Calcium electron configuration

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. 

As befits the electron configuration of elemental calcium, the metal is very reactive, readily losing two valence electrons to form the dispositive ion. In aqueous solution and ia its compounds, is colorless. Most calcium compounds ate white, unless the cation is paired with a colored anion. The ion... 

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. 

By losing two electrons, calcium attains the electron configuration of argon and thereby acquires a charge of 2+. ... 

By gaining one electron, the bromine atom attains the electron configuration of krypton and also attains a charge of 1-. The two ions expected are therefore Ca + and Br. Since calcium bromide as a whole cannot have any net charge, there must be two bromide ions for each calcium ion hence, the formula is CaBr2. 

We could follow the procedures just illustrated to write the electron configurations of elements 11 through 18 in which the 3s and 3p orbital are being filled. However, we will not write all of these out rather, we will summarize the electron configuration of argon, Is2 2s2 2p2 3s2 3p6, as (Ar). When this is done, the next element, potassium, has the configuration (Ar) 4s1 and that of calcium is (Ar) 4s2. The sum (n + l) is 4 for both the 3p and 4s levels, and the lower value of n is used first (3p). The next levels to be filled are those for which ( + ) = 5, and these are the 3d, 4p, and 5s. In this case, the 3d orbitals... 

Calcium reacts with element X to form an ionic compound. If the ground-state electron configuration of X is ls22s22p4, what is the simplest formula for this compound ... 

This Group IIA (or Group 2) element (atomic symbol, Ca atomic number, 20 atomic weight, 40.078 electronic configuration = ls 2s 2p 3s 3p 4s ) loses both As electrons to form a divalent cation of 0.99A ionic radius. Ionic calcium combines readily with oxygen ligands (chiefly water, phosphates, polyphosphates, and carbox-ylates) to form stable metal ion complexes. Ca under-... 

For brevity, many chemists record the electron configuration of an atom by giving only its outermost subshell, like As for potassium or 4/ for calcium. These electrons are most distant from the positive nucleus and, therefore, are most easily transferred between atoms in chemical reactions. These are the valence electrons. 

The charges on the chlorine, potassium, and calcium ions result from a strong tendency of valence electrons to adopt the stable configuration of the inert gases, with completely filled electronic shells. Notice that the 3 ions have electronic configurations identical to that of inert argon. 

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. 

Look at the electron configurations of potassium and calcium, the s-block elements immediately preceding the first transition series. These atoms have 4s valence electrons, but no d electrons ... 

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. 

Figure 5.4 Electron Transfer in Calcium Oxide Figure 5.5 Electron Transfer and Electron Configurations for Calcium Oxide ...

To illustrate the principles of electron configurations in stable, solid ionic compounds, we will consider the formation of an ionic compound from calcium and oxygen. We can predict what compound will form by considering the valence electron configurations of the two atoms ... 

For example, the atomic number of calcium is 20 (corresponding to 20 electrons). Therefore the electronic configuration is ... 

---