hey so I have these 20 chem questions to do over the night for homework, since we were supposed to read the text book which I did not so I bassicly do not understand any of the homework. So any help on any of the problems would be great. If you cant write them on your computer feel free to do it by hand and then take a picture if thats easy thanks in advance! 1. For each of the following polar molecules, indicate the direction of the resulting dipole: a. H-F b. H-C1 c. H-Br d. H-I 2. a. What is the meaning of the term polar, as applied to chemical bonding? b. Distinguish between polar-covalent and nonpolar-covalent bonds. 3. On the basis of individual bond polarity and orientation, determine whether each of the following molecules would be polar or nonpolar: a. H20 b. I2 c. CF4 d. NH3 e. CO2 4. Draw a Lewis structure for each of the following molecules, and then use the VSERP theory to predict the molecular geometry of each: a. SCI2 b. PI3 c. C120 d. NH2C1 e. SiC13Br f. ONC1 5. Arrange the following pairs from strongest to weakest attraction: a. polar molecule and polar molecule b. nonpolar molecule and nonpolar molecule c. polar molecule and ion d. ion and ion 6. A. What are intermolecular forces? B. In general, how do these forces compare in strength with those in ionic and metallic bonding? C. Where are the strongest intermolecular forces found? 7. Explain the role of molecular geometry in determining molecular polarity. 8. Determine the electro negativity difference, the probable bond type, and the more electronegative atom with respect to bonds formed between the following pairs of atoms. a. H and I b. S and O C. K and Br D. S and C1 E. H and F F. Se and S G. C and H 9. What happens to the energy level and stability of two bonded atoms when they are separated and become individual atoms? 10. Determine the electro negativity difference, the probable bonding type, and the more electronegative atom for each of the following pairs of atoms: a. Zn and O b. Br and I c. S and Cl 11. What determines bond length? B) In general, how are bond energies and bond lengths related? 12. Describe the octet rule in terms of noble-gas configurations and potential energy. 13. Use electron-dot notations to illustrate the number of valence electrons present in one atom of each of the following elements. a. Li e. C b. Ca f. P c. Cl g. Al d. O h. S 14. Draw Lewis structures for each of the following molecules. a. contains one C and four F atoms b. Contains two H and on Se atom c. Contains one N and three I atoms d. Contains one Si and four Br atoms e. contains one C on Cl, and three H atoms. 15. How do ionic and covalent bonding differ? How does an ionic compound differ from a molecular compound? How does an ionic compound differ from a metal? 16. Write the electron-dot notations for each of the following elements. a. He d. P b. Cl e. B c. O 17. Draw the Lewis structure for BeCl2 (Hint: Beryllium atoms do not follow the octet rules) 18. In general, how do ionic and molecular compounds compare in terms of melting points, boiling points, and ease of vaporization? What accounts for the observed differences in the properties of ionic and molecular compounds? Cite three physical properties of ionic compounds. 19. Expalin metallic bonding in terms of the sparsely populated outermost orbitals of metal atoms. 20. According to the VSEPR theory, what molecular geometries are associated with the following types of molecules? a. AB2 d.AB5 b. AB3 e. AB6 c. AB4
5. d. ion and ion c. polar molecule and ion a. polar molecule and polar molecule b. nonpolar and nonpolar I know its only one question, but last time I took a chem class was two years ago. yay for physics!
I suggest reading your textbook. Honestly, these questions aren't hard and even a bit of light skimming should help you answer most of these questions.
2. a. What is the meaning of the term polar, as applied to chemical bonding? Sharing electrons unequally due to different electronegativities b. Distinguish between polar-covalent and nonpolar-covalent bonds. Nonpolar covalent is when electrons are shared equally between atoms, whereas polar covalent is when electrons are shared unequally. For instance, H2O is polar covalent because electrons spend more time orbitting around the oxygen atom