Alkaline Earth Metals Valence Electrons
half-dozen.10: Alkaline Earth Metals
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How are oyster shells and chemical science related?
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 take large amounts of calcium compounds in them and play important roles in maintaining the structure of the organism. The vanquish provides a solid surrounding for the oyster. Basic give support to the body so the person can move effectually and non just be a soft mass of tissue.
Alkaline Earth Metals
Group ii elements are referred to as "alkaline metal earth" metals (tan column below). The proper noun "alkaline" comes from the fact that compounds of these elements formbasic(pH greater than seven) or alkali metal solutions when dissolved in h2o. If the Group 1 elements all have one \(s\) electron in their outer orbital, we can predict that the Group 2 elements will have two electrons in that outer shell.
The beryllium atom, the showtime chemical element of Group 2, has an atomic number of four. The atom has the 1s shell filled every bit well every bit the 2s shell, giving a full of four electrons (\(1s^2 2s^two\)). Notation that there are two \(due south\) electrons in the outer crush, a construction that is characteristic of the Grouping two elements. Barium (atomic number 56) has the same outer vanquish structure of two electrons in the \(s\) orbital, even though the internal electron structure for barium is quite complicated.
Radium (atomic number 88) has similar backdrop to barium and is besides in the Group 2 category. However, radium is a radioactive element and is generally nether the category of radioisotopes in addition to being an alkaline earth metal, because it is not a stable element.
The Group two elements tend to be less reactive than their Group ane counterparts. The need to remove two electrons in order for the material to react means more energy is needed for electron removal. Nevertheless, these elements are reactive plenty that they do not be in their elemental forms in nature, but are nowadays as compounds.
Uses of Element of group i 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 tummy 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 tin be used in paints, filler for rubber, plastic, and resins, and every bit 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 2 of the periodic table.
- These elements each have ii s electrons in their outer vanquish.
- The alkaline earth elements are less reactive than the alkali metals.
Review
- Why are these elements known as "alkaline earth" elements?
- How many electrons are in the outer shell of the alkaline earth elements?
- Are the alkaline metal earth elements more or less reactive than the brine metals? Explain your answer.
- Is radium usually considered as part of the alkaline earth category in terms of chemistry? Explain your answer.
Alkaline Earth Metals Valence Electrons,
Source: https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_%28CK-12%29/06:_The_Periodic_Table/6.10:_Alkaline_Earth_Metals
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