CHEM133 Week 11 Lesson 5 Quiz

1. Question: When comparing Be2 and H2: 2. Question: Atoms that are sp2 hybridized form ____ pi bond(s). 3. Question: The hybridization of the nitrogen atom in the cation NH2+ is: 4. Question: Which one of the following molecules has an atom with an incomplete octet? 5. Question: Nitrous oxide (N2O) is sometimes called "laughing gas". What is the formal charge on the central nitrogen atom in the most favorable Lewis structure for nitrous oxide based on minimizing formal charge overall? 6. Question: How many lone electron pairs are in the NH4+ ion? 7. Question: Based on formal charge considerations, the electron-dot structure of CO32– ion has 8. Question: Each of the three resonance structures of NO3– has how many lone pairs of electrons? 9. Question: How many double and single bonds are in the resonance form for SO2 in which the formal charges on each atom are zero? 10. Question: The total number of bonding electrons in a molecule of formaldehyde (H2CO) is 11. Question: BeF42– is called the fluoberyllate ion. The formal charge on the beryllium atom in this ion is 12. Question: The electron configuration of a particular diatomic species is 13. Question: If a non metal on the periodic table bonds with another nonmetal, what happens? 14. Question: If the central atom has four groups of electrons around it, what type of electronic geometry is present? 15. Question: Draw the structure of ozone according to VSEPR theory. What would be its associated molecular geometry? 16. Question: Some atoms are better at attracting electrons compared to others. Which term below best describes that? 17. Question: According to the electronegativity table, the value for carbon and nitrogen is 2.5 and 3.0, respectively. What type of bond would you expect to form between these two elements? 18. Question: If the center atom has four single bonds around it, what type of molecular geometry is present? 19. Question: If the center atom has a double bond, a single bond, and 1 lone pair around it, what type of molecular geometry is present? 20. Question: Draw the Lewis structure for the carbonate polyatomic ion. How many valence electrons does it have? 21. Question: If you were to use Lewis theory to predict the formula for the compound between selenium and oxygen, it would most likely be 22. Question: According to Lewis dot theory, what types of electron pairs would you find surrounding the central atom of the sulfate ion? 23. Question: What is the electronic geometry around the central atom of the ammonium ion according to VSEPR theory? 24. Question: Draw the structure of sulfur dioxide according to VSEPR theory. What would be its associated molecular geometry? 25. Question: When counting the total number of valence electrons to be used for the Lewis structure, what is the total for the hypochlorite ion?