Molar mass | Vapor pressure at 20 oC (mm Hg) | |
|---|---|---|
CBr4 | 331.6 | 0.8 |
CCl4 | 153.8 | 115.0 |
Based on the information in the table above, which of the following best explains why CCl4 has a higher vapor pressure that CBr4?
CCl4 has stronger dipole-dipole forces that CBr4.
CCl4 has weaker dipole-dipole forces that CBr4.
CCl4 has stronger London dispersion forces that CBr4.
CCl4 has weaker London dispersion forces that CBr4.
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Which of the following best describes the solid represented in the diagram above?
It is a brittle, water soluble electrolyte with poor electrical and thermal conductivity as a solid.
It has a low melting point and high electrical and thermal conductivity as a solid.
It is malleable and has poor electrical and thermal conductivity as a solid.
It is soft and has high electrical and thermal conductivity as a solid.
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Which of the following statements about silicon dioxide is correct?
I. Silicon dioxide is a covalent network solid
II. Each silicon atom is covalently bonded to four oxygen atoms
III. Silicon dioxide is a good electrical conductor
I and II only
I and III only
II and III only
I, II and III
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Which of the following could be the identity of a solid that exhibits the following properties?
It melts at 996 oC.
It does not conduct electricity as a solid.
It conducts electricity when dissolved in water.
MgBr2 (s)
C12H22O11 (s)
SiC (s)
Cu (s)
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Which of the following metals would have the highest melting point?
Na
Mg
Al
K
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Which of the following statements about diamond and graphite is correct?
The carbon atoms are joined together by three covalent bonds.
They both conduct electricity due to delocalized electrons in their structure.
The differences in their properties can be explained by their different structural arrangements.
They both have high melting points due to their strong intermolecular forces.
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Different substances have characteristic melting and boiling points, depending on the strength of the bonds or forces holding them together.
Which explains why methane has a lower melting point than sodium chloride?
Covalent bonds are weaker than ionic bonds.
Intermolecular forces are weaker than ionic bonds.
Covalent bonds are stronger than ionic bonds.
Intermolecular forces are stronger than ionic bonds.
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Which of the following best explains why liquids have a definite volume but no definite shape?
The particles in a liquid are in fixed positions and can only vibrate.
The particles in a liquid are loosely packed and can move past each other, but are still close together.
The particles in a liquid are spread out and move freely in all directions.
The particles in a liquid are tightly packed and cannot move.
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Which of the following statements explains why gases are highly compressible compared to solids and liquids?
Gases are composed of particles that are in constant random motion, which prevents them from having a fixed shape.
The particles in a gas have very little intermolecular force, allowing them to move freely.
Gases are highly compressible because the particles are widely spaced, leaving large amounts of empty space between them.
The pressure of a gas is determined by the frequency and force with which particles strike the walls of their container.
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Which of the following best describes the difference between crystalline and amorphous solids?
Crystalline solids are composed of molecules in fixed positions, while amorphous solids allow molecules to flow freely.
Crystalline solids have an orderly, repeating atomic structure, while amorphous solids have a disordered, non-repeating structure.
Amorphous solids are more compressible than crystalline solids due to their disordered structure.
Crystalline solids are typically formed when liquids cool quickly, while amorphous solids are formed when liquids cool slowly.
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The structure of cellulose is shown above. Cellulose is a polymer that is insoluble in water, but it is made from water soluble glucose monomers.
Which of the following types of noncovalent interactions is most likely responsible for the structure and insolubility of cellulose in water?
Hydrogen bonding.
Electrostatic/Ionic interactions.
Hydrophobic interactions.
Van der Waals interactions.
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Which of the following factors is primarily responsible for the increase in melting points observed as you move down Group 7A from fluorine to astatine?
Atomic mass increases.
Intermolecular forces become stronger.
The size of the molecules decreases.
The atomic number decreases.
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