Name two ways in which isotopes of an element differ.?
105589
the amount of neurons, and, they weigh differently... yea thats it.
531279
monatomic elements don't have molecular structures, molecules do.  your question is therefore confusing.\n\nelements have different isotopes (more or less neutrons)\n\nmolecules have different isomers (same number of elements, just connected differently)
93157
Isotopes are forms of an element whose nuclei have the same atomic number–-the number of protons in the nucleus--but different mass numbers because they contain different numbers of neutrons.\n\nThe word isotope, meaning at the same place, comes from the fact that all isotopes of an element are located at the same place on the periodic table.\n\nCollectively, the isotopes of the elements form the set of nuclides. A nuclide is a particular type of atomic nucleus, or more generally an agglomeration of protons and neutrons. Strictly speaking, it is more correct to say that an element such as fluorine consists of one stable nuclide rather than that it has one stable isotope.\n\nIn scientific nomenclature, isotopes (nuclides) are specified by the name of the particular element by a hyphen and the number of nucleons (protons and neutrons) in the atomic nucleus (e.g., helium-3, carbon-12, carbon-14, iron-57, uranium-238). In symbolic form, the number of nucleons is denoted as a superscripted prefix to the chemical symbol (e.g., 3He, 12C, 14C, 57Fe, 238U).\n\nSee link below for more info.
797180
Atomic mass depends on the element. It accounts for all isotopes and does a sort of weighted average, depending on how often the isotope occurs in nature.\nMass number depends on the isotope.\n\nFor example, atomic mass of hydrogen is 1.0079. The mass number of most hydrogen atoms is 1. Deuterium is an isotope with a neutron in its nucleus, so its mass number is 2. Tritium is an isotope with two neutrons, so its mass number is 3.
705478
An ion differs from the original element in terms of the number of electrons.\n\nThe mass of an electron is about 1/1836 of a proton or a neutron.\n\nTherefore there would be a tiny difference in atomic mass, however in most cases it's fairly negligable.
980733
neutron\n\nhowever, it is already an isotope, changing the neutrons would make it a different isotope\n\nchanging the protons would change the element\nchanging the electrons would change the charge
714932
An isotope of the element Plutonium.  An isotope means that an electron has been removed from or added to the element's valence shell configuration.  Plutonium-210 is radioactive and emits particles (alpha particles, beta particles) and gamma radiation.  Alpha particles can be dangerous to a human if they come in contact with soft tissues (ie. swallowed, absorbed into wounds.)
921116
I'm not directly giving you the answers, you have to know how to do this stuff, but I'll give you the process to get to each.\n\n9: Americium and Curium (wikipedia!)\n\n10: Potassium ion wants to be like the noble gas closest to it (the one right before it), so it loses 1e- to get there and be K+.  If that's not a choice, then look for another ion, positive or negative, that adds up to the electronic configuration of the aforementioned noble gas. (1s2 2s2 2p6 3s2 3p6), 18 total e-'s...\n\n11: Mg is in column 2, things in the same period tend to be chemically similar.  Find the other one in the choices that's in that column\n\n12: U235 and U238 are isotopes, same atomic number, different weight.  If you change the number of protons, you change the atomic number, so that wouldn't be U anymore.  Changing electrons can make ions, but not change weight.  So different number of neutrons for the same element makes an isotope.\n\n13: Same explanation as above, it'll also be Hydrogen's atomic number because it's an isotope.\n\n14: shell 2 contains the 2s and 2p subshells.  2s can hold 2 because it's an s orbital.  2p can hold 2 per p orbital, and a p subshell has 3 p orbitals, so 6.  Total would then be...\n\n15: If an atom loses electrons, it's LOSING -1 per electron lost, so it's becoming more positive.\n\n16: Which element in that list only has 1s shell? Which one has a  stable ion as just a proton or with a configuration like Helium (1s2)?\n\n17: Inert elements are on the far right of the periodic table.  They are inert because they have 8 valence (outer shell) electrons (or 2 in Helium's case) so they can't take anymore and are stable.  Look at your periodic table or count up electrons for each of those atomic numbers.  Only one of them will have 8 in the outer shell...
16762
The atomic number is the number of protons.
838540
Isotopes are atoms with the same amount of protons, but different numbers of neutrons.
435218
Iso- as a prefix means "the same". Thus isobar (same pressure), isosceles triangle (two sides the same length) and isotope two or more versions of the same element which all have the same number of protons (or it would be a different element!) but varying numbers of neutrons in the nucleus.\n\nAs protons are positively charged and neutrons have no charge (electrons have a negative charge) neutrons are needed as "packing materials" to help keep the positive charges fom repelling one another and making the nucleus unstable.\n\nWith elements of low atomic number, the number of neutrons will be the same or just greater than the number of protons. But with elements of high atomic number, more packing materials are needed, and the ratio of neutrons to protons begins to climb towards 1.5:1\n\nThere is only a narrow range of options for that ratio for isotpes that are stable. Those with too few or too many neutrons, iutside that range, are unstable and decay.\n\nCompare Carbon 12 and Carbon 14 with Uranium 235 and Uranium 238\n\nCarbon 12 has 6 protons and 6 neutrons and is stable\n\nCarbon 14 has 6 protons and 8 neutrons and is unstable, it decays\n\nU235 has 92 protons, 143 neutrons and is unstable.\n\nU238 has 92 protons, 146 neutrons and is unstable\n\nAs regards silver (Ag) oy has two stable isotopes Ag 107 (47p, 60n) and Ag 109 (47p, 62n) But very short-lived isotopes varying in atomic mass from the neutron-deficient Ag 93 (47p, 46 n) to Ag 123 (47p 76n) also exist.
361815
The similarity is the atomic number, as determined by the number of protons. Also the same number of electrons if not ionised.\n\nThe difference is the number of neutrons. Also differences in mass and binding energy per nucleon.\n\nA decay from 15N7 to 15O8 means the number of nucleons remains the same, but it has one more proton and one less neutron.\n\nNeutron decay is as follows:\n\n(n0) -> (p+) + (e-) + (-v)\n\nNeutron -> Proton + Electron + Antineutrino\n\nThis is negative beta decay since it produces a negative electron (which will almost certainly orbit the nucleus which now has an extra proton).\n\nThe atomic decay is:\n\n15N7 -> 15O8 + (e-) + (-v)\n\nSee the link for the appropriate notation
730866
They are different elements. \n\nNo element of higher atomic number than uranium (92) occurs naturally because they are all radioactive and decay over time.\n\nPlutonium is a transuranic element atomic number 94 that is a by product from nuclear reactors.\n\nOnly some isotopes of uranium are fissile (U 238 is stable). Plutonium is always fissile, and so is more useful and more potent in atomic weapons.
131141
Please edit your question to say what element you mean.  Same for the other one a few minutes earlier.
298477
neutrons\n\nIsotopes have to have the same numbers of protons\nor they'd be different elements.  Since the\nelectrons match up with the protons, the electron\ncount is consistent too.
795345
Same number of protons\n\ndifferent number of neutrons
693553
The atomic number of an element is equal to the number of protons the element has in the nucleus of one atom.\nThe number of protons in the nucleus determine what element it is.\n\nThe atomic mass of an element is equal to the sum of number of protons and the number of neutrons in the nucleus.  The electrons around the atom are neglected since their mass is negligible, as well as the fact that atoms can form ions by gaining and/or loosing electrons even though the element is the same.