Final answer:
The Bohr-Rutherford diagram and Lewis structure diagram for an atom of a Transition Metal can be drawn by representing the nucleus, electron shells, and valence electrons. Atoms of the same element have the same atomic number, but can have different mass numbers due to isotopes. The atomic number and electron configuration determine an atom's position on the periodic table.
Step-by-step explanation:
a) Bohr-Rutherford Diagram:
A Bohr-Rutherford diagram for an atom of a Transition Metal, such as Iron (Fe), would consist of a nucleus with protons and neutrons represented, and electron shells surrounding the nucleus. The first shell would have 2 electrons, the second shell would have 8 electrons, and the third shell would have the remaining electrons.
b) Lewis Structure Diagram:
A Lewis structure diagram for Iron (Fe) would have the atomic symbol for Iron in the center, with dots around it representing the valence electrons. In the case of Iron, there would be 2 dots on the upper side, 2 dots on the lower side, and 4 dots on both the left and right sides.
All atoms of the same element have the same atomic number, which is unique to each element. However, atoms of the same element can have different mass numbers due to the presence of isotopes. Isotopes are atoms of the same element that have different numbers of neutrons.
The two features of an atom that determine its position on the periodic table are its atomic number (which represents the number of protons) and its electron configuration. For example:
- a) Metal: Iron (Fe)
- b) Non-Metal: Oxygen (O)
- c) Transition Metal: Copper (Cu)
- d) Noble Gas: Neon (Ne)
- e) Halogen: Chlorine (Cl)
- f) Alkali Metal: Sodium (Na)