A student began to read the chart below and did not understand how these elements can have several different forms, but still be the same element. She knows where to find Hydrogen on the periodic table of elements, but is confused about why these are considered isotopes. Using your periodic table and referring to the data above, what is the best response to her confusion about Hydrogen and the atoms shown beneath it? image A. Hydrogen (H1), Deuterium (H2), and Tritium (H3) are all isotopes of hydrogen. They each have an atomic number of 1, because they have 1 proton. Hydrogen has 0 neutrons, Deuterium has 1 neutron, and Tritium has 2 neutrons. B. Hydrogen (H1), Deuterium (H2), and Tritium (H3) are all different elements. They are given different names, because they have different atomic numbers and different atomic masses.

C. Hydrogen (H1), Deuterium (H2), and Tritium (H3) are all different elements. They are given different names, because they have different atomic masses but the same atomic numbers.

D. Hydrogen (H1), Deuterium (H2), and Tritium (H3) are all isotopes of hydrogen. They each have an atomic number of 1, because they have 1 proton. Hydrogen has 1 neutron, Deuterium has 2 neutrons, and Tritium has 3 neutrons