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 76
Capitolo 8, Problema 76

Arrange these elements in order of decreasing first ionization energy: Cl, S, Sn, Pb.

Guida verificata passo dopo passo
1
Understand that first ionization energy is the energy required to remove the outermost electron from a neutral atom in the gaseous state.
Recall that ionization energy generally increases across a period (from left to right) and decreases down a group (from top to bottom) in the periodic table.
Identify the positions of the given elements in the periodic table: Cl (Chlorine) and S (Sulfur) are in the same period, while Sn (Tin) and Pb (Lead) are in the same group.
Compare Cl and S: Since Cl is to the right of S in the same period, Cl has a higher first ionization energy than S.
Compare Sn and Pb: Since Sn is above Pb in the same group, Sn has a higher first ionization energy than Pb.

Concetti chiave

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

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. It is a key factor in determining an element's reactivity and is influenced by the atomic structure, including the number of protons and the distance of the outer electrons from the nucleus.
Video consigliato:
Percorso guidato
01:19
Ionization Energy

Trends in the Periodic Table

Ionization energy generally increases across a period from left to right due to increasing nuclear charge, which holds electrons more tightly. Conversely, it decreases down a group as the outer electrons are farther from the nucleus and experience greater shielding from inner electrons, making them easier to remove.
Video consigliato:
Percorso guidato
00:38
Periodic Trends

Comparison of Elements

When comparing elements like Cl, S, Sn, and Pb, it is essential to consider their positions in the periodic table. Chlorine (Cl) is a non-metal in period 3, sulfur (S) is also a non-metal in period 3, while tin (Sn) and lead (Pb) are metals in periods 5 and 6, respectively, which typically have lower ionization energies due to their larger atomic radii and increased electron shielding.
Video consigliato:
Percorso guidato
02:35
Elemental Forms of Elements
Pratica correlata
Domanda del libro di testo

Choose the element with the higher first ionization energy from each pair. d. P or Sn

480
views
Domanda del libro di testo

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

2072
views
Domanda del libro di testo

Arrange these elements in order of increasing first ionization energy: Si, F, In, N.

1501
views
2
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 higher first ionization energy from each pair. a. P or I b. Si or Cl c. P or Sb d. Ga or Ge

1734
views
1
rank
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