Which of the following correctly describes subatomic particles? Mass: e− < p+ = n Magnitude of charge: n < e− = p+ Location: outside nucleus e−, p+, inside nucleus n 2 only 1 and 2  1 only 3 only

Write the following isotopes in hyphenated form (e.g., carbon-14). (a) N1124a (b) A1329l (c) K3673r (d) I77194r

2.92 A candy manufacturer makes chocolate-covered cherries. Although all of the products look roughly the same, 3% of them are missing the cherry. The mass of the candy with a cherry is 18.5 g; those missing the cherry weigh only 6.4 g. (a) How would you compute the average mass of a box of 100 of these chocolate covered cherries from this manufacturer? (b) I low is this question analogous to the determination of atomic weights?

Bromine has two occuring isotopes: 79Br with atomic mass 78.9183 and 81Br with atomic mass 80.9163. Without using a calculator, what would you estimate the % abundance of Br-79 to be?

How many Ag atoms are present in a piece of pure silver jewelry weighing 21.3 g?

In what way are isotopes of a given element always different? In what way(s) are they always the same?

The mass-to-charge ratio for the positive ion F+ is 1.97 107 kg/C. Using the value of 1.602 1019 C for the charge on the ion, calculate the mass of the fluorine atom. (The mass of the electron is negligible compared with that of the ion, so the ion mass is essentially the atomic weight.)

The following table presents the abundances and masses of the isotopes of zinc. What is the atomic weight of zinc?

An atom has a very small nucleus surrounded by an electron cloud. Figure 2.1 represents the nucleus with a diameter of about 2 mm and describes the electron cloud as extending over 200 m. If the diameter of an atom is 1 10-8 cm, what is the approximate diameter of its nucleus?

2-103 The element silver has two naturally occurring isotopes: 109Ag and 107Ag with a mass of 106.905 amu. Silver consists of 51.82% 07Ag and has an average atomic mass of 107.868 amu. Calculate the mass of 109Ag