Ch.2 - Atoms, Molecules, and Ions

Problem 15

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Chapter 2, Problem 15

Which of the subatomic particles in an atom does not have a charge (and was therefore the last to be discovered)?

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Identify the three main subatomic particles in an atom: protons, neutrons, and electrons.

Recall that protons have a positive charge, electrons have a negative charge, and neutrons have no charge.

Understand that the discovery of subatomic particles was influenced by their charge and mass.

Recognize that because neutrons have no charge, they do not interact with electric or magnetic fields, making them harder to detect.

Conclude that neutrons were the last of the three main subatomic particles to be discovered due to their lack of charge.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Subatomic Particles

Subatomic particles are the fundamental constituents of atoms, primarily including protons, neutrons, and electrons. Protons carry a positive charge, electrons carry a negative charge, and neutrons are neutral, meaning they have no charge. Understanding these particles is essential for grasping atomic structure and behavior.

Neutrons

Neutrons are neutral subatomic particles found in the nucleus of an atom alongside protons. They play a crucial role in stabilizing the nucleus by offsetting the repulsive forces between positively charged protons. Neutrons were the last of the three main subatomic particles to be discovered, highlighting their significance in atomic theory.

Atomic Structure

Atomic structure refers to the arrangement of subatomic particles within an atom, which includes the nucleus (composed of protons and neutrons) and the electron cloud surrounding it. This structure determines the chemical properties of elements and their interactions. A clear understanding of atomic structure is vital for studying chemical reactions and bonding.

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Atom Structure

Related Practice

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: Compound Mass of Iodine (g) Mass of Fluorine (g) 1 4.75 3.56 2 7.64 3.43 3 9.41 9.86 (a) Calculate the mass of fluorine per gram of iodine in Compound 3.

In a series of experiments, a chemist prepared three different compounds that contain only iodine and fluorine and determined the mass of each element in each compound: Compound Mass of Iodine (g) Mass of Fluorine (g) 1 4.75 3.56 2 7.64 3.43 3 9.41 9.86 (b) How do the numbers in part (a) support the atomic theory?

An unknown particle is caused to move between two electrically charged plates, as illustrated in Figure 2.7. You hypothesize that the particle is a proton. (a) If your hypothesis is correct, would the particle be deflected in the same or opposite direction as the b rays?

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Textbook Question

An unknown particle is caused to move between two electrically charged plates, as illustrated in Figure 2.7. You hypothesize that the particle is a proton. (b) Would it be deflected by a smaller or larger amount than the b rays?

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Textbook Question

Which set of statements is true about Rutherford’s gold foil experiment?

i. This is the main experiment that showed that atoms have a dense nucleus.

ii. The data from the experiment showed that alpha particles scattered equally at all angles from the gold foil.

iii. Electrons were emitted from the gold atoms in straight lines.

a. i only

b. ii only

c. iii only

d. i and ii

e. i and iii