Ch.8 - Periodic Properties of the Elements

Tro - Chemistry: A Molecular Approach 4th Edition

Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook

Tro 4th Edition

Ch.8 - Periodic Properties of the Elements

Problem 78

Chapter 8, Problem 78

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?

Verified step by step guidance

Identify the pattern in the ionization energies: Notice the large jump between IE3 and IE4.

Recall that a large increase in ionization energy typically indicates the removal of an electron from a new, inner shell.

Determine the number of valence electrons: The large jump after IE3 suggests that the element has 3 valence electrons.

Identify the third-period element with 3 valence electrons: In the periodic table, elements in the third period with 3 valence electrons are in Group 13.

Conclude the element: The third-period element in Group 13 is Aluminum (Al).

Verified video answer for a similar problem:

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.

Ionization Energy

Ionization energy is the amount of energy required to remove an electron from an atom or ion in its gaseous state. It is a key indicator of an element's reactivity and can vary significantly among different elements. Generally, ionization energy increases across a period in the periodic table due to increasing nuclear charge, which holds electrons more tightly.

Trends in Ionization Energies

Ionization energies exhibit specific trends in the periodic table. As you move from left to right across a period, ionization energy tends to increase due to the greater effective nuclear charge experienced by the outer electrons. Conversely, as you move down a group, ionization energy decreases because the outer electrons are further from the nucleus and experience more shielding from inner electrons.

Identification of Elements

To identify an element based on its ionization energies, one can compare the given values to known ionization energies of elements in the same period. The significant jump in ionization energy values, particularly between IE3 and IE4, suggests that the element has a stable electron configuration after losing three electrons, indicating it is likely a non-metal in the third period, such as phosphorus or sulfur.

Recommended video:

Guided course

01:15

Chalcogen Identification Example

Related Practice

Textbook Question

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

480

views

Textbook Question

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

2072

views

Textbook Question

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

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

324

views

Textbook Question

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

431

views

Textbook Question

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

rank

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?

Verified video answer for a similar problem:

Key Concepts

Ionization Energy

Trends in Ionization Energies

Identification of Elements

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?