Chemistry, Bonding Practice Set 1 Spring, Regents Prep

Transcription

1 Name: Date: Pd: Chemistry, Bonding Practice Set 1 Spring, Regents Prep 1. Compared to a calcium atom, the calcium ion Ca 2+ has (1) fewer electrons (2) more protons (3) fewer protons (4) more electrons 2. Given the Lewis electron-dot diagram: Which electrons are represented by all of the dots? (1) the carbon and hydrogen valence electrons (2) the carbon valence electrons, only (3) all of the carbon and hydrogen electrons (4) the hydrogen valence electrons, only 3. Metallic bonding occurs between atoms of (1) copper (2) neon (3) sulfur (4) fluorine 4. Which type of bond is present in a water molecule? (1) polar covalent (2) ionic (3) nonpolar covalent (4) electrovalent 5. Which compound contains only covalent bonds? (1) CH3OH (2) Ba(OH)2 (3) NaOH (4) Ca(OH)2 6. Which quantities must be conserved in all chemical reactions? (1) charge, volume, density (2) charge, volume, energy (3) mass, charge, density (4) mass, charge, energy 7. A substance that has a melting point of 1074 K conducts electricity when dissolved in water, but does not conduct electricity in the solid phase. The substance is most likely (1) an ionic solid (2) a molecular solid (3) a metallic solid (4) a network solid 8. An oxygen molecule contains a double bond because the two atoms of oxygen share a total of (1) 1 electron (2) 2 electrons (3) 3 electrons (4) 4 electrons 9. When a sodium atom reacts with a chlorine atom to form a compound, the electron configurations of the ions forming the compound are the same as those in which noble gas atoms? (1) neon and helium (2) krypton and neon (3) krypton and argon (4) neon and argon 10. Which type of bonding is usually exhibited when the electronegativity difference between two atoms is 1.1? (1) covalent (2) metallic (3) ionic (4) network 11. Which type of bond is found in sodium bromide? (1) hydrogen (2) ionic (3) metallic (4) covalent 12. Which properties are characteristic of the Group 1 metals? (1) low reactivity and the formation of stable compounds (2) low reactivity and the formation of unstable compounds (3) high reactivity and the formation of unstable compounds (4) high reactivity and the formation of stable compounds 13. Which type of bonding involves positive ions immersed in a sea of mobile electrons? (1) ionic (2) metallic (3) nonpolar covalent (4) polar covalent 14. Why is a molecule of CO2 nonpolar even though the bonds between the carbon atom and the oxygen atoms are polar? (1) The CO2 molecule has an excess of electrons. (2) The shape of the CO2 molecule is asymmetrical. (3) The shape of the CO2 molecule is symmetrical. (4) The CO2 molecule has a deficiency of electrons. 15. Which sample contains particles in a rigid, fixed, geometric pattern? (1) KCl(s) (2) CO2(aq) (3) H2O( ) (4) HCl(g) 16. The elements Li and F combine to form an ionic compound. The electron configurations in this compound are the same as the electron configurations of atoms in Group (1) 1 (2) 14 (3) 17 (4) What is the total number of pairs of electrons shared in a molecule of N2? (1) two pairs (2) one pair (3) four pairs (4) three pairs 18. A characteristic of ionic solids is that they (1) conduct electricity (2) have high melting points (3) are non-crystalline (4) have low boiling points 19. An element with an electronegativity of 0.9 bonds with an element with an electronegativity of 3.1. Which phrase best describes the bond between these elements? (1) mostly ionic in character and formed between two nonmetals (2) mostly covalent in character and formed between two nonmetal (3) mostly covalent in character and formed between a metal and a nonmetal (4) mostly ionic in character and formed between a metal and a nonmetal 20. Which terms describe a substance that has a low melting point and poor electrical conductivity? (1) ionic and metallic (2) covalent and metallic (3) ionic and molecular (4) covalent and molecular HSVD Ms. Chang Page 1

2 21. Which substance contains particles held together by metallic bonds? (1) Ni(s) (2) N2(s) (3) I2(s) (4) Ne(s) 22. As a bond between a hydrogen atom and a sulfur atom is formed, electrons are (1) shared to form an ionic bond (2) shared to form a covalent bond (3) transferred to form an ionic bond (4) transferred to form a covalent bond 23. Which formula represents a nonpolar molecule? (1) H2O (2) CH4 (3) HCl (4) NH3 24. Which molecule contains a nonpolar covalent bond? (1) (2) (3) (4) 25. Which molecule is nonpolar and contains a nonpolar covalent bond? (1) HF (2) HCl (3) F2 (4) CCl4 26. At STP, fluorine is a gas and bromine is a liquid because, compared to fluorine, bromine has (1) weaker intermolecular forces (2) stronger intermolecular forces (3) stronger covalent bonds (4) weaker covalent bonds 27. Which type of bonding is characteristic of a substance that has a high melting point and electrical conductivity only in the liquid phase? (1) ionic (2) nonpolar covalent (3) metallic (4) coordinate covalent 28. As a chlorine atom becomes a negative ion, the atom (1) loses an electron and its radius increases (2) gains an electron and its radius increases (3) gains an electron and its radius decreases (4) loses an electron and its radius decreases 29. Which statement explains why low temperature and high pressure are required to liquefy chlorine gas? (1) Chlorine molecules have weak intermolecular forces of attraction. (2) Chlorine molecules have weak covalent bonds. (3) Chlorine molecules have strong intermolecular forces of attraction. (4) Chlorine molecules have strong covalent bonds. 30. Given the formula of a substance: What is the total number of shared electrons in a molecule of this substance? (1) 9 (2) 11 (3) 6 (4) Which formula represents an ionic compound? (1) N2O (2) HCl (3) NaCl (4) H2O 32. Which type of bonding is found in all molecular substances? (1) hydrogen bonding (2) metallic bonding (3) covalent bonding (4) ionic bonding 33. Which of these elements has an atom with the most stable outer electron configuration? (1) Na (2) Ne (3) Ca (4) Cl 34. Which compound contains ionic bonds? (1) CO2 (2) CaO (3) NO2 (4) NO 35. A chemist performs the same tests on two homogeneous white crystalline solids, A and B. The results are shown in the table below. The results of these tests suggest that (1) solid A contains only ionic bonds and solid B contains only covalent bonds (2) both solids contain only ionic bonds (3) solid A contains only covalent bonds and solid B contains only ionic bonds (4) both solids contain only covalent bonds 36. Which type of bond results when one or more valence electrons are transferred from one atom to another? (1) a nonpolar covalent bond (2) an ionic bond (3) a hydrogen bond (4) a polar covalent bond HSVD Ms. Chang Page 2

3 37. Given the balanced equation representing a reaction: H2(g) + Cl2(g) 2HCl(g) + energy Which statement describes the energy changes in this reaction? (1) Energy is absorbed as bonds are broken, and energy is released as bonds are formed. (2) Energy is released as bonds are broken, only. (3) Energy is absorbed as bonds are formed, only. (4) Energy is absorbed as bonds are formed, and energy is released as bonds are broken. 38. Given the balanced equation representing a reaction: Cl2 Cl + Cl What occurs during this reaction? (1) A bond is formed as energy is absorbed. (2) A bond is broken as energy is absorbed. (3) A bond is broken as energy is released. (4) A bond is formed as energy is released. 39. Which molecule contains a nonpolar covalent bond? (1) I2 (2) H2O (3) NH3 (4) CO 40. What type of bond exists in a molecule of iodine? (1) polar covalent (2) nonpolar covalent (3) ionic (4) metallic HSVD Ms. Chang Page 3

4 41. Base your answer to the following question on the information below and on your knowledge of chemistry. The formulas and the boiling points at standard pressure for ethane, methane, methanol, and water are shown in the table below. Explain, in terms of molecular polarity, why the solubility of methanol in water is greater than the solubility of methane in water. Base your answers to questions 42 and 43 on the information below. During a fireworks display, salts are heated to very high temperatures. Ions in the salts absorb energy and become excited. Spectacular colors are produced as energy is emitted from the ions in the form of light. The color of the emitted light is characteristic of the metal ion in each salt. For example, the lithium ion in lithium carbonate, Li2CO3, produces a deep-red color. The strontium ion in strontium carbonate, SrCO3, produces a bright-red color. Similarly, calcium chloride is used for orange light, sodium chloride for yellow light, and barium chloride for green light. 42. Write the formula for the salt used to produce green light in a fireworks display. 43. Identify the two types of chemical bonds found in the salt used to produce a deep-red color. HSVD Ms. Chang Page 4

5 44. Base your answer to the following question on the information below. In the space in your answer booklet, draw a Lewis electron-dot diagram for CF4. Base your answers to questions 45 through 47 on the information below and on your knowledge of chemistry. Rubbing alcohol is a product available at most pharmacies and supermarkets. One rubbing alcohol solution contains 2-propanol and water. The boiling point of 2-propanol is 82.3 C at standard pressure. 45. Explain in terms of electronegativity differences, why a C O bond is more polar than a C H bond. 46. Explain, in term of charge distribution, why a molecule of the 2-propanol is a polar molecule. 47. Draw a structural formula formula for the 2-propanol. 48. Base your answer to the following question on the information below. Ammonium chloride is dissolved in water to form a 0.10 M NH4Cl(aq) solution. This dissolving process is represented by the equation below. Explain, in terms of ions, why a 10.0-milliliter sample of 0.30 M NH4Cl(aq) is a better conductor of electricity than a 10.0-milliliter sample of the 0.10 M NH4Cl(aq). 49. Base your answer to the following question on the information below and on your knowledge of chemistry. The balanced equation below represents a reaction. O2(g) + energy O(g) + O(g) Explain, in terms of bonds, why energy is absorbed during this reaction. 50. Identify the type of bonding in solid potassium. HSVD Ms. Chang Page 5

6 Chemistry Name Class Date HSVD Ms. Chang Page 6