1. [6.4% ) Write down the electron configuration for Br. 2. [6.4 %) Draw resonance structures...
urgent help!!!! 31. Helium atoms do not combine to form Hemolecules, yet He atoms do attract one another weakly through A) dipole-dipole forces. B) ion-dipole forces. C) dispersion forces. D) dipole-induced dipole forces. E) hydrogen bonding. 32. Copper crystallizes in a face-centered cubic unit cell. The density of copper is 8.94 g/cm'. Calculate the length of the edge of the unit cell in pm. 33. The heat capacity of liquid water is 4.18 J/g.°C and the heat of vaporization is...
R1.20 atm) needed to produce 1.1x1o gofs. 2) ll there is excess SO2 present. S(g) + SO2(g) → 3 S(s) + 2 H2O(g) 6 L B) 88.0 L E) 132 L C) 45.4 L the following must be overcome during the boiling of so,? Make sure to 2. dipole-dipole forces D) 68.2 L draw a Lewis structure first. 1. dispersion forces A) 1 only 3. hydrogen B) 2 only C) 1 and 2 D) 1 and 3 1, 2, and...
Consider the molecule below: o=s=o: Select ALL the intermolecular forces that are expected to be present between two of these molecules. Select as many answers as are applicable, however points will be deducted for incorrect guesses. Select one or more: Dispersion forces Dipole/dipole forces Hydrogen bonding Check What amount of thermal energy (in kJ) is required to convert 136 g of ice at -16 °C completely to water vapour at 217 °C? The melting point of water is 0°C and...
(a) Which of the ions Sr 2+, Rb . Cs will have the largest heat of hydration? Which the smallest? (b) of the two compounds CaF 2 and KF, which has the stronger intermolecular forces? (c) of the two compounds H 20 and CCl4, which has the stronger intermolecular forces? 5. Calculate the heat (in kJ) required to transform 45.70 g of bromine from a solid at a temperature of -7.2 °C to a gas at 82 °C. Report your...
2. Identify the strongest type of intermolecular forces in acetone, ethanol, water and hexane. (Structures listed on page 15.) Experiment 2 Intermolecular Forces There are three general types of intermolecular forces. All substances exhibit London Dispersion Forces (LDF), and they are generally the weakest of the three types. These London forces are due to the attractions between small, temporary dipoles that arise from the constant, random movement of the electrons in a substance. As molar mass increases, the size of...
1. Liquid nitrogen at −196° C (nitrogen’s boiling point) is placed in a container with 3 kg of water at 25° C. (a) Suppose you add just enough liquid nitrogen such that all the water just freezes (i.e., the final state of the water is ice at 0° C). Draw a complete energy interaction diagram for this scenario, including a conservation of energy equation. (b) How much liquid nitrogen should you put in the container such that all the water...
1. Select the two compounds that are more likely to be a gas at room temperature (as opposed to a liquid). CH4 CH3OH C2H6 H2O 2. The separation of charges within a polar molecule is called a(n) ________. polar bond strong attraction dipole ionic bond dipole-dipole 3. Which of the following intermolecular forces best describes why nonpolar molecules like gasoline (C8H18) have only limited solubility in water? dipole-dipole ion-dipole Both dipole-dipole and induced dipole-induced dipole induced dipole-induced dipole dipole-induced dipole...
A metal with a molar mass of 192.22 g mol-1 and an atomic radius of 1.80 x 102 pm packs in a face centred cubic structure. Calculate the density of the metal in units of g cm 3 A mineral has the unit cell shown below contains nitrogen,lithium and boron. Determine the empirical formula of the mineral. B atoms are the nine smallest spheres on the corners and in the body - centre Li atoms are the fourteen medium spheres...
1-4 please 1. A drop of rainwater tends to bead up when placed on a leat. What physical property of water of water causes this to occur. How does this physical property relate to intermolecular forces? 2. Draw molecular orbital diagrams for F, and 0,. Determine which species is more stable. Explain your answer. 3. For each of the following: determine the total valence count, draw a valid Lewis structure, and indicate whether the molecule is polar or nonpolar. a....
5) Consider the phase diagram for carbon dioxide(10). Supercritical fluid Solid Liquid Pressure (atm) -78.5 -56.4 Temperature (°C)— a) What is the critical temperature for carbon dioxide? b) What is the critical pressure for carbon dioxide? c) What phase(s) is/are present at -10°C and 30 atm. d) What phase(s) is/are present at -60°C and 10 atm. - e) What phase(s) is/are present at-78.5°C and 1 atm. f) What phase(s) is/are present at-56.4°C and 5.11 atm. g) What is the normal...