3) How many electrons will each of the following gain or lose when it forms an ion? (i) chlorine (ii) calcium (iii) aluminum

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1 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 (iv). A) (i) metals (ii) anions (iii) nonmetals (iv) cations B) (i) nonmetals (ii) cations (iii) metals (iv) anions C) (i) metals (ii) polyatomic ions (iii) nonmetals (iv) anions D) (i) nonmetals (ii) anions (iii) metals (iv) cations E) (i) metals (ii) cations (iii) nonmetals (iv) anions 2) An anion is always (i) and a cation is always (ii). A) (i) negative (ii) negative B) (i) positive (ii) positive C) (i) negative (ii) positive D) (i) positive (ii) negative E) (i) metals (ii) nonmetals 3) How many electrons will each of the following gain or lose when it forms an ion? (i) chlorine (ii) calcium (iii) aluminum A) (i) gain 1 (ii) gain 2 (iii) gain 3 B) (ii) gain 1 (ii) lose 2 (iii) gain 3 C) (iii) lose 1 (ii) gain 2 (iii) lose 3 D) (iii) lose 1 (ii) lose 2 (iii) lose 3 E) (iii) gain 1 (ii) lose 2 (iii) lose 3 4) What is the symbol for the ion with 19 protons and 18 electrons? A) F+ B) F- C) Ar+ D) K- E) K+ 5) The number of electrons in an ion with 20 protons and an ionic charge of 2 + is A) 24. B) 22. C) 20. D) 18. E) P a g e

2 6) Elements in group 2 of the periodic table form ions with a charge of A) 1+ B) 1- C) 2+ D) 3+ E) 2-7) What is the correct formula for the oxide ion? A) O 2- B) O C) O + D) O 2+ E) O 3+ 8) What is the formula of the nitride ion? A) N 3- B) NO 2 C) NO 3 3 D) NO 3 2 E) NO 3 9) Classify each of the following compounds as molecular or ionic. a. OF2 = b. K2S = c. KBr = d. FeCl3 = e. XeF2 = f. PH3 = g. PbF4 = h. P2F4 = i. NF3 = 10) An ionic compound A) has a net positive charge. B) has a net negative charge. C) contains only cations. D) contains only anions. E) has a net charge of zero. 2 P a g e

3 11) A group of covalently bonded atoms that has an overall electrical charge is called a(n) A) ionic compound. B) anion. C) polyatomic ion. D) cation. E) molecule. 12) What is the correct formula for the iron(ii) ion? A) Fe + B) Fe 2+ C) Fe 3+ D) Fe 2- E) Fe 3-13) Which one of the following compounds contains an ion with a 3+ charge? A) KCl B) Na 2 O C) FeCl 3 D) CuCl E) MgCl 2 14) The name of the Cu + ion is A) copper(ii). B) copper(i). C) cobalt. D) copper. E) carbon. 15) In a molecule with covalent bonding A) oppositely charged ions are held together by strong electrical attractions. B) atoms of metals form bonds to atoms of nonmetals. C) atoms of different metals form bonds. D) atoms are held together by sharing electrons. E) atoms of noble gases are held together by attractions between oppositely charged ions. 16) The types of compounds that use prefixes in their names are A) ionic compounds. B) ionic compounds involving transition metals. C) polyatomic ions. D) covalent compounds. E) compounds that contain polyatomic ions. 3 P a g e

4 17) In a covalently bonded molecule, the number of electrons that an atom shares with others is usually equal to the number of electrons A) in the atom. B) in its nucleus. C) in all the atoms. D) in its ion. E) needed to give it a stable electron configuration. 18) Which of the following formulas are correctly written? Select ALL the correct formulas, this is a multiple response question. a. CaS b. AlP c. AlS d. Ca3N2 e. Al3Se2 f. Sr3(PO4)2 g. SrSO4 h. NaNO2 i. Ba(NO3)2 j. Na2NO3 19) Which of the following formulas are correctly written? Select ALL the correct formulas, this is a multiple response question. a. NH4ClO4 b. (NH4)3PO4 c. NH4SO4 d. H4NO2 e. NH4Cl f. NH4CO3 g. NH4ClO h. (NH4)2S i. (NH4)2NO3 j. (NH4)2SO3 4 P a g e

5 20) Which of the following formulas are correctly written for the names given? Select ALL the correct formulas, this is a multiple response question. a. tin (II) oxide = SnO? b. iron (III) oxide = FeO3? c. iron (II) nitide = FeN? d. tin (IV) nitride = Sn3N4? e. copper (I) oxide = CuO? f. cobalt (II) nitrate = CO2NO3? g. divanadium trioxide = V2O3? h. vanadium (III) oxide = V2O3? i. copper (II) nitride = Cu3N2? j. copper (II) hydroxide = Cu(OH)2? k. iron (III) nitride = FeN? l. lead (II) oxide = PbO2? 21) Which of the following names are correctly written from the formulas? Select ALL the correct formulas, this is a multiple response question. a. N2O4, dinitrogen tetraoxide b. Li2O, dilithium monoxide c. H2O, dihydrogen monoxide d. Na2CO3, disodium carbonate e. Na3PO4, sodium phosphate f. (NH4)2S, diammonium sulfide g. AlCl3, aluminum chloride h. CuCl2, copper (II) chloride i. ZnCl2, zinc dichloride 22) In the Lewis structure of CO2, C has (i) lone pairs of electrons and (ii) bonded pairs of electrons. A) 0, 2 B) 0, 4 C) 1, 3 D) 1, 4 E) 1, 5 5 P a g e

6 23) In the Lewis structure of H2S, S has (i) lone pairs of electrons and (ii) bonded pairs of electrons. A) 0, 4 B) 0, 2 C) 2, 2 D) 2, 0 E) 1, 2 24) In the Lewis structure of SiCl4, Si has (i) lone pairs of electrons and (ii) bonded pairs of electrons. A) 0, 4 B) 2, 2 C) 4, 0 D) 0, 8 E) 1, 5 25) In the Lewis structure of XeF4, Xe has (i) lone pairs of electrons and (ii) bonded pairs of electrons. A) 0, 3 B) 0, 4 C) 1, 3 D) 1, 4 E) 1, 5 26) In the Lewis structure of SO 3 2 where all the atoms satisfy the octet rule, S has (i) lone pairs of electrons and (ii) bonded pairs of electrons. A) 0, 3 B) 0, 4 C) 1, 3 D) 1, 4 E) 1, 5 27) In the Lewis structure of IBr 4, I has (i) nonbonded electrons and (ii) bonded electrons. A) 0, 8 B) 2, 8 C) 2, 4 D) 4, 8 E) 4, 2 28) How many double bonds are present in the Lewis structure of SO3? A) 0 B) 1 C) 2 D) 3 E) 4 6 P a g e

7 29) Double and triple bonds form because A) the atoms involved have high electronegativities. B) single covalent bonds do not give all of the atoms in the molecule eight valence electrons. C) one of the atoms in the molecule has more than eight valence electrons. D) the ions involved have charges larger than one. E) there is at least one hydrogen atom involved in the bond. 30) The ability of an atom to attract the shared electrons in a covalent bond is its A) electronegativity. B) bonding ability. C) polarity. D) ionic character. E) nonpolarity. 31) On the periodic table, electronegativity increases: A) down and to the right B) up and to the left C) down and to the left D) up and to the right E) it varies across the periodic table. 32) Which of the following substances contains a nonpolar covalent bond? A) H 2 O B) NaCl C) NH 3 D) MgF 2 E) N 2 33) Which of the following elements has the lowest electronegativity? A) Li B) C C) N D) O E) F 34) Which of the following compounds contains a polar covalent bond? A) NaF B) HCl C) Br 2 D) MgO E) O 2 7 P a g e

8 35) Which of the following compounds contains an ionic bond? A) NH 3 B) H 2 O C) CaO D) H 2 E) CH 4 36) If the electronegativity difference between elements X and Y is 2.1, the bond between the elements X-Y is A) ionic. B) nonpolar ionic. C) nonpolar covalent. D) polar covalent. E) impossible. 37) Ionic bonding is expected in which of these compounds? A) Cl 2 B) KF C) OF 2 D) HF E) H 2 38) A polar covalent bond is found in which of these compounds? A) H 2 O B) F 2 C) NaCl D) H 2 E) N 2 39) The bond in Cl 2 is a(n) A) ionic bond. B) nonpolar covalent bond. C) metallic bond. D) polar ionic bond. E) no bond. 40) The VSEPR theory allows us to determine the most favorable A) shape of a molecule. B) charge on an ion. C) color of a compound. D) bond type for a molecule. E) formula for a compound. 8 P a g e

9 41) The shape of the carbon tetrachloride molecule is A) linear B) bent C) trigonal pyramidal. D) tetrahedral. E) trigonal planar 42) The shape of the ammonia molecule (NH3) is A) linear B) bent C) trigonal pyramidal. D) tetrahedral. E) trigonal planar 43) The shape of carbon dioxide (CO2) is A) linear B) bent C) trigonal pyramidal. D) tetrahedral. E) trigonal planar 44) The shape of the water molecule (H2O) is A) linear B) bent C) trigonal pyramidal. D) tetrahedral. E) trigonal planar 45) Hydrogen sulfide, H 2 S, has a shape similar to A) carbon dioxide. B) carbon monoxide. C) hydrogen chloride. D) water. E) carbon tetrachloride. 46) The carbon tetrachloride molecule, CCl 4, is A) a polar molecule with polar bonds. B) a nonpolar molecule with polar bonds. C) a nonpolar molecule with nonpolar bonds. D) a polar molecule with nonpolar bonds. E) a polar molecule with ionic bonds. 9 P a g e

10 47) The ammonia molecule (NH3) is A) a polar molecule with polar bonds. B) a nonpolar molecule with polar bonds. C) a nonpolar molecule with nonpolar bonds. D) a polar molecule with nonpolar bonds. E) a polar molecule with ionic bonds. 48) The strongest interactions between molecules of ammonia (NH3) are A) ionic bonds. B) hydrogen bonds. C) polar covalent. D) dipole-dipole. E) dispersion forces. 49) The strongest interactions between molecules of hydrogen (H2) are A) ionic bonds. B) hydrogen bonds. C) polar covalent. D) dipole-dipole. E) dispersion forces. 50) The strongest interactions between molecules of hydrogen chloride (HCl) are A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces. 51) The strongest interactions between molecules of iodine I2 are examples of A) ionic bonds. B) covalent bonds. C) hydrogen bonds. D) dipole-dipole interactions. E) dispersion forces. 52) From weakest to strongest, list the inter- and intra- molecular forces: A) Dipole-dipole < London dispersion < covalent < ionic < Hydrogen bond B) ionic < covalent < London dispersion < dipole-dipole < Hydrogen bond C) London dispersion < Hydrogen bond < dipole-dipole < covalent < ionic D) London dispersion < Dipole-dipole < Hydrogen bond < covalent < ionic E) covalent < London dispersion < ionic < Hydrogen bond < dipole-dipole 10 P a g e