Final answer:
The mass-to-charge ratio for fluorine cannot be directly determined from its atomic number or mass. Measurements in a magnetic field or mass spectrometry are typically required to determine this physical property. The values provided in the question options (a-d) do not represent the mass-to-charge ratio of fluorine.
Step-by-step explanation:
The mass-to-charge ratio for an atom or ion is not directly given by the atomic or mass numbers. In the case of fluorine, with an atomic symbol F and atomic number 9, its most common isotope has a mass number of 19. The standard atomic weight of fluorine is approximately 18.998 amu. To find the mass-to-charge ratio, it typically refers to ions and their movement in a magnetic field or some form of mass spectrometry, and it is thus a physical measurement, not just calculated from atomic and mass numbers.
Regarding question 3, since fluorine has an atomic number of 9 and a mass number of 19, the number of neutrons is 19 (mass number) minus 9 (atomic number), which equals 10 neutrons.
For question 12 about the binding energy of fluorine-18, the mass defect given is 2.44×10-28 kg. The binding energy can be calculated using Einstein's equation E=mc2, where m is the mass defect and c is the speed of light.
In response to question 17, the binding energy per atom or per nucleon would need a detailed calculation that takes into account the atomic mass and the mass of the individual protons and neutrons, as well as the number of nucleons.
Finally, the correct answer to the mass-to-charge ratio question for fluorine would not be one of the values given (a-d) since that information is not directly obtained solely from atomic or mass numbers. Instead, it would be determined through experimental measurements depending on the specific ionization state of the fluorine in question.