An element’s reactivity is determined by the number of protons found in an atom of the element.

The number of electrons in the outermost shell of an atom determines its reactivity. Noble gases have low reactivity because they have full electron shells. Halogens are highly reactive because they readily gain an electron to fill their outermost shell.

Reactant concentration, the physical state of the reactants, and surface area, temperature, and the presence of a catalyst are the four main factors that affect reaction rate.

Within each group of metals, reactivity increases as you go down the group. The valence electrons are less tightly bound and easier to remove, because they are farther away from the nucleus of the atom. A nonmetal tends to attract additional valence electrons to attain a full valence shell.

In the periodic table, the number of valence electrons in each element decreases from left to right across each period. The reactivity of a metal depends on how easily it loses its valence electrons.

Noble gases

Element No. 8 on the Periodic Table of the Elements is a colorless gas that makes up 21 percent of Earth’s atmosphere. Because it’s all around, oxygen is easy to dismiss as dull and inert; in fact, it’s the most reactive of the non-metallic elements.

lithium

s-block elements

P-block metals have a few more electrons to lose to take part in a reaction and are less likely to form a compound or take part in a reaction.

The halogens, alkali metals, and alkaline earth metals are highly reactive.

• The most reactive element is fluorine, the first element in the halogen group.
• The most reactive metal is francium, the last alkali metal (and most expensive element).
• The least reactive elements are the noble gases.

Due to low ionisation ethalpy of metals, s-block elements ( both alkali and alkaline earth metals) are good reducing agents. Alkali metals have very low ionization energy and thus they are oxidised very easily and act as very strong reducing agents.

The following table provides the reduction potentials of the indicated reducing agent at 25 °C. For example, among sodium (Na), chromium (Cr), cuprous (Cu+) and chloride (Cl−), it is Na that is the strongest reducing agent while Cl− is the weakest; said differently, Na is the weakest oxidizing agent in this list while …

S-Block elements or alkali metals are good reducing agents mainly because of their strong tendency to lose the single valence electrons during a chemical reaction.

: a substance that reduces a chemical compound usually by donating electrons.

Break the reaction down into a net ionic equation and then into half-reactions. The substance that loses electrons is being oxidized and is the reducing agent. The substance that gains electrons is being reduced and is the oxidizing agent.

C is a better reducing agent than F III. Cl is smaller in size than F. IV. F can be oxidised more readily than Cl”.

Chlorine is an oxidising agent since it needs one electron in its valence shell to occupy the one empty space. Chlorine is capable of taking electrons from both iodide and bromide ions. Those electrons will not be reclaimed by bromine and iodine from the produced chloride ions.

Basic facts. The iodide ions lose electrons to form iodine molecules. In other words, they are oxidized. The chlorine molecules gain electrons to form chloride ions— they are reduced.

SO2 is more powerful reducing agent in alkaline medium. Was this answer helpful?

The oxalic acid acts as a reducing agent, and the KMnO4 acts as an oxidizing agent, KMnO4 acts as an indicator of where the permanganate ions are a deep purple colour.

The above reaction can be performed in an acidic or a basic medium….Chemical Properties Of Potassium Permanganate.

An acid which can decolourise purple coloured potassium permanganate solution is: (a) sulphuric acid.

KMnO4 has a deep purple color because of the charge transfer from the ligand (O2−) to the metal center. This is called ligand to metal charge transfer.

The oxalic acid acts as a reducing agent, and the KMnO4 acts as an oxidizing agent. In this redox titration, MnO4– is reduced to colourless manganous ions (Mn2+) in the acidic medium. The last drop of permanganate gives a light pink colour on reaching the endpoint.

Potassium permanganate(KMnO4) is colored because it absorbs light in the visible range of the electromagnetic spectrum. The permanganate ion is the source of the color, as a ligand-to-metal charge transfer takes place between the oxygen’s p orbitals and the empty d-orbitals on the metal.

KMnO4 solutions are dark purple. When used as a titrant, as soon as the endpoint is reached and the KMnO4- is in excess, the solution has a permanent pink hue (provided that the solution is initially colorless). Thus KMnO4 acts as its own indicator.

KMnO4 is not used as primary standard because it is difficult to obtain the pure state of KMnO4 as it is not free from MnO2. Also, the colour is so intense that it acts as its own indicator.

Potassium Permanganate is a versatile and powerful oxidant that can be used to determine many substances by direct or indirect titration. A unique advantage of Potassium Permanganate is that it serves as its own indicator. Titrations with Permanganate must be carried out in strong acid solution.

Permanganate Titration EndpointA redox titration using potassium permanganate as the titrant. Because of its bright purple color, KMnO4 serves as its own indicator.