Chapter 7

The successive ionization energies for an unknown element are $$\begin{array}{rl}{I}_1& =896\mathrm{kJ}/\mathrm{mol}\\ I_2& =1752\mathrm{kJ}/\mathrm{mol}\\ I_3& =14,807\mathrm{kJ}/\mathrm{mol}\\ I_4& =17,948\mathrm{kJ}/\mathrm{mol}\end{array}$$ To which family in the periodic table does the unknown element most likely belong?

In the ground state of cadmium, Cd, a. how many electrons have $\ell =2$ as one of their quantum numbers? b. how many electrons have $n=4$ as one of their quantum numbers? c. how many electrons have $m_{\ell }=-1$ as one of their quantum numbers? d. how many electrons hav $m_s=-\frac{1}{2}$ as one of their quantum numbers?

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?

Assume that a hydrogen atom's electron has been excited to the $n=6$ level. How many different wavelengths of light can be emitted as this excited atom loses energy?

Determine the maximum number of electrons that can have each of the following designations: $2f,2d_{xy},3p,5d_{yz},$ and 4$p.$

Consider the ground state of arsenic, As. How many electrons have $\ell =1$ as one of their quantum numbers? How many electrons have $m_{\ell }=0?$ How many electrons have $m_{\ell }=+1?$

Which of the following statements is (are) true? a. The 2$s$ orbital in the hydrogen atom is larger than the 3s orbital also in the hydrogen atom. b. The Bohr model of the hydrogen atom has been found to be incorrect. c. The hydrogen atom has quantized energy levels. d. An orbital is the same as a Bohr orbit. e. The third energy level has three sublevels, the s,p, and d sublevels.

Identify the following three elements. a. The ground-state electron configuration is $[\mathrm{Kr}]5s^{2}4d^{10}5p^4$ b. The ground-state electron configuration is $[\mathrm{Ar}]4s^{2}3d^{10}4p^2$ c. An excited state of this element has the electron configuration 1$s^{2}2s^{2}2p^{4}3s^1$

Which of the following statements is(are) true? a. F has a larger first ionization energy than does Li. b. Cations are larger than their parent atoms. c. The removal of the first electron from a lithium atom (electron configuration is 1$s^{2}2s^1)$ is exothermic - that is, removing this electron gives off energy. d. The He atom is larger than the ${\mathrm{H}}^{+}$ ion. e. The Al atom is smaller than the Li atom.

Three elements have the electron configurations 1$s^2{2}^{2}2p^{6}3s^2$ 1$s^{2}2s^{2}2p^{6}3s^{2}3p^4$ , and 1$s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^2.$ The first ionization energies of these elements (not in the same order) are 0.590 , 0.999, and 0.738 MJ/mol. The atomic radii are 104, 160, and 197 pm. Identify the three elements, and match the appropriate values of ionization energy and atomic radius to each configuration. Complete the following table with the correct information.