1. Which best describes the energy change during the reaction? 5. Base your answer to the following question on the table below.

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1 1. Which best describes the energy change during the reaction? 5. Base your answer to the following question on the table below. H2(g) + Cl2(g) 2 HCl(g) A) Breaking the H H bond releases energy B) Breaking the Cl Cl bond releases energy C) Forming the H Cl bond absorbs energy D) Forming the H Cl bond releases energy Breaking the H CL bond releases energy 2. The attractive force between the protons of one molecule and the electrons of another molecule are strongest A) in the solid phase B) in the liquid phase C) in the gaseous phase D) during sublimation during fusion 3. Covalent bonds are the result of the A) attraction of electrons to each other B) attraction of an electron pair by two nuclei C) elevation of electrons to higher energy levels D) transfer of electrons from one atom to another the attraction of two nuclei to eachother 4. All chemical bonds result from A) overlapping of unoccupied orbitals of two or more atoms. B) loss of one or more electrons by atoms which are gained by other atoms. C) simultaneous attraction of one electron by two nuclei. D) overlapping of two electron filled orbitals with different energy levels. the attraction of two ions. Which bond has the shortest average bond length? A) O H B) C C C) C=O D) H Cl It cannot be determined from the information given. 6. Atom M whose electronegativity is 1.0 combines with atom N whose electronegativity is 3.5. Which diagram best represents the combination? A) M N + B) M + N C) M N D) M:N M N 7. Elements listed in order of increasing electronegativity are A) lithium, potassium, sodium B) lithium, sodium, potassium C) sodium, potassium, lithium D) potassium, sodium, lithium potassium, lithium, sodium 8. The term electronegativity is used because A) some elements conduct electricity and others do not. B) an electric current is a stream of negative particles. C) it requires energy to remove electrons from neutral atoms. D) the nucleus is negatively charged. the attraction for electrons in a bond formed between two different atoms can be uneven.

2 9. The bond between which elements exhibits the greatest ionic character? A) chlorine and fluorine B) lithium and fluorine C) potassium and fluorine D) sodium and fluorine carbon and oxygen 10. Base your answer to the following question on the table below. Consider the shell electron configuration of five elements. 14. Ionic bonds result from the A) sharing of electrons by atoms B) union of atoms with equal ionization energies C) transfer of one or more electrons from one atom to another D) reaction of alkali metals with alkaline earths the attraction of two positively charged nuclei 15. The molecular shape resulting from an sp 3 combination of bonding orbitals in which all four orbitals form chemical bonds is A) bent B) pyramidal C) tetrahedral D) planar triangular linear 16. Which pairs of the elements represented in the diagram would most likely form ionic bonds when reacting together? The most electronegative element is A) I B) II C) III D) IV V 11. Which compound has the greatest ionic character in its bonds? A) KCl B) CaCl2 C) GaCl3 D) AsCl3 O2 12. Which of the following bonds is the longest? A) N N B) Br Br C) O=O D) C=C C C 13. Which substance is an ionic solid? A) I B) II C) III D) IV None of the above A) I and II only B) I and V only C) II and V only D) III and IV only IV and V only 17. The highest ionic character will occur between atoms with the electron configurations A) ls 2 2s 2 2p 1 and ls 2 2s 2 2p 5 B) ls 2 2s 2 2p 1 and ls 2 2s 2 2p 6 3s 2 C) ls 2 2s 2 2p 5 and ls 2 2s 2 2p 6 3s 1 D) ls 2 2s 2 2p 1 and ls 2 2s 2 2p 6 3s 1 ls 2 2s 2 2p 1 and ls 2 2s 2 2p 6 3s Which will conduct an electric current in the molten state, but not in the solid state? A) HCl B) CH4 C) SiO2 D) N2 KBr

3 19. Which Lewis electron dot diagram correctly represents the ionic compound MgCl2? 20. Which compound contains both ionic and covalent bonds? A) HCl(g) B) NaCl(s) C) NH4Cl(s) D) CCl4(l) CH3Cl 21. Which element exists as diatomic molecules at STP? A) copper B) helium C) hydrogen D) silicon chromium 22. The bond in an N2 molecule is A) an ionic bond B) a polar covalent bond C) a double covalent bond D) a triple covalent bond a metallic bond 23. A covalent bond is best described as A) the bond between two oppositely charged ions B) the bond between small stable atoms like helium atoms C) the bond formed when an alkali metal reacts with a halogen D) the bond between two nuclei in a sea of electrons a pair of electrons shared between atoms 24. Nonpolar compounds A) conduct an electric current B) have high melting points C) have low solubility in water D) dissolve in water to form ions are composed of metallic atoms 25. Which type of bond is present in CS2? A) network B) electrovalent C) polar covalent D) metallic nonpolar covalent 26. Which compound exhibits the most covalent character? A) NO B) CsF C) MgO D) Rb2S NaCl 27. In a nonpolar covalent bond, electrons are A) attracted to electrons from the other atom B) shared unequally by two atoms C) transferred from one atom to another D) located in a mobile "sea" shared by many atoms shared equally by two atoms 28. Which is a polar molecule? A) PCl3 B) PCl5 C) CO2 D) SF6 BF3 29. The bond in HCl is polar covalent because the A) shared electrons are closer to the chlorine atom. B) chlorine has a higher atomic number than hydrogen. C) hydrogen chloride molecules are weakly held together. D) chemical bonds consist of electrical forces between atoms. shared electrons are closer to the hydrogen atom. 30. How many fluorine atoms will bond with boron? A) 1 B) 2 C) 3 D) A coordinate covalent bond is one in which A) two atoms are bonded by one electron B) one atom shares two of its electrons with another atom C) two atoms each contribute one electron to a common bond D) two atoms each contribute two electrons to a common bond two atoms with opposing charges attract each other

4 32. In the diagram of an ammonium ion to the right, why is bond A considered to be a coordinate covalent bond? A) Hydrogen provides a pair of electrons to be shared with nitrogen. B) Nitrogen provides a pair of electrons to be shared with hydrogen. C) Hydrogen transfers a pair of electrons to the nitrogen. D) Nitrogen transfers a pair of electrons to hydrogen. Hydrogen and nitrogen each provide an electron. 33. A factor distinguishing a metallic bond from either an ionic or a covalent bond is the mobility of A) nuclei B) protons C) electrons D) kernel ions neutrons 34. Metals are generally better conductors of both heat and electricity than nonmetals because A) atoms of metals contain more electrons. B) metals usually have higher melting points. C) valence electrons in metals are more mobile than in nonmetals. D) ionization energies of metals are greater than those of nonmetals. metals are both ductile and malleable. 35. A substance that consists of positive ions bonded together by electrons which move freely from ion to ion is A) Au B) Kr C) NaCl D) P4 C 36. Which of the following is a polar compound A) CCl4 B) CO2 C) H2S D) O2 none of the above 37. Which of the following molecules is nonpolar? A) H2O B) NH3 C) CO2 D) CHCl3 CO 38. The water molecule is A) ionic. B) a dipole. C) electrovalent. D) a macromolecule. linear. 39. In which pair are both compounds polar molecules? A) CH3Cl, CH4 B) NH3, CCl4 C) NH3, H2S D) H2O, BF3 CO2, CO 40. The main attractive force between polar molecules is A) ionic bonding B) dipole attraction C) hydrogen bonding D) van der Waals attractions molecule ion forces 41. The heat of vaporization of water is almost five times greater than that of oxygen, demonstrating that water A) evaporates more readily than oxygen. B) molecules have more mass than oxygen molecules. C) has forces between molecules that are greater than those between oxygen molecules. D) has forces within molecules that are smaller than those within oxygen molecules. is more likely to be found in the gaseous form than oxygen. 42. In ice, the molecules of H2O(s) are held together by A) covalent bonds. B) hydrogen bonds. C) ionic bonds. D) oxygen bonds. Van der Waals forces.

5 43. Which statement best accounts for the boiling point of H2O being considerably higher than that of H2S? A) The molecular mass of H2O is lower. B) Van der Waals forces are greater in H2O. C) London dispersion forces are greater in H2O. D) H2O molecules have more unshared pairs of valence electrons. Hydrogen bonding is more pronounced in H2O. 44. Which kinds of bonds are found in a sample of liquid H2O? A) covalent bonds, only B) hydrogen bonds, only C) ionic bonds, only D) both covalent and hydrogen bonds both ionic and hydrogen bonds 45. The bonds between molecules in solid nitrogen are A) Van der Waals forces B) covalent bonds C) hydrogen bonds D) ionic bonds network bonds 46. The forces which hold together the atoms in liquid helium are A) ionic bonds B) covalent bonds C) Van der Waals bonds D) hydrogen bonds network bonds 47. Van der Waals forces are greatest between the molecules of A) iodine B) bromine C) chlorine D) fluorine hydrogen 48. What is the weakest type of attractive force between particles? A) Covalent bond B) Hydrogen bond C) Permanent dipoles D) molecule ion forces van der Waals forces 49. Van der Waals forces will increase when there is an increase in the A) number of neutrons B) number of electrons C) number of molecules D) distance between molecules electronegativity 50. In which chemical system is molecule to ion attractions present? A) KNO3(s) B) KNO3(l) C) KNO3(aq) D) KNO3(g) None of the above 51. Which diagram shows the orientation of the water molecules and the calcium ions when calcium chloride is dissolved in water? 52. The Lewis electron dot representation of element 16 is 53. The Lewis electron dot diagram for CO2 is

6 54. Which is the correct Lewis electron dot diagram for NH3? 55. Consider the electron dot structure shown below. Which diatomic molecules could X' represent? A) oxygen B) chlorine C) nitrogen D) hydrogen helium 56. Which Lewis electron dot diagram shows an electron in a hybridized state? 57. All of the following are resonance structures for NO3 except 58. The bonding orbitals on the central atom in a CF4 molecule are A) s orbitals B) p orbitals C) sp orbitals D) sp 2 orbitals sp 3 orbitals 59. In which compound is sp 2 hybridization present in the bonding? A) BH3 B) C2H2 C) CH4 D) H2O CO 60. Which Lewis electron dot diagram shows an atom in the hybridized state? 61. Carbon dioxide is A) linear and polar B) linear and nonpolar C) bent and polar D) bent and nonpolar trigonal planar and polar 62. The shape of the ammonia (NH3) molecule is A) linear B) tetrahedral C) trigonal planar D) trigonal pyramidal square planar 63. The shape of methane molecules, CH4, is A) bent B) triangular C) tetrahedral D) octahedral planar 64. What is the structural shape of the SF6 molecule? A) linear B) octahedral C) tetrahedral D) square planar hexahedral 65. The bonding orbitals on the boron atom in BF3 molecule are A) s orbitals B) sp orbitals C) sp 2 orbitals D) sp 3 orbitals p orbitals 66. A transparent crystalline substance is soft and to has a low melting point. The crystal is a(n) A) ionic solid B) network solid C) metallic solid D) molecular solid metalloid 67. Which will not conduct an electric current in either the molten or solid state? A) Ca B) SiF4 C) KBr D) NaCl CaCO3

7 68. Which could represent the empirical and the molecular formula of a given compound? A) CH4 and C3H8 B) CH2 and C5H10 C) CHO and C6H12O6 D) CH2O and C2H6O2 CH2 and C5H What is the molecular formula of the compound whose empirical formula is P2O5? A) PO B) PO2 C) PO2.5 D) PO3 P4O The oxidation number of boron in the compound B2 H6 is A) 1 B) 2 C) 3 D) The total number of atoms represented in the formula NH4C2H3O2 is A) 5 B) 8 C) 11 D) Two molecules of carbon dioxide are best represented by A) 2CO2 B) C2O4 C) 2C2O D) C4O2 2(C2O) 73. Which compound has the empirical formula CH2? A) CH4 B) C2H4 C) C3H8 D) C6H6 C2H 74. The name of a chemical compound ends in ide ; the compound is A) acidic B) basic C) binary D) an oxide tertiary 75. The name corresponding to the formula Na2SO3 is A) sodium sulfide B) sodium sulfite C) sodium sulfate D) sodium sulfur trioxide bisodium sulfide 76. A compound with the chemical formula SnCl4 is named A) tin chloride. B) tin (IV) chloride. C) stannous (II) chloride. D) stannous (IV) chloride. tin tetrachloride. 77. The name of the compound represented by the formula PCl5 is phosphorus A) dichloride B) tetrachloride C) pentachloride D) heptachloride chloride 78. Which acid has a name starting with hydro and ending with ic? A) H2O B) HBr C) HNO3 D) HClO4 H2S 79. The name of the acid, H2SO3, is A) sulfuric B) sulfurous C) persulfuric D) hydrosulfuric sulfuridic 80. Which substance has a chemical name ending in ide? A) TiCl4 B) ZnSO4 C) H2SO3 D) HClO Zn(BrO2)2 81. Which compound is correctly named? A) PbCO3 lead (IV) carbonate B) Cu2SO4 copper (I) bisulfate C) Fe(ClO2)3 iron (III) chlorite D) Mn2S4 manganese (II) sulfide Zn(OH)2 zinc (II) hydride 82. The name of the compound KMnO4 is potassium A) manganate B) permanganate C) hypomanganate D) manganese oxide maganite

8 83. The name of the compound Na2O2 is A) disodium oxide B) sodium dioxide C) sodium (II) oxide D) disodium dioxide sodium peroxide 84. NH4ClO3 is called A) ammonium chlorate B) ammonium chlorite C) ammonium trichlorate D) ammonium perchlorate ammonium chloride 85. The name of Ca(NO2)2 is A) calcium nitrate B) calcium nitrite C) calcium nitride D) calcium nitrous calcium dinitrite 86. Which compound is correctly named? A) Fe2O3, iron (II) oxide B) Ba(OH)2, barium dihydride C) AgNO3, silver nitride D) MgSO3, magnesium sulfate H2SO4, sulfuric acid 87. If the name of an acidic substance has the ending ic acid, then the formula for the per ic acid of the same family is obtained by A) adding one oxygen atom. B) adding two oxygen atoms. C) subtracting one oxygen atom. D) subtracting two oxygen atoms. subtracting all the oxygen atoms. 88. In which pair of anions do both names end in -ate? A) NO2, PO4 3 B) SO3 2, HCO3 C) S 2, CrO4 2 D) ClO3, SO4 2 SO3 2, PO Which is the correct name for VO? A) vanadium (I) oxide B) vanadium (II) oxide C) vanadium (III) oxide D) vanadium (IV) oxide vanadium (V) oxide 90. Which is the correct name for CO2? A) oxalate ion B) carbonate ion C) carbon (II) oxide D) carbon (IV) oxide carbon oxide 91. Which is the correct name for HgO? A) mercury (I) oxide B) mercury (I) oxate C) mercury (II) oxide D) mercury (II) oxate mercury (II) oxylate 92. What is the name of the compound whose formula is N2O5? A) nitrogen (X) oxide B) nitrogen (II) oxide C) nitrogen (III) oxide D) nitrogen (IV) oxide nitrogen (V) oxide 93. An oxy acid is a compound which A) is a binary compound. B) is usually a basic compound. C) turns litmus from red to blue. D) contains at least three elements. contains more than one oxygen atom. 94. The correct formulas for potassium bromide, aluminum phosphide, and silver sulfide are A) KBr2, AlP, AgS B) K2Br, Al2P3, AgS C) KBr, AlP, Ag2S D) KBr, AlP3, AgS2 KBr, AlP, Ag2SO4 95. An example of a binary compound is A) NaOH B) O2 C) H2S D) Co NO3 96. Which is the correct formula for silver phosphite? A) Ag3PO3 B) Ag3PO4 C) Ag3(PO3)2 D) Ag3(PO4)2 Ag3PO2

9 97. The formula of iron (II) oxide is A) FeO B) FeO2 C) Fe2O D) Fe2O3 Fe(II) O 98. The oxidation number of copper, in most copper compounds, is A) +1 or +2 B) +1 or +3 C) +2 or +3 D) +3 or +5 1 or 2