Give the protons neutrons and electrons for the following atomic symbol96 Zr+2Protons= 40ANeutrons = 56Electrons = 42BProtons= 40Neutrons = 56Electrons = 38Protons = 40CNeutrons = 90DElectrons = 42Protons= 38Neutrons = 38Electrons = 40EProtons = 38Neutrons = 38Electrons = 36

Option a: This option is incorrect because Zr+2 having 38 electrons, not 42. Option b: This option…

Answered: Give the protons neutrons and electrons…

Chemistry In Focus

7th Edition

ISBN:9781337399692

Author:Tro, Nivaldo J.

Publisher:Tro, Nivaldo J.

Chapter3: Atoms And Elements

Section: Chapter Questions

Problem 2SC

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Mass spectrometric analysis showed that there are four isotopes of an unknown element having the following masses and abundances: Three elements in the periodic table that have atomic weights near these values are lanthanum (La), atomic number 57, atomic weight 138.9055; cerium (Ce), atomic number 58, atomic weight 140.115; and praseodymium (Pr), atomic number 59, atomic weight 140.9076. Using the data above, calculate the atomic weight, and identify the element if possible.
Give the atomic number (Z) and the mass number (A) for each of the following: a. a carbon atom with 8 neutrons b. an aluminum atom with 14 neutrons c. an argon atom with 20 neutrons d. a copper atom with 36 neutrons
Though the common isotope of aluminum has a mass number of 27, isotopes of aluminum have been isolated (or prepared in nuclear reactors) with mass numbers of 24, 25, 26, 28, 29, and 30. How many neutrons are present in each of these isotopes? Why are they all considered aluminum atoms, even though they differ greatly in mass? Write the atomic symbol for each isotope.
The element gallium, used in gallium arsenide semiconductors, has an atomic weight of 69.72 amu. There are only two isotopes of gallium, Ga with a mass of 6.9257 amu and Ga with a mass of 70.9249 amu. What are the isotopic abundances of gallium? Gallium melts just above room temperature
2.87 What is the heaviest element to have an atomic weight that is roughly twice its atomic number? What does this suggest must he true about the nuclei of atoms with higher atomic numbers?
An element has the following natural abundances and isotopic masses: 90.92% abundance with 19.99 amu, 0.26% abundance with 20.99 amu, and 8.82% abundance with 21.99 amu. Calculate the average atomic mass of this element.
Atoms are electrically neutral. This means that an atom will contain a.more protons than neutrons. b.more electrons than protons. c.an equal number of protons and electrons. d.None of the above.
2-27 If each atom in Problem 2-26 acquired two more neutrons, what element would each then be?
2-102 An element consists of 90.51% of an isotope with a mass of 19.992 amu, 0.27% of an isotope with a mass of 20.994 amu, and 9.22% of an isotope with a mass of 21.990 amu. Calculate the average atomic mass and identify the element.
1. The mass of an atom of manganese is 54.9380 u. How many neutrons are contained in one atom of this element? 25 29 30 55

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Give the protons neutrons and electrons for the following atomic symbol 96 Zr+2 Protons= 40 A Neutrons = 56 Electrons = 42 B Protons= 40 Neutrons = 56 Electrons = 38 Protons = 40 C Neutrons = 90 D Electrons = 42 Protons= 38 Neutrons = 38 Electrons = 40 E Protons = 38 Neutrons = 38 Electrons = 36