Ch.8 - Periodic Properties of the Elements

Problem 62

Previous problem

Next problem

Chapter 8, Problem 62

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

Verified step by step guidance

1. The size of an atom is determined by the number of energy levels it has, which is equivalent to the period number on the periodic table. The more energy levels an atom has, the larger it is.

2. For each pair, locate the elements on the periodic table and identify their period numbers. The element with the higher period number is the larger atom.

3. For pair a (Sn or Si), Sn is in period 5 and Si is in period 3. Therefore, Sn is the larger atom.

4. For pair b (Br or Ga), Br is in period 4 and Ga is in period 4. However, Br is a halogen and Ga is a metal. Halogens are generally larger than metals in the same period, so Br is the larger atom.

5. For pair c (Sn or Bi), Sn is in period 5 and Bi is in period 6. Therefore, Bi is the larger atom.

6. For pair d (Se or Sn), Se is in period 4 and Sn is in period 5. Therefore, Sn is the larger atom.

Verified Solution

Video duration:

This video solution was recommended by our tutors as helpful for the problem above.

Was this helpful?

Key Concepts

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

Atomic Size

Atomic size refers to the distance from the nucleus to the outermost electron shell of an atom. Generally, atomic size increases down a group in the periodic table due to the addition of electron shells, while it decreases across a period from left to right due to increased nuclear charge, which pulls electrons closer to the nucleus.

Periodic Trends

Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change as you move across a period or down a group. Key trends include atomic radius, ionization energy, and electronegativity, which help predict the behavior of elements in chemical reactions and their relative sizes.

Comparison of Elements

When comparing elements, it is essential to consider their positions in the periodic table. Elements in the same group typically have similar properties, while those in the same period show a gradual change in properties. Understanding these relationships allows for accurate comparisons of atomic size and other characteristics between different elements.

Recommended video:

Guided course

02:35

Elemental Forms of Elements

Previous problem

Next problem

Related Practice

Textbook Question

If core electrons completely shielded valence electrons from nuclear charge (i.e., if each core electron reduced nuclear charge by 1 unit) and if valence electrons did not shield one another from nuclear charge at all, what would be the effective nuclear charge experienced by the valence electrons of each atom? c. O d. C

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.)

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

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

Open Question

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-

712

views