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Chapter 7: Problem 104

How many valence electrons do each of the following elements have, and what are the specific valence electrons for each element? a. Ca b. O c. element 117 d. In e. Ar f. Bi

Short Answer

Expert verified
a. Ca has 2 valence electrons (\(4s^2\)). b. O has 6 valence electrons (\(2s^2 2p^4\)). c. Element 117 has 7 valence electrons (\(7s^2 7p^5\)). d. In has 3 valence electrons (\(5s^2 5p^1\)). e. Ar has 8 valence electrons (\(3s^2 3p^6\)). f. Bi has 5 valence electrons (\(6s^2 6p^3\)).

Step by step solution

01

a. Ca (Calcium)

Calcium is an alkaline earth metal and is found in Group 2, Period 4 of the periodic table. Its symbol is 'Ca' and its atomic number is 20. The electron configuration for Calcium is \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2\). The valence electrons are the electrons in the highest occupied energy level, which is the 4s orbital. Calcium has 2 valence electrons, specifically the \(4s^2\) electrons.
02

b. O (Oxygen)

Oxygen is a non-metal and is found in Group 16, Period 2 of the periodic table. Its symbol is 'O' and its atomic number is 8. The electron configuration for Oxygen is \(1s^2 2s^2 2p^4\). The valence electrons are the electrons in the highest occupied energy level, which is the 2s and 2p orbitals. Oxygen has 6 valence electrons, specifically the \(2s^2\) and \(2p^4\) electrons.
03

c. Element 117

Element 117 hasn't got a common symbol, as it's a synthetic element that isn't found naturally. It's placed in Group 17 and Period 7 of the periodic table, and its atomic number is 117. The electron configuration for element 117 is [Rn] \(5f^{14} 6d^{10} 7s^2 7p^5\). As it's a member of the halogens group, we can infer it has 7 valence electrons, specifically the \(7s^2\) and \(7p^5\) electrons.
04

d. In (Indium)

Indium is a metal and is found in Group 13, Period 5 of the periodic table. Its symbol is 'In' and its atomic number is 49. The electron configuration for Indium is [Kr] \(4d^{10} 5s^2 5p^1\). The valence electrons are the electrons in the highest occupied energy level, which is the 5s and 5p orbitals. Indium has 3 valence electrons, specifically the \(5s^2\) and \(5p^1\) electrons.
05

e. Ar (Argon)

Argon is a noble gas and is found in Group 18, Period 3 of the periodic table. Its symbol is 'Ar' and its atomic number is 18. The electron configuration for Argon is \(1s^2 2s^2 2p^6 3s^2 3p^6\). The valence electrons are the electrons in the highest occupied energy level, which is the 3s and 3p orbitals. Argon has 8 valence electrons, specifically the \(3s^2\) and \(3p^6\) electrons.
06

f. Bi (Bismuth)

Bismuth is a metal and is found in Group 15, Period 6 of the periodic table. Its symbol is 'Bi' and its atomic number is 83. The electron configuration for Bismuth is [Xe] \(4f^{14} 5d^{10} 6s^2 6p^3\). The valence electrons are the electrons in the highest occupied energy level, which are the 6s and 6p orbitals. Bismuth has 5 valence electrons, specifically the \(6s^2\) and \(6p^3\) electrons.

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Most popular questions from this chapter

The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.

It takes \(7.21 \times 10^{-19} \mathrm{J}\) of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this?

For hydrogen atoms, the wave function for the state \(n=3\) \(\ell=0, m_{\ell}=0\) is $$\psi_{300}=\frac{1}{81 \sqrt{3 \pi}}\left(\frac{1}{a_{0}}\right)^{3 / 2}\left(27-18 \sigma+2 \sigma^{2}\right) e^{-\sigma \beta}$$ where \(\sigma=r / a_{0}\) and \(a_{0}\) is the Bohr radius $\left(5.29 \times 10^{-11} \mathrm{m}\right) .$ Calculate the position of the nodes for this wave function.

Predict some of the properties of element 117 (the symbol is Uus, following conventions proposed by the International Union of Pure and Applied Chemistry, or IUPAC). a. What will be its electron configuration? b. What element will it most resemble chemically? c. What will be the formula of the neutral binary compounds it forms with sodium, magnesium, carbon, and oxygen? d. What oxyanions would you expect Uus to form?

It takes 476 kJ to remove 1 mole of electrons from the atoms at the surface of a solid metal. What is the maximum wavelength of light that can remove a single electron from an atom at the surface of this solid metal?
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