#### • Class 11 Physics Demo

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# chemical reactivity trend

Question:we are supposed to draw arrows on a periodic table to indicate the 4 different trends. for example the atomic radius would have and arrow pointing down to indicate the increase in size as well as an arrow pointing to the right. however i cant find the trend for reactvity so it would be great if someone could help me out. thanks =)

Answers:Reactivity - Reactivity refers to how likely or vigorously an atom is to react with other substances. This is usually determined by how easily electrons can be removed (ionization energy) and how badly they want to take other atom's electrons (electronegativity) because it is the transfer/interaction of electrons that is the basis of chemical reactions. Metals Period - reactivity decreases as you go from left to right across a period. Group - reactivity increases as you go down a group Why? The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity. Non-metals Period - reactivity increases as you go from the left to the right across a period. Group - reactivity decreases as you go down the group. Why? The farther right and up you go on the periodic table, the higher the electronegativity, resulting in a more vigorous exchange of electron

Question:

Answers:they get more reactive as you go down (at least they do with water)

Question:Its asking me what periodic trends of reactivity occur with the alkali metals...what is it asking for??

Answers:Metals Period - reactivity decreases as you go from left to right across a period. Group - reactivity increases as you go down a group Why? The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity. Non-metals Period - reactivity increases as you go from the left to the right across a period. Group - reactivity decreases as you go down the group. Why? The farther right and up you go on the periodic table, the higher the electronegativity, resulting in a more vigorous exchange of electron.

Question:What model can be used to explain these trends?

Answers:Four major factors: nuclear charge, atomic radius, shielding effect and sublevel arrangement (of electrons.) Metal reactivity relates to ability to lose electrons (oxidize), form basic hydroxides, form ionic compounds with non-metals yada yada... In general, the bigger the atom, the greater the ability to lose electrons. The greater the shielding, the greater the ability to lose electrons. Therefore, metallic character increases going down the table, and decreases going across -- so the most active metal is towards the left and down. (Keep in mind these are trends, not absolutes) For non-metals, it is nearly the opposite. Non-metallic character is the ability to be reduced (be an oxidizing agent), form acidic hydroxides, form covalent compounds with non-metals... These characteristics increase with a larger nuclear charge and smaller radius, with no increase in shielding. The most active non-metal would be the one farthest up and to the right -- not including the noble gases (non-reactive.) Is this what you're looking for?