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1 Bonding Page 1 Name 2/14 1. Which formula represents an ionic compound? A) NaCl B) N2O C) HCl D) H2O 2. Which type of bond results when one or more valence electrons are transferred from one atom to another? A) a hydrogen bond B) an ionic bond C) a nonpolar covalent bond D) a polar covalent bond 3. Compared to a calcium atom, the calcium ion Ca 2+ has A) more protons B) fewer protons C) more electrons D) fewer electrons 4. Which sample contains particles in a rigid, fixed, geometric pattern? A) CO2(aq) B) HCl(g) C) H2O( ) D) KCl(s) 5. Which particles may be gained, lost, or shared by an atom when it forms a chemical bond? A) protons B) electrons C) neutrons D) nucleons 6. Which quantities must be conserved in all chemical reactions? A) mass, charge, density B) mass, charge, energy C) charge, volume, density D) charge, volume, energy 7. Which symbol represents an atom in the ground state with the most stable valence electron configuration? A) B B) O C) Li D) Ne 8. Which element has the lowest electronegativity value? A) F B) Fr C) Cl D) Cr 9. Which statement correctly describes diamond and graphite, which are different forms of solid carbon? A) They differ in their molecular structure,only. B) They differ in their properties, only. C) They differ in their molecular structure and properties. D) They do not differ in their molecular structure or properties. 10. Which compound contains both ionic and covalent bonds? A) ammonia B) methane C) sodium nitrate D) potassium chloride 11. The bond between which two atoms is most polar? A) Br and Cl B) Br and F C) I and Cl D) I and F 12. What is the name of the polyatomic ion in the compound Na2O2? A) hydroxide B) oxalate C) oxide D) peroxide

2 Bonding Page Given the balanced equation representing a reaction: 16. Given the Lewis electron-dot diagram: H2 + energy H + H What occurs as bonds are broken in one mole of H2 molecules during this reaction? A) Energy is absorbed and one mole of unbonded hydrogen atoms is produced. B) Energy is absorbed and two moles of unbonded hydrogen atoms are produced. C) Energy is released and one mole of unbonded hydrogen atoms is produced. D) Energy is released and two moles of unbonded hydrogen atoms are produced. 14. When lithium reacts with bromine to form the compound LiBr, each lithium atom A) gains one electron and becomes a negatively charged ion B) gains three electrons and becomes a negatively charged ion C) loses one electron and becomes a positively charged ion D) loses three electrons and becomes a positively charged ion 15. In a bond between an atom of carbon and an atom of fluorine, the fluorine atom has a A) weaker attraction for electrons B) stronger attraction for electrons C) smaller number of first-shell electrons D) larger number of first-shell electrons Which electrons are represented by all of the dots? A) the carbon valence electrons, only B) the hydrogen valence electrons, only C) the carbon and hydrogen valence electrons D) all of the carbon and hydrogen electrons 17. Which term indicates how strongly an atom attracts the electrons in a chemical bond? A) alkalinity B) atomic mass C) electronegativity D) activation energy 18. Which element reacts with oxygen to form ionic bonds? A) calcium B) hydrogen C) chlorine D) nitrogen 19. Gold can be flattened into an extremely thin sheet. The malleability of gold is due to the A) radioactive decay mode of the isotope Au-198 B) proton-to-neutron ratio in an atom of gold C) nature of the bonds between gold atoms D) reactivity of gold atom 20. Which Lewis electron-dot diagram correctly represents a hydroxide ion? A) B) C) D)

3 Bonding Page A sample of a substance has these characteristics: melting point of 984 K hard, brittle solid at room temperature poor conductor of heat and electricity as a solid good conductor of electricity as a liquid on in an aqueous solution This sample is classified as A) a metallic element B) a radioactive element C) a molecular compound D) an ionic compound 22. Which type of substance can conduct electricity in the liquid phase but not in the solid phase? A) ionic compound B) molecular compound C) metallic element D) nonmetallic element 23. Based on bond type, which compound has the highest melting point? A) CH3OH B) C6H14 C) CaCl2 D) CCl4 24. The data table below represents the properties determined by the analysis of substances A, B, C, and D. Which substance is an ionic compound? A) A B) B C) C D) D

4 Bonding Page Which pair of atoms has the most polar bond? A) H Br B) H Cl C) I Br D) I Cl 26. The electronegativity difference between the atoms in a molecule of HCl can be used to determine A) the entropy of the atoms B) the atomic number of the atoms C) the first ionization energy of the atoms D) the polarity of the bond between the two atoms 27. Which compound has hydrogen bonding between its molecules? A) CH4 B) CaH2 C) KH D) NH3 28. Which diagram best illustrates the ion-molecule attractions that occur when the ions of NaCl(s) are added to water? A) B) C) D)

5 Bonding Page 5 Base your answers to questions 29 and 30 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. 29. Identify the two types of chemical bonds found in the salt used to produce a deep-red color. 30. Write the formula for the salt used to produce green light in a fireworks display. 31. Base your answer to the following question on the information below. Heat is added to a 200.-gram sample of H2O(s) to melt the sample at 0 C. Then the resulting H2O( ) is heated to a final temperature of 65 C. Compare the amount of heat required to vaporize a 200.-gram sample of H20( ) at its boiling point to the amount of heat required to melt a 200.-gram sample of H2O(s) at its melting point. 32. Base your answer to the following question on the information below and on your knowledge of chemistry. The balanced equation below represents a reaction. Draw a Lewis electron-dot diagram of one oxygen atom.

6 Base your answers to questions 33 and 34 on the information below. In 1864, the Solvay process was developed to make soda ash. One step in the process is represented by the balanced equation below. NaCl + NH3 + CO2 + H2O NaHCO3 + NH4Cl 33. Explain, in terms of electronegativity difference, why the bond between hydrogen and oxygen in a water molecule is more polar than the bond between hydrogen and nitrogen in an ammonia molecule. 34. Write the chemical formula for one compound in the equation that contains both ionic bonds and covalent bonds. 35. Base your answer to the following question on the information below and on your knowledge of chemistry. A sample of seawater is analyzed. The table below gives the concentration of some ions in the sample. Write a chemical formula of one compound formed by the combination of ions with one of these ions as water completely evaporates from the seawater sample. Bonding Page 6

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