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Q: Define ionization enthalpy and electron gain enthalpy?
A: Ionization enthalpy and electron gain enthalpy are defined as:
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A: Mass of KOH = 128 mg1mg = 10-3 gMass of KOH = 0.128 gMolar Mass of KOH = 56.1 g/molMoles of KOH =…
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A: pOH of sodium hydroxide = 2.46 pH of sodium hydroxide = ?
Q: -NH2 но NH b. OH
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Q: What is the degree of ionization (i) for U(OH)6(aq)? A) 1 B) 2 C) 3 D) 7 E) 13
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A: Oxyacids are the compounds that have an oxygen atom bonded to a hydrogen atom and another atom, X.…
Q: Explain protonation of HNO3 ?
A: The protonation of HNO3 has to be explained below.
Q: Write a Lewis diagram for I-3, the linear (tri-iodide) ion.
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Q: Explain the Lewis definition of bases ?
A: Lewis acid - an electron pair acceptor species (i.e., an electrophile having vacant orbitals).
Q: Rank the following acids in order of increasing strength: ClCH2SH, CH3SH, H2S.
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Q: List the acids containing the group 7 elements HF, HCl, HBr and HIin order of increasing bond length…
A: The acids given are HF, HCl, HBr and HI.
Q: In the following reaction, identify the Lewis acid. Co** (ag) + 6NH3 (ag) - Co(NH3),**(aq)
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Q: The elements sodium, aluminum, and chlorine are in the same period.(a) Which has the greatest…
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Q: 2. Which of the following is expected to be a neutral compound in terms of acid-base behavior in…
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- Among the following Lewis acids, which has the maximum electron-acceptor character? (a) PCl3 (b) PCl,R (c) PF3 (d) PCIR,The molecule (CH3)2N-PF2 has two atoms that can act as Lewis bases. With boron compounds, BH3 attachesto phosphorus, while BF3 attaches to nitrogen. Give your reasoningThe elements sodium, aluminum, and chlorine are in the same period. (a) Which has the greatest electronegativity? (b) Which of the atoms is smallest? (c) Which is the largest possible oxidation state for each of these elements? (d) Will the oxide of each element in the highest oxidation state (write its formula) be acidic, basic, or amphoteric?
- 6. Acids and bases are defined by their donation or acceptance of a proton according to the (a) Arrhenius model. (b) Bronsted-Lowry model. (c) Lewis model.18. (a) Molecule N₂H4 (1) + 2 H₂O2 (1) → N2(g) + 4 H₂O (1) Complete the following table: Lewis Dot Structure (use dots or lines to show bonds) (b) (c) (d) N₂H4 H₂O2 N₂ H₂O Calculate the AH°rxn using average bond energies (Table 9.4 in textbook) Calculate the AH°rxn using the standard enthalpies of formation (Appendix 2 in textbook) Why are these two values slightly different?Ammonium chloride, NH4Cl, is a very soluble salt in water.(a) Draw the Lewis structures of the ammonium and chlorideions. (b) Is there an N—Cl bond in solid ammonium chloride?(c) If you dissolve 14 g of ammonium chloride in 500.0 mLof water, what is the molar concentration of the solution?(d) How many grams of silver nitrate do you need to add tothe solution in part (c) to precipitate all of the chloride as silverchloride?
- state whether each of the statement is true or false. Justify your answer in each case(a) sulphuric acid is a monoprotic acid.(b) HCL is a weak acid.(c) methanol is a base.Boric acid, B(OH)3, is an acid that acts differently from the usual Brønsted-Lowry acids. It reacts with water according to B(OH);(aq) + 2 H,0(€)2B(OH), (aq) + H;O* (aq) K, = 5.8 × 10¬10 (a) Draw Lewis structures for B(OH); and B(OH)4. Can these be described as Lewis acids or Lewis bases? (b) Calculate the pH of a 0.20 M solution of B(OH)3(aq).Why is (CH3)3Cl considered to be a Lewis Acid?
- Each of the chemically active Period 2 elements forms stable compounds in which it has bonds to fluorine. (a) What are the names and formulas of these compounds? (b) Does ∆EN increase or decrease left to right across the period? (c) Does percent ionic character increase or decrease left to right? (d) Draw Lewis structures for these compoundsExplain which is the stronger acid, H3PO4 or H2SO3; CCl3CH2COOH or CCl2FCH2COOH. [Draw possible Lewis structure models]The sulfate ion can be represented with four S-O bonds or with two S-O and two So=O bonds.(a) Which representation is better from the standpoint of formal charges?(b) What is the shape of the sulfate ion, and what hybrid orbitals of S are postulated for the σ bonding?(c) In view of the answer to part (b), what orbitals of S must be used for the π bonds? What orbitals of O?(d) Draw a diagram to show how one atomic orbital from S and one from O overlap to form a π bond.