8. The physical and chemical properties of an element are often an \"average\" o
ID: 560920 • Letter: 8
Question
8. The physical and chemical properties of an element are often an "average" of the properties of the surrounding elements. Consider Osmium, element number 76. 1t is preceded by Rhenium, Re, and followed by Iridium, Ir. Look up the aelting points and boiling points of iridium and rhenium in K from the Perio Chart. Predict the melting point and boiling point for Osnium by taking averages Then look up the actual values for 0smiunm compare. Predicted Actual R melting point boiling point Neon are Noble gases. They form very few compounds to be known as "inert" gases. Consult the Periodic Table 9. Helium and and used and write the names and symbols of the other elementrs expect to be Noble gases on the basis of atomio structure , explain why the atoms of the alkali metals are so much larger than the atoms of the noble gases which precede them. CHint: write the eleotron configuration for Li and then for He which precedes it.) 10. Ionization Potential and Electron Affinity a. Ionization Potential is a measure of the energy necessary to remove an electron from a neutral gaseous atom. If Z repre- sents an atom, then z energy 2 Based on your understanding of an atom gaining or losing electrons to attain a stable electron configuration, would it be a metal or a non easier to remove an electron from metal? tion potentials Family, the ionization potentials ioniza- Thus, we say that metals have than non-metals. As one goes down a Group or Page 4 of Formal Report 6Explanation / Answer
8.
The melting and boiling points of Re, Ir and Os are taken from internet and predicted melting and boiling points of Os are calculated from average of both the melting and boiling points of Re and Ir.
9. In the periodic table, the noble gases are in 18th group. Apart from helium (He) and neon (Ne), other noble gases are argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).
The size of alkali metals is much larger than the noble gases because of the addition of extra shell. For example, the electronic configuration of He is 1s2, while for Li, it is 1s2 2s1. So, we can see here that for Li, another shell of 2s has been added to it. It is the same reason for all other alkali atoms and noble gases atoms.
10. In periodic table, the metals lie in 1st and 2nd group (i.e. alkali and alkaline earth metals). The non-metals lie in the middle of the periodic table. For metals, on removing 1 or 2 electrons, leads to noble gas configuration. For example, Li is an alkali metal. It has electronic configuration of 1s2 2s1. On removing one electron by using ionisation energy, it will have electronic configuration of 1s2. This is same as He, which is a noble gas an thus make it stable. So, it is easy for metals to lose electron. While for non-metals, even after losing one electron, they can not attain noble gas configuration, so they are unstable. The fill in the blanks are:
Based on the understanding of an atom gaining or losing electrons to attain a stable electron configuration, would it be easier to remove an electron from a metal or a non-metal? Metal
Thus, we say that metals have less ionisation potentials than non-metals.
As one goes down a Group or family, the ionisation potentials decreases. (the reason is that as we move down the group, the size of the atom increases and the electron is loosely held by the nucleus. So, it becomes easy to remove the electron.)
Property Re Ir Predicted for Os Actual for Os Melting point 3455 K 2720 K 3087.5 K 3306 K Boiling point 5870 K 4403 5136.5 K 5300 KRelated Questions
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