Organic Chemistry Questions

A reaction between lead (II) nitrate and potassium iodide is a synthesis reaction single displacement reaction combustion reaction double displacement reaction

Is the following reaction endothermic or exothermic? H₂(g) + I₂(g) → 2HI + 21 kJ exothermic endothermic

Few chemical reactions are permanent. True False

Which set of numbers will correctly balance the given equation? Mg(NO3)₂(aq) + Na₂Cr₂O7(aq) → MgCr₂O7(s) +_ NaNO3(aq) -1, 1, 1, 2 1, 2, 2, 2 1,4, 1, 2 2, 1, 1, 4

A student is making a measurement with a metric ruler that can measure to the tenths of a centimeter. Which of the following would be the student's properly recorded measurement with this ruler? 47 cm 47.1 cm 47.13 cm 47.134 cm

If the ions Fe+2 and O-2 react, what ionic formula will result? Fe+2O-2 Fe²O2 FeO Fe³O²

Explain how iconic and covalent bonds are similar and how they are different. Give an example of two elements that would ionically bond, and two elements that would covalently bond.

Atom X has 27 protons, 29 neutrons, and 27 electrons. Atom Y has 27 protons, 30 neutrons, and 27 electrons. Atoms X and Y are _. isomers isobars isotopes isoelectronic

Determine the type of reaction shown and balance the equation. In addition, explain the process you used to balance the equation. Na + O₂ → Na₂O

Hund's Rule is being broken in which of the following orbital diagrams?

Which of the following statements is NOT part of Dalton's atomic theory? All matter is made up of atoms Atoms of two or more different elements combine to form compounds The nucleus of an atom is dense and positively charged Atoms are never created or destroyed during a chemical reaction

Which of the following is an ionic compound? NH3 CH4 Na₂O C12H22011

Calculate the density of a substance occupying a volume of 270.0 mL and having a mass of 120.5 g. 0.4463 g/mL 2.241 g/mL 3.254 x 104 g/mL 270.0 g/mL

Carry out the following calculations with the correct number of significant figures: 22.41 +0.523 + 26.4012 49.3342 49.334 49.33 49.3

Which of these is not suitable for the synthesis of 3-methyl butanoic acid? treat 1-bromo-2-methyl-propane with Mg, ether, than treat with CO2, then aqueous acid workup 3-methyl but-1-ene treated with B₂H6-THF, followed by H₂O₂ in NaOH; then treat with Na₂Cr₂O7 in aq. H₂SO4 4-methyl pent-1-ene treated with hot acidic KMnO4 2-bromo-3-methyl butane treated with NaCN followed by hydrolysis (H3O+, heat)

When multiplying or dividing measured numbers, we use the measurement with the least number of significant figures to determine the number of significant figures (sf) in our answer. For example: 3.5 cm x 4.75 cm = 17 cm² (even though the calculator gives 16.675) Solve the following problems assuming all are measured numbers. Report the correct number of significant figures. a. 7.00 x 15.00 = b. 40.21.901 = c. (0.003) (13.2) = d. 1.590 0.3975 =

Arrange in the increasing order of pka. 2-bromo-3-methyl-butanoic acid (A) 3-bromo-2-methyl butanoic acid (B) 2-ethyl-3-methyl butanoic acid (C) 2-chloro-3-methyl butanoic acid (D) A<B<D<C D<B<A<C D<A<B<C C<B<A<D

In chemistry the volume for a certain gas is given by V = 20T, where Vis measured in cc and T is temperature in °C. If the temperature varies from 70°C to 120°C, find the set of volume values. (Enter your answer using interval notation.)

Industrial agriculture requires A. no fertilizer B. large amounts of water C. no pesticides D. only renewable energy sources

What volume of hydrogen gas, at standard conditions (STP), can be liberated by the reaction of sulfuric acid with 0.067 g Mg? Write a balanced equation for the reaction? Determine the volume of H₂ liberated? In a different trial but same experiment, calculate the mass of magnesium metal that should be used to generate 50.0 mL of H₂ at standard conditions.

Refer to the following unbalanced equation: C6H14+ O2 CO2 + H₂O What mass of oxygen (O₂) is required to react completely with 19.5 g of C6H14? 5.93 × 10³ g 34.4 g 7.24 g 68.8 g 0.226 g

A chemist reacts 101.66 g of O2 and 25.47 g of C3H8 as shown below. O₂ + C3H8 --> CO₂ + H₂O Part a) Calculate the maxium mass of CO2 that can be produced. Part b) Identify the limiting reactant. Part c) Calculate the maximum mass of H2O that can be produced from this reaction. Part d) When complete, the reaction actually produced 38.95 g of H2O. Calculate the percent yield. Select all answer choices that apply to questions a-d. Note: calculated values are rounded to 2 decimal places.

A 1.9-mol sample of KCIO3 was decomposed according to the equation 2KCIO,(s)→2KC(s) + 30₂ (g) How many moles of O₂ are formed assuming 100% yield? 1.3 mol 1.6 mol 1.9 mol 1.0 mol 2.8 mol

What is the wavelength of light associated with an n=3@n=2 transition in a hydrogen atom, 443 nm 656 nm 091 nm 2.74 106 m 3.65-10-7 m-1

Determine the order of atomic radius that is correct for Ar, Na, Mg, Si, and P. Na > Mg > Si > P > Ar Si > P> Ar> Na > Mg Mg > Na > P > Si > Ar Ar > P > Si > Mg > Na Ar > Si > P > Na> Mg

For which of the following elements is gaining an electron the most energetically favorable (i.e., which has the most negative value of electron affinity)? H si Ar CI Fe

Which set of quantum numbers below describe the electron that is highest in energy. n=4, 1=2, m₁ = 2₁ mg = + ½ n= 1, 1 = 0, m₁ = 0, ms = + ½ n= 1, 1 = 0, m₁ = 0, ms = -1/2 n = 4,1 = 2, m₁= 3, mç = -1/2 n=3, 1=2, m₁ = 1, ms = +½

What is the valence electron configuration of a group 2 element. ns²np7 ns² ns¹ ns² np5 ns²np6

How many valence electrons are in an atom of gallium? three five one four two

What is the energy of green light with a wavelength of 542 nm 2.72 1018 J 2.72 1027 J 5.55 1014 J 3.68 10-28 J 3.68 10-19 J

The wavelength of light that has a frequency of 1.66 x 109 s-1 is 5.53 2.00 × 10-9 0.181 5.53 x 108 4.98 × 1017

1. When a sample of solid at 35°C (specific heat capacity = 0.89 J/g "C) is heated using 75.5J of energy, its temperature was raised to 48°C. What is the mass of this solid ? Give your answer using the correct significant figure

Select the most metallic element from the group below. sodium calcium barium cesium magnesium

Select the formula unit for the compound that consists of iron(II) and the phosphide ion. Fe₂P Fe3P2 FePO4 FeP2 FeP

How many orbitals are present in the n = 4 shell of an atom? 32 4 10 16 5

The ground-state electron configuration of the element is [kr]5s14d5. OTC OMn Mo cr Nb

Which of these elements has the highest first ionization energy? Rb Li Ne O F

Indicate the ground state electron configuration for aluminum. 15²2s²2p¹ 15²25²2p635¹3p² 15²25²20635² 15²25²2p63s²3pº 15²25²2635²3p¹

In which set of elements would all members be expected to have very similar chemical properties? Br, I, At Ne, Na, Mg P, Se, I Si, As, Te Cl, Br, Na

What is true below for an atom that is in its ground state electron configuration. Unpaired electrons in the same orbitals have opposite spins. Orbitals within a subshell are filled to maximize the pairing of electrons. Electrons are promoted to a higher-energy orbital before they are paired in the same orbital. Electrons fill higher-energy shells before filling lower-energy shells. Unpaired electrons in different orbitals have opposite spins.

How many moles of CO₂(g)are produced when 10 moles of O₂(g) react by the reaction C(s) +O₂(g)→→ CO₂(g) Assume all reactants and products are at the same temperature and pressure. 5 10 15 20

Which of the following is NOT a structural isomer of 2-methylpentane? 1. 1,2 dimethylbutane 2. hexane 3. 2,2-dimethylbutane 4. 2,2-dimethylpropane 5. 2 ethyl butane

The element with atomic number 30 is a transition element a non-metal a noble gas an alkali metal

Identify the atom with the ground-state electron configuration shown for its valence shell. 4s²3d¹04p6

The name 4-ethylpentane is not an accepted name for the compound described. What would be the correct name for this compound? 1. 2-ethylpentane 2. 4-methylhexane 3. 1-ethyl-1-methylbutane 4. 3-methylhexane 5. n-heptane

Starting with 2-bromobutane, which of the following reagents would you use to produce 1-butene as the major product? 1. 2. 3. 4. 1) CH₂CH₂ONA / CH₂CH₂OH 2) ((CH₂)CH)₂NLi / ether 3) CH₂SNa / acetone 4) CH₂CO₂Na/CH₂CO₂H

When CH3CCI is treated with excess phenylmagnesium bromide in ether, with subsequent aqueous work up, the resultant product: can undergo elimination with Kotbu can be oxidized by jones reagent can be reduced with Lithium aluminum hydride can undergo SN2 reaction to produce alkyl halide

The pk, of acetic acid, CH3COOH, is 4.76. What is the value of the equilibrium constant Keq, for the following equilibrium? Show work using the equation function from the menu above CH₂COOH + H₂O H₂00+ CH₂COO

To produce butyl benzene, what would be a correct approach? treat butyl chloride+AlCl3 with Benzene and then treat with H₂N-NH2 followed by NaOH Treat Benzene with Br2+FeBr3 then treat with Mg, ether, then treat with butanol treat butyl chloride +AICI3 with Benzene Treat CH3CH₂CH₂COCI + AICI3 with benzene and then treat it with Zn(Hg) HCI

Using the periodic table, what do you know about Indium? It is a large metal and likely to react with nonmetals. It is a small metal and unlikely to react with anything else It is a small nonmetal and likely to react with other metals It is a large nonmetal and unlikely to react with other metals It is a large nonmetal and likely to react with other nonmetals