Dalton proposed an Atomic Theory in which all atoms of an element are identical and have the same mass and properties. Isotopes, on the other hand, don't fit this prediction. Why? O Because isotopes can be radioactive. O Because isotopes have different natural abundances. Because isotopes have different chemical properties. Because isotopes have different mass numbers.

There are 3 stable isotopes of Argon: Argon-36, Argon-38, and Argon-40. What would atoms of these isotopes have in common? What would be different about their atoms? O All are gases; they each have different numbers of neutrons O All are the element Argon; they have different numbers of neutrons O All have the same atomic number while they have different mass numbers O All of the above

Gallium has two naturally occurring isotopes, 69Ga and 71Ga. The average atomic mass of galllium is 69.70 amu. Which of the following statements concerning the relative abundance of each isotope is correct? a) The abundance of 71Ga is greater than 69Ga. b) The abundance of 71Ga is less than 69Ga. c) The abundance of 71Ga is exactly equal to the abundance of 69Ga. d) Based on the atomic mass, only 69Ga occurs naturally. e) Not enough data is provided to determine the correct answer.

Fill in the blanks. The positions of atoms on the periodic table of the ____ are determined by how many _____  are present in their nuclei; this also is called their atomic _____.  An atom's nucleus is made up of protons, which have _____ charges and ___ that do not have a ____charge.  The total of protons and neutrons in an atom defines its atomic ____ .  Two atoms with the same number of protons but different numbers of neutrons in their nuclei are considered _____ . The nucleus is surrounded by electrons, which have  charges.  Electrons are not found randomly, but occur in discrete _____ that are grouped into "shells".  The chemical properties of an atom, that is, the kinds of chemical reactions it has with other atoms or molecules, are determined by properties of its outermost set of orbitals, which is called its _____ shell.  Two atoms will react with each other if the reaction leads to a more stable state; specifically so that their valence shells are ____  .  The most common…

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

Which of the following represents a pair of isotopes? Atomic Number | Mass Number 1. 6| 14 A II. 7| 14 1. 617 B II. 14 | 14 1. 6| 14 II. 14 | 28 I. 7 | 13 D II. 7 | 14 1. 8 10 II. 16 20

There are two naturally occurring isotopes of gallium. Gallium-69 has a mass of 68.9256 u. Gallium-71 has a mass of 70.9247 u. Determine the abundance of each isotope.

An unknown element has two naturally occurring isotopes. Isotope 1 has a mass of 121.0 amu and an abundance of 55.10%. Isotope 2 has a mass of 123.0 amu. What is the atomic mass of the element?

Consider the elements Co-60 and Ni-60. a) How many neutrons and protons does each element have? b) Are these elements isotopes, isotones, isobars or isomers? c) Are the chemical properties of these two elements similar? Why or why not?

NucleonsThe term nucleon refers to the particles found in the nucleus of an atom, namely protons and neutrons. A single hydrogen atom (one proton plus one electron) has a mass of 1.007825 amu. A single neutron has a mass of 1.008665 amu. Note that amu stands for "atomic mass unit" and is sometimes abbreviated with the symbol uu. 1 uu is equivalent to 1.665387×10-27 kgPart A Calculate the mass defect of the fluorine nucleus 19-9F. The mass of neutral  19-9F is equal to 18.998403 atomic mass units.   Part B Calculate the binding energy E of the fluorine nucleus 19 9F  (1eV=1.602×10-19J)   Part C Calculate the binding energy per nucleon of the fluorine nucleus 19-9F