Skip to main content
Ch.9 - Periodic Properties of the Elements
Tro - Chemistry: A Molecular Approach 5th Edition
Tro5th EditionChemistry: A Molecular ApproachISBN: 9780134874371Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 5th EditionCh.9 - Periodic Properties of the ElementsProblema 59
Capitolo 9, Problema 59

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

Guida verificata passo dopo passo
1
Identify the periodic trend: Atomic size increases as you move down a group in the periodic table and decreases as you move across a period from left to right.
Compare Al and In: Both are in Group 13, but In is below Al, so In is larger.
Compare Si and N: Both are in Period 2, but Si is to the left of N, so Si is larger.
Compare P and Pb: P is in Group 15 and Period 3, while Pb is in Group 14 and Period 6. Pb is much lower in the periodic table, so Pb is larger.
Compare Si and Cl: Both are in Period 3, but Si is to the left of Cl, so Si is larger.

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.
Durata del video:
2m

Concetti chiave

Ecco i concetti essenziali che devi comprendere per rispondere correttamente alla domanda.

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.
Video consigliato:
Percorso guidato
02:10
Atom Structure

Periodic Trends

Periodic trends are patterns observed in the periodic table that describe how certain properties of elements change across periods and down groups. Key trends include atomic radius, ionization energy, and electronegativity, which help predict the behavior of elements in chemical reactions and their relative sizes.
Video consigliato:
Percorso guidato
00:38
Periodic Trends

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 different groups may vary significantly. Understanding these relationships allows for accurate predictions about which atom is larger based on their respective group and period placements.
Video consigliato:
Percorso guidato
02:35
Elemental Forms of Elements
Pratica correlata
Domanda del libro di testo

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

715
views
Domanda del libro di testo

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.)

1059
views
1
rank
Domanda del libro di testo

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

528
views
Domanda del libro di testo

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

2895
views
1
rank