Question

1. Based on the periodic trends for metallic properties, whichelements have the biggest atomicradius?2. Sort the elements in order ofincreasing metallic properties. Ca,M.Sc, Be, Bd3. Why is the electronegativityvalue of most noble gases zero?4. A nonmetal has a smaller ionicradius compared with a metal ofthe same period. Do you agree?​

Answer 1

1) The largest atomic radius has element 1) tin 2) carbon 3) Germanium 4) silicon. 

2) Be, Mg Ca, Sc,???

3) All their energy levels are filled to the end, so they do not act as oxidizers and restorers, although they are non-metallic.

4) I agree, that atomic radii, when moved from left to right in the same period, decrease. This is because electrons are more attracted to the nucleus as the core charge increases. Even an increase in the number of electrons on the outer shell (e.g. fluoride compared to oxygen) does not increase the size of the atom. That is, the fluoride atom is smaller than the oxygen atom.

Answer 2

1. Based on the periodic trends for metallic properties, the elements with the biggest atomic radius are generally found in the bottom left corner of the periodic table. These elements are known as the alkali metals and alkaline earth metals. Examples of elements with large atomic radii include cesium (Cs), francium (Fr), and barium (Ba).

2. To sort the elements in order of increasing metallic properties among Ca, M.Sc, Be, and Bd, we need to consider factors such as ionization energy, electron affinity, and electronegativity. Generally, metallic properties increase from right to left and from top to bottom on the periodic table. Based on this trend, the ordering would be: Bd < Ca < Be < M.Sc.

3. The electronegativity value of noble gases is zero because these elements have a full valence shell of electrons and are highly stable. Noble gases have a completely filled outer electron shell, making them very unreactive. As a result, they have no tendency to attract or gain additional electrons, leading to an electronegativity value of zero.

4. No, I do not agree. In general, nonmetals have larger ionic radii compared to metals of the same period. This is because nonmetals tend to gain electrons to form negatively charged ions, resulting in an increase in the electron cloud surrounding the nucleus and thus larger ionic radii. Metals, on the other hand, tend to lose electrons to form positively charged ions, which leads to a decrease in the electron cloud size and therefore smaller ionic radii.