Where is fluorine in the reactivity series?
Fluorine is the most reactive element of all in Group 7. You can see the trend in reactivity if you react the halogens with iron wool.
What reactivity does fluorine have?
Fluorine readily forms compounds with most other elements, even with the noble gases krypton, xenon and radon. It is so reactive that glass, metals, and even water, as well as other substances, burn with a bright flame in a jet of fluorine gas. In aqueous solution, fluorine commonly occurs as the fluoride ion F-.
Is fluorine high or low reactivity?
fluorine (F), most reactive chemical element and the lightest member of the halogen elements, or Group 17 (Group VIIa) of the periodic table. Its chemical activity can be attributed to its extreme ability to attract electrons (it is the most electronegative element) and to the small size of its atoms.
Which is the correct order of reactivity series?
According to the electrochemical series the correct order of reactivity is Na>Mg>Zn>Cu.
Which is an application of the reactivity series?
Apart from providing insight into the properties and reactivities of the metals, the reactivity series has several other important applications. For example, the outcome of the reactions between metals and water, metals and acids, and single displacement reactions between metals can be predicted with the help of the activity series.
Which is the correct order of reactivity of water?
The order of reactivity, as shown by the vigour of the reaction with water or the speed at which the metal surface tarnishes in air, appears to be potassium > sodium > lithium > alkaline earth metals, the same as the reverse order of the (gas-phase) ionization energies.
Which is part of the reactivity series of manganese?
Long Tabular Form of the Reactivity Series Reactivity Series of Metals Ions Formed Manganese Mn2+ Zinc Zn2+ Chromium Cr3+ Iron Fe3+
Why are metals placed higher on the reactivity series?
Metals that are placed higher on the reactivity series have the ability to displace metals that are placed lower from their salt solutions. Higher ranking metals require greater amounts of energy for their isolation from ores and other compounds.