Which of the following compounds would be expected to have the HIGHEST boiling p

Question

Which of the following compounds would be expected to have the HIGHEST boiling point? CaF_2 KF CsF H_2O CF_4 Which bonding interaction best describes the intermolecular forces in AlH3? ionic bonding ion-dipole interactions dipole-dipole forces primarily hydrogen bonding metallic bonding Which of the following compounds would be expected to have the HIGHEST crystal lattice energy? Na_2O K_2O K_2O_2 KO_2 CaO See question 38 and 39 for explanation. Of the following, would be expected to have the HIGHEST melting point. NaF NaCl KBr Csl LiF The critical point of carbon tetrachloride is 283 degree C and 45 atm pressure. Liquid carbon tetrachloride has a vapor pressure of 10.0 atm at 178 degree C Which of the following statements must be true? The normal boiling point of CCl_4 must be greater than 178 degree C. Liquid CCl_4 can exist at temperatures greater than 283 degree C if the pressure is greater than 45 atm. triple point must be less than 178 degree C. Liquid and solid can only be in equilibrium at one temperature-the freezing point Vapor and liquid can only be in equilibrium at one temperature-the normal boiling

Explanation / Answer

40) In the given compounds CaF2 has the highest boiling point.

Reason

->It is the most ionic in the all compounds and ionic character increase the boiling point.

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