5-2 Final Project Milestone 2

Give typed full explanation of all subparts otherwise leave it Not a single word hand written otherwise leave it

Butanol has the chemical formula C4H9OH.   d)    In the molecule of butanol, there are C-C bonds, C-H bonds, a C-O bond and a O-H bond. Order these bonds from most to least polar  e)    On average, would you expect C-C to have longer or shorter bonds than C-H Briefly explain your answer.  f)    From the reaction 2.57 L of carbon dioxide was produced and captured. Calculate the number of molecules of carbon dioxide if the temperature was 25.0 C and the pressure 1. 01 × 105 Pa.  g)    The empirical and molecular formula for butanol is the same. Briefly explain why.

Use the notes on the green page to help.  Use CER, Claim-answer to the question, reasoning-why its drawn correctly, evidence- to show why the others are incorrect. Answer completely.

Describe how you could separate and purify compound A from a mixture of two neutral compounds (A and B) when A comprises 95% of the total and B the other 5% of the total. Assume that A and B have similar polarities.

Answer the questions in the table below about this molecule:

compound hydrogen-bonding force Between Between molecules of formula or Lewis molecules of the the compound and molecules of water? name structure compound? H H | Н — С | | yes yes N-chloromethylamine - no no H. yes yes hydrogen iodide HI no no :0: || н —с —с-о — н H yes yes acetic acid no no H O O

6 с 12.01 1 7 N 16.00 14.01 Surface of water. __ 8 1.008 From the atoms above, draw the THREE (3) types of bonds that are POLAR COVALENT Draw COH4 (methanol, liquid) in LEWIS DOT, show all charges Show the methanol in the presence of TWO (2) water molecules. Show all bonds that will form with water (if any) and all charges. NO need to draw the molecules in Lewis dot for this part. Module Problem 1.20

Calculate the Enthalpy Change (ΔH) from average bond energies, which have been listed below in KJ/mol, for the following reaction and identify the nature of the reaction: CH3COOH + CH3OH → CH3COOCH3 + H2O [C‒H: 413; C‒C: 347; C=O: 745; C=C: 614; Cl‒Cl: 239, C‒O: 358; O‒H: 467]

Predict the chemical formula for a compound composed of Na+ and S2- and give the appropriate name.

1. Draw Lewis structures for ozone and for dioxygen. Using the data given below, qualitatively compare the bond enthalpies, bond orders, and bond lengths of these two compounds. O₂ (g) 20 (g) AH" = +498 kJ O(g) + O₂(g) →O, (g) AH-105 kJ

Here's an electrostatic potential map for water (H₂O): Draw and upload here as an attachment (remember no heic files!) a Lewis structure that represents a water molecule (H₂O). Label with partial charges (8* and 8) the relative polarities of the atoms, if any. How did you determine whether there are partial charges and how did you determine where to put them?

Draw all of the Lewis structures of O22- which obey the octet rule and use this Lewis structure or these resonance structures to predict how many covalent bonds connect each oxygen atom in the real structure to the central O atom. Assume that the octet rule is followed for the O atom when you draw your structure(s). Pick the correct statement from the choices below. a) Each oxygen atom is connected to the central O atom with 1 covalent bonds. b) Each oxygen atom is connected to the central O atom with 1.33 covalent bonds. c) Each oxygen atom is connected to the central O atom with 2 covalent bonds. d) Each oxygen atom is connected to the central O atom with 1.67 covalent bonds. e) Each oxygen atom is connected to the central O atom with 1.25 covalent bonds.

Draw the structural formula (with lone pairs) for the two molecules, water (H2O) and isopropanol (C3H8O). Draw a dipole arrow to show the direction the electrons are being pulled and label the areas of partial positive and negative charges. Note: the bond between C and H is NOT POLAR. Do not draw dipole arrows or partial charges for those bonds.

Define the Ground-level ozone, which is the primary component of smog, forms when HC and NOx react in the presence of sunlight on hot, calm days.

What is the greenhouse effect? How does the excess  CO2 gas in the atmosphere cause the greenhouse effect?

A chemist wants to observe the following reaction: 2H2 + O2 → 2H2O The chemist is standing inside a room with oxygen in the air and has a balloon filled with hydrogen. The chemist holds a small flame up to the hydrogen balloon. When the balloon pops, the hydrogen explodes in a ball of fire. Based on what you know about breaking and forming bonds, explain which part of the reaction is higher in energy (i.e., does it take more energy to break the bonds of the reactants, or is more energy given off when the product bonds are formed?). Defend your answer in three to five sentences.

Rank the elements or compounds in the table below in decreasing order of their boiling points. That is, choose 1 next to the substance with the highest boiling point, choose 2 next to the substance with the next highest boiling point, and so on.

Answer question one please

need help with the questions the arrows are pointing at SQ 3-The balanced chemical equation for the reaction of sodium bicarbonate and citric acid is below. 3 NaHCO3(aq) + C6H807(s) → Na3C6H5O7(aq) + 3H₂O(l) + 3CO2(g) = SQ 4-Write the Lewis Structure for all species in the net ionic equation. Reactants: Products: K SQ 5-Circle the bonds that are broken in the reactants and the bonds that are formed in the products.

Look very closely at those images. Look at those lines and look at those electrons. Use the image attached to help.

7. Estimate the enthalpy of reaction (in kJ/mol) for the combustion of methane. Be sure to show a lewis structure for each molecule. CH, (g) + 20, (g) ·CO, (g) + H,O (g) Bond Bond Enthalpy (kJ/mol) C-O 351 C=0 799 CEO 1070 O-O 142 O=0 498 C-H 414 O-H 460

This one is a little different, but can u answer it as well

Using bond energies, explain the reaction sequence of ozone-destroying capability in the stratosphere of hydrocarbons containing the halogens: Br > Cl> F

Because carbon and silicon are both elements in group 14 on the periodic table, we expect them to react with other elements in similar ways. To some extent, they do, but in some cases, carbon and silicon compounds that seem to have analogous structures have very different chemical characteristics. For example, carbon tetrachloride, CCl4, is very stable in the presence of water, but silicon tetrachloride, SiCl4, reacts quickly with water. The unbalanced equation for this reaction is SiCl4 + H2O → Si(OH)4 + HCl Balance this equation. Write a conversion factor that could be used to convert between moles of SiCl4 and moles of H2O. How many moles of SiCl4 react with 24 moles of water? Write a conversion factor that could be used to convert between moles of Si(OH)4 and moles of water. How many moles of Si(OH)4 form when 4.01 moles of H2O react with an excess of SiCl4?

Testosterone is an anabolic steroid. The structure of testosterone is shown below. What is the idealised bond angle at the indicated atom (ii) ? Hint: atom (iv) has been completed for you as an example. (iv) bond angle: 109.5°, geometry of the electron pairs: tetrahedral, shape of the bonds: tetrahedral ·····|||I H ····||||I ii iv

A vessel originally contained 0.055 mol iodine monobromide (IBr), 0.0012 mol I2, and 0.0060 mol Br2. I2(g) + Br2(g)  2 IBr(g)     What is the value of Q?

Draw a skeletal ("line") structure of this molecule: OH O || CH -C-CH₂-CH3 CH3 || Show Transcribed Text G CI Ĉ Suppose all the chlorine atoms in this molecule are replaced by hydrogen atoms: Draw a skeletal ("line") structure of the new molecule.

Methanal can be made through the partial oxidation of methane using O2 in the presence of a catalyst: CH4 (g) + O2 (g) → CH2O(g) + H,O(g) a. Use bond dissociation enthalpies to estimate the enthalpy change for this reaction. Bond ΔΗ (kJ/mol) C-H 413 O=0 498 O=C 745 0-H 463 Enthalpy change = kJ b. Calculate the enthalpy change for this reaction from enthalpies of formation. Substance A;H (kJ/mol) CH4 (g) -74.87 O2 (g) H2 O(g) -241.8 CH20(g) -115.9 Enthalpy change kJ

Many free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical- radical combination reaction is the formation of a new electron-pair bond. Consider the formation of hydrogen peroxide. 2 OH(g) → H₂O₂(g) Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons. OH(g) Select Draw Rings More / ||| ||| Erase Q2 Q H₂O₂(g) Select Draw Rings More 3 S H Erase Q2 Q Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemistry Publisher: University Science B