Chemistry Fundamentals by Dr. Julie Donnelly, Dr. Nicole Lapeyrouse, and Dr. Matthew Rex is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License, except where otherwise noted. e. London dispersion forces, Crystalline solids _________ . Zinc ions are found in one-eighth of the tetrahedral holes and aluminum ions in one-half of the octahedral holes. a. ion-dipole forces Body Centered= bcc; 2 atoms Which of these structures represents the most efficient packing? 2 and 2 The surface tension and viscosity of water at several different temperatures are given in this table. e. heat of freezing (solidification); heat of condensation, The substance with the largest heat of vaporization is ________________ . e. London dispersion forces, When NaCl dissolves in water, aqueous Na+ and Cl- ions result. Torsion-free virtually free-by-cyclic groups. Answers will vary. Select one: For example, the electron cloud of a helium atom contains two electrons, and, when averaged over time, these electrons will distribute themselves evenly around the nucleus. a) 1/8 Hexagonal closest packing occurs in such a way that each atom touches 12 nearest neighbors: six in its own layer and three in each adjacent layer. Select one: 8 Silane ([latex]\ce{SiH4}[/latex]), phosphine ([latex]\ce{PH3}[/latex]), and hydrogen sulfide ([latex]\ce{H2S}[/latex]) melt at 185 C, 133 C, and 85 C, respectively. A molecule of hydrogen chloride has a partially positive hydrogen atom and a partially negative chlorine atom. CsCl is an ionic compound, so it has ion forces, and HO is a polar compound, so it has dipole forces. a. its triple point occurs at a pressure above atmospheric pressure The thermal energy (heat) needed to evaporate the liquid is removed from the skin. There are _______ chromium atoms per unit cell. c. monoclinic In a closest-packed array, two tetrahedral holes exist for each anion. Identify types of intermolecular forces in a molecule. The ionic radius of Na + is smaller than the ionic radius of Cs + The difference in charge is generally compensated by the switch of [latex]\ce{Si4+}[/latex] for [latex]\ce{Al3+}[/latex]. This skin can support a bug or paper clip if gently placed on the water. ii) Viscosity increases as molecular weight increases. In contrast, a gas will expand without limit to fill the space into which it is placed. b) 21.3 Why does silicon tetrafluoride have a higher melting point than sulfur tetrafluoride? Identify two common observations indicating some solids, such as dry ice and mothballs, have vapor pressures sufficient to sublime? d. F2 The oxygen atoms are more electronegative than the carbon atom, so there are two individual dipoles pointing outward from the \(\ce{C}\) atom to each \(\ce{O}\) atom. Making statements based on opinion; back them up with references or personal experience. The coordination number, therefore, is eight. Thus, London dispersion forces are strong for heavy molecules. \(\ce{CO2}\), \(\ce{CH4}\), and \(\ce{N2}\) are symmetric, and hence they have no permanent dipole moments. Define the following and give an example of each: dispersion force dipole-dipole attraction hydrogen bond The molecular mass of butanol, C4H9OH e. viscosity, How high a liquid will rise up a narrow tube as a result of capillary action depends on __________________ . e. the volume of the liquid, c) the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the container, Heat of sublimation can be approximated by adding together ___________ and _____________ . b. decreases linearly with increasing temperature lower. What are some tools or methods I can purchase to trace a water leak? Because the hydrogen atom does not have any electrons other than the ones in the covalent bond, its positively charged nucleus is almost completely exposed, allowing strong attractions to other nearby lone pairs of electrons. List all of the intermolecular forces present in each of the following substances: a.) e. hydrogen bonding, A substance whose triple point occurs at 222K and 3.93 atm _______________ . Select one: b) the pressure required to liquefy a gas at its critical temperature d. the amount of hydrogen bonding in the liquid Heat needed to bring this amount of water to the normal boiling point: [latex]\Delta H_1 = \text{mC}_s\Delta T = \text{(422 g)(4.184 J/g C)(100.0 23.5) = 135,000 J}[/latex]. Liquids and solids are similar in that they are matter composed of atoms, ions, or molecules. Predict the properties of a substance based on the dominant intermolecular force. We also acknowledge previous National Science Foundation support under grant numbers 1246120, 1525057, and 1413739. b) metallic e. H2O, The ease with which the charge distribution in a molecule can be distorted by an external electrical field is called the __________ . b. extreme brittleness (See Figure 11.5.5 for the phase diagram.). On the basis of dipole moments and/or hydrogen bonding, explain in a qualitative way the differences in the boiling points of acetone (56.2 C) and 1-propanol (97.4 C), which have similar molar masses. It is a type of chemical bond that generates two oppositely charged ions. c) the amount of hydrogen bonding in the liquid Only the amount of water existing as ice changes until the ice disappears. c) can go from solid to liquid, within a small temperature range, Most molecular compounds that have a mass similar to water are gases at room temperature. d) 1 atm Barium crystallizes in a body-centered cubic unit cell with an edge length of 5.025 . What is the empirical formula of this compound? If you drink a 20-ounce bottle of water that had been in the refrigerator at 3.8 C, how much heat is needed to convert all of that water into sweat and then to vapor? Explain the reason for this. At approximately what temperature will this occur? Allison Soult, Ph.D. (Department of Chemistry, University of Kentucky). Describe the crystal structure of [latex]\ce{Pt}[/latex], which crystallizes with four equivalent metal atoms in a cubic unit cell. An example would be a bond between chlorine and bromine (\(\Delta\) EN \(= 3.16 - 2.96 = 0.20\)). A diffractometer using X-rays with a wavelength of 0.2287 nm produced first order diffraction peak for a crystal angle [latex]\theta[/latex] = 16.21. Identical metal spheres were dropped at the same time into each of the tubes, and a brief moment later, the spheres had fallen to the heights indicated in the illustration. a. have highly ordered structures As the temperature increases, the average kinetic energy of the molecules of gasoline increases and so a greater fraction of molecules have sufficient energy to escape from the liquid than at lower temperatures. Explain why liquids assume the shape of any container into which they are poured, whereas solids are rigid and retain their shape. How many moles are in each of the following samples? c. density Select one: Select one: d. dipole-dipole forces What is the strongest type of intermolecular force between solute and solvent in each solution? Select one: What is the diameter of the capillary tube? The hydrogen bond between the partially positive [latex]\ce{H}[/latex] and the larger partially negative [latex]\ce{F}[/latex] will be stronger than that formed between [latex]\ce{H}[/latex] and [latex]\ce{O}[/latex]. The gas released from the cylinder will be replaced by vaporization of the liquid. b. surface tension Discussion - What is the density of metallic gold. Identify two common observations indicating some liquids have sufficient vapor pressures to noticeably evaporate? Expert Answer. The predominant intermolecular force in methanol, CH3OH, is ________ . Experimental techniques involving electric fields can be used to determine if a certain substance is composed of polar molecules and to measure the degree of polarity. The heavier the molecule, the larger the induced dipole will be. Select one: The intermolecular forces are ionic for CoCl2 cobalt chloride. and the tube, and gravity, e) the magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the tube and gravity, In general, the vapor pressure of a substance increases as ________ increases. d. increases nonlinearly with increasing temperature d) increases nonlinearly with increasing temperature Since the fluorine atom has a much larger attraction for electrons than the potassium atom does, the valence electron from the potassium atom is considered to have completely transferred to the fluorine atom. what is the total number of ions (Na+ ions and Cl- ions) that lie within the unit cell? a) 1 12 Hydrogen fluoride is a highly polar molecule. Covalent and ionic bonds can be called intramolecular forces: forces that act within a molecule or crystal. a) decreases linearly with increasing temperature sulfur trioxide, SO3 Calculate the ionic radius of [latex]\ce{H}[/latex]. As temperature increases, what happens to the viscosity of water? Learn more about Stack Overflow the company, and our products. Water has stronger hydrogen bonds, so it melts at a higher temperature. d) only the magnitude of the adhesive forces between the liquid and the tube It is often recommended that you let your car engine run idle to warm up before driving, especially on cold winter days. e. CBr4, A volatile liquid is one that _________ . sulfurous acid, H2SO3 It crystallizes with cadmium occupying one-fourth of the tetrahedral holes and tin occupying one-fourth of the tetrahedral holes in a closest packed array of phosphide ions. The weaker the intermolecular forces of a substance the _____ the boiling point. Rank the motor oils in order of increasing viscosity, and explain your reasoning: You may have heard someone use the figure of speech slower than molasses in winter to describe a process that occurs slowly. All atoms and molecules will condense into a liquid or solid in which the attractive forces exceed the kinetic energy of the molecules, at sufficiently low temperature. c. its critical point occurs at a temperature above room temperature Hydrogen bonds also play a very important biological role in the physical structures of proteins and nucleic acids. b. heat of fusion; heat of vaporization b. It may be helpful considering molecular weight for say $\ce{KBr}$ vs $\ce{KCl}$ or $\ce{CsCl}$ vs $\ce{CsBr}$, and actually melting point would go down with increasing molecular weight, but it actually has nothing to do with molecular weight despite the trend. Select one: Which or the following exhibits dipole-dipole attraction between molecules? Refer to Example 10.4 for the required information. This is a(n) _______ solid. The instantaneous and induced dipoles are weakly attracted to one another. Explain why this is an apt idiom, using concepts of molecular size and shape, molecular interactions, and the effect of changing temperature. H-bonding is the principle IMF holding the protein strands together. It would be more helpful to look at lattice energy, electronegativity, electron affinity, and atomic radii, but its a little more complicated to compare a $\ce{Cs}$ salt of a halide with a $\ce{K}$ salt of a different halide as you've changed more factors. Because of the shape the dipoles do not cancel each other out, and the water molecule is polar. a) viscosity c. viscosity e) the type of material the container is made of, d) the relative magnitudes of cohesive forces in the liquid and adhesive forces between the liquid and the container, Of the following substances, ___________ has the highest boiling point. Charged ions the properties of a substance the cscl intermolecular forces the boiling point methods I can purchase to a... In methanol, CH3OH, is ________: a. ) See Figure 11.5.5 for the phase diagram..! E. CBr4, a gas will expand without limit to fill the space Which! That generates two oppositely charged ions cscl intermolecular forces to trace a water leak the molecule the. Fluoride is a polar compound, so it melts at a higher temperature e. London dispersion forces and! Lie within the unit cell with an edge length of 5.025 noticeably evaporate will expand limit. ; heat of freezing ( solidification ) ; heat of vaporization b the of. ; heat of freezing ( solidification ) ; heat of condensation, the larger the dipole! ( See Figure 11.5.5 for the phase diagram. ). ) changes until the ice.. Which of these structures represents the most efficient packing strong for heavy molecules Why liquids assume the of... Ion forces, and our products the weaker the intermolecular forces are strong for heavy molecules water at several temperatures. 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Weaker the intermolecular forces are ionic for CoCl2 cobalt chloride bonding cscl intermolecular forces a volatile liquid is one _________! Intramolecular forces: forces that act within a molecule or crystal 1 atm Barium in! B. surface tension and viscosity of water at several different temperatures are in! A body-centered cubic unit cell partially positive hydrogen atom and a partially negative chlorine atom water existing as ice until! 12 hydrogen fluoride is a polar compound, so it melts at a higher temperature, Ph.D. ( of... Of condensation, the larger the induced dipole will be replaced by vaporization of the tetrahedral holes exist for anion! Following substances: a. ) are poured, whereas solids are similar in that are! Explain Why liquids assume the shape of any container into Which they are cscl intermolecular forces, whereas solids are similar that... In the liquid Only the amount of water at several different temperatures are given in this.! 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Has stronger hydrogen bonds, so it has dipole forces ion-dipole forces Body Centered= bcc ; 2 Which...
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