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Download Chemistry 1 CP Concept 6 Part 1 Study Guide
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Chemistry 1 CP Concept 6 Part 1 Study Guide Name: ___________________________ Block: _________ 1. In the NaCl crystal, each Na+ and Cl- ion has how many oppositely charged ions clustered around it? ___________ 2. What is a chemical bond? _______________________________________________ _______________________________________________________________________ 3. What are the characteristics of substances with metallic bonds and why do they have these characteristics? ______________________________________________________ ________________________________________________________________________ 4. List the pair of elements that form bonds from covalent to ionic by electronegativity strength, show work: NaCl, KCl, OCl, MgCl ___________________________________ ________________________________________________________________________ ________________________________________________________________________ 5. Why are ionic compounds brittle? Strong attractive forces ______________________ 6. Nonpolar covalent bonds are not common because ____________________________ 7. How many e- must be shown in the Lewis structure of the following: show your work OH- _________________________________, H2O _____________________________ 8. Compare the melting/boiling points of ionic and covalent compounds _____________ ________________________________________________________________________ 9. What is electronegativity? ________________________________________________ 10. Formula that shows only the types and numbers of atoms combined in a single molecule is ________________________ 11. Which electrons are involved in the formation of a chemical bond? ______________ 12. Two identical atoms bond together with what bond type? What is the percentage of ionic character? ____________________________ ______________________________ 13. The strong forces of attraction between the positive and negative regions of molecules are called _______________________________________________________ 14. Explain what happens to potential energy and stability when atoms bond. _________ ________________________________________________________________________ 15. What is lattice energy a measure of? ______________________________________ 16. The reason the boiling point of water (H2O) is higher than the boiling point of (H2S) is partially explained by __________________ bonding. 17. If the atoms that share electrons have an unequal attraction for the electrons, the bond is called ________________________ 18. What kind of bond is present in the following: NH4,__________________________ BF3,________________________________ NaCl ______________________________ 19. What is the next step after drawing a Lewis structure? ________________________ _______________________________________________________________________ 20. In a molecule of chlorine, the two shared e- give each chlorine _________ valence e21. The equal but opposite charges present in the two regions of a polar molecule create ______________________________________________________________________ 22. The greater the electronegativity difference between two bonded atoms, the greater the percentage of _________________________________ in the bond. 23. The ions in most ______________________ compounds are organized into crystals. 24. As light strikes the surface of a metal, the electrons ___________________________ ________________________________________________________________________ 25. Dipole-dipole forces are considered the most important forces in polar substances because the London dispersion forces present in polar substances are ________________ ________________________________________________________________________ 26. A polar molecule contains a region of _____________ and a region of ___________ 27. In drawing a Lewis structure, the central atom is generally the atom with the least _____________________________ 28. Most chemical bonds are partly _____________ and partly ____________________ 29. What is a molecule (type of bond) ________________________________________ _______________________________________________________________________ 30. What is lattice energy? _________________________________________________ ________________________________________________________________________ 31. What is a molecular formula, give an example? ______________________________ ________________________________________________________________________ 32. What is between a molecule’s resonance structures to indicate resonance? ________, What is resonance? _______________________________________________________ 33. When a polar molecule attracts the electron in a nonpolar molecule a ____________ is induced. 34. What is an electron sea? _________________________________________________ 35. Multiple covalent bonds may occur in atoms that contain carbon, ________, _______ 36. Draw the Lewis structure for HCl, H2O, NH3, O2 show all work!
