AP Chemistry Chapter 8 – Bonding

AP Chemistry Chapter 8 – Bonding

AP Chemistry Chapters 8 & 9 – Bonding Study Guide

Students should be able to。。。

∙Define: chemical bond, ionic, covalent, metallic, diatomic, polar, nonpolar, and VSEPR ∙Use electronegativity to determine the type of bond formed between two elements

∙Calculate bond energies.

∙Determine the polarity of a dipole.

∙Draw Lewis structures for covalent molecules, including double and triple bonds。

∙Draw Lewis structures for polyatomic ions

∙Use formal charge to determine the best Lewis structure

∙Use VSEPR chart to determine electron arrangement and molecular geometry.

∙Use VSEPR chart to write Lewis structures that include bond angles。 Be able to draw resonance structures for covalent molecules

∙Calculate the enthalpy of formation, lattice energy, and associated information.

∙Determine hybridization of orbitals within a molecule

∙Identify sigma and pi bonds

Sample AP Problems from Bonding:

Questions 8-10 refer to the following diatomic species.

(A) Li2

(B) B2

(C) N2

(D) O2

(E) F2

8. Has the largest bond-dissociation energy

9. Has a bond order of 2

10. Contains 1 sigma (s) and 2 pi (p) bonds

15. In a molecule in which the central atom exhibits sp3d2 hybrid orbitals, the electron pairs are directed toward the corners of

(A) a tetrahedron

(B) a square-based pyramid

(C) a trigonal bipyramid

(D) a square

(E) an octahedron

17。 The Lewis dot structure of which of the following molecules shows only one unshared pair of valence electron?

(A) Cl2

(B) N2

(C) NH3

(D) CCl4

(E) H2O2

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