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Chapter 2: Problem 11

With regard to electron configuration, what do all the elements in Group IIA of the periodic table have in common?

Short Answer

Expert verified
Answer: All elements in Group IIA of the periodic table have 2 valence electrons in their outermost s-orbital.

Step by step solution

01

Identify Group IIA elements

Group IIA elements (alkaline earth metals) include Beryllium (Be), Magnesium (Mg), Calcium (Ca), Strontium (Sr), Barium (Ba), and Radium (Ra).
02

Determine electron configurations

Write down the electron configurations for each element: - Beryllium (Be): 1s^2 2s^2 - Magnesium (Mg): 1s^2 2s^2 2p^6 3s^2 - Calcium (Ca): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 - Strontium (Sr): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 - Barium (Ba): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 - Radium (Ra): 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^10 6p^6 7s^2
03

Identify the common feature

Observe the electron configurations and look for similarities. In each electron configuration, the outermost (highest energy level) orbital always has two electrons. These electrons are called valence electrons and are represented by the "s^2" in the electron configuration. All Group IIA elements have 2 valence electrons in their outermost s-orbital. Therefore, the answer to the question is: All elements in Group IIA of the periodic table have 2 valence electrons in their outermost s-orbital.

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Most popular questions from this chapter

To what group in the periodic table would an element with atomic number 112 belong?

(a) What electron subshell is being filled for the rare earth series of elements on the periodic table? (b) What electron subshell is being filled for the actinide series?

Without consulting Figure \(2.8\) or Table \(2.2\), determine whether each of the following electron configurations is an inert gas, a halogen, an alkali metal, an alkaline earth metal, or a transition metal. Justify your choices. (a) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{5}\) (b) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{7} 4 s^{2}\) (c) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6}\) (d) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1}\) (e) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{10} 4 s^{2} 4 p^{6} 4 d^{5} 5 s^{2}\) (f) \(1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2}\)

For the \(K\) shell, the four quantum numbers for each of the two electrons in the \(1 s\) state, in the order of \(n l m_{l} m_{s}\), are \(100 \frac{1}{2}\) and \(100\left(-\frac{1}{2}\right)\). Write the four quantum numbers for all of the electrons in the \(L\) and \(M\) shells, and note which correspond to the \(s, p\), and \(d\) subshells.

Silicon has three naturally occurring isotopes: \(92.23 \%\) of \({ }^{28} \mathrm{Si}\), with an atomic weight of \(27.9769\) amu; \(4.68 \%\) of \({ }^{29} \mathrm{Si}\), with an atomic weight of \(28.9765 \mathrm{amu} ;\) and \(3.09 \%\) of \({ }^{30} \mathrm{Si}\), with an atomic weight of \(29.9738\) amu. On the basis of these data, confirm that the average atomic weight of \(S i\) is \(28.0854 \mathrm{amu}\).
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