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Chemistry
Q:
Which of the following statements concerning isomers is/are correct?
1/ Two types of stereoisomers exist: geometric isomers and optical isomers.
2/ Optical isomers are molecules with nonsuperimposable mirror images.
3/ Ethanol (CH3CH2OH) and dimethyl ether (CH3OCH3) are examples of geometric isomers.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
Which of the following statements concerning structural isomers is/are correct?
1/ Structural isomers have the same elemental composition, but the atoms are linked in different ways.
2/ Structural isomers have identical physical properties, but different chemical properties.
3/ Structural isomers have identical structures, but contain different isotopes of the same elements.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
Draw a Lewis structure of xenon trioxide. What is the hybridization of the xenon atom in this molecule?
Q:
The hybridization of the xenon atom in XeOF4 is ________.
Q:
Iodine trifluoride, IF3, has a trigonal-bipyramidal electron-pair geometry and a t-shaped molecular geometry. The hybridization of the central iodine atom is ________.
Q:
In molecular orbital theory, the bond order is defined as 1/2 (the number of electrons in ________ orbitals minus the number of electrons in antibonding orbitals).
Q:
In valence bond theory, each sigma bond in CH4 is formed from the overlap of a hydrogen atom's 1s orbital with a(n) ________ hybridized orbital on the carbon atom.
Q:
Which theory, valence bond or molecule orbital, correctly predicts the existence of paramagnetic molecules?
Q:
Benzene, C6H6, consists of a six member ring of sp2 hybridized carbon atoms. Each carbon atom has one unhybridized p orbital. How many p2p bonding, antibonding, and nonbonding molecular orbitals exist for benzene?
A.Three p2p molecular orbitals exist; two bonding and one antibonding.
B.Three p2p molecular orbitals exist; one bonding, one antibonding, and one nonbonding.
C.Six p2p molecular orbitals exist; three bonding and three antibonding.
D.Six p2p molecular orbitals exist; two bonding, two nonbonding, and two antibonding.
E.Twelve p2p molecular orbitals exist; six bonding and six antibonding.
Q:
In the NO2- ion, each atom can be viewed as sp2 hybridized. Thus, each atom has one remaining unhybridized p orbital. How many p2p molecular orbitals (including both bonding and antibonding orbitals) are formed using the unhybridized p orbitals?A.1B.3C.4D.6E.12
Q:
Which molecule will have the following valence molecular orbital energy level diagram?
s*2p
p*2p
s2p
p2p
s*2s
s2s
A.Be2
B.B2
C.C2
D.N2
E.O2
Q:
The following valence molecular orbital energy level diagram is appropriate for which one of the listed species?
s*2p
p*2p
s2p
p2p
s*2s
s2s
A.B22+
B.C22+
C.N22+
D.O22+
E.F22+
Q:
Which molecule will have the following valence molecular orbital level energy diagram?
s*2p
p*2p
s2p
p2p
s*2s
s2s
A.Li2
B.Be2
C.B2
D.C2
E.N2
Q:
Diagram 9-1The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.Energy ________ s*2p________ ________ p*2p________ s2p________ ________ p2p________ s*2s________ s2s________ s*1s________ s1sRefer to Diagram 9-1. Assuming that the molecular orbital energy diagram for a homonuclear diatomic molecule applies to a heteronuclear diatomic molecule, determine which of the following species is paramagnetic.A.NO+B.COC.CN-D.OF-E.NO
Q:
Diagram 9-1The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.Energy ________ s*2p________ ________ p*2p________ s2p________ ________ p2p________ s*2s________ s2s________ s*1s________ s1sRefer to Diagram 9-1. Assuming that the molecular orbital energy diagram for a homonuclear diatomic molecule applies to a heteronuclear diatomic molecule, determine which of the following species has the highest bond order.A.NO-B.OF-C.C2D.O22-E.NO+
Q:
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.
Energy ________ s*2p ________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. Assume that the molecular orbital energy diagram for a homonuclear diatomic molecule applies to a heteronuclear diatomic molecule. What is the molecular orbital configuration of CO?
A.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2
B.[core electrons] (s2s)2 (s*2s)2 (p2p)2 (s2p)2 (p*2p)2
C.[core electrons] (s2s)2 (s*2s)2 (p2p)2 (s2p)4
D.[core electrons] (s2s)2 (s*2s)2 (p2p)6
E.[core electrons] (s2s)2 (s*2s)2 (p2p)3 (s2p)3
Q:
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.
Energy ________ s*2p ________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. What is the molecular orbital configuration of N22+?
A.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2 (p*2p)2
B.[core electrons] (s2s)2 (s*2s)2 (p2p)4
C.[core electrons] (s2s)2 (s*2s)2 (p2p)2 (s2p)2
D.[core electrons] (s2s)4 (s*2s)4
E.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2 (p*2p)4
Q:
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.
Energy ________ s*2p ________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. What is the molecular orbital configuration of F2?
A.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2 (s*2p)2
B.[core electrons] (s2s)2 (s*2s)2 (p2p)2 (s2p)2 (p*2p)2
C.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (p*2p)4
D.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2 (p*2p)6
E.[core electrons] (s2s)2 (s*2s)2 (p2p)4 (s2p)2 (p*2p)4
Q:
Diagram 9-1The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.Energy ________ s*2p________ ________ p*2p________ s2p________ ________ p2p________ s*2s________ s2s________ s*1s________ s1sRefer to Diagram 9-1. Use molecular orbital theory to predict which ion is paramagnetic.A.F22+B.O22-C.O22+D.N22+E.B22-
Q:
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.
Energy ________ s*2p ________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. Use molecular orbital theory to predict which species is paramagnetic.
A.N2
B.B2
C.F2
D.Li2
E.H2
Q:
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.
Energy ________ s*2p ________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. Consider the molecules B2, C2, N2 and F2. Which two molecules have the same bond order?
A.B2 and C2
B.B2 and F2
C.C2 and N2
D.C2 and F2
E.N2 and F2
Q:
Diagram 9-1The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.Energy ________ s*2p________ ________ p*2p________ s2p________ ________ p2p________ s*2s________ s2s________ s*1s________ s1sRefer to Diagram 9-1. According to molecular orbital theory, which of the following lists ranks the fluorine species in terms of increasing bond order?A.F22+ < F22- < F2B.F22- < F2 < F22+C.F2 < F22+ < F22-D.F2 < F22- < F22+E.F22+ < F2 < F22-
Q:
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.
Energy ________ s*2p ________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. According to molecular orbital theory, what is the bond order of O2+?
A.1
B.3/2
C.2
D.5/2
E.3
Q:
Diagram 9-1The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.Energy ________ s*2p________ ________ p*2p________ s2p________ ________ p2p________ s*2s________ s2s________ s*1s________ s1sRefer to Diagram 9-1. According to molecular orbital theory, what is the bond order of oxygen, N22-?A.1B.3/2C.2D.5/2E.3
Q:
Diagram 9-1The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.Energy ________ s*2p________ ________ p*2p________ s2p________ ________ p2p________ s*2s________ s2s________ s*1s________ s1sRefer to Diagram 9-1. According to molecular orbital theory, which of the following species has the highest bond order?A.F2B.F22+C.C22-D.Li2E.B22+
Q:
Diagram 9-1The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.Energy ________ s*2p________ ________ p*2p________ s2p________ ________ p2p________ s*2s________ s2s________ s*1s________ s1sRefer to Diagram 9-1. According to molecular orbital theory, which of the following species is least likely to exist (i.e., has the lowest bond order)?A.H22-B.F22+C.C22-D.O22+E.B22-
Q:
Diagram 9-1The molecular orbital diagram below may be used for the following problem(s). For oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However, the diagram will still yield correct bond order and magnetic behavior for these molecules.Energy ________ s*2p________ ________ p*2p________ s2p________ ________ p2p________ s*2s________ s2s________ s*1s________ s1sRefer to Diagram 9-1. According to molecular orbital theory, which of the following species is the most likely to exist (i.e., which will have the greatest bond order)?A.H22+B.F22-C.N22-D.Be2E.O22+
Q:
A molecular orbital that decreases the electron density between two nuclei is said to be ____.
A.hybridized
B.bonding
C.antibonding
D.pi-bonding
E.nonpolar
Q:
Atomic orbitals combine most effectively to form molecular orbitals when
A.electrons in the orbitals have no spins.
B.electrons in the orbitals have the same spin.
C.the atoms have an equal number of valence electrons.
D.the atomic orbitals have similar energies.
E.only d-orbitals are used in bonding.
Q:
All of the following statements concerning molecular orbital (MO) theory are correct EXCEPT
A.the Pauli exclusion principle is obeyed.
B.Hund's rule is obeyed.
C.electrons are assigned to orbitals of successively higher energy.
D.a bonding molecular orbital is lower in energy than its parent atomic orbitals.
E.the combination of two atomic orbitals creates only one molecular orbital.
Q:
Which of the underlined atoms (C1, C2, N, and O) are sp2 hybridized? A.C1 and C2
B.C1, N, and O
C.N and O
D.O and C2
E.O only
Q:
For which of the following compounds is it possible for cis and trans isomers to exist? A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
Dichloromethane, CH2Cl2, is a common organic solvent. Which of the following statements concerning dichloromethane is/are CORRECT?
1/ CH2Cl2 has two isomers. For one isomer of CH2Cl2, the chlorine atoms are adjacent to each other and the molecule is polar.
2/ CH2Cl2 has two isomers. For one isomer of CH2Cl2, the chlorine atoms are on opposites sides of the carbon atom and the molecule is nonpolar.
3/ The hybridization of the central carbon atom is sp3.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
Which of the following characteristics apply to NCl3?
1/ polar bonds
2/ nonpolar molecule
3/ triangular-planar molecular shape
4/ sp2 hybridized
A.1 only
B.1 and 2
C.3 and 4
D.1, 2, and 3
E.1, 2, 3, and 4
Q:
Which of the following hybridized atoms is not possible?
A.an sp hybridized nitrogen atom
B.an sp2 hybridized oxygen atom
C.an sp3 hybridized boron atom
D.an sp3d hybridized phosphorus atom
E.an sp3d2 hybridized chlorine atom
Q:
Nitric acid, HNO3, dissociates in water to form nitrate ions and hydronium ions. What change in hybridization of the nitrogen atom occurs in this dissociation?
A.sp2 to sp3
B.sp2 to sp
C.sp3 to sp
D.sp to sp3
E.no change
Q:
Sulfur trioxide reacts with water to produce sulfuric acid. What change in hybridization of the sulfur atom occurs in this reaction?
A.sp3 to sp2
B.sp3 to sp
C.sp2 to sp3
D.sp2 to sp3d2
E.no change
Q:
Upon combustion, ethene (C2H4) is converted to carbon dioxide and water.What change in the hybridization of carbon occurs in this reaction?
A.sp to sp2
B.sp2 to sp3
C.sp3 to sp
D.sp2 to sp
E.sp3 to sp2
Q:
What is the hybridization of a central atom that has four sigma bonds and has no lone pairs of electrons?
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
Q:
What is the molecular geometry around a central atom that is sp3d hybridized and has one lone pair of eletrons?
A.trigonal bipyramidal
B.trigonal-pyramidal
C.see-saw
D.tetrahedral
E.square-planar
Q:
What is the molecular geometry around a central atom that is sp2 hybridized, has three sigma bonds, and one pi bond?
A.trigonal-planar
B.trigonal-pyramidal
C.bent
D.T-shaped
E.tetrahedral
Q:
What is the molecular geometry around a central atom that is sp3d2 hybridized and has two lone pairs of electrons?
A.tetrahedral
B.trigonal-bipyramidal
C.square-planar
D.square-pyramidal
E.see-saw
Q:
What is the molecular geometry around a central atom that is sp3 hybridized and has one lone pair of electrons?
A.bent
B.linear
C.trigonal-planar
D.trigonal-pyramidal
E.trigonal-bipyramidal
Q:
For which of the following molecules or ions does the central atom have sp hybridization: N3-, O3, and I3-?A.N3- onlyB.O3 onlyC.I3- onlyD.O3 and I3-E.I3- and N3-
Q:
For which of the following molecules and ions does the central atom have sp2 hybridization? (The central atom is listed first in each formula below.)A.SO42-B.CO2C.NOBrD.SBr2E.N2O
Q:
For which of the following molecules does the carbon atom have sp3 hybridization?
A.Cl2CO
B.CO
C.CS2
D.CH2Cl2
E.HCN
Q:
What is the hybridization of each carbon atom in benzene, C6H6? Benzene contains a six-member carbon ring.
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
Q:
What is the hybridization of the central atom in a molecule with a square-pyramid molecular geometry?
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
Q:
What is the hybridization of the sulfur atom in sulfur tetrafluoride, SF4?
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
Q:
What is the hybridization of the central sulfur atom in sulfur dioxide, SO2?
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
Q:
What is the hybridization of the central iodine atom in I3-?A.spB.sp2C.sp3D.sp3dE.sp3d2
Q:
What is the hybridization of the sulfur atom in SCl2?
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
Q:
What is the hybridization of the central nitrogen atom in N2O?
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
Q:
What is the maximum number of hybridized orbitals formed by an oxygen atom?
A.1
B.2
C.3
D.4
E.6
Q:
To form a molecule with an octahedral electron geometry, what set of pure atomic orbitals must be mixed?
A.one s and three p
B.one s, three p, and one d
C.one s, three p, and two d
D.two s, six p, and two d
E.two s, six p, and four d
Q:
How many sigma (s) bonds and pi (p) bonds are in the following molecule? A.seven s and three p
B.seven s and two p
C.five s and five p
D.five s and three p
E.five s and two p
Q:
How many sigma (s) bonds and pi (p) bonds are in carbon dioxide?
A.three s, zero p
B.two s, one p
C.two s, two p
D.one s, two p
E.zero s, three p
Q:
How many sigma (s) bonds and pi (p) bonds are in propene, CH2CHCH3?
A.six s, two p
B.seven s, one p
C.seven s, two p
D.eight s, zero p
E.eight s, one p
Q:
Which of the following statements concerning hybrid orbitals is/are CORRECT?
1/ The number of hybrid orbitals equals the number of atomic orbitals that are used to create the hybrids.
2/ When atomic orbitals are hybridized, the s orbital and at least one p orbital are always hybridized.
3/ To create tetrahedral structures, the s orbital and all three p orbitals must be hybridized..
A.1 only
B.2 only
C.3 only
D.2 and 3
E.1, 2, and 3
Q:
Which of the following statements is/are CORRECT according to valence bond theory?
1/ The overlap between an s orbital and a p orbital is called a pi-bond.
2/ The overlap of two s orbitals in H2 is called a sigma bond.
3/ HF is formed from the overlap of a hydrogen 1s orbital with a fluorine 2p orbital.
A.1 only
B.2 only
C.3 only
D.2 and 3
E.1, 2, and 3
Q:
Which of the following statements concerning valence bond (VB) theory is/are CORRECT?
1/ VB theory can describe molecular bonding in excited states.
2/ VB theory predicts that electrons are localized between pairs of atoms.
3/ VB theory correctly predicts the phase (g, , or s) of a molecule as a function of temperature.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
Which of the following statements concerning molecular orbital (MO) bond theory is/are CORRECT?
1/ MO theory can describe molecular bonding in excited states.
2/ MO theory accurately describes bonding in O2 and NO, VB theory does not.
3/ MO theory predicts that electrons are localized between pairs of atoms.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Q:
One might expect PCl3 to have a trigonal planar molecular geometry since its central atom is surrounded by three outer atoms. However, PCl3 has a trigonal pyramidal geometry. Explain.
Q:
In benzene, C6H6, the six carbon atoms are arranged in a ring. Two equivalent Lewis structures can be drawn for benzene. In both structures, the carbon atoms have a trigonal planar geometry. These two equivalent structures are referred to as ________ structures.
Q:
In PCl5, the Cl-P-Cl bond angle between an axial and an equatorial chlorine atom is ________ degrees.
Q:
If a molecule has a positive and negative end, the molecule is said to have a(n) ________ moment.
Q:
The molecular geometry of a molecule whose central atom has four single bonds and one lone pair of electrons is ________.
Q:
When heated, azomethane decomposes into nitrogen gas and ethane gas.CH3N=NCH3(g) N2(g) + C2H6(g)Bond Bond Enthalpy (kJ/molrxn) Bond Bond Enthalpy (kJ/molrxn)C-H 413 N-N 163C-N 305 N=N 418C-C 346 NN 945Using average bond energies, calculate the enthalpy of reaction.A.-611 kJB.-527 kJC.-429 kJD.-313 kJE.-263 kJ
Q:
Calculate the enthalpy change (DrH) for the decomposition of hydrogen peroxide,2 H2O2(g) 2 H2O(g) + O2(g)given the bond enthalpies of the reactants and products.Bond Bond Enthalpy(kJ/molrxn)H-H 436O-H 463O-O 146O=O 498A.-314 kJB.-206 kJC.-498 kJD.-255 kJE.+314 kJ
Q:
Calculate the enthalpy change (DrH) for the reaction below,N2(g) + 3 F2(g) 2 NF3(g)given the bond enthalpies of the reactants and products.Bond Bond Enthalpy(kJ/molrxn)N-N 163N=N 418NN 945F-F 155N-F 283A.-288 kJB.-1070 kJC.-637 kJD.+288 kJE.+293 kJ
Q:
Use Lewis structures to predict the bond order for a sulfur-oxygen bond in sulfur trioxide.A.1/2B.1C.4/3D.3/2E.2
Q:
Use Lewis structures to predict the bond order for a nitrogen-oxygen bond in nitrite ion, NO2-.A.1/2B.1C.4/3D.3/2E.2
Q:
In molecules, as bond order increases,A.both bond length and bond energy increase.B.both bond length and bond energy decrease.C.bond length increases and bond energy is unchanged.D.bond length is unchanged and bond energy increases.E.bond length decreases and bond energy increases.
Q:
Linus Pauling noticed that the energy of a polar bond is often greater than expected. He attributed the greater bond energy toA.a coulombic attraction between atoms with partially positive and negative charges.B.the greater bond lengths of the heteronuclear bonds.C.one of the many unexplainable phenomena that scientists encounter.D.the ability of heteronuclear species to form double and triple bonds.E.the greater number of valence electrons found in heteronuclear molecules.
Q:
Three possible structures of C2H2Cl2 are shown below. Which of these molecules are polar? A.1 only
B.2 only
C.3 only
D.1 and 3
E.2 and 3
Q:
Which one of the following molecules is polar?
A.CS2
B.SO2
C.XeF2
D.XeF4
E.SO3
Q:
Which one of the following molecules is polar?
A.CCl4
B.SF4
C.SO3
D.Br2
E.BCl3
Q:
Which of the following statements is/are correct?
1/ The atom with the greatest electronegativity is usually the central atom in a molecule.
2/ Electronegativity increases down each group of the periodic table.
3/ As the difference in electronegativity between two bonded atoms increases, the percent ionic character of the bond increases.
A.1 only
B.2 only
C.3 only
D.2 and 3
E.1, 2, and 3
Q:
Predict which of the following compounds has covalent bond(s) that are the most polar.A.HFB.I3-C.NOD.Cl2OE.HI
Q:
Choose which central atom in the following molecules is most electronegative.
A.PH3
B.CH4
C.H2S
D.H2O
E.NH3