General organic chemistry Questions and Answers

Does a reaction occur when aqueous solutions of potassium sulfide and nickel(II) nitrate are combined? If a reaction does occur, write the net ionic equation. Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds. Be sure to specify states such as (aq) or (s).

Assume that 6600 NaOH units were dissolved in a sample of water. How many units of Nations does the solution contain? How many units of OH ions does the solution contain?

Which definition best describes polygenic traits? A. traits that are carried on linked genes B. traits that are controlled by multiple genes C. traits that affect several features D. traits that express both alleles of a gene pair

Which one of the following is not one of the four "driving forces" that pull reactants to form products during chemical reactions? Gas evolution Water formation Solid formation Electron transfer Formation of a product

Balance the following reaction: (remember to include any 1's on appropriate compounds) C4H100₂+0₂ -CO₂ + H₂O

When the hydroboration oxidation of 2-methylbut-2-ene is carried out, the major product of the reaction will be a tertiary alcohol. secondary alcohol. primary alcohol. mixture of a primary and secondary alcohols.

Consider the structure of hex-3-ene. Which of the following statements describes this compound? The heat of combustion of the cis isomer is lower than that of the trans isomer. The cis isomer is more stable than the trans isomer. Conversion of the trans isomer to the cis isomer would have a negative AG. The cis isomer acts as a Lewis base while the trans isomer acts as a Lewis acid. Stereoisomerism is not possible for this substance.

Draw structures using wedges and hashed lines where necessary which fit the following descriptions: (16 points) (a) one isomer of 1,2,4-trimethylcyclohexane that is chiral: (b) two enantiomers of 2,3-butanediol as their line-angle formulas:

Which of the following molecules would exhibit cis-trans isomerism? 3-ethyl-5-methyloct-3-ene pent-2-ene but-1-ene 2,3-dimethylbut-2-ene Both pent-2-ene and 3-ethyl-5-methyl-3-ene

Thailanstatin A is a natural product that was isolated from Thailandensis burkholderia MSMB43, and has been studied for use as an anticancer agent. Answer the following questions related to this molecule. a. Circle and label all functional groups (Be sure to label any amines or alcohols as primary, secondary, or tertiary). b. Clearly label one primary carbon, one secondary carbon, and one tertiary carbon.

Provide the expected product for the reaction of each of the following alkenes with H₂SO4 and H₂O. If you expect a racemic mixture or an equimolar mixture of diastereomers, draw both stereoisomers. Draw the molecule(s) on the canvas by choosing buttons from the Tools (for bonds and charges), Atoms, and Templates toolbars. Show the appropriate stereochemistry by choosing the dashed or wedged buttons and then clicking a bond on the canvas.

You will require the following molecule diagrams for your individual assignment on Blackboard: Question: Functional groups Classify each of the following molecules according to it's functional group.

Consider the following cyclohexane a) Draw a chair conformation for the cyclohexane derivative above showing equatorial and axial positions at the carbon atoms bearing the substituents. b) Draw the flipped chair conformation showing axial and equatorial position at the carbon atoms that bear the substituents. Determine which structure is more stable (8a or 8b)? Describe and give your reasons.

What is the index of hydrogen deficiency for each of the following molecular formulas? C6H8O2 Express your answer as an integer.

Given the name, draw the structure of the following compounds. cis-6,7-dimethylcyclohepta-1,4-diene Draw the molecule on the canvas by choosing buttons from the Tools (for bonds and charges), Atoms, and Templates toolbars. Show the appropriate stereochemistry by choosing the dashed or wedged buttons and then clicking a bond on the canvas.

Compare 1-butene to butane. Which of the following would definitely be different between these two species? boiling point free bond rotation Both bond rotation and IHD. water solubility IHD

Rank the following carbocations from most stable to least stable. (Carbocations, like radicals, are electron deficient.)

If one wanted to convert 1-ethylcyclohexene to ethylcyclohexane, this could be accomplished by using which of the following reagents? HBr, H₂O2 H₂SO4, H₂O HBr H₂ and Pt catalyst.

Which of the following could probably not be produced by electrophilic addition of an alkene? 2-bromo-4-methylpentane 2-bromo-2-methylpentane 1-bromohexane 2-bromopentane

Which of these sentences with can or able to is grammatically correct? A) I not able to swim very fast. B) I can't swim very fast. C) I will be able swim very fast. D) I cannot to swim very fast.

How many moles of Care formed upon complete reaction of 2 mol of B according to the generic chemical reaction: A + 2 B-C

After reading/listening to "The Family Life of Lowland Gorillas" on page 4, doing the exercises, ad reading grammar explanations, answer these questions. When do we usually use Simple Present tense? A) For simple actions B) To describe routines and habits C) To present facts and general truths D) To describe temporary situations E) B ad C

Use the Internet or another resource to find out how the size of an atom compares with the size of its nucleus. Is the diameter of an atom 10 times, 1,000 times, or 100,000 times the diameter of the nucleus?

In the reaction shown below, how much of 1.15 M solution of AgNO3 is needed to completely react with 0.421 mol of magnesium chloride according to the equation: MgCl₂(aq) + 2 AgNO3(aq) → Mg(NO3)2(aq) + 2 AgCl(s) 0.968 L 0.484 L 36.6 mL 0.366 L 0.732 L

Carbon tetrachloride was widely used for many years as a solvent until its harmful properties became well established. Carbon tetrachloride may be prepared by the reaction of natural gas (methane, CH₂) and elemental chlorine gas in the presence of ultraviolet light. Choose the unbalanced chemical equation for this process. CH₂(g) + HI(g) → CCL (1) CHI(g) + O₂(g) → CCL (1) + HCl(g) CH. (g) → CCL (1) + HCl(g) CH₁ (9) + Cl₂(g) → CCL (1) + HCl(g)

Balance the following chemical equation: RbO₂ (s) + H₂O(l) → RbOH(aq) + O₂(g) + H₂O₂ (aq) 3RbO₂ (s) + H₂O(l) → RbOH(aq) +202 (9) + H₂O2 (aq) 4RbO₂ (s) + 6H2₂O(l) → 4RbOH(aq) + O₂(g) + 4H₂O₂ (aq) RbO₂ (s) + H₂O(l) → RbOH(aq) + O2(g) + H₂O₂(aq) RbO₂ (s) + 2H₂O(1)→ 5RbOH(aq) + O2(g) + H₂O₂ (aq) b Balance the following chemical equation: MgO(s) + HNO3(aq) → Mg(NO3)2 (aq) + H₂O(l) 5MgO(s) + 3HNO3(aq) → 5Mg(NO3)2 (aq) + H₂O(1) 2MgO(s) + 2HNO3(aq) → Mg(NO3)2 (aq) + 3H₂O(1) MgO(s) + HNO3(aq) → Mg(NO3)2 (aq) + H₂O(1) MgO(s) + 2HNO3(aq) → Mg(NO3)2 (aq) + H₂O(l) C Balance the following chemical equation: C3H8 (g) + O2(g) → CO₂(g) + H₂O(g) C3Hs (g) + 802(g) → 3CO₂(g) + H₂O(g) C3H8 (g) +502 (g) → 3CO2(g) + 4H₂O(g) C3Hs (9) + O2(g) → CO₂(g) + H₂O(g) C3Hs (g) + 802(g) → 3CO2(g) + 2H₂O(g)

Acetylene gas (C₂H₂) is often used by plumbers, welders, and glass blowers because it burns in oxygen with an intensely hot flame. The products of the combustion of acetylene are carbon dioxide and water vapor. Choose the unbalanced chemical equation for this process. C₂H₂(g) + H₂O(g) → CO₂(g) + O2(g) C₂H₂(g) + N₂(g) → CO₂(g) + H₂O(g) C₂H₂(g) + O₂(g) → CO₂(g) + H₂O(g) C₂H₂(g) → CO₂(g) + H₂O(g) + O2(g)

arbon tetrachloride was widely used for many years as a solvent until its harmful properties became well established, Carbon tetrachloride may be prepared by the reaction of natural gas (methane, CH,) and elemental lorine gas in the presence of ultraviolet light. Choose the unbalanced chemical equation for this process. CH₂(g) + HCl(g) → CCL (1) CH (9) + O2(g) → CCL (1) + HCl(g) CH (9)→ CCL (1) + HCl(g). CHI(g) + Cl₂(g) → CCL (1) + HCl(g)

Solid iron(II) oxide reacts with oxygen gas to produce solid iron(III) oxide. Balance the equation for this reaction (in lowest multiple integers). What are the formulas for the reactants and product?

Rubidium oxide is sometimes very challenging to store in the chemistry laboratory. This compound reacts with moisture in the air and is converted to rubidium hydroxide. If a bottle of rubidium oxide is left on the shelf too long, it gradually absorbs moisture from the humidity in the laboratory. Eventually, the bottle cracks and spills the rubidium hydroxide that has been produced. Choose the unbalanced chemical equation for this process. RbOH(s)→ Rb₂O(s) + H₂O(g) Rb₂O(s)→ RbOH(s) + H₂O(g) RbOH(s) + H₂O(g) → Rb₂O(s) Rb₂O(s) + H₂O(g) → RbOH(s)

The element tin often occurs in nature as the oxide SnO₂. To produce pure tin metal from this sort of tin ore, the ore usually is heated with coal (carbon). This produces pure molten tin, with the carbon being removed from the reaction system as the gaseous by-product carbon monoxide. Choose the unbalanced chemical equation for this process. Previous Page 4 of 12 SnO₂ (s) + O₂(g) + C(s) → Sn(1) + C(g) SnO₂ (s) + C(s) → Sn(l) + CO₂(g) SnO₂ (s) + CO(g) → Sn(1) + C(s) SnO₂ (s) + C(s) → Sn(1) + CO(g)

In addition to your regular PreLab: 1. Look up the boiling points for 2-methylcyclohexanol methylcyclohexene and 3-methylcyclohexene. (cis/trans mixture), 1- 2. Calculate the volume needed to acquire 0.1 mole of 2-methylcyclohexanol. You'll need to figure out the molar mass. The density is 0.94 g/mL.

Barium chloride is used in the manufacturing of pigments, and may be synthesized by direct combination of its constituent elements. Choose the unbalanced chemical equation for this process. BaO(aq)+Cl(g) → BaCl,(s) +0,(g) Ba(s) + Cl₂(g) → BaCl₂ (s) BaCl(s) + Cl₂ (9)→ BaCl₂ (8) Ba(s) + O₂(g) → BaCl₂ (s)

Butane gas (C4H10) burns in oxygen gas to produce carbon dioxide gas and water vapor. Balance the equation for this reaction (in lowest multiple integers). To check if you balanced the equation correctly, make sure the number of each type of atom totals the same on both sides of the equation.

The illustration on the left represents a mixture of H₂ (light blue) molecules and I₂ (purple) molecules. If these were to react to form HI molecules, what is the maximum number of HI molecules that could form?

Methanol (methyl alcohol), CH3OH, is a very important industrial chemical. Formerly, methanol was prepared by heating wood to high temperatures in the absence of air. The complex compounds present in wood are degraded by this process into a charcoal residue and a volatile portion that is rich in methanol. Today, methanol is instead synthesized from carbon monoxide and elemental hydrogen. Choose the balanced chemical equation for this latter process. 3H₂(g) + 2CO2(g) → 2CH3OH(g) 2H₂(g) + CO(g) → CH3OH(9) 2CH3OH(g) → 3H₂(g) + 2C(g) CH₂OH(g) → H₂(g) + 3CO(g)

For each pair, choose the combination of nucleophile and solvent that would give the faster SN2 reaction with ethyl iodide. Explain why. a. NaOCH₂CH3 in ethanol or NaOCH₂CH3 in DMSO. b. NaOCH₂CH3 in acetic acid or NaOCH₂CH3 in DMF.

The pure, natural enantiomer of (-)-menthol, has an specific rotation [a]20 = -50° (Formula: (A-B)/(A+B) = ee = ap20/[a]020 - show work!) a) What is the ee of a mixture of 1.50 g (+)-menthol and 3.50 g (-)-menthol? b) What is the rotation co2 of this mixture under standard conditions?

What is the molecular formula of oxybenzone?

Formic acid, HCOOH, is a weak electrolyte. What solute particles are present in an aqueous solution of HCOOH? Weak electrolytes such as formic acid (HCOOH) will be present mostly in solution in its neutral form, with only a small fraction dissociated into ions. For example, in a solution of acetic acid (CH3 COOH), only a small fraction is dissociated into H+ and CH3COO ions. Enter the chemical equation for the ionization of HCOOH.

C6H12O6 is an organic compound. Calculate its molar mass to 2 decimal spaces.

Identify the correct chair conformations of the following compound and then indicate which one is more stable. I and II are correct chair structures and I is most stable I and II are correct chair structures and II is most stable I and III are correct chair structures and III is most stable II and III are correct chair structures and II is most stable II and III are correct chair structures and III is most stable

A solution of NH2Br is rapidly made acidic and the [NH2Br] is followed as the reaction proceeds to form NHBr2. A plot of 1/[NH2Br] on the Y axis and time on the X axis is seen to be linear. a. The reaction is first order with respecct to NH₂Br. b. The reaction is zero order with respect to NH₂Br. c. The reaction is second order with respect to NH₂Br d. The reaction order cannot be determined in this manner. e. The [NHBr2] must be followed to determine the order in [NH2Br].

The presence of [Select] on the central atom is an indicator that the molecule is polar, if there are 3 or 4 electron regions. Two shapes that are always polar are bent and [Select]

Carbon-hydrogen bonds exhibit a range of different chemical reactivity that depends on molecular structure. Classify the C-H bonds at the carbons labeled a-c in the structure below. Possible classifications are: primary, secondary, & tertiary or none if there are no hydrogens at the labeled carbon.

The transformation above can be performed with some reagent or combination of the reagents listed below. Give the necessary reagent(s) in the correct order, as a string of letters (without spaces or punctuation, such as "EBF"). If there is more than one correct solution, provide just one answer.

Give the formula and name for the ionic compound formed from the combination of the indicated metal and carbonate, CO3 , a polyatomic ion. Express your answer as a chemical formula. formula: Spell out the full name of the compound.

CH3CH2CH2CH=CH2 Draw the molecule on the canvas by choosing buttons from the Tools (for bonds), Atoms, and Advanced Template toolbars. The single bond is active by default.

Draw two constitutional isomers that share the molecular formula C₂H5N. Your structures will have the same molecular formula but will have different connectivities. • Draw one structure per sketcher. Add additional sketchers using the drop-down menu in the bottom right corner. • Separate structures with + signs from the drop-down menu.

A piece of metal weighing 59.047 g was heated to 100.0 °C and then put it into 100.0 mL of water (initially at 23.7 °C). The metal and water were allowed to come to an equilibrium temperature, determined to be 27.8 °C. Assuming no heat lost to the environment, calculate the specific heat capacity of the metal.