Chapter 3 1. 1 atom of X = atomic mass (amu) 1 mole f X=atomic mass in grams 1 mole of something = 6.022 x 1023 units of that substance 1 mole of a compound =66.022 x 1023 atoms 6.022 x 1023 amu =1 g 2. What is the mass of 6 atoms of Fe? Answer: 6 atoms of Fe x 55.85 amu÷atom of Fe x 1 g of Fe÷6.022 x 1023 amu = 3. How many atoms does it take to make 1 g of Gold (Au)? Answer: 197.0 g Au =1 mole of Au
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produced? A) 48.8 g B) 32.5 g C) 131.2 g D) 73.2 g E) 65.1 g 2. Naturally occurring element X exists in three isotopic forms: X-28 (27.979 amu‚ 92.21% abundance)‚ X-29 (28.976 amu‚ 4.70% abundance)‚ and X-30 (29.974 amu‚ 3.09% abundance). Calculate the atomic weight of X. A) 28.09 amu B) 35.29 amu C) 28 amu D) 86.93 amu E) 25.80 amu 3. The Claus reactions‚ shown below‚ are used to generate elemental sulfur from hydrogen sulfide. 2H2S + 3O2 2SO2 + 2H2O SO2 + 2H2S 3S
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Structure of An Atom Table: Properties & Location of Protons‚ Neutrons & Electrons In Atom Subatomic Symbol Relative Mass Mass Location Particle electrical (g) (amu) charge Proton p+ +1 1.6726 1 In the x 10-24 nucleus Electron e-1 9.1094 0.0005 Outside x 10-28 the nucleus Neutron n0 0 1.6749 1 In the x 10-24 nucleus 1 atomic mass unit (amu) = 1.6605 x 10-24 g ATOMIC NUMBER (Z) Number of
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mass of 62.9296 amu. Copper-65 is 30.83% abundant and it has a mass of 64.9278 amu. What is the weighted average mass of these two isotopes? 3. Calculate the atomic mass of silicon. The three silicon isotopes have atomic masses and relative abundances of 27.9769 amu (92.2297%)‚ 28.9765 amu (4.6832%) and 29.9738 amu (3.0872%). 4. Gallium has two naturally occurring isotopes. The mass of gallium-69 is 68.9256 amu and it is 60.108% abundant. The mass of gallium-71 is 70.9247 amu and it is 39.892%
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Assignment 1. Questions from chapters 1 and 2 of McMurry and Fay Question numbers are from the fourth edition. Chapter 1. Chemistry: Matter and Measurement 1 1.1 1.2 1.3 (a) Cd (b) Sb (a) silver (c) Am (c) rhenium (d) cesium (e) argon (f) arsenic (b) rhodium (a) Ti‚ metal (d) Sc‚ metal (b) Te‚ semimetal (e) At‚ semimetal (c) Se‚ nonmetal (f) Ar‚ nonmetal 1.4 1.5 The three Acoinage metals@ are copper (Cu)‚ silver (Ag)‚ and gold (Au). (a) The decimal point must be shifted
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weight of a proton is one amu. Protons are located inside the nucleus and cannot move from inside the nucleus. The proton symbol is . Neutrons are also located inside the nucleus and have a neutral charge. Neutrons are also one amu like protons. Neutrons can move from the nucleus of an atom making an atom an isotope. The neutron symbol is . Electrons are located outside the nucleus in energy levels. Electrons have a negative charge and weigh approximately 1/2000th of an amu. The weight is almost
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mole limiting reactant 5 feet 10 inches to meters 55 miles per hour to cm per second 5.0 quarts to liters 1.00 ft2 to cm2 32.06 amu to g 25 g of carbon to moles of carbon 1.00 g of gold to number of atoms of gold 25 °F to Kelvins How many significant figures are in the following numbers? a) 3.1416 b) 6.022 X 1023 atoms/mole c) 0.000104 g d) 6.0 g/mL e) 1.00794 amu f) 5000 mi 5. Perform the following operations and give the correct number of significant figures in your answers. a) (0.031
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Atomic masses: Proton 1.672621777(74) × 10^-27 kg 1.007276466812(90) amu Neutron 1.674927351(74) × 10^−27 kg 1.00866491600(43) amu Electron 9.10938291(40) × 10^−31 kg 5.4857990946(22) × 10^−4 amu What is an Isotope? -An Isotope is an Atom with the same number of protons‚ but differing numbers of neutrons. Isotopes are different forms of a Single element. Elements and their uses to our human body Oxygen is the third most abundant element found in the sun‚ and it plays
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atom _loses_ (lose‚ gain) electrons. 5. Calculate the atomic mass of the following sample of Silicon. 92.21 % 28Si‚ 4.70% 29Si‚ and 3.09% 30Si. Answer to 2 decimal places‚ remember units. 0.9221 x 28 = 25.8188 amu 0.0470 x 29 = 1.363 amu 0.0309 x 30 = 0.927 amu 28.1088 amu = 28.11 amu 6. When at atom gains two electrons‚ it becomes an ion with a charge of _-2___. Nuclear Chemistry Complete the following nuclear decay reactions. Type of Decay (α‚ β‚ γ) 7. __gamma____ 99m43Tc 9943Tc
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CHAPTER 4 The Structure of the Atom Resource Manager Section 86A Objectives Activities/Features Section 4.1 1. Compare and contrast the atomic Discovery Lab: Observing Electrical Early Theories of Matter 1 session 1/2 block models of Democritus and Dalton. 2. Define an atom. Charge‚ p. 87 Section 4.2 3. Distinguish between the subatomic Problem-Solving Lab: Interpreting STM Subatomic Particles and the Nuclear Atom 1 session 1/2 block particles in terms of relative charge and mass
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