Accounting
Anthropology
Archaeology
Art History
Banking
Biology & Life Science
Business
Business Communication
Business Development
Business Ethics
Business Law
Chemistry
Communication
Computer Science
Counseling
Criminal Law
Curriculum & Instruction
Design
Earth Science
Economic
Education
Engineering
Finance
History & Theory
Humanities
Human Resource
International Business
Investments & Securities
Journalism
Law
Management
Marketing
Medicine
Medicine & Health Science
Nursing
Philosophy
Physic
Psychology
Real Estate
Science
Social Science
Sociology
Special Education
Speech
Visual Arts
Chemistry
Q:
How many lone pairs of electrons are on the P atom in PF3?
A) 0
B) 1
C) 2
D) 3
Q:
How many of the σ bonds in H2SO4 are coordinate covalent bonds?
A) 0
B) 2
C) 4
D) 6
Q:
The nitrogen-nitrogen bond in :NN: 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:
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) CF4B) CO2C) 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.
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:
Which compound is most likely to exist as a gas at room temperature?
A) Al4C3
B) CF4
C) CaF2
D) WC
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 has the weakest bonds?
A) CF4
B) CCl4
C) CBr4
D) CI4
Q:
Which molecule contains the most easily broken carbon-carbon bond?A) H3C-CH3B) H2C=CH2C) F2C=CF2D) HC CH
Q:
Which bond should have the highest bond dissociation energy?A) N NB) N NC) N ND) All three bonds should have about the same dissociation energy.
Q:
Which is the longest bond?A) N NB) N=NC) N ND) All three bond lengths should be about the same.
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:
Are the -bonds in CH3CO2- delocalized or localized?
Q:
Predict whether removing two electrons from F2 will create an ion that is diamagnetic or paramagnetic and have an F-F that is stronger or weaker than the bond in F2.
Q:
When an electron is added to the lowest unoccupied molecular orbital of N2, the electron is added to a(n) ________ (antibonding, bonding) molecular orbital and the N N bond order will ________ (decrease, increase).
Q:
According to molecular orbital theory, is the highest energy orbital that contains an electron antibonding or bonding in O22- ?
Q:
The hybrid orbital used by carbon to overlap with hydrogen in C2H2 is ________.
Q:
The carbon-carbon bond in C2H2 contains ________ and ________ bonds.
Q:
The hybrid orbital used by nitrogen to overlap with the 1s orbital of hydrogen in CH3NH2 is ________.
Q:
Of NH4+and NH4-the one with the smaller bond angles is ________.
Q:
Of BrF3 and PF3, the one with the smaller bond angles is ________.
Q:
Of XeF2 and XeF4, the one with the smaller bond angles is ________.
Q:
The molecular geometry of COCl2 is ________.
Q:
Based on formal charges, the PO bond order in POCl3 is expected to be ________.
Q:
Based on formal charges, the best Lewis electron-dot structure of BF3 has a B-F bond order equal to ________.
Q:
The number of Lewis electron dot resonance structures required to describe NO2- is ________.
Q:
Of H2CO and CO and CO2, the compound having the strongest CO bond 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:
Using only the elements Ba, F, and P, give the formula of a compound having largely polar covalent bonds.
Q:
Using only the elements Ba, Cl, and P, give the formula of a compound having largely ionic bonds.
Q:
Classify bonds in CaO as largely ionic, nonpolar covalent, or polar covalent.
Q:
Classify bonds in As4 as largely ionic, nonpolar covalent, or polar covalent.
Q:
Which compound is most likely to exist as a gas at room temperature?
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 HC CH, the compound with the strongest carbon-carbon bond is ________, and the compound with the longest carbon-carbon bond is ________.
Q:
The orbital hybridization on the carbon atom in C2H2 is
A) sp.
B) sp2.
C) sp3.
D) sp3d2.
Q:
The VSEPR model predicts the H O H bond angle in H3O+ to beA) 60.B) 90.C) less than 109.5 but greater than 90.D) 109.5.
Q:
What are the F Po F bond angles in PoF6 ?A) 60B) 90C) 109.5D) 120
Q:
What is the molecular geometry of TeCl4?
A) seesaw
B) square planar
C) square pyramidal
D) tetrahedral
Q:
Which of the following best describes Cl F2-? It has a molecular geometry that is
A) linear with no lone pairs on the Cl atom.
B) linear with lone pairs on the Cl atom.
C) nonlinear with no lone pairs on the Cl atom.
D) nonlinear with lone pairs on the Cl atom.
Q:
What is the molecular geometry of SF5-?
A) octahedral
B) seesaw
C) square pyramidal
D) trigonal bipyramidal
Q:
What is the O O bond angle in BO33-?A) less than 109.5B) 109.5C) 120D) greater than 120
Q:
What is the molecular geometry of N Cl3?
A) T-shaped
B) tetrahedral
C) trigonal planar
D) trigonal pyramidal
Q:
What is the molecular geometry of Cl F4-?
A) seesaw
B) square planar
C) square pyramidal
D) tetrahedral
Q:
What geometric arrangement of charge clouds is expected for an atom that has four charge clouds?
A) trigonal bipyramidal
B) octahedral
C) tetrahedral
D) square planar
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:
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 As Cl3?
A) 0
B) 1
C) 2
D) 3
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 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 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 drawing represents the molecular orbital containing the highest energy electrons in the O22- molecular ion in its the ground state?
A) B) C) D)
Q:
Which drawing represents the molecular orbital containing the highest energy electrons in the F2 molecule in its ground state?
A) B) C) D)
Q:
Which drawing represents the lowest energy unoccupied molecular orbital in the N2 molecule in its ground state?
A) B) C) D)