7. If an element, “X" has two isotopes with the following masses and abundances: 46X = 45.974 amu , 24.32% abundance 38X = 38.012 amu , 75.68% abundance Calculate the relative atomic mass of the element "X"? Identify the element “X".

7. If an element, “X" has two isotopes with the following masses and abundances: 46X = 45.974 amu , 24.32% abundance 38X = 38.012 amu , 75.68% abundance Calculate the relative atomic mass of the element "X"? Identify the element “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

Chapter3: Stoichiometry

Section: Chapter Questions

Problem 43E: The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has...

See similar textbooks

Related questions

Q: Three magnesium isotopes have atomic masses and relative abundances of 23.985 amu (79.99%), 24.986…

A: The atomic of an element = Σ Atomic mass ( Isotope ai ) X Abundance (Isotope ai) Atomic masses and…

Q: Almost all boron atoms are found in two forms: boron-10 and boron-11. Both isotopes behave alike…

A: Given, Boron atoms are found in two forms: boron-10 and boron-11 Average mass of B = 10.81 amu

Q: Magnesium (average atomic mass = 24. 305 amu) consists of three isotopes with masses 23.9850 amu,…

A: Given: average atomic mass = 24. 305 amu three isotopes with masses 23.9850 amu, 24.9858 amu, and…

Q: Indium has two isotopes. One of the isotopes has an atomic weight of 114.9 amu and an abundance of…

Q: Gallium has two naturally occurring isotopes with the follow- ing masses and natural abundances:…

Q: An element X exists as two isotopes - 46X and 49X and weigh 45.95 amu and 48.95 amu, respectively.…

A: Given :- Atomic wt.of 46X = 45.95 amu Atomic wt.of 49X = 48.95 amu Average atomic wt.of X = 46.66…

Q: An unknown element is determined to have two naturally occurring isotopes. Isotope 1 has a mass of…

Q: A certain element XX has four isotopes. 0.5600% of XX has a mass of 83.91343 amuamu. 9.860% of XX…

Q: Consider the following atoms in which X represents the chemical symbol of the element:11/22X,…

A: In an atom of the element, there is a nucleus present in the center. protons and neutrons are…

Q: 6. Isotopes. Silicon (Si) is a major component of semiconductor chips. It has three naturally…

A: Calculate electron, proton and neutron in each case---

Q: Question attached

A: Given data contains, Abundance of X53 is 19.61. Mass of X53 is 52.62. Abundance of X56 is 53.91.…

Q: An unknown element is a mixture of isotopes ¹²⁹X and ¹³²X. The average atomic mass of X is 129.47…

A: Average atomic mass has Following formula - Average atomic mass = atomic mass of first isotope × % +…

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 isotope is used as the standard in establishing the atomic mass scale? The atomic weight of…

A: The mass number given in the periodic table is the average mass of all the isotopes of an element.…

Q: Fill in the gaps in the following table: Symbol P3- Protons 35 49 Neutrons 45 66 118 Electrons 46 76…

Q: Which pair of atoms constitutes a pair of isotopes of the same element? 29. 14 28 58 B) X 26 A) X…

A: Isotopes are defined as the elements having same atomic number but different mass number. X1328…

Q: Consider the following atoms in which X represents the chemical symbol of the element: 19/42X,…

A: Atomic number gives the number of protons present in the nucleus or the number of electrons present…

Q: Three of the isotopes of Tellurium, Te, have mass numbers of 124, 126, and 130. Tellurium-124 has 52…

A: Isotope label is same as isotope notation and is written as follows: Xnm is the isotope label where…

Q: Consider an element Z that has two naturally occurring isotopes with the following percent…

A: average atomic mass= ∑%abundant×Molar mass/100 using this we can calculate the average atomic mass…

Q: An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99…

A: Given, Natural abundances (in %) with isotopic masses (in amu )90.92% with 19.99 amu0.26% with 20.99…

Q: An element consists of two isotopes. The abundance of one isotope is 95.72% and its atomic mass is…

A: From given Mass and percentage is given . So average atomic mass is determined by using the formula…

Q: The atomic mass of bromine is 79,904 amu. The atomic mass of the Br-81 isotope is 80.9163 amu and…

A: The atomic mass of bromine is 79.904 amu. This is actually the average atomic mass of Bromine which…

Q: If a fictitious element, X, has 2 naturally occurring isotopes; X-44 and X-46. The atomic mass of…

A: Given: Fictitious element, X, has 2 naturally occurring isotopes; X-44 and X-46. The atomic mass of…

Q: 151 has an abundance of 48.03% and Europium-153 has an abundance of 51.97%. What is the atomic mass…

A: Calculation of average masses and abundance of isotopes.

Q: 1. Here are three isotopes of an element: a. The element is: 19"K "K “K b. The number 19 refers to…

A: Isotopes are those compounds which have same atomic number but different mass number. Here given…

Q: A hypothetical element exists as two isotopes: I = 92.00 amu and II = 98.00 amu. If the atomic mass…

A: Suppose fraction of isotope I = A Fraction of isotope II = (1 - A) Atomic mass = A x atomic mass of…

Q: An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99…

A: Given natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abudance with…

Q: What is the average atomic mass of chlorine if the mass of one isotope is 34.97 amu and has a per…

A: The average atomic mass of an element can be calculated as shown below.

Q: 4.38 Strontium has four naturally occurring isotopes, with mass numbers 84, 86, 87, and 88. a. Write…

A: To find: Why is the atomic mass of strontium listed on the periodic table not a whole number? Which…

Q: A completely made up element called Krystogen has two naturally occurring isotopes. The atomic…

A: Every atom in periodic table has some atomic mass and atomic number. When atomic number of two…

Q: A 5.235.23 g sample of calcium sulfide was decomposed into its constituent elements, producing…

A: According to Law of Definite Proportions, compounds always occur in a certain fixed ratio. For…

Q: An unknown element is a mixture of sotopes 129X and 132X. The average atomic mass of X is 130.35…

Q: Sycamorium Sy, a hypothetical element occurs in three isotopes, who masses and abundances are given…

A: Given: Isotope Mass Abundance Isotope1 297.021 21.9% Isotope2 299.010 33.3% Isotope3…

Q: 5. A sample of Magnesium contains three isotopes and its average atomic weight is 24.35 amu. If the…

Q: What is the average atomic mass of an element that has 3 isotopes with the data below? Isotope…

A: Average Atomic mass=((molecular mass Isotope 1 x % abundance )+(molecular mass Isotope 2 x %…

Q: An unkown element is a mixture of isotopes 120X and 122X. Theaverage atomic mass of X is 121.58 amu.…

A: • Two Isotopes 120X and 122X average atomic = 121.58 amu.Suppose the amount of 122X = y…

Q: An imaginary element Xq consists of two isotopes having masses of 100.0 amu and 102.0 amu. A sample…

A: When an element exists in the form of two or more than two isotopes, the term average atomic mass Is…

Q: what is the average atomic mass for a hypothetical element that has two isotopes with relative…

A: Given two isotopes with relative masses and % abundances as follows: 12.2 amu, 25%; and 13.3 amu,…

Q: SCH3U Isotopes and Isotopic Abundance 1. What are the names, symbols, electrical charges, and…

A: (1) There are following three subatomic particles in an atom - Subatomic particle name Symbol…

Q: 1. Use the concepts of relative abundance and relative weight to explain why carbon has an atomic…

A: If the element have isotopes then its average atomic mass is calculated.

Q: [Atomic mass and isotopes] An unknown element has two naturally occurring isotopes: X- 69 and X-71.…

A: Given Natural abundance of X-71 = 49.31% Mass of X-71 = 70.9163 amu

Q: Silver has two naturally occurring isotopes, 107Ag (isotopic mass 106.90509 amu) and 109Ag (isotopic…

A: Assuming the percent abundance of 109Ag isotope is y. Hence the percent abundance of 107Ag isotope…

Q: 4) Chromium has four isotopes. Chromium-50 (mass of 49.946 amu and 4.35% abundance), chromium-52…

A: Given, The chromium four isotopes are Chromium-50, (mass= 49.946 amu, % of abundance = 4.35% ),…

Q: On another planet, the isotopes of titanium have the given natural abundances. Mass (u) Isotope 46T¡…

A: The atomic mass and abundance of the isotopes of Ti given are,

Q: On the planet Invertios, boron has two isotopes as follows: Isotope Mass (amu)…

A: Many naturally occuring elements exists as more than one isotope. On the basis of their percentage…

Q: Rubidium has two naturally occurring isotopes: 85 Rb (atomic mass = 84. 9118 AMU)and 87 Rb (atomic…

Q: Silver has two isotopes, one with 60 neutrons (percent abundance = 51.839%) and the other with 62…

A: Given: Silver has two isotopes. percent abundance of Isotope with 60 neutrons ( Ag47107 ) = 51.839%…

Q: Potassium (atomic mass= 39.10 amu) has three isotopes with masses 38.9367 amu, 39.9640amu, and 40.…

A: Given, Atomic Mass of Potassium = 39.10 amu Three isotopes having masses : 38.9367 amu , 39.9640 amu…

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

7. If an element, “"X" has two isotopes with the following masses and abundances:
46X = 45.974 amu , 24.32% abundance
38X = 38.012 amu , 75.68% abundance
Calculate the relative atomic mass of the element “X"? Identify the element “X".

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

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

The element europium exists in nature as two isotopes: 151Eu has a mass of 150.9196 u and 153Eu has a mass of 152.9209 u. The average atomic mass of europium is 151.96 u. Calculate the relative abundance of the two europium isotopes.
Chlorine has two isotopes, Cl-35 and Cl-37. Their abundances are 75.53% and 24.47%, respectively. Assume that the only hydrogen isotope present is H-1. (a) How many different HCI molecules are possible? (b) What is the sum of the mass numbers of the two atoms in each molecule? (c) Sketch the mass spectrum for HCI if all the positive ions are obtained by removing a single electron from an HCI molecule.
2.91 Strontium has four stable isotopes. Strontium—84 has a very low natural abundance, but 86Sr, 87Sr, and 88Sr are all reasonably abundant. Knowing that the atomic weight of strontium is 87.62, which of the more abundant isotopes predominates?
A hypothetical element X is found to have an atomic weight of 37.45 amu. Element X has only two isotopes, X-37 and X-38. The X-37 isotope has a fractional abundance of 0.7721 and an isotopic mass of 37.24. What is the isotopic mass of the other isotope?
Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the Mix Isotopes tab, hide the Percent Composition and Average Atomic Mass boxes, and then select the element boron. Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts. Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice. Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes from their bins or click on More and then move the sliders to the appropriate amounts. Reveal the Percent Composition and Average Atomic Mass boxes. How well does your mixture match with your prediction? If necessary, adjust the isotope amounts to match your prediction. Select Nature’s mix of isotopes and compare it to your prediction. How well does your prediction compare with the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match Nature’s amounts as closely as possible. 21. Repeat Exercise 2.20 using an element that has three naturally occurring isotopes.
2.92 A candy manufacturer makes chocolate-covered cherries. Although all of the products look roughly the same, 3% of them are missing the cherry. The mass of the candy with a cherry is 18.5 g; those missing the cherry weigh only 6.4 g. (a) How would you compute the average mass of a box of 100 of these chocolate covered cherries from this manufacturer? (b) I low is this question analogous to the determination of atomic weights?
Two elements, R and Q, combine to form two binary compounds. In the first compound, 14.0 g of R combines with 3.00 g of Q. In the second compound, 7.00 g of R combines with 4.50 g of Q. Show that these data are in accord with the law of multiple proportions. If the formula of the second compound is RQ, what is the formula of the first compound?
2.90 Naturally occurring europium has an average atomic weight of 151.964 amu. If the only isotopes of europium present are 151Eu and 153Eu, describe how you would determine the relative abundance of the two isotopes. Include in your description any information that would need to be looked up.
Two samples of different compounds of sulfur and oxygen have the following compositions. Show that the compounds follow the law of multiple proportions. What is the ratio of oxygen in the two compounds for a fixed amount of sulfur? Amount S Amount O Compound A l.210g 1.811 g Compound B 1.783 g 1.779 g
There are 2.619 1022 atoms in 1.000 g of sodium. Assume that sodium atoms are spheres of radius 1.86 and that they are lined up side by side. How many miles in length is the line of sodium atoms?
Click on the site (http://openstaxcollege.org/l/16PhetAtomMass) and select the Mix Isotopes tab, hide the Percent Composition and Average Atomic Mass boxes, and then select the element boron. Write the symbols of the isotopes of boron that are shown as naturally occurring in significant amounts. Predict the relative amounts (percentages) of these boron isotopes found in nature. Explain the reasoning behind your choice. Add isotopes to the black box to make a mixture that matches your prediction in (b). You may drag isotopes from their bins or click on More and then move the sliders to the appropriate amounts. Reveal the Percent Composition and Average Atomic Mass boxes. How well does your mixture match with your prediction? If necessary, adjust the isotope amounts to match your prediction. Select Nature’s mix of isotopes and compare it to your prediction. How well does your prediction compare with the naturally occurring mixture? Explain. If necessary, adjust your amounts to make them match Nature’s amounts as closely as possible.
2.74 The accompanying table provides the identity of the two naturally occurring isotopes for four elements and the atomic weights for those elements. (In each case, the two isotopes differ in mass number by two.) Which element has the mass spectrum shown? Explain your answer.