Unit 2.1: Lewis Dot Structures and Ionic Bonding
Unit 2.1: Lewis Dot Structures and Ionic
Bonding
Bell Work October 6
Agenda:1.Turn in Test Corrections and anything you forgot to turn in while I was gone2.Planner: No Homework3.Notes4.Lewis Dot Structure Activity
Bell Work:
•Write down 2 things you learned while I was on Outdoor Ed.
•My Favorite Demonstration of All Time
Chemical Reactions
• When substances react and new substances form• Chemical Bond: the force of attraction that holds two atoms together as
a result of the rearrangement of electrons between them.• When atoms bond, electrons may be transferred from one atom to
another or shared between the atoms. • Chemical Reactions are shown with chemical equationsChemical Reactions Video
Chemical Equations
• Show the rearrangement of atoms to form new substances in a chemical reaction• Example:
• CH4 + 2O2 CO2 + 2H2O
• Reactants: The substances that react; what you start with (left side of arrow)• Products: The substances that are produced; what you make (right side
of arrow)
Reading a Chemical Equation
• CH4 + 2O2 CO2 + 2H2O• CH4: Methane• O2: Oxygen• CO2: Carbon Dioxide• H2O: Water
• “Methane and oxygen react to form carbon dioxide and water”• + : “and”• : “react to form”• Coefficients are the number of molecules of each substance
Valence Electrons
• Electrons in the outermost shell of an atom• Atoms can give away, take away, or share
electrons to get to 0 or 8 valence electrons• Remember, they want an empty or full
valence shell, if they don’t have one then they are unstable (HAPPY OCTOPUS!)
Lewis Dot Structures of Elements• Lewis Dot structures are used to show valence
electrons• Can be helpful when predicting how elements bond• Rules:
• Look on the periodic table to determine how many valence electrons are in an element
• Write the symbol of the element• Imagine that the element is in a box with 4 sides• Start on top and rotate clockwise putting one dot (electron)
at a time• Continue to circle, double electrons when needed. • Do not add more than 2 electrons to each side
Write the Lewis Dot Structure for the following Elements:
• Lithium (Li):
• Aluminum (Al):
• Bromine (Br):
Bell Work October 7
Agenda:1.Turn in Article and Article Summary2.Planner: Lewis Dot Structure of Ionic Compounds3.Lewis Dot Structure Activity4.Notes
Ions1. An Ion is a charged particle2. The number of electrons is NOT equal to the
number of protons3. Atoms become charged particles when they
gain or lose electrons
Cations and Anions
Naming Ions
What type of Ions do each group form?• Remember, elements are lazy, they do whatever is easiest• They want to either gain or lose electrons to get to 0 or 8 valence
electrons• Example:• If I have 1-3 valence electrons, it is easier to lose electrons than to gain them• If I have 5-7 valence electrons, it is easier to gain electrons than to lose them• IF I have 4, I could go either way
Bell Work October 8
Agenda:1.Planner: Lewis Dot Structure of Ionic Compounds2.Notes3.Lewis Dot Structure of Ionic Compounds 4.Notes5.Lattice Structure Activity6.Notes
Bell Work:•Label the following as a metal or a nonmetal. Label if it will form a cation or an anion.• N• Al• F• Li
Ionic Charges
• Atom gaining electrons = anion• Adding a negatively charged particle makes the atom more negative
• Atoms losing electrons = cation• Taking away an electron means you take away something that is negative. This
makes the atom more positive
• Example:• Negative people in your life will make you more negative• If you get rid of this negative person, then you will be happier or more positive
Ions form Ionic Bonds
• Electrons are TRANSFERRED from one atom to another to form ions• This creates a negatively charged ion (anion) and a
positively charged ion (cation)•Opposites attract, the anion is attracted to the cation,
this creates an IONIC BOND•Dogs Teach Bonding Video
Ions form Ionic Bonds
•Transfer of electrons from metals to nonmetals•All Ionic Bonds are called “Salts”•Ionic Bonds are weak, compared to other types of bonds•Bond between METAL and NONMETAL
Lewis Dot Structures of Ionic Compounds
• Na + Cl
• K + F
• Be + I + I
Properties of Ionic Bonds
• Solubility: the ability to dissolve in a solvent (typically water, but can include other liquids such as alcohols)•Conductivity: describes if a substance can carry
electric current•Melting Points: temperature at which compounds
melt (Celsius)
Crystal Lattice
• Styrofoam Ball Activity
•Positive ions (cations)
are attracted to
negative ions (anions)
Solubility
• Solubility: Ability to dissolve in a solvent• Insoluble: Not Soluble (Does not dissolve)• Partially Soluble: Only partially dissolves• Ionic compounds tend to dissolve well in water or alcohol but not in
things like oil
Solubility
•When ionic compounds dissolve, they are pulled out of their lattice structure and into their ionic state•Dissociation: when ionic compounds are pulled into their ions and out of their lattice structure• Ionic Dissociation Animation
Conductivity
• Conductivity: The ability to conduct electricity• Ionic compounds are not conductive in their solid state• They are conductive in their liquid state because the ions are
dissociated• Aqueous: Dissolved in water• Electrolyte an aqueous salt solution• Conductivity Animation
Melting Point
•Melting Point (MP): temperature at which compounds melt•Melting Points are extremely high for ionic compounds due to their lattice structure and the strength of their bond
Flame Test
•Metals turn a very specific color when exposed to flame if they are in an ionic compound•Every metal has it’s own specific color•You can identify an unknown metal by the color of the flame•They use this for fireworks!