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Concept explainers
Interpretation:
The following observation has to be explained -
Concept introduction:
Intermolecular forces are the interactions between the molecules in a compound.
The physical state of a substance depends on the strength of the intermolecular forces present in the molecules of that substance.
Very strong intermolecular forces bind the molecules together tightly and form “solids”. The molecules are held together strongly in solids that they hardly move from their respective position.
Liquid molecules have relatively low strength of intermolecular forces between them. Thus they move freely and because of this liquids do “flow”.
Gaseous substances have weakest intermolecular forces between them. Usually intermolecular forces are considered negligible in case of gaseous compounds. Gaseous molecules exhibit very rapid and random movement.
The classification of intermolecular forces can be summarized as follows –
Figure 1
There are three types of intermolecular forces - London dispersion forces, dipole-dipole forces and hydrogen bonding. These forces are collectively known as Van der Waals forces.
London dispersion forces exist in non-polar covalent compounds.
Dipole-dipole forces present in polar covalent compounds.
Hydrogen bonding is formed in polar covalent compounds containing Hydrogen and other high electronegativity like Fluorine, Oxygen or Nitrogen. It is relatively the strongest one.
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Chapter 9 Solutions
Chemistry: An Atoms First Approach
- Define critical temperature and critical pressure. In terms of the kinetic molecular theory, why is it impossible for a substance to exist as a liquid above its critical temperature?arrow_forwardYou and a friend each synthesize a compound with the formula XeCI2F2. Your compound is a liquid and your friend's compound is a gas (at the same conditions of temperature and pressure). Explain how the two compounds with the same formulas can exist in different phases at the same conditions of pressure and temperature.arrow_forwardPredict which liquid—glycerol, HOCH2CH(OH)CH2OH, or hexane, C6H14—has the greater surface tension. Explain your prediction.arrow_forward
- Which of the following do you expect to be molecular solids? a silicon tetrachloride, SiCl4 b lithium bromide, LiBr c sodium fluoride, NaF d bromine chloride, BrClarrow_forwardDiethyl ether (CH3CH2OCH2CH3) was one of the first chemicals used as an anesthetic. At 34.6C, diethyl ether has a vapor pressure of 760. torr, and at 17.9C, it has a vapor pressure of 400. torr. What is the H of vaporization for diethyl ether?arrow_forwardLiquid hexane (bp = 69°C) is placed in a closed container at room temperature. At first, the pressure of the vapor phase increases, but after a short time, it stops changing. Why?arrow_forward
- Air conditioners dry the air while they cool the air. Suppose an air conditioner is used to cool a room that is 6.88 m x 11.22 m × 2.26 m when the outside temperature is 37 °C. At this temperature, the vapor pressure of water is 47.1 torr. The partial pressure of water in the air is 84.5% of the vapor pressure of water. How much water, in grams, is removed from the air each time the air from the room is cycled through the air conditioner? mass of H,O:arrow_forwardWhat is the boiling point of water at an elevation of 1.15x10^4 ft? Use three significant figures.arrow_forwardThe molecular mass of butanol, C4H,OH, is 74.14; that of ethylene glycol, CH2(OH)CH,OH, is 62.08, yet their boiling points are 117.2 °C and 174 °C, respectively. Explain the reason for the difference. The two hydroxyl groups in ethylene glycol provide more locations for the formation of hydrogen bonds. The existence of more hydrogen bonds considerably decreases the boiling point O The two hydroxyl groups in ethylene glycol provide less locations for the formation of hydrogen bonds. The existence of less hydrogen bonds considerably increases the boiling point The two hydroxyl groups in ethylene glycol provide more locations for the formation of hydrogen bonds. The existence of more hydrogen bonds considerably increases the boiling pointarrow_forward
- The vapor pressure of liquid octane, C3H18, is 100. mm Hg at 339 K. A sample of C3H18 is placed in a closed, evacuated 526 mL container at a temperature of 339 K. It is found that all of the C3H15 is in the vapor phase and that the pressure is 58.0 mm Hg. If the volume of the container is reduced to 363 mL at constant temperature, which of the following statements are correct? Choose all that apply. O Some of the vapor initially present will condense. OLiquid octane will be present. O No condensation will occur. O The pressure in the container will be 100. mm Hg. O Only octane vapor will be present.arrow_forwardStudy the following phase diagram of Substance X. pressure (atm) 1.2- 0.6- 0. 0 solid liquid 200 gas 400 temperature (K) Use this diagram to answer the following questions. Suppose a small sample of pure X is held at 106. °C and 0.5 atm. What will be the state of the sample? Suppose the temperature is held constant at 106. °C but the pressure is decreased by 0.3 atm. What will happen to the sample? Suppose, on the other hand, the pressure is held constant at 0.5 atm but the temperature is decreased by 145. °C. What will happen to the sample? (choose one) (choose one) (choose one) î ↑ ↑arrow_forwardHow does intermolecular force of attraction in a substance relate to its phase?arrow_forward
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