Ch3ch2ch2oh Intermolecular Forces

A) The rate of crystallization > the rate of solution. The strongest intermolecular bond is Hydrogen bond (H with F, O, N). It is clear from our boiling point data that hydrogen bonding interactions are much stronger than either dispersion forces or dipole-dipole attractions. pdf), Text File (. The Organic Chemistry Tutor 624,636 views 45:36. 1331 – CHAPTER 11 QUESTIONS IGNORE QUESTIONS 3, 10, 37 onwards Intermolecular Forces 1. Intramolecular forces are those within the molecule that keep the molecule together, for example, the bonds between the atoms. 1) In liquid propanol, CH3CH2CH2OH which intermolecular forces are present?: Dispersion, hydrogen bonding and dipole-dipole forces are present. an ionic solid. The interparticle force is the same as the intermolecular force: the ionic bond and it is the strongest of the interparticle forces. Thermal Energy The energy associated with the movement of molecules and atoms. 15 No , at 1. This colorless liquid is also known as propan-1-ol, 1-propyl alcohol, n-propyl alcohol, and n-propanol. 9ch3ch2ch2ch2ch2oh 2. The students deduced that the heat change was due only to the formation of intermolecular forces between ethyl ethanoate molecules and trichloromethane molecules. Place the following compounds in order of decreasing strength of intermolecular forces. a) London-dispersion forces Xe in nonpolar, and methanol is an organic compound with low polarity. Answer: A Diff: 3 Page Ref: 11. C) Only dispersion and dipole-dipole forces are present. CH2Cl2 is polar, whereas CCl4 is not. A) CH3CH2CH2NH2 B) CH3CH2CH2F C) CH3CH2CH2OH D) CH3CH2COOH E) CH3CH(OH)CH3 ANS: B PTS: 1 DIF: easy REF: 11. What kind (s) of intermolecular forces exist in H2O2 (l)? Select all that apply? It has a dipole moment, so it'll have dipole-dipole interactions. Which of the following is true about kinetic energy, E k, and potential energy, E p, when liquid pentane at 35 ° C is compared with pentane vapor at 35 ° C?. CH3CH2CH2OH which intermolecular forces are present? Only hydrogen bonding forces are present. CH3CH2OH and H2O. Intermolecular forces of attraction in liquid chloroethane are larger due to dipole-dipole attraction; thus a higher boiling point for chloroethane. Why are intermolecular forces generally much weaker than bonding forces? II. The ethylene glycol can form hydrogen bonds on both ends of the molecule resulting in much stronger intermolecular forces and a higher boiling point. D) Only hydrogen bonding forces are present. Since NH3’s intermolecular forces are bigger than those of CH4, the bonds of NH3 take more kinetic energy to break them and thus have a higher boiling point. IONIC FORCES: The forces holding ions together in ionic solids are electrostatic forces. (f) higher. " aLjLjW"MMM £'7'7828 2L008L 6 000 06 L-hh 2 2-LD-D N8SI. For compounds of comparable molecular mass, the more polar the functional group, the stronger the intermolecular forces, the higher the viscosity. Dispersion, hydrogen bonding and dipole-dipole forces are present. in terms of the intermolecular forces between each of the solutes and water. Liquid and Intermolecular Forces, Chapter 12. Chemistry 222 Oregon State University Worksheet 4 Notes 1. Hydrogen bonds are the strongest of all intermolecular forces. List the different intermolecular forces you would expect for each of the following compounds. Forces and Liquid Structure Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding) *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids) Molecular Shape and Structure. This intermolecular attraction of a hydrogen atom to an electronegative atom is referred to as hydrogen bonding. Topic: Intermolecular forces. And Hydrogen bonding is a special case of dipole - dipole bonding that only appears in HF, HN and HO molecules due to the large difference in electronegativities. Chromium Has A Monatomic Body-centered Cubic Structure. 1 atm, water boils at a temperature above 100° C, since it is more difficult for gas molecules to escape the. 🤓 Based on our data, we think this question is relevant for Professor Albright's class at UMICH. 1-pentanol The answer for Q1 is (a) and. As carbons get added onto an alkane, London forces are greatly increased because many protons and electrons are being added. Zumdahl Chapter 1 Chemical Foundations Questions The difference between a law and a theory is the difference between what and why. Intermolecular forces just extend the thinking to forces between molecules and follows the patterns already set by the bonding within molecules. Here we have to rank the following in order of increasing surface tension at a given temperature, and have to explain our ranking. C)wood alcohol. 26) In liquid propanol, CH3CH2CH2OH which intermolecular forces are present? A) Dispersion, hydrogen bonding and dipole-dipole forces are present. CH3CH2OH < CH3CH2CH2OH < CH3CH2CH2CH2OH. 2 Answers to 5. 7a: One example of a homologous series is the alcohols. The stronger the interparticle attractions, the higher the temperature at which the substance will boil. B) The rate of solution > the rate of crystallization. They dissolve in water in any amount. Determine the kinds of intermolecular forces that are present in each element or compound. Which substance has the highest boiling point?. What type of intermolecular forces are likely to be similar in strength?. None of these 11. how do you figure out intermolecular forces in a molecule? 1. This process is no longer a significant source of 1-propanol. If we compare the boiling points of methane (CH 4) -161ºC, ammonia (NH 3) -33ºC, water (H 2 O) 100ºC and hydrogen fluoride (HF) 19ºC, we see a greater variation for these similar sized molecules than expected from the data presented above for polar compounds. Air conditioners not only cool air but dry it as well. d) As intermolecular forces increase, the heat of vaporization increases because more energy is needed to separate molecules from the liquid phase. The heat capacity of liquid water is 4. The permanent dipoles can also interact with each other, in the form of. A) (i) only B) (ii) and (iii) C) (i) and (iii) D) none E) all 3) 4) The shape of a liquidʹs meniscus is determined by _____. Hydrogen Bonding. 10 99) Which of the molecules below has the. 1-pentanol The answer for Q1 is (a) and. Propan-1-ol is the parent member of the class of propan-1-ols that is propane in which a hydrogen of one of the methyl groups is replaced by a hydroxy group. covalent network bonds. A) F 2 < NH 2 CH 3 < CO 2. hydrogen bonding, dipole-dipole force, and induced dipole/induced dipole force ____ 9. Intermolecular forces & boiling points of alcohols compared to other organic molecules Naming Chloroalcohols CH4O CH3OH CH3-OH C2H6O C2H5OH CH3CH2OH CH3-CH2-OH CH3OCH3 CH3-O-CH3 C3H8O C2H5CH2OH C3H7OH CH3CH2CH2OH CH3-CH2-CH2-OH CH3CH2OCH3 CH3OCH2CH3 CH3-O-CH2CH3 CH3-CH2-O-CH3 C4H10O C4H9OH C3H7CH2OH CH3CH2CH2CH2OH C5H11OH C5H12O C6H13OH. As for part c(ii), both butanoic acid and propanoic acid contain the same functional groups, except that butanoic acid contains an extra $\ce{CH3}$. a covalent network solid. a) single and double bonds, only. The ether is not. Hydrogen Bonding. Higher intermolecular forces -> more energy needed to pull molecules apart from each other to convert from a liquid state to gaseous, so a higher boiling point. None of these 11. CH3CH2CH2OH c. Dispersion Force Weakest Force: Exhibited in all molecules and atoms. Explain the difference. It is a colorless liquid with a slightly irritating, fruity odor. NF3 dispersion forces. CH3CH2CH2OH (C−C and C−H bonds, and one C−OH bond) CH3CH2CHO (C−C and C−H bonds, and one C=O bond) Based on the general trends of intermolecular forces, rank these molecules in order of increasing boiling point. organic water could be greater because of the fact the density of ice is under that of water. To rank items as equivalent, OVERLAP THEM. d) As intermolecular forces increase, the heat of vaporization increases because more energy is needed to separate molecules from the liquid phase. In the IUPAC system, the name of the alkane chain loses the terminal “e” and adds “ol”, e. In order to form this intermolecular bond, or several, the path has to be clear. CH 2Cl 2 is ionic while CH 2F 2 is molecular. Friday 10 June 2016 Afternoon Time allowed: 1 hour 30 minutes. What are the different types of intermolecular forces? Which is the strongest?. dispersion forces dipole-dipole forces CH3CH2CH2OH or CH3OH. molecules will have enough energy to overcome the intermolecular forces and enter into the gas phase. hydrogen bonding and induced dipole/induced dipole force e. Why are intermolecular forces generally much weaker than bonding forces? II. Browse from thousands of Intermolecular Force questions and answers (Q&A). Since the molecules have roughly the same mass and number of electrons, the London forces are expected to be comparable. In the IUPAC system, the name of the alkane chain loses the terminal “e” and adds “ol”, e. dispersion forces dipole-dipole forces dispersion forces and dipole-dipole forces dispersion forces, dipole-dipole forces, and hydrogen bonding b. Give the structural formula of (a) and write the equations for all the reactions. In liquid propanol, CH3CH2CH2OH which intermolecular forces are present? Dispersion, hydrogen bonding and dipole-dipole forces present: Compounds that exhibits only dipole-dipole intermolecular interactions: CH3Br: The normal boiling point for H2Se is higher than the normal boiling point for H2S. A: CH3CH2CH2CH3 < CH3CH2CH2OH < CH3CH2CHO. The normal boiling point of a substance is determined by its molecular mass and its intermolecular forces. Propionaldehyde or propanal is the organic compound with the formula CH 3 CH 2 CHO. This is due to intermolecular forces (hydrogen bonding in particular) The first compound has one site for hydrogen boding, the second has two, and the third has three. Chemistry 222 Oregon State University Worksheet 4 Notes 1. H3PO4 phosphoric acid B. Factors that affect the strength of London Forces 1) The more protons and electrons in a molecule, the stronger the London Forces-(higher molar mass usually means stronger London Forces) 2) A molecule with a linear shape will have stronger London Forces than a molecule with a spherical shape (if p+ and e-are the same). CH3(CH2)2CH3 or butane exhibits van der waals forces, this is the weakest type of intermolecular forces. This takes place when polar compounds are attracted to one another. 1110L Explanation: n=1:5kgC6H12O6 ¢ 1000g 1kg ¢ molC6H12O6 180gC6H12O6 3molCH4 1molC6H12O6 =25molCH4 T=300K. You can write a book review and share your experiences. Rank from highest to lowest vapor pressure. They are all bent like water) H 2 Se H 2 S H 2 Po H 2 Te 5 Using your knowledge of molecular structure, identify the main intermolecular force in the following compounds. -in this type of intermolecular force, there is an attraction between the positive end of one permanent dipole and the negative end of another permanent dipole. What is the lewis structure of acetone? What is the geometry around each carbon atom? Is acetone polar or non-polar? Why? What type(s) of intermolecular forces exist between acetone molecules? 1-propanol CH3CH2CH2OH has a molecular weight similar to acetone, but boils at 97. Substance B c. Determine if each pair of compounds forms a homogeneous solution when combined. Only dispersion and dipole-dipole forces are present. During this time, you may not be able to log into ChemSpider. SiO 2 is a macromolecular covalent substance and to separate the atoms requires the breaking of strong Si-O covalent bonds. And Hydrogen bonding is a special case of dipole - dipole bonding that only appears in HF, HN and HO molecules due to the large difference in electronegativities. NF3 nitrogen trifluoride E. (c) Explain, in terms of the intermolecular forces in both compounds, why ammonia has a higher boiling temperature than phosphine, PH3. What kind (s) of intermolecular forces exist in CH3CH2CH2OH (l)?Select all that apply. If you're behind a web filter, please make sure that the domains *. CH3COCH3CH2. organic water could be greater because of the fact the density of ice is under that of water. Determine if each pair of compounds forms a homogeneous solution when combined. • The larger the dipoles, the stronger the force of attraction between the two molecules, the stronger the. 04 fuerzas intermoleculares 1. Intermolecular attractive forces, collectively referred to as van der Waals forces, are responsible for the behavior of liquids and solids and are electrostatic in nature. CH3CH2CH2OH Which statement about intermolecular forces is true?. N-propanol appears as a clear colorless liquid with a sharp musty odor like rubbing alcohol. These are: London Dispersion Forces - a force of attraction between two molecules created by temporary dipoles which. The molcule of H2O2 happens to be quite polar, with the oxygen ends being extremely negative and the hydrogen ends being positive. Intermolecular Forces - Free download as Powerpoint Presentation (. CH 2Cl 2 is ionic while CH 2F 2 is molecular. From most to least volatile: methane; methanol; ethanol; propanol. Ionic forces can be seen as extreme dipoles in a certain way, there is a grey area when electronegativity becomes large enough, that it can be seen either as a molecular structure or ionic structure. Intermolecular forces refers to the force of attraction or force of repulsion between two molecules of same or other type. In liquid propanol, CH3CH2CH2OH which intermolecular forces are present? Dispersion, hydrogen bonding and dipole-dipole forces present: Compounds that exhibits only dipole-dipole intermolecular interactions: CH3Br: The normal boiling point for H2Se is higher than the normal boiling point for H2S. 4d: Based on the types of intermolecular force present, explain why butan-1-ol has a higher 11N. Hydrogen bondings are the strongest IMF. Concept Introduction: London dispersion force also called an induced dipole-induced dipole attraction is a temporary attractive force that results when the electrons in two adjacent atoms occupy positions that make the atoms form temporary dipoles. The intermolecular forces present in CH 3 OCH 3 are: 4. Both compounds have a tetrahedral geometry so and are non-polar. Hydrogen bond contributes the most. OK, let's review the kinds of intermolecular forces you can have: 1. Nov 08, 2015 · "F"_2 < "Cl"_2 < "Br"_2 As you know, a molecule's boiling point depends on the strength of the intermolecular forces of attraction its molecules exhibit. Rank from highest to lowest vapor pressure. C) Only dispersion and dipole-dipole forces are present. COMPLETE TEXT BOOK SOLUTION WITH ANSWERS INSTANT DOWNLOAD SAMPLE QUESTIONS Chemistry Ninth Edition Steven S. Rank the following compounds in order of decreasing vapor pressure. The stronger the intermolecular forces, the higher the boiling point of the compound is. there are no ion-ion, ion-dipole, or dipole-dipole forces in CH4 because those rely on the polarity of the molocule and because Cl is polar, CHCl3 has more intermolecular forces and a higher boiling point. 1-propanol (CH3CH2CH2OH) d. Intermolecular Forces One of the biggest sources of difficulty for a chemistry student is the distinction between chemical bonds and intermolecular forces. CO is an unusual molecule. B) Only dipole-dipole and ion-dipole forces are present. I know the different forces (dipole, hydrogen bond, and London, kinda) I just can't match them up with the compounds. Do the problems on your own BEFORE looking at the answers. on StudyBlue. HF O2 CO2 HF > CO2 > O2 2. CH3CH2OH < CH3CH2CH2OH < CH3CH2CH2CH2OH. This can be explained by. LDF relates to the size of the molocule, giving CHCl3 more intermolecular forces than CH4already. 6ch3ch2ch2ch2ch2ch2ch2oh 0. 2-propanol (CH3CHOHCH2CH3) 2. Thus the presence of hydrogen bonding in the unknown substance is the best answer. PLAN: Consider the intermolecular forces which can exist between solute molecules and consider whether the solvent can provide such interactions and thereby substitute. London dispersion forces, which result from short-lived dipoles induced by fluctuations in the electron shell of molecules, are also present. The ethylene glycol can form hydrogen bonds on both ends of the molecule resulting in much stronger intermolecular forces and a higher boiling point. Ar dispersion forces dipole-dipole forces dispersion forces and dipole-dipole forces dispersion forces, dipole-dipole forces, and hydrogen bonding b. solid state - ice. (d) CH 3 CH 2 CH 2 OH or CH 3 CH 2 CHO Both molecules possess dipole-dipole interactions due to the presence of electronegative oxygen, CH 3 CH 2 CH 2 OH, however, contains. With stronger intermolecular attraction, of course CH 2F 2 will have a lower boiling point. This is an overly simplistic question that does not have a clearly defined answer. Consulting online information about the boiling points of these compounds (i. Whether you've loved the book or not, if you give your honest and detailed thoughts then people will find new books that are right for them. You then can envision the molecular geometry in order to find whether the molecule is polar (see text Sections 10. forces also include dipole forces. For future reference: these questions are a process of deduction based on the strength of the intermolecular forces. arrange the following in order of increasing boiling point: CH4 CH3CH2CH3- CH3CH2CH2Cl- CH3CH2CH2OH- i have found the boiling points for these but for some reason its not working out , can anyone help? please, only helpful answers. Createassignment,54705,Exam2,Nov05at1:25pm 6 at300Kand770torr. Factors that affect the strength of London Forces 1) The more protons and electrons in a molecule, the stronger the London Forces-(higher molar mass usually means stronger London Forces) 2) A molecule with a linear shape will have stronger London Forces than a molecule with a spherical shape (if p+ and e-are the same). Intermolecular Forces - Free download as Powerpoint Presentation (. Therefore, CH2Cl2 interacts with H2O via dipole-dipole forces, while CCl4 only interacts with water via dipole/induced dipole forces or LDFs, which would be weaker. In liquid propanol, CH3CH2CH2OH which intermolecular forces are present? Dispersion, hydrogen bonding and dipole-dipole forces present: Compounds that exhibits only dipole-dipole intermolecular interactions: CH3Br: The normal boiling point for H2Se is higher than the normal boiling point for H2S. 57 Ethanol is a polar molecule capable of hydrogen bonding with itself and water. 332–340) The molecule with the lowest vapor pressure will be the one with the strongest intermolecular forces. d) They have very strong intermolecular forces. Here are some tips and tricks for identifying intermolecular forces. Monica Mame Soma N. 00 PM (GMT). intermolecular forces present hydrocarbons; most important kinds intermolecular forces present chcl3; ch3ch2ch2oh intermolecular forces. Determine the kinds of intermolecular forces that are present in each element or compound. CH 2Cl 2 has hydrogen-bonding while CH 2F 2 does not. A: CH3CH2CH2CH3 < CH3CH2CH2OH < CH3CH2CHO. Rank the compounds in each group in order of increasing strength of intermolecular forces. forces also include dipole forces. Crystalline Solids Atoms and molecules are composed in 3D. CH3CH2CH2F is the largest and only polar compound and therefore has the greatest intermolecular forces (both dipole-dipole and the greatest London Dispersion forces) and is eliminated. they will surround the more electronegative atom in the bond). Solids, liquids, and gases are held together by intermolecular forces. D)rubbing. water experiences adhesive forces with glass that are stronger than its cohesive forces, causing it to climb the surface of a glass tube. Three types of intermolecular forces exist. d)Only dipole-dipole and ion-dipole forces are present. organic water could be greater because of the fact the density of ice is under that of water. Dispersion Force Weakest Force: Exhibited in all molecules and atoms. brown, lemay ap chemistry monta vista high school. Answer Save. Rank the following compounds in order of decreasing … Rank the following compounds in order of decreasing … data a by type of intermolecular force. different states of matter. 5 degree angles. BP does not break covalent bonds that would be cracking of hydrocarbons. When (a) is reacted with sodium metal it gives compound (d), C 8 H 18 which is different from the compound formed when n-butyl bromide is reacted with sodium. Snyder, Jon Antilla | download | B–OK. CH3CH2CH2O H CH3OH c. It is almost nonpolar its physical properties are almost identical to N2 but with very different chemical properties. inter- molecular Intermolecular Forces and Bonding in Solids -. Answer: A Diff: 3 Page Ref: 11. Alkanes: This type of organic compound contains only the weakest intermolecular force, London forces and therefore has the lowest boiling point. C) Only dispersion and dipole-dipole forces are present. Thus the order. methanol (CH3OH) b. 2 is more polar and thus must have stronger binding forces. 2 There are two competing intermolecular forces at play: • Dipole-dipole forces increase as the halogen becomes more electronegative (I < Br < Cl < F). liquid state -. Here we have to rank the following in order of increasing surface tension at a given temperature, and have to explain our ranking. also has van der waals CH3CH2OH or ethanol also has van der waals, It also has Hydrogen bonding due to the very high electronegativity which polarises the hydrogen to make it slightly positive, this then. It has a role as a protic solvent and a metabolite. Intermolecular Forces Properties of Liquids Stronger intermolecular forces → molecules are more attracted to each other → they stick together better → they are harder to separate from each other. Hydrogen bonding between O and H atom of different molecules. Considering these two factors, predict the order of increasing boiling points for the following substances: H2, NaCl, H2O, and CO2. CH3CH2CH2CH3 < CH3CH2CH2CH2Cl < CH3CH2CH2CH2OH. C) CO 2 < NH 2 CH 3 < F 2. dispersion forces dipole-dipole forces CH3CH2CH2OH or CH3OH. D) Only hydrogen bonding forces are present. The normal boiling point of a substance is determined by its molecular mass and its intermolecular forces. Intermolecular Forces (5) Ionic Bonding (2) Ionic Compounds (3) Ionization Energy (1) Laboratory Activity Task (1) Laboratory work (1) Learning Objective (1) Lemon Shell Game (1) Lewis Acids and Bases (1) Misconception (1) Mol Concept (2) Molecular Geometry (2) Molecular Shapes (1) Negative Ions (1) Neutralization (3) Nomenclature (4) Non Polar. Propan-1-ol is the parent member of the class of propan-1-ols that is propane in which a hydrogen of one of the methyl groups is replaced by a hydroxy group. 6 atm, substance D must be heated to about 60˚C 25. List the different intermolecular forces you would expect for each of the following compounds. Predict which two interactions are stronger than the other two. Sodium or potassium dichromate acidified with dilute sulphuric acid can bring about oxidation in straight chained alcohols. organic water could be greater because of the fact the density of ice is under that of water. hydrogen bonding c. ppt), PDF File (. Question 4 0. CH 3 CHO is more polar than CH 3 OCH 3 and so CH3CHO has stronger intermolecular dipole − dipole attraction than CH 3 OCH 3 CH 3 CH 2 CH 3 has only weak van der Waals force. CH3CH2CH2F is the largest and only polar compound and therefore has the greatest intermolecular forces (both dipole-dipole and the greatest London Dispersion forces) and is eliminated. 2: How Bonding affects Physical Properties. Consulting online information about the boiling points of these compounds (i. Describe two features of a homologous. Predict which two interactions are stronger than the other two. Nov 08, 2015 · "F"_2 < "Cl"_2 < "Br"_2 As you know, a molecule's boiling point depends on the strength of the intermolecular forces of attraction its molecules exhibit. 7)The alcohol which contains only one carbon atom and has the common name of wood alcohol is A)methanol. Propionamide has the strongest intermolecular forces, It should have the highest boiling point. In both cases these attractive forces can occur between molecules of the same compound or different compounds. 04 fuerzas intermoleculares 1. A dipole is a molecule that has split charge. • Intermolecular dipole-dipole forces are weaker than ionic forces or covalent bonds. intermolecular forces present hydrocarbons; most important kinds intermolecular forces present chcl3; ch3ch2ch2oh intermolecular forces. dipole-dipole interactions hydrogen bonding dispersion forces. Pentane, C 5 H 12, boils at 35 ° C. The longer chain has more electrons (more bonds) and so it possesses the stronger dispersion forces. Dispersion Force Weakest Force: Exhibited in all molecules and atoms. Which one of the following decreases as the strength of the attractive intermolecular forces increases? The vapor pressure of a liquid Rank the following molecules in order of increasing normal boiling point: CH3CH2OH, CH3CH2CH2OH, CH3CH2OCH3. D is the only opposites. The students deduced that the heat change was due only to the formation of intermolecular forces between ethyl ethanoate molecules and trichloromethane molecules. To rank items as equivalent, OVERLAP THEM. Propionaldehyde or propanal is the organic compound with the formula CH 3 CH 2 CHO. The Organic Chemistry Tutor 624,636 views 45:36. The relative strength of Ep vs. However, acetone forms hydrogen bonds to water much more effectively than chloroethane does, resulting in greater solubility of acetone in water. D) Only hydrogen bonding forces are present. CH3CH2CH2OH which intermolecular forces are present? A) Dispersion, hydrogen bonding and dipole-dipole forces are present. a high critical temperature E. What types of intermolecular attractions do each of the alcohols exhibit and how might they affect the tendency for an alcohol. - [Voiceover] Consider the molecules represented above and the data in the table below. Remember, the prefix inter means between. Regents review Organic chemistry A)functional groups B)molecular masses C)numbers of covalent bonds D)percent compositions by mass 15. The intermolecular forces between discrete carbon dioxide molecules are weak and hence molecules separate easily under the influence of thermal energy. 這些范德華力的強度都不及 ch3ch2ch2oh 分子間的氫鍵,所以它們的沸點都較 ch3ch2ch2oh 低。 2007-10-12 20:29:54 補充: Van der Waals forces are intramolecular fources; whereas covalent bonds and ionic bonds are intermolecular attractions. You can write a book review and share your experiences. The action of intermolecular forces must be observed through a microscope and by analyzing data, including vapor pressure. While both are used to hold chemical systems together, they each introduce their own specific qualities into structures. In the gas phase, Ep << Ek because the gas particles experience little attraction for one another and the particles are moving. That is, strong intermolecular forces result in low vapor pressure and weak intermolecular forces result in high vapor pressure. a high boiling point B. They are all bent like water) H 2 Se H 2 S H 2 Po H 2 Te 5 Using your knowledge of molecular structure, identify the main intermolecular force in the following compounds. C) CO 2 < NH 2 CH 3 < F 2. Intramolecular forces (covalent) are stronger than intermolecular forces (London & hydrogen bonding). The students deduced that the heat change was due only to the formation of intermolecular forces between ethyl ethanoate molecules and trichloromethane molecules. It would be I,II,III. inter- molecular Intermolecular Forces and Bonding in Solids -. What kind(s) of intermolecular forces exist in the compounds given below? (a) CH3CH2CH2CH2CH3(l) dispersion forces dipole-dipole forces hydrogen bonding (c) H2CO(l) dispersion forces dipole-dipole forces hydrogen bonding (b) CH3CH2OH(l) dispersion forces dipole-dipole forces hydrogen bonding (d) O2(l) dispersion forces dipole-dipole forces hydrogen bonding. B) The rate of solution > the rate of crystallization. For future reference: these questions are a process of deduction based on the strength of the intermolecular forces. Exercise 11. solid state - ice. 1-pentanol The answer for Q1 is (a) and. E) NH 2 CH 3 < CO 2 < F 2. Factors that affect the strength of London Forces 1) The more protons and electrons in a molecule, the stronger the London Forces-(higher molar mass usually means stronger London Forces) 2) A molecule with a linear shape will have stronger London Forces than a molecule with a spherical shape (if p+ and e-are the same). Problem Set 11. What kind of intermolecular forces are present in hydrogen sulfide? Dipole -Dipoles are permanent charge seperations. Why are intermolecular forces generally much weaker than bonding forces? II. The intermolecular forces of propanol are hydrogen bonding, dipole-dipole forces and London dispersion forces. This Van Der Waals force is relatively weak due to the absence of a permanent dipole. H2CCHCH3 propene D. It has an H bonded to an O so it can hydrogen bond. Molecules attract each other, an the force of attraction increases rapidly as the intermolecular distance decreases. (f) higher. 12-1 CHAPTER 12 INTERMOLECULAR FORCES: LIQUIDS, SOLIDS, AND PHASE CHANGES 12. London dispersion forces, which result from short-lived dipoles induced by fluctuations in the electron shell of molecules, are also present. forces also include dipole forces. : indefinite shape and volume. (c)What kinds of intermolecular attractive forces exist between acetone molecules? (d) 1-Propanol, CH3CH2CH2OH, has a molecular weight that is very similar to that of acetone, yet acetone boils at 56. Intermolecular forces are the attractive forces which impart characteristic physical properties to the substance. intermoleculuar forces strength increases boiling point increases and vapour pressure decreases. What type of intermolecular forces are likely to be similar in strength?. FUERZAS INTERMOLECULARESFuerzas de atracción que existen entre lasmoléculas de la misma o diferente especie Interacción dipolo-dipolo Puente o enlace de hidrógeno Fuerzas de dispersión de London (dipoloinducido-dipolo inducido). Problem Set 11. London Dispersion Forces - the force of attraction between all molecules (any two at one time), created by temporary dipoles, which are caused by the movement of electrons around two atoms. arrange the following in order of increasing boiling point: CH4 CH3CH2CH3- CH3CH2CH2Cl- CH3CH2CH2OH- i have found the boiling points for these but for some reason its not working out , can anyone help? please, only helpful answers. This is due to intermolecular forces (hydrogen bonding in particular) The first compound has one site for hydrogen boding, the second has two, and the third has three. Instructions. Carboxylic acids and alcohols are often warmed together in the presence of a few drops of concentrated sulphuric acid in order to observe the smell of the esters formed. Choose all substances with a hydrogen atom that would participate in hydrogen bonding with an appropriate acceptor atom. (b) Both chloroethane and acetone are polar. Intermolecular Forces Properties of Liquids Stronger intermolecular forces → molecules are more attracted to each other → they stick together better → they are harder to separate from each other. b)Dispersion, hydrogen bonding and dipole-dipole forces are present. ch3och2ch3, ch3ch2ch2oh, ch3ch(ch3)2 Boiling point of Organic Compound: The general quality of the four intermolecular forces is: Ionic > Hydrogen holding > dipole > Van der Waals dispersion powers. a molecular solid containing nonpolar molecules. composed of molecules held together by intermolecular London forces. Hydrogen bond contributes the most. 1-propanol (CH3CH2CH2OH) d. Due to this, more energy would be required to break the bonds in option A than the CH3CH2CH2OH. A dipole is a molecule that has split charge. They dissolve in water in any amount. Chapter 11 Homework 11. It occurs between H and F's, O's, and N's. A) F 2 < NH 2 CH 3 < CO 2. Which of these is the weakest of the intermolecular attractive forces? A) Ion-ion B) Dispersion forces C) Dipole-dipole D) Covalent bonding E) Hydrogen bonding Ans: B Topic: Intermolecular forces. Hydrogen bonding > Dipole-dipole > Dispersion Dispersion is a force that all molecules have, dipole-dipole is only in polar molecules, and hydrogen bonding is only present in molecules where hydrogen is directly bonded to oxygen. In a nutshell, the difference between propan-1-ol and propan-2-ol is the position of their respective hydroxyl (-OH) groups. High boiling points occur when intermolecular forces are strong. a) London-dispersion forces Xe in nonpolar, and methanol is an organic compound with low polarity. dipole-dipole forces. If there’s one thing you learn how to do well in Org 1, it’s make alcohols. 6 Intermolecular Forces. Why are intermolecular forces generally much weaker than bonding forces? II. intermolecular forces between large hydrocarbons. George Hademenos - Schaums Outline of Theory and Problems of Organic Chemistry (1999 McGraw-Hill). CH 3 CHO is more polar than CH 3 OCH 3 and so CH3CHO has stronger intermolecular dipole − dipole attraction than CH 3 OCH 3 CH 3 CH 2 CH 3 has only weak van der Waals force. how do you figure out intermolecular forces in a molecule? 1. Chemistry 222 Oregon State University Worksheet 4 Notes 1. In liquid propanol, CH3CH2CH2OH, which intermolecular forces are present? Dispersion, hydrogen bonding and dipole-dipole forces are present. in terms of the intermolecular forces between each of the solutes and water. B) Only dipole-dipole and ion-dipole forces are present. Therefore, the intermolecular. a metallic solid. For compounds of comparable molecular mass, the more polar the functional group, the stronger the intermolecular forces, the higher the viscosity. CH3CH2CH2OH or CH3CH2OCH3 Answer: CH3CH2CH2OH has the higher boiling point since it is capable of intermolecular hydrogen bonding. intermoleculuar forces strength increases boiling point increases and vapour pressure decreases. CH3CH2CH2OH which intermolecular forces are present? A) Dispersion, hydrogen bonding and dipole-dipole forces are present. Thionyl Chloride, SOCl 2 In a blatant plug for the Reagent Guide and the Reagents App for iPhone , each Friday I profile a different reagent that is commonly encountered in Org 1/ Org 2. It is clear from our boiling point data that hydrogen bonding interactions are much stronger than either dispersion forces or dipole-dipole attractions. 6 Intermolecular Forces. Answer: A Diff: 3 Page Ref: 11. intermolecular forces, look for the one that is the most polar or that has the most electronegative atoms or the most hydrogen bonding groups. Intramolecular forces are those within the molecule that keep the molecule together, for example, the bonds between the atoms. A: CH3CH2CH2CH3 < CH3CH2CH2OH < CH3CH2CHO. Explain the difference. Water and ethyl alcohol will both have dipole-dipole interactions. CH3CH2CH2F is the largest and only polar compound and therefore has the greatest intermolecular forces (both dipole-dipole and the greatest London Dispersion forces) and is eliminated. It is a colorless liquid with a slightly irritating, fruity odor. Strength of intermolecular forces depends on the in. Topic: Intermolecular forces. And all molecules have dispersion forces. The molecular masses of the given compounds are in the range 44 to 46. • The larger the dipoles, the stronger the force of attraction between the two molecules, the stronger the. Factors that affect the strength of London Forces 1) The more protons and electrons in a molecule, the stronger the London Forces-(higher molar mass usually means stronger London Forces) 2) A molecule with a linear shape will have stronger London Forces than a molecule with a spherical shape (if p+ and e-are the same). (van der Waals force exist in all molecules and is significantly weaker than hydrogen bonds, so it will not be mentioned here) First draw the structure out, and find all possible dipoles. Whether you've loved the book or not, if you give your honest and detailed thoughts then people will find new books that are right for them. This is why if you leave ice in the freezer for a long time it "disappears. CH3CH2CH2OH or CH3CH2OCH3 Answer: CH3CH2CH2OH has the higher boiling point since it is capable of intermolecular hydrogen bonding. trans-2-butene b. Both have only LDF but since hexane is a more complex molecule, it has more electrons and thus more polarization opportunities. Autoignites at 700°F. Here all the given molecules have hydrogen bond. CH3CH2CH2CH3 < CH3CH2CH2CH2Cl < CH3CH2CH2CH2OH. A) F 2 < NH 2 CH 3 < CO 2. CH3CH2CH2OH which intermolecular forces are present? A) Dispersion, hydrogen bonding and dipole-dipole forces are present. Intermolecular forces of attraction in liquid chloroethane are larger due to dipole-dipole attraction; thus a higher boiling point for chloroethane. A) The rate of crystallization > the rate of solution. 2: How Bonding affects Physical Properties. This is due to intermolecular forces, not intramolecular forces. E) NH 2 CH 3 < CO 2 < F 2. - [Voiceover] Consider the molecules represented above and the data in the table below. Covalent > ionic > H-bond > DD > VDW 1. on StudyBlue. List all the intermolecular forces present in pure acetone. 1-Propanol is a primary alcohol with the formula CH 3 CH 2 CH 2 OH (sometimes represented as PrOH or n-PrOH). With stronger intermolecular attraction, of course CH 2F 2 will have a lower boiling point. This process is no longer a significant source of 1-propanol. What kind of intermolecular forces are present in hydrogen sulfide? Dipole -Dipoles are permanent charge seperations. TsCl (p-toluenesulfonyl chloride) And MsCl (methanesulfonylchloride) As Reagents In Organic Chemistry. 3) Identify the characteristics of a gas. Therefore, the boiling point of CH3CH2CH2CH3 is higher. Explain the difference. (C) the higher the vapor pressure. Interpretation: Identify the intermolecular forces that must be overcome to perform the reaction. Starting with the four-carbon butanol the solubility of alcohols is starting to decrease. In liquid propanol, CH3CH2CH2OH Which intermolecular forces are present? And how? - 113560. Determine the kinds of intermolecular forces that are present in each element or compound. The strongest intermolecular bond is Hydrogen bond (H with F, O, N). d) They have very strong intermolecular forces. Answer: CH3CH2CH2CH3 has greater van der Waals forces because it has a greater contact area than isobutane. As carbons get added onto an alkane, London forces are greatly increased because many protons and electrons are being added. Chapter 11. e) Vapor Pressure As the intermolecular forces increase (↑), the vapor pressure decreases (↓). All solids also have a vapor pressure. H3PO4 phosphoric acid B. A would definitely have a higher boiling point than CH3-CH2-CH2-OH because in option A, there is an additional CH2 bond in it. 332–340) The molecule with the lowest vapor pressure will be the one with the strongest intermolecular forces. an ionic solid. Forces and Liquid Structure Interionic and Intermolecular Forces (Ion-Ion, Ion-Dipole, Dipole-Dipole, Dipole-Induced Dipole, Dispersion/Induced Dipole-Induced Dipole/London Forces, Hydrogen Bonding) *Liquid Structure (Viscosity, Surface Tension, Liquid Crystals, Ionic Liquids) Molecular Shape and Structure. 1) CH4 has weak dispersion forces and CH3Cl has dipole -dipole forces. For the following pair of compounds,. a high vapor pressure C. And all molecules have dispersion forces. (B) the lower the boiling point. 6 Intermolecular Forces. • Intermolecular dipole-dipole forces are weaker than ionic forces or covalent bonds. CCl4 and H2O b. Which of the following is true about kinetic energy, E k, and potential energy, E p, when liquid pentane at 35 ° C is compared with pentane vapor at 35 ° C?. Since NH3’s intermolecular forces are bigger than those of CH4, the bonds of NH3 take more kinetic energy to break them and thus have a higher boiling point. e) Vapor Pressure As the intermolecular forces increase (↑), the vapor pressure decreases (↓). 5 degree angles. If you are also interested in the other intermolecular forces (van der Waals dispersion forces and dipole-dipole interactions), there is a link at the bottom of the page. For example, at 25 oC water has a vapor pressure of 24 torr, whereas acetone (C3H6O) and diethyl ether (C4H10O) have vapor pressures of about 230 torr and 530 torr, respectively. Describe two features of a homologous. Acetone (CH3)2CO is used as a solvent and boils at 56. b) hydrogen. 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. Determine the kinds of intermolecular forces that are present in each element or compound. It is clear from our boiling point data that hydrogen bonding interactions are much stronger than either dispersion forces or dipole-dipole attractions. Thionyl Chloride, SOCl 2 In a blatant plug for the Reagent Guide and the Reagents App for iPhone , each Friday I profile a different reagent that is commonly encountered in Org 1/ Org 2. Asked in Chemistry , Elements and Compounds , Ammonia What is the intermolecular. Examples range from simple molecules like CH 3 NH 2 (methylamine) to large molecules like proteins and DNA. Since O has significant. check_circle Expert Answer. Find more Chemistry widgets in Wolfram|Alpha. Higher intermolecular forces -> more energy needed to pull molecules apart from each other to convert from a liquid state to gaseous, so a higher boiling point. Opposite charges attract each other. org are unblocked. The intermolecular forces experienced by liquid fluorine are dispersion forces which are weak forces due to temporary induced dipole. Graham Solomons, Craig B. organic chemistry basic text book Report this link. This causes regions of both of these molecules that have partial negative charges and other regions wind up with. (B) the lower the boiling point. • London dispersion forces are in the order of less than 1/100 of a covalent bond. The stronger intermolecular forces make the boiling point of ethanol higher. Dispersion forces are the only intermolecular forces in these compounds. txt) or view presentation slides online. dipole-dipole force and induced dipole/induced dipole force d. For (a) CH3CH2CH2OH has one less R-OH group than HOCH2CH2OH and therefore can make fewer. Home Molecules The Kinetic Molecular Theory Boiling Points of Simple Hydrides. Asked in Science. Rank the following compounds in order of decreasing vapor pressure. Hydrogen bond contributes the most. Considering these two factors, predict the order of increasing boiling points for the following substances: H2, NaCl, H2O, and CO2. Examples range from simple molecules like CH 3 NH 2 (methylamine) to large molecules like proteins and DNA. Only dipole-dipole and ion-dipole forces are present. Favourite answer. H2CCHCH3 propene D. Explain each of the following in terms of atomic and molecular structures and/or intermolecular forces. Hydrogen bonding in organic molecules containing nitrogen. The stronger the intermolecular forces, the higher the boiling point of the compound is. CH3CH2OH < CH3CH2CH2OH < CH3CH2CH2CH2OH. (HO)2SO sulfurous acid G. OK, let's review the kinds of intermolecular forces you can have: 1. inter- molecular Intermolecular Forces and Bonding in Solids -. b answer because of the fact of hydrogen bonding between the patial + charge of hydrogen and partial adverse charge of oxygen. Problem: Propyl alcohol (CH3CH2CH2OH) and isopropyl alcohol [(CH3)2CHOH], whose space-filling models are shown, have boiling points of 97. B: CH3CH2CHO < CH3CH2CH2CH3 < CH3CH2CH2OH. In liquid propanol, CH3CH2CH2OH which intermolecular forces are present? a)Only dispersion and dipole-dipole forces are present. Place the following compounds in order of increasing strength of intermolecular forces. None of these 11. Choose all substances with a hydrogen atom that would participate in hydrogen bonding with an appropriate acceptor atom. CH3CH2CH2OH falls into this category. (a) CH 2 Cl 2 or CH 2 Br 2. Answer: A Diff: 3 Page Ref: 11. TOP: phases | liquid KEY: intermolecular forces | hydrogen bonding MSC: general chemistry 55. For the following pair of compounds,. a covalent network solid. CH 3 CHO is more polar than CH 3 OCH 3 and so CH3CHO has stronger intermolecular dipole − dipole attraction than CH 3 OCH 3 CH 3 CH 2 CH 3 has only weak van der Waals force. Intermolecular attractive forces, collectively referred to as van der Waals forces, are responsible for the behavior of liquids and solids and are electrostatic in nature. intermolecular bonding - hydrogen bonds This page explains the origin of hydrogen bonding - a relatively strong form of intermolecular attraction. I know the different forces (dipole, hydrogen bond, and London, kinda) I just can't match them up with the compounds. Which of the following liquids would have the highest viscosity at 25°C? A. CHAPTER 7 ALCOHOLS, THIOLS, PHENOLS, ETHERS Several new functional groups are presented in this chapter. 🤓 Based on our data, we think this question is relevant for Professor Jackson's class at CALGARY. Hydrogen Bonding. All of the four listed compounds are molecular and their sizes are comparable. hydrogen bonding and induced dipole/induced dipole force e. Ionic forces can be seen as extreme dipoles in a certain way, there is a grey area when electronegativity becomes large enough, that it can be seen either as a molecular structure or ionic structure. (d) CH 3 CH 2 CH 2 OH or CH 3 CH 2 CHO Both molecules possess dipole-dipole interactions due to the presence of electronegative oxygen, CH 3 CH 2 CH 2 OH, however, contains. Intermolecular Forces. Propanol, CH3CH2CH2OH; b. what kind(s) of intermolecular forces exist in ch3ch2ch2oh(l)? select all that apply. Types of Forces. (D) the smaller the deviation from ideal gas behavior. If the molecules have very different molar masses (by a factor of 2 or. Intermolecular forces are the attractive forces which impart characteristic physical properties to the substance. The addition of only London forces allows for such a range each time a carbon (accompanied by 3 hydrogens) is added, which. a high vapor pressure C. That CH 2Cl 2 has a higher boiling point proves that is has stronger intermolecular. 1 atm, water boils at a temperature above 100° C, since it is more difficult for gas molecules to escape the. 1st attempt Items (3 items) (Drag and drop into the appropriate area) CH3CH2CH2OH CH3CH20% CH3CH2CH2F fullscreen. Which of the following would be most soluble in water? a. Interpretation: Identify the intermolecular forces that must be overcome to perform the reaction. Become a part of our community of millions and ask any question that you do not find in our Intermolecular Force Q&A library. For the vapor pressure/temperature diagram shown, approximate the normal boiling points for: a. To rank items as equivalent, OVERLAP THEM. You then can envision the molecular geometry in order to find whether the molecule is polar (see text Sections 10. In liquid propanol, CH3CH2CH2OH which intermolecular forces are present? Dispersion, hydrogen bonding and dipole-dipole forces present: Compounds that exhibits only dipole-dipole intermolecular interactions: CH3Br: The normal boiling point for H2Se is higher than the normal boiling point for H2S. dipole-dipole interactions hydrogen bonding dispersion forces. CH3CHCHCH3 cis-2-butene F. • Intermolecular dipole-dipole forces are weaker than ionic forces or covalent bonds. CH3CH2CH2F is the largest and only polar compound and therefore has the greatest intermolecular forces (both dipole-dipole and the greatest London Dispersion forces) and is eliminated. Covalent bond is only within the molecule not intermolecule bonding force. They are responsible for the weak interactions between the alkyl chains, like in other alkanes and non-polar molecules. Both ethanol and propanol are alcoholic compounds that contain a hydroxyl group (-OH) as the functional group of the molecule. trans-2-butene b. just check Wikipedia or some MSDS site) confirms the theory. In 2-propanol, the methyl groups obstruct part of the way, so a molecule approaching from a random. n-butane d. You would normally use small quantities of everything heated in a test tube stood in a hot water bath for a couple of minutes. While both are used to hold chemical systems together, they each introduce their own specific qualities into structures. The first type, which is the weakest type of intermolecular force, is a London Dispersion force. As carbons get added onto an alkane, London forces are greatly increased because many protons and electrons are being added. That is, strong intermolecular forces result in low vapor pressure and weak intermolecular forces result in high vapor pressure. All liquids have some vapor pressure. Determine if each pair of compounds forms a homogeneous solution when combined. Alkanes: This type of organic compound contains only the weakest intermolecular force, London forces and therefore has the lowest boiling point. CH3CH2CH2OH Which statement about intermolecular forces is true?. propanol is one of those inorganic molecules that can have both a polar and non-polar end. The intermolecular forces of propanol are hydrogen bonding, dipole-dipole forces and London dispersion forces. Fe(s) KNO3(s) SiO2(s) HCl(s) For questions 5 and 6 choose from the following. Do the problems on your own BEFORE looking at the answers. Created Date: 12/11/2017 10:08:51 AM. Since ethanol has only two carbon atoms, there is only one. 🤓 Based on our data, we think this question is relevant for Professor Jackson's class at CALGARY. Which of the following liquids would have the highest viscosity at 25°C? A. 12-1 CHAPTER 12 INTERMOLECULAR FORCES: LIQUIDS, SOLIDS, AND PHASE CHANGES 12. CH3CH2CH2OH which intermolecular forces are present? Only hydrogen bonding forces are present. What kind(s) of intermolecular forces exist in ch2cl2(l)? select all that apply. The ethylene glycol can form hydrogen bonds on both ends of the molecule resulting in much stronger intermolecular forces and a higher boiling point. So I'm just wondering if the longest chain would have the. how do you figure out intermolecular forces in a molecule? 1. You would normally use small quantities of everything heated in a test tube stood in a hot water bath for a couple of minutes. 18 J/g·qC and the heat of vaporization is 40. Alcohols have hydrogen bonding available, and are therefore much more involatile than the analogous alkanes. Forces between Molecules. (b) Both chloroethane and acetone are polar. The strength of the intermolecular materials in a substance determine physical. Dispersion Force Weakest Force: Exhibited in all molecules and atoms. Since O has significant. Study 20 Chapter 12 flashcards from Sean A. If there’s one thing you learn how to do well in Org 1, it’s make alcohols. If you're seeing this message, it means we're having trouble loading external resources on our website. All liquids have some vapor pressure. List the different intermolecular forces you would expect for each of the following compounds. NF3 dispersion forces. DON'T even READ THE REST OF THE QUESTION WHEN YOU SEE KEYWORDS ("Underline!" -Dr. This can be explained by. London is the weakest. So these are intermolecular forces that you have here. 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. liquid state -. For (a) CH3CH2CH2OH has one less R-OH group than HOCH2CH2OH and therefore can make fewer. b) dipole-dipole and London-dispersion forces. And we have this data in the table. (iii) Propanol can be oxidized to propanoic acid using potassium dichromate(V). Place the following compounds in order of decreasing strength of intermolecular forces. The stronger the intermolecular forces, the higher the boiling point of the compound is. Hydrogen bond contributes the most. Explain the difference. NF3 dispersion forces. (HO)2SO sulfurous acid G. Intermolecular Forces: Liquids and Solids Phases and Phase Diagrams Liquids and Liquid Properties Intermolecular Forces Heating Curves Introduction to Solids Cubic Packing Arrangements Closest-Packed Structures Density of a Crystalline Solid Ionic Solids and Interstitial Sites The Born-Haber Cycle. 89lql4xbim7 9wbg0otcwkfu hqmawlb3zu8ncn z83ds8c6bvb24k7 6d18kuq4nb 5wa6oj0rtarh 2ub3tahjxyhz p0mr90kqugmd604 t8cztv6ysimki5k 1wtww68tllqe bowgnuc6ew f3jrgm1o56 zjotnjqdhl md2ug7atb7kh6 ww6h24xdky0c 0b0d19552519h 4brkmklsueo4 l6jniim2vg92r g83qfsg3jt p5rlp2s2rnksxl lmr3nq9vg730 fb6og2jdac t1b8q3v4zsr k2e9pt6aerma 6cjpo6nnuk bn62l8lxsjgp bzi1q0m452j 4gzy5mg4vt8gypj 1mmk7xzwyig94h s3nqymuussf7