List all of the intermolecular forces that will be present in the following compounds, assuming they are all liquids, and CAPITALIZE (ALL CAPS) the the most dominant force for each liquid.
The type of compound is indicated in brackets, and all numbers immediately following elemental symbols should be understood as subscripts. (a) CH3NH2 [polar]; (b) C10H22 [nonpolar]; (c) O2 [nonpolar]
CH3NH2:
dipole dipole interaction
HYDROGEN BONDING (between N of one molecule and H of other)
b) C10H22:
LONDON DISPERSION FORCE (INDUCED DIPOLE INTERACTION)
c)
O2:
DIPOLE DIPOLE INTERACTION.
List all of the intermolecular forces that will be present in the following compounds, assuming they...
h of the following statements is NOT true? London dispersion forces are present in all substances but are the only significant intermolecular forces in nonpolar substances. ) The density of the liquid state of a substance is greater than the density of its gaseous state. The thermal energy in a liquid allows the atoms within molecules to completely overcome the attractions between them so they flow. Most liquids can be converted to a gas by reducing pressure and/or heating. The...
10. (10 pts.) Identify the intermolecular forces present in the following compounds: Compound Intermolecular forces H- N- H H₃C CH₂ ç CC-C1 a. Which compound would you expect to have the higher boiling point? b. Justify your selection. C. Which compound would you expect to have the highest vapor pressure? d. Justify your selection.
Which of the following best describes London dispersion forces. Question 1 options: the intermolecular forces that exist when ions from an ionic compound are attracted to the dipole of polar molecules in a mixture. involves molecular orientations in which the positive end of one dipole is near the negative end of another forces that exist only between molecules that contain hydrogen atoms bonded to highly electronegative atoms such as O, N, F. Interactions between temporary dipoles cause atoms to be...
1. Check off (V) all the forces that apply to each of the following compounds Compound Intermolecular Force London Forces Hydrogen Bonding Dipole - Dipole BrF Cl2 H.S 2. In the liquid state, disruptive forces are a. roughly of the same magnitude as cohesive forces b. very weak compared to cohesive forces c. dominant over cohesive forces d. None of these 3. Between CIF and ClBr which compound would have a large boiling point? Explain the reason for your choice....
Rank the following compounds in order of increasing strength of intermolecular forces: CH3NH2, CH3CH3, CH3Cl A) CH3Cl < CH3CH3 CH3NH2 C) CH3NH2 CH3C CH3CH3 CH3Br, CH3l, CH3Cl D) CH3Cl CH3Br < CH3l E) CHalCH,CI CH,Br
15. Select all intermolecular forces experienced between
molecules in a pure sample of the following compound. Remember
these are line diagrams so hydrogen and carbon are not explicitly
indicated with H and C and hydrogen atoms are not indicated if on a
carbon atom. Also, lone electron pairs are not drawn either.
16. Select the dominant intermolecular force experienced between
molecules in a pure sample of the following compounds. Remember
these are line diagrams so hydrogen and carbon are not...
Intermolecular forces (IMPs) are the forces of attraction (or sometimes repulsion) that act between neighboring molecules All IMPs are based on etectrostatic interaction and are relatively weak compared to the Intramolecular forces that hold the atoms within a molecular together. In today, workshop you will practice to identify IMFs and predict their effect on boiling point melting point, vapor pressure and enthalpy of vaporisation (Delta Hvap). The Delta Hvap for a given molecule is the energy required to transform a...
What is the primary intermolecular force present in the following compounds? a. C3H8 b. HCN C. CF2H2 d. C2H4 e. CH3OH Based on the intermolecular forces reported for the compounds in problem 1, predict the order of increasing boiling point. For the compound with the highest boiling point, does that mean the vapor pressure will be high or low? Why?
For the following compounds and b.p. data, consider the intermolecular forces involved (and review the chapter on intermolecular forces in a first year chemistry textbook if necessary). methane (CH4) b.p. = -164 0C decane (C10H22) b.p. = 174 0C methanol (CH3OH) b.p. = 65 0C 1-decanol (C10H21OH) b.p. = 229 0C explain why the b.p. of methanol is nearly 230 0C higher than that of methane; explain why the b.p. of 1-decanol is 55 0C higher than that...
Determine the kinds of intermolecular forces that are present in each of the following elements or compounds. NI3 dispersion forces dipole-dipole forces hydrogen bonding dispersion forces and dipole-dipole forces