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Name:___________________________________ Date:___________ Period:____ Review Chemistry I Unit 6: Covalent Bonding and Nomenclature 1. Why do atoms share electrons in covalent bonds with other atoms rather than remaining as single atoms? To acquire a more stable electron configuration (8 valence electrons) 2. A molecule is a neutral group of atoms held together by ______ . A. B. C. D. ionic bonds unshared electrons partial charges covalent bonds 3. Compounds formed by covalent bonds usually contain _______________. A. B. C. D. halogens and oxygen two or more nonmetals a metal and a nonmetal positive and negative ions 4. Which of the following is a covalent compound? A. B. C. D. Na2O AlCl3 SCl6 CuO 5. How do atoms form covalent double bonds? A. B. C. D. C C One atom loses two electrons to the other atom in the bond. Two atoms share two pairs of electrons. Two atoms share two single electrons. Two atoms share one electron. 6. Which of these elements does NOT exist as a diatomic molecule? A. B. C. D. P Cl O N ? ? 1 7. A bond formed between a carbon atom and hydrogen atom is likely to be ____. A. B. C. D. polar covalent dipolar ionic nonpolar covalent 8. Which of the following bonds is the most polar (i.e. has the greatest difference in electronegativity)? A. B. C. D. C—C H—N O—H H—F 9. Which of the following covalent bonds is the least polar? A. B. C. D. H—Cl H—C Cl—Cl H—N 10. Which is TRUE of a nonpolar covalent bond? A. B. C. D. electrons are shared unequally between atoms a cation is bonded to an anion electrons are transferred between atoms electrons are shared equally between atoms 11. Draw the Lewis dot structure for CO2 : Does CO2 contain polar bonds? ___yes Is CO2 a polar molecule? __no_ If so, how many? __2_ If not, explain why not. __the polar bonds are symmetrically arranged and cancel each other out.__ 12. The following molecules contain polar bonds. Which is the only nonpolar molecule? A. B. C. D. HCl NH3 H2O CBr4 (hint: drawing the Lewis structures can help) 2 water molecule water molecule 13. Water molecules are polar because they have _______polar bonds___________ that are arranged __asymmetrically in a bent shape___________. 14. Describe properties that are common in typical molecular compounds. conductor: good or poor melting point: high or low boiling point: high or low net charge: neutral or charged #15-20 Write the NAME or FORMULA for the following molecular compounds: 15. CS2 ____carbon disulfide________ 16. CCI4 ____carbon tetrachloride______ 17. S2O6 ___disulfur hexoxide______ 18. triboron monoxide __B3O__ 19. tetraphosphorus pentoxide __P4O5__ 20. arsenic trihydride _AsH3__ 21. In drawing a Lewis structure, what is special about hydrogen (H) ? A. B. C. D. It achieves an octet of 8 electrons. It can form up to four bonds with 8 shared electrons. It can only form one double bond. It can only form one single bond with no unshared electrons around it. 3 For #22-27: -Draw the Lewis dot structures for the following compounds. -Identify the shape of the molecule as one of these 5: linear, bent, trigonal planar, trigonal pyramidal, tetrahedral -Identify the molecule as polar or nonpolar by circling the correct label. 22. HBr shape: polar or nonpolar polar or nonpolar polar or nonpolar polar or nonpolar polar or nonpolar polar or nonpolar linear 23. NI3 shape: trigonal pyramidal 24. N2 shape: linear 25. Cl2 shape: linear 26. SO2 shape: bent 27. CH2F2 shape: tetrahedral 4