Skip to main content
Ch.8 - Periodic Properties of the Elements
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Non è quello che usi tu?Cambia libro di testo
Tutti i libri di testoTro 4th EditionCh.8 - Periodic Properties of the ElementsProblema 79a
Capitolo 8, Problema 79a

Choose the element with the more negative (more exothermic) electron affinity from each pair. a. Na or Rb

Guida verificata passo dopo passo
1
Understand that electron affinity refers to the energy change when an electron is added to a neutral atom in the gaseous state. A more negative electron affinity indicates a greater tendency to gain an electron.
Recall that electron affinity generally becomes more negative across a period from left to right and less negative down a group in the periodic table.
Identify the position of Na (Sodium) and Rb (Rubidium) in the periodic table. Na is in the third period, while Rb is in the fifth period.
Consider the trend: as you move down a group, the electron affinity becomes less negative due to increased atomic size and electron shielding, which makes it harder for the nucleus to attract additional electrons.
Based on the periodic trend, predict that Na, being higher up in the group than Rb, will have a more negative (more exothermic) electron affinity compared to Rb.

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:
1m

Concetti chiave

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

Electron Affinity

Electron affinity is the energy change that occurs when an electron is added to a neutral atom in the gas phase. A more negative electron affinity indicates that the process is more exothermic, meaning energy is released when the atom gains an electron. This property is crucial for understanding how easily an atom can accept an electron and form an anion.
Video consigliato:
Percorso guidato
01:34
Electron Affinity

Trends in the Periodic Table

Periodic trends refer to the predictable patterns observed in the properties of elements as you move across or down the periodic table. For electron affinity, it generally increases (becomes more negative) across a period from left to right and decreases down a group. Understanding these trends helps in predicting the electron affinity of elements based on their position in the periodic table.
Video consigliato:
Percorso guidato
00:38
Periodic Trends

Group 1 Elements

Group 1 elements, also known as alkali metals, include lithium, sodium, potassium, rubidium, cesium, and francium. These elements have low ionization energies and tend to lose one electron easily, making their electron affinities less negative compared to other groups. When comparing sodium (Na) and rubidium (Rb), it is essential to consider their positions in the group and how their atomic size affects their ability to attract additional electrons.
Video consigliato:
Percorso guidato
00:50
Main Group Elements: Density Example
Pratica correlata
Domanda del libro di testo

Choose the element with the more negative (more exothermic) electron affinity in each pair. a. Mg or S b. K or Cs c. Si or P d. Ga or Br

699
views
1
rank
Domanda del libro di testo

Consider this set of ionization energies. IE1 = 578 kJ/mol IE2 = 1820 kJ/mol IE3 = 2750 kJ/mol IE4 = 11,600 kJ/mol To which third-period element do these ionization values belong?

5849
views
1
comments
Domanda del libro di testo

Choose the element with the more negative (more exothermic) electron affinity from each pair. c. C or N d. Li or F

324
views
Domanda del libro di testo

Choose the element with the more negative (more exothermic) electron affinity from each pair. b. B or S

431
views
Domanda del libro di testo

For each element, predict where the 'jump' occurs for successive ionization energies. (For example, does the jump occur between the first and second ionization energies, the second and third, or the third and fourth?) a. Be b. N c. O d. Li

3121
views