CJ Bianconi Chem 102 Spring 2015 Mock Half Exam 1. Electronegativity increases as you go __________ and __________ on the Periodic Table. 2. A place where amplitude is 0 is called a __________. 3. A cation has (more/less) electrons than the neutral atom while an anion has (more/less) electrons than the neutral atom. 4. The 4th shell has _____ (#) subshells and _____ (#) orbitals. 5. A 5d subshell can hold _____ (#) electrons. 6. Arsenic (As) has _____ (#) 4s electrons, _____ (#) 4d electrons, and _____ (#) 4p electrons. 7. A central atom with a steric number of 4 will have bond angles of _____°. 8. If a molecule has linear geometry, the central atom will have _____ (#) hybridized subshells that are labeled _____. 9. When two electrons form a bond, the amplitudes of their waves are __________ together by the process called __________ __________. 10. Atoms prefer to have _____ (#) electrons around them according to the __________ __________. True/False 11. ( T / F ) Sigma bonds are only found in single bonds. 12. ( T / F ) Carbon always has sp3 hybrid orbitals used in sigma bonding. 13. ( T / F ) A filled 5d subshell will have 5 electron pairs in it. 14. ( T / F ) A filled p orbital has 1 electron exclusively on the positive amplitude side and 1 electron exclusively on the negative amplitude side. 15. ( T / F ) A compound with 3 atoms always has linear geometry. 16. ( T / F ) Sigma bonds allow free rotation of the participating atoms. 17. ( T / F ) A bromide (Br -) ion has one half-filled orbital. 18. ( T / F ) UV light has lower wavelength than X-rays. 19. ( T / F ) Steric number counts single, double, and triple bonds equally. 20. ( T / F ) The amplitude of a wave determines its energy. 21. Above is the structure for the chemical dopamine. How many pi bonds are in this molecule? How many sigma bonds are there? 22. What is the hybridization for the atoms marked with a 1, 2, and 3? What are the bond angles for the hybridized orbitals? 23. Draw the Lewis Dot Structure for Nitrogen gas (N2). Symbolically represent all bonds in the element by detailing whether they are sigma or pi bonds, and listing the orbitals used in the bonds. 24. Draw the electromagnetic spectrum and label the directions of energy, wavelength, and frequency. 25. Draw the orbital diagram for ground-state oxygen, then draw oxygen’s orbital diagram when it is sp hybridized. 26. According to Valence Bond Theory, bonds are formed by: 27. Draw the Lewis Dot Structure of CH3OH and identify any net dipole on the molecule. What is the predominant IMF expressed by this molecule? 28. Draw the Lewis Dot Structure of CHCl3 and identify any net dipole on the molecule. What is the predominant IMF expressed by this molecule? 29. Draw the Lewis Dot Structure of C6H14 and identify any net dipole on the molecule. What is the predominant IMF expressed by this molecule? 30. Draw a diagram of two molecules that shows a momentary dipole occurring. 31. Draw a diagram of two molecules that shows a dipole-dipole interaction occurring. 32. Complete this chart: # of e- directions in space hybridization # of unhybridized p orbitals electron pair geometry 33. Symbolically represent all of the bonds in C2H3Cl. 34. Symbolically represent all of the bonds in HCN. 35. Symbolically represent all of the bonds in CO2.