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? b. Ca
Ch.8 - Periodic Properties of the Elements
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
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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.
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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.
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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.
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Related Practice
Textbook Question
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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.)
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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
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Open Question
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. O2-
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