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      • Measurement Lesson 1
      • Measurement Lesson 2 Scientific Measurements
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    • 1. Matter & Energy >
      • Matter Lesson 1 Types of Matter
      • Matter Lesson 2 Mixtures and Separation
      • Matter Lesson 3 Properties and Changes
      • Matter Lesson 4 Phases of Matter
      • Energy Lesson 5 Heating and Cooling Curves
      • Energy Lesson 6 Heat Definitions
      • Energy Lesson 7 Calculating Heat
    • 2. Gas laws >
      • Gas Laws Lesson 1 Gas Laws
      • Gas Laws Lesson 2 Combined Gas Law
    • 3. Atomic Theory & Periodic Table >
      • Lesson 1 Atomic Theory
      • Lesson 2 Subatomic Particles
      • Lesson 3 Foundations of PT
      • Lesson 4 Types of Elements
      • Lesson 5 Electrons
      • Lesson 6 Atoms vs Ions
      • Lesson 7 Oxidation Numbers
      • Lesson 8 Electron Dot Diagrams
      • Lesson 9 Isotopes
      • Lesson 10 Periodic Trends
    • 4. Bonding >
      • Bonding Lesson 1 Basics
      • Bonding Lesson 2 Ionic Bonds
      • Bonding Lesson 2b Stock System
      • Bonding Lesson 3 Covalent Bonds
      • Bonding Lesson 3b Naming Covalent Bonds
      • Bonding Lesson 3c Multiple Bonds and Bond Strength
      • Bonding Lesson 4 Metallic Bonds
      • Bonding Lesson 5 Symmetry
      • Bonding Lesson 6 IMF
    • 5. Nuclear >
      • Nuclear Lesson 1 Transmutation
      • Nuclear Lesson 2 Radioisotope Uses
      • Nuclear Lesson 3 Radiation Penetration
      • Nuclear Lesson 4 Artificial Transmutation
      • Nuclear Lesson 5 Half Life
    • 6. Formulas and Equations >
      • Formulas & Equations Lesson 1 Types of Formulas
      • Formulas & Equations Lesson 2 Types of Reactions
      • Formulas & Equations Lesson 3 Balancing Equations
    • Semester 2 >
      • 10. Math & Moles >
        • Math Lesson 1 Mass
        • Math Lesson 2 Percent Composition
        • Math Lesson 3 Avogadro
        • Math Lesson 4 Molecular Formula from Empirical
        • Math Lesson 5 Mole Ratios
      • 11. Solutions >
        • Solutions Lesson 1 Solutions
        • Solutions Lesson 2 Solubility
        • Solutions Lesson 3 Concentration
        • Solutions Lesson 4 Colligative Properties
      • 12. Acids & Bases >
        • Acids and Bases Lesson 1 Properties
        • Acids and Bases Lesson 2 Naming
        • Acids and Bases Lesson 3 Reactions
        • Acids and Bases Lesson 4 pH Scale
        • Acids and Bases Lesson 5 Indicators
      • 13. Kinetics & Equilibrium >
        • Kinetics & Equilibrium Lesson 1 Collision Theory and Factors
        • Kinetics & Equilibrium Lesson 2 PE Diagrams
        • Kinetics & Equilibrium Lesson 3 Equilibrium
        • Kinetics & Equilibrium Lesson 4 LeChateliers Principle
        • Kinetics & Equilibrium Lesson 5 Entropy and Enthalpy
      • 14. Oxidation Reduction >
        • RedOx Lesson 2 RedOx Reactions
        • RedOx Lesson 3 Half Reactions
        • RedOx Lesson 4 Spontaneous Reactions
        • RedOx Lesson 5 Electrochemical Cells
      • 15. Organic >
        • Organic Lesson 1 Intoduction
        • Organic Lesson 2 Hydrocarbons
        • Organic Lesson 3 Functional Groups
        • Organic Lesson 4 Reactions
  • Review Material
    • Textbook Unit Review Sheets
  • NYS Chemistry Curriculum

Bonding & Intermolecular Forces of Attraction

Learning Objectives for Bonding
1. I can determine changes in energy when bonds are broken (endo) and when bonds are formed (exo). BARF
2. I can predict whether an atom will lose or gain electrons depending on where it is on the periodic table. I can also determine how this will affect the radius of the ion (lose e- get smaller; gain e- get bigger).
3. I can identify they three types of bonds as ionic (transfer of electrons), covalent (share electrons) or metallic (sea of mobile electrons).
4. I can calculate electronegativity differences to assist in determining bond type (*CAUTION – there are exceptions to the rule).  I can also use this information to determine the degree of polarity (as the electronegativity difference increases, so does the polarity).
5. I can determine how many pairs of electrons are shared by looking at the valence electrons (O has 6 so 2; F has 7 so 1; N has 5 so 3).
6. I can recall that certain elements are not found in nature and will bond with themselves if there are no other options.These elements are Br2I2N2Cl2H2O2F2.
7. I can associate the term molecule with compounds that are covalent (share electrons).
8. I can identify covalent (share electrons) bonds as either polar (unequal sharing of electrons) or non-polar (equal sharing of electrons); and that the element with the higher electronegativity will have a stronger pull on the electrons being shared.
9. I can identify compounds that contain polyatomic ions (Table E) as ones that are both ionic and covalent.

​Learning Objectives for Intermolecular Forces of Attraction
10. I can recall that the term molecular represent two nonmetals bonded together sharing electrons.
11. I can comprehend that Hydrogen bonding is not a bond but a force of attraction between molecules when hydrogen is bonded to either F, O, N.This strong force of attraction will cause these molecules to have higher boiling than other elements in their families when bonded with hydrogen.
12. I can use the symmetry of the shape of molecules to determine the polarity.If the molecule is symmetrical then it is nonpolar; if it is asymmetrical then it is polar. SNAP
13. I can explain using van der Waal’s forces why the elements of group 17 are found in all three phases of matter (s,l,g); as the mass increases so does the force of attraction between the molecules.
14. I can draw molecules to show how dipole-dipole forces of attraction cause the molecules to adjust so that the partially positive end of one molecule will line up with the partially negative end of another molecule.
15. I can draw diagrams to show molecule-ion attractions.
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