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56 Cards in this Set
- Front
- Back
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Which of the following does not have eight valence electrons?
A) Ca+ B) BrC) Rb+ D) Xe E) All of the above have eight valence electrons. |
A
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The chloride of which of the following metals should have the greatest lattice energy?
A) cesium B) potassium C) rubidium D) sodium E) lithium |
E
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) In which of the molecules below is the carbon-carbon distance the shortest?
A) H2C=C=CH2 B) H3C-CH3 C) H-C=C-H D) H3C-CH2-CH3 E) H2C=CH2 |
C
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Of the atoms below, ________ is the most electronegative.
A) Cl B) O C) F D) N E) B |
C
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Of the atoms below, ________ is the least electronegative.
A) Ca B) F C) Cl D) Rb E) Si |
D
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Of the molecules below, the bond in ________ is the most polar.
A) HI B) HCl C) HF D) HBr E) H2 |
C
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Of the bonds between the elements below, the bond between ________ is the least polar.
A) Na, S B) C, F C) P, S D) Na, Cl E) Si, Cl |
C
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The Lewis structure of N2H2 shows ________.
A) each hydrogen has one nonbonding electron pair B) a nitrogen-nitrogen triple bond C) each nitrogen has one nonbinding electron pair D) each nitrogen has two nonbinding electron pairs E) a nitrogen-nitrogen single bond |
C
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In the nitrite ion (NO2
-), ________. A) both bonds are double bonds B) one bond is a double bond and the other is a single bond C) both bonds are the same D) there are 20 valence electrons E) both bonds are single bonds |
C
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Resonance structures differ by ________.
A) number of atoms only B) placement of electrons only C) number of electrons only D) placement of atoms only E) number and placement of electrons |
B
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To convert from one resonance structure to another, ________.
A) electrons must be added B) electrons and atoms can both be moved C) neither electrons nor atoms can be moved D) only electrons can be moved E) only atoms can be moved |
D
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For resonance forms of a molecule or ion, ________.
A) all the resonance structures are observed in various proportions B) there cannot be more than two resonance structures for a given species C) one always corresponds to the observed structure D) the same atoms need not be bonded to each other in all resonance forms E) the observed structure is an average of the resonance forms |
E
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Of the following, ________ cannot accommodate more than an octet of electrons.
A) I B) P C) As D) O E) S |
D
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A valid Lewis structure of ________ cannot be drawn without violating the octet rule.
A) IF3 B) PF3 C) NF3 D) SO4 2- E) SbF3 |
A
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A valid Lewis structure of ________ cannot be drawn without violating the octet rule.
A) SeF4 B) PO4 3- C) NF3 D) SiF4 E) CF4 |
A
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The central atom in ________ does not violate the octet rule.
A) KrF2 B) CF4 C) SF4 D) XeF4 E) ICl4- |
B
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Bond enthalpy is ________.
A) unpredictable B) always negative C) always positive D) always zero E) sometimes positive, sometimes negative |
C
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Of the bonds CN, C=N, and CN, the CN bond is ________.
A) strongest/longest B) strongest/shortest C) weakest/shortest D) weakest/longest E) intermediate in both strength and length |
D
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As the number of covalent bonds between two atoms increases, the distance between the atoms
________ and the strength of the bond between them ________. A) decreases, increases B) decreases, decreases C) increases, increases D) increases, decreases E) is unpredictable |
A
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Of the possible bonds between carbon atoms (single, double, and triple), ________.
A) a double bond is longer than a triple bond B) a double bond is stronger than a triple bond C) a triple bond is longer than a single bond D) a single bond is stronger than a double bond E) a single bond is stronger than a triple bond |
A
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The molecular geometry of ________ is square planar.
A) CCl4 B) XeF4 C) XeF2 D) ICl3 E) PH3 |
B
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The basis of the VSEPR model of molecular bonding is ________.
A) atomic orbitals of the bonding atoms must overlap for a bond to form B) hybrid orbitals will form as necessary to, as closely as possible, achieve spherical symmetry C) regions of electron density on an atom will organise themselves so as to maximise s-character D) regions of electron density in the valence shell of an atom will arrange themselves so as to maximise overlap E) electron domains in the valence shell of an atom will arrange themselves so as to minimise repulsionsE |
E
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The electron-domain geometry of ________ is tetrahedral.
A) XeF4 B) PH3 C) CBr4 D) CCl2Br2 E) All of the above except XeF4B |
D
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Of the following species, ________ will have bond angles of 120°.
A) ClF3 B) BCl3 C) NCl3 D) PH3 E) All of these will have bond angles of 120°. |
A
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An electron domain consists of ________.
a) a nonbonding pair of electrons b) a single bond c) a multiple bond A) a only B) b only C) c only D) a, b, and c E) b and c |
D
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The electron-domain geometry and the molecular geometry of a molecule of the general formula
ABn are ________. A) sometimes the same B) always the same C) mirror images of one another D) never the same E) not related |
A
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The electron-domain geometry and the molecular geometry of a molecule of the general formula
ABn will always be the same if ________. A) n is less than four B) there are no lone pairs on the central atom C) n is greater than four D) the octet rule is obeyed E) there is more than one central atom |
B
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For molecules of the general formula ABn, n can be greater than four ________.
A) for any element A B) only when A is boron or beryllium C) only when A is Xe D) only when A is carbon E) only when A is an element from the third period or below the third period |
E
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Of the molecules below, only ________ is nonpolar.
A) NH3 B) CO2 C) TeCl2 D) H2O E) HCl |
B
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Of the molecules below, only ________ is polar.
A) CCl4 B) SiCl4 C) BF4 D) CH4 E) SeF4 |
E
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Three monosulfur fluorides are observed: SF2, SF4, and SF6. Of these, ________ is/are polar.
A) SF2 only B) SF2 and SF4 only C) SF4 only D) SF2, SF4, and SF6 E) SF6 only |
B
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Of the following molecules, only ________ is polar.
A) NCl3 B) Cl2 C) BCl3 D) CCl4 E) BeCl2 |
A
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Of the following, only ________ has sp2 hybridisation of the central atom.
A) CO3 2- B) I 3- C) PF5 D) ICl3 E) PH3 |
A
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Of the following, the central atom is sp3d2 hybridised only in ________.
A) PCl5 B) XeF4 C) BeF2 D) PH3 E) Br3- |
B
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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 B) atomic, hybrid C) hybrid, hybrid or atomic D) hybrid, hybrid E) hybrid or atomic, hybrid or atomic |
A
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A typical triple bond consists of ________.
A) three sigma bonds B) two sigma and one pi bond C) one sigma and two pi bonds D) three pi bonds E) three ionic bonds |
C
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The N to N bond in HNNH consists of ________.
A) one σ bond and one π bond B) two σ bonds and one π bond C) two σ bonds and two π bonds D) one σ bond and two π bonds E) one σ bond and no π bonds |
A
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Valence bond theory does not address the issue of ________.
A) excited states of molecules B) hybridisation C) multiple bonds D) molecular shape E) covalent bonding |
A
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Of the following, ________ is a greenhouse gas.
A) CH4 B) C2H4 C) Xe D) O2 E) Cl2 |
A
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Which of the following statements about gases is false?
A) Gases are highly compressible. B) Gases expand spontaneously to fill the container they are placed in. C) All gases are colourless and odourless at room temperature. D) Non-reacting gas mixtures are homogeneous. E) Distances between molecules of gas are very large compared to bond distances within molecules. |
C
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One significant difference between gases and liquids is that ________.
A) gases are always mixtures B) a gas assumes the volume of its container C) a gas may consist of both elements and compounds D) a gas is made up of molecules E) All of the above answers are correct. |
B
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Molecular compounds of low molecular weight tend to be gases at room temperature. Which of the
following is most likely not a gas at room temperature? A) LiCl B) H2 C) Cl2 D) HCl E) CH4 |
A
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Of the following, ________ is a correct statement of Boyle's law.
A) P V = constant B) V T = constant C) n P = constant D) V P = constant E) PV = constant |
E
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Of the following, only ________ is impossible for an ideal gas.
A) V1 V2 = T1 T2 = 0 B) V1 T1 = V2 T2 C) V1T1 = V2T2 D) V2 = T2 T1 V1 E) V1 V2 = T1 T2 |
C
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A 255 mL round-bottom flask is weighed and found to have a mass of 114.85 g. A few milliliters of
an easily vapourised liquid are added to the flask and the flask is immersed in a boiling water bath. All of the liquid vapourises at the boiling temperature of water, filling the flask with vapour. When all of the liquid has vapourised, the flask is removed from the bath, cooled, dried, and reweighed. The new mass of the flask and the condensed vapour is 115.23 g. Which of the following compounds could the liquid be? (Assume the ambient pressure is 1 bar.) A) C3H7OH B) C4H9OH C) C4H10 D) C2H5OH E) C2H6 |
D
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SO2 (5.00 g) and CO2 (5.00 g) were placed in a 750.0 mL container at 50.0°C. The partial pressure of
CO2 in the container was ________ kPa. A) 162 B) 687 C) 407 D) 19.4 E) 279 |
E
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The kinetic-molecular theory predicts that pressure rises as the temperature of a gas increases
because ________. A) the average kinetic energy of the gas molecules decreases B) the gas molecules collide less frequently with the wall C) the gas molecules collide more energetically with the wall D) the gas molecules collide more frequently with the wall E) both the gas molecules collide more frequently with the wall and the gas molecules collide more energetically with the wall |
E
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Which of the following is not part of the kinetic-molecular theory?
A) Attractive and repulsive forces between gas molecules are negligible. B) Gases consist of molecules in continuous, random motion. C) The volume occupied by all of the gas molecules in a container is negligible compared to the volume of the container. D) Collisions between gas molecules do not result in the loss of energy. E) Atoms are neither created nor destroyed by ordinary chemical reactions |
E
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An ideal gas differs from a real gas in that the molecules of an ideal gas ________.
A) have no attraction for one another B) have an average molecular mass C) have a molecular weight of zero D) have no kinetic energy E) have appreciable molecular volumes |
A
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A real gas will behave most like an ideal gas under conditions of ________.
A) high temperature and low pressure B) high temperature and high pressure C) STP D) low temperature and high pressure E) low temperature and low pressure |
A
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When gases are treated as real, via use of the van der Waals equation, the actual volume occupied
by gas molecules ________ the pressure exerted and the attractive forces between gas molecules ________ the pressure exerted, as compared to an ideal gas. A) increases, decreases B) does not affect, decreases C) does not affect, increases D) increases, increases E) decreases, increases |
A
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Which substance in the reaction below either appears or disappears the fastest?
4NH3 + 7O2 → 4NO3 + 6H2O A) NH3 B) O2 C) H2O D) NO2 E) The rates of appearance/disappearance are the same for all of these. |
B
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Of the following, all are valid units for a reaction rate except ________.
A) M/s B) mol/hr C) g/s D) mol/L hr E) mol/L |
E
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The rate law for a reaction is
rate = k [A][B]2 Which one of the following statements is false? A) k is the reaction rate constant B) If [B] is doubled, the reaction rate will increase by a factor of 4. C) The reaction is first order in A. D) The reaction is second order overall. E) The reaction is second order in B |
D
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The overall reactions and rate laws for several reactions are given below. Of these, only ________
could represent an elementary step. A) A + 2B → P rate = k[A]2 B) A + 2B → P rate = k[A][B] C) A + B + C → P rate = k[A][C] D) A + B → P rate = k[A][B] E) 2A → P rate = k[A] |
D
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Of the following, ________ will lower the activation energy for a reaction.
A) removing products as the reaction proceeds B) increasing the pressure C) raising the temperature of the reaction D) increasing the concentrations of reactants E) adding a catalyst for the reaction |
E
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