3 When chemical compounds form, valence electrons are those that may be A lost only. C shared only. B gained only. D lost, gained, or shared.
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1 CLASS SET ID: A Chapter 12 Prep-Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1 A measure of the ability of an atom in a chemical compound to attract electrons is called A electron affinity. C electronegativity. B electron configuration. D ionization potential. 2 The element that has the greatest electronegativity is A oxygen. C chlorine. B sodium. D fluorine. 3 When chemical compounds form, valence electrons are those that may be A lost only. C shared only. B gained only. D lost, gained, or shared. 4 For Groups 13 through 18, the number of valence electrons is equal to the group number A plus 1. C minus the period number. B plus the period number. D minus How many valence electrons are in an atom of phosphorus? A 2 C 4 B 3 D 5 6 How many valence electrons does a helium atom have? A 2 C 4 B 3 D 5 7 What is the charge on the strontium ion? A 2 C 1 B 1 D 2 8 How does oxygen obey the octet rule when reacting to form compounds? A It gains electrons. B It gives up electrons. C It does not change its number of electrons. D Oxygen does not obey the octet rule. 9 Ionic compounds are normally in which physical state at room temperature? A solid C gas B liquid D plasma 1
2 10 Which of the following particles are free to drift in metals? A protons C neutrons B electrons D cations 11 An Ionic bond is a bond between. A a cation and an anion C the ions of two different metals B valence electrons and cations D the ions of two different nonmetals 12 A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n) A dipole. C chemical bond. B Lewis structure. D London force. 13 A chemical bond results from the mutual attraction of the nuclei of atoms and A electrons. C neutrons. B protons. D dipoles. 14 The Na - F bond in NaF (electronegativity for Na is 0.9; electronegativity for F is 4.0) is A polar covalent. C nonpolar covalent. B ionic. D pure covalent. 15 In which of these compounds is the bond between the atoms NOT a nonpolar covalent bond? A Cl 2 C HCl B H 2 D O 2 16 What is the Lewis structure for hydrogen chloride, HCl? A A C C B B D D 17 VSEPR theory is a model for predicting A the strength of metallic bonds. C lattice energy values. B the shape of molecules. D ionization energy. 18 Use VSEPR theory to predict the molecular shape of the carbon tetraiodide molecule, CI 4. A tetrahedral C bent B linear D trigonal planar 19 Which molecule is linear? A SO2 C H2S B CO2 D Cl2O 2
3 20 What is the molecular geometry of this lewis structure (NF 3 )? A square pyramidal C trigonal pyramidal B tetrahedral D linear 21 Which of the following compounds has an ionic bond? A SO3 C NaCl B HCl D CO2 22 Which of the following is the best representation of the compound rubidium chloride? A C B D 23 How many valence electrons are in a Se -2 ion? A 8 C 6 B 7 D 2 24 In the Molecular Models Lab, you built the structure for Hydrogen Fluoride. What is the polarity of that molecule and why? A Nonpolar because H and F have the same electronegativities. C Polar because F is more electronegative than H. B Polar because H and F are both nonmetals. D Nonpolar because H is more electronegative than F. 3
4 Matching Match each item with the correct statement below. A halide ion E valence electron B octet rule F acid base reaction C ionic bond G metallic bond D electron dot structure 25 an electron in the highest occupied energy level of an atom 26 Atoms react so as to acquire the stable electron structure of a noble gas. 27 a depiction of valence electrons around the symbol of an element 28 the attraction of valence electrons for metal ions 29 the force of attraction binding oppositely charged ions together 4
5 Chapter 12 Prep-Test Answer Section MULTIPLE CHOICE 1 ANS: C PTS: 1 DIF: I OBJ: ANS: D PTS: 1 DIF: II OBJ: ANS: D PTS: 1 DIF: I OBJ: ANS: D PTS: 1 DIF: I OBJ: ANS: D PTS: 1 DIF: L1 REF: p. 187 OBJ: STA: Ch.1.c Ch.2.a Ch.1.d 6 ANS: A PTS: 1 DIF: L1 REF: p. 188 OBJ: STA: Ch.1.c Ch.2.a Ch.1.d 7 ANS: D PTS: 1 DIF: L1 REF: p. 190 OBJ: STA: Ch.1.c Ch.2.g 8 ANS: A PTS: 1 DIF: L1 REF: p. 191 OBJ: STA: Ch.1.g Ch.2.a 9 ANS: A PTS: 1 DIF: L1 REF: p. 196 OBJ: STA: Ch.2.a 10 ANS: B PTS: 1 DIF: L1 REF: p. 201 OBJ: STA: Ch.2.a 11 ANS: A PTS: 1 DIF: L1 REF: p. 201 OBJ: STA: Ch.2.a 12 ANS: C PTS: 1 DIF: I OBJ: ANS: A PTS: 1 DIF: I OBJ: ANS: B PTS: 1 DIF: III OBJ: ANS: C PTS: 1 DIF: II OBJ: ANS: D PTS: 1 DIF: III OBJ: ANS: B PTS: 1 DIF: I OBJ: ANS: A PTS: 1 DIF: III OBJ: ANS: B PTS: 1 20 ANS: C PTS: 1 21 ANS: C PTS: 1 22 ANS: C PTS: 1 23 ANS: A PTS: 1 24 ANS: C PTS: 1 MATCHING 25 ANS: E PTS: 1 DIF: L1 REF: p. 187 OBJ: STA: Ch.2.a 1
6 26 ANS: B PTS: 1 DIF: L1 REF: p. 188 OBJ: STA: Ch.2.a 27 ANS: D PTS: 1 DIF: L1 REF: p. 188 OBJ: STA: Ch.2.e 28 ANS: G PTS: 1 DIF: L1 REF: p. 192 OBJ: ANS: C PTS: 1 DIF: L1 REF: p. 194 OBJ: STA: Ch.2.a 2
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Today: Ionic Bonding vs. Covalent Bonding Bond Polarities: Nonpolar Covalent vs. Polar Covalent vs. Ionic Electronegativity Differences Dipole Moments Molecular Polarities: Molecular Symmetry QUIZ 3 Next
3) How many electrons will each of the following gain or lose when it forms an ion? (i) chlorine (ii) calcium (iii) aluminum
Chapter 6 Ionic and Molecular Compounds Practice Problems 1) In ionic compounds, (i) lose their valence electrons to form positively charged (ii) and (iii) gain valence electrons to form negatively charged