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Chemistry
Q:
According to valence-bond theory, what is the hybridization scheme of the sulfur atom in SF4?A) B) C) D) E)
Q:
What is the hybridization of I in IF4-?A) sp2B) spC) sp3dD) sp3d2E) sp3
Q:
What is the hybridization of Br in BrF3?
A) sp3
B) sp
C) sp3d2
D) sp2
E) sp3d
Q:
What is the hybridization of Se in SeF6?
A) sp3d
B) sp3d2
C) sp2
D) sp
E) sp3
Q:
Which of the following statements is incorrect regarding the water molecule?A) There are two lone pairs and two bonding pairs on the central atom.B) The molecule is polar.C) The hybridization of oxygen is sp3.D) The hybridization of hydrogen is sp.E) The molecular geometry is bent.
Q:
What hybrid orbitals of sulfur are involved in the bonding in sulfur trioxide?
A) sp2
B) sp2d
C) sp3
D) sp3d2
E) sp
Q:
How many sigma and pi bonds are in the molecule pictured below? A) thirteen sigma bonds and one pi bond
B) eleven sigma bonds and two pi bonds
C) thirteen sigma bonds and two pi bonds
D) eleven sigma bonds and five pi bonds
E) five sigma bonds and eleven pi bonds
Q:
When an atom in a molecule or ion is described as sp3d2hybridized, its molecular geometry is
A) octahedral.
B) trigonal bipyramidal.
C) linear.
D) tetrahedral.
E) trigonal planar.
Q:
Which one of the following statements provides the best evidence that all the carbon compounds listed below have tetrahedral molecular geometries instead of square planar molecular geometries?
A) Only one CH4compound is known and it is nonpolar.
B) Only one CH3F compound is known and it is polar.
C) Only one CH2F2compound is known and it is polar.
D) Only one CF4compound is known and it is nonpolar.
E) Only one CHF3compound is known and it is polar.
Q:
Which of the following molecules is nonpolar?
A) SF4
B) PF5
C) ClF3
D) PF3
E) CH2F2
Q:
Which of the following statements best describes N2O?
A) The molecular geometry is bent and the molecule is nonpolar.
B) The molecular geometry is linear and the molecule is nonpolar.
C) The molecular geometry is linear and the molecule is polar.
D) The molecular geometry is trigonal planar and the molecule is nonpolar.
E) The molecular geometry is bent and the molecule is polar.
Q:
Which of the following molecules is polar?
A) SF6
B) CCl4
C) BF3
D) NO2
E) CO2
Q:
Which of the following compounds is nonpolar?
A) H2S
B) XeF2
C) SO2
D) N2O
E) HCl
Q:
Which of the following molecules has a dipole moment?
A) SO2
B) CS2
C) ClCCCCCl
D) CCl4
E) HCCH
Q:
Which of the following molecules has a dipole moment?
A) PF5
B) FOOF
C) HCCH
D) F2CCF2
E) SF6
Q:
Which of the following molecules does not have a permanent dipole moment?
A) sulfur tetrafluoride, SF4
B) iodine trichloride, ICl3
C) nitrogen trifluoride, NF3
D) phosphorus pentafluoride, PF5
E) sulfur dioxide, SO2
Q:
Which of the following molecules has a permanent dipole moment?A) SF6B) CCl4C) NF3D) SiCl4E) BF3
Q:
Which of the following concerning molecular geometry and dipole moments is/are correct?
1) Only molecules with polar bonds may have a permanent dipole moment.
2) All molecules with polar bonds have a permanent dipole moment.
3) All square planar molecules are nonpolar.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 1, 2, and 3
Q:
Which molecule is polar?
A) C2H4
B) CS2
C) C6H6
D) SO2
E) CF4
Q:
Which of the following molecules is nonpolar?A) B) C) D) E)
Q:
For which molecule or ion does the nitrogen atom have the positive end of the dipole moment?A) NH4+B) CN-C) NOD) HCNE) N2
Q:
Which molecule or ion does not have a tetrahedral molecular geometry?A) ICl4-B) CCl4C) GeCl4D) BrO4-E) SiCl4
Q:
Which molecule or ion does not have a tetrahedral molecular geometry?A) BF4-B) NF4+C) GeF4D) XeF4E) BeF42-
Q:
Which molecule or ion does not have a tetrahedral molecular geometry?A) ClF4"B) SiF4C) NF4+D) CF4E) BF4"
Q:
What is the molecular geometry of the ICl4-ion?A) octahedralB) pentagonalC) tetrahedralD) rectangularE) square planar
Q:
In ClF3, the electron pairs are arranged about the chlorine atom in
A) a square plane.
B) a tetrahedron.
C) an octahedron.
D) a trigonal pyramid.
E) a trigonal bipyramid.
Q:
In the ICl4-ion, the electron pairs are arranged around the central iodine atom in the shape ofA) a tetrahedron.B) an octahedron.C) a square plane.D) a trigonal bipyramid.E) a trigonal pyramid.
Q:
In the I3-ion, how many electron groups surround the central atom?A) 5B) 3C) 6D) 4E) 2
Q:
In the ICI4-ion, how many electron groups surround the central iodine atom?A) 2B) 4C) 5D) 6E) 3
Q:
What is the HOH bond angle in water?
A) 90
B) slightly less than 109
C) 180
D) 120
E) 109
Q:
What is the HCC bond angle in ethylene, H2CCH2?
A) slightly less than 120
B) 90
C) 109
D) 120
E) 180
Q:
Which of the following characteristics does not apply to PF3?A) has three bondsB) contains polar bondsC) polar moleculeD) one lone pair of electrons on phosphorusE) trigonal planar
Q:
Which of the following statements correctly describes the reaction of BF3with NH3to form F3B"NH3?
A) Both nitrogen and boron change from trigonal planar to tetrahedral geometry during the reaction.
B) Boron changes from trigonal planar to tetrahedral geometry during the reaction.
C) There are no changes in the formal charge on any atom during the reaction.
D) Nitrogen changes from trigonal planar to tetrahedral geometry during the reaction.
E) There is no change in geometry around the nitrogen or boron atoms.
Q:
What is the molecular geometry of the bromate ion, BrO3-?A) square planarB) trigonal planarC) square pyramidalD) tetrahedralE) trigonal pyramidal
Q:
What is the molecular geometry around the nitrogen atom? A) trigonal pyramidal
B) bent
C) tetrahedral
D) see-saw or distorted tetrahedral
E) trigonal planar
Q:
What is the molecular geometry around carbon atom C1? A) tetrahedral
B) trigonal planar
C) linear
D) trigonal pyramidal
E) bent
Q:
Which of the following concerning the formation of ions is/are correct?
1) Compounds of +4 ions are rare because of the large amount of energy required to form a +4 ion.
2) Some main group metals may have more than one possible positive charge because of the different energies required to remove s versus p valence electrons.
3) The nonmetals closest to the noble gases (Group 6A and 7A) tend to form monatomic anions with noble gas configurations.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
Q:
Which of the following concerning the formation of ions is/are correct?
1) Elements with large electron affinities tend to form monoatomic anions.
2) No ionic compounds are found with positive ions having charges greater than the element group number.
3) Group 1A and 2A metals always have a positive charge equal to their group number in their ionic compounds.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
Q:
All of the following species have ground-state noble-gas electron configurations exceptA) Ge4+B) K+C) KrD) I-E) P3-
Q:
Which of the following is the Lewis dot structure for one formula unit of magnesium sulfide?A) B) C) D) E)
Q:
Which of the following is the Lewis dot structure for the bromide ion?A) B) C) D) E)
Q:
Which of the following is the Lewis dot structure for the rubidium ion?A) B) C) D) E)
Q:
Atoms of an element X have the ground-state electron configuration 1s22s22p63s23p4. What type of ion is X most likely to form?A) X6+B) X3-C) X4+D) X-E) X2-
Q:
Which of the following compounds would be expected to have the highest melting point?
A) NCl3
B) OCl2
C) MgCl2
D) LiCl
E) CCl4
Q:
Which of the following compounds would be expected to have the highest melting point?
A) CsF
B) LiCl
C) LiF
D) NaBr
E) CsI
Q:
Which of the following compounds would be expected to have the lowest melting point?
A) AlF3
B) RbF
C) NaF
D) MgF2
E) CaF2
Q:
Which of the following compounds has the most ionic bonding (has the highest percentage of ionic character)?
A) CaF2
B) LiI
C) OF2
D) CsF
E) LiF
Q:
Calculate the lattice energy for LiF(s) given the following: sublimation energy for Li(s)+166 kJ/molHºf for F(g)+77 kJ/molfirst ionization energy of Li(g)+520. kJ/molelectron affinity of F(g)-328 kJ/molenthalpy of formation of LiF(s)-617 kJ/molA) 1052 kJ/molB) 285 kJ/molC) -650. kJ/molD) 800. kJ/molE) none of these
Q:
Which of the following processes is not exothermic?A) B) C) D) E)
Q:
In the Born-Haber cycle for , which of the following processes corresponds to the electron affinity of F?A) B) C) D) E)
Q:
In the Born"Haber cycle for , which of the following processes corresponds to the enthalpy of formation of ?
A) B) C) D) E)
Q:
In the Born"Haber cycle for , which of the following processes corresponds to the first ionization energy of Na?
A) B) C) D) E)
Q:
Which of the following is a correct description of lattice energy?
A) The energy change that occurs when electrons are removed from a lattice.
B) The energy change that occurs when a gas condenses to a liquid.
C) The energy change that occurs when a liquid freezes.
D) The energy change that occurs when an ionic solid is separated into its ions in the gas phase.
E) The lattice energy of a substance is identical to the ionic bond energy determined from coulombs law.
Q:
Which of the following statements concerning lattice energy is false?
A) MgO has a larger lattice energy than NaF.
B) The lattice energy for a solid with 2+ and 2" ions should be two times that for a solid with 1+ and 1" ions.
C) MgO has a larger lattice energy than LiF.
D) Lattice energy is often defined as the change in energy that occurs when an ionic solid is separated into isolated ions in the gas phase.
E) All of these are true.
Q:
Which one of the following has an enthalpy change that is equal to the lattice energy of ?
A) B) C) D) E)
Q:
When the cations Na+, K+, Rb+, Cs+are combined with chloride ion in the gas phase to form ion pairs, which pair formation releases the greatest amount of energy?
A) KCl
B) All release the same amount of energy.
C) RbCl
D) NaCl
E) CsCl
Q:
Which of the following concerning Coulomb's law is/are correct?
1) The energy of an ionic bond is proportional to the size of the ion charges.
2) The energy of an ionic bond is inversely proportional to the distance between the charges.
3) The size of an ion is not important in determining the energy of an ionic bond.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1, 2, and 3
Q:
The following representation of an atom is called A) a Lewis dot structure.
B) an ion.
C) a structural formula.
D) an electrostatic potential map.
E) an ionic bond.
Q:
In which pair do both compounds exhibit predominantly ionic bonding?
A) RbCl and CaO
B) PCl5and HF
C) KI and O3
D) Na2SO3and BH3
E) NaF and H2O
Q:
Use the bond energies provided to complete the following statement.________ when all of the bonds in acetic acid (CH3COOH) are broken.Bond Energy (kJ/mol)C-H413C-O358O-H463C=O745C-C348C=C614A) 3153 kJ/mol of energy is consumedB) 3153 kJ/mol of energy is releasedC) 2805 kJ/mol of energy is releasedD) 2805 kJ/mol of energy is consumedE) 2766 kJ/mol of energy is consumed
Q:
Which of the following covalent molecules does nothave the proper Lewis dot formula?A) B) C) D) E)
Q:
Based on the following data, what is the bond energy of the C=C bond in 1,1-difluoroethylene, CF2CH2?CH4(g) → C(g) + 4H(g); Hº= 1656 kJCF4(g) → C(g) + 4F(g); Hº= 1756 kJCF2CH2(g) → 2C(g) + 2H(g) + 2F(g); Hº= 2317 kJA) 611 kJ/molB) 845 kJ/molC) 820 kJ/molD) 1706 kJ/molE) 1910 kJ/mol
Q:
Based on the following data, what is the Br-Br bond energy?H2(g) + Br2(g) → HBr(g); Hº= -36.44 kJ BondBond Energy (kJ/mol)H-H435H-Br362A) 399 kJ/molB) 216 kJ/molC) -216 kJ/molD) -289 kJ/molE) 289 kJ/mol
Q:
Using bond-energy data, what is Hº for the following reaction?CH3OH(g) + H2S(g) → CH3SH(g) + H2O(g) BondBond Energy (kJ/mol)C-H413C-O358O-H463C-S259S-H339A) -25 kJB) - 124 kJC) 25 kJD) -2763 kJE) 2738 kJ
Q:
Using bond-energy data, what is Hº for the following reaction?CH4(g) + 2Cl2(g) → CCl4(g) + 2H2(g) BondBond Energy (kJ/mol)C-H413H-H432Cl-Cl242C-Cl328A) -40 kJB) -150 kJC) 40 kJD) 1415 kJE) 150 kJ
Q:
Consider the reaction2HCl(g) → H2(g) + Cl2(g); Hº= 185 kJWhich of the following statements is false?A) The reaction is endothermic.B) HCl(g) has a negative enthalpy of formation.C) The products have more enthalpy than the reactants.D) The HCl bond is longer than either the H2bond or the Cl2bond.E) The bond order of each of the products is one.
Q:
Which of the following diatomic molecules has the greatest bond energy?
A) H2
B) HCl
C) Cl2
D) CO
E) HF
Q:
Which of the following diatomic species do you expect to have the longest bond length?A) O2+B) O22-C) O2D) O2-E) they are all identical
Q:
Which of the following species has the shortest bond distance?
A) F2
B) Cl2
C) Br2
D) I2
E) H2
Q:
Which of the following statements is true?
A) The triple bond in N2has a smaller bond order and a smaller bond length than the single bond in F2.
B) The triple bond in N2has a larger bond order and a smaller bond length than the single bond in F2.
C) The triple bond in N2has a smaller bond order and a larger bond length than the single bond in F2.
D) The triple bond in N2has a larger bond order and a larger bond length than the single bond in F2.
E) The triple bond in N2and the single bond in F2have the same bond order and the same bond length.
Q:
As the number of bonds between two carbon atoms increases, which of the following decrease(s)?
A) only the bond length
B) only the bond energy
C) only the number of electrons between the carbon atoms
D) all of these
E) none of these
Q:
Which Lewis dot formula for pyrophosphate, P2O74-, minimizes formal charge?A) B) C) D) E)
Q:
In the Lewis dot formula for the bromate ion (BrO3-) that minimizes formal charge, the central atom is surrounded byA) two bonding pairs and two lone pairs of electrons.B) four bonding pairs and one lone pair of electrons.C) three bonding pairs and no lone pairs of electrons.D) five bonding pairs and one lone pair of electrons.E) three bonding pairs and one lone pair of electrons.
Q:
In the Lewis dot formula that minimizes formal charge, how many bonds are there in the tetrathionate ion, S4O62- ?A) 7B) 9C) 15D) 11E) 13
Q:
What is the formal charge on the chlorine atom in the chlorate ion, ClO3-, in the Lewis dot formula that minimizes formal charge?A) -2B) +1C) 0D) -1E) +2
Q:
What is the correct Lewis dot formula for sulfuric acid, H2SO4, that minimizes formal charge?A) B) C) D) E)
Q:
In which of the following species is the octet rule violated by the central atom when the central atom has a formal charge of zero?
A) SOCl2
B) CCl4
C) H2S
D) PF3
E) N2F4
Q:
Which of the following statements is true concerning the Lewis formula that minimizes formal charge for H2SO4?A) The formal charge of S is +2, the formal charge of each O is 0, and the formal charge H is 0.B) The formal charge of S is +2, the formal charge of O is either 0 or -2, and the formal charge of H is +1.C) The formal charge of S is +2, the formal charge of O is either 0 or -2, and the formal charge of H is 0.D) The formal charge of S is +2, the formal charge of O is 0, and the formal charge of H is +1.E) The formal charge of S is 0, the formal charge of O is 0, and the formal charge of H is 0.
Q:
In the Lewis formula that minimizes formal charge, what is the formal charge on the sulfur atom in sulfur trioxide, SO3?A) +2B) +4C) +6D) -2E) 0
Q:
Which of the following is/are true concerning formal charge?
1) The formal charge of each individual atom in a molecule or ion is an actual atomic charge that can be experimentally determined.
2) The formal charge of each individual atom is always the same for each possible resonance form.
3) The sum of the formal charges of each atom in a molecule or ion equal the overall charge of the molecule or ion.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) none