Ch.4 Atoms and Elements

Timberlake - Chemistry: An Introduction to General, Organic, and Biological Chemistry 13th Edition

Timberlake13th EditionChemistry: An Introduction to General, Organic, and Biological ChemistryISBN: 9780134421353Non è quello che usi tu?Cambia libro di testo

Timberlake 13th Edition

Ch.4 Atoms and Elements

Problema 37b

Capitolo 4, Problema 37b

Argon has three naturally occurring isotopes, with mass numbers 36, 38, and 40.
b. How are these isotopes alike?

Guida verificata passo dopo passo

Understand the concept of isotopes: Isotopes are atoms of the same element that have the same number of protons but different numbers of neutrons. This means they share the same atomic number but differ in their mass numbers.

Identify the element in question: Argon is the element being discussed. Its atomic number is 18, which means all isotopes of argon have 18 protons.

Recognize the similarity among isotopes: Since isotopes of argon all have the same number of protons (18), they also have the same chemical properties because chemical behavior is determined by the electron configuration, which depends on the number of protons.

Note the shared characteristics: All isotopes of argon are chemically identical, belong to the same element, and occupy the same position in the periodic table.

Conclude the similarity: The isotopes of argon are alike because they have the same number of protons (18), the same atomic number, and the same electron configuration, which results in identical chemical properties.

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Isotopes

Isotopes are variants of a chemical element that have the same number of protons but different numbers of neutrons. This results in different mass numbers for each isotope. For example, argon has isotopes with mass numbers 36, 38, and 40, all of which are forms of argon but differ in their neutron count.

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04:36

Isotopes

Chemical Properties

Isotopes of an element exhibit nearly identical chemical properties because they have the same electron configuration. This means that isotopes of argon will react similarly in chemical reactions, despite their differences in mass. Their behavior in chemical processes is largely determined by their electron arrangement rather than their mass.

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02:11

Chemical Properties Example 1

Stability and Radioactivity

Isotopes can be stable or unstable (radioactive). Stable isotopes do not undergo radioactive decay, while unstable isotopes do, leading to the emission of radiation. In the case of argon, the isotopes 36 and 38 are stable, while 40Ar is also stable, which means they do not change into other elements over time.

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02:52

Measuring Radioactivity Concept 1

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Argon has three naturally occurring isotopes, with mass numbers 36, 38, and 40.

c. How are they different?

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How many protons and electrons are there in a neutral atom of each of the following elements?

a. argon

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Indium consists of two isotopes, ¹¹³₄₉In and ¹¹⁵₄₉In. If the atomic mass for indium on the periodic table is 114.8, are there more atoms of ¹¹³₄₉In or ¹¹⁵₄₉In in a sample of indium?

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Argon has three naturally occurring isotopes, with mass numbers 36, 38, and 40.

a. Write the atomic symbol for each of these atoms.

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Argon has three naturally occurring isotopes, with mass numbers 36, 38, and 40.

d. Why is the atomic mass of argon listed on the periodic table not a whole number?

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