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ANES 500 Chapter 2 Assignment Name: ________________________ Fall 2021_2022 Grade__________ General Instructions Provide suitable responses for the problems shown below. The assignment is to be completed individually and returned by 11:30 pm EST on Monday, September 20, 2021. Where applicable, show your work to receive full credit. Late assignments will be assessed a penalty of 10 % of the overall grade per day late. How to Return This Assignment You may upload the document to the drop box in Canvas as a Word file, a pdf file, a jpeg file, a scanned file, etc. The document may also be returned as an email attachment in canvas. If the file is too large, try compressing it using free services such as wecompress.com. Do not return the file using our outlook email. For those who save each page of the assignment as a pdf or image file, you may combine them into one document as follows: • Locate the files in Windows File Explorer. • Right click on the first file. • Choose “Combine Supported Files in Acrobat…” A new dialog box will pop up, but you may have to minimize other files to see it. • Drag the files from Explorer into this box. • If necessary, change the order of the files using “Move Up” or “Move Down.” • Click on “Combine Files.” You will be prompted for a file name. If applicable, you may also copy and paste images in a Word document, and then save the document as a pdf file. Instructions for writing or type on a pdf document will be sent to you as a separate document. Please ensure that your work is legible and your file is complete before and after sending. ANES 500 Chapter 2 Assignment Fall 2021 Name_____________________ Due 11:30 pm on 9/20/2021 Grade__________ Provide suitable responses to the problems shown below. Where applicable, show your work to receive full credit. 1. Complete the table below and give the nuclide symbol with charge where applicable. (4 pts) 2. Lawrencium–262 can be obtained by bombarding Californium–252 with Boron–10. Determine the number of electrons, protons, and neutrons for the neutral forms of these atoms. (3 pts) 3. The masses and fractional abundances of the six naturally occurring isotopes of an element are tabulated below. (a) Complete the table by reporting each product to 5 decimal places, and the atomic mass of the element to 5 significant figures. (b) Write the chemical symbol of the element. (4 pts) 4. Classify each of the following substances as an element, compound, or mixture. (3 pts) (a) 5% Dextrose injection: ____________________________________ (b) Pure brass (70% copper and 30% zinc): _______________________ (c) Glycerol: _______________________ (d) Liquid diatomic bromine: __________________________ (e) The covalently bonded ring of atoms shown below: ___________________________ (f) Normal saline solution _________________________________________ 5. Give a chemical symbol for each class of elements identified below. (3 pts) Chemical Symbol (a) (b) (c) (d) (e) (f) Classification A transition element that is liquid at room temperature (RT). A noble gas with the same number of valence electrons as Be or Mg. A metalloid with the same number of energy levels and same number of valence electrons. A halogen that is a liquid at room temperature. A nonmetal that is a gas at room temperature but with the same number of valence electrons as Na. The smallest alkaline earth metal in the Periodic Table. 6. Match the following terms to their proper definitions. (10 pts) 1. Valence electrons 6. Isotopes 2. Ionization energy 7. Transition elements 3. Metals 8. Elements 4. Nonmetals 5. Electronegativity 9. Neutrons 10. Electrons (a) ______ Relative ability of an atom to attract electrons in a bond. (b) ______ They lack luster, conduct heat and electricity poorly, and tend to for anions. (c) ______ Subatomic particles found in these isotopes of hydrogen except the first. (d) ______ The outer electrons that are involved in chemical bonding and other changes. (e) ______ Examples of these pure substances are shown below. They cannot be decomposed into simpler substances by chemical processes. (f) _____ The lightest subatomic particles that occupy nearly the entire volume of an atom. (g) ______ They are shiny, they conduct heat and electricity, and they tend to for cations. (h) ______ Elements found in Groups 3-12 of the periodic table. (i) ______ The energy required to remove an electron from a gaseous atom or ion. (j) ______ General term for atoms of the same element such as those shown below. 7. Perform the following exercises: (6 pts) (a) Arrange P, Cl, and Al in order of increasing electronegativity: _____ Al < P < Cl _______ (b) Arrange S, O, and Se in order of increasing electronegativity: __________________ (c) Select 2 elements with similar properties from V, Ni, Ag, P, S, and Ta. ______________ (d) Identify a metalloid with as many valence electrons as titanium: ____________________ (e) Arrange Cl, F, I and Br in order of increasing atomic radius: ______________________ (f) Arrange Mg, Mg2+, and S in order of increasing radius: ___________________________ 8. Write the name or chemical symbol of an alkali metal with 6 energy levels. 9. For the atom with the electron arrangement shown below (X: 2, 8, 8, 1), give the chemical symbol, the group number, and the period number. (3 pts) 10. For the atom with the electron arrangement shown below (X: 2, 8, 5), give the chemical symbol, the group number, and the period number. (3 pts) 11. Classify the following compounds as ionic compounds or covalent compounds. (3 pts) (a) SOCl2 (b) POCl3 (c) CaO28H2O (d) Cs2S2O4 (e) C2N2 12. Determine the charge on the cation ion for each of the following compounds: (4 pts) (a) (NH4)2S2O4 (b) ZrC (c) MnO4- (d) K2O (f) MnO2 13. Write formulas for the compounds produced from the following ions: (5 pts) (a) Rb+ and N3- (b) Mn4+ and [BO3]3- (d) Ba2+ and [B4S7]2- (e) Cu+ and [PS3]2- (c) V3+ and [HPO4]2- 14. Using the list of anions shown below and on the lecture slides, write chemical formulas for compounds (a) – (j): (10 pts) Anion Name Anion Name Anion Name C2O42AsO43- Oxalate Arsenate C2H3O2- Acetate perchlorate CNHCO3- Cyanide Bicarbonate As3- Arsenide ClO3- Chlorate HSO4- Bisulfate CrO42- Chromate IO3- Iodate MnO4- Permanganate Cr2O72- Dichromate BrO3- Bromate S2O32- Thiosulfate ClO4 – (a) Manganese (II) sulfate monohydrate (f) Tin (IV) acetate (b) Lithium thiosulfate tetrahydrate (g Dibromine heptasulfide (c) Tetraphosphorus nonasulfide (h) Barium arsenate (d) Iron (II) sulfate pentahydrate (i) Nickel (III) iodate (e) Cobalt (III) Dichromate (j) Iodine heptabromide 15. Provide systematic names for the compounds shown below. (6 pts) (a) Zn(NO3)2•6H2O (b) IF3 (c) Cr(CN)3 (Specify charge) (d) CuClO4 (Specify charge) (e) IBr (f) K2CrO4 ANES 500 Chapter 2 Assignment Name: ________________________ Fall 2021_2022 Grade__________ General Instructions Provide suitable responses for the problems shown below. The assignment is to be completed individually and returned by 11:30 pm EST on Monday, September 20, 2021. Where applicable, show your work to receive full credit. Late assignments will be assessed a penalty of 10 % of the overall grade per day late. How to Return This Assignment You may upload the document to the drop box in Canvas as a Word file, a pdf file, a jpeg file, a scanned file, etc. The document may also be returned as an email attachment in canvas. If the file is too large, try compressing it using free services such as wecompress.com. Do not return the file using our outlook email. For those who save each page of the assignment as a pdf or image file, you may combine them into one document as follows: • Locate the files in Windows File Explorer. • Right click on the first file. • Choose “Combine Supported Files in Acrobat…” A new dialog box will pop up, but you may have to minimize other files to see it. • Drag the files from Explorer into this box. • If necessary, change the order of the files using “Move Up” or “Move Down.” • Click on “Combine Files.” You will be prompted for a file name. If applicable, you may also copy and paste images in a Word document, and then save the document as a pdf file. Instructions for writing or type on a pdf document will be sent to you as a separate document. Please ensure that your work is legible and your file is complete before and after sending. ANES 500 Chapter 2 Assignment Fall 2021 Name_____________________ Due 11:30 pm on 9/20/2021 Grade__________ Provide suitable responses to the problems shown below. Where applicable, show your work to receive full credit. 1. Complete the table below and give the nuclide symbol with charge where applicable. (4 pts) 2. Lawrencium–262 can be obtained by bombarding Californium–252 with Boron–10. Determine the number of electrons, protons, and neutrons for the neutral forms of these atoms. (3 pts) 3. The masses and fractional abundances of the six naturally occurring isotopes of an element are tabulated below. (a) Complete the table by reporting each product to 5 decimal places, and the atomic mass of the element to 5 significant figures. (b) Write the chemical symbol of the element. (4 pts) 4. Classify each of the following substances as an element, compound, or mixture. (3 pts) (a) 5% Dextrose injection: ____________________________________ (b) Pure brass (70% copper and 30% zinc): _______________________ (c) Glycerol: _______________________ (d) Liquid diatomic bromine: __________________________ (e) The covalently bonded ring of atoms shown below: ___________________________ (f) Normal saline solution _________________________________________ 5. Give a chemical symbol for each class of elements identified below. (3 pts) Chemical Symbol (a) (b) (c) (d) (e) (f) Classification A transition element that is liquid at room temperature (RT). A noble gas with the same number of valence electrons as Be or Mg. A metalloid with the same number of energy levels and same number of valence electrons. A halogen that is a liquid at room temperature. A nonmetal that is a gas at room temperature but with the same number of valence electrons as Na. The smallest alkaline earth metal in the Periodic Table. 6. Match the following terms to their proper definitions. (10 pts) 1. Valence electrons 6. Isotopes 2. Ionization energy 7. Transition elements 3. Metals 8. Elements 4. Nonmetals 5. Electronegativity 9. Neutrons 10. Electrons (a) ______ Relative ability of an atom to attract electrons in a bond. (b) ______ They lack luster, conduct heat and electricity poorly, and tend to for anions. (c) ______ Subatomic particles found in these isotopes of hydrogen except the first. (d) ______ The outer electrons that are involved in chemical bonding and other changes. (e) ______ Examples of these pure substances are shown below. They cannot be decomposed into simpler substances by chemical processes. (f) _____ The lightest subatomic particles that occupy nearly the entire volume of an atom. (g) ______ They are shiny, they conduct heat and electricity, and they tend to for cations. (h) ______ Elements found in Groups 3-12 of the periodic table. (i) ______ The energy required to remove an electron from a gaseous atom or ion. (j) ______ General term for atoms of the same element such as those shown below. 7. Perform the following exercises: (6 pts) (a) Arrange P, Cl, and Al in order of increasing electronegativity: _____ Al < P < Cl _______ (b) Arrange S, O, and Se in order of increasing electronegativity: __________________ (c) Select 2 elements with similar properties from V, Ni, Ag, P, S, and Ta. ______________ (d) Identify a metalloid with as many valence electrons as titanium: ____________________ (e) Arrange Cl, F, I and Br in order of increasing atomic radius: ______________________ (f) Arrange Mg, Mg2+, and S in order of increasing radius: ___________________________ 8. Write the name or chemical symbol of an alkali metal with 6 energy levels. 9. For the atom with the electron arrangement shown below (X: 2, 8, 8, 1), give the chemical symbol, the group number, and the period number. (3 pts) 10. For the atom with the electron arrangement shown below (X: 2, 8, 5), give the chemical symbol, the group number, and the period number. (3 pts) 11. Classify the following compounds as ionic compounds or covalent compounds. (3 pts) (a) SOCl2 (b) POCl3 (c) CaO28H2O (d) Cs2S2O4 (e) C2N2 12. Determine the charge on the cation ion for each of the following compounds: (4 pts) (a) (NH4)2S2O4 (b) ZrC (c) MnO4- (d) K2O (f) MnO2 13. Write formulas for the compounds produced from the following ions: (5 pts) (a) Rb+ and N3- (b) Mn4+ and [BO3]3- (d) Ba2+ and [B4S7]2- (e) Cu+ and [PS3]2- (c) V3+ and [HPO4]2- 14. Using the list of anions shown below and on the lecture slides, write chemical formulas for compounds (a) – (j): (10 pts) Anion Name Anion Name Anion Name C2O42AsO43- Oxalate Arsenate C2H3O2- Acetate perchlorate CNHCO3- Cyanide Bicarbonate As3- Arsenide ClO3- Chlorate HSO4- Bisulfate CrO42- Chromate IO3- Iodate MnO4- Permanganate Cr2O72- Dichromate BrO3- Bromate S2O32- Thiosulfate ClO4 – (a) Manganese (II) sulfate monohydrate (f) Tin (IV) acetate (b) Lithium thiosulfate tetrahydrate (g Dibromine heptasulfide (c) Tetraphosphorus nonasulfide (h) Barium arsenate (d) Iron (II) sulfate pentahydrate (i) Nickel (III) iodate (e) Cobalt (III) Dichromate (j) Iodine heptabromide 15. Provide systematic names for the compounds shown below. (6 pts) (a) Zn(NO3)2•6H2O (b) IF3 (c) Cr(CN)3 (Specify charge) (d) CuClO4 (Specify charge) (e) IBr (f) K2CrO4

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