Ch.7 - Periodic Properties of the Elements

Brown - Chemistry: The Central Science 15th Edition

Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook

Brown 15th Edition

Ch.7 - Periodic Properties of the Elements

Problem 27a

Chapter 7, Problem 27a

Identify each statement as true or false: (a) Cations are larger than their corresponding neutral atoms.

Verified step by step guidance

Step 1: Understand the concept of cations. Cations are positively charged ions that are formed when an atom loses one or more electrons.

Step 2: Consider the effect of losing electrons on the size of an atom. When an atom loses electrons, it has more protons than electrons. This causes the electrons to be pulled closer to the nucleus, making the atom smaller.

Step 3: Compare the size of a cation to its corresponding neutral atom. Since a cation is an atom that has lost electrons and thus become smaller, it is generally smaller than its corresponding neutral atom.

Step 4: Based on the above understanding, the statement 'Cations are larger than their corresponding neutral atoms' is generally false.

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Key Concepts

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

Atomic Size and Ionization

Atomic size refers to the distance from the nucleus to the outermost electron shell. When an atom loses one or more electrons to form a cation, the remaining electrons experience a stronger effective nuclear charge, pulling them closer to the nucleus and resulting in a smaller ionic radius compared to the neutral atom.

Cations vs. Neutral Atoms

Cations are positively charged ions formed when an atom loses electrons. This loss of electrons reduces electron-electron repulsion in the electron cloud, allowing the remaining electrons to be drawn closer to the nucleus, which decreases the size of the ion compared to its neutral counterpart.

Trends in Ionic Radii

Ionic radii trends indicate that cations are generally smaller than their neutral atoms due to the loss of electrons and increased nuclear attraction. This trend is essential for understanding the behavior of elements in the periodic table and their interactions in chemical reactions.

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Ranking Ionic Radii

Related Practice

Textbook Question

Which neutral atom is isoelectronic with each of the following ions? Ga³⁺, Zr⁴⁺, Mn⁷⁺, I⁻, Pb²⁺.

Identify each statement as true or false: (b) Li⁺ is smaller than Li.

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Textbook Question

Using only the periodic table, arrange each set of atoms in order from largest to smallest: (a) Ar, As, Kr (b) Cd, Rb, Te (c) F, O, N.

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Textbook Question

For each set of atoms and ions, pick the smallest one.

a. I, I+, I−

b. Be2+, Ca2+, Mg2+

c. Fe, Fe2+, Fe3+

Textbook Question

Using only the periodic table, arrange each set of atoms in order of increasing radius. b. In, Sn, As

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Textbook Question

Which of the following statements about the bonding atomic radii in Figure 7.7 is incorrect? (i) For a given period, the radii of the representative elements generally decrease from left to right across a period. (ii) The radii of the representative elements for the n = 3 period are all larger than those of the corresponding elements in the n = 2 period. (iii) For most of the representative elements, the change in radius from the n = 2 to the n = 3 period is greater than the change in radius from n = 3 to n = 4. (iv) The radii of the transition elements generally increase moving from left to right within a period. (v) The large radii of the Group 1 elements are due to their relatively small effective nuclear charges.

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