1. What is a chemical bond? 2. What is the octet rule? Why do atoms in bonding follow it?
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1 Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations 1. What is a chemical bond? 2. What is the octet rule? Why do atoms in bonding follow it? 3. What are oxidation numbers? How do we find them? 4. What are polyatomic ions? How do we find them? Name 3 examples. 5. How do we name ionic compounds? (Basic rules). 6. What does the Roman numeral represent? Do we use Roman numerals in covalent compounds? 7. How do we name covalent compounds? (Basic rules). 8. What are ionic bonds? Describe essential characteristics.
2 9. What are polar covalent bonds? Describe essential characteristics. 10. What are non-polar covalent bonds? Describe essential characteristics. 11. What does the term polar mean? 12. What does the term dipole mean? 13. How do we know if a bond is polar? 14. How do we know if a molecule has a dipole? (If the molecule is polar) 15. What are metallic bonds? Describe essential characteristics. 16. What are intermolecular forces? Why are they important? 17. What are hydrogen bonds? What 3 common atoms do they occur in? 18. What are dipole dipole forces? How are they different from hydrogen bonds?
3 19. What are London dispersion forces? (Van der waals forces). What molecules/atoms do they occur in? 20. Rank the 3 intermolecular forces from least to greatest. 21. Draw the hydrogen bond water makes with another water molecule. 22. Draw the hydrogen bond NH 3 makes with ammonia. 23. What type of substance conducts electricity in the solid phase, liquid phase, and aqueous? 24. What type of substance does not conduct electricity as a solid, but conducts as a liquid and aqueous? 25. What type of compound does the term molecule describe? 26. What are the 3 different types of molecular shapes? Name and draw an example for each. 27. Draw CBr 4. What is the shape of CBr 4? Are the bonds polar and why? Is the molecule polar and why? 28. Draw NH 3. What is the shape of NH 3? Are the bonds polar and why? Is the molecule polar and why?
4 29. Draw H 2 O. What is the shape of H 2 O? Are the bonds polar and why? Is the molecule polar and why? 30. Name the following compounds: a) Ag 2 SO 4 b) Fe(OH) 2 c) P 4 S Write the formula of: a) Dintriogen Trioxide b) Chromium III Carbonate c) Ammonium nitrate. 32. Draw the structures and determine the shape and polarity of the molecule: a) F 2 b) O 2 c) CH 2 Br 2 d) N Why is CO 2 non-polar even though the bonds are polar? 34. Which compound contains both ionic and covalent bonds? a) CO 2 b) HCl c) NH 4 Br d) CI What type of bond is present in steel? 36. What happens to the energy when a bond is broken? 37. What is an electrolyte?
5 Name: Date: Chemistry ~ Ms. Hart Class: Anions or Cations Unit 5 Key Questions Chemical Bonding Answers! 1. What is a chemical bond? a. Glue that holds atoms together. 2. What is the octet rule? Why do atoms in bonding follow it? a. Atoms need 8 electrons. In bonding, atoms will do whatever possible to fill their valence shell, which needs 8 to be filled. 3. What are oxidation numbers? How do we find them? a. Charge when an atom forms an ion. Upper right corner on the periodic table. 4. What are polyatomic ions? How do we find them? Name 3 examples. a. Polyatomic ions are covalently bonded ions. We find them in Table E on the reference table. CN -, OH -, and SCN - are all examples. 5. How do we name ionic compounds? (Basic rules). a. See HW and notes for complete naming. Essential Rules: i. Use ide at the end. Positive (cation) always written first. ii. Use roman numerals if transition metal is present. iii. Use names of polyatomic ions without adding ide. 6. What does the Roman numeral represent? Do we use Roman numerals in covalent compounds? a. Roman numerals represent the charge on a transition metal in an ionic compound name. We do not use them in covalent compounds. 7. How do we name covalent compounds? (Basic rules). a. See HW for more complete rules. Essential rules: i. Use ide at the end ii. Use mono (sometimes), di, tri, etc. as prefixes. 8. What are ionic bonds? Describe essential characteristics. a. Ionic bonds are where electrons are transferred. Always between a metal and nonmetal. Bonds are formed by electrostatic interactions. High melting points. Do not conduct as solids, but conduct as liquids and aqueous. 9. What are polar covalent bonds? Describe essential characteristics. a. Bonds where electrons are shared unequally. Two nonmetals. More electronegative atom is partially negative (gets more electrons) EN difference. 10. What are non-polar covalent bonds? Describe essential characteristics. a. See Table in Notes. Bond where electrons are shared equally EN difference. 11. What does the term polar mean? a. Unequal distribution of charge. A more electronegative atom will pull more electrons becoming more negative. 12. What does the term dipole mean? a. Same as polar. 13. How do we know if a bond is polar? a. If the EN difference is more than How do we know if a molecule has a dipole? (If the molecule is polar) a. If we can draw a line of symmetry for charge. (one side negative and the other side positive). 15. What are metallic bonds? Describe essential characteristics. a. Bonds between metals via a sea of electrons. The valence shell electrons separate from the atom and the electrons are used by all metals. Metals conduct electricity in the solid, liquid, and aqueous phases. 16. What are intermolecular forces? Why are they important? a. Intermolecular forces are forces between molecules. They are important because they hold molecules together. In water for example, intermolecular forces prevent water from becoming a gas, giving it a high boiling point. 17. What are hydrogen bonds? What 3 common atoms do they occur in?
6 a. Hydrogen bonds are an intermolecular represented by a dashed line between a hydrogen atom and N, O, or F. 18. What are dipole dipole forces? How are they different from hydrogen bonds? a. Dipole dipole forces are where the slightly positive side of a molecule is attracted to the slightly negative side of another. Different because it is the whole molecule interacting, not just 2 atoms. 19. What are London dispersion forces? (Van der waals forces). What molecules/atoms do they occur in? a. Where a dipole forms in a molecule due to electrons moving and creates a positive and negative side. This interacts with the positive/negative side of another molecule. They occur in ALL molecules/atoms, even noble gases and non-polar molecules. 20. Rank the 3 intermolecular forces from least to greatest. a. London dispersion < dipole dipole < Hydrogen Bonds 21. Draw the hydrogen bond water makes with another water molecule. a. See Notes. 22. Draw the hydrogen bond NH 3 makes with ammonia. a. See Notes. 23. What type of substance conducts electricity in the solid phase, liquid phase, and aqueous? a. Metallic 24. What type of substance does not conduct electricity as a solid, but conducts as a liquid and aqueous? a. Ionic, also called a salt. 25. What type of compound does the term molecule describe? a. Covalent. 26. What are the 3 different types of molecular shapes? Name and draw an example for each. a. Linear, tetrahedral, and bent. (CO 2 is linear, CH 4 is tetrahedral, H 2O is bent) 27. Draw CBr 4. What is the shape of CBr 4? Are the bonds polar and why? Is the molecule polar and why? a. Tetrahedral. Bonds are polar b/c of high EN difference. Molecule is non-polar because you cannot draw a line of symmetry for charges. 28. Draw NH 3. What is the shape of NH 3? Are the bonds polar and why? Is the molecule polar and why? a. Trigonal pyramidal (no need to know the term). Polar bonds b/c of high EN difference. Molecule is polar because you can draw a line of symmetry for charge. 29. Draw H 2O. What is the shape of H 2O? Are the bonds polar and why? Is the molecule polar and why? a. Bent. Polar bonds b/c of high EN difference. Molecule is polar because you can draw a line of symmetry for charge. 30. Name the following compounds: a) Ag 2SO 4 b) Fe(OH) 2 c) P 4S 5 a. A) silver sulfate B) Iron (II) hydroxide C) Tetraphosphorus pentasulfide 31. Write the formula of: a) Dintriogen Trioxide b) Chromium III Carbonate c) Ammonium nitrate. a. A) N 2O 3 B) Cr 2(CO 3) 3 C) NH 4NO Draw the structures and determine the shape and polarity of the molecule: a) F 2 b) O 2 c) CH 2Br 2 d) N 2 a. A) Linear, nonpolar B) Linear, nonpolar C) Tetrahedral, polar D) Linear, nonpolar 33. Why is CO 2 non-polar even though the bonds are polar? a. You cannot draw a line of symmetry for charge. 34. Which compound contains both ionic and covalent bonds? a) CO 2 b) HCl c) NH 4Br d) CI 4 a. C 35. What type of bond is present in steel? a. Metallic 36. What happens to energy when a bond is broken? a. Energy is required for a bond to break. Breaking up is hard to do 37. What is an electrolyte? a. An electrolyte is an ionic compound!
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