1) The basis of the VSEPR model of molecular bonding is ________. |
D) electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions |
2) In counting the electron domains around the central atom in VSEPR theory, a ________ is not included. |
C) core level electron pair |
3) The H-C-H bond angle in the CH4 ion is approximately ________. |
C) 109.5 |
3) The electron-domain geometry of ________ is tetrahedral. |
E) all of the above except XeF4 |
4) Of the following species, ________ will have bond angles of 120°. |
D) BCl3 |
5) The molecular geometry of the BrO3- ion is ________. |
A) trigonal pyramidal |
6) The molecular geometry of the left-most carbon atom in the molecule below is ________. A) trigonal planar |
C) tetrahedral |
10) The central Xe atom in the XeF4 molecule has ________ unbonded electron pair(s) and ________ bonded electron pair(s) in its valence shell. |
B) 2, 4 |
11) An electron domain consists of ________. a) a nonbonding pair of electrons A) a only |
D) a, b, and c |
12) The molecular geometry consists of ________. a) a nonbonding pair of electrons A) a only |
E) b and c |
13) The electron-domain geometry and the molecular geometry of a molecule of the general formula ABn are ________. |
C) sometimes the same |
14) The electron-domain geometry and the molecular geometry of a molecule of the general formula ABn will always be the same if ________. |
A) there are no lone pairs on the central atom |
15) A molecule has the formula AB3 and the central atom is in a different plane from the surrounding three atoms. Its molecular shape is ________. |
B) trigonal pyramidal |
16) PCl5 has ________ electron domains and a ________ molecular arrangement. |
D) 5, trigonal bipyramidal |
17) For molecules of the general formula ABn, n can be greater than four ________. |
B) only when A is an element from the third period or below the third period |
(i) PCl3 (ii) CCl4 (iii) TeCl4 (iv) XeF4 (v) SF6 18) For which of the molecules is the molecular geometry (shape) the same as the VSEPR electron domain arrangement (electron domain geometry)? |
C) (ii) and (v) |
19) Of the molecules below, only ________ is polar. |
C) SeF4 |
20) Of the molecules below, only ________ is nonpolar. |
A) BF3 |
21) Three monosulfur fluorides are observed: SF2, SF4, and SF6. Of these, ________ is/are polar. |
B) SF2 and SF4 only |
22) The molecular geometry of the PF3 molecule is ________, and this molecule is ________. |
C) trigonal pyramidal, polar |
23) Of the following molecules, only ________ is polar. |
D) SiH2Cl2 |
24) Of the following molecules, only ________ is polar. |
C) NCl3 |
25) For molecules with only one central atom, how many lone pairs on the central atom guarantees molecular polarity? |
A) 1 |
26) The molecular geometry of the CHF3 molecule is ________, and the molecule is ________. |
D) tetrahedral, polar |
27) The molecular geometry of the BCl3 molecule is ________, and this molecule is ________. |
D) trigonal planar, nonpolar |
(i) PCl3 (ii) CCl4 (iii) TeCl4 (iv) XeF4 (v) SF6 28) Which of the molecules has a see-saw shape? |
(iii) TeCl4 |
(i) PCl3 (ii) CCl4 (iii) TeCl4 (iv) XeF4 (v) SF6 29) In which of the molecules does the central atom utilize d orbitals to form hybrid orbitals? |
D) (iii), (iv), and (v) (iii) TeCl4 (iv) XeF4 (v) SF6 |
30) The combination of two atomic orbitals results in the formation of ________ molecular orbitals. |
B) 2 |
31) Of the following, the central atom is sp3d2 hybridized only in ________. |
B) XeF4 |
32) The sp3d2 atomic hybrid orbital set accommodates ________ electron domains. |
E) 6 |
33) The sp2 atomic hybrid orbital set accommodates ________ electron domains. |
B) 3 |
34) The hybridizations of nitrogen in NF3 and NH3 are ________ and ________, respectively. |
D) sp3, sp3 |
35) The hybridizations of iodine in IF3 and IF5 are ________ and ________, respectively. |
B) sp3d, sp3d2 |
36) The hybridizations of bromine in BrF5 and of arsenic in AsF5 are ________ and ________, respectively. |
D) sp3d2, sp3d |
37) The hybrid orbitals used for bonding by the sulfur atom in the SF4 molecule are ________ orbitals. |
D) sp3d |
38) The hybrid orbitals used for bonding by Xe in the unstable XeF2 molecule are ________ orbitals. |
C) sp3d |
39) The hybridization scheme for BeF2 is ________. |
A) sp |
41) The electron-domain geometry of the AsF5 molecule is trigonal bipyramidal. The hybrid orbitals used by the As atom for bonding are ________ orbitals. |
D) sp3d |
42) ________ hybrid orbitals are used for bonding by Xe in the XeF4 molecule. |
D) sp3d2 |
(i) PCl3 (ii) CCl4 (iii) TeCl4 (iv) XeF4 (v) SF6 43) In which of the molecules is the central atom sp3d2 hybridized? |
(iv) XeF4 (v) SF6 |
44) When four atomic orbitals are mixed to form hybrid orbitals, how many hybrid orbitals are formed? |
D) four |
45) A triatomic molecule cannot be linear if the hybridization of the central atoms is ________. |
D) sp2 or sp3 |
46) Valence bond theory does not address the issue of ________. |
A) excited states of molecules |
47) A typical double bond ________. |
E) All of the above answers are correct. |
48) A typical triple bond ________. |
A) consists of one σ bond and two π bonds |
49) In a polyatomic molecule, "localized" bonding electrons are associated with ________. |
B) two particular atoms |
50) There are ________ σ bonds and ________ π bonds in H3C-CH2-CH CH-CH2-C CH. |
E) 16, 3 |
51) Which of the following molecules or ions will exhibit delocalized bonding? A) SO2, SO3, and SO32- |
C) SO2 and SO3 |
52) Which of the following molecules or ions will exhibit delocalized bonding? A) NH4+ and N3- |
B) NO2- only |
53) In order to exhibit delocalized π bonding, a molecule must have ________. |
B) at least two resonance structures |
54) In a typical multiple bond, the σ bond results from overlap of ________ orbitals and the π bond(s) result from overlap of ________ orbitals. |
A) hybrid, atomic |
55) The carbon-carbon σ bond in ethylene, H2C=CH2, results from the overlap of ________. |
C) sp2 hybrid orbitals |
56) The π bond in ethylene, H2C=CH2, results from the overlap of ________. |
E) p atomic orbitals |
57) A typical double bond consists of ________. |
D) one sigma and one pi bond |
58) The N-N bond in HNNH consists of ________. |
A) one σ bond and one π bond |
59) The hybridization of the terminal carbons in the H2C=C=CH2 molecule is ________. |
B) sp2 |
60) The hybridization of nitrogen in the H—C=N: molecule is ________. |
A) sp |
61) The hybridization of carbon in the H—C=N: molecule is ________. |
D) sp |
65) Electrons in ________ bonds remain localized between two atoms. Electrons in ________ bonds can become delocalized between more than two atoms. |
B) sigma, pi |
66) Structural changes around a double bond in the ________ portion of the rhodopsin molecule trigger the chemical reactions that result in vision. |
C) retinal |
67) The bond order of any molecule containing equal numbers of bonding and antibonding electrons is ________. |
A) 0 |
68) In comparing the same two atoms bonded together, the ________ the bond order, the ________ the bond length, and the ________ the bond energy. |
D) smaller, longer, smaller |
69) In comparing the same two atoms bonded together, the ________ the bond order, the ________ the bond length, and the ________ the bond energy. |
A) greater, shorter, greater |
70) Based on molecular orbital theory, the bond orders of the H—H bonds in H2, H2+, and H2- are ________, respectively |
D) 1, 1/2, and 1/2 |
71) Based on molecular orbital theory, the bond order of the H—H bond in the H2+ ion is ________. |
B) 1/2 |
72) An antibonding π orbital contains a maximum of ________ electrons. |
B) 2 |
73) According to MO theory, overlap of two s atomic orbitals produces ________. |
E) one bonding molecular orbital and one antibonding molecular orbital |
74) A molecular orbital can accommodate a maximum of ________ electron(s). |
2 |
75) Molecular Orbital theory correctly predicts paramagnetism of oxygen gas, O2. This is because ________. |
D) there are two unpaired electrons in the MO electron configuration of O2 |
76) Molecular Orbital theory correctly predicts diamagnetism of fluorine gas, F2. This is because ________. |
C) all electrons in the MO electron configuration of F2 are paired. |
77) Based on molecular orbital theory, the only molecule in the list below that has unpaired electrons is ________. |
D) O2 |
78) Based on molecular orbital theory, there is/are ________ unpaired electron(s) in the OF+ ion. |
D) 2 |
79) Based on molecular orbital theory, the bond order of the N—N bond in the N22+ ion is ________. |
D) 2 |
80) Based on molecular orbital theory, the bond order of the Be—Be bond in the Be2 molecule is ________. |
A) 0 |
81) Of the following, only ________ appears to gain mass in a magnetic field. |
D) O2 |
82) Of the following, ________ appear(s) to gain mass in a magnetic field. B2 N2 O2 A) O2 only |
E) B2 and O2 |
83) According to MO theory, overlap of two p atomic orbitals produces ________. |
B) one bonding molecular orbital and one antibonding molecular orbital |
84) According to MO theory, overlap of two p atomic orbitals produces ________. |
C) one π MO and one π MO or one σ MO and one σ σ* MO |
85) An antibonding MO ________ the corresponding bonding MO. |
D) is always higher in energy than |
86) The more effectively two atomic orbitals overlap, ________. |
E) the lower will be the energy of the resulting bonding MO and the higher will be the energy of the resulting antibonding MO |
87) The bond order of a homonuclear diatomic molecule can be decreased by ________. |
A) removing electrons from a bonding MO or adding electrons to an antibonding MO |
88) The order of MO energies in B2, C2, and N2 (σ2p > π2p), is different from the order in O2, F2, and Ne2 (σ2p > π2p). This is due to ________. |
D) greater 2s-2p interaction in B2, C2, and N2 |
1) For a molecule with the formula AB2, the molecular shape is ________. |
A) linear or bent |
2) For a molecule with the formula AB3, the molecular shape is ________. |
E) trigonal planar, trigonal pyramidal, or T-shaped |
3) The molecular geometry of ________ is square planar. |
B) XeF4 |
4) The molecular geometry of the CS2 molecule is ________. |
A) linear |
5) The molecular geometry of the SiH2Cl2 molecule is ________. |
B) tetrahedral |
6) The molecular geometry of the PHCl2 molecule is ________. |
C) trigonal pyramidal |
7) The molecular geometry of the CHCl3 molecule is ________. |
D) tetrahedral |
8) The molecular geometry of the SF2 molecule is ________. |
B) bent |
9) The molecular geometry of the PF4+ ion is ________. |
B) tetrahedral |
10) The F-B-F bond angle in the BF2- ion is approximately ________. |
C) 120° |
11) The Cl-Si-Cl bond angle in the SiCl2F2 molecule is approximately ________. |
B) 109.5° |
12) The F-B-F bond angle in the BF3 molecule is ________. |
C) 120° |
13) The O-S-O bond angle in SO2 is slightly less than ________. |
C) 120° |
14) The F-N-F bond angle in the NF3 molecule is slightly less than ________. |
B) 109.5° |
15) The molecular geometry of the H3O+ ion is ________. |
D) trigonal pyramidal |
16) The electron-domain geometry of a sulfur-centered compound is trigonal bipyramidal. The hybridization of the central sulfur atom is ________. |
D) sp3d |
17) The hybridization of orbitals on the central atom in a molecule is sp. The electron-domain geometry around this central atom is ________. |
B) linear |
18) The hybridization of orbitals on the central atom in a molecule is sp2. The electron-domain geometry about this central atom is ________. |
C) trigonal planar |
19) The hybridization of the carbon atom in carbon dioxide is ________. |
A) sp |
20) The hybridization of the central atom in the XeF4 molecule is ________. |
E) sp3d2 |
21) The electron-domain geometry of the AsF6- ion is octahedral. The hybrid orbitals used by the As atom for bonding are ________ orbitals. |
D) sp3d2 |
22) In order to produce sp3 hybrid orbitals, ________ s atomic orbital(s) and ________ p atomic orbital(s) must be mixed. |
B) one, three |
24) The angles between sp2 orbitals are ________. |
120 |
25) There are ________ σ and ________ π bonds in the H—C≡C—H molecule. |
A) 3 and 2 |
26) There are ________ σ and ________ π bond(s) in the H2C=CH2 molecule. |
E) 5 and 1 |
27) There are ________ σ and ________ π bonds in the H2C=C=CH2 molecule. |
E) 6, 2 |
28) The total number of π bonds in the H—C≡C—C≡C—C≡N molecule is ________. |
C) 6 |
1) ClF3 has "T-shaped" geometry. There is/are ________ non-bonding domain(s) in this molecule. |
B) 2 |
2) The electron domain and molecular geometry of SO3 are ________. |
D) trigonal planar, trigonal planar |
5) The central atom in the ICl4- ion has ________ nonbonded electron pair(s) and ________ bonded electron pair(s) in its valence shell. |
C) 2, 4 |
6) The central atom in a certain molecule has 1 nonbonded electron pairs and 2 bonded electron pairs in its valence shell. The molecular geometry of this molecule is ________. |
B) bent |
7) The central atom in a certain molecule has 4 nonbonded electron pairs and 2 bonded electron pairs in its valence shell. The molecular geometry of this molecule is ________. |
B) square planar |
8) The central atom in the O3 molecule has ________ nonbonded electron pair(s) and ________ bonded electron pair(s) in its valence shell. |
B) 1, 3 |
9) According to VSEPR theory, if there are three electron domains in the valence shell of an atom, they will be arranged in a(n) ________ geometry. |
E) bent |
10) The electron-domain geometry and molecular geometry of iodine trichloride are ________ and ________, respectively. |
C) trigonal bipyramidal, T-shaped |
11) The electron-domain geometry and molecular geometry of the nitrite ion are ________ and ________, respectively. |
D) trigonal planar, bent |
12) Using the VSEPR model, the electron-domain geometry of the central atom in O3 is ________. |
B) trigonal planar |
13) Using the VSEPR model, the electron-domain geometry of the central atom in ClO3- is ________. |
C) tetrahedral |
14) Using the VSEPR model, the electron-domain geometry of the central atom in ClF3 is ________. |
D) trigonal bipyramidal |
15) Using the VSEPR model, the electron-domain geometry of the central atom in XeF4 is ________. |
E) octahedral |
16) Using the VSEPR model, the molecular geometry of the central atom in KrF2 is ________. |
A) linear |
17) Using the VSEPR model, the molecular geometry of the central atom in SO3 is ________. |
B) trigonal planar |
45) The highest energy occupied molecular orbital in the C—C bond of the C2 molecule is _____. |
C) π2p |
44) The highest energy occupied molecular orbital in the F—F bond of the F2 molecule is _____. |
D) π*2p |
1) There are __________ paired and __________ unpaired electrons in the Lewis symbol for a phosphorus atom. A) 4, 2 |
C) 2, 3 |
2) In the Lewis symbol for a fluorine atom, there are __________ paired and __________ unpaired electrons.
A) 4, 2 |
D) 6, 1 |
3) Based on the octet rule, magnesium most likely forms a __________ ion. A) Mg2+ |
A) Mg2+ |
4) Based on the octet rule, phosphorus most likely forms a __________ ion. A) P3+ |
B) P3- |
5) Based on the octet rule, iodine most likely forms an __________ ion. A) I 2+ |
E) I — |
6) There are __________ unpaired electrons in the Lewis symbol for an oxygen atom. A) 0 |
C) 2 |
7) How many unpaired electrons are there in the Lewis structures of N3- a ion? A) 0 |
A) 0 |
8) How many unpaired electrons are there in an O2- ion? |
A) 0 |
9) The electron configuration of the phosphide ion ( P^3-) is __________. A) [Ne]3s^2 |
E) [Ne]3s^2 3p^6 |
10) The halogens, alkali metals, and alkaline earth metals have __________ valence electrons, respectively. A) 7, 4, and 6 |
D) 7, 1, and 2 |
11) The only noble gas without eight valence electrons is __________. A) Ar |
C) He |
12) Which of the following would have to lose two electrons in order to achieve a noble gas electron configuration? A) O, Se |
B) Sr |
13) Which of the following would have to gain two electrons in order to achieve a noble gas electron configuration? A) Br |
D) O, Se |
14) For a given arrangement of ions, the lattice energy increases as ionic radius __________ and as ionic charge __________. A) decreases, increases |
A) decreases, increases |
15) The electron configuration of the S2- ion is __________. |
D) [Ne] 3s^2 3p^6 |
16) The principal quantum number of the electrons that are lost when tungsten forms a cation is __________. A) 6 |
A) 6 |
17) Which one of the following species has the electron configuration [Ar] 3d^4? A) Mn2+ |
B) Cr2+ |
17) Which one of the following species has the electron configuration [Ar]3d^4 ? A) Mn 2+ |
B) Cr^2+ |
18) What is the electron configuration for the ion? A) [Ar] 4s^1 3d^6 |
B) [Ar] 4s^0 3d^7 |
19) What is the electron configuration for the Fe2+ ion? A) [Ar]4s^0 3d^6 |
A) [Ar]4s^0 3d^6 |
20) The formula of palladium(IV) sulfide is __________. A) Pd2S4 |
D) PdS2 |
21) Elements from opposite sides of the periodic table tend to form __________. A) covalent compounds |
B) ionic compounds |
22) Determining lattice energy from Born-Haber cycle data requires the use of __________. A) the octet rule |
D) Hess’s law |
23) How many single covalent bonds must a silicon atom form to have a complete octet in its valence shell? A) 3 |
B) 4 |
24) A __________ covalent bond between the same two atoms is the longest. A) single |
A) single |
25) How many hydrogen atoms must bond to silicon to give it an octet of valence electrons? A) 1 |
D) 4 |
26) A double bond consists of __________ pairs of electrons shared between two atoms. A) 1 |
B) 2 |
27) What is the maximum number of double bonds that a hydrogen atom can form? A) 0 |
A) 0 |
28) What is the maximum number of double bonds that a carbon atom can form? A) 4 |
D) 2 |
29) In the molecule below, which atom has the largest partial negative charge __________?
A) Cl |
B) F |
30) The ability of an atom in a molecule to attract electrons is best quantified by the __________. A) paramagnetism |
C) electronegativity |
31) Given the electronegativities below, which covalent single bond is most polar? A) C-H |
C) O-H |
32) Electronegativity __________ from left to right within a period and __________ from top to bottom within a group. A) decreases, increases |
C) increases, decreases |
33) A nonpolar bond will form between two __________ atoms of __________ electronegativity. A) different, opposite |
E) identical, equal |
34) The ion ICL4- has __________ valence electrons. A) 34 |
C) 36 |
35) The ion NO- has __________ valence electrons. A) 15 |
E) 12 |
36) The Lewis structure of shows __________ nonbonding electron pair(s) on As. A) 0 |
B) 1 |
37) The Lewis structure of shows that the central phosphorus atom has __________ nonbonding and __________ bonding electron pairs. A) 2, 2 |
B) 1, 3 |
38) The Lewis structure of HCN (H bonded to C) shows that __________ has __________ nonbonding electron pairs. A) C, 1 |
B) N, 1 |
39) The formal charge on carbon in the molecule below is __________. A) 0 |
A) 0 |
40) The formal charge on nitrogen in NO3- is __________.
A) -1 |
C) +1 |
41) The formal charge on sulfur in SO4^2- is __________, where the Lewis structure of the ion is:
A) -2 |
B) 0 |
42) In the Lewis structure of ClF, the formal charge on Cl is __________ and the formal charge on F is __________. A) -1, -1 |
B) 0, 0 |
43) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is __________. A) 0 |
B) +1 |
44) How many equivalent resonance forms can be drawn for – (carbon is the central atom)? A) 1 |
C) 3 |
45) How many equivalent resonance forms can be drawn for without expanding octet on the sulfur atom (sulfur is the central atom)? A) 0 |
B) 2 |
46) How many equivalent resonance structures can be drawn for the molecule of SO3 without having to violate the octet rule on the sulfur atom? A) 5 |
E) 3 |
47) How many different types of resonance structures can be drawn for SO3^2- the ion where all atoms satisfy the octet rule? A) 1 |
A) 1 |
53) Using the table of bond dissociation energies, the for the following reaction is __________ kJ.
A) -359 |
A) -359 |
1) Which ion below has a noble gas electron configuration? A) Li 2+ |
B) Be2+ |
2) Of the ions below, only __________ has a noble gas electron configuration. A) S3+ |
E) Cl- |
3) Which of the following has eight valence electrons? A) Ti4+ |
E) all of the above |
4) Which of the following does not have eight valence electrons? A) Ca |
A) Ca |
5) The chloride of which of the following metals should have the greatest lattice energy? A) potassium Answer: D |
… |
6) Lattice energy is __________. A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase |
A) the energy required to convert a mole of ionic solid into its constituent ions in the gas phase |
7) In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion charges _______ and the radii __________. A) increases, decrease, increase |
D) increases, increase, decrease |
9) Which energy change corresponds to the first ionization energy of potassium? A) 2 |
D) 3 |
10) The electron configuration [Kr]4d10 represents __________. A) Sr+2 |
D) Ag+1 |
11) Fe+2 ions are represented by __________. A) [Ar]3d1 |
C) [Ar]3d6 |
13) The type of compound that is most likely to contain a covalent bond is __________. A) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table |
C) one that is composed of only nonmetals |
14) In which of the molecules below is the carbon-carbon distance the shortest? A) H2C=CH2 |
B) H–C=C–H |
15) Of the atoms below, __________ is the most electronegative. A) Br |
E) F |
16) Of the atoms below, __________ is the most electronegative. A) Si |
B) Cl |
17) Of the atoms below, __________ is the least electronegative. A) Rb |
A) Rb |
18) Which of the elements below has the largest electronegativity? A) Si |
D) S |
19) Of the molecules below, the bond in __________ is the most polar. A) HBr |
D) HF |
20) Of the bonds below, __________ is the least polar. A) Na, S |
B) P, S |
21) Which of the following has the bonds correctly arranged in order of increasing polarity? A) Be–F, Mg–F, N –F, O–F |
B) O –F, N–F, Be–F, Mg–F |
22) Which two bonds are most similar in polarity? A) O–F and C–F |
A) O–F and C–F |
23) The bond length in an HI molecule is 1.61 Å and the measured dipole moment is 0.44 D. What is the magnitude (in units of e) of the negative charge on I in HI?
A) 1.6 x 10^-19 |
B) 0.057 |
24) Which of the following names is/are correct for the compound ? A) titanium dioxide and titanium (IV) oxide |
A) titanium dioxide and titanium (IV) oxide |
25) Which of the following names is/are correct for the compound ? A) tin (II) chloride and tin (IV) chloride |
B) tin tetrachloride and tin (IV) chloride |
26) The Lewis structure of N2H2 shows __________. A) a nitrogen-nitrogen triple bond |
C) each nitrogen has one nonbonding electron pair |
27) There are __________ valence electrons in the Lewis structure of CH3CH2Cl. A) 14 |
D) 20 |
28) In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons. A) 2, 2 |
B) 4, 2 |
28) In the Lewis symbol for a sulfur atom, there are __________ paired and __________ unpaired electrons. A) 2, 2 |
B) 4, 2 |
31) Resonance structures differ by __________. A) number and placement of electrons |
E) placement of electrons only |
32) The oxidation number of phosphorus in PF3 is __________. A) -2 |
C) +3 |
33) To convert from one resonance structure to another, __________. A) only atoms can be moved |
C) only electrons can be moved |
34) For resonance forms of a molecule or ion, __________. A) one always corresponds to the observed structure |
C) the observed structure is an average of the resonance forms |
(i) (ii) (iii) (iv) (v) 35) There can be four equivalent best resonance structures of __________. A) (ii) |
D) (iv) |
36) In which of the ions do all X-O bonds (X indicates the central atom) have the same length? A) none |
B) all |
37) Of the following, __________ cannot accommodate more than an octet of electrons. A) P |
C) O |
38) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) NF3 |
B) IF3 |
39) Based on the octet rule, boron will most likely form a __________ ion. A) B3- |
C) B3+ |
40) Which of the following does not have eight valence electrons? A) Cl- |
E) Sr+1 |
41) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) PO4^3- |
D) SeF4 |
42) The central atom in __________ does not violate the octet rule. A) SF6 |
C) CF4 |
43) The central atom in __________ violates the octet rule. A) NH3 |
C) BF3 |
44) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) ClF3 |
A) ClF3 |
45) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) NI3 |
C) ICL5 |
46) A valid Lewis structure of __________ cannot be drawn without violating the octet rule. A) NF3 |
B) BeH2 |
47) Why don’t we draw double bonds between the Be atom and the Cl atoms in ? A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. |
A) That would give positive formal charges to the chlorine atoms and a negative formal charge to the beryllium atom. |
48) Which atom can accommodate an octet of electrons, but doesn’t necessarily have to accommodate an octet? A) N |
E) B |
49) Bond enthalpy is __________. A) always positive |
A) always positive |
50) Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform is __________ kJ/mol. A) 1241 |
A) 1241 |
51) Of the bonds , and , the bond is __________. A) strongest/shortest |
D) weakest/longest |
52) As the number of covalent bonds between two atoms increases, the distance between the atoms __________ and the strength of the bond between them __________. A) increases, increases |
D) decreases, increases |
53) Of the possible bonds between carbon atoms (single, double, and triple), __________. A) a triple bond is longer than a single bond |
D) a double bond is longer than a triple bond |
54) Most explosives are compounds that decompose rapidly to produce __________ products and a great deal of __________. A) gaseous, gases |
E) gaseous, heat |
55) Dynamite consists of nitroglycerine mixed with __________. A) potassium nitrate |
D) diatomaceous earth or cellulose |
56) Dynamite __________. A) was invented by Alfred Nobel |
E) all of the above |
Oxides of most nonmetals combine with water to form __________. |
an acid |
Which noble gas has the lowest first ionization energy? |
Radon |
Screening the nuclear charge by core electrons in atoms is |
More efficient than that by valence electrons |
Lattice energy is ________ |
The energy required to convert a mole of ionic solid into its constituent ions in the gas phase |
Atomic radius generally increases as we move |
Down a group and from right to left across a period |
The ion with the largest diameter is |
I- |
OF the following elements, ________ has the most negative electron affinity’ |
S |
Ca reacts with element X to form an ionic compound with the formula CaX. Al will react with X to form ____ |
Al2X2 |
Ozone is a(n) ________ of oxygen |
allotrope |
Hydrogen is unique among the elements because |
1, 2, 3, 5 |
Consider the following electron configurations to answer the questions that follow |
(iv) |
1) In which set of elements would all members be expected to have very similar chemical properties? |
Br, I, At |
Electrons in the 1s subshell are much closer to the nucleus in Ar than in He due to the larger __________ in Ar. |
nuclear charge |
3) The atomic radius of main-group elements generally increases down a group because __________. |
The Principle Quantum number of the Valence orbitals increase |
Atomic radius generally increases as we move __________. |
A) down a group and from right to left across a period |
Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr? |
K,CA,Ge,As,Kr |
6) Which isoelectronic series is correctly arranged in order of increasing radius? |
D) |
7) Of the choices below, which gives the order for first ionization energies? |
B) |
__________ have the lowest first ionization energies of the groups listed. |
A |
Which equation correctly represents the first ionization of aluminum? |
D |
Of the following species, __________ has the largest radius. A) Rb+ B) Sr2+ C) Br- D) Kr E) Ar |
C |
11) Of the following elements, __________ has the most negative electron affinity. A) S B) Cl C) Se D) Br E) I |
B |
12) ) Sodium is much more apt to exist as a cation than is chlorine. This is because ________. |
B |
13) In the generation of most anions, the energy change (kJ/mol) that _______ an electron is ________. |
D |
The list that correctly indicates the order of metallic character is __________. |
A |
15) Oxides of most nonmetals combine with base to form __________. |
C |
16) Oxides of the active metals combine with water to form __________. |
A |
Consider the general valence electron configuration of ns2np5 and the following statements: |
I II IV |
Write the condensed electron configurations for the following ions and (a) indicate which ones have noble gas configurations, (b) which ones are paramagnetic (have unpaired electrons). A) S2- B) Ag+ C) Ti4+ D) Sn2+ E) Co2+ F. As3- |
… |
Which of the following is not true about alkali metals? A) They are low density solids at room temperature. |
C |
the first ionization energies of the elements _____ as you go from left to right across a period of the periodic table, and _____ as you go from bottom to top. |
A |
In ionic bond formation, the lattice energy of ions_____ as the magnitude of the ion charges______ and the radii ____ . |
D |
Chem exam 3!!!
Share This
Unfinished tasks keep piling up?
Let us complete them for you. Quickly and professionally.
Check Price