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Chapter 4: Problem 18

Why is barium, Ba, placed in Group 2 and in Period 6\(?\)

Short Answer

Expert verified
Barium (Ba) is placed in Group 2 because it has two electrons in its outermost shell, and in Period 6 because it has six shells of electrons.

Step by step solution

01

Understand the Periodic Table

The structure of the Periodic Table is important for this exercise. The Periodic Table groups elements based on similar properties and atomic structure. Vertically, elements are divided into groups or families, and horizontally into periods. In the Periodic Table, each period represents one new energy level being filled with electrons. Each group represents the number of electrons in the outermost energy level.
02

Understanding Barium's Position

Barium (Ba) is placed in Group 2 because it has two electrons in its outermost energy level, like all Alkaline Earth Metals. Thus, it belongs to Group 2 in the Periodic Table.
03

Understand Periods in the Periodic Table

Periods on the other hand, represent the number of energy levels. Barium (Ba) is placed in Period 6 because it has six energy levels or shells of electrons.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Barium
Barium is a fascinating element with the symbol Ba and atomic number 56. It is one of the alkaline earth metals, known for its distinctive properties and practical uses. Barium is soft, silvery-white, and highly reactive. This element does not occur freely in nature, and is typically found in combination with other elements in various minerals. For example, barium sulfate and barium carbonate are common compounds.
  • Barium is known for its high density and ability to absorb X-rays, making it valuable in medical imaging techniques.
  • It is also used in the production of glass, ceramics, and rubber, providing unique benefits due to its chemical properties.
  • Barium compounds can impart a green color to fireworks, enhancing displays with their vibrant hues.
Group 2 elements
The Group 2 elements on the Periodic Table are known as the alkaline earth metals. This group includes beryllium, magnesium, calcium, strontium, barium, and radium. They share several common characteristics:
  • Each of these elements has two electrons in their outermost energy level. This configuration influences their chemical reactivity and bonding properties.
  • Alkaline earth metals tend to lose their two valence electrons to form +2 ions. This makes them typically highly reactive, although generally less reactive than Group 1 metals (alkali metals).
  • They are all shiny and silvery-white in appearance when pure, but tarnish when exposed to air due to oxidation.
  • The members of this group also have relatively low densities, melting points, and boiling points compared to transition metals.
Period 6 elements
Elements in Period 6 of the Periodic Table have unique and interesting features. This period contains a diverse range of elements, from metals and nonmetals to metalloids, and is longer than any preceding period. Period 6 elements include Cesium, Barium, and the Lanthanides. Here鈥檚 what sets them apart:
  • The elements in Period 6 have six principal energy levels or electron shells.
  • Moving across the period, the elements fill the 6s, 4f, 5d, and 6p subshells. The inclusion of f-block elements in this period makes it notably longer.
  • Barium, in particular, has a full 6s subshell, placing it within the alkaline earth metals, while other elements further along the period display varying valence electron configurations.
  • Periodicity in properties such as atomic radius and ionization energy is observed across the elements in this period, due to the gradual filling of electron shells.

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Most popular questions from this chapter

Without looking at the periodic table, identify the period and group in which each of the following elements is located. $$\begin{array}{l}{\text { a. }[\mathrm{Rn}] 7 s^{1}} \\ {\text { b. }[\mathrm{Ar}] 4 s^{2}} \\ {\text { c. }[\mathrm{Ne}] 3 s^{2} 3 p^{6}}\end{array}$$

Which of the following ions has the electron configuration of a noble gas: \(\mathrm{Ca}^{+}\) or \(\mathrm{Cl}^{-} ?\) (Hint: Write the electron configuration for each ion.)

Why was Mendeleev's periodic table accepted by most chemists?

Why don't chemists define atomic radius as the radius of the electron cloud that surrounds a nucleus?

Write a paragraph describing in your own words how synthetic elements are created. Discuss what modification has to be made to the equipment in order to synthesize super-heavy elements.
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