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.
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.
