Isotope+mnm+Lab copy 2

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A particular element "X" has two naturally occurring isotopes: Isotope of "X"                                   Approximate % Abundance                   X-79                                                               50.7% X-81                                                               49.3% Calculate the atomic mass of an atom of "X" Report the answer with the correct units and round to one decimal place. Also, identify the element represented by "X" based on your calculated atomic mass.  Identity of element "X" based on the atomic mass _________________?

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Model 5: Isotope Natural Abundances Atom Most common isotope C O S N CI Br 12C (100) 160 (100) 32S (100) 14N (100) 35 CI (100) Jump in Mass Next most common isotope (no. extra neutrons) (no. found for every 100 atoms of most common isotope) +1 13C (1.11) 180 (0.20) 34S (4.40) 15N (0.38) 37 Cl (32.5) "¹Br (98.0) 79Br (100) For example: There are 1.11 *C atoms on the planet for every 100 ¹2C atoms. Equivalent ways of saying this are: There are likely to be 111 1³C atoms in a sample of 10,111 carbon atoms or 1.10% of the carbon on the planet is 1³C (since 111/10,111 x 100% = 1.10%). Critical Thinking Questions 15. What does the superscript to the left of each atom label tell you (e.g., the 12 in ¹2C)?

Element: Lead Number of Number of Abundar (decima Name of isotope Mass (amu) Abundance Protons Neutrons (%) Lead-204 203.973 Lead-206 205.974 24.10% Lead-207 206.976 22.10% Lead-208 207.977 52.40% Isotope Mass Abundance

Use the periodic table to find the atomic masses for carbon and oxygen in order to show that the mass is conserved for the following chemical equation : 2CO(g) + O_{2}(g) -> 2C*O_{2}(g)

Convert 1.00 g of each element to moles. How many moles of beryllium are in 1.00 g? 1.00 g Be= How many moles of manganese are in 1.00 g? $ 1.00 g Mn = F How many moles of carbon are in 1.00 g? 14 R %6 G Search or type URL 5 T G B tv 6 MacBook Pro Y H 9 N U J 8 M I K ( 9 < O < H I 2Me -0 O L 10 command P : ; T { option ? mol Be mol Mn I 1 de

4 of 13 M Review Constants Periodic Tabl What is the mass percentage of each element in the compound Al2O3? Enter the percent mass of aluminum and the percent mass of oxygen, respectively, separated by a comma. View Available Hint(s) Πν ΑΣφ % Al, % O = Submit Request Answer 10:30 PM 81% 2/13/2020 *- F11 Insert Delete PrtSc F12 F9 F7 F8 F10 & Backspace 9. +II * 08

A fictitious element Z has an average atomic mass of 223.21 u.223.21 u. Element Z has two naturally occuring isotopes. The more abundant isotope has an exact mass of 224.42 u224.42 u and a relative abundance of 60.75%.60.75%. Calculate the exact mass of the second isotope.   mass of second isotope: _______________________ u

An unknown element has two naturally occurring isotopes with the following isotopic masses: X-205 (204.77235 amu) and X-207 (206.10897 amu). The average atomic mass of this element is 205.87 amu. The fractional abundance of the lighter of the two isotopes is __________.

Introduction to Soll Scdence- Lab 3 Chemial Elements Name Date Some lasics regarding Chemical Elements A Chemical element found on the Perlodic Table of Elements (found on the Inside cover of your text) isa pure substance which cannot be decomposed by chemical change. The names of Elements are often abbrevlated to slmplify formoulas ustng these elements. These abbreviations are refened to u chemical symbols. For Hydrogen, the symbol "H', for Onygen, "O, and for Carbon, "C. Sometimes two letters are necessary to distingutsh bebween two or more elements when the names of the elements begin with the sume letter. For Example Ca for Caldum. Cr for Chromlum, Co for Cobalt, Cl for Chlorine, etc. No symbols contain more than two letters and the first letter is always capitalized. Some symbolk are abbrevlations of Latin names ofelements (Le. Fe for Iron; Latin, ferrum). Each Element has an atomic number and an atomic welght. The welght is in relative ternos as an atom of exch element is…

Row 2: Your answer is incorrect. olo There are only two naturally-occuring stable isotopes of boron, the masses of which are listed in the table below. Use whatever data you need from the ALEKS Periodic Table to calculate the natural abundance of each isotope and complete the table. 10. 11 Ar Round your entry for "B to 3 significant digits and your entry for "B to 3 significant digits. mass natural isotope x10 (amu) abundance 10B % 10.013 11.009