LO 1.7 The student is able to describe the electron structure of the atom, using PES (photoelectron spectroscopy) data, ionization energy data, and/or.

LO 1.7 The student is able to describe the electron structure of the atom, using PES (photoelectron spectroscopy) data, ionization energy data, and/or Coulomb’s Law to construct explanations of how the energies of electrons within shells in atoms vary. (Sec 9.6) LO 1.15 The student can justify the selection of a particular type of spectroscopy to measure properties associated with vibrational or electronic motions of molecules. (Sec 9.6) LO 2.18 The student is able to rank and justify the ranking of bond polarity on the basis of the locations of the bonded atoms in the periodic table. (Sec 9.4) LO 2.21 The student is able to use Lewis diagrams and VSEPR to predict the geometry of molecules, identify hybridization, and make predictions about polarity. (Sec 9.1, 9.6)

AP Learning Objectives, Margin Notes and References
LO 2.21 The student is able to use Lewis diagrams and VSEPR to predict the geometry of molecules, identify hybridization, and make predictions about polarity.

Draw the Lewis structure for methane, CH4.
EXERCISE! Draw the Lewis structure for methane, CH4. What is the shape of a methane molecule? tetrahedral What are the bond angles? 109.5o The shape of CH4 is tetrahedral. The bond angles are 109.5o. Copyright © Cengage Learning. All rights reserved

What is the valence electron configuration of a carbon atom? s2p2
CONCEPT CHECK! What is the valence electron configuration of a carbon atom? s2p2 Why can’t the bonding orbitals for methane be formed by an overlap of atomic orbitals? The valence electron configuration of a carbon atom is s2p2. Because this would lead to two different types of C-H bonds and we know that methane has four identical C-H bonds that are 109.5° apart from each other (not 90° from each other). Copyright © Cengage Learning. All rights reserved

sp3 Hybridization Combination of one s and three p orbitals.
Whenever a set of equivalent tetrahedral atomic orbitals is required by an atom, the localized electron model assumes that the atom adopts a set of sp3 orbitals; the atom becomes sp3 hybridized. The four orbitals are identical in shape. Copyright © Cengage Learning. All rights reserved

An Energy-Level Diagram Showing the Formation of Four sp3 Orbitals
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The Formation of sp3 Hybrid Orbitals

Tetrahedral Set of Four sp3 Orbitals

Draw the Lewis structure for C2H4 (ethylene)?
EXERCISE! Draw the Lewis structure for C2H4 (ethylene)? What is the shape of an ethylene molecule? trigonal planar around each carbon atom What are the approximate bond angles around the carbon atoms? 120o The shape of an ethylene molecule is trigonal planar around each carbon atom. The approximate angles are 120o. Copyright © Cengage Learning. All rights reserved

Why can’t sp3 hybridization account for the ethylene molecule?
CONCEPT CHECK! Why can’t sp3 hybridization account for the ethylene molecule? Because sp3 hybrid orbitals are at angles of 109.5o rather than the required 120o. Copyright © Cengage Learning. All rights reserved

sp2 Hybridization Combination of one s and two p orbitals.
Gives a trigonal planar arrangement of atomic orbitals. One p orbital is not used. Oriented perpendicular to the plane of the sp2 orbitals. Copyright © Cengage Learning. All rights reserved

An Orbital Energy-Level Diagram for sp2 Hybridization

The Hybridization of the s, px, and py Atomic Orbitals

Formation of C=C Double Bond in Ethylene
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Draw the Lewis structure for CO2.
EXERCISE! Draw the Lewis structure for CO2. What is the shape of a carbon dioxide molecule? linear What are the bond angles? 180o The shape of CO2 is linear. The bond angles are 180o. Copyright © Cengage Learning. All rights reserved

sp Hybridization Combination of one s and one p orbital.
Gives a linear arrangement of atomic orbitals. Two p orbitals are not used. Needed to form the π bonds. Copyright © Cengage Learning. All rights reserved

The Orbital Energy-Level Diagram for the Formation of sp Hybrid Orbitals on Carbon

Draw the Lewis structure for PCl5.
EXERCISE! Draw the Lewis structure for PCl5. What is the shape of a phosphorus pentachloride molecule? trigonal bipyramidal What are the bond angles? 90o and 120o The shape is trigonal bipyramidal with bond angles of 90o and 120o. Copyright © Cengage Learning. All rights reserved

dsp3 Hybridization Combination of one d, one s, and three p orbitals.
Gives a trigonal bipyramidal arrangement of five equivalent hybrid orbitals. Copyright © Cengage Learning. All rights reserved

The Orbitals Used to Form the Bonds in PCl5

Draw the Lewis structure for XeF4.
EXERCISE! Draw the Lewis structure for XeF4. What is the shape of a xenon tetrafluoride molecule? octahedral What are the bond angles? 90o and 180o The shape is octahedral with bond angles of 90o and 180o. Copyright © Cengage Learning. All rights reserved

d2sp3 Hybridization Combination of two d, one s, and three p orbitals.
Gives an octahedral arrangement of six equivalent hybrid orbitals. Copyright © Cengage Learning. All rights reserved

How is the Xenon Atom in XeF4 Hybridized?

Draw the Lewis structure for HCN. Which hybrid orbitals are used?
CONCEPT CHECK! Draw the Lewis structure for HCN. Which hybrid orbitals are used? Draw HCN: Showing all bonds between atoms. Labeling each bond as σ or π. sp hybrid orbitals are used in the bonding of HCN. Two sigma bonds and two pi bonds are present. Copyright © Cengage Learning. All rights reserved

CONCEPT CHECK! Determine the bond angle and expected hybridization of the central atom for each of the following molecules: NH3 SO2 KrF2 CO2 ICl5 NH3 – 109.5o, sp3 SO2 – 120o, sp2 KrF2 – 90o, 120o, dsp3 CO2 – 180o, sp ICl5 – 90o, 180o, d2sp3 NH3 – 109.5o, sp3 SO2 – 120o, sp2 KrF2 – 90o, 120o, dsp3 CO2 – 180o, sp ICl5 – 90o, 180o, d2sp3

Using the Localized Electron Model
Draw the Lewis structure(s). Determine the arrangement of electron pairs using the VSEPR model. Specify the hybrid orbitals needed to accommodate the electron pairs. Copyright © Cengage Learning. All rights reserved

LO 2.18 The student is able to rank and justify the ranking of bond polarity on the basis of the locations of the bonded atoms in the periodic table.

Heteronuclear Diatomic Molecule: HF
The 2p orbital of fluorine is at a lower energy than the 1s orbital of hydrogen because fluorine binds its valence electrons more tightly. Electrons prefer to be closer to the fluorine atom. Thus the 2p electron on a free fluorine atom is at a lower energy than the 1s electron on a free hydrogen atom. Copyright © Cengage Learning. All rights reserved

Orbital Energy-Level Diagram for the HF Molecule

The diagram predicts that the HF molecule should be stable because both electrons are lowered in energy relative to their energy in the free hydrogen and fluorine atoms, which is the driving force for bond formation. Copyright © Cengage Learning. All rights reserved

The Electron Probability Distribution in the Bonding Molecular Orbital of the HF Molecule

The σ molecular orbital containing the bonding electron pair shows greater electron probability close to the fluorine. The electron pair is not shared equally. This causes the fluorine atom to have a slight excess of negative charge and leaves the hydrogen atom partially positive. This is exactly the bond polarity observed for HF. Copyright © Cengage Learning. All rights reserved

LO 1.7 The student is able to describe the electron structure of the atom, using PES (photoelectron spectroscopy) data, ionization energy data, and/or Coulomb’s Law to construct explanations of how the energies of electrons within shells in atoms vary. LO 1.15 The student can justify the selection of a particular type of spectroscopy to measure properties associated with vibrational or electronic motions of molecules. LO 2.21 The student is able to use Lewis diagrams and VSEPR to predict the geometry of molecules, identify hybridization, and make predictions about polarity. Additional AP References LO 1.15 (see APEC #1 “Energy Levels and Electron Transitions”) LO 1.15 (see Appendix 7.4 “Molecular Spectroscopy: An Introduction”)

Can be used to determine the relative energies of electrons in individual atoms and molecules.
High-energy photons are directed at the sample, and the kinetic energies of the ejected electrons are measured. Copyright © Cengage Learning. All rights reserved

LO 1.7 The student is able to describe the electron structure of the atom, using PES (photoelectron spectroscopy) data, ionization energy data, and/or.

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LO 1.7 The student is able to describe the electron structure of the atom, using PES (photoelectron spectroscopy) data, ionization energy data, and/or.

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Presentation on theme: "LO 1.7 The student is able to describe the electron structure of the atom, using PES (photoelectron spectroscopy) data, ionization energy data, and/or."— Presentation transcript:

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