Ch.2 - Atoms & ElementsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

Solution: Chorline exists mainly as two isotopes 35Cl and 37Cl,a) Which is more abundant?b) How do you know?c) Compute the percentage of chlorine that is the 37Cl isotope.

Problem

Chorline exists mainly as two isotopes 35Cl and 37Cl,

a) Which is more abundant?

b) How do you know?

c) Compute the percentage of chlorine that is the 37Cl isotope.

Solution

Isotopes represent atoms of an element that contain the same atomic number (same number of protons), but different mass numbers (different number of neutrons). 


a. 35Cl is more abundant


b. The average atomic mass of Cl is 35.45 amu. 

Since 35.45 amu is closer to the mass of 35Cl (35 amu) than 37Cl (37 amu), this means that 35Cl has a mass greater contribution to 35.45 as compared to 37Cl


We’re being asked to percent 37Cl. We can use the following equation:


Atomic Mass = mass×f.a.isotope 1+mass×f.a.isotope 2


where atomic mass = average atomic mass of the element and f.a. = fractional abundance of the isotope


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