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Chapter 2: Problem 94

In your own words, define or explain these terms or symbols: (a) \(\underset{\mathbf{Z}}{\mathbf{A}} \mathbf{E} ;\) (b) \(\boldsymbol{\beta}\) particle; \(\mathbf{( c )}\) isotope; \(\mathbf{( d )}^{16} \mathbf{O}\) (e) molar mass.

Short Answer

Expert verified
(a) \(\underset{\mathbf{Z}}{\mathbf{A}} \mathbf{E}\) is a symbol used to denote isotopes of an element E, where A is the mass number and Z is the atomic number. (b) A \(\boldsymbol{\beta}\) particle is a charged particle emitted in beta decay. (c) An isotope is a form of a chemical element with the same number of protons but a different number of neutrons. (d) \(^{16} \mathbf{O}\) is an isotope of oxygen with 8 protons and 8 neutrons. (e) Molar mass is the mass in grams of one mole of a substance.

Step by step solution

01

Understand \(\underset{\mathbf{Z}}{\mathbf{A}} \mathbf{E}\)

This notation is used in nuclear physics and chemistry to denote different isotopes of an element. E stands for the element under consideration. The letter A at the upper position denotes the mass number of the isotope, which is the total number of protons and neutrons in the nucleus. At the lower position, the letter Z represents the atomic number of the isotope, which is the number of protons in the nucleus.
02

Define \(\boldsymbol{\beta}\) particle

\(\boldsymbol{\beta}\) particle refers to a charged particle that is emitted in a type of radioactive decay called beta decay. There are two types of beta particles: \(\beta^-\) particles, which are electrons, and \(\beta^+\) particles, which are positrons.
03

Define isotope

An isotope is a form of a chemical element whose atomic nucleus contains a specific number of neutron(s) in addition to the number of protons that is unique to the element. Different isotopes of the same element have the same atomic number (number of protons in the nucleus) but different mass numbers due to the different numbers of neutrons.
04

Identify \(^{16} \mathbf{O}\)

The notation \(^{16} \mathbf{O}\) denotes a particular isotope of oxygen. The number 16 represents the mass number - the total amount of protons and neutrons in the nucleus of the atom. Therefore, an atom of \(^{16} \mathbf{O}\) has 8 protons (as the atomic number of oxygen is 8) and 8 neutrons.
05

Define molar mass

Molar mass is the mass in grams of one mole (6.022 x 10^23 particles) of a substance. It has the units gram per mole (g/mol). The molar mass of an element is numerically equivalent to the element's relative atomic mass.

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Most popular questions from this chapter

Without doing detailed calculations, determine which of the following samples occupies the largest volume: (a) 25.5 mol of sodium metal \(\left(d=0.971 \mathrm{g} / \mathrm{cm}^{3}\right)\) (b) 0.725 L of liquid bromine \((d=3.12 \mathrm{g} / \mathrm{mL})\) (c) \(1.25 \times 10^{25}\) atoms of chromium metal \(\left(d=9.4 \mathrm{g} / \mathrm{cm}^{3}\right)\) (d) \(2.15 \mathrm{kg}\) of plumber's solder \(\left(d=9.4 \mathrm{g} / \mathrm{cm}^{3}\right), \mathrm{a}\) lead-tin alloy with a 2: 1 atom ratio of lead to tin

In an experiment, \(125 \mathrm{cm}^{3}\) of zinc and \(125 \mathrm{cm}^{3}\) of iodine are mixed together and the iodine is completely converted to \(164 \mathrm{cm}^{3}\) of zinc iodide. What volume of zinc remains unreacted? The densities of zinc, iodine, and zinc iodide are \(7.13 \mathrm{g} / \mathrm{cm}^{3}, 4.93 \mathrm{g} / \mathrm{cm}^{3}\) and \(4.74 \mathrm{g} / \mathrm{cm}^{3}\), respectively.

Explain the important distinctions between each pair of terms: (a) cathode rays and X-rays (b) protons and neutrons (c) nuclear charge and ionic charge (d) periods and groups of the periodic table (e) metal and nonmetal (f) the Avogadro constant and the mole

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