For each of the following statements, provide a detailed explanation: a. The Cl- ion is larger than the Cl atom b. The S2- ion is larger than the O2- ion c. The K+ ion is larger than the Ca2+ ion
Automotive air bags inflate when sodium azide(NaN3) decomposes explosively to its constituent elements according to the equation: 2NaN3(s) ---------> 2Na(s) + 3N2 How many moles of N2 are prodeuce by the decomposition of 2.50 moles of NaN3 and how many grams of NaN3 are required to form 6.00 g of N2 gas?
How do you estimate the percentage covalent nature of different compounds using the Pauling's Electronegativity Scale? Using Pauling's Electronegativity Scale, estimate the percent covalent nature of the following compounds: i) MgO ii) Al2O3 iii) SiO2 iv) Si3N4 v) SiC.
1. Four metals are tested: A,B,C,D. If A is more active than C and C is more active than B, is it necessary to test A and B? Explain your answer. 2. You observe that when copper is added to a solution containing gold ions, the copper dissolves and the gold precipitates. Similarly, almost all other metals will displace gold fr
Consider two metals: M and N. A strip of solid N is placed into 2mL of a 0.10 M M(NO3)2 solution. The solution changes from blue to green and the solid appears tarnished after time. a) What color is M(2+) b) What color is N(2+) C Which species is a better oxidizing agent, M or N? d) Which species is a better reducing agent
1. Use the VSEPR model to predict the probable shapes of (a) PCl4+, (b) PCl4-, (c) AsCl5. 2. Give balanced chemical equations for each of the following reactions. (a) Oxidation of P4 with excess oxygen, (b) reaction of the product from part (a) with excess water, (c) reaction of the product from part (b) with a solution o
E. Balance the equation for the disproportionation of sulfur into sulfide and thiosulfate (symbol in attachment) in base. Determine if the reaction spontaneous. Second question also present in the attachment.
1. Draw the Lewis structures of diphenylsilanediol and of the tetramer of diphenylsiloxane. Need not attempt to draw resonance structures involving the electrons in the phenyl groups. 2. Describe the geometry and hybridization of the silicon atoms, oxygen atoms, and carbon atoms in diphenylsilanediol and the tetrameric form dip
1. Identify the conjugate acids of the bases C5H5N (pyridine), HPO42-, O2-, CH3COOH, [Co(CO)4]-, CN-. 2. Use Pauling's rules to place the following acids in order of increasing acid strength: HNO2, H2SO4, HBrO3, and HClO4 in a nonlevelling solvent. 3. Which member of the following pairs is the stronger acid? Give reasons for t
1. Calculate the concentration of the HCl(aq) solution ( 25mL of .1M unstandardized HCl solution, 2 drops of phenolphthalein indicator used. Titrated with 15.2mL of sodium hydroxide solution) 2. Calculate the concentration of the Na2B4O7 solution two ways a) From the HCl titration of the Na2B4O7 solution ( 10mL of ~0.07M u
Synthesis and Characterization of Mo2(O2CCH3)4 and K4Mo2Cl8: Compounds that contain Metal-Metal Quadruple bonds. Procedure Place 2.0g of molybdenum hexacarbonyl and .10g of trimethylamine-N-oxide and a few boiling chips in the three-neck flask. Lightly grease the center neck of the flask and attach the reflux condenser t
The difference between Kc and Kp is confusing to me. Can you show me the difference to me if at 35 degrees C when the vapor pressure of water is 0.0555 atm what is the Kc and the Kp. Thank you H2O(l)= H2O(g)
1. Complete and balance the following reactions. CaO(s) + H2O(l) → Mg(s) + H2O(l) ⎯⎯Δ→ Na(s) + xss O2(g) ⎯⎯Δ→ 2. V. Deduce the oxidation state of the metal centers in the following 3 compounds. SrO2 Li3N K2S2
Using the molecular weight, density and crystal structure from your periodic table determine the metallic radius R of Cesium.
The following 5 problems concern electron configuration, the shape of orbitals, and calculation of Bohr wavelengths. Please see the attached file for the fully formatted problems. 1. A hydrogen atom in a certain excited state has its electron in a 5f subshell. The electron drops down to the 3d subshell, releasing a photon in
Could you please write the electron configuration for the following substance, using the orbital notation. Bromine(Br)
Describe the patterns in the electronic configurations of the elements. Each row across the periodic table is called a period and the elements gradually change properties from left to right. Can you explain this in terms of the electronic configurations? Each column of the periodic table is called a family. Elements in t
Lab Experiment: Interactive Valence Shell Electrons 1. You will need a bag of colored candies such as "Skittles" or "M&M" You should have at least 80 pieces of this candy. You will also need eighteen index cards. Nine sheets of notebook paper torn in half will work as well as index cards. 2. Separate the candies by color.
The question arises concerning the density of saltwater: is it because water molecules have moved out of the system, replaced by sodium and chlorine ions, which are heavier, or have the ions moved into the interstices, creating a greater number of particles in the solution? By the gas laws, a cubic meter of gas always maintain
Chlorine gas can be prepared in the laboratory by the reaction of manganese dioxide with hydrochloric acid: MnO2(s) + 4HCl(aq) --> MnCl2(aq) + 2H2O(l) + Cl2(g) How much MnO2 should be added to excess HCl to obtain 275mL of chlorine gas at 5.0C and 650 mmHg?
Count the number of valence electrons associated with each metal in the list below. Determine if they obey the 18-electron rule. If they violate the 18-electron rule, comment on the stability/reactivity of the complexes. a) [V(CO)6] b) cis-[Rh(Br)(CO)2(PPh3)] c) [Fe2(CO)4(Cp)2] d) [Mn(CO)5(CH3)].
1. Write a balanced net ionic equation for the reaction of each of the following compounds with water. (a.) Na3PO 4 (b.) NaHSO4 (c.) (CH3)3NHCl 2. The following species are amphiprotic. Write the formulas of the corresponding conjugate acids and bases: (a.) HSe- (b.) PH3 (c.) HPO32- 3. For each of the following nona
How could you separate tellurium dioxide, TeO2 from silicon dioxide SiO2?
Use the Solubility Rules to write net ionic equations for the reactions that occur when solutions of the following are mixed. Instructions 1. Write reactants and products in the following order: Cation + Anion = Precipitate 2. Use "->" (hyphen + greater than) to indicate 'yields' 3. Write subscripts as numbers with no
Write the electron configuration for Ba, atomic number 56.
For AgCl, what will occur if 250ml of 1.5 A 10^-13 M of NaCl is mixed with 250mL of 2.0 A 10^-7 M of AgNO3? a. A precipitate would form because Ksp>P b. A precipitate would form because P>Ksp c. No precipitate would form because Ksp>P d. No precipitate would form because P>Ksp e. No precipitate would form because P=Ksp
How many geometric isomers exist for Cu(en)Br2?
The formation constant for Cu(NH3)4(exponent 2 positive) is 2x10(exponent 12). What is the ratio of Cu(NH3)4(exponent 2 positive) to Cu(exponent 2 positive) in 0.1M NH3?
The crystal field splitting energy for TiF6^-3 is 203 kJ/mol. At what wavelength does the maximum absorbance of light occur for this complex?
Question: Determine the number of unpaired electrons in an octahedral, strong-field Co(exponent positive 2) complex ion.