Why Does Reactivity Decrease?

Period – reactivity decreases as you go from left to right. Period – reactivity increases as you go from the left to the right.

Does reactivity of metals increase or decrease going across a period?

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.

Why does reactivity of non metals increase across a period?

For Non-Metals, the farther right-up in the table you go, the higher the electronegativity. That is why as you go up a group Chemical Reactivity increases because it is easier for elements to gain electrons when they have high electronegativity.

Why does reactivity increase down the group?

Explaining trends

The reactivity of Group 1 elements increases as you go down the group because: the atoms get larger as you go down the group. … the attraction between the nucleus and outer electron gets weaker as you go down the group – so the electron is more easily lost.

Why does reactivity increase down Group 2?

As you progress down Group 2, the reactivity increases. This is due to a decrease in ionisation energy as you progress down the group. As it requires less energy to form the ions, the reactivity increases.

How does reactivity of metals vary in a period?

Reactivity of metals depends on the tendency to lose electrons. … As we move down the group, the tendency to gain electrons decreases because as the atomic size increases, the effective nuclear charge decreases.

How does it change across a group and period?

Across each period, from left to right, the increasing attraction between the nuclei and the outermost electrons causes the metallic character to decrease. Conversely, non-metallic character generally decreases down groups and increases across a period.

Why does the atomic radius change across a period?

Across a period, effective nuclear charge increases as electron shielding remains constant. A higher effective nuclear charge causes greater attractions to the electrons, pulling the electron cloud closer to the nucleus which results in a smaller atomic radius.

Why does reactivity increase up Group 7?

The group 7 elements want to gain one more electron so that they have a stable electronic structure. The smaller the atom, the easier it is to grab an electron from another atom, making the atom more reactive. As you go down group 7, the atomic radius increases and it becomes more difficult to attract another electron.

Why does non metal reactivity decrease down a group?

Nonmetal reactivity decreases down a group because the nucleus’ ability to gain more valence electrons weakens due to more nuclear shielding. For Metals: the most reactive metals are those that can lose their valence electrons the most easily. … Francium is the most reactive metal.

How does atomic radius affect reactivity?

The smaller the atomic radius, the more influence the nucleus has on reactivity. … The nucleus of smaller atoms is more exposed and thus exhibits a stronger pull. Therefore, the smaller the atomic radius, the more reactive the halogen atom, making fluorine the most reactive element in Group 17.

Why does electron affinity increase across a period?

When moving left to right across a period, the electron affinity increases. … The increase in positive charge increases the attraction between the nucleus and the electrons of the atom. Thus, the electrons are held more tightly towards the nucleus, increasing electron affinity.

Why does electronegativity decrease down a group and increase across a period?

So, as you move down a group on the periodic table, the electronegativity of an element decreases because the increased number of energy levels puts the outer electrons very far away from the pull of the nucleus. Electronegativity increases as you move from left to right across a period on the periodic table.

Does reactivity decrease across a period?

Period – reactivity decreases as you go from left to right across a period. 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.

Does reactivity decrease down a group?

As we go down the group, the atom gets bigger. The bigger the atom, the further away the last electron. Therefore, the attraction between the nucleus and the last electron gets weaker. This makes it easier for the atom to give up the electron which increases its reactivity.

Why is the periodic trend for reactivity opposite for metals and non metals?

Since the ionization energy decreases going down a group (or increases going up a group), the increased ability for metals lower in a group to lose electrons makes them more reactive. … Nonmetals tend to gain electrons in chemical reactions and have a high attraction for electrons within a compound.

Does the reactivity increase or decrease in Group 2?

The reactivity of the group 2 elements increase as you go down the group. This is because, as explained previously, it is much easier to remove an outer shell electron as you go further down the group (lower ionisation energies).

How does reactivity change down group 1 and group 2 elements?

Reactivity increases down the group. This is because the smaller the atom the closer the outer electrons are to the nucleus. Therefore there is a greater attraction between the nucleus and electrons in magnesium than there is in calcium.

What is the main reason for this decrease down the group?

Going down a group, the ionisation energy decreases. This is due to the shielding or screen effect of the outer electrons from the nucleus and so the attraction is weaker and they are more easily removed.

Why does reactivity increase going down the alkali family while it increases going up the halogen family?

Halogens from bromide to fluorine get more reactive because the force of attraction between the nucleus (core) and the outer electron get stronger as you go up group 7 elements. … As you go down group 1 (the alkali metals) in the periodic table, the elements get more reactive.

Does reactivity increase down Group 0?

All elements in group 0 are un-reactive(have eight electrons in the outer shell) and gases. boiling points of the gases increase down the group. … Alkali metals have similar chemical properties because when they react their atoms need to lose one electron so that they have a stable electronic structure.

Why is the reactivity of alkali metal increases down the group while reactivity of halogens decreases?

Alkali metals have one electron in their respective valence shells. … Thus, the reactivity of alkali metals depend upon their ability to lose electrons. Since their tendency to lose electrons increases down the group hence their reactivity increases down the group.

Why does atomic size affect reactivity?

The larger an atom is, the more reactive it will be. It helps to think about the size of an atom with the location of the electrons and nucleus in mind. … This makes it easier for the valence electrons to leave the atom and form an ionic bond or to interact with another atom to form a covalent bond.