Last, need help with question Number 5 D. Empty Volume Determination of AluminumA sample of aluminum weighs 27.0 g and has a volume of 10.0 cm3. The atomic radiusof metallic aluminum has been determined by x-ray diffraction to be 0.143 nm. There are 6.02x 1023 total atoms in the piece of metal.1. Calculate the volume of individual atoms assuming that atoms are spheres.2. Calculate the volume of atoms in the sample3. Calculate the volume of the empty space in the aluminum sample4. Calculate the percentage of the empty space in the aluminum sample5. What kind of unit will the aluminum sample have? Explain your answer.

Answered: Image /qna-images/answer/724bcef4-89e4-4fb2-b302-b704bb0190bd.jpg

Answered: D. Empty Volume Determination of…

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter5: Atomic Theory : The Nuclear Model Of The Atom

Section: Chapter Questions

Problem 62E

See similar textbooks

Similar questions

A cylindrical piece of pure copper (d=8.92g/cm2) has diameter 1.15 cm and height 4.00 inches. How many atoms are in that cylinder? (Note: the volume of a right circular cylinder of radius r and height h is V=r2 h .)
A combustion reaction involves the reaction of a substance with oxygen gas. The complete combustion of any hydrocarbon (binary compound of carbon and hydrogen) produces carbon dioxide and water as the only products. Octane is a hydrocarbon that is found in gasoline. Complete combustion of octane produces 8 L of carbon dioxide for every 9 L of water vapor (both measured at the same temperature and pressure). What is the ratio of carbon atoms to hydrogen atoms in a molecule of octane?
We have seen that the reactivity of an element is determined by its electron configuration. What is the electron configuration of the ion Cl-? (Hint: You must add one additional electron beyond the number of electrons that chlorine would normally have.) How does its reactivity compare with neutral Cl? How would the reactivities of Na and Na+ compare?
Scientists J. J. Thomson and William Thomson (Lord Kelvin) made numerous contributions to our understanding of the atom’s structure. Which subatomic particle did J. J. Thomson discover, and what did this lead him to postulate about the nature of the atom? William Thomson postulated what became known as the “plum pudding” model of the atom’s structure. What did this model suggest?
Do the proton and the neutron have exactly the same mass? How do the masses of the proton and the neutron compare to the mass of the electron? Which particles make the greatest contribution W the mass of an atom? Which particles make the greatest contribution to the chemical properties of an atom?
lton believed that atoms were indivisible. Thomson and Rutherford helped to show that this was not true. What if atoms were indivisible? How would this affect the types of reactions you have learned about in this chapter?
One of the best indications of a useful theory is that it raises more questions for further experimentation than it originally answered. Does this apply to Daltons atomic theory? Give examples.
Your friend tells you about an article that he read in a tabloid that reported the discovery of a new form of carbon containing eight protons in the nucleus of its atoms. He claims that scientists are eager to explore the properties of this new form of carbon. What is wrong with the tabloid's claim? a. Nothing. The claim is believable. b. The claim must be false because an atom with eight protons would be oxygen, which is already known. c. The claim must be false because all forms of carbon are already known.
Without consulting your textbook or notes, state as many points as you can of Dalton’s atomic theory. Explain in your own words each point of the theory.
Predict and test the behavior of a particles fired at a Rutherford atom model. Predict the paths taken by a particles that are fired at atoms with a Rutherford atom model structure. Explain why you expect the particles to take these paths. If a particles of higher energy than those in (a) are fired at Rutherford atoms, predict how their paths will differ from the lower-energy a particle paths. Explain your reasoning. Predict how the paths taken by the particles will differ if they are fired at Rutherford atoms of elements other than gold. What factor do you expect to cause this difference in paths, and why? Now test your predictions from (a), (b), and (c). Open the Rutherford Scattering simulation (http://openstaxcollege.org/I/16PhetScatter) and select the Rutherford Atom tab. Due to the scale of the simulation, it is best to start with a small nucleus, so select 20 for both protons and neutrons, mm for energy, show traces, and then start firing a particles. Does this match your prediction from (a)? If not, explain why the actual path would be that shown in the simulation. Pause or reset, set energy to max, and start firing a particles. Does this match your prediction from (b)? If not, explain the effect of increased energy on the actual path as shown in the simulation. Pause or reset, select 40 for both protons and neutrons, mm for energy, show traces, and fire away. Does this match your prediction from (c)? If not, explain why the actual path would be that shown in the simulation. Repeat this with larger numbers of protons and neutrons. What generalization can you make regarding the type of atom and effect on the path of a particles? Be clear and specific.
The average atomic masses of some elements may vary, depending upon the sources of their ores. Naturally occurring boron consists of two isotopes with accurately known masses ( 10B, 10.0129 amu and 11B, 11.0931 amu). The actual atomic mass of boron can vary from 10.807 to 10.8 19, depending on whether the mineral source is from Turkey or the United States. Calculate the percent abundances leading to the two values of the average atomic masses of boron from these two countries.
Titanium and thallium have symbols that are easily confused with each other. Give the symbol, atomic number, atomic weight, and group and period number of each element. Are they metals, metalloids, or nonmetals?

SEE MORE QUESTIONS

Recommended textbooks for you

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

World of Chemistry, 3rd edition

Chemistry

ISBN:

9781133109655

Author:

Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:

Brooks / Cole / Cengage Learning

Chemistry In Focus

Chemistry

ISBN:

9781337399692

Author:

Tro, Nivaldo J.

Publisher:

Cengage Learning,

Introductory Chemistry: An Active Learning Approa…

Chemistry

ISBN:

9781305079250

Author:

Mark S. Cracolice, Ed Peters

Publisher:

Cengage Learning

World of Chemistry, 3rd edition

Chemistry

ISBN:

9781133109655

Author:

Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste

Publisher:

Brooks / Cole / Cengage Learning

Chemistry In Focus

Chemistry

ISBN:

9781337399692

Author:

Tro, Nivaldo J.

Publisher:

Cengage Learning,

Introductory Chemistry: A Foundation

Chemistry

ISBN:

9781337399425

Author:

Steven S. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry: An Atoms First Approach

Chemistry

ISBN:

9781305079243

Author:

Steven S. Zumdahl, Susan A. Zumdahl

Publisher:

Cengage Learning

Chemistry by OpenStax (2015-05-04)

Chemistry

ISBN:

9781938168390

Author:

Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:

OpenStax

SEE MORE TEXTBOOKS