2023 F CH202-4-6 - M1 Review Lecture Worksheet

In order to have a large partial positive charge to be involved in a hydrogen bond, the molecule must be polar and have a In order to have a large partial negative charge to be involved in a hydrogen bond, the molecule must be polar and have an a. F-H, O-H, or N-H bond b. F, O, or N

Is the compound soluble or insoluble in water? What is the geometry around each carbon atom?  What is the bond angle around each carbon atom? What is the hybridization of each carbon atom?

11. ВеСI, а. Lewis structure b. Drawing of shape (label angles) Name of shape C. d. Polar or nonpolar? e. Hybridization 12. BF, a. Lewis structure b. Drawing of shape (label angles) Name of shape С. d. Polar or nonpolar? e. Hybridization

Which statement A-D about VSEPR theory is not correct? Select one: a. The molecular shape or geometry can differ from the electron- pair geometry. b. Statements A-D are all correct. c. The steric number of a central atom is the sum of the number of bonds and lone pairs around the atom. d. In VSEPR theory, th shape or geometry of a molecule is determined by electron-electron repulsion. e. The steric number has five values from 2 to 6.

4. The H-O-H bond angle of water is 104.5°, which is less than the ideal tetrahedral bond angle of 109.5°. The reason for this is: Water is a liquid. Bonding pairs of electrons occupy more space than lone pairs of electrons. c. Water does not have a tetrahedral electron a. b. geometry. d. Water has a bent electron geometry. e. Lone pairs of electrons occupy more space than bonding pairs of electrons.

Which of the following can be best explained by temporary dipole moments? Choose one or more: A. This explains why ammonia and nitrogen gas exhibit an attractive force between them. B. This explains how the molecules hydrogen fluoride and methanol can exhibit uncharacteristically strong intermolecular forces. C. This explains why long hydrocarbon chains have relatively high boiling points. D. This explains how two noble gases' molecules can have an attractive force between them. E. This explains why the dipole-dipole attractive force between dimethyl ether and acetone does not entirely account for the attractive force between these molecules.

24

Please refer to the photo! Thank you so much!

1. Draw a single valid Lewis structure for the molecule. 2. Identify the number of charge clouds around the central atom. 3. Identify the approximate bond angle of the charge clouds around the central atom.4. Identify the molecular geometry corresponding to the bond angles.5. classify as polar or nonpolar

Question 5

14 and 15 only

Which statement A-D about VSEPR theory is not correct? Select one: a. The steric number has five values from 2 to 6. b. Statements A-D are all correct. c. In VSEPR theory, the shape or geometry of a molecule is determined by electron-electron repulsion. d. The steric number of a central atom is the sum of the number of bonds and lone pairs around the atom. e. The molecular shape or geometry can differ from the electron-pair geometry.

7. Identify the type of bond and strongest intermolecular forces between the particles of each of the following a. Clh b. HF c. Sic Identaly and explain. bigher melting point aNaCl or HCI DOLL

Complete the statement of the trend, name the type of forces that account for each trend, and explain how the forces account for each trend: 1. The larger a molecular substance, the its m.p. and b.p. its m.p. and b.p. 2. The more polar a molecular substance, the 3. Molecular substances containing H bonded to N, O, or F have extremely m.p. and b.p.

What is the electron -group geometry and molecular geometry around the oxygen in the structure to the right? A linear, linear B. linear, angular C. tetrahedral, linear D. tetrahedral, angular tetrahedral, tetrahedral H— I—0—I -0-H