There are two unknown compounds, #19 and #39, and their various spectra are attached (see attachment). Using the spectra and justification, find the structures of the unknowns. The spectra include IR, UV, Mass Spec, and H and C NMR.
What are common household bleaches? What are oxidizing and reducing bleaches? What is the chemistry of bleaching action? What makes the dyes and pigments appear colored?
Does the electronic configuration of carbon result in the various allotropes of carbon?
Consider the following elements and arrange them in order of increasing number of electrons depicted in electron dot symbols. Which one occupies the intermediate position in the series? P, Se, Si, I and B A. P B. B C. Si D. I Consider the following elements and select the one which has the smallest number of electrons
Answer and explain 1) As the volatility of a liquid increases, its equilibrium vapor pressure? A) increases B) decreases C) remains the same 2) Which substance contains molecules that will not form hydrogen bonds? A) hydrogen B) hydrogen fluoride C) water D) ammonia 3) At what temp would CO2 gas be most soluble?
My text gives the example of the following reaction: H2(g) + Cl2(g)-->2HCl(g) / 2 moles HCl To break bond 1 mole H-H bonds x 432 kJ/mol = 432 kJ 1 mole Cl-Cl bonds x 240 kJ/mole = 240 kJ 432 + 240 = 672 kJ Energy released / bond making 2 mol H-CL bonds x 428 = 856 kJ bond breaking +672 bond making -856 net ch
Please see the attached file for the fully formatted problems. 1. If a muscle tissue sample is 125 microns thick, what is the thickness in inches? (Given: 1 micron = 3.94 x 10^-5 inches) 3. If a patient is injected with 0.500 L of I.V. liquid, what is the volume in quarts? (Given: 1 quart = 0.946 L) 5. BONUS (4 pts): Exha
Please see the attached file for the complete problems. Problem 4.100. Select the more polar bond in each of the following pairs. Part A: C-C or C-O Part B: P-Br or P-Cl Part C: Si-S or Si-Cl Part D: F-Cl or F-Br Part E: P-O or P-S Problem 4.104 Classify each of the following bonds as nonpolar covalent,
Please see the attached file for the complete problems. Problem 4.36.Write the correct formula for the following compounds. Part A. aluminum chlorate Part B. ammonium oxide Part C. magnesium bicarbonate Part D. sodium nitrite Part E. copper(I) sulfate Problem 4.40. State the number of valence electrons,
State the chemical formula of salt and classify the bond as ionic, polar covalent, or non-polar covalent. A freshman is currently enjoying the Arts Studio program she is pursuing at a well-known university. In her free time, she likes to skate, take salsa dance lessons, and cook. She particularly enjoys pickling and decides to pickle olives over a leisurely weekend. According to the recipe, she needs to add three teaspoons of salt to one cup of diced olives. However, she erroneously adds six teaspoons instead. Each teaspoon of salt weighs about 5g and contains about 2,300 mg of sodium. Determine the amount of sodium that has been actually added, in grams.
A freshman is currently enjoying the Arts Studio program she is pursuing at a well-known university. In her free time, she likes to skate, take salsa dance lessons, and cook. She particularly enjoys pickling and decides to pickle olives over a leisurely weekend. According to the recipe, she needs to add three teaspoons of salt t
### Please refer to the actual attached document as everything is properly formatted and easier to see in the document. ### 1. For each of the following situations, identify those for which a reaction is likely to occur. For those that do occur, write a net ionic equation. a) A solution of lead(ll) nitrate mixed with a solut
Please see the attached file. 1. Answer the following problems about gases. a) The average atomic mass of naturally occurring neon is 20.18 amu. There are two common isotopes of naturally occurring Neon as indicated in the table below. (i) Using the information above, calculate the percent abundance of each isotope. (ii)
The 'normal' boiling point of a substance depends on the molecular mass, and the type of intermolecular attractions. Rank the following compounds in order of increasing boiling points, and describe the intermolecular forces which affect the ranking. a. H2Se b. H2S c. H2Te
The functional groups determine the reactivity of their molecules because of their ability to direct the interactions of the overall molecule. - Choose two functional groups from chapter 11 or 12. For each functional group find a household product that contains the functional groups you chose (e.g. fingernail polish remover c
1) What is the major product of dehydration of an alcohol? 2) Why does the simplest ketone have three carbon atoms and no fewer? 3) An alcohol has an OH functionality in it. Do you expect it to be a base? Why, or why not? 4) Name the following: a) CH3CH2CH(OH)COOH b) CH3OCH2CH2CH3 c) C4H9O(C=O)CH3 5) When acetic acid re
Calculate the following: (a) Moles of malachite in 1g: Cu2CO3(OH)2 Cu= 63.55 x 2=127.1 C= 12.01 O= 16 x 5= 80 H=1.008 x 2= 2.016 (b) Moles of CuO produced: .72 g CuO produced (c) Ratio of moles of CuO produced per moles of malachite decomposed 3. Use the mole ratio of CuO produced per mole of malachite
1) Which general formula applies to hydrocarbons with one double covalent between adjacent atoms? A. CnH2n+2 B. CnH2n C. CnH2n-2 D. CnH2n-4 E. CnH2n-6 2) The compound, 2-methyl-2-propanol, is an isomer of A. butane B. propane C. butanol D. propanol E. methanol 3) Which organic compound is an ele
1. Summarize in your own words the rules for writing Lewis electron-dot structures. Use and example of a simple molecule (not SO2, CO2, or H2O) to illustrate the application of these rules. NO3- . . 2. For the molecule you used in example in Question1 above, explain the reasoning in how the VSEPR theory would be used
The plant that I work at uses a zinc borate (US Borax) compound whose chemical formula is 2ZnO-3H2BO3-3.5H2O ----- essentially a hydrated mixture of zinc oxide, boric acid, and water to form the granular zinc borate.We use it as a wood preservative and must keep it in an insoluble form in our process chemistry. My question ho
Can you explain zeta potential in simple terms? If you haven't deduced by now, my study mates and I are all Chem Engineering grads from the early 80's and sadly have forgotten much of what we academically one knew....we are all now pursuing Master's degrees and it is a struggle re-learning much of this material. Also...we
Wood preservatives range from pentachlorophenol, to creosote, to chromated copper arsenate etc. etc. While most of these compounds are intended to deter rot and fungal decay of the wood, they also exhibit a significant water repellent characteristic? 1) What is it about these compounds that repels water? It may have something
The full electron configuration (1s^22s^2,etc..) for each of the following. Helium, Z = 2 Neon, Z = 10 Argon, Z = 18 Krypton, Z = 36 If you use the symbol of the previous noble gas to help indicate core electrons, help write the electron configuration for each of the following elements. Zirocnium, Z = 40 Vanadium, Z = 2
Could you please help me better understand the formation of aluminum hydroxide --- for instance: Again, lets assume we have a generally weak acid solution to which we add aluminum sulfate. The objective is to precipitate aluminum hydroxide per the following reaction which I believe to be correct. Al2(SO4)3 + HCO3- = 2Al(OH
The Law of Dulong and Petit states that the heat capacity per mole of many metals is approximately 6.0 calories per mole-degree C. Knowing that the specific heat capacity of three metals in Joules per gram-degree C is 0.45 for Fe, 0.24 fo Ag, and 0.13 for Au, do these metals agree with the law of Dulong and Petit? How do you kn
The conversion of diamond to graphite is a spontaneous reaction and has increasing entropy. Explain why this reaction is not observed in jewelry stores and what might need to be done to make it occur - assuming someone wanted to make graphite out of diamonds.
In phosphine, PH3, the H-P-H has angles at 93.6 degrees. Describe the bonding of the molecule per valence bond theory.
The measured dipole for a binary molecule is 0.53 D with a bond length of 219 pm. What is the separated charge, in coulombs? 1D = 3.34 X 10 TO POWER OF -30 C/M A. 8.08 X 10 to the power of -19 B. 8.08 x 10 to the power of -21 C. 2.42 x 10 to the power of -21 D. 1.38 x 10 to the power of -15 E. 3.88 x 10 to the power of
Which combination of elements would be most likely to form covalent bonds? a. lithium-flourine b. carbon-sodium c. carbon-flourine d. sodium-lithium e. sodium-flourine.
KrF4 is_______________? a. a polar molecule with five polar bonds b. a polar molecule with four bonds c. a non-polar molecule with two polar and two non-polar bonds d. a non-polar molecule with four non-polar bonds e. a non-polar molecule with four polar bonds.
1. Explain why some authors never write H+, but always write H3O+. 2. Any + ion in solution is attracted to the polar water molecules, but we often write Na+ ignoring the water. What is different about H+ that many chemists never write it alone? 3. Explain why choloracetic acid is a stronger acid than acetic acid.