The acid-base behaviour of the "hydroxides" (using the term in the widest possible sense) of the Period 3 elements. The physical properties of the chlorides of the elements from sodium to sulphur, their structure and bonding, and their reactions with water. Group - reactivity decreases as you go down the group. Group - reactivity increases as you go down a group In Non-metals Period - reactivity increases as you go from the left to the right. Reactions of the oxides with water, and their acid-base behaviour. In Metals: Period - reactivity decreases as you go from left to right.
Example: Calcium is in the 2nd group therefore it has 2 electrons in the outer shell and a. As you move from left to right across the periodic table, atoms have more electrons in their outer energy level and more. The reactions of the elements from sodium to argon with water, oxygen and chlorine.ĭiscusses the link between the physical properties of the oxides of the elements from sodium to chlorine and their structure and bonding. Elements increase in atomic number across each period by one. The overall trend is that reactivity with water decreases across Period 3 from left to right, with Chlorine being the slight exception. Across a period from left to right, the covalent radius decreases. Which oxide dissolves in water to give a solution with a pH below 7 A. As the atomic size reduces, it becomes more difficult to eliminate an electron nearer to a more central nucleus. Which trends are correct across period 3 (from Na to Cl) I. As you move across a period, the first ionization energy increases. The low ones elements tend to be reducing agents. In 1871 he arranged the elements in vertical columns by their atomic. ĭiscusses the trends in first ionisation energy, atomic radius, electronegativity, conductivity, melting point and boiling point as you go across the period from sodium to argon. The ionization energy of an element can be used to determine its reactivity. Dmitri Mendeleev was the first to organize the elements by their periodic properties. Physical and atomic properties of the elements.
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