Warm Up  What are the three types of bonds?   Determine the type of bond, and how many of each element are present in:  Na 2 O   CO 2   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:  MgCl 2

Example  Draw the Lewis structure for:  Na 2 O

You Try  Draw the Lewis structure for:  KI   BeI 2   SrF 2

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:  CF 4

Examples  Draw the lewis structures for the following:  H 2 O

Examples  Draw the lewis structures for the following:  PH 3

Examples  Draw the lewis structures for the following:  O 2

You Try  Draw the lewis structures for the following:  NH 3   F 2 O   CO 2

Warm Up  What elements and how many are present in:  CO 2   PH 3   MgBr 2  Draw the Lewis structures for:  KCl   CaF 2

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.  = Nonpolar covalent = Polar Covalent Greater 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:  Na 2 O  CO 2  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:  MgCl 2

Example  What type of elements and how many are in:  NH 3

Example  What type of elements and how many are in:  CF 4

Example  Identify each element and amount of each element in the following compounds:  H 2 O  CH 4  NaCl  Li 2 O

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:  MgCl 2

Example  Draw the Lewis structure for:  Na 2 O

You Try  Draw the Lewis structure for:  KI   BeI 2   SrF 2

Warm Up  What elements and how many are present in:  CO 2   PH 3   MgBr 2  Draw the Lewis structures for:  KCl   CaF 2

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:  CF 4

Examples  Draw the lewis structures for the following:  H 2 O

Examples  Draw the lewis structures for the following:  PH 3

Examples  Draw the lewis structures for the following:  O 2

You Try  Draw the lewis structures for the following:  NH 3   F 2 O   CO 2

Exit Card  Identify the type of bond as polar or non-polar:  CCl 4  CH 4  Identify the elements and their amounts of the compounds above.  Draw the Lewis structures for:  NH 3  CF 4

Day 2

Warm Up  Classify the following bonds as ionic, polar covalent, or non-polar covalent.  F 2   MgI 2   NH 3  Draw the Lewis structures for the following:  F 2   MgI 2   NH 3

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:  SO 3

Example  Predict the shape of the following:  H 2 O

Example  Predict the shape of the following:  NH 3

You Try  Predict the shape of the following  PF 3   MgCl 2   SiO 2 

Exit Card  What does VSEPR stand for?  List the five different shapes of molecules.  Predict the shape of the following:  H 2 S  O 3  CCl 4

Warm Up  What does VSEPR stand for?  List the 6 different shapes of molecules.  Predict the shape of the following:  H 2 S   O 3   CCl 4

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. CH 4 vs. CH 2 F 2

Examples  Determine if the following molecules are polar or non-polar.  SiBr 4

Examples  Determine if the following molecules are polar or non-polar.  OI 2

Examples  Determine if the following molecules are polar or non-polar.  O 3

Examples  Determine if the following molecules are polar or non-polar.  CO 2

Examples  Determine if the following molecules are polar or non-polar.  S 3 O

Examples  Determine if the following molecules are polar or non-polar.  CSeF 2

You Try  Determine if the following molecules are polar or non-polar.  NF 3   SO 2   H 2 S

Warm Up  Determine if the following molecules are polar or non-polar.  NF 3   SiO 2   H 2 S

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.  PH 3  CH 4  CO 2  H 2 O

Example  Which will have a higher Mp? Why?  NH 3 or PH 3

Example  Water boils at 100C and H 2 S 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.  SBr 2  NH 3  SiO 2

You Try  Rank the following in order of increasing boiling point.  F 2 O  Cl 2  Br 2 O

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   CO 2   ZnCu   H 2 O

Example  Which of the following will be a liquid at room temperature?  NaCl   CO 2   ZnCu   H 2 O

Example  Which of the following will be a gas at room temperature?  NaCl   CO 2   ZnCu   H 2 O

You Try  Predict the state of matter for each of the following at room temperature.  MgBr 2   O 3   SO 3   HgZn

Exit Card  Determine if the molecule is polar or non-polar and predict the state of matter at room temperature:  NH 3  HCl  O 2  CHF 3  OF 2

Warm Up  Determine the probable state of matter at room temperature for the following:  CS 2   PH 3   CBr 4   H 2 O

Objectives  Predict the properties of the compounds based on the type of molecule.

Examples  Predict the state of matter at room temperature of:  CO 2   SrF 2   PCl 3

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.  H 2 O  NH 3  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?  CO 2, Na 2 O, H 2 O

Warm Up  Determine the polarity of:  SO 3   H 2 S

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   CO 2   ZnCu   H 2 O

Example  Which of the following will be a liquid at room temperature?  NaCl   CO 2   ZnCu   H 2 O

Example  Which of the following will be a gas at room temperature?  NaCl   CO 2   ZnCu   H 2 O

You Try  Predict the state of matter for each of the following at room temperature.  MgBr 2   O 3   SO 3   HgZn

Exit Card  Which of the following would dissolve in water:  NaCl  CH 4  NH 3  Rank the following in order of increasing boiling point:  NH 3  CO 2  CSF 2

Exit Card  Which of the following would dissolve in water:  NaCl  CH 4  NH 3  Rank the following in order of increasing boiling point:  NH 3  CO 2  CSF 2

Warm Up  Identify the type of compounds as ionic, covalent, metalic:  CaS  BrF  Draw the Lewis Structure for AsI 3, predict the shape, determine its polarity, and predict its’ state of matter at room temperature.