3
OF2
Warm Up
Determine the probable state of matter at room temperature for the following:
CS2
PH3
CBr4
H2O
Objectives
Predict the properties of the compounds based on the type of molecule.
Examples
Predict the state of matter at room temperature of:
CO2
SrF2
PCl3
Exit Card
List one property of ionic compounds, metallic compounds, polar compounds, and non-polar compounds.
Predict the state of matter for the following at room temperature.
H2O NH3
Cu-Zn BaO
Warm Up
What is the typical state of matter for: Ionic substances Polar compounds Non-polar compounds Which of the following would have the
highest boiling point? Lowest? CO2, Na2O, H2O
Warm Up
Determine the polarity of: SO3
H2S
Objectives
Predict the properties of a substance based on the type of compound and its’ polarity.
(Honors) Describe the intermolecular forces present in molecules.
(Honors) Rank molecules based on the intermolecular forces involved.
Properties of Ionic Substances Hard Brittle A solid at room temperature Very high melting points (≈800C) Very high boiling Points Soluble in water Conduct electricity when dissolved in
water or as a liquid.
Properties of Metals
Shiny Solid at room temperature. Very very high melting point (≈1000C) Very Very high boiling point Insoluble in water Conduct electricity Malleable and ductile
Properties of Polar Molecules
Typically a liquid at room temperature. Low melting points (≈20C) Medium boiling points Soluble in water Not a of conductor electricity
Properties of Non-polar molecules Typically a gas at room temperature. Very low melting (≈-100C) Very low boiling points Insoluble in water Not a conductor of electricity.
How to Determine Properties First: Draw the Lewis structures of all
compounds involved. Next: Predict the shape of all compounds Then: Based on the shape determine the
polarity of the compound Finally: Once the polarity is determined
look up the properties for that type of compound.
Example
Which of the following will conduct electricity?
NaCl CO2
ZnCu H2O
Example
Which of the following will be a liquid at room temperature?
NaCl CO2
ZnCu H2O
Example
Which of the following will be a gas at room temperature?
NaCl CO2
ZnCu H2O
You Try
Predict the state of matter for each of the following at room temperature.
MgBr2
O3
SO3
HgZn
Exit Card
Which of the following would dissolve in water: NaCl CH4
NH3
Rank the following in order of increasing boiling point:
NH3
CO2
CSF2
Exit Card
Which of the following would dissolve in water: NaCl CH4
NH3
Rank the following in order of increasing boiling point:
NH3
CO2
CSF2
Warm Up
Identify the type of compounds as ionic, covalent, metalic:
CaS BrF Draw the Lewis Structure for AsI3, predict
the shape, determine its polarity, and predict its’ state of matter at room temperature.
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