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- 1. Multiple Choice
Ethane, C2H6, has the following bonding:
ionic
metallic
nonpolar covalent
polar covalent
- 2. Multiple Choice
Copper (II) nitride, Cu3N2, has the following bonding:
ionic
metallic
nonpolar covalent
polar covalent
- 3. Multiple Choice
Cesium chloride, CsCl(s) has the following bonding:
lattice of positive and negative ions held together by electrostatic forces
closely packed lattice with delocalized electrons throughout
strong single covalent bonds with weak intermolecular forces
strong multiple covalent bonds with weak intermolecular forces
- 4. Multiple Choice
Carbon dioxide, CO2, has the following bonding:
lattice of positive and negative ions held together by electrostatic forces
closely packed lattice with delocalized electrons throughout
strong single covalent bonds with weak intermolecular forces
strong multiple covalent bonds with weak intermolecular forces
- 5. Multiple Choice
Which of the following typically has the lowest melting point?
Metals
Covalent network solids
Ionic compounds
Covalent molecules
- 6. Multiple Choice
Which of the following probably has the highest solubility in water?
Metals
Covalent network solids
Ionic compounds
Covalent molecules
- 7. Multiple Choice
Which of the following probably has the highest solubility in hexane, C6H14?
Metals
Polar covalent molecules
Ionic compounds
Nonpolar covalent molecules
- 8. Multiple Choice
Of the following molecules, which is the most polar?
CO
CO2
O2
HF
F2
- 9. Multiple Choice
Which of the following has the lowest melting point?
Zn
SiO2
CaCl2
C2H6
- 10. Multiple Choice
Which of the following is most likely to be soluble in water?
NaF
C12H22O
Mn
Cl2
- 11. Multiple ChoiceIntermolecular force present in HCl?dipole dipoledispersionH-bondionic
- 12. Multiple ChoiceType of intermolecular force present in I2, Br2, and Cl2.dipole dipoleH-bonddispersionmetallic
- 13. Multiple ChoiceWhich of the following has the highest boiling point?H2NH3N2O2
- 14. Multiple ChoiceWhat information do we look for on the periodic table if we want to examine intermolecular forces?atomic massatomic numberelectronegativityionization
- 15. Multiple ChoiceWhat explains the very high melting and boiling point of waterStrong dipole-dipole bonds between water moleculesStrong hydrogen bonds between water moleculesDispersion forces which are present in all moleculesAsymmetrical shape of the polar bonds.
- 16. Multiple ChoiceWhich of these typically increases when intermolecular forces increase?Boiling PointMelting PointViscosityAll of these
- 17. Multiple ChoiceRank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attractiondipole-dipole>covalent bond>hydrogen bond>LondonLondon>dipole-diple>hydrogen bond>covalent bondcovalent bond>hydrogen bond>dipole-dipole>Londonhydrogen bond>dipole-dipole>London>covalent bond - 18. Multiple ChoiceWhat best explains the difference in melting points between Cl2 (-101.5) and F2 (-219)?Increased mass (polarizability) of chlorineIncreased electronegativity of fluorineIncreased number of electrons in chlorineDecrease metallic character of fluorine
- 19. Multiple ChoiceWhich of the following statements correctly explains why hydrogen bonding is such a strong intermolecular force?There is an attraction between a small, weakly electronegative hydrogen atom and a large, strongly electronegative atom of fluorine, nitrogen, or oxygenThere is an attraction between a small, highly electronegative hydrogen atom and a large, highly electronegative fluorine atomThere is an attraction between the hydrogen and oxygen atoms onlyThere is an attraction between the hydrogen and nitrogen atoms only
- 20. Multiple Choice
How many sigma bonds does this have?1234 - 21. Multiple ChoiceWhat is the hybridization on Nitrogen?spsp2sp3None of these
- 22. Multiple Choice
According to kinetic molecular theory, in which of the following gases will the root mean square speed of the molecules be the highest at 200ºC?
SF6
H2O
HCl
Cl2
None, the molecules of all gases have the same root mean square speed at any given temperature.
- 23. Multiple Choice
Consider a sample of helium gas in a container fitted with a piston, as pictured below. The piston is frictionless, but has a mass of 10.0 kg. How many of the following processes will cause the piston to move away from the base and decrease the pressure of the gas? Assume ideal behavior.
I. heating the helium
II. removing some of the helium from the container
III. turning the container on its side
IV. decreasing the pressure outside the container
0
1
2
3
4
- 24. Multiple ChoiceA sample of gas with a volume of 30.0 mL at 25.0oC is heated to 50.0oC. What is the new volume of the gas?60.0 mL15.0 mL27.5 mL32.5 mL
- 25. Multiple Choice
The density of an unknown gas is 2.00 grams per Liter at 3.00 atmosphere pressure and 127oC. What is the molar mass of this gas?
(254/3) R
188 R
(800/3) R
600 R
- 26. Multiple Choice
A gaseous mixture containing 7.0 moles of nitrogen, 2.5 moles of oxygen, and 0.5 moles of helium exerts a total pressure of 0.90 atmosphere. What is the partial pressure of the nitrogen?
0.13 atm
0.27 atm
0.63 atm
0.90 atm
- 27. Multiple Choice
Samples of F2 gas and Xe gas are mixed in a container of fixed volume. The initial partial pressure of the F2 gas is 8.0 atmospheres and that of the Xe gas is 1.7 atmospheres. When all of the Xe gas reacted, forming a solid compound, the pressure of the unreacted F2 gas was 4.6 atmospheres. The temperature remained constant. What is the formula of the compound?
XeF
XeF3
XeF4
XeF6
- 28. Multiple Choice
NH4NO3(s) → N2O(g) + 2 H2O(g)
A 0.03 mol sample of NH4NO3(s) is placed in a 1 L evacuated flask, which is then sealed and heated. The NH4NO3(s) decomposes completely according to the balanced equation above. The total pressure in the flask measured at 400 K is closest to which of the following? ( The value of the gas constant, R, is 0.082 L atm mol–1 K–1)
3 atm
1 atm
0.5 atm
0.1 atm
- 29. Multiple Choice
Which of the following is an assumption of the kinetic-molecular theory of gases?
Collisions between gas particles are inelastic.
Gases consist of closely spaced particles.
Gas particles move around in an orderly manner.
The temperature of a gas depends on the average kinetic energy of the gas particles.
- 30. Multiple Choice
1. Under which conditions does a real gas behave very much like an ideal gas?
high temperature and low pressure
high temperature and high pressure
low temperature and high pressure
low temperature and low pressure
- 31. Multiple Choice
1. Liquids are more ordered than gases because liquids have ?
Weaker Intermolecular Forces And Lower Mobility Of The Particles
stronger intermolecular forces and lower mobility of the particles.
weaker intermolecular forces and greater mobility of the particles
stronger intermolecular forces and greater mobility of the particles
- 32. Multiple ChoiceWater exists as a _____________ at 700 mmHg and 50 °C.solidliquidgassupercritical fluid
- 33. Multiple ChoiceWhat is true regarding CO2 for temperatures above 31 °C?It can never be liquified.It decomposes.It has a high pressure.It is a plasma.
- 34. Multiple ChoiceWhat is the normal melting point of this substance?150 °C100 °C-50 °C0 °C
- 35. Multiple Choice
Chromatography separates solutions on the basis of _____ while distillation separates solutions on the basis of ______.
IMFs; solubility
solubility; conductivity
IMFs; boiling point
boiling point; solubility
- 36. Multiple ChoiceYou have a 0.5 M MgSO4 stock solution available. Calculate the volume of the stock solution needed to make 2.0 L of 0.20 M MgSO4.0.8 L5 L0.1 L0.5 L
- 37. Multiple ChoiceWhich of the following solutions made from one mole of the following solutes in 100.0 mls of water has the lowest freezing point?MgBr2Al2(CO3)3NH4C2H3O2N2O4
- 38. Multiple Choice
A dissolved solute that does not form ions is
a nonelectroyte
a weak electrolyte
a strong electrolyte
insoluble
- 39. Multiple Choice
Which does not affect the rate at which a solid solute dissolves?
the vapor pressure of the solvent
the temperature of the solvent
the surface area of the solid
the speed at which the solution is stirred
- 40. Multiple Choice
Which of the following occurs as temperature increases?
solubility decreases
solubility increases
solubility remains the same
molarity doubles
- 41. Multiple ChoiceA student extracts the colour from some green smarties and uses paper chromatography to separate components colours. She finds blue has a Rf =0.38 and yellow Rf =0.75 this suggeststhe yellow is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.the yellow is more strongly adsorbed onto the stationary phase and is more soluble in the mobile phase.the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.the blue is more strongly adsorbed onto the stationary phase and is less solublein the mobile phase.
- 42. Multiple ChoiceA high Rf value indicates strongstrong affinity to the stationary phasestrong affinity to the mobile phaseno affinity to the stationary phaseno affinity to the stationary phase
- 43. Multiple ChoiceThe Rf value for the blue component is0.30.7103
- 44. Multiple ChoiceThe Rf value for the red component is0.30.7107
- 45. Multiple ChoiceA certain photon of light has a wavelength of 4.22x10-7nm. What is the frequency? (v=c/λ)7.11x1014 Hz7.11Hz1.41x10-15-1.41x1015
- 46. Multiple ChoiceSelect the correct order of waves on the EMSRadio, Micro, Infra, Visible, Ultra, X-ray, GammaGamma, X-ray, Ultra, Vis, Infra, Micro, RadioVis, Micro, Infra, Ultra, X-ray, Gamma, RadioMicro, Radio, Vis, Infra, Ultra, X-ray, Gamma
- 47. Multiple ChoiceAs the frequency of an electromagnetic wave increases, the amount of energy in that wave...increases.decreases.stays the same.
- 48. Multiple ChoiceWhat is the Energy of a blue light with the frequency of 6.91x1014Hz? (E=hv)4.56x1049J9.55x10-49J4.56x10-19J5.82x1019J
- Answer choicesTagsAnswer choicesTags