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Chemistry
Q:
What is the geometry around the central atom in the following molecular model of NO2-? A) linear
B) bent
C) trigonal planar
D) trigonal pyramidal
Q:
What is the geometry around the central atom in the following molecular model of SO2? A) linear
B) bent
C) trigonal planar
D) trigonal pyramidal
Q:
What is the geometry around the central atom in the following molecular model of NO3-? A) linear
B) bent
C) trigonal planar
D) trigonal pyramidal
Q:
What is the geometry around the central atom in the following molecular model of BCl3? A) linear
B) bent
C) trigonal planar
D) trigonal pyramidal
Q:
Which is the best description of the bonding in NO3-?A) 3 N-O bonds and no N-O bondsB) 3 N-O bonds and 3 N-O bondsC) no N-O bonds and delocalized N-O molecular orbitals extending over all four atomsD) 3 N-O bonds and delocalized N-O molecular orbitals extending over all four atoms
Q:
The SO3 molecule can be described as having 3 S-O bonds and molecular orbitals containingA) 2 electrons.B) 4 electrons.C) 6 electrons.D) 8 electrons.
Q:
Molecular orbitals extending over more than two atoms provide an explanation for
A) coordinate covalent bonding.
B) ionic bonding.
C) paramagnetism.
D) resonance.
Q:
Which statement concerning any homonuclear diatomic molecule and its 1- ion must be true?
A) X2 must be more stable than X2-.
B) X2 must be less stable than X2-.
C) X2- must be paramagnetic and X2 must be diamagnetic.
D) X2- must be paramagnetic and X2 may be paramagnetic or diamagnetic.
Q:
The paramagnetism of O2 is explained by
A) coordinate covalent bonding.
B) molecular orbital theory.
C) resonance.
D) valence bond theory.
Q:
Given that O2 is paramagnetic and has a bond order of 2, and its highest occupied molecular orbital is antibonding, what would be the expected bond orders for O22- and O22+?
A) 1 for O22- and 3 for O22+
B) 3/2 for O22- and 5/2 for O22+
C) 5/2 for O22- and 3/2 for O22+
D) 3 for O22- and 1 for O22+
Q:
The following MO diagram is appropriate for Li2 and Be2. Based on this diagram, A) both are stable and diamagnetic.
B) Li2 is stable and diamagnetic, but Be2 is unstable.
C) Be2 is stable and diamagnetic, but Li2 is unstable.
D) Be2 is stable and paramagnetic, but Li2 is unstable.
Q:
The MO diagram below is appropriate for B2. Based on this diagram, B2 A) has a bond order of one and is diamagnetic.
B) has a bond order of one and is paramagnetic.
C) has a bond order of two and is diamagnetic.
D) has a bond order of two and is paramagnetic.
Q:
Which molecular orbitals for homonuclear diatomic molecules are degenerate?A) molecular orbitalsB) molecular orbitalsC) molecular orbitals and molecular orbitalsD) neither molecular orbitals nor molecular orbitals
Q:
Compare the energies of molecular orbitals of homonuclear diatomic molecules with the energies of the atomic orbitals with which they correlate.
A) Both bonding and antibonding molecular orbitals lie lower in energy than the atomic orbitals.
B) Bonding orbitals are lower and antibonding orbitals are higher in energy than the atomic orbitals.
C) Bonding orbitals are higher and antibonding orbitals are lower in energy than the atomic orbitals.
D) Both bonding and antibonding molecular orbitals are higher in energy than the atomic orbitals.
Q:
Based on formal charges, the best Lewis electron-dot structure of BF3 has a B"F bond order = ________.
Q:
The number of Lewis electron dot resonance structures required to describe NO2- is ________.
Q:
The Lewis electron-dot structure of H2CO has ________ nonbonding electron pairs, ________ bonding electron pairs, and a carbon-oxygen bond order of ________.
Q:
The Lewis electron-dot structure of N2 has ________ nonbonding electrons pairs, ________ bonding electron pairs, and a bond order of ________.
Q:
Of the bonds C-C, C-N, C-O, and C-F, the bond that is most polar is ________.
Q:
Ionic compounds consist of a single three-dimensional network of ions that are attracted to one another by strong ________ and usually exist in the solid state at room temperature, whereas covalent compounds consist of molecules that are attracted to one another by weak ________ and can exist in gaseous, liquid, or solid state at room temperature.
Q:
Among the compounds H3C-CH3, H2C=CH2, and HCCH, the compound with the strongest carbon-carbon bond is ________, and the compound with the longest carbon-carbon bond is ________.
Q:
How many lone pairs are on the Br atom in BrCl2-?
A) 0
B) 1
C) 2
D) 3
Q:
How many lone pairs of electrons are on the S atom in SF4?
A) 0
B) 1
C) 2
D) 3
Q:
Which of the following contains an atom that does not obey the octet rule?
A) CsI
B) SnO2
C) ClF5
D) ClF
Q:
Which element can expand its valence shell to accommodate more than eight electrons?
A) N
B) O
C) Br
D) He
Q:
How many lone pairs of electrons are on the As atom in AsCl3?
A) 0
B) 1
C) 2
D) 3
Q:
The name for the diatomic binary compound formed from fluorine and bromine is
A) bromine monofluoride
B) fluorine monobromide
C) monobromine monofluoride
D) monofluorine monobromide
Q:
The iodine atom in I2 would be expected to have aA) charge of 1-.B) partial charge -.C) partial charge +.D) charge of 0.
Q:
The compound ClF contains
A) ionic bonds.
B) nonpolar covalent bonds.
C) polar covalent bonds with partial negative charges on the F atoms.
D) polar covalent bonds with partial negative charges on the Cl atoms.
Q:
The electronegativity is 2.1 for H and 1.9 for Pb. Based on these electronegativities PbH4 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) Sr
B) I
C) Ba
D) At
Q:
Of the following elements, which has the highest electronegativity?
A) S
B) Cl
C) Ti
D) Se
Q:
Which of the following is not considered to be a free radical?A) B) NC) D) NO
Q:
Electrostatic potential maps use color to portray the calculated electron distribution in a molecule. Atoms that are electron poor and carry a + charge are shown in blue. Atoms that are electron rich and carry a - charge are shown in red. Atoms with little or no charge are shown in green. The electrostatic potential map of CH3Li below should showA) C blue and Li red.B) C blue and Li green.C) C green and Li blue.D) C red and Li blue.
Q:
Electrostatic potential maps use color to portray the calculated electron distribution in a molecule. Atoms that are electron poor and carry a + charge are shown in blue. Atoms that are electron rich and carry a - charge are shown in red. Atoms with little or no charge are shown in green. The electrostatic potential map of CH3Cl below should showA) C blue and Cl red.B) C blue and Cl green.C) C green and Cl blue.D) C red and Cl blue.
Q:
Electrostatic potential maps use color to portray the calculated electron distribution in a molecule. Atoms that are electron poor and carry a + charge are shown in blue. Atoms that are electron rich and carry a - charge are shown in red. Atoms with little or no charge are shown in green. The electrostatic potential map of H2O below should showA) H blue and O red.B) H blue and O green.C) H green and O blue.D) H red and O blue.
Q:
In order to complete an electron-dot structure of alanine, the oxygen atom labeled O2 needs
A) 1 additional bond and 1 nonbonded pair of electrons.
B) 1 additional bond and 2 nonbonded pairs of electrons.
C) 1 nonbonded pair of electrons.
D) 2 nonbonded pairs of electrons.
Q:
In order to complete an electron-dot structure of alanine, the oxygen atom labeled O1 needs
A) 1 additional bond and 1 nonbonded pair of electrons.
B) 1 additional bond and 2 nonbonded pairs of electrons.
C) 1 nonbonded pair of electrons.
D) 2 nonbonded pairs of electrons.
Q:
The following ball-and-stick molecular model is a representation of the amino acid alanine (unshaded spheres = H). Only the connections between atoms are shown; multiple bonds and nonbonded electrons are not indicated.In order to complete an electron-dot structure of alanine, the nitrogen atom needsA) 1 additional bond and 1 nonbonded pair of electrons.B) 1 additional bond and 2 nonbonded pairs of electrons.C) 1 nonbonded pair of electrons.D) 2 nonbonded pairs of electrons.
Q:
How many double and single bonds are in the resonance form for SO2 in which the formal charges on each atom are zero?A) two single bonds and no double bondsB) one single bond and one double bondC) no single bonds and two double bondsD) Each of the above is possible.
Q:
Assign formal charges to all atoms in the following resonance form for HNO3. A) 0 for all atoms
B) +1 for N, -1 for oxygen (c), 0 for all other atoms
C) +1 for N and H, -1 for oxygen (a) and oxygen (c), 0 for oxygen (b)
D) +1 for H, -2 for each oxygen, +5 for N
Q:
Which electron dot structure for OCN- has a formal charge of -1 on the most electronegative atom?
A) [:= C =:] "
B) [: N C ":] "
C) [: " C O :] "
D) [:" O C :] "
Q:
Assign formal charges to each atom in the resonance form for SOCl2 given below. A) 0 for Cl, 0 for S, and 0 for O
B) 0 for Cl, +1 for S, and -1 for O
C) -1 for Cl, +4 for S, and -2 for O
D) -1 for Cl, -2 for S, and -2 for O
Q:
Assign formal charges to each atom in the resonance form for SOCl2 given below. A) 0 for Cl, 0 for S, and 0 for O
B) 0 for Cl, +1 for S, and -1 for O
C) -1 for Cl, +4 for S, and -2 for O
D) -1 for Cl, -2 for S, and -2 for O
Q:
Two resonance forms for SOCl2 are given below. Which is favored by the octet rule and which by formal charge considerations?
A) I is favored by the octet rule and by formal charge considerations.
B) I is favored by the octet rule and II by formal charge considerations.
C) II is favored by the octet rule and I by formal charge considerations.
D) II is favored by the octet rule and by formal charge considerations.
Q:
In the best Lewis structure for NO+, what is the formal charge on the N atom?
A) -1
B) 0
C) +1
D) +2
Q:
Based on formal charge considerations, the electron-dot structure of CO32" ion has
A) two resonance structures involving two single bonds and one double bond.
B) two resonance structures involving one single bond and two double bonds.
C) three resonance structures involving two single bonds and one double bond.
D) three resonance structures involving one single bond and two double bonds.
Q:
Which one of the following is expected to exhibit resonance?
A) NH4+
B) HCN
C) CO2
D) NO2-
Q:
Which of the following are allowed resonance forms of NCS-?
I [: N C ":]" and [:= C =:] "
II [: N C ":] " and [: N C =:] "
III [: N C " :] " and [:" C N :] "
A) only I
B) only II
C) only III
D) I and III
Q:
What is the approximate carbon-oxygen bond order in CO32-?
A) 1
B) 4/3
C) 5/3
D) 2
Q:
How many resonance structures are required in the electron-dot structure of CO32-?
A) two
B) three
C) four
D) five
Q:
NO2" is be expected to have
A) two single bonds.
B) one single and one double bond.
C) two double bonds.
D) two identical bonds intermediate between a single and a double bond.
Q:
How many lone pairs are on the Br atom in BrF2-?
A) 0
B) 1
C) 2
D) 3
Q:
Consider a molecule with the following connections: When a valid electron dot structure is written, how many double bonds will the molecule contain?
A) 0
B) 1
C) 2
D) 4
Q:
Draw the Lewis Dot structure for B. The number of electrons placed on the central atom is
A) 6
B) 7
C) 8
D) 4
Q:
Draw the Lewis Dot structure for . The number of hydrogen terminal atoms attached to the central atom is
A) 0
B) 1
C) 2
D) 3
Q:
Identify the fourth-row element X that forms the ion A) Ge
B) As
C) Se
D) Kr
Q:
How many electrons are in the valence shell of I in IF4-?
A) 8
B) 10
C) 12
D) 14
Q:
How many lone pairs of electrons are on the Xe atom in XeF6?
A) 0
B) 1
C) 2
D) 3
Q:
Which of the following contains an atom that does not obey the octet rule?
A) KBr
B) CO2
C) ClF3
D) ICl
Q:
Which element can accommodate more than eight electrons in its valence shell?
A) C
B) O
C) P
D) He
Q:
Elements that can accommodate more than eight electrons in their valence shell occur only in periodic table periods
A) 2 through 7.
B) 3 through 7.
C) 4 through 7.
D) 5 through 7.
Q:
Which molecule contains a triple bond?
A) F2
B) O3
C) HCN
D) H2CO
Q:
In the most acceptable electron-dot structure for carbonyl fluoride, COF2 the central atom is
A) C, which is singly-bonded to O.
B) C, which is doubly-bonded to O.
C) O, which is singly-bonded to C
D) O, which is doubly-bonded to C.
Q:
Which is the most acceptable electron dot structure for N2H2?
A) H """ H
B) H "=" H
C) H " N N " H
D) H "" H
Q:
How many lone pairs of electrons are on the P atom in PF3?
A) 0
B) 1
C) 2
D) 3
Q:
A coordinate covalent bond may be formed when
A) the central atom donates both electrons in forming a single bond
B) the central atom donates a pair of electrons and the terminal atom donates a pair of electrons to from a double bond.
C) a covalent bond has a bond order of 1.5.
D) a covalent bond has a bond order of 3.
Q:
The nitrogen-nitrogen bond in :NN: has a bond order of
A) 3
B) 1
C) 2
D) 6
Q:
A::A represents
A) a double bond.
B) a quadruple bond.
C) one lone pair of electrons.
D) two lone pairs of electrons.
Q:
The compound, NO2, is named
A) nitrate.
B) nitrite.
C) nitrogen dioxide.
D) nitrogen(IV) oxide.
Q:
The formula for dinitrogen trioxide is
A) N(OH)3.
B) (NO3)2.
C) N2O3.
D) N3O2.
Q:
Arrange the following in order of increasing ionic character: Al2S3, MgS, Na2S, P4S3, S8.
A) MgS, Na2S, Al2S3, P4S3, S8
B) Na2S, MgS, Al2S3, P4S3, S8
C) S8, P4S3, Al2S3, MgS, Na2S
D) S8, P4S3, Al2S3, Na2S, MgS
Q:
The electronegativities for the elements vary from 0.7 for cesium to 4.0 for fluorine. The electronegativity for iodine is 2.5. Based entirely on the general guidelines for electronegativities and bond character,A) binary compounds with iodine should all be polar covalent with a - on I.B) binary compounds with iodine should all be polar covalent with a + on I.C) compounds with iodine may be ionic, polar covalent, or nonpolar covalent.D) no binary compounds with iodine should be substantially ionic.
Q:
Based on the indicated electronegativities, arrange the following in order of increasing ionic character: CsBr, LaBr3, PBr3, MgBr2. A) CsBr, LaBr3, MgBr2, PBr3
B) CsBr, MgBr2, PBr3, LaBr3
C) PBr3, LaBr3, MgBr2, CsBr
D) PBr3, MgBr2, LaBr3, CsBr
Q:
Element A has an electronegativity of 0.8 and element B has an electronegativity of 3.0. Which statement best describes the bonding in A3B?A) The AB bond is largely covalent with a - on A.B) The AB bond is largely covalent with a + on A.C) The compound is largely ionic with A as the cation.D) The compound is largely ionic with A as the anion.
Q:
A chlorine atom in Cl2 should have aA) charge of 1-.B) partial charge -.C) partial charge +.D) charge of 0.
Q:
The phosphorus atom in PCl3 would be expected to have aA) partial positive (+) charge.B) partial negative (-) charge.C) 3+ charge.D) 3- charge.
Q:
The electronegativity for both sulfur and carbon is 2.5. Therefore the compound CS2 would be expected to
A) be ionic with C as the anion.
B) be ionic with C as the cation.
C) have nonpolar covalent bonds between C and S.
D) have polar covalent bonds between C and S.
Q:
Which molecule contains the most polar bonds?
A) CF4
B) CO2
C) CN"
D) CH4
Q:
The greater the electronegativity difference between two bonded atoms, the
A) greater the bond order.
B) greater the covalent character of the bond.
C) greater the ionic character of the bond.
D) more unstable the bond.