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- 1. Draw three molecules of each compound, i.e. draw the molecules next to one another to visualize IMF.a. Propane, CH 3 CH 2 CH 3b. Heptane, CH 3 (CH 2 ) 5 CH 3c. Propanol, CH 3 CH 2 CH 2 OHd. Heptanol, CH 3 (CH 2 ) 6 OH2. For each compound, consider whether or not H-bonding can occur between its molecules. Use a dashed lineto show any H-bonding.3. For each compound, consider whether or not any polar bonds are present.a. Use a different coloured pen to identify any polar bondsb. Which compounds are polar? Which compounds are nonpolar? Explain your reasoning4. Compare your drawings for propanol and heptanol.a. Which compound has stronger dispersion forces? Explain your answer.b. Which compound has a higher boiling point? Explain your answer.5. Compare your drawings of heptane and heptanol.a. Which compound is more polar? Explain your answer.b. Which compound is more soluble in water? Explain your answer Analysis:1. Which compound has higher solubility in water?a. A polar compound or a…21. Which of the following does have the lowest polarizability? Z of Br = 35, I = 53, F = 9, S = 16 a.Fb.S-c.Br-d.I-Which of the following compounds has the same molecular shape as CCl2Hl2? Select one: a. SiF4 b. C2H4 c. SF4 d. C2H2 e. KrF4
- 2. Describe "SP2 and SP3 bonding" and describe "crystal structure" according to each "bonding structure" in "carbon crystal structure" Describe the 'difference and reason for electrical conductivity' accordingly.Analyze the structure of the molecule below D. Carbon 8 has a bond angle C7-C8-C9 _________________ A. 90o B. 109.5o C. 120o D. 180o E. Can’t tell E. Comparing the bond C2-C3, and C6-C7, the LONGER bond is _________________ F. Below is a list of functional groups (other than alkane) present in this molecule. The correct one is ___________ A. alkene, ketone, alkyne and ether B. alkyne, amide, ketone and ether C. alkyne, alkene, alcohol and ester D. ether, alkyne, , amide, and alkene E. None of the aboveWhich of the following can be best explained by temporary dipole moments? Choose one or more: A. This explains why ammonia and nitrogen gas exhibit an attractive force between them. B. This explains how the molecules hydrogen fluoride and methanol can exhibit uncharacteristically strong intermolecular forces. C. This explains why long hydrocarbon chains have relatively high boiling points. D. This explains how two noble gases' molecules can have an attractive force between them. E. This explains why the dipole-dipole attractive force between dimethyl ether and acetone does not entirely account for the attractive force between these molecules.
- 12. The presence of a lone pair in the structure of ammonia (NH ) causes the H-N-H bond angle to deviate from the ideal value of 109.5° for tetrahedral geometry. What is the expected deviation for the value of the H-N-H bond angle? a. H-N-H bond angle > 109.5°b. it will not deviate from the ideal valuec. H-N-H bond angle < 109.5°d. cannot be determined 13. Which of the following statements are TRUE regarding the valence shell electron pair repulsion (VSEPR) theory? (Choose all that applies. a. 3D arrangement of the nuclei joined by electron groups result to the molecular shapeb. each electron group repels other groups to minimize the angle between themc. electron group arrangements are defined by both the bonding and nonbonding valence electron groups around the central atom 14. TRUE/FALSE: Secondary bonds are stronger than primary bonds due to the longer distance between the molecules involved in the interactions.This table displays the chemical make-up of human bones. Below, you can see an example of an amino acid, which is what makes up proteins. Proteins are a major component of human skin. HSe HO Structure of selenocysteine, from Wikipedia 8. a. What type of chemical bonding is predominately occurring in bones? b. Using the given information and recalling what we learned about bonding models back in Unit 1, explain how X-rays are able to show us bone damage, even though bones are under our skin.Gg.84.
- Select among the statements below the ones which are TRUE. There may be more than one true statement in the choices. a. In the band model, the electrons are assumed to occupy molecular orbitals.b. Usually, the gaseous form of a substance can still be solidified near (but not beyond) the critical point.c. In the electron sea model, the valence electrons in metals are assumed to be fixed in the lattice points.d. Conduction bands are closely spaced molecular orbitals with filled electron spaces.e. In p-type semiconductors, the dopant element typically contains three-valence electrons. Considering intermolecular forces, which of the following is INCORRECT?a. Ammonia, NH3 : H-bondingb. Acetone, H3C-C(=O)-CH3 : Dipole-dipolec. Bromine, Br2 : Dispersion forcesd. Formaldehyde, H2C=O : H-bondingRank the following in terms of increasing melting point: MgCl2 NaCl AlCl3C. This semiconductor is a gryisH D. A white solid with a melting point of 770 C. The solid does not conduct electricity, but the liquid does. E. White hygroscopic solid that melts at 2525°C. The solid does not conduct electricity, but the liquid does. b) H e) Br 10.) In pure samples of each of these compounds, which one(s) can form . bydrogen bonds? Which molecule(s) shown here have a dipole? Which molecule(s) have only dispersion forces? Which is more polarizable, c) or f)? Which has a greater viscosity, e) or f)? H-C-C CI Br CoBr H. H. Br H. H. H. H-O---H H. hj 11.) A) Which would have a greater melting point, (a) or (b)? Explain. B. al 8 H. H. b) B) Which would have a greater enthalpy of fusion, AH (c) or (d)? Explain d) A,4 shea to 145.0 C How much heat does the water absorb