Chapter 3

If \(q\) for an electron is \(-1\), a) what is \(q\) for a proton? b) what is \(q\) for a neutron? c) what is \(q\) for the nucleus of a \(C\) atom?

Recall that a \({ }^{1} \mathrm{H}\) atom consists of a proton as the nucleus and an electron outside of the nucleus. Is the potential energy of a hydrogen atom a positive or negative number?

Which of the following systems will have the larger ionization energy? Explain your reasoning. a) an electron at a distance of \(500 \mathrm{pm}\) from a nucleus with charge \(+2\) b) an electron at a distance of \(700 \mathrm{pm}\) from a nucleus with charge \(+2\)

Which of the following systems will have the larger ionization energy? Explain your reasoning. a) an electron at a distance \(d_{1}\) from a nucleus with charge \(+2\) b) an electron at a distance \(d_{1}\) from a nucleus with charge \(+1\)

Consider a hydrogen atom and a helium ion, \(\mathrm{He}^{+} .\) Which of these do you expect to have the larger ionization energy? Explain your reasoning, including any assumptions you make.