Electron configurations magnesium

Magnesium [7439-95-4] atomic number 12, is in Group 2 (IIA) of the Periodic Table between beryllium and calcium. It has an electronic configuration of 1T2T2 3T and a valence of two. The element occurs as three isotopes with mass numbers 24, 25, and 26 existing in the relative frequencies of 77, 11.5, and 11.1%, respectively. 

Write out the electron configuration of sodium, magnesium, and aluminum and find the ionization energies for all their valence electrons (Table 20-IV, p. 374). Account for the trend in the heats of vaporization and boiling points (Table 20-1) of these elements. Compare your discussion with that given in Section 17-1.3. 

Exercises 21-1 and 21-2 pose some of the simplest questions we can ask about the alkaline earths. The periodic table arranges in a column elements having similar electron configurations. We can expect elements on the left side of the periodic table to be metals (as magnesium is). Furthermore, we can expect that the elements in a given column will be more like each other than they will be like elements in adjacent columns. Thus, when we find that the chemistry of magnesium is almost wholly connected with the behavior of the dipositive magnesium ion, Mg+l, we can expect a similar situation for calcium, and for strontium, and for each of the other alkaline earth elements. This proves to be so. 

The alkaline earth metals in Group 2 of the periodic table must lose two electrons to reach a more stable state. Magnesium is an alkaline earth metal with an electron configuration of... 

It must lose two electrons in its 3s orbital to obey the octet rule. This creates a magnesium ion with a charge of +2. Thus, a magnesium ion has the same electron configuration as the sodium ion but a different charge. Both ions have the same stable electron configuration as the noble gas neon ... 

Suppose we want to write the electron configuration of scandium (atomic number 21). We can rewrite the first 12 electrons that we wrote above for magnesium, and then just keep going. As we added electrons, we filled the first shell of electrons first, then the second shell. When we are filling the third shell, we have to ask if the electrons with n = 3 and / = 2 will enter before the n = 4 and 1 = 0 electrons. Since (n + /) for the former is 5 and that for the latter is 4, we must add the two electrons with n = 4 and / = 0 before the last 10 electrons with n = 3 and / = 2. In this discussion, the values of m and s tell us how many electrons can have the same set of n and / values, but do not matter as to which come first. 

EXAMPLE 17.10. Write the electron configuration of magnesium. ls-2s22p63s2. 

Magnesium reacts with element X to form an ionic compound. If the ground-state electron configuration of Xis Is 2s 2p, what is the simplest formula for this compound ... 

Use the aufbau principle to write complete electron configurations and complete orbital diagrams for atoms of the following elements sodium, magnesium, aluminum, silicon, phosphorus, sulfur, chlorine, and argon (atomic numbers 11 through 18). 

Ateacher asks the class to write electron configurations for magnesium, iron, and tin. Lois does not have a periodic table available. Edward s advice is to use a memory aid that is shown below. Write a short paragraph to explain howto use this memory aid. 

Indicate the position of beryllium, magnesium, calcium, strontium, and barium in Mendeleev s periodic table of the elements, the electron configurations and size of their atoms, and their oxidation states. 

This group contains the elements beryllium (Be), magnesium (Mg), calcium (Ca), strontium (Sr), barium (Ba) and radium (Ra). After the alkali metals, they are the second most active metals. Their electron configurations end with ns2. They become positive two charged ions by giving of their two valence electrons in chemical reactions. At room temperature, they occur in a monoatomic structure and they are solid at room temperature. Radium, a solid element, is the only radioactive member of this group. 

The third ionization energy of magnesium is very high because the electron configuration of Mg2+ has noble gas stability. 

With these definitions, the ground state of the magnesium atom is then represented by the electron configuration for the orbitals Is, 2s, 2p, and 3s (see Fig. 1.1) and the symbols for the angular momenta and parity as... 

An experiment is said to be, within a certain theoretical framework, perfect or complete if from different experimental observations complementary information can be obtained which finally allows the determination of all matrix elements involved and, therefore, all possible observables. This will be illustrated for 2p photoionization in atomic magnesium (ground state electron configuration ls22s22p63s2). 

Magnesium can lose the two electrons in its valence shell and attain the electronic configuration of neon. 

All magnesium nuclei have charge +12 electronic units, so that 12 electrons orbit the nucleus of the neutral atom. Its electronic configuration can be abbreviated as an inner core of inert neon (a noble gas) plus two more electrons (Ne)3s2, which locates Mg beneath beryllium in Group II of the periodic table. Magnesium therefore has valence +2 and combines readily with oxygen atoms as MgO. 

EXAMPLE 4.12. Using the periodic table, determine the detailed electronic configuration of magnesium. 

By losing two electrons, a magnesium atom attains the electronic configuration of a neon atom and thereby acquires... 

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