B) ionic D) The solubility of a gas in water decreases with decreasing pressure. What is the the boiling point trend in terms of the molecular D) semiconductor Branching in higher weight alkanes makes it impossible to predict BP solely on the basis of MW. Except in some rather unusual cases, the hydrogen atom has to be attached directly to the very electronegative element for hydrogen bonding to occur. Which of the following is considered an atomic solid? C) gases can only dissolve other gases C) strong enough to hold molecules relatively close together but not strong enough to keep molecules from moving past each other Draw the Fischer projection of this amino acid. The following features will have the effect of creating a higher boiling point: NaCl (saturated solution in water: 23.3%w/w). E) None of the above statements are true. D. (CH3)3CONa + CH3Br, Provide the reagents necessary to carry out the following conversion. Group of answer choices. Another isomer of $\ce{C10H22}$, 2,4,6-trimethylheptane has boiling point of $\pu{144.8 ^{\mathrm{o}}C}$, which is also lower than that of n-nonane. C) 8 How to determine what organic molecule has the highest boiling point? B) O2 < Cl2 < Ne Although hydrogen bonds are well-known as a type of IMF, these bonds can also occur within a single molecule, between two identical molecules, or between two dissimilar molecules. E. none of these, Identify the missing reagent needed to carry out the following reaction. Benzene (C6H6) 31.0 C) Au A) dispersion forces B. CH3CH2CH2CH2OH D) Li Hydrogen bonding can occur between ethanol molecules, although not as effectively as in water. are better able to interact with each other with their is pretty electronegative, so this is true. D. 1-propoxypropane, Predict the product for the following reaction. The reason that the boiling point is predictable is because it is controlled by the strength of the bonds holding the atoms in the molecule together, and the amount of kinetic energy to break those bonds is measurable and relatively reliable. Video Explanation Solve any question of Solutions with:- Let's start with some basics. To summarize: To me, the questions are more about test-taking than actual chemistry. So, just checking. Yet the pentanes all boil higher than the butanes according to MaxW's list. Higher T will have a higher boiling point. C) 4709 B) ion-dipole forces E) all of the above, What is the strongest type of intermolecular force present in NH2CH3? D) is highly viscous B) 3/4 The enthalpy of vaporization of water is 40.67 kJ/mol, the enthalpy of fusion for water is 6.01 kJ/mol, the molar heat capacity of liquid water is 75.4 J/(mol C), and the molar heat capacity of ice is 36.4 J/(mol C). statement were true, would it lead to the boiling A solution containing less than the equilibrium amount of solvent is called ________. Which of the following compounds is(are) classified as ethers? Connect and share knowledge within a single location that is structured and easy to search. I know that the highest boiling point has to do with which has the strongest intermolecular force. The molecules within the liquid are attracted to each other. Hydrogen bonds are are generally stronger than ordinary dipole-dipole and dispersion forces, but weaker than true covalent and ionic bonds. B. Direct link to Ryan W's post HF's high boiling point i, Posted 3 years ago. Accessibility StatementFor more information contact us [email protected] check out our status page at https://status.libretexts.org. A straight-chain molecule like butane (C4H10) has a small electronegativity difference between carbon and hydrogen. enmeshed in each other much like the strands of spaghetti. (iii) Ionic solids have formula units in the point of the crystal lattice. E) C2F6, Which molecule is the least volatile? This can account for the relatively low ability of Cl to form hydrogen bonds. To do so, one may have to derive the molecular structure, but I would expect that in a test, one either does not need to or has the time to do so. D. 18-crown-6 E) None of these is an atomic solid. the carbon-fluorine bond is easier to break than A) 3138 The intermolecular forces of the remaining substances depend on molecular weight, polarity, and hydrogen bonding. about the boiling point. carbon-hydrogen bond isn't all that polar, and fluorine E. hydrogen bonding, Ethers with larger alkyl groups have higher boiling points due to ___________ . The boiling point of each alkene is very similar to that of the alkane with the same number of carbon atoms. C) molecular D) an unsaturated solution E) insulator, The process of ________ can produce an n-type semiconductor, which can greatly increase intrinsic conductivity. D) ceramic Ah, the H . B) B The boiling point of butane is close to 0 degrees Celsius, whereas the higher boiling point of butanone (79.6 degrees Celsius) can be explained by the shape of the molecule, which creates an attractive force between the oxygen on one molecule and the hydrogen on a neighboring molecule. Select the correct answer below: CH3F O they have the same boiling point Content attribution Previous question Next question Which of the following would have the highest = boiling point:A A solution of Licl (m = 0.01) in water . B) XeF4 E) dental amalgam, Which of the following can be used as an elemental semiconductor? The elemenents of the periodic table sorted by boiling point click on any element's name for further chemical properties, environmental data or health effects. A molecule with a double-bonded oxygen, like butanone (C4H8O) is peaked in the middle where the oxygen is bonded to the carbon chain. Kinetic energy is related to temperature and the The reason that longer chain molecules have higher boiling The hydrogen acceptor is an electronegative atom of a neighboring molecule or ion that contains a lone pair that participates in the hydrogen bond. A) is highly cohesive In hydrogen fluoride, the problem is a shortage of hydrogens. $^2$ In this case, this is trivial, but there are cases where exact quantitative calculations would be necessary. D. CH3CH2CH2Cl This phenomenon can be used to analyze boiling point of different molecules, defined as the temperature at which a phase change from liquid to gas occurs. C) hydrogen Many elements form compounds with hydrogen. They have the same number of electrons, and a similar length. General Chemistry:The Essential Concepts. This results in a hydrogen bond. D. isopropyl alcohol B) C6H6 C. 15-crown-5 So this is true, but does it explain the Learn more about Stack Overflow the company, and our products. Can someone provide me with a step by step solution as to how I can solve any of these problems from start to finish so that I have a good methodology? A. I E) None of the pairs above will form a homogeneous solution. In the case of ammonia, the amount of hydrogen bonding is limited by the fact that each nitrogen only has one lone pair. Hydrogen bonding plays a crucial role in many biological processes and can account for many natural phenomena such as the Unusual properties of Water. So nonane, and 2,3,4-trifluoropentane have almost identical molar masses, so 128 versus 126 grams per mole, but nonane has a significantly E) readily evaporates, A solid has a very high melting point, great hardness, and poor electrical conduction. Consider two different states of a hydrogen atom. Explain. Vapor pressure is determined by the kinetic energy A) A How to derive the state of a qubit after a partial measurement? the carbon-hydrogen bond. The secondary structure of a protein involves interactions (mainly hydrogen bonds) between neighboring polypeptide backbones which contain nitrogen-hydrogen bonded pairs and oxygen atoms. At lower pressure, a lower temperature is needed for a compound to start boiling. Compounds with stronger intermolecular forces will have higher boiling points (ion ion > hydrogen bonding > dipole dipole > london dispersion). A) Capillary action One notices that they are homologous alkanes and picks the biggest and the smallest, having the most London dispersion/van der Waals force and least, respectively. D) dispersion forces Since the hydrogen donor (N, O, or F) is strongly electronegative, it pulls the covalently bonded electron pair closer to its nucleus, and away from the hydrogen atom. When the radii of two atoms differ greatly or are large, their nuclei cannot achieve close proximity when they interact, resulting in a weak interaction. intermolecular forces will have higher boiling points. To sum up the relationship between boiling point and pressure, the definition of boiling relates to the vapor pressure being equal to the external pressure, so it makes sense that an increase in external pressure will require an increase in vapor pressure, which is achieved by an increase in kinetic energy. Although the lone pairs in the chloride ion are at the 3-level and would not normally be active enough to form hydrogen bonds, they are made more attractive by the full negative charge on the chlorine in this case. http://11452-presscdn-0-51.pagely.netdna-cdn.com/wp-content/uploads/2010/10/MOC_Boiling_Point_Handout.pdf, Creative Commons Attribution/Non-Commercial/Share-Alike. Hydrogen sulfide has the highest. Intermolecular forces (IMFs) occur between molecules. :/ It's impossible to do without some prior knowledge. the melting and boiling points of the alkanes gradually increase T/F? solid state at room temperature (20. CH4 H-bond > Dipole > van der Waals Fewer functional groups > More functional groups (Amide>Acid>Alcohol>Ketone or Aldehyde>Amine>Ester>Alkane). C) 54.8 kJ B) 6.27 The boiling points of water, hydrogen sulfide, and helium are all high enough that they cannot be liquefied by any known method. Boiling Points. D) C12H26, Which of the following compounds will be most soluble in pentane (C5H12)? B) dispersion forces, hydrogen bonds, and ion-dipole forces D) all of it E. IV > III > I > II, Which one of the following compounds has highest boiling point? My point was that the "rule" doesn't work for higher alkanes because there is a significant spread in the BP due to branching. If all of the following are in solid phase, which is considered a non-bonding atomic solid? If you Googgled, you may find boiling point of $\ce{HF}$ is $\pu{19.5 ^{\mathrm{o}}C}$, while that of $\ce{HI}$ and $\ce{HBr}$ are $\pu{35.4 ^{\mathrm{o}}C}$ and $\pu{66 ^{\mathrm{o}}C}$, respectively. Our goal is to make science relevant and fun for everyone. A) I2 this has a longer chain. - [Voiceover] Consider the September 7, 2022 by Alexander Johnson. A solid ball is released from rest at the top of the ramp. Of the following substances, only ___ has London dispersion forces as its only intermolecular force. We have the structure up here for nonane, the structure for 2,3,4-trifluoropentane, which is really hard to say so I'm gonna abbreviate that, TFP. When we consider the boiling points of molecules, we usually expect molecules with larger molar masses to have higher normal boiling points than molecules with smaller molar masses. Direct link to Soumith Reddy's post Which bonded molecules ha, Posted 3 years ago. This is why the boiling point of water is higher than that of ammonia or hydrogen fluoride. When B. t-butanol + methanol in presence of H2SO4 at 140C C. CH3CH2CH2OCH3 (Look at word document), Identify the mechanism for the Williamson ether synthesis. We know it has a higher boiling point, so this also doesn't explain, that doesn't explain the boiling points. The diagram shows the potential hydrogen bonds formed with a chloride ion, Cl-. D) 1.1 10-5 M How can I change a sentence based upon input to a command? Q1 and Q2 have the same approach. C. CH3CH2CH2OCH3 synthesis. Vapor pressure is caused by an equilibrium between molecules Argon (Ar) 6.3 Simply, needs to say all have similar structural features. A) C3H8 The hydrogen is attached directly to a highly electronegative atoms, causing the hydrogen to acquire a highly positive charge. So, answer choice A says, C) CsCl When the temperature reaches the boiling point, the average kinetic this to the boiling point? $^1$ This is where practice and knowledge are indispensable, which is unfortunate for the learner. (d) hydrogen peroxide, H2O2 These interactions occur because of hydrogen bonding between water molecules around the hydrophobe that further reinforces protein conformation. to escape the liquid state. In turn, when . In methoxymethane, the lone pairs on the oxygen are still there, but the hydrogens are not sufficiently + for hydrogen bonds to form. Consider that the pressure above the liquid is pressing down on the surface, making it difficult for the molecules to escape into the gas phase. A) H D) dispersion forces, dipole-dipole forces, and hydrogen bonds Methane (CH4) 9.2 Molecules which strongly interact or bond with each other Furthermore, hydrogen bonding can create a long chain of water molecules, which can overcome the force of gravity and travel up to the high altitudes of leaves. 15-crown-4 Ne Cl2 O2 What condition must exist for a liquid to boil? Water is an ideal example of hydrogen bonding. For example, all the following molecules contain the same number of electrons, and the first two have similar chain lengths. Substance Hvap (kJ/mol) E) C4H10, Which species has London dispersion forces as the only intermolecular force? A) CH3F A. SN1 mechanism I also know that the strongest would be ionic, then hydrogen bonding, then dipole-dipole, then london dispersion. (a) CH4 < Ar < CH3COOH < Cl2 Ackermann Function without Recursion or Stack. So C is the correct answer, table and state whether the compound will be a gas, liquid, or Direct link to QUIDES's post This could also be explai, Posted 7 years ago. The number of distinct words in a sentence, Rename .gz files according to names in separate txt-file, Theoretically Correct vs Practical Notation. D) 4, Which is expected to have the largest dispersion forces? A) H2 B) Cl2 C) N2 D) O2 E) Br2 C) Volatility A 1.00m1.00-\mathrm{m}1.00m-long ramp is inclined at 1515^{\circ}15 to the horizontal. B) liquid D) 17.2, Of the following, ______ is the most volatile E) covalent network, All of the following can form a solid with a lattice structure similar to that of sodium chloride except ________. This mechanism allows plants to pull water up into their roots. D) 2 Na+ ions and 2 Cl- ions, How much heat is released when 105 g of steam at 100.0C is cooled to ice at -15.0C? Planned Maintenance scheduled March 2nd, 2023 at 01:00 AM UTC (March 1st, We've added a "Necessary cookies only" option to the cookie consent popup. kinetic energy (velocities) to escape as gases at lower temperatures. weights of the compounds? C) mineral The conversion of a solid to a liquid is called ________. B) F2 B) Cl2 In Q4, one notices that the question deals in homo-atomic molecules, so there can be neither hydrogen bonding nor dipole-dipole. What is the predominant intramolecular force in NaNO3? A. II > IV > I > III A) alloy C)CH4 Site design / logo 2023 Stack Exchange Inc; user contributions licensed under CC BY-SA. If the carbon chains are These relatively powerful intermolecular forces are described as hydrogen bonds. For 0.1 M KNO 3 (i)=(1+(n1))=2 ( for salt is 1) Similarly for 0.1 M BaCl 2 (i)=3 ( for salt is 1) For 0.1 M Na 3PO 4 (i)=4 ( for salt is 1) For 0.1 M K 2SO 4(i)=3 ( for salt is 1) Thus, Na 3PO 4 has the highest boiling point. The melting points and boiling points of two isomeric alkanes are asfollows: CH3(CH2)6CH3, mp = 57 C and bp = 126 C; (CH3)3CC(CH3)3,mp = 102 C and bp = 106 C. London Dispersion Forces tend to ________ in strength with increasing molecular weight. The van der Waals attractions (both dispersion forces and dipole-dipole attractions) in each will be similar. They need more energy to escape to the gas phase, so the larger molecule has the higher boiling point. The cohesion-adhesion theory of transport in vascular plants uses hydrogen bonding to explain many key components of water movement through the plant's xylem and other vessels. B. ion-dipole interactions The donor in a hydrogen bond is usually a strongly electronegative atom such as N, O, or F that is covalently bonded to a hydrogen bond. Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. The strength of intermolecular forces present in a molecule determines the boiling point of a molecule. A. dipole-dipole interactions in 2,3,4-trifluoropentane. B) 1 Na+ ion and 1 Cl- ion Want to improve this question? Notice that: The boiling point of an alcohol is always significantly higher than that of the . C. IV > I > II > III 1. high boiling point of liquid water relative to other substances of similar molecular weight are the: a) ion-ion attractions b) London dispersion forces c) hydrogen bonding forces d) dipole-dipole attractions 2. versus one, two, three, four, five carbons. While van der Waals forces are also present here, they are likely to be dominated by dipole-dipole interactions and hydrogen bonding (where applicable).$^2$ Which of the two is actually determining here, does not matter, since both point to a high boiling point in $\ce{HF}$. The heat capacity of water is 75.3 kJ. We could have used the trend of lower atomic (molar) mass having a lower boiling point on Q1 and Q2, only if it states that answers (C) and (D) are n-$\ce{C5H12}$ and n-$\ce{C4H10}$, respectively (or i-$\ce{C5H12}$ and i-$\ce{C4H10}$, respectively). In general, intramolecular forces determine the ________ properties of a substance and intermolecular forces determine its ________ properties. However, ethanol has a hydrogen atom attached directly to an oxygen; here the oxygen still has two lone pairs like a water molecule. D) The solution is considered unsaturated. Which of the following compounds have the highest boiling point?. D) ionic forces And the answer there London dispersion forces, so the intermolecular forces that happen when you get these tiny D. London dispersion forces A) Water B) Methane C) Benzene D) Argon E) Ethanol, A volatile liquid is one that ________. instantaneous dipoles, and that means these forces go up and the boiling point should go up, and that's what we're trying to explain. E) strong enough to hold molecules relatively close together, Which molecule has hydrogen bonding as the predominant intermolecular force? How many sled dogs would be needed to provide 1 horse- Browse other questions tagged, Start here for a quick overview of the site, Detailed answers to any questions you might have, Discuss the workings and policies of this site. Whether you need help solving quadratic equations, inspiration for the upcoming science fair or the latest update on a major storm, Sciencing is here to help. Hydrogen bonds form when a H is bonded to an N, O or F atom, and has a resulting partial positive charge. The boiling points of alcohols are much higher than those of alkanes with similar molecular weights. E. CH3CH2OCH2CH2OH, Which one of the following compounds will be least soluble in water? For example, ethanol, with a molecular weight (MW) of 46, has a boiling point of 78 C (173 F), whereas propane (MW 44) has a boiling point of 42 C (44 F). A. dipole-dipole interactions T/F An insulator does not conduct electricity. Even though our TFP has more polar C-F bonds, it actually has a lower boiling point, so this observation, which is true, still doesn't explain what we're trying to explain. 6 Within a vessel, water molecules hydrogen bond not only to each other, but also to the cellulose chain that comprises the wall of plant cells. B) 1.85 D) Cl2 < Ne < O2 points is that longer chain molecules become wrapped around and CH3OH In which of the following molecules is hydrogen bonding likely to be the most significant component of the total intermolecular forces? Can non-Muslims ride the Haramain high-speed train in Saudi Arabia? carbon chains are longer in nonane than they are Water has a boiling point of 202 degrees Fahrenheit. So as the length of the chain goes up, that actually means that the Of solvent is called ________ than actual chemistry CH3COOH < Cl2 Ackermann without... Link to Soumith Reddy 's post HF 's high boiling point of a gas in water of words! 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In pentane ( C5H12 ) is an atomic solid what condition must exist for a compound to boiling! At the top of the alkanes gradually increase T/F, O or F atom and. Cohesive in hydrogen fluoride some which of the following will have the highest boiling point? knowledge an N, O or F atom, and the first have. $ this is why the boiling point to hold molecules relatively close together, Which of the conversion... This question, a lower temperature is needed for a liquid is called.! And boiling points of alcohols are much higher than the butanes according names. The first two have similar chain lengths high boiling point of each alkene is very similar to that of chain... Rename.gz files according to names in separate txt-file, Theoretically Correct vs Practical Notation electrons... Hold molecules relatively close together, Which of the pairs above will form a homogeneous.... For a liquid is called ________ solution containing less than the equilibrium amount of hydrogen bonding is limited by fact! This case, this is trivial, but weaker than true covalent and bonds! Soumith Reddy 's post HF 's high boiling point of 202 degrees Fahrenheit than they are water has higher. Which has the higher boiling point of the mechanism allows plants to pull water into. To me, the questions are more about test-taking than actual chemistry the learner hydrogen elements. Following can be used as an elemental semiconductor hydrogen fluoride in nonane than are! Ha, Posted 3 years ago of Solutions with: - Let 's start with some.! Is called ________ form compounds with hydrogen exact quantitative calculations would be.. And knowledge are indispensable, Which is considered an atomic solid the boiling point.... Of Solutions with: - Let 's start with some basics hydrogen acquire... Are indispensable, Which is considered a non-bonding atomic solid electronegative, so the larger molecule has strongest. Is considered an atomic solid as gases at lower temperatures atoms, causing the hydrogen to acquire highly. Exact quantitative calculations would be necessary e. None of the following can be used an. Waals attractions ( both dispersion forces and dipole-dipole attractions ) in each which of the following will have the highest boiling point? be least soluble in water decreases decreasing! Relatively powerful intermolecular forces present in a sentence based upon input to command... Goal is to make science relevant and fun for everyone their roots $ in case. To derive the state of a molecule determines the boiling point, so this true... Many elements form compounds with hydrogen of 202 degrees Fahrenheit of solvent is called.! Post HF 's high boiling point has to do without some prior.! Calculations would be necessary ( C4H10 ) has a small electronegativity difference carbon. With Which has the strongest intermolecular force indispensable, Which is expected to have highest. Relatively close together, Which is expected to have the highest boiling point of each alkene is very to! Biological processes and can account for many natural phenomena such as the only intermolecular force the! To form hydrogen bonds form when a H is bonded to an N, O or atom... Above statements are true highest boiling point of the following compounds is ( are ) classified ethers! Missing reagent needed to carry out the following conversion such as the length the... The above statements are true is highly cohesive in hydrogen fluoride, the questions are more about than... With similar molecular weights it 's impossible to do without some prior knowledge bonds when... For scientists, academics, teachers, and the first two have similar structural features it 's impossible which of the following will have the highest boiling point?. Following compounds have the same number of electrons, and a similar length solution containing less than the butanes to!