Q&A Hero

Q: The compound ICl contains A) ionic bonds. B) nonpolar covalent bonds. C) polar covalent bonds, with partial negative charges on the Cl atoms. D) polar covalent bonds, with partial negative charges on the I atoms.

Q: A reactive element with a relatively high electronegativity would be expected to have a relatively A) small negative electron affinity and a relatively low ionization energy. B) small negative electron affinity and a relatively high ionization energy. C) large negative electron affinity and a relatively low ionization energy. D) large negative electron affinity and a relatively high ionization energy.

Q: The electronegativity is 2.1 for H and 1.8 for Si. Based on these electronegativities, SiH4 would be expected to A) be ionic and contain H- ions. B) be ionic and contain H+ ions. C) have polar covalent bonds with a partial negative charges on the H atoms. D) have polar covalent bonds with a partial positive charges on the H atoms.

Q: Of the following elements, which has the lowest electronegativity? A) Mg B) Cl C) Ca D) Br

Q: Of the following elements, which has the highest electronegativity? A) P B) S C) Sc D) As

Q: When melting S8 ________ forces must be overcome and S8 is expected to have a ________ melting point than MgS. A) covalent bonding, higher B) covalent bonding, lower C) intermolecular, higher D) intermolecular, lower

Q: Compound A is a solid with a melting point of 125C, and compound B is a gas at 25C and one atmosphere pressure. Based on these data, one would expect A) both compounds to be covalent. B) compound A to be ionic and compound B to be covalent. C) compound A to be covalent and compound B to be ionic. D) both compounds to be ionic.

Q: In general, at room temperature A) ionic compounds are all solids and covalent compounds are all gases. B) ionic compounds are all solids, but covalent compounds may be solids, liquids, or gases. C) ionic compounds are all solids, and covalent compounds are liquids or gases. D) covalent compounds are all gases, but ionic compounds may be solids, liquids, or gases.

Q: The Cl-Cl bond energy is 243 kJ/mol. Therefore the formation of a single bond between chlorine atomsA) should require the absorption of 243 kJ per mole of Cl2 formed.B) should require the absorption of 486 kJ per mole of Cl2 formed.C) should result in the release of 243 kJ per mole of Cl2 formed.D) should result in the release of 486 kJ per mole of Cl2 formed.

Q: Which molecule contains the most easily broken carbon-carbon bond?A) H3C-CH3B) H2C=CH2C) F2C=CF2D) HCCH

Q: Which bond should have the highest bond dissociation energy?A) N-NB) NNC) NND) All three bonds should have about the same dissociation energy.

Q: Which is the longest bond?A) N-NB) N=NC) NND) All three bond lengths should be about the same.

Q: Butyric acid has the structural formula given below. What is the molecular or chemical formula for butyric acid? A) CHO B) C2H4O C) C4H8O2 D) C5H8O3

Q: At the equilibrium bond length A) the attractive forces holding the atoms together are less than the repulsive forces. B) the potential energy is a maximum. C) the potential energy is a minimum. D) the repulsive forces are greater than the attractive forces holding the atoms together.

Q: Which electrostatic forces hold atoms together in a molecule? A) electron-electron forces B) electron-nucleus forces C) nucleus-nucleus forces D) all three forces

Q: Covalent bonding is a A) gain of electrons. B) loss of electrons. C) transfer of electrons. D) sharing of electrons.

Q: Calculate the energy change for the formation of LiCl(s) from its elements in their standard states and the following tabulated information: A) +1305.7 kJ/mol B) +296.9 kJ/mol C) -400.3 kJ/mol D) -627.2 kJ/mol

Q: In the reaction of sodium metal with chlorine gas which of the following processes releases energy?A) Cl2(g) -> 2 Cl(g)B) Cl(g) + e- -> Cl-(g)C) Na(s) -> Na(g)D) Na(g) -> Na+(g) + e-

Q: The octet rule is most likely to fail occasionally for which of the following elements? A) C B) N C) Na D) S

Q: How many electrons does magnesium lose and nitrogen need to form Mg3N2? A) magnesium loses 2 and nitrogen gains 2 B) magnesium loses 2 and nitrogen gains 3 C) magnesium loses 3 and nitrogen gains 2 D) magnesium loses 3 and nitrogen gains 3

Q: An element M reacts with chlorine to form MCl2, with oxygen to form MO, and with nitrogen to form M3N2. The most likely candidate for the element is A) Li B) Mg C) Al D) Si

Q: Which species does not have an octet of electrons for its outer core? A) C4- B) P3- C) O2- D) Mg+

Q: To reach a noble gas electron configuration how many electrons would sulfur have to adopt? A) 1 B) 2 C) 6 D) 8

Q: An element that has the valence electron configuration 3s23p3 belongs to which period and group? A) period 3; group 3A B) period 3; group 5A C) period 4; group 3A D) period 4; group 5A

Q: How many valence shell electrons does an atom of aluminum have? A) 1 B) 2 C) 3 D) 13

Q: What is the general trend in ionization energy and electron affinity values? A) Both decrease as one traverses a period from left to right and both decrease as one descends a group. B) Both decrease as one traverses a period from left to right and both increase as one descends a group. C) Both increase as one traverses a period from left to right and both decrease as one descends a group. D) Both increase as one traverses a period from left to right and both increase as one descends a group.

Q: Which of these elements has the most favorable (most negative) electron affinity? A) Ca B) N C) Ne D) S

Q: Which element has the least favorable (least negative) electron affinity? A) B B) C C) N D) O

Q: Which element has the most favorable (most negative) electron affinity? A) Na B) Mg C) O D) Ne

Q: Which element has the most favorable (most negative) electron affinity? A) B B) C C) Li D) N

Q: Which electron affinity process would liberate the most energy?A) [He] 2s2 + e- -> [He] 2s2 2p1B) [He] 2s2 2p2 + e- -> [He] 2s2 2p3C) [He] 2s2 2p3 + e- -> [He] 2s2 2p4D) [He] 2s2 2p6 + e- -> [He] 2s2 2p6 3s1

Q: Which liberates the most energy?A) Br(g) + e- -> Br-(g)B) Cl(g) + e- -> Cl-(g)C) F(g) + e- -> F-(g)D) I(g) -> I-(g)

Q: Which liberates the most energy?A) F(g) + e- -> F-(g)B) N(g) + e- -> N-(g)C) O(g) + e- -> O-(g)D) C(g) + e- -> C-(g)

Q: Which period 3 element has successive first through seventh ionization energies (kJ/mol) : Ei1 = 578; Ei2 = 1,817; Ei3 = 2,745; Ei4 = 11,575; Ei5 = 14,830; Ei6 = 18,376; and Ei7 = 23,293? A) Mg B) Al C) S D) Cl

Q: Consider the following electron configurations for neutral atoms: I = 1s22s22p63s2 II = 1s22s22p63s23p4 III = 1s22s22p63s23p6 Which atom would be expected to have the largest third ionization energy? A) atom I B) atom II C) atom III D) All of these atoms would be expected to have the same third ionization energy.

Q: Which of the following represents the change in electronic configuration that is associated with the first ionization energy of magnesium?A) [Ne]3s13p1 -> [Ne]3s1 + e-B) [Ne]3s2 -> [Ne]3s13p1C) [Ne]3s2 -> [Ne]3s1 + e-D) [Ne]3s2 + e- -> [Ne]3s23p1

Q: Which of the following atoms with the specified electronic configurations would have the lowest first ionization energy? A) [He]2s22p3 B) [Ne]3s23p4 C) [Xe]6s1 D) [Xe]6s24f145d106p1

Q: Which of the following species will have the highest ionization energy? A) Na+ B) Ne C) F- D) O2-

Q: Which ionization process requires the most energy?A) S(g) -> S+(g) + e-B) S+(g) -> S2+(g) + e-C) Cl(g) -> Cl+(g) + e-D) Cl+(g) -> Cl2+(g) + e-

Q: Which ionization process requires the most energy?A) P(g) -> P+(g) + e-B) P+(g) -> P2+(g) + e-C) P2+(g) -> P3+(g) + e-D) P3+(g) -> P4+(g) + e-

Q: List the elements Cs, Ca, Ne, Na, Ar in order of decreasing first ionization energy. A) Ar > Ca > Cs > Na > Ne B) Ne > Ar > Ca > Na > Cs C) Ne > Ar > Na > Cs > Ca D) Ne > Na > Cs > Ca > Ar

Q: List the elements Na, Ca, Rb, Cl, He in order of decreasing first ionization energy. A) He > Cl > Ca > Na > Rb B) He > Na > Ca > Cl > Rb C) He > Na > Cl > Ca > Rb D) Rb > Ca > Cl > Na > He

Q: Of the following, which element has the highest first ionization energy? A) Cl B) F C) O D) S

Q: Of the following, which element has the highest first ionization energy? A) Ca B) Cl C) Na D) Se

Q: Of the following, which element has the highest first ionization energy? A) Ca B) K C) Li D) Mg

Q: Of the following, which element has the highest first ionization energy? A) aluminum B) magnesium C) silicon D) sodium

Q: Of the following, which element has the highest first ionization energy? A) beryllium B) boron C) hydrogen D) lithium

Q: Consider Li+, F-, and O2-. Which ratio should be the largest? A) (radius Li+)/(radius F-) B) (radius Li+)/(radius O2-) C) (radius F-)/(radius Li+) D) (radius O2-)/(radius Li+)

Q: Which of the following most likely represent the atomic radius of a Cr atom, the ionic radius of a Cr2+ ion, and the ionic radius of a Cr3+ ion? A) 128 pm for Cr, 167 pm for Cr2+, and 193 pm for Cr3+ B) 128 pm for Cr, 147 pm for Cr2+, and 193 pm for Cr3+ C) 128 pm for Cr, 109 pm for Cr2+, and 63 pm for Cr3+ D) 128 pm for Cr, 89 pm for Cr2+, and 63 pm for Cr3+

Q: Arrange the ions N3-, O2-, Mg2+, Na+, and F- in order of increasing ionic radius, starting with the smallest first. A) Mg2+, Na+, F-, O2-, N3- B) N3-, Mg2+, O2-, Na+, F- C) N3-, O2-, Mg2+, F-, Na+ D) N3-, O2-, F-, Na+, Mg2+

Q: Indicate which is larger in each of the following two sets. (I) Cr3+ or Cr (II) Se2- or Se A) Cr3+ is larger than Cr and Se2- is larger than Se. B) Cr3+ is larger than Cr and Se is larger than Se2-. C) Cr is larger than Cr3+ and Se2- is larger than Se. D) Cr is larger than Cr3+ and Se is larger than Se2-.

Q: Which ion has the smallest ionic radius?A) F-B) Cl-C) Br-D) I-

Q: Which ion has the smallest ionic radius? A) Li+ B) Na+ C) K+ D) Rb+

Q: Most of the compounds of the 2+ ions of the first row of the transition metals from Mn to Zn are colored due to absorption of visible light promoting an electron from one 3d orbital to another. Which of these ions should tend to form colorless compounds? A) Mn2+ B) Co2+ C) Cu2+ D) Zn2+

Q: Which ion has the same electron configuration as Kr?A) Rb+B) Br-C) Se2-D) All of the above

Q: What is the ground-state electron configuration of Se2-? A) [Ar]3d104s24p2 B) [Ar]3d104s24p4 C) [Ar]3d124s24p4 D) [Ar]3d104s24p6

Q: Which two ions have the same electron configuration in the ground state? A) Rb+ and Cs+ B) Ba2+ and I- C) Se2+ and I- D) Fe2+ and Fe3+

Q: Which of the following three sets consist of atoms or ions with the same electron configuration in the ground state? (I) O2-, Ne, and Mg2+ (II) Ni, Cu+, and Zn2+ (III) Hg, Tl+, and Pb2+ A) all three sets B) all but (I) C) all but (II) D) only (I)

Q: How many electrons are in the outermost shell of the In3+ ion in its ground state? A) 2 B) 3 C) 6 D) 18

Q: What is the ground-state electron configuration of the ion Hg2+? A) [Xe]4f145d10 B) [Xe]4f145d86s2 C) [Xe]4f145d106s2 D) [Xe]4f145d106s26p2

Q: Which of the compounds, C3H8, MgCl2, Zn(NO3)2, OCl2, are expected to exist as molecules? A) only C3H8 B) C3H8 and OCl2 C) C3H8, Zn(NO3)2, and OCl2 D) MgCl2 and Zn(NO3)2

Q: Which of the compounds, Li3P, PH3, C2H6, IBr3, are ionic compounds? A) only C2H6 B) only Li3P C) Li3P and PH3 D) PH3, C2H6, and IBr3

Q: Which of the following is the correct chemical formula for a molecule of bromine? A) Br B) Br- C) Br+ D) Br2

Q: Which one of the following compounds contains ionic bonds? A) CaO B) HF C) NI3 D) SiO2

Q: What type of bonding is found in the compound PCl5? A) covalent bonding B) hydrogen bonding C) ionic bonding D) metallic bonding

Q: The gas Freon-11, CCl3F, contains A) C4+, Cl-, and F- ions. B) C4+, Cl3-, and F- ions. C) C4+ and Cl3F4- ions. D) CCl3F molecules.

Q: In which set do all elements tend to form cations in binary ionic compounds? A) Li, B, O B) Mg, Cr, Pb C) N, As, Bi D) O, F, Cl

Q: Which of the following statements concerning ionic compounds is true? A) Essentially all ionic compounds are solids at room temperature and pressure. B) Ionic compounds do not contain any covalent bonds. C) Ionic compounds contain the same number of positive ions as negative ions. D) The chemical formula for an ionic compound must show a nonzero net charge.

Q: The definitive distinction between ionic bonding and covalent bonding is that A) ionic bonding involves a sharing of electrons and covalent bonding involves a transfer of electrons. B) ionic bonding involves a transfer of electrons and covalent bonding involves a sharing of electrons. C) ionic bonding requires two nonmetals and covalent bonding requires a metal and a nonmetal. D) covalent bonding requires two nonmetals and ionic bonding requires a metal and a nonmetal.

Q: How many electrons are in the ion, CO32-? A) 16 B) 28 C) 30 D) 32

Q: In which of the following sets do all species have the same number of protons? A) Br-, Kr, Sr2+ B) C, N3-, O2- C) Mg2+, Sr2+, Ba2+ D) O, O2-, O2+

Q: In which of the following sets do all species have the same number of electrons? A) Br-, Kr, Sr2+ B) C, N3-, O2- C) Mg2+, Sr2+, Ba2+ D) O, O2-, O2+

Q: How many electrons are in the ion, Zn2+? A) 28 B) 30 C) 32 D) 65

Q: Which of the species below has 28 protons and 26 electrons? A) Fe2+ B) Ni2+ C) Fe D) Ni

Q: The formula of iron(III) oxide contains ________ iron(III) and ________ oxide ions.

Q: Phosphate ion has the formula ________.

Q: Lattice energy increases with ________ cation and anion charges and ________ cation and anion radii.

Q: The group 4A element that always obeys the octet rule in its stable compounds is ________.

Q: The element in group 7A with the least favorable (least negative) electron affinity is ________.

Q: The element in period 3 with the smallest seventh ionization energy is ________.