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

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

What information does the molecular representation provide? (more than one option)1. The number and type of atoms2. Two-dimensional structure of molecules3. The type of link4. How Atoms Bond5. The intermolecular force6. Three-dimensional structure of molecules7. Polarity8. More realistic representation of molecules

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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

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

6. Circle the molecule below with the lower boiling point Explain why NH2

5. Answer the following questions about the molecules CH2S (C is the centralatom).a. Draw the Lewis structure.b. Write the valence shell electron configuration for C.c. Draw the valence orbital diagram for C.d. Draw the hybridized orbital diagram for C.e. Give a bond description for each bond in the molecule.

Please help with this last question thank you.

. Draw the Lewis diagram for acetamide. ( CH3CONH2)                                                                                        a. What is the electron geometry around each of the two carbon atoms.                                                  b. What is the hybridization type of each of the carbon atoms.                                                               c. What are the bond types and orbitals involved in bonding for all bonds between the C and O atoms.

8. SO3 а. Lewis structure b. Drawing of shape (label angles) С. Name of shape d. Polar or nonpolar? e. Hybridization 9. NO, Lewis structure a. b. Drawing of shape (label angles) c. Name of shape d. Polar or nonpolar? e. Hybridization 10. ΗΝΟ, а. Lewis structure b. Drawing of shape (label angles) Name of shape С. d. Polar or nonpolar? , e. Hybridization 11 RoCl

1) Consider the following 2 molecules: arsane which has the molecular formula AsH3, and dimethylether, an ether which has the molecular formula C2H6O.Which of these molecules is polar? a. Dimethylether is polar but arsane is not. b. Both are polar. c. Neither are polar. d. Arsane is polar but dimethylether is not.   Consider a pure sample of silane which has the formula SiH4. Of the options listed below, what is the strongest attractive force in this sample? a. Ionic bonding b. Ion-dipole forces c. Hydrogen bonding d. Dispersion forces e. Dipole-dipole forces

Number of Molecule valence electrons Formal Charge Electron-Group Geometry Molecular Geometry Resonance HSO4 S: S: Select one . S: Select one .. Select one XeTe4 Хе: Xe: Select one ... Xe: Select one .. Select one PHO P: P: Select one ... P: Select one .. Select one ... v PCIO P: P: Select one ... P: Select one .. Select one ..

CH3F is a polar molecule, even though the tetrahedral geometry often leads to nonpolar molecules.  Which of the following reasons below explains why CH3F is a polar molecule? A. None of the above gives a valid explanation. B. Even though CH3F has a tetrahedral geometry, the hydrogen atoms in the molecule are more electronegative than the fluorine resulting in the molecule being polar. C. Even though CH3F has a tetrahedral geometry, the carbon atom in the molecule, being the central atom, is more electronegative than the hydrogen and fluorine atoms in the molecule resulting in the molecule being polar. D. Even though CH3F has a tetrahedral geometry, the fluorine atom in the molecule, being the central atom, is more electronegative than the hydrogen and carbon atoms in the molecule resulting in the molecule being polar. E. Even though CH3F has a tetrahedral geometry, the molecule is not symmetric due to the presence of the fluorine atom in the structure resulting in the…

Which model best describes why bonds form between some atoms, but not others? A. Valence bond diagram  b. Molecular orbital diagram  c. Potential energy diagram

9 A molecule (or ion) has _______ electrons. It is composed of a central atom surrounded by identical atoms. Draw a generic Lewis structure using A for the central atom and X for the outer atoms. Identify at least one molecule and one ion that have the above electron configuration. The electron geometry is The molecular shape is The bond angles are The hybridization of the central atom is MacBook Pro

Please help me answer this questions

Need help on a-d

Use the following Lewis diagram for 1-propanol to answer the questions: H H H 1 H H 2 H 13 H H Remember that geometry refers to the geometry defined by the atoms, not the electron pairs. The geometry about atom C₁ is The ideal value of the C-C-C angle at atom C₂ is The geometry about atom 03 is degrees.

1 and 2 answer only

23. Which molecules is/are polar? A. H2O B. NH3 C. All are polar D. CH3F

Number of Molecule valence electrons Formal Charge Electron-Group Geometry Molecular Geometry Resonance COSe C: C: Select one ... C: Select one.. Select one .. SH412 S: S: Select one .. S: Select one .. Select one ... SeHĄBr2 Se: Se: Select one... Se: Select one ... Select one ... AtGeN Ge: Ge: Select one ... Ge: Select one ... Select one ... CIGEP Ge: Ge: Select one... Ge: Select one ... Select one ... V 10000

6. Questions pertain to the structure shown below: CH HC H3C. CH H3C H3C 6.1 Which of the following is the strongest bond? A. A carbon to carbon single bond B. A carbon to carbon double bond C. A carbon to carbon triple bond D. None of the above, the all have the same strength 6.2The total number of sp3 hybridized carbon(s) is/are: 6.3 The total number of sp2 hybridized carbon(s) is/are 6.4 The total number of sp hybridized carbon(s) is/are: 6.5 The total number of T bonds are:

10. Shown below are the structures of six molecules. For each molecule: i.) Indicate whether the molecule features delocalized n bonding. ii.) Indicate which atoms in each molecule possessp orbitals that are not hybridized. iii.) If the molecule does feature delocalized n bonding, draw at least one resonance structure that exists for the molecule. F. NH2 D. Е. `NH2