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Ch.8 - Periodic Properties of the Elements

Tro 4th Edition

Ch.8 - Periodic Properties of the Elements

Problem 63

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Chapter 8, Problem 63

Arrange these elements in order of increasing atomic radius: F, S, Si, Ge, Ca, Rb.

Verified step by step guidance

1

<Identify the periodic trend for atomic radius: Atomic radius increases as you move down a group and decreases as you move across a period from left to right.>

<Locate each element on the periodic table: F (Fluorine), S (Sulfur), Si (Silicon), Ge (Germanium), Ca (Calcium), Rb (Rubidium).>

<Compare elements within the same group: Ge and Si are in Group 14, with Ge below Si, so Ge has a larger atomic radius than Si.>

<Compare elements within the same period: F, S, and Si are in Period 2 and 3, with F having the smallest atomic radius and Si the largest among them.>

<Arrange the elements based on their position in the periodic table, considering both group and period trends: F, S, Si, Ge, Ca, Rb.>

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Related Practice

Textbook Question

In Section 3.6, we estimated the effective nuclear charge on beryllium's valence electrons to be slightly greater than 2+. What would a similar treatment predict for the effective nuclear charge on boron's valence electrons? Would you expect the effective nuclear charge to be different for boron's 2s electrons compared to its 2p electron? In what way? (Hint: Consider the shape of the 2p orbital compared to that of the 2s orbital.)

Textbook Question

Choose the larger atom in each pair. a. Al or In b. Si or N c. P or Pb d. Si or Cl

Textbook Question

Choose the larger atom in each pair. a. Sn or Si b. Br or Ga c. Sn or Bi d. Se or Sn

Arrange these elements in order of decreasing atomic radius: Cs, Pb, Sb, Se, S.

Textbook Question

Write the electron configuration for each ion. a. O^2-

Textbook Question

Write the electron configuration for each ion. b. Br^-