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Recently Asked Inorganic Chemistry Questions

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Q1:6. Li₂ has electron. 02s 02s* ¹2p ¹2p о2р л р* П2р* 2p* Li₂+ () () 0 0 0 0 0 0 As a result of how the electrons fill the MO diagram, the bond order is meaning that the bond between Li and Li isbond. There is _unpaired electron.See Answer
Q2:1. The nitrosyl ion, NO+, has electrons. 02s 02s 2p 2p 02p 02p NO+ () () () () () () () () As a result of how the electrons fill the MO diagram, the bond order is meaning that the bond between the N and the O is a bond. There are unpaired electrons.See Answer
Q3:1. The nitrosyl ion, NO+, has electrons. 02s 02s 2p 2p 02p 02p NO+ () () () () () () () () As a result of how the electrons fill the MO diagram, the bond order is meaning that the bond between the N and the O is a bond. There are unpaired electrons.See Answer
Q4:14 12 10 8 6 4 20 pka1 pka2 V₁ + V₁ N -V₁ V₂ Volume of base added Figure 9.2: pH versus Volume of titrant plot for phosphoric acid pKa values, i.e. pka1, pKa2 and pKa3. The titration curve would be expected to show three corresponding steep rises. However, in practice only two sharp rises are detected. The shape of the expected pH versus Volume of titrant for the titration of phosphoric acid is shown in Figure 9.2. unpex This plot shows two endpoints V₁ and V₂. As before pKa values can be determined by reading the pH values at the volumes corresponding to half neutralisation. As shown in Figure 9.2, pkai is the pH of the solution at the volume and pKa2 is the pH of the solution at the volume V₁ + V2V₁(= V₁+V/₂). epede Calibra side of Take mark Swirl Rep NaO sults/nTable 2: Change in pH on addition of 0.1 M NaOH to 50 cm³ sample of 0.05 M H3PO4 pH Volume of NaOH PH added (cm³) Volume of NaOH added (cm³) 2.0 H-O 6.0 10-0 12.0 14 O 16-0 18-0 20.0 22.0 24-0 26.0 28-0 30-0 32.0 34.0 From graph: Equivalence point 1: Half-equivalence point 1: pka1: Kat (show calculation): 1.78 179 1.89 2.08 2.21 2.46 3.00 4.91 5.66 6.05 6.29 6.49 682 7.69 9.70 10.19 10.38 10-52 2.0 4.0 6.0 8.0 10.0 12-0 14.0 16.0 16.5 17.0 17.5 18.0 18.5 19.0 F1.5 20.0 20-5 21.0 1.79 2.39 2.25 pka2: Ka2 (show calculation): Equivalence point 2: Half-equivalence point 2: 2.32 2.5H 3.02 3.99 5.72 5.86 5.97 $6.04 6-11 6.18 6.22 6.29 6.35 6.39 6.46/nDATA SHEET Table 1: Change in pH on addition of 0.1 M NaOH to 50 cm³ sample of 0.1 M CH₂COOH Volume of NaOH pH added (cm3) e revoo oneloitt 501 Jor дел 2:0 за но 10.0 12.0 TH O льо en qmets PH 18.0 2010 22.0 26:0 30.0 32.0 From graph: Equivalence point: Half-equivalence point: рка: Ka (show calculation): 2 70 3 90 З'Но 3:66 383 3-98 bio наа h35 тва 483 5 io 5.36 10 31 10.59 10.H9 Volume of NaOH added (cm3) до во 10.0 10 IN.O JH.S 15.0 15:5 16.0 16.5 17.0 17:5 180 19.0 За 3:46 3.68 3:86 3.99 ня наб ная н:33 4.36 4-39 Н.Н3 Н.НЗ 4 50 H.SS 4.58 нь3See Answer
Q5:1) 40 points total with 8 points for each question: Sodium hydride has the same crystal structure as the table salt NaCl is shown in the figure with the positions of the ions in the cubic unit cell as the followings: Nat (0 0 0) (1/2 1/2 0) (1/2 0 1/2) (0 1/2 1/2) H- (0 1/2 0) (1/2 0 0) (0 0 1/2) (1/2 1/2 1/2). Chloride ion Sodium ion Approximate the Debye-Waller factor as 1, a) Calculate the squared structure factor |F(T)² at T =(hkl) in analytic form for neutron Bragg diffraction when common 'H is contained in the hydride. b) Repeat to get the analytic squared structure factor when ID is used to synthesize the hydride. c) Calculate the Bragg powder diffraction intensity mF(T)² at T =(111) and (200) for NaH and NaD. Pay attention to the multiplicity of the Bragg peaks. d) Take the diffraction patterns on page 10 of the Lecture 6, now take 30min to count each data point, what will be the peak counts at (111) and (200) for NaH and NaD and what will be their standard deviations? e) Similarly, estimate the background intensity with the error bar at (111) and (200), then give the peak intensity (peak value-background) of them with the error bar for NaH and NaD. Are the intensity ratio I(111)/(200) consistent with your theoretic values for the two materials?See Answer
Q6: Lab 5 Post-Lab - Properties of CO2 and the Determination of NaHCO3 (2pts) Determination of Carbon Dioxide How will you collect data for this experiment? virtually Mass of system before reaction (g) Mass of system after reaction (g) Temperature CO2(g) in °C Atmospheric pressure in lab (mmHg) Volume (mL) CO₂(g) Data 95-740 95.500 25.0 756 124.7 (7pts) Calculations Calculations Mass of CO2 gas (g) Volume of CO₂ (L) Density CO2 (g/L) Calculations (0/1pts) 1.State the theoretical density of CO2 (g/L) and then state the temperature and pressure of this value in the essay field below. Also, include the source of your value. 2.State the temperature and pressure of your theoretical density value, includind the source of your value 3.Calculate the percent error of your density. (8pts) Molar mass carbon dioxide Calculate the molar mass of CO2 using the ideal gas law and mass of CO2. Use the true gas constant, o.08206 L-atm/mol·K. To determine the vapor pressure of water, use this table. Molar mass of CO2 Calculations Vapor pressure of water in (mmHg) Partial pressure of CO2 (torr) Partial pressure of CO2 (atm) Temperature of CO2 (K) Moles of CO2 Experimental Molar mass CO2 (g/mol) Theoretical Molar mass CO2 (g/mol) Percent Error (6pts) Post-lab Questions (pending/2pts) 1. Describe how close your experimental values were to the actual values for density and molar mass. Saved (pending/2pts) 2. Explain two possible reasons for the differences between your values and the actual values. (pending/2pts) 3. If the percent errors were different for density and molar mass, give one possible reason for why one was closer than the other. Saved (10pts) Part 2 - Determination of the Purity of a Sodium Bicarbonate Sample Report (pending/10pts) Upload the group report here. It should include the following: Header information 1. 2. Problem being solved 3. Summary of the procedure 4. Detailed procedure 5. Data table for Part 2 (including units) 6. 7. 8. Statement of % Purity of the sample Discussion of your answer with evidence Answer to the neutralization reactionSee Answer
Q7: Exploring the Correlation Between d-Orbital Splitting and Ligand Identity in Chromium(III) Complexes and Metal Ion Identity in First-Row Transition Metal Complexes By: Vicky Villarosa Reference: This procedure was adapted from the “Analysis of d-orbital splitting in transition metal complexes Part I: UV-Vis spectroscopy Lab Procedure," "Analysis of d-orbital splitting in transition metal complexes Part II: Magnetic susceptibility Lab Procedure,” and the “Data Sheet For SALEN & TP complexes” modules on the Winter 2024 CHM230 Laboratory Canvas page. The synthesis of the iron-tp complex and the iron-salen complex is found in the “Synthesis of Transition Metal Complexes Part I: Salen species Lab Procedure” and the "Synthesis of Transition Metal Complexes Part II & III Lab Procedure” assignments on the Winter 2024 CHM230 Laboratory Canvas page. Abstract: Different approaches were used to explore different transition metal complexes and compare their impact on d-orbital splitting. Part I involved using a spectrophotometer to determine the maximum wavelength for Cr(acac)3, [Cr(en)3]Cl3, Cr(H2O)63, Cr(Tp)2, and CrCl3-6H2O, allowing for the calculation of energy required for electron transitions. This energy, which reflects d-orbital splitting in octahedral complexes, was influenced by the ligand type, leading to the establishment of a spectrochemical ligand series: Cl¯ < H₂O < acac < en<Tp. In Part II, a magnetic susceptibility balance was used to determine the number of unpaired electrons and electron arrangements in various transition metals through effective magnetic moment calculations. Mn(acac)3 had four unpaired electrons, Cr(acac)3 had three, and Fe(C16H14N2O2), CoCl2 6H2O, and Fe(Tp)2 each had one. These findings facilitated the synthesis of a spectrochemical series for metal ligands: Mn²* < Ni²* < Co²* < Fe²* < Fe³* < Cr³*. Overall, these results deepen our understanding of factors influencing electron arrangement in transition metal complexes, particularly d-orbital splitting, highlighting the importance of both ligand and metal cation identity. Introduction: Exploring d-Orbital Splitting in Transition Metal Complexes: Insights from Ligand-Field Theory Understanding ligand strength is key to deciphering d-orbital splitting in transition metal complexes. This involves quantifying the energy gap between d-orbitals using Ao values. Exploring ligand-field theory and the spectrochemical series helps uncover the principles behind the optical and magnetic properties of these complexes. Transition metal complexes are essential in chemical processes, including those related to the origin of magnetism. One fundamental aspect of transition metal complexes is the splitting of d-orbitals in the presence of ligands, known as d-orbital splitting (Figure 1). This phenomenon, led by the ligand's strength and the metal's properties, significantly influences the complex's optical and magnetic properties. Figure 1. D-orbital splitting of a metal ion in an octahedral field. free metal ion eg dz² dx²-y² 125 dxz dyz dxy metal ion in octahedral field Reference: "Analysis of d-orbital splitting in Transition Metal Complexes Part I: UV-vis" Laboratory procedure from the Canvas site for the Winter 2024 Chemistry 230L Course. Through a series of experiments, the relationship between ligand strength, metal-ligand interactions, and the resulting spectroscopic and magnetic behaviors of these complexes is explored. First, a foundational objective could be established by synthesizing and analyzing various chromium(III) complexes. If UV-visible spectroscopy is used, it would help reveal absorption spectra and λmax values, which are crucial for calculating Ao. Hence, magnetic susceptibility measurements offer valuable insights into the magnetic behavior of these complexes, enhancing our comprehension of d-orbital splitting. Furthermore, this data serves as a foundation for establishing a spectrochemical series of varying metal complexes, providing additional insights into their properties. By clarifying the intricate relationships between ligand strength, metal-ligand interactions, and d-orbital splitting, the goal was to provide a comprehensive perspective on transition metal complexes as illustrated in a spectrochemical series: halides < o-ligands <n-ligands < c-ligands. This series incorporated insights into the behavior of metal cations, further enriching our understanding of the factors influencing d-orbital splitting. Experimental Materials: All chemicals were secured from the CHM 230 laboratory stock except iron(II) salen (Fe(C16H14N2O2) made January 21, 2024 using the procedure found in the document titled, "The Synthesis of Transition Metal Complexes Part I: the Salen Ligand and a Salen Complex” and the metal sandwich Fe(Tp)2 and Cr(acac)3 made February 11, 2024 using the procedure found in the document titled "Synthesis of Transition Metal Complexes, Parts II and III.” The Mn(acac)3 was borrowed and the ZnCl2 was included with the lab materials provided. . UV-visible spectra were acquired using the SpectraVis Plus UV vis Spectrophotometer. Magnetic susceptibility was acquired using the Johnson-Matthey Magnetic Susceptibility Balance. Collecting Spectrophotometer Data of Chromium Transition Metal Complexes Part I: UV-vis Solutions of different chromium(III) complexes, including Cr(acac)3 (Chromium(III) acetylacetonate), [Cr(en)3] Cl3 (Tris(ethylenediamine)chromium(III) chloride), Cr(H2O)6C13 (Hexaaquachromium(III) nitrate), and CrCl³·6H₂O (Chromium(III) chloride hexahydrate) were prepared in their designated solvents: toluene for Cr(acac)3 and water for the other complexes. Each solution was placed in a suitable cuvette (quartz/glass for Cr(acac)3 and polystyrene for the others) and ensured to have a concentration suitable for spectroscopic analysis (0.5 < max A < 1.5), with initial concentrations ranging from 5 to 12 mg/mL (Table 1). A glass cuvette was used for toluene since the interaction between toluene and polystyrene is unfavorable, leading to potential damage or dissolution of the polystyrene material. Table 1. Masses of Cr samples and volume of solvent used for UV-Vis. Sample Cr(acac)3 Mass [g] Volume of Solvent [mL] 0.0350 7.40 [Cr(en)3]Cl 0.0250 3.29 [Cr(en)3] Cl 0.0500 3.10 CrCl₂.6H₂O 0.0250 3.10 Complex Observations When dissolving into their designated solvents, CrCl3 • 6H₂O salt created a green solution, [Cr(H2O)6](NO3)3 salt created a black-grey-colored solution, [Cr(en)3]Cl3 salt created a yellow-orange colored solution, and Cr(acac)3 solution was bright purple. Spectrophotometer Analysis and Calulations of Chromium Transition Metal Complexes After the initial scan of CrC13 • 6H2O, it was allowed to settle for two hours before undergoing another UV-vis spectrophotometer analysis. A subsequent plot was generated (see supplemental information), comparing the first scan of CrC13 • 6H2O with Cr(H2O)63, and the second scan of CrC13 • 6H20, to examine the differences between the two scans and another Cr(III) compound with 6H2O as a ligand. Next, UV-visible spectra were recorded for each chromium(III) complex solution using a spectrophotometer displaying the complex's maximum absorbance. The longest wavelength absorption maximum (λmax) for each spectrum was identified and recorded in nanometers (nm). These values were then converted into energy units 1 1.107 nm 0.01196 kJ.cm to calculate Ao using the formula Ao = • To calculate лтах (пт) 1 cm 1 mol concentration, Equation 1 was used. Equation 1. The formula for the concentration of a complex.See Answer
Q8:Question 5 Calculate the standard cell potential in volts for this cell diagram. Au- 1.0 M Au³- 3+ 1.0 M Cu+ 1.0 M Cu2+ PtSee Answer
Q9:Question 4 1 points SaveAnswer Imagine a galvanic cell is composed of two compartments, one containing lithium metal and the other 1.0 atm fluorine gas. Using data from your textbook, calculate the standard cell potential.See Answer
Q10:Question 2 Use the four dropdown menus to complete the statements regarding this reaction: MnO4 → MnO2 When balanced under basic conditions, this half-reaction has: i. 4 ii. 3 moles of OH- on the right ✓ side of the equation; moles of electrons; and iii. is a(n) reduction .See Answer
Q11:1. Use both the diagram and activity series below to fill in the missing answers in the table below. Use these answers provided as clues in adding the missing information. Then answer the questions that follow. • Most active (most easily Li K oxidized; Ba Sr loses electrons Ca most easily) Na Mg Al Mn Zn Fe Cd Co Ni Sn Pb H Cu 5 Ag Hg Least active Au = 1 Metal copper strip 6 Solution = cadmium nitrate 2 Solution = copper (II) nitrate 7 3 Cathode or Anode? 8 Metal = cadmium 4 9 5 Cathode or Anode? Refer to the activity series above. Which metal should be the anode and the cathode? Explain your answer. • Describe in detail how the electrons will flow through the device. • Provide a detailed explanation for how this wet voltaic cell works. Your explanation must include the actual oxidation and reduction half-reactions that are occurring in this cell.See Answer
Q12: PART A. FREEZING POINT OF LAURIC ACID Mass lauric acid, mass, Tf, trial 1 Tf, trial 2 1,2. Average Tf Data Unrounded Value S 43.5000 1.952 42.7 44.3 ✔ g YOUR PROGRESS ON FREEZING POINT OF LAURIC ACID °C °C Rounded Value 43.5 Unit °C Unit PART B. FREEZING POINT OF SOLUTION OF (LAURIC ACID+ UNKNOWN) UNKNOWN ID AND MASS Unknown ID VB Mass solvent, mass, Mass solute, mass2 ✓ Table to report mass values from experiment • Kf of lauric acid is 3.90 °C kg mol-¹ • Use your average freezing point for lauric acid Data 1.952 3 g Note: report LabQuest values as is for intercepts and slopes. Unit g GRAPH DATA 3. Slope of line 1, m₁ 4. Intercept of line 1, b₁ Table to report graph data from LabQuest 5. Slope of line 2, m₂ 6. Intercept of line 2, b₂ CALCULATIONS 7.8. T 9,10. ΔΤ, 11,12. Molar mass of unknown Data D D Unrounded Value 5 Unit CE dill 2 2 2 2 Rounded Value 3 > Unit 2 2 X SCORE: 21% Choose molar mass closest to your value: ERROR 13,14. % Error, molar mass CORRECT YOUR PROGRESS ON FREEZING POINT OF SOLUTION OF (LAURIC ACID + UNKNOWN) 1 17 Unrounded Value SAVED: 5.16. T/ PART C. ADDITIONAL QUESTION 6 Unrounded Value POINTS AWARDED 3 53 Rounded Value AUTOSOLVED The molar mass of a-linolenic acid is 278.43 g mol-¹ Rounded Value 0 17 If 0.213 g of mass, (a-linolenic acid) is dissolved in 2.912 g of mass3 (lauric acid), calculate the expected freezing point of the solution. NOT FINISHED 21 23 If 0.213 g of mass (a-linolenic acid) is dissolved in 2.912 g of mass, (lauric acid), calculate the expected freezing point of the solution. 15,16. T CORRECT YOUR PROGRESS ON THE ADDITIONAL QUESTION Unrounded Value Extra Stats to show: 02 YOUR OVERALL PROGRESS 7 25 CORRECT ANSWERS Units Rounded Value POINTS AWARDED 0 10 Calculations POINTS AWARDED 16 79 AUTOSOLVED Rounding Concepts AUTOSOLVED 0 25 02 NOT FINISHED NOT FINISHED 23 34 2/2/nman I Part A Mass of lauric acid 5₂ 1.952 After freezing Value of y = Tf₁ = 1-4.0914, g 1 299 27 Before freezing m₁ = Before freezing 48.96 aftur freezing = -0.22788 Locker/ Desk No. Freezing point of lauric acid: Trial 1: 42.7°C (42.7° 52.9) x2 = 47.8°c (326.95k) Trial 2: 52.9°C 2.099 Average freezing point of pure lauric acid, Te 320.95 K Part B Unknown ID A mass of unknown 0.315g Course & Section No. Tr Trials Before freezing m₁ = -8.0645m₁ Before freeding b₁ = 47.151 After freezing m2=0.5446 | 'value of y = Tf' = b2 = 37.599 Average value of freezing & point of lauric acid/unknown Solution Tf= Show cate how you calculated the value of te for one of your trials: Depression of freezing point, Stp = Te-Tp. MSee Answer
Q13:Observation of catalase in different Temperatures: Temperature Foam height (cm) 0.8 cm 0°C Room Temperature 37°C 50°C 70°C 1.2 cm 1.8 cm 1.5 cm 0.0 cm Reason Lower foam height due to reduced enzyme activity at low temperatures. Increased foam height as enzyme activity improves with higher temperatures. Maximum foam height, the optimum temperature for catalase activity. Decreased foam height duel to enzyme denaturation at high temperatures. No foam produced due to extensive enzyme denaturation, rendering. catalase inactive. Question: 1) Based on the data obtained, plot a graph with the height-readings obtained (Temperature on X-axis versus height in cm on Y-axis). 10. From this graph determine the optimum temperature and also the denaturation temperature for the enzyme. Note on drawing graphs: Most of the graphs, which you will draw in biology, will have a vertical and horizontal axis: • Horizontal Axis (x-axis). The set conditions (independent variable) of the experiment is always placed on the horizontal axis. These include known criteria like pH or temperature, or some other condition. Label the axis with the name and units (e.g. temperature (°C)) and values. • Vertical Axis (y-axis). The results recorded (under the set conditions) are placed on the Vertical Axis. Prior to doing the experiment, these readings are unknown. Again, label the axis with the name (e.g. time (seconds)), units and values./nEffect of pH on catalase enzyme activity: Theoretical pH Vol. of NaH2PO4 (ml) 5.6 6.2 7.0 8.05 9.05 Question: 0.5 2.0 6.0 9.5 10.0 Vol. of KH2PO4 (ml) 9.5 8.0 4.0 0.5 0 Actual pH (verified with pH meter) 5.49 7.03 7.83 8.83 9.73 1) Identify the optimum pH? 2) Plot a graph of your results, pH against foam height. Foam level (cm) 1.55 3.3 2.9 2.7 2.3See Answer
Q14:Handout 4-1 Periodic Table 1. The elements on the Periodic Table are arranged in order of increasing 1) atomic mass 2) atomic number 3) molar mass 4) oxidation number 2. Which element exists as a diatomic molecule at STP? 1) bromine 2) argon 3. The element in Group 14, Period 3, of the Periodic Table is classified as a 1) metal 2) noble gas 3) neon 4) carbon 1) Li, Na, Rb 2) Cr, Mo, W 4. Which list of elements consists of a metal, a metalloid, and a nonmetal? 3) metalloid 4) nonmetal 3) Sn, Si, C 4) O, S, Te 5. Which list includes elements with the most similar chemical properties? 1) Br, Ga, Hg 3) O, S, Se 4) N, O, F 2) Cr, Pb, Xe 6. Which statement identifies the element arsenic? 1) Arsenic has an atomic number of 33. 2) Arsenic has a melting point of 84 K. 3) An atom of arsenic in the ground state has eight valence electrons. 4) An atom of arsenic in the ground state has a radius of 146 pm. 7. Which statement explains why sulfur is classified as a Group 16 element? 1) A sulfur atom has 6 valence electrons. 2) A sulfur atom has 16 neutrons. 3) Sulfur is a yellow solid at STP. 4) Sulfur reacts with most metals. 1) hydrogen 2) calcium 8. Element X is a solid that is brittle, lacks luster, and has six valence electrons. In which group on the Periodic Table would element. X be found? 2) 2 3) 15 4) 16 1) 1 9. Which element is an alkali metal? 3) sodium 4) zinc 10. Most of the groups in the Periodic Table of the Elements contain 1) nonmetals, only 2) metals, only 3) nonmetals and metals 4) metals and metalloids 11. As the elements in Group 15 are considered in order of increasing atomic number, which sequence in properties occurs? 1) nonmetal → metalloid → metal 2) metalloid →→ metal → nonmetal 3) metal metalloid →→> nonmetal 4) metal →→nonmetal → metalloid 12. Which group contains both metals and nonmetals? 1) 1 2) 3 3) 15 4) 7 13. Which element is in Group 2 and Period 7 of the Periodic Table? 1) magnesium 3) radium 2) manganese 4) radon 14. Bromine has chemical properties most similar to 1) fluorine 2) potassium 3) krypton 4) mercury 15. Which group is known as the halogens? 1) 1 2) 2 3) 17 4) 18 16. An atom of an element contains 20 protons, 20 neutrons, and 20 electrons. This element is in Group 1) 1 2) 2 3) 4 4) 18 17. Which element is malleable and ductile? 1) S 2) Si 3) Au 4) C 18. Which of these elements is the best conductor of electricity? 1) Sb 3) Si 4) Zn 2) I/n19. What is a property of most metals? 1) They tend to gain electrons easily when bonding. 2) They tend to lose electrons easily when bonding. 3) They are poor conductors of heat. 4) They are poor conductors of electricity. 20. Which element has properties of electrical conductivity and luster and exists as a liquid at STP? 1) Hg 2) Br 3) C 4) I 21. Metallic substances will conduct electricity in 1) the solid phase, only 2) the liquid phase, only 3) both the solid and the liquid phase 4) neither the solid nor the liquid phase 22. At STP, graphite and diamond are two solid forms of carbon. Which statement explains why these two forms of carbon differ in hardness? 1) Graphite and diamond have different ionic radii. 2) Graphite and diamond have different molecular structures. 3) Graphite is a metal, but diamond is a nonmetal. 4) Graphite is a good conductor of electricity, but diamond is a poor conductor of electricity. 23. Which particle diagram represents the arrangement of F2 molecules in a sample of fluorine at 95 K and standard pressure? Key O atom of fluorine = त O 8 3) 4) 24. At STP, which element is brittle and not a conductor of electricity? 1) S 2) K 3) Na 4) Ar 25. Which characteristics describe most nonmetals in the solid phase? 1) They are malleable and have metallic luster. 2) They are malleable and lack metallic luster. 3) They are brittle and have metallic luster. 4) They are brittle and lack metallic luster. 26. Which element tends not to react with other elements? 1) neon 2) hydrogen 3) phosphorous 4) potassium 27. An atom of argon in the ground state tends not to bond with an atom of a different element because the argon atom has 1) more protons than neutrons 2) more neutrons than protons 3) a total of two valence electrons 4) a total of eight valence electrons 28. Which element has both metallic and nonmetallic properties? 1) Rb 2) Rn 3) Si 4) Sr 29. At 25°C, in which phase of matter do most of the known elements exist? 1) solid 2) liquid 3) gas 4) supercooled liquid 30. Which group in the Periodic Table contains elements that are all gases at STP? 1) 11 2) 17 3) 12 4) 18 31. Which group on the Periodic Table has at least one element in each of the three phases of matter at STP? 1) 1 2) 2 3) 17 4) 18 32. Which statement describes oxygen gas, O2(g), and ozone gas, O3(g)? 1) They have different molecular structures, only. 2) They have different properties, only. 3) They have different molecular structures and different properties. 4) They have the same molecular structure and the same properties./n33. Which element has the greatest density at STP? 1) calcium 2) carbon 3) chlorine 4) copper 34. An atom that has an electron configuration of 2-8-13-2 is classified as 1) an alkali metal 2) an alkaline earth metal 3) a transition element 4) a noble gas element 35. Magnesium and calcium have similar chemical properties because their atoms in the ground state have 1) equal numbers of protons and electrons 2) equal numbers of protons and neutrons 3) two electrons in the first shell 4) two electrons in the outermost shell 36. Which compound forms a green aqueous solution? 1) RbCl 2) CaCl2 3) NiCl24) ZnCl2 37. Based upon your knowledge of metallic activity, which element would most readily react with water? 1) Zn 2) Cu 3) Fe 4) Li 38. Which ionic compound dissolves in water to form a colored solution? 1) Ca(NO3)2 2) Cu(NO3)2 3) KNO3 4) AI(NO3)3 39. Which set of properties is most characteristic of transition elements? 1) colorless ions in solution, multiple positive oxidation states 2) colorless ions in solution, multiple negative oxidation states 3) colored ions in solution, multiple positive oxidation states 4) colored ions in solution, multiple negative oxidation states 40. Compared to the radius of a chlorine atom, the radius of a chloride ion is 1) larger because chlorine loses an electron 2) larger because chlorine gains an electron 3) smaller because chlorine loses an electron 4) smaller because chlorine gains an electron 41. Compared to an atom of potassium, an atom of calcium has a 1) larger radius and lower reactivity 2) larger radius and higher reactivity 3) smaller radius and lower reactivity 4) smaller radius and higher reactivity 42. As an atom becomes an ion, its mass number 3) remains the sam 1) decreases 2) increases 43. Which two characteristics are associated with metals? 1) low first ionization energy and low electronegativity 2) low first ionization energy and high electronegativity 3) high first ionization energy and low electronegativity 4) high first ionization energy and high electronegativity 44. As the elements in Period 2 of the Periodic Table are considered in order from left to right, which property generally decreases? 1) atomic radius 3) ionization energy 2) electronegativity 4) nuclear charge 45. Which of the following Period 4 elements has the most metallic characteristics? 1) Ca 2) Ge 3) As 4) Br 46. Which trends are observed as each of the elements within Group 15 on the Periodic Table is considered in order from top to bottom? 1) Their metallic properties decrease and their atomic radii decrease. 2) Their metallic properties decrease and their atomic radii increase. 3) Their metallic properties increase and their atomic radii decrease. 4) Their metallic properties increase and their atomic radii increase. Page 3/n47. As the elements in Period 2 of the Periodic Table are considered in succession from left to right, there is a decrease in atomic radius with increasing atomic number. This may best be explained by the fact that the 1) number of protons increases, and the number of shells of electrons remains the same 2) number of protons increases, and the number of shells of electrons increases 3) number of protons decreases, and the number of shells of electrons remains the same 4) number of protons decreases, and the number of shells of electrons increases 48. Which of the following electron configurations represents the element with the smallest atomic radius? 1) 2-4 2) 2-5 3) 2-6 4) 2-7 49. An atom with the electron configuration 2-8-7 would most likely 1) decrease in size as it forms a positive ion 2) increase in size as it forms a positive ion 3) decrease in size as it forms a negative ion 4) increase in size as it forms a negative ion 50. Which ion has the largest radius? 1) Br 2) Cl- 3) F- 4) 1- 51. Which ion has the largest radius? 1) Na+ 2) Mg²+ 3) K+ 4) Ca²+ 52. As the elements in Group I of the Periodic Table are considered from top to bottom, each successive element has a 1) smaller first ionization energy 2) larger first ionization energy 3) smaller number of protons 4) larger number of valence electrons 53. Elements that readily gain electrons tend to have 1) high ionization energy and high electronegativity 2) high ionization energy and low electronegativity 3) low ionization energy and low electronegativity 4) low ionization energy and high electronegativity 54. How do the atomic radius and metallic properties of sodium compare to the atomic radius and metallic properties of phosphorus? 1) Sodium has a larger atomic radius and is more metallic. 2) Sodium has a larger atomic radius and is less metallic. 3) Sodium has a smaller atomic radius and is more metallic. 4) Sodium has a smaller atomic radius and is less metallic. 55. As the elements of Group 16 are considered in order from top to bottom, the covalent radius of each successive element increases. This increase is primarily due to an increase in 1) atomic number 2) mass number 3) the number of protons occupying the nucleus 4) the number of occupied electron shells 56. Compared to the atomic radius of a sodium atom, the atomic radius of a magnesium atom is smaller. The smaller radius is primarily a result of the magnesium atom having 1) a larger nuclear charge 2) a smaller nuclear charge 3) more principal energy levels 4) fewer principal energy levels 57. Which term represents the strength of the attraction an atom has for the electrons in a chemical bond? 1) electrical conductivity 2) electronegativity 3) first ionization energy 4) specific heat capacity 58. Based on Table S, an atom of which element has the strongest attraction for electrons in a chemical bond? 1) chlorine 2) nitrogen 3) oxygen 4) selenium 59. Which element requires the least amount of energy to remove the most loosely held electron from a gaseous atom in the ground state? 1) Na 2) Ar 3) P 4) CI Page 4/nShort Answers Base your answers to questions 1 through 3 on the information below and on your knowledge of chemistry. A technician recorded data for two properties of Period 3 elements. The data are shown in the table below. Element Ionic Radius (pm) Reaction with Cold Water Na 95 reacts vigorously Two Properties of Period 3 Elements Si P 41 Mg Al 51 66 S 184 no no no reacts no very observable observable observable observable slowly reaction reaction reaction reaction 1. Identify the element in this table that is classified as a metalloid. CI 181 reacts slowly Ar no observable reaction 2. State evidence from the technician's data which indicates that sodium is more active than aluminum. 3. State the phase of chlorine at 281 K and 101.3 kPa. (hint: use Reference Table S) Explain. Base your answers to questions 4 through 7 on the information below and on your knowledge of chemistry. Sir William Ramsey is one scientist credited with identifying the noble gas argon. Sir Ramsey separated nitrogen gas from the air and reacted it with an excess of magnesium, producing solid magnesium nitride. However, a small sample of an unreactive gas remained with a density different from the density of the nitrogen gas. Sir Ramsey identified the unreactive gas as argon and later went on to discover neon, krypton, and xenon. 4. Compare the chemical reactivities of nitrogen gas and argon gas based on Sir Ramsey's experiment using magnesium. 5. Compare the density of nitrogen gas to the density of argon gas when both gases are at 298 Kand 101.3 kPa. 6. State, in terms of valence electrons, why the noble gases that Sir Ramsey discovered have similar chemical properties. 7. State the trend, at standard pressure, of the boiling points of these noble gases, as they are considered in order of increasing atomic number. Page 1/nchemistry. Some properties of the element sodium are listed below. • is a soft, silver-colored metal • melts at a temperature of 371 K • oxidizes easily in the presence of air • forms compounds with nonmetallic elements in nature • forms sodium chloride in the presence of chlorine gas 8. Identify one chemical property of sodium from this list. 9. Convert the melting point of sodium to degrees Celsius. Base your answers to questions 10 and 11 on the information below. Densities of Group 14 Elements Density at STP (g/cm³) 3,51 Element C Si Ge Sn Pb 2.33 5.32 7.31 11.35 10. Identify one element from this table for each type of element: metal, metalloid, and nonmetal. 11. Calculate the volume of a tin block that has a mass of 95.04 grams at STP. Your response must include both a numerical setup and the calculated result. Round your answer to the correct number of significant figures. Base your answers to questions 12 through 14 on the information below and on your knowledge of chemistry. Periodic trends are observed in the properties of the elements in Period 3 on the Periodic Table. These elements vary in physical properties, such as phase, and in chemical properties, such as their ability to lose or gain electrons during a chemical reaction. 12. Identify the metals in Period 3 on the Periodic Table. 13. Identify the element in Period 3 that requires the least amount of energy to remove the most loosely held electrons from a mole of gaseous atoms of the element in the ground state. 14. State the general trend in atomic radius as the elements in Period 3 are considered in order of increasing atomic number. Page 2/nBase your answers to questions 15 through 17 on the information below and on your knowledge of chemistry. The elements in Group 2 on the Periodic Table can be compared in terms of first ionization energy, electronegativity, and other general properties. 15. Describe the general trend in electronegativity as the metals in Group 2 on the Periodic Table are considered in order of increasing atomic number. 16. Explain, in terms of electron configuration, why the elements in Group 2 have similar chemical properties. 17. Explain, in terms of atomic structure, why barium has a lower first ionization energy than magnesium. Base your answers to questions 18 through 20 on the information below and on your knowledge of chemistry. Rubidium and iodine have different chemical and physical properties. Some of these properties are shown in the table below. Some Physical and Chemical Properties of Rubidium and lodine Rubidium lodine silvery-white solid forms ionic compounds with nonmetals reacts with oxygen in the air specific heat = 0.363 J/g+K 18. State the chemical property of iodine listed in this table. bluish-black lustrous solid forms ionic bonds with active metals sublimes at room temperature specific heat = 0.214 J/g.K 19. Compare the atomic radius of an atom of iodine to the atomic radius of an atom of rubidium when both atoms are in the ground state. 20. Compare the electrical conductivity of these two elements at STP. Page 3See Answer
Q15:The irreducible representations for the four ligands on ML4 (Figure; 1) belonging to C3v point group is 2A1+ E. The energy of the d-orbitals on M considering only sigma-bonding is dz2 >dx2-y2 & dxy > dxz & dyz (Should be in non-bonding). the SALCs of Where, ₁,₂ have a1 symmetry and 43 and 44 have e symmetry (Figure:2) are stabilized to the same extent that the d-orbitals are destabilized. Complete the MO diagram for ML4 ( given below) the ligand field only (i.e. the d- orbitals). , 90° L3ML 120⁰ L₂ Figure 1 L4 M SALOS T: (1/5K++2) (1/2)(2-0₂-) Figure 2 Complete MO diagram with SALCS Oo (1/50++-2) (1/2-) LSee Answer
Q16:This ML4 geometry can be enforced via the tren ligand: H₂N 1. dx2-y2: 2. dxy: H₂N N M−NH2 M(tren) Question 1: Using the Angular Overlap Chart, calculate the energy of the d-orbitals assuming that only sigma-bonding is important:See Answer
Q17:Part D: Research (Outcomes S2 and S3) Potentially Useful Source for this section: Engineeringlibrary.org Metals are often used in engineering applications. These metals commonly are used in construction, bridges, etc and are exposed to stress and respond by elongating, which we call strain. The two stages of elastic response are called elastic deformation and plastic deformation. 1. Research and summarize what these two deformations are. 2. Try to find a stress/strain plot and the Elastic (Young's) Modulus of your metal. Embed this plot in your document. Watch this video to learn from: Stress-Strain Diagrams (CU Boulder) • Watch Understanding Young's Modulus Video from The Efficient Engineer to help you learn and respond to the following questions. o What does the elastic modulus value tell us? (What does a high value mean, what does a low value mean?) o How does this value help us understand sagging power lines after a winter storm? (And thus help engineers decide what material to use and how far apart to place the power poles.) Would your metal be suitable for use in power lines (or other applications where the wire will carry a load)? o o For what application is your metal suitable? 3. What is the difference between substitutional and interstitial alloys? See Alloys from LibreTexts for reading. • What kind of alloy does your metal form? Why and how? Please relate your answer back to the particular crystal structure that your metal utilizes. What are the Hume-Rothery rules for alloy formation? See Hume-Rothery Rules Video (CU Boulder) • Indicate one metal that would easily form a substitutional alloy over the entire composition range with your metal. Indicate one metal that would not.See Answer
Q18:Part C: Electron Configurations and Crystal Structures (Outcomes 6.1-6.4, 8.1-8.2 and S4) 1. Write the full electron configuration for your element. Identify the core and valence electrons. Draw the orbital diagram for the valence electrons. Choose one of the valence electrons (circle it) and write the set of 4 quantum numbers for it. EXPLAIN WHY these are the quantum numbers for that electron. What charge does your element typically form? Can you hypothesize why that is based on the electron configuration? 2. Find the atomic emission or absorption spectrum for your metal. Embed this into your document. Pick a transition wavelength and calculate the energy and frequency of that transition. Be sure to show and explain all work. 3. Do a little research and determine in what crystal structure the atoms of your metal arrange themselves. Webelements.com 4. Model this crystal structure (ball and stick, space filling, or with truncated atoms). Include a screen shot or drawing of these in your document. Feel free to use what you want to do this-solid works? Hand-drawings? Other computer stuff? Online Crystal Structure Modeling (Site from CalPoly) 5. Using the radius of an atom of your metal and its crystal structure, calculate the density of your metal. 6. Compare this calculated density to the density provided in reliable sources Determine the % difference and explain any significant differences between your density value and the accepted density value. (HINT: Think about the methods by which atomic radius can be measured)See Answer
Q19:Part A: Hybridization, VSEPR, and Intermolecular Forces-Use the compound you have been assigned on the Homework C Page (Outcomes 7.3, 7.4, 8.3, 8.4) 1. Research the chemical formula of your compound 2. Hand Draw the Lewis Structure of your compound. This should be neatly drawn and large enough to clearly see the bonds and lone pairs. Label the following use different colors to clearly identify the pieces-you can create a key/legend for me) Identify the hybridization of each atom that is bonded to more than one other atom. Identify the VSEPR/Molecular Geometry around each atom that is bonded to more than one other atom. Identify the bond angle around each atom that is bonded to more than one other atom. 3. Model your compound to accurately reflect bond lengths and angles. Below are a couple of programs you may find helpful on this step. Screen shot your model and embed it into your document. MolView • ChemSketch: https://www.acdlabs.com/resources/freeware/index.php 4. Is your substance polar or nonpolar? Explain how you know. 5. What IMFs (intermolecular forces) are possible for your compound? • Draw a couple of your molecules exhibiting the strongest of these forces. You can use dashed lines (in a different color) to show between which atoms of the molecule the IMFs occurSee Answer
Q20:3. Calculate the energy released per gram of Ethane. Ethane gas is burned in the presence of Oxygen. When Ethane gas, C₂H6, burns, Carbon Dioxide gas, CO₂, and water, H₂O are formed. The following unbalanced chemical equation shows this reaction [12 Marks]: CH + O, → CO2 + H2O HH H-C-C- -C-H HHSee Answer

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