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 84

Chapter 8, Problem 84

Arrange these elements in order of decreasing metallic character: Sr, N, Si, P, Ga, Al.

Verified step by step guidance

Understand that metallic character refers to how easily an element can lose electrons to form positive ions (cations).

Recall that metallic character increases as you move down a group in the periodic table and decreases as you move across a period from left to right.

Identify the positions of the given elements in the periodic table: Sr (Strontium) is in Group 2, N (Nitrogen) is in Group 15, Si (Silicon) is in Group 14, P (Phosphorus) is in Group 15, Ga (Gallium) is in Group 13, and Al (Aluminum) is in Group 13.

Compare the elements based on their positions: Sr is the most metallic as it is in Group 2 and further down the group, followed by Al and Ga which are in Group 13, then Si in Group 14, and finally P and N in Group 15.

Arrange the elements in order of decreasing metallic character: Sr, Al, Ga, Si, P, N.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Metallic Character

Metallic character refers to the set of properties associated with metals, including conductivity, malleability, ductility, and luster. It generally increases as you move down a group in the periodic table and decreases across a period from left to right. This trend is due to the increasing atomic size and decreasing ionization energy, which make it easier for atoms to lose electrons.

Periodic Trends

Periodic trends are predictable patterns observed in the periodic table, such as atomic radius, electronegativity, and ionization energy. Understanding these trends helps in predicting the behavior of elements, including their metallic character. For instance, elements on the left side of the periodic table tend to exhibit more metallic properties compared to those on the right.

Group and Period Position

The position of an element in the periodic table, defined by its group (vertical column) and period (horizontal row), significantly influences its properties. Elements in the same group share similar characteristics, while those in the same period show a gradual change in properties. For example, alkaline earth metals like strontium (Sr) are highly metallic, while nonmetals like nitrogen (N) are not.

Recommended video:

Guided course

01:33

Lone Pair Positions

Related Practice

Textbook Question

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

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

Arrange these elements in order of increasing metallic character: Fr, Sb, In, S, Ba, Se.

704

views

Textbook Question

Write the balanced chemical equation for the reaction of solid strontium with iodine gas.

974

views

Textbook Question

Write the balanced chemical equation for the reaction of solid lithium with liquid water.

862

views