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2.52: Alkaline Earth Metals

Difficulty Level: At Grade Created by: CK-12
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We take a lot of chemistry for granted.  Very few of us think about the chemistry of bone or oyster shells.  Both of these materials have large amounts of calcium compounds in them and play important roles in maintaining the structure of the organism.  The shell provides a solid surrounding for the oyster. Bones give support to the body so the person can move around and not just be a soft mass of tissue.

Alkaline Earth Metals

Group II elements are referred to as “alkaline earthmetals (tan column below).  The name “alkaline” comes from the fact that compounds of these elements form basic (pH greater than 7) or alkaline solutions when dissolved in water.  If the Group I elements all have one s electron in their outer orbital, we can predict that the Group II elements will have two electrons in that outer shell.

The beryllium atom, the first element of Group II, has an atomic number of four.  The atom has the 1s shell filled as well as the 2s shell, giving a total of four electrons (1s22s2). Note that there are two s electrons in the outer shell, a structure that is characteristic of the Group II elements. Barium (atomic number 56) has the same outer shell structure of two electrons in the s orbital, even though the internal electron structure for barium is quite complicated.

Radium (atomic number 88) technically falls in the Group II category, but is usually not considered as far as the chemistry goes.  Radium is a radioactive element and is generally under the category of radioisotopes since it is not a stable element.

The Group II elements tend to be less reactive than their Group I counterparts.  The need to remove two electrons in order for the material to react means more energy is needed for electron removal.  However, these elements are reactive enough that they do not exist in their elemental forms in nature, but are present as compounds.

Uses of Alkaline Earth Compounds

Since magnesium burns brightly, it is used in flares and fireworks.  Magnesium alloys with aluminum provide light weight and sturdy materials for airplanes, missiles, and rockets.  Several antacids use magnesium hydroxide to neutralize excess stomach acid.

Calcium compounds are widely found in limestone, marble, and chalk.  Calcium is an important constituent of cement.  Other uses include calcium chloride as a deicer and limestone as a white pigment in paints and toothpaste.

Strontium is widely used in fireworks and magnets.  Barium compounds can be used in paints, filler for rubber, plastic, and resins, and as a contrast medium for X-rays. Many beryllium compounds are toxic, but these materials have been employed in metal alloys

Summary

  • The alkaline earth elements are in Group II of the periodic table.
  • These elements each have two s electrons in their outer shell.
  • The alkaline earth elements are less reactive than the alkali metals.

Practice

Use the link below to answer the following questions:

http://www.rsc.org/chemsoc/visualelements/pages/data/intro_groupii_data.html

  1. What color are all the alkaline earth elements?
  2. In what compounds is magnesium found in nature?
  3. In what compounds is calcium found in nature?

Review 

  1. Why are these elements known as “alkaline earth” elements?
  2. How many electrons are in the outer shell of the alkaline earth elements?
  3. Are the alkaline earth elements more or less reactive than the alkali metals? Explain your answer?
  4. Is radium usually considered as part of the alkaline earth category in terms of chemistry? Explain your answer.

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Vocabulary

alkaline Earth metal

Metal in group 2 of the periodic table that has two valence electrons and is very reactive but less so than an alkali metal.

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Difficulty Level:
At Grade
Grades:
7 , 8
Date Created:
Oct 31, 2012
Last Modified:
Sep 13, 2016
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