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What part of the atom contains practically all its mass?

Short Answer

Expert verified
The nucleus, which contains the protons and neutrons, contains practically all the mass of an atom.

Step by step solution

01

Identify Atomic Structure Components

The atom is composed of protons, neutrons, and electrons. Protons and neutrons form the nucleus, while electrons orbit around the nucleus.
02

Analyze Mass Contribution

Protons and neutrons have much greater mass than electrons. Therefore, their combined mass contributes mostly to the overall mass of the atom.
03

Conclude the Source of Mass

Since protons and neutrons reside in the nucleus and make up nearly all the mass of the atom, the nucleus is the part that contains practically all the mass.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Protons and Neutrons
Understanding the weight of an atom requires us to delve into its fundamental constituents, primarily protons and neutrons. These particles are commonly referred to as nucleons because they reside within the nucleus of the atom. Protons are positively charged particles, while neutrons have no charge at all, hence their name. Interestingly, despite the difference in electrical charge, protons and neutrons are remarkably similar in terms of mass. They are approximately 1,836 times heavier than electrons, the atom's third constituent. Because of this significant difference in mass, electrons contribute negligibly to the atom’s overall weight. It’s the accumulation of protons and neutrons that gives an atom the majority of its mass. Moreover, these nucleons are bound together in the nucleus by the strong nuclear force, one of the four fundamental forces in physics, which is also comprehensible for holding the nucleus together.
Atomic Structure
The atomic structure is a captivating subject that visualizes an atom as a tiny solar system where electrons orbit the nucleus, resembling how planets revolve around the sun. This nucleus, located at the heart of the atom, is a dense core packed with protons and neutrons. Surrounding this nucleus are layers or shells of orbiting electrons, which are in constant motion. The organization of electrons across these shells is governed by quantum mechanics and determines the chemical properties of the element. To visualize this, imagine bustling cities (electrons) orbiting around a highly condensed and massive core (nucleus). Knowing this structure is crucial because it dictates how atoms interact with one another to form molecules, which are the building blocks of all matter.
Mass of Atom
When we refer to the mass of an atom, we are essentially talking about the aggregate mass of its protons, neutrons, and electrons. But, as we've established, electrons are almost like the weightless specks of dust when compared to the hefty textbooks, which represent protons and neutrons. The standard unit used to measure atomic mass is the atomic mass unit (amu), with one amu being roughly equivalent to the mass of a single proton or neutron. To precisely measure the mass of an atom, scientists use devices known as mass spectrometers, which can determine the mass of an atom with astonishing accuracy. This allows researchers to understand the nuances of chemical reactions and the formations of different molecules.
Nucleus of Atom
The nucleus is the command center of an atom. It is incredibly small compared to the entire atom, yet it holds almost all of its mass. This core is where protons and neutrons live and where most of the action takes place. It is akin to a dense, microscopic marble in the center of an expansive stadium. Just as the density of the marble far exceeds that of air in the stadium, the density of the nucleus far exceeds that of the space where the electrons reside. This stark contrast is because the nucleus is extremely compact and dense due to the strong nuclear force that holds the nucleons tightly together. The makeup of the nucleus, in terms of the number of protons and neutrons, is also what defines the identity of an element on the periodic table and determines the behavior of the atom in chemical reactions.

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Most popular questions from this chapter

Elemental iridium is composed of two stable isotopes, iridium-191 and iridium-193. (a) How many protons and neutrons are found in these two isotopes of iridium? (b) Write the correct isotopic notation for each of these isotopes of iridium. (c) Calculate the mass percent of protons in the nucleus of each of these isotopes.

Which subatomic particles are not in the nucleus? What do an ion of Ca and an atom of Ar have in common?

Congratulations! You discover a new element you name wyzzlebium \((W z)\). The average atomic mass of \(W z\) was found to be \(303.001 \mathrm{u}\), and its atomic number is 120 . (a) If the masses of the two isotopes of wyzzlebium are \(300.9326 \mathrm{u}\) and \(303.9303 \mathrm{u}\), what is the relative abundance of each isotope? (b) What are the isotopic notations of the two isotopes? (e.g., \({ }_{\text {Z W W ) }}\) (c) How many neutrons are in one atom of the more abundant isotope?

Place each of the following elements in order of increasing number of neutrons (least to most); \({ }^{156} \mathrm{Dy},{ }^{160} \mathrm{Gd},{ }^{162} \mathrm{Er},{ }^{165} \mathrm{Ho}\). Does this order differ from the elements' positions on the periodic table?

An unidentified atom is found to have an atomic mass \(7.18\) times that of the carbon-12 isotope. (a) What is the mass of the unidentified atom? (b) What are the possible identities of this atom? (c) Why are you unable to positively identify the element based on the atomic mass and the periodic table? (d) If the element formed a compound \(\mathrm{M}_{2} \mathrm{O}\), where \(\mathrm{M}\) is the unidentified atom, identify \(\mathrm{M}\) by writing the isotopic notation for the atom.

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