Notes: 9.5 OBJECTIVES: Students will be able to (SWBAT)

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Presentation transcript:

Notes: 9.5 OBJECTIVES: Students will be able to (SWBAT) Determine the polarity of molecules QUESTIONS TO PONDER: What is electronegativity? How do you determine the bond character or type between 2 atoms? What symbols are used to represent a dipole moment? What does the polarity of a molecule depend on? In order to determine the polarity of a molecule, what would be the first thing you should do?

Electronegativity and Polarity (Chapter 9, Section 5)

Electronegativity (EN) Difference EN is a comparison of e- pulling strength EN difference = difference of EN values of 2 atoms Bigger EN value (chart on page 263)  stronger pull on electrons Differences higher than 0 UNEQUAL SHARING OF ELECTRONS (more pull of e- to one side) 2.55 2.55 Difference = 2.55 – 2.55 = 0

Bond Character Metal & nonmetal  IONIC  large difference (opposite sides of PT) Nonmetal & nonmetal  COVALENT  small difference (close to each other on PT) 2 types of covalent bond Non-polar covalent EN difference is very small  equal sharing of e- Polar covalent EN differences is higher  unequal sharing of e-

Bond Types EN DIFFERNCE

FULL POSITIVE CHARGE FULL NEGATIVE CHARGE

Polar Covalent Bonds and Dipole Moments “δ” – means “partial” Arrow points toward negative side Cross is at the positive side Arrow represents a DIPOLE MOMENT where one side is partially + and one side is partially - 2.6 4.0 4.0 – 2.6 = 1.4 Polar covalent

State whether IONIC, NONPOLAR COVALENT or POLAR COVALENT Cl-Cl | 3.0 – 3.0 | = 0.0 nonpolar covalent H-S | 2.1 – 2.5 | = 0.4 polar covalent Na-Cl | 0.9 – 3.0 | = 2.1 ionic O-H | 3.5 – 2.1 | = 1.4 polar covalent I-Br | 2.5 – 2.8 | = 0.3 nonpolar covalent Fe-O | 1.8 – 3.4 | = 1.6 polar covalent

Polarity of Molecules Polarity of an entire compound depends on: Dipole moment of each bond Shape and symmetry of the molecule Location of lone pairs Add/combine all dipole moments (arrows) for the TOTAL DIPOLE MOMENT of the molecule Side with lone pairs have more partial negative charge

δ+ δ- δ+ δ- Combined dipole moment:

Practice nonpolar N2 nonpolar HF polar CH4 nonpolar polar NH3 nonpolar CH3F polar nonpolar polar nonpolar polar polar