Survey of recent news. Transition metals Social Research Paper

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Transition metals
In chemistry, an interactive periodic table presents a dynamic arrangement of elements according to their atomic number, electron configuration as well as physical and chemical properties. Rows, which are also referred to as periods showcase metals to the left, while columns which are groups contain non-metals. Generally, periodic table helps to bring about the relationship of various elements and discovering synthesized elements using their chemical reactions and behavior. Looking at elements across the table, their electrons in the outer layer of the atoms have little shielding effects, hence an increase in protons leading to an effective nuclear charge.
Consequently, the smaller the atomic radius, the higher the ionization energy, improved electronegativity, and more nonmetallic character. As elements continue to the right of the table, there reaches a point where this property breaks at a calcium whose number of protons Zis 20. After that, the first transition series are remarkably similar in their physical and chemical properties. Their similarity lies over a minimal difference in nuclear charge. The free electron occupies the space in the 3d layer and forms a protective layer between the nucleus and the outer shell. Therefore the table clearly describes transition elements as those whose d electron is fully filled.
Elements with similar chemical properties are generally presented in similar groups of the periodic table. It is relatively easy to define stoichiometry of an element if he understands the characteristics around the group. The following are both physical and chemical properties of transition metals.
1 They have a large atomic radius with a great charge
2 They have a gradual increase in density due to their increase in atomic radii.
3 The metals are boiling, and the melting point is high as well. This is due to their strong metallic bonding as a result of delocalization of electrons.
4 They form paramagnetic compounds
5 Oxidation state varies
6 Form colored ions and compound
7 Moreover, finally, they form stable complexes
Continuously, there are trends in the properties of each metal group. For example, group 3 elements (scandium Sc, yttrium Y, lanthanum La, and actinium Ac) share similarities with group 1 and 2. Loose of the three free electrons characterizes the oxidation state of these elements. Based on periodic trends, these elements react highly with metals and powerful reductants having La and Ac being the most reactive. The electropositivity of these elements makes them react with water to yield the metal hydroxide and hydrogen gas:
2M(s) +6H2O (l) →2M(OH)3(s)+3H2(g)
Metals are generally shiny, greatly conducting solids that form compounds when reacted with one another and salty compounds with nonmetals. Group of transition metals; titanium (Ti), zirconium (Zr) and hafnium (Hf) are highly attracted to oxygen and occur naturally as oxidized metals due to losing the four free valence electrons. This oxidation state represents the chemistry of these metals Ti having the lowest. Concerning their role in the society, titanium off late has been used in aerospace application due to its extreme melting point 1668°C instead of aluminum which has 660°C. Supersonic aircraft operate under temperatures almost to an aluminum melting point. Thereby, titanium can resist these temperatures and resist corrosion. Metallic zirconium is exploited in making fuel rods when hafnium makes control rods in nuclear reactors. Metal dioxides (MO2) and chalcogens (MY2) are formed after reaction with oxygen. Importantly, TiO2 is industrially used in making the white color in paints. The binary compounds formed by these group 4 elements are nonstoichiometric and are best metallic conductors.
TiCl4(g)+O2(g)&...