Skip to main content
Ch.2 - Atoms, Molecules & Ions
McMurry - Chemistry 8th Edition
McMurry8th EditionChemistryISBN: 9781292336145Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoMcMurry 8th EditionCh.2 - Atoms, Molecules & IonsProblema 123
Capitolo 2, Problema 123

Germanium has five naturally occurring isotopes: 70^Ge, 20.5%, 69.924; 72^Ge, 27.4%, 71.922; 73^Ge, 7.8%, 72.923; 74^Ge, 36.5%, 73.921; and 76^Ge, 7.8%, 75.921. What is the atomic weight of germanium?

Guida verificata passo dopo passo
1
Identify the mass number and relative abundance for each isotope of Germanium. For example, for the isotope 70^Ge, the mass number is 69.924 and its abundance is 20.5%.
Convert the percentage abundance of each isotope into a decimal by dividing by 100. For instance, 20.5% becomes 0.205.
Multiply the mass number of each isotope by its decimal abundance to find the weighted contribution of each isotope to the overall atomic weight. For 70^Ge, this would be 69.924 multiplied by 0.205.
Sum the weighted contributions of all isotopes to get the total atomic weight of Germanium. Add the results from the previous step for all isotopes.
The sum calculated in the previous step represents the atomic weight of Germanium.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
2m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

Isotopes

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons, resulting in different atomic masses. For example, germanium has several isotopes, each with a unique mass and natural abundance, which contribute to the element's average atomic weight.
Video consigliato:
Percorso guidato
04:36
Isotopes

Atomic Weight Calculation

The atomic weight of an element is calculated as the weighted average of the masses of its isotopes, taking into account their relative abundances. This involves multiplying the mass of each isotope by its percentage abundance (expressed as a fraction) and summing these values to obtain the overall atomic weight.
Video consigliato:
Percorso guidato
02:00
Calculating Atomic Mass

Percentage Abundance

Percentage abundance refers to the proportion of each isotope of an element present in a natural sample, expressed as a percentage. In the case of germanium, each isotope's abundance must be converted to a decimal fraction to accurately calculate the weighted average for the atomic weight.
Video consigliato:
Percorso guidato
5:41
Calculating Abundance Example
Pratica correlata
Domanda del libro di testo
A sample of naturally occurring silicon consists of 28^Si (27.9769), 29^Si (28.9765), and 30^Si (29.9738). If the atomic weight of silicon is 28.0855 and the natural abundance of 29^Si is 4.68%, what are the natural abundances of 28^Si and 30^Si?
822
views
Domanda del libro di testo
What is the mass in grams of each of the following samples? (a) 1.505 mol of Ti (b) 0.337 mol of Na (c) 2.583 mol of U
1039
views
Domanda del libro di testo

Magnesium has three naturally occurring isotopes: 24Mg (23.985) with 78.99% abundance, 25Mg (24.986) with 10.00% abundance, and a third with 11.01% abundance. Look up the atomic weight of magnesium, and then calculate the mass of the third isotope.

6869
views
1
rank
1
comments
Domanda del libro di testo
Copper metal has two naturally occurring isotopes: copper-63 (69.15%; isotopic mass = 62.93) and copper-65 (30.85%; isotopic mass 64.93). Calculate the atomic weight of copper, and check your answer in the periodic table.
2367
views
Domanda del libro di testo
How many moles are in each of the following samples? (a) 11.51 g of Ti (b) 29.127 g of Na (c) 1.477 kg of U
915
views