6. is model 1 accurate in its representation of magnesium at the atomic level? explain.\n8. if you could…
6. is model 1 accurate in its representation of magnesium at the atomic level? explain.\n8. if you could pick up a single atom of magnesium and put it on a balance, the mass of that atom would most likely be ____ amu. explain your reasoning.\n9. refer to a periodic table and find the box for magnesium.\na. write down the decimal number shown in that box.\nb. does the decimal number shown on the periodic table for magnesium match any of the atomic masses listed in model 2?\n10. the periodic table does not show the atomic mass of every isotope for an element.\na. explain why this would be an impractical goal for the periodic table.\nb. is it important to the average scientist to have information about a particular isotope of an element? explain.
Answer
6.
Brief Explanations:
To determine if Model 1 is accurate in representing magnesium at the atomic level, we need to know details about the model such as the number of protons, neutrons, and electrons it shows, electron - shell distribution etc. Without information about Model 1, we can't say. But in general, an accurate atomic - level model of magnesium should have 12 protons (since atomic number of Mg is 12), a number of neutrons consistent with its isotopes (common isotopes have 12, 13, or 14 neutrons), and 12 electrons arranged in 3 electron shells (2 in the first, 8 in the second, and 2 in the third).
Answer:
Insufficient information to determine.
8.
Brief Explanations:
Magnesium has several isotopes. The most common isotopes of magnesium are Mg - 24, Mg - 25, and Mg - 26. The atomic mass unit (amu) of an atom is approximately equal to the sum of protons and neutrons in the nucleus. Mg - 24 has 12 protons and 12 neutrons, so its mass is 24 amu; Mg - 25 has 12 protons and 13 neutrons (mass = 25 amu); Mg - 26 has 12 protons and 14 neutrons (mass = 26 amu). Since Mg - 24 is the most abundant isotope (about 78.99% abundance), if we pick up a single atom, it is most likely to be Mg - 24 with a mass of 24 amu.
Answer:
24 amu
9.
a.
Brief Explanations:
Looking at a periodic table, the decimal number shown for magnesium is its average atomic mass which takes into account the relative abundances of its isotopes. The average atomic mass of magnesium is approximately 24.305.
Answer:
24.305
b.
Brief Explanations:
If Model 2 lists the atomic masses of individual isotopes (which are whole - number values for the most part, e.g., 24, 25, 26 for Mg isotopes), the average atomic mass (24.305) shown on the periodic table will not match the atomic masses of individual isotopes exactly because it is a weighted average.
Answer:
No
10.
a.
Brief Explanations:
There are many isotopes for most elements. Listing the atomic mass of every isotope on the periodic table would make the table extremely cluttered and difficult to read. Also, many isotopes are unstable and have very short half - lives, and their atomic masses may not be as relevant for general chemical and physical applications.
Answer:
Would make the table cluttered and many isotopes are unstable/less relevant.
b.
Brief Explanations:
For some applications, like in nuclear chemistry, radiopharmaceuticals, and certain types of research, information about specific isotopes is crucial. For example, Mg - 26 can be used in nuclear magnetic resonance studies. But for general chemistry reactions and most day - to - day scientific work, the average atomic mass is sufficient. So it depends on the area of research. For an average chemist doing general synthesis or analysis, it may not be as important, but for a nuclear scientist or a researcher in isotope - specific fields, it is important.
Answer:
It depends on the area of research. For some (e.g., nuclear science), yes; for general chemistry, not always.