# Finding Isotope Mass or Natural Abundance from Atomic MassThere are only two naturally-occurring stable isotopes of copper, 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.**Round your entry for \(^{63}\text{Cu}\) to 4 significant digits and your entry for \(^{65}\text{Cu}\) to 4 significant digits.**| Isotope | Mass (amu) | Natural Abundance ||----------|------------|-------------------|| \(^{63}\text{Cu}\) | 62.930 | || \(^{65}\text{Cu}\) | 64.928 | |### Instructional ComponentThe task requires calculating the natural abundance of each copper isotope using data which could be retrieved from an additional source. Once the data is obtained, it is essential to round the values to four significant digits.- **Table Overview**: - The table contains two isotopes of copper, \(^{63}\text{Cu}\) and \(^{65}\text{Cu}\). - Corresponding masses in atomic mass units (amu) are provided. - Natural abundances are indicated as percentages but are initially left blank for calculation.Be sure to utilize accurate atomic mass information to derive the natural abundances correctly. This involves understanding isotope distribution and applying weighted average calculations based on atomic mass.

According to the question we have, The Atomic mass of 63Cu (isotope I) is given by = 62.930 amu The…

Finding isotope mass or natural abundance from atomic mass There are only two naturally-occuring stable isotopes of copper, 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. Round your entry for 63 Cu to 4 significant digits and your entry for 65 Cu to 4 significant digits. isotope 63 Cu 65 Cu mass (amu) 62.930 64.928 natural abundance 0% 0% 0/5 X

Finding isotope mass or natural abundance from atomic mass There are only two naturally-occuring stable isotopes of copper, 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. Round your entry for 63 Cu to 4 significant digits and your entry for 65 Cu to 4 significant digits. isotope 63 Cu 65 Cu mass (amu) 62.930 64.928 natural abundance 0% 0% 0/5 X

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: An element has two naturally occurring isotopes. Isotope 1 has a mass of 184.9530 amuamu and a…

Q: There are only two naturally-occuring stable isotopes of boron. The mass and natural abundance of…

A: Number of naturally occuring stable isotopes of boron = 2Given isotope = 11BMass of given isotope =…

Q: A primary goal of medievel alchemists was to turn base metals in gold. Typically they worked with…

A: Mass number = number of neutrons + number of protons Atomic number = number of protons

Q: There are two naturally occurring isotopes of chlorine. 35 Cl has a mass of 34.9689 u. 37 Cl has a…

Q: Boron has two naturally occurring isotopes: ^10B has a mass of 10.01 amu and 11^B has a mass of…

Q: Given the information below, calculate the abundance and mass for the missing isotope of platinum.…

A: With datas given From the total abundance of percentage , abundance percentage is found and with the…

Q: Calculate the average atomic mass of silver. The percentages denote the relative abundances. Isotope…

A: Given data,Relative abundance of 109Ag=48.16%Relative abundance of 107Ag=51.84%Atomic mass of…

Q: A Chemistry student at Agora is calculating the average atomic mass of Potassium using the following…

A: Given, Relative abundance of potassium Isotope of K Relative abundance K-39 93.12 % K-41…

Q: Back on planet Earth, elements have different isotopic distributions. The atom Chlorine ( Cl ) has…

Q: An unknown element is determined to have two naturally occurring isotopes. Isotope 1 is 62.11%…

A: Atomic mass of element can be determined by adding the product of %abundant and mass of isotopes.…

Q: Back on planet Earth, elements have different isotopic distributions. The atom Chlorine ( Cl ) has…

A: Given isotopic Atomic mass of Cl -35 = 34.968853 amu Isotopic atomic mass of Cl-37 = 36.965903…

Q: Write the atomic symbol for the isotope with mass number 84. Express your answer as an isotope.…

A: An atom is made up of electrons, protons, and neutrons. The nucleus of the atom contains the…

Q: An unknown element X has the following isotopes: 25X (80.50% abundant, mass = 25.03 amu) and 27X…

A: isotopes of X 25X: abundance - 80.50% (P1) = 80.50/100 = 0.8050 mass…

Q: What is the relative atomic mass of the element that consists of the following isotopes in the…

A: Given,

Q: Isn't 'O' the right answer for question Part A or am i wrong if so can someone please help with…

A: In the isotopic symbol of a nuclide, ZXA z indicates the atomic number which means the number of…

Q: a) An element has two naturally occurring isotopes. Isotope l has a mass of 120.9038 u and a…

Q: A manufacturer begins with 15.00 kg15.00 kg of cinnabar and produces 12.93 kg12.93 kg of elemental…

A: Since you have posted multiple questions, we are entitled to answer the first clear question only.…

Q: There are only two naturally-occuring stable isotopes of chlorine, the masses of which are listed in…

Q: ne element carbon has two naturally occurring isotopes. The isotopic masses and abundances of these…

Q: The most abundant isotope of Hydrogen has a mass of 1 amu. Therefore, the average atomic mass on…

Q: A made up element ey has three natural isotopes. The isotopes each have an atomic mass of 33.02…

Q: Be sure your answers have the correct number of significant digits. mass natural isotope Ox10 (amu)…

A: The average atomic mass of element is equal to the product of the masses of the isotope and its…

Q: Magnesium has three stable isotopes. The most commonly occurring isotope, 24Mg, has an isotopic mass…

A: Average atomic mass of an atom can be calculated using the mass of their isotopes and their…

Q: Which orbital is lower in energy in a many-electron atom? 4s O 3s X S

A: Energy of sub orbitals are gone by above principle and (n +l)rule

Q: An element exist as 3 isotopes in nature. The isotopic masses (in amu) and percent abundance’s are…

A: The average atomic mass of element is equal to the product of the masses of the isotope and its…

Q: In Star Trek, a (fake) element that often plays a role in the plot is dilithium (Dt), which has…

A: Since the % abundance is not given exactly, it is a variable, thus answer will be given in terms of…

Q: An element has three naturally occurring isotopes with the following masses and natural abundances:…

A: In order to calculate relative atomic mass, simply multiply each isotopic mass by the percentage…

Q: There are two naturally occurring isotopes of boron. 10B has a mass of 10.0129 u.11B has a mass of…

A: Given, Atomic mass of 10B (isotope I) = 10.0129 u Atomic mass of 11B (isotope II) = 11.0093 u Let…

Q: The newly-discovered "element ~X" has 3 stable isotopes, each with the listed mass and abundance.…

Q: Zinc has five naturally occurring isotopes with an average mass of 65.39 amu. If two isotopes,…

A: To answer: Which pair of isotopes will have the highest abundances? 64Zn, 63.9291 amu and 66Zn,…

Q: There are only two naturally-occuring stable isotopes of boron, the masses of which are listed in…

Q: A robot spacecraft returned samples from the planetesimal 98765 ALEKS, located in the outer Solar…

A: The elements which have same atomic number but different atomic masses are known as…

Q: Enter your answer in the provided box. Calculate the atomic weight of the element given the mass…

A: A numerical problem based on nuclear chemistry, which is to be accomplished.

Q: There are only two naturally-occuring stable isotopes of lithium. The mass and natural abundance of…

Concept explainers

Atomic Structure

The basic structure of an atom is defined as the component-level of atomic structure of an atom. Precisely speaking an atom consists of three major subatomic particles which are protons, neutrons, and electrons. Many theories have been stated for explaining the structure of an atom.

Shape of the D Orbital

Shapes of orbitals are an approximate representation of boundaries in space for finding electrons occupied in that respective orbital. D orbitals are known to have a clover leaf shape or dumbbell inside where electrons can be found.

Question

# Finding Isotope Mass or Natural Abundance from Atomic Mass

There are only two naturally-occurring stable isotopes of copper, 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.

**Round your entry for \(^{63}\text{Cu}\) to 4 significant digits and your entry for \(^{65}\text{Cu}\) to 4 significant digits.**

| Isotope | Mass (amu) | Natural Abundance |
|----------|------------|-------------------|
| \(^{63}\text{Cu}\) | 62.930 | |
| \(^{65}\text{Cu}\) | 64.928 | |

### Instructional Component

The task requires calculating the natural abundance of each copper isotope using data which could be retrieved from an additional source. Once the data is obtained, it is essential to round the values to four significant digits.

- **Table Overview**:
- The table contains two isotopes of copper, \(^{63}\text{Cu}\) and \(^{65}\text{Cu}\).
- Corresponding masses in atomic mass units (amu) are provided.
- Natural abundances are indicated as percentages but are initially left blank for calculation.

Be sure to utilize accurate atomic mass information to derive the natural abundances correctly. This involves understanding isotope distribution and applying weighted average calculations based on atomic mass.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

What is the chemical symbol and the name of an element with three different isotopes with the corresponding mass (amu) and abundance (%): isotope 1 mass of 23.99 and abundance of 78.70, isotope 2 mass of 24.99 and abundance 10.13, isotope 3 mass of 25.98 and abundance of 11.17.
There are only two naturally-occuring stable isotopes of chlorine. The mass and natural abundance of one of them is listed in the table below. Use whatever data you need from the ALEKS Periodic Table to determine the identity, mass and natural abundance of the other isotope, and complete the table. Be sure your answers have the correct number of significant digits. isotope 35 Cl Da mass (amu) 34.969 0 natural abundance 75.78% % 0 X 000 Ar
There are only two naturally-occuring stable isotopes of boron. The mass and natural abundance of one of them is listed in the table below. Use whatever data you need from the ALEKS Periodic Table to determine the identity, mass and natural abundance of the other isotope, and complete the table. Round your entry for mass to 3 significant digits and your entry for natural abundance to 3 significant digits. isotope 10B OB В mass (amu) 10.013 0 natural abundance 19.9% % x10 X Ś
An unknown element is determined to have two naturally occurring isotopes. Isotope 1 is 68.11% abundant and has a mass of 68.925580 amu, and isotope 2 has a mass of 70.9247005 amu. Determine the atomic mass of the unknown element. Express your answer to four significant figures.
There are only two naturally-occuring stable isotopes of chlorine, 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. 35 Round your entry for C1 to 4 significant digits and your entry for isotope 35 Cl 37 Cl mass (amu) 34.969 36.966 natural abundance 1% % ☐x10 X 37 C1 to 4 significant digits. Ś
Part 1 As seen on the periodic table, the element silicon (Si) has an atomic mass of 28.086 amu. This element is composed of three naturally-occurring isotopes. The first isotope, silicon-28, has a mass of 27.977 amu and a natural abundance of 92.229%. The second isotope, silicon-30, has a mass of 29.974 amu and a natural abundance of 3.087%. What is the mass (in amu) of silicon's third isotope? write your final answer (with the correct significant figures) Part 2 Based on the answer for part 1, the name of the third isotope of silicon is ___. An atom of that particular isotope contains___ protons and ____ neutrons.
A robot spacecraft returned samples from the planetesimal 98765 ALEKS, located in the outer Solar System. Mass-spectroscopic analysis produced the following data on the isotopes of tin in these samples: mass relative isotope (amu) abundance 112 Sn 90.3% 111.9 119 Sn 9.7% 118.9 Use these measurements to complete the entry for tin in the Periodic Table that would be used on 98765 ALEKS. Round your entry for the atomic mass to 3 significant digits. Caution: your correct answer will have the same format but not necessarily the same numbers as the entry for tin in the Periodic Table we use here on Earth. Sn
1- For each of the following atoms, calculate the number of protons and neutrons in the nucleus and the number of electrons outside the nucleus (assume neutral atoms). element number of number of number of electrons mass number (A) symbol 126C protons (Z) neutrons 12 10 12 10 14 27 10 23,1Na 11 17 18 2- Calculate the atomic mass to four significant figures for carbon, given the following data: Isotope Exact Atomic Mass (amu) 12.00000 13.00335 Abundance in Nature (%) 98.89 1.110 12C 13C
T Please don't provide the handwriting solution
Write the atomic symbols for isotopes with the following characteristics: 16 protons and 16 neutrons Express your answer as an isotope. 35 protons and 45 neutrons Express your answer as an isotope. 13 electrons and 14 neutrons Express your answer as an isotope. an iodine atom with 74 neutrons Express your answer as an isotope. a mercury atom with 122 neutrons Express your answer as an isotope.
A hypothetical element, M, has four stable isotopes with the masses shown below. 109M = 108.9842 amu 107M = 106.9085 amu 105M = 104.9904 amu 103M = 102.9991 amu If the percentage abundance of 109M is 10.5%, 105M is 6.6% and the average atomic mass of M is 106.6785 amu, then what is the percentage abundance for 103M? Enter your answer as a percentage but without the % symbol. Use one decimal place.
I need help with #3