The Strongest Intermolecular Interactions Between Octane (C8h18) Molecules Arise From

Chemistry 1315

TrueVaporization is an endothermic process
TrueMore energy is required to break intermolecular attractions when water vaporizes compared to the energy required to break intermolecular attractions when ice melts
TrueBased on principles of the kinetic molecular theory, the gas least likely to become liquid below 0°C given CH4, C3H8, C4H10 would be CH4
TrueWhen water freezes, the energy released is an exothermic process
TrueThe larger the dipole, the larger the attractive force, the higher the boiling point
TrueIon dipole interactions are weaker when the distance between two species is larger
TrueIt takes more energy to break a covalent bond or an ionic bond than it does to melt a solid or evaporate a liquid
TrueThe strength of the intermolecular forces that exist between molecules of a pure substance will affect the physical properties of that substance
TrueAs the temperature of a gas increases, the kinetic energy increases
TrueChanges in pressure do not significantly affect the intermolecular attractive forces for solids.
TrueCCl4 has a greater polarizability than CH4
TrueLondon dispersion forces are the weakest of the intermolecular forces.
TrueThe viscosity of a liquid generally increases with decreasing temperature
TrueStrong intermolecular forces yield high surface tension for liquids
TrueFor most ionic substances, solubility in water increases with increasing temperature
TrueThe solubility of a gas in liquid is affected by pressure
TrueThe solubility of a gas in water decreases with increasing temperature
TrueWater is an effective solvent used to dissolve many polar compounds
TrueStrong electrolytes are solutes that consist predominately of ions once dissolved in water
TrueHighly soluble compounds are not necessarily strong electrolytes
TrueSolutions of weak electrolytes consist of both ions and molecules but with a greater proportion of molecules
TrueHNO3, H2SO4, NaOH, and Ca(OH)2 are strong electrolytes
TrueSubstances with poor solubility may be strong electrolytes
TrueMost molecular compounds are non-electrolytes.
TrueStrong electrolytes are solutes that form predominantly ions once dissolved in water.
TrueAs intermolecular forces increase, vapor pressure decreases
TrueSolid water is less dense than liquid water (above 4°C)
TrueIncreasing the pressure over a liquid will increase the boiling point
TrueThe covalent bonds between hydrogen atoms and the oxygen within a water molecule are much stronger than the intermolecular forces that exist between water molecules.
TrueLess energy is required to melt a substance than to evaporate the same substance.
TrueThe sigma bond between the two carbon atoms in C2H4 is stronger than the pi bond between the two carbon atoms
TrueThe triple bond between the carbon atoms in C2H2 is shorter than the single bond between the carbon atoms in C2H6.
TrueDouble bonds between carbon atoms are always shorter than single bonds between carbon atoms
TrueThe distance between the nuclei of the atoms in a bond within an organic called the bond length
TrueOn a phase diagram, the melting point is the same as the freezing point
TrueSaturated solutions are stable solutions that contain the maximum possible amount of dissolved solute
TrueA volatile liquid is one that easily evaporates
TrueVapor pressure decreases with increasing strength of intermolecular forces
TrueMolecules or atoms in molecular solids are held together via intermolecular forces
TrueMetallic solids have atoms at the lattice points of the unit cell
TrueA body centered unit cell contains the net equivalent of two atoms or molecules.
TrueIn face centered cubic, the packing in this lattice is more efficient that body centered cubic; if the atoms have radius r, then the length of the cube edges is square root of 8 x r; there are four atoms per unit cell in this type of packing; the packing efficiency in this lattice and hexagonal close packing are the same.
TrueGiven: CH3OCH3, CH3CH2OH, CH3CH2CH3; CH3CH2OH would have the highest surface tension.
TrueA liquid boils when the external pressure over a liquid equals the vapor pressure
TrueAs molecules are forced together due to increased pressure, intermolecular attractions become more significant.
TrueAn unsaturated is one that will allow for more solute to be dissolved into the solvent
TrueA saturated solution is one that is one that contains the maximum amount of solute that will dissolve at a specific temperature.
TrueAir is a solution
FalseChanges in pressure do not affect intermolecular attractive forces for gases
FalseHCl exhibits significant hydrogen bonding
FalseSublimation is an exothermic process
FalseIn separate 1.0L containers at the same temperature, H2O has a higher vapor pressure than Ne once a dynamic equilibrium has been established
FalseNon-polar benzene, C6H6 will dissolve CaF2 better than Br2
FalseMost molecular compounds are electrolytes
FalseStrong acids are weak electrolytes
FalseThe viscosity of a liquid increases with increasing temperature
FalseHe has a greater polarizability than CH4
FalseDipole-dipole is the weakest intermolecular force
FalseSurface tension decreases with increasing intermolecular forces
FalseCondensation is an exothermic process
FalseThe strength of a carbon-carbon double bond is exactly twice that of the strength of a carbon-carbon single bond
FalseLondon dispersion forces tend to decrease in strength with increasing molecular weight
FalseIonic solids have formula units in the center of the unit cell
FalseIn face centered cubic, the coordination number of the atoms in the lattice is 8
FalseSiO2 (molecular) exists in solid state
FalseMore energy is required for a substance to undergo a phase change from solid to liquid compared to phase change from liquid to gas because it is necessary to override more intermolecular attractions in the phase change from solid to liquid.
FalseThe stronger the intermolecular forces between molecules of a pure substance, the lower melting and boiling points.
FalseAs temperature decreases, kinetic energy decreases, therefore attractions between particles will decrease.
FalseA supersaturated solution is a stable solution.
FalseA solid can’t be a solvent
HeliumGiven H2O, CH4, CH3Br, CH3Cl, & He which molecule will have the highest vapor pressure when at the same temperature and volume?
H2OGiven H2S, HCl, NH3, CH4, H2O, which molecule will have the highest boiling point?
Ne, C2H6, HBr, NH3List in order of increasing boiling point: Ne, HBr, NH3, C2H6
H2OGiven CO2, CH4, Kr, HBr, H2O, which molecule will have the highest boiling point?
CI4Given CF4, CCl4, CBr4, CH4, CI4, which molecule will have the highest boiling point?
Molecular solidA crystalline solid that is soft, has a low melting point, doesn’t conduct heat or electricity well in solid, molten, or aqueous form. Examples: SO2, I2
CondensationA polymer made in polymerization rxn that produces small molecules (like water)
Unsaturated hydrocarbonA compound in which one or more carbons have double or triple bonds
ConformationConversion of one form of a molecule into another form by rotation about a C-C single bond occurs very rapidly at room temperature. These different forms are conformations.
8, 2Europium in body-centered cubic
– Coordination #= ?
– # atoms in 1 unit cell= ?
1Cesium chloride in primitive cubic
– # Cesium ions in 1 unit = ?
12, 4Gold in cubic close packed (face centered cubic lattice)
– Coordination #= ?
– # atoms in 1 unit cell= ?
8KCl in face centered cubic
– # K+ & Cl- ions in 1 unit cell= ?
6Hexagonal close packing
– # atoms surrounding atom in same plane= ?
8, 2Metal in body centered cubic
– Coordination #= ?
– # metal atoms in 1 unit cell= ?
4, 8Ionic crystal empirical form: XY2
– X occupies 8 corners & 6 faces
– # X ions in 1 unit cell= ?
– # Y ions in 1 unit cell= ?
1, 3Ionic crystal empirical form AX3 in simple cubic
– A ions are lattice points
– # of A ions in 1 unit cell= ?
– # of X ions in 1 unit cell= ?
4Chromium in face centered cubic
– # atoms per unit cell= ?
2Chromium in body centered cubic
– # atoms per unit cell= ?
Hydrogen bondinghe dissolution of water in octane (C8H18) is prevented mostly by:
SO2, Na2SO4What’s more soluble than benzene?
CO2, C2H6, Br2, CH4What’s less soluble than benzene?
YesShould C8H18 be soluble in CCl4
CCl4Given the choices: CH3CH2OH, NH3, NaCl, HBr, what should dissolve in benzene?
YesWill NiBr2+ AgNO3 precipitate?
NaI, CH2OWhat’s more soluble in water than benzene, given: Br2, NaI, CCl4, CH2O
SrCO3 (s)What is the precipitate of Sr(NO3)2 + Na2CO3?
Ag3PO4(s)What is the precipitate of 3Ag+(aq)+PO43-(aq)+3K+(aq)+3NO3-(aq)–>?
PbCO3What is the precipitate of Pb2+(aq)+ CO32-(aq)–>?
Lead(II)acetate plus sodium carbonate
SrCO3What is the precipitate of Sr(NO3)2(aq)+ Na2CO3(aq)–>?
BaSO4What is the precipitate of CuSO4(aq)+ BaCl2(aq)–>?
Hg2Cl2What is the precipitate of 2NaCl(aq)+Hg2(NO3)2(aq)–>?
AgIWhat is the precipitate of AgNO3(aq) + KI(aq)
Truemolecules have dipole-dipole interactions, hydrogen bonding, and dispersion forces
London dispersion forceWhat is the the intermolecular force responsible for the fact that CH4 has the lowest boiling point in the set CH4, SiH4, GeH4, and SnH4?
Dipole dipole forceThe strongest intermolecular interactions between hydrogen sulfide (H2S) molecules arise from?
A low vapor pressureWhat property indicates presence of strong intermolecular forces in a liquid?
London dispersion forceWhat is the intermolecular force responsible for SnH4 having the highest boiling point in comparison to CH4, SiH4, GeH4?
Dipole dipolehydrogen bromide, what’s the most important molecular force
Hydrogen bondingThe strongest intermolecular attractions between ethyl alcohol (CH3CH2OH) arise from?
Ion dipoleWhat is the strongest intermolecular forces given ion-induced, dipole induced, ion-dipole, dipole-dipole, and dispersion?
Weak electrolyteWhat is a mixture of molecules and ions, but with a greater portion of molecules? Examples: H2O, N2, CH3COOH (acetic acid), C2H6O (ethanol)
Strong electrolyteWhat is a mixture of molecules and ions, but with a greater portion of ions? Example: Strong base, strong acid, ions only, KOH.
NoIs argon an electrolyte?
YesAre these all electrolytes? (1) HCl (2) Rb2SO4 (3) KOH (4) NaCl (5) HBr
TrueIn trans-2-butene, Carbon #2 is sp2 hybridized
FalseIn trans-2-butene
– The molecule has two pi bonds
– There’s free rotation around every bond in the molecule
– 2-butyne is its structural isomer
AlkyneWhat is this? C2H4. Alkane, Alkene, or Alkyne?
AdditionWhat is the most characteristic reaction of an alkyne?
AdditionWhat is the most characteristic reaction of an alkene?
TruePH3: Dipole-dipole
True or False
TrueCH4: London dispersion force
True or False
TrueBr2: London dispersion force
True or False
TrueH2O2: Hydrogen bonding
True or False
TrueAu: Metal crystal
True or False
TrueNiO: Ionic crystal
True or False
TrueC: Covalent crystal
True or False
TrueH2O: Molecular crystal
True or False
TrueSO2: Dipole-dipole
True or False
TrueHe: London dispersion force
True or False
TrueCH3CH2-OH: Hydrogen bonding
True or False
TrueAsH3: Dipole-dipole
True or False
TrueC(diamond): Covalent network
True or False
TrueNaCl: Ionic network
True or False
TrueC(Graphite): Covalent network
True or False
TrueNa: Metallic
True or False
TrueC8H18 (octane): London dispersion force
True or False
FalseHI: Hydrogen bonding
True or False
FalseCS2: Dipole-dipole
True or False
FalseCH3F: Hydrogen bonding
True or False
FalseCO2: Dipole-dipole
Truen or False
FalseCH2F2: London dispersion force
True or False
FalseHF: Dipole-dipole
True or False
AldehydeWhat functional group is H2CO?
Carboxylic acidWhat functional group is CH3CO2H?
AlcoholWhat functional group is CH3CH2OH?
KetoneWhat functional group is CH3CCH2CH3?
sigma, sp3C-H bond of carbonyl carbon in an Aldehyde is a ______ bond and the carbon atom is ____hybridized
YesAre these structural isomers of 1-pentene?
(1) 2-penetene
(2) 2-methyl-2-butene
(3) Cyclopentane
(4) 3-methyl-butene
NoIs this a structural isomer of 1-pentene?
YesAre these cis or trans isomers?
(1) 1,2-dibromoethane (both?)
(2) 2-butene
(3) 3-hexene
(4) 1,2-dichloroethene
(5) 1,2-dichloro-1-pentene
(6) 2,3-dicholoro-2-hexene
2How many isomers of C2H2Cl2 are polar?
11How many structural isomers can be drawn for C5H10?
6How many isomers (stereo and constitutional) are possible, C4H8?
4How many constitutional isomers are possible for c4h9cl?
YesIs 2-chlorobutane chiral?
YesIs 2,3-dibromopentane chiral?
YesIs 1,3-dibromobutane chiral?
YesIs 1-bromo-2-chlorobutane chiral?
NoIs CH2Cl2 chiral?
NoIs HN(CH3)2 chiral?
NoIs 2-chloropropane chiral?
NoIs 3-chloropentane chiral?
NoIs 1,4-dibromobutane chiral?
Water and an esterWhat does Carboxylic acid+ alcohol produce?
4many isomeric alcohols have molecular formula C4H10O?
Presence of two functional groupsWhat is a critical characteristic for the monomers that form condensation polymers?