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chemistry
organic chemistry

Questions and Answers of Organic Chemistry

Draw a potential-energy diagram for a molecule such as Cl2. Indicate the bond length (194 pm) and the bond dissociation energy (240 kJ/mol).
Write Lewis formulas for the following: a. AlCl4 b. AlF63 c. BrF3 d. IF6+
Give resonance descriptions for the following: a. SeO2 b. N2O4
Give resonance descriptions for the following: a. CH3NO2 b. C2O42
The compound S2N2 has a cyclic structure with alternating sulfur and nitrogen atoms. Draw all resonance formulas in which the atoms obey the octet rule. Of these, select those in which the formal
Acetic acid has the structure CH3CO(OH), in which the OH group is bonded to a C atom. The two carbon–oxygen bonds have different lengths. When an acetic acid molecule loses the H from the OH group
The atoms in N2O5 are connected as follows:No attempt has been made here to indicate whether a bond is single or double or whether there is resonance. Obtain the Lewis formula (or formulas). The
Methyl nitrite has the structureNo attempt has been made here to indicate whether a bond is single or double or whether there is resonance. Obtain the Lewis formula (or formulas). The N€“O
Use bond energies to estimate ∆H for the reaction H2(g) + O2(g) → H2O2(g)
Use bond energies to estimate ∆H for the reaction 2H2(g) + N2(g) → N2H4(g)
Use bond energies to estimate ∆H for the reaction N2F2(g) + F2(g) → N2F4(g)
Give an example of a molecule that has a coordinate covalent bond.
Use bond energies to estimate ∆H for the reaction HCN(g) + 2H2(g) → CH3NH2(g)
Compare the properties of an ionic material such as sodium chloride with a room temperature ionic liquid. Explain this difference.
What advantages does using an ionic liquid as a solvent have over using an organic solvent?
Explain the decomposition of nitroglycerin in terms of relative bond energies.
What property of a chemical bond gives rise to the infrared spectrum of a compound?
What kind of information can be obtained about a compound from its infrared spectrum?
The octet rule correctly predicts the Lewis formula of many molecules involving main group elements. Explain why this is so.
Give the symbol of an atomic ion for each of the following electron configurations: a. 1s22s22p63s23p6 b. 1s22s22p63s23p64s1 c. 1s22s22p63s23p63d8 d. 1s22s22p63s23p63d104s2 e.
Draw resonance structures for the azide ion, N3, and for the nitronium ion, NO2+. Decide which resonance structure is the best description of each ion.
Consider hypothetical elements X and Y. Suppose the enthalpy of formation of the compound XY is –336 kJ/mol, the bond energy for X2 is 414 kJ/mol, and the bond energy for Y2 is 159 kJ/mol. Estimate
Nitrous oxide, N2O, has a linear structure NNO. Write resonance formulas for this molecule and from them estimate the NN bond length in the molecule. Use the data in Example 9.12. Example
Phosphorous acid, H3PO3, has the structure (HO)2PHO, in which one H atom is bonded to the P atom, and two H atoms are bonded to O atoms. For each bond to an H atom, decide whether it is polar or
Hypophosphorous acid, H3PO2, has the structure (HO)PH2O, in which two H atoms are bonded to the P atom, and one H atom is bonded to an O atom. For each bond to an H atom, decide whether it is polar
An ionic compound has the following composition (by mass): Mg, 10.9%; Cl, 31.8%; O, 57.3%. What are the formula and name of the compound? Write the Lewis formulas for the ions.
An ionic compound has the following composition (by mass): Ca, 30.3%; N, 21.2%; O, 48.5%. What are the formula and name of the compound? Write the Lewis formulas for the ions.
A gaseous compound has the following composition by mass: C, 25.0%; H, 2.1%; F, 39.6%; O, 33.3%. Its molecular mass is 48.0 amu. Write the Lewis formula for the molecule.
A liquid compound used in dry cleaning contains 14.5% C and 85.5% Cl by mass and has a molecular mass of 166 amu. Write the Lewis formula for the molecule.
A compound of tin and chlorine is a colorless liquid. The vapor has a density of 7.49 g/L at 151°C and 1.00 atm. What is the molecular mass of the compound? Why do you think the compound is
A compound of arsenic and fluorine is a gas. A sample weighing 0.100 g occupies 14.2 mL at 23°C and 765 mmHg. What is the molecular mass of the compound? Write the Lewis formula for the molecule.
Calculate the enthalpy of reaction forHCN(g) †’ H(g) + C(g) + N(g)from enthalpies of formation (see Appendix C). Given that the C€“H bond energy is 411 kJ/mol, obtain a value for
Assume the values of the C€“H and C€“C bond energies given in Table 9.5. Then, using data given in Appendix C, calculate the C=O bond energy in acetaldehyde,Compare your result
According to Pauling, the A–B bond energy is equal to the average of the A–A and B–B bond energies plus an energy contribution from the polar character of the bond: BE(A–B) = 1/2 [BE(A–A) +
Because known compounds with N€“I bonds tend to be unstable, there are no thermodynamic data available with which to calculate the N€“I bond energy. However, we can estimate a
Using Mulliken€™s formula, calculate a value for the electronegativity of chlorine. Use values of the ionization energy from Figure 8.18 and values of the electron affinity from Table 8.4.
Using Mulliken€™s formula, calculate a value for the electronegativity of oxygen. Convert the result to a value on Pauling€™s scale. See Problem 9.139.Problem 9.139Using
What is a resonance description of a molecule? Why is this concept required if we wish to retain Lewis formulas as a description of the electron structure of molecules?
Describe the kinds of exceptions to the octet rule that we encounter in compounds of the main-group elements. Give examples.
What is the relationship between bond order and bond length? Use an example to illustrate it.
Define bond energy. Explain how one can use bond energies to estimate the heat of reaction.
a. Consider a metal atom, which we will give the symbol M. Metal M can readily form the M+ cation. If the sphere on the left below represents the metal atom M, which of the other three spheres would
When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule:X(g) + X(g) → X2(g)a. Would you predict that this reaction is exothermic or
You land on a distant planet in another universe and find that the n = 1 level can hold a maximum of 4 electrons, the n = 2 level can hold a maximum of 5 electrons, and the n = 3 level can hold a
Which of the following represent configurations of thallium ions in compounds? Explain your decision in each case. a. Tl2+ [Xe]4f145d106p1 b. Tl3+ [Xe]4f145d10 c. Tl4+ [Xe]4f145d9 d. Tl+
Below on the left side are models of two atoms, one from a metal, the other from a nonmetal. On the right side are corresponding monatomic ions of those atoms. Decide which of these ions is the
Predict a possible monatomic ion for Element 117, Uus. Given the spherical models below, which should be labeled €œatom€ and which should be labeled €œion€?
Examine each of the following electron-dot formulas and decide whether the formula is correct, or whether you could write a formula that better approximates the electron structure of the molecule.
Explain what energy terms are involved in the formation of an ionic solid from atoms. In what way should these terms change (become larger or smaller) to give the lowest energy possible for the solid?
For each of the following molecular models, write an appropriate Lewis formula.
For each of the following molecular formulas, draw the most reasonable skeleton structure. a. CH2Cl2 b. HNO2 c. NOF d. N2O4 What rule or concept did you use to obtain each structure?
Below are three resonance formulas for N2O (nitrous oxide). Rank these in terms of how closely you think each one represents the true electron structure of the molecule. State the rules and concepts
Sodium, Na, reacts with element X to form an ionic compound with the formula Na3X.a. What is the formula of the compound you expect to form when calcium, Ca, reacts with element X?b. Would you expect
The enthalpy change for each of the following reactions was calculated using bond energies. The bond energies of X–O, Y–O, and Z–O are all equal.X–X + O=O → X–O–O–X; ∆H = –275
Write Lewis symbols for the following: a. P b. P3 c. Ga d. Ga3+
Write Lewis symbols for the following: a. Br b. Br c. Sr d. Sr2+
Use Lewis symbols to represent the transfer of electrons between the following atoms to form ions with noble-gas configurations: a. Ca and Br b. K and I
Use Lewis symbols to represent the electron transfer between the following atoms to give ions with noble-gas configurations: a. Mg and S b. Ba and I
For each of the following, write the electron configuration and Lewis symbol: a. As b. As3+ c. Se d. Se2
Define lattice energy for potassium bromide.
For each of the following, write the electron configuration and Lewis symbol: a. In b. In c. K+ d. I
Give the electron configurations of Ni2+ and Ni3+.
Give the electron configurations of Cu+ and Cu2+.
Arrange the members of each of the following pairs in order of increasing radius and explain the order: a. Sr, Sr2+ b. Br, Br
Arrange the members of each of the following pairs in order of increasing radius and explain the order: a. Te, Te2 b. Al, Al3+
Which has the larger radius, N3 or P3? Explain. (You may use a periodic table.)
Why do most monatomic cations of the main-group elements have a charge equal to the group number? Why do most monatomic anions of these elements have a charge equal to the group number minus eight?
Arrange the following in order of increasing ionic radius: Cl, Na+, and S2. Explain this order. (You may use a periodic table.)
Use Lewis symbols to show the reaction of atoms to form hydrogen selenide, H2Se. Indicate bonding pairs and lone pairs in the electron-dot formula of this compound.
Use Lewis symbols to show the reaction of atoms to form arsine, AsH3. Indicate which electron pairs in the Lewis formula of AsH3 are bonding and which are lone pairs.
Assuming that the atoms form the normal number of covalent bonds, give the molecular formula of the simplest compound of arsenic and bromine atoms.
Assuming that the atoms form the normal number of covalent bonds, give the molecular formula of the simplest compound of silicon and chlorine atoms.
Using a periodic table (not Figure 9.15), arrange the following in order of increasing electronegativity: a. P, O, N b. Na, Al, Mg c. C, Al, Si
With the aid of a periodic table (not Figure 9.15), arrange the following in order of increasing electronegativity: a. Sr, Ca, Rb b. Ca, Ge, Ga c. Se, As, Sb
Arrange the following bonds in order of increasing polarity using electronegativities of atoms: P–O, C–Cl, As–Br.
Decide which of the following bonds is least polar on the basis of electronegativities of atoms: H–N, Si–Br, N–Cl.
Indicate the partial charges for the bonds given in Problem 9.57, using the symbols δ+ and δ–. Problem 9.57 Arrange the following bonds in order of increasing polarity using electronegativities
The 2+ ions of transition elements are common. Explain why this might be expected.
Indicate the partial charges for the bonds given in Problem 9.58, using the symbols δ+ and δ–. Problem 9.58 Decide which of the following bonds is least polar on the basis of electronegativities
Write Lewis formulas for the following molecules: a. Br2 b. H2S c. NF3
Write Lewis formulas for the following molecules: a. NOCl b. PBr3 c. IF
Write Lewis formulas for the following molecules: a. P2 b. COBr2 c. HNO2
Write Lewis formulas for the following molecules: a. CO b. BrCN c. N2F2
Write Lewis formulas for the following ions: a. ClO b. SnCl3 c. S22
Write Lewis formulas for the following ions:a. IBr2+b. ClF2+c. CN
Write resonance descriptions for the following:a. HNO3b. SO3
Write resonance descriptions for the following:a. NO2b. FNO2
Use resonance to describe the electron structure of nitromethane, CH3NO2. The skeleton structure is
Explain how ionic radii are obtained from known distances between nuclei in crystals.
Give the resonance description of the formate ion. The skeleton structure is
Write Lewis formulas for the following:a. XeF2b. SeF4c. TeF6d. XeF5+
Write Lewis formulas for the following:a. I3b. ClF3c. IF4d. BrF5
Write Lewis formulas for the following:a. BCl3b. TlCl2+c. BeBr2
Write Lewis formulas for the following:a. AlI3b. BeCl2c. BeF3
Write a Lewis formula for each of the following, assuming that the octet rule holds for the atoms. Then obtain the formal charges of the atoms.a. O3b. COc. HNO3
Write a Lewis formula for each of the following, assuming that the octet rule holds for the atoms. Then obtain the formal charges of the atoms. a. ClNO b. POCl3 c. N2O (NNO)
For each of the following, use formal charges to choose the Lewis formula that gives the best description of the electron distribution: a. SOF2 b. H2SO3 c. HClO2
For each of the following, use formal charges to choose the Lewis formula that gives the best description of the electron distribution: a. ClO2F b. SO3 c. BrO3
Describe the trends shown by the radii of the monatomic ions for the main-group elements both across a period and down a column.
Calculate the bond length for each of the following single bonds, using covalent radii (Table 9.4):a. C€“Hb. S€“Clc. Br€“Cld. Si€“O

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