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Chem 1A Answers

by: Amir Mahmoodi

Chem 1A Answers Chem 1A

Amir Mahmoodi
GPA 3.5

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Here are the answers to my Chem 1A worksheets
Study Guide
chem 1A, Chemistry, GChem, UCI, UC Irvine, Arasasingham
50 ?





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This 16 page Study Guide was uploaded by Amir Mahmoodi on Thursday February 11, 2016. The Study Guide belongs to Chem 1A at University of California - Irvine taught by ARASASINGHAM, R. in Fall 2015. Since its upload, it has received 33 views.


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Date Created: 02/11/16
AMIR M AHMOODI AMAHMOO 1@ UCI.EDU O FFICEHOURS : FRIDAY10-11 AM, 12-1 PM LOCATION : RH 517 Amir’s Week 2 Worksheet 1) What is the atomic number of Iodine? What is its atomic mass? How many neutrons does it have? How many electrons? A: #53, 126.9047 g/mol, 73 neutrons, 53 e - 2) Fred created a subatomic particle accelerator that can shoot electrons at speeds of up to 295,000,000 m/s. How fast is that in nanometers per second? (Use scientific notation and don’t forget about Sig Figs! All work must be shown.) A: (2.95x10 m/s) x (10 nm/1 m) = 2.95x10 14nm/s 3) Arman has 389.001 seconds to run from his house to his neighbor’s house before the party starts. He does so in 88.1 seconds. Upon his arrival, how much time will be left until the party? (Scientific notation and Sig Figs) 2 A: 389.001 – 88.1 = 3.009x10 s 4) What is the number of electrons, protons, and neutrons in 23Ra ?+ - A: 86 e , 230 – 88 = 142 neutrons, 88 protons 5) What is the difference between an Isotope of Lithium and a Lithium Ion? A: An Isotope has more or less neutrons than described on the periodic table. An Ion has more or less electrons than the Iodine described on the periodic table. 6) Which has more atoms: 25.00g of Oxygen or 100.50g of Helium? Explain (show  work; Scientific notation and Sig Figs). 23 23 A:  25.00g (1mol/ 16.00g)(6.022x10  atoms/ 1mol) =  9.409x10  atoms of Oxygen 23 25  100.50g (1mol/4.003g)(6.022x10  atoms/ 1mol) = 1.512x10 atoms of Helium. 14 7) Determine the mass (in grams) of a 256  N atoms. (Scientific notation and Sig Figs) A: 256 atoms (1mol/6.022x10 atoms)(14g/1mol) =  5.952x10      grams AMIR M AHMOODI AMAHMOO 1@ UCIEDU O FFICEHOURS : RIDAY 10-11 AM, 12-1 PM LOCATION: RH 517 Amir’s Week 3 Worksheet 1. Atom Q has 3 different Isotopes. It has a relative molar mass of 300 amu. The relative molar masses of its Isotope and their 290 315 ? abundances are listed as: Q(55%) , Q(30%), Q(15%). Find the unknown molar mass of the third Isotope. 300 = 290(.55) + 315(.30) + ?(0.15) ? = 306. 6mu 2. Atom Σ has two Isotopes whose molar masses are 125 amu and 125 196 amu. Σ’s abundance in nature is 300 out of every 600 Σ atoms. What is the relative molar mass of Σ? 300/600 = 0.5 125(.5) + 196(.5) = 160. 5mu is the relative molar mass of Σ 3. The relative molar mass of atom Ψ is 900 amu. If Ψ has only two 896 904 isotopes, Ψ and Ψ, find the relative abundance of each Isotope in nature. 896(x) + 904(1 – x) = 900 x = 0.5 therefore (1 – x) = 0.5 The relative abundace of both Isotopes is 50% 4. How many protons, Neutrons, and electrons does 14C have? 6 p+ 6 + 2 = 8e - 14 – 6 = 8n Amir’s Week 5 Answers AMIR M AHMOODI AMAHMOO 1@ UCIEDU O FFICEHOURS : UESDAY 9-11 AM LOCATION: RH 517 Amir’s Week 6 Worksheet 1) List these atoms from the highest to lowest electronegativity. O, F, N, C, Na, K, Sr, Al, H and explain why this trend exists. F > O > N > C > H > Al > Na > Sr > K This Electronegativity trend exists because as the atomic radius gets smaller and as the atom gets closer to achieving a full shell, it will attract the other atoms’ electrons with more strength. 2) For the above atoms, which ones are capable of making an ionic bond? Write all possible combinations. + - + - 2+ 2- 3+ 3- Na F , K F , Sr O , Al N 3) Which ones will make a covalent bond? Which covalent bond is the most polar? H 2 , O 2 F 2 N ,2CH , 4O , H2…… and many more. However only F, O, N, C, and H can make covalent bonds because they’re non-metals. The most polar bond that can be formed is H – F. 4) Order the above atoms in decreasing atomic radius. K > Sr > Na > Al > C > N > O > F > H 5) Which one has the most endothermic electron affinity: N or F? Explain. Nitrogen has a more endothermic electron affinity because Fluorine will want to give up more energy to obtain an electron because it almost has a full octet and wants it more than Nitrogen does. A  MIR M  AHMOODI  AMAHMOO   1@   UC EDU O  FFICE H  OURS :   UESDAY   9­11 AM L OCATION  : RH 517 Amir’s Week 7 Worksheet Consider the following molecules for questions 1 ­ 4.   a) AsCl 5 and HF b) NaCl and S 3 c) FrF and MgO 1) In which pair do both compounds exhibit predominantly ionic bonding?         In pair c)     2) In which pair do both compounds exhibit predominantly covalent bonding?                    In pair a)     3) From each pair, select the molecule with strongest intermolecular forces and explain  why.     a) HF because of hydrogen bonding.  b) NaCl because of Ionic bonding    c) MgO because 2 , 2  > 1 , 1              4) Based on your knowledge of bond strength, which molecule would have the strongest  bond out of all a, b, and c? Explain.         MgO because Ionic is stronger than any other IMF and 2 , 2  > 1 , 1 ­ + ­ 5) In HOF which bond is stronger? (H­O or O­F) Expalin.  The H­O bond because Hydrogen bonding is much stronger than covalent bonding. AMIR MAHMOODI AMAHMOO 1@ UCI.EDU OFFICEH OURS: UESDAY 9-11AM LOCATION: RH 517 Amir’s Week 8 Worksheet Notice: Come to office hours if you need to see the answers to these questions 1) Draw the Lewis Structure for Cl4 and explain why this is the best structure. Can’t draw it on my laptop but. It is the best structure because you cannot have more than two double bonds to a central atom. (there is not enough room). i) What is the molecular geometry of the Cl atom? Tetrahedral. Sp3 ii) What is the molecular geometry of each of the O atoms? Os without double bond = Tetrahedral Electron geometry and linear molecular molecular geometry. With double bond = Trigonal planar electron geometry and linear molecular geometry 2) What is the molecular geometry of Xe in Xe5 ? Octahedral E’ Geometry but Square Pyramidal molecualr i) What is the molecular geometry of each F? Tetrahedral E’ geometry but Linear molecular ii) Draw the molecule and indicate bond angles. Cant draw on my computer but bond angles are 90, 120, and less than 120. 2- - 3) List these atoms from the biggest to smallest: F , F , and F. Explain why. F > F > F. Because with each added electron, the electron repulsions become higher and push the next orbital out more. AMIR M AHMOODI AMAHMOO 1@ UC.EDU O FFICH OURS: TUESDAY 9-11AM LOCATION: RH 517 Amir’s Week 9 Worksheet 1) List these compounds from highest to lowest boiling points and Explain why the boiling point increases. HF, NaCl, 4H . NaCl > HF > CH Th4s is because Ionic bonds are the strongest bonds followed by dipole to dipole whose strength depends on the electronegativity difference of the atoms in the compound. A) Which one of these compounds can form a Hydrogen bond? Draw this HF is capable of Hydrogen bonding. H-F H-F H-F 2) Complete the Lewis structures of the following molecules, predict their molecular shape, bond angles, and the hybridization of the central atom. Lewis Structures drawn in office hours. Can’t draw them on Word. A) CO3 Trigonal Planar – 120 – Sp Hybrid + B) H3O o 3 Trigonal Pyramidal – less than 109.5 – Sp Hybrid C) CH2O Trigonal Planar – 120 – Sp Hybrid D) CO 2 o Linear – 180 – Sp Hybrid          


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