Reactivity increases down the group for metals. It decreases down the group for non-metals.
In the alkali metals column (Group 1), atomic radius increases down the group and reactivity increases. There are more shells preventing the attraction between the positive nucleus and negatively charged outer electron. (All Group 1 elements have 1 electron in their outer shell). Also, because they contain more shells down the group, the distance between the nucleus and electrons is increased. Therefore the electrostatic force is lessened between them. Both of these allow the outer electron to be lost easier to other elements, thus increasing reactivity.
Chemical properties. The classic example is the Group (I) Alkali metals, they all react with water., to produce the hydroxide, and liberate hydrogen gas. Here is the general equation 2M + 2H2O = 2MOH + H2 However in going down this Group , their reactivity with water becomes more violent, from genetle fizzing (Lithium) to explosive (Francium). Francium is not found in a lab. because it is also radio-active. Group (II) Alkaline Earth metals also have a similar property, but their reactivity is more genetle. M + 2H2O = M(OH)2 + H2
Caesium belong to Group (1) The Alkali metals. Since it is the lowest in the Group , except for 'Francium', its reactivity with water and oxygen is 'explosive'. Going down the Group (1) the elements are , with increasing reactivity , Lithium, Sodium, Potassium, Rubidium, Caesium, and Francium. You will not find francium in the open lab. as it is radio-active.
The Alkali Earth metals are found in group 1 and 2 of the periodic table. When reacted with hydrochloric acid, the vigour of the reactions increases going down the groups. So Lithium will react gently with hydrochloric acid whilst Caesium will react explosively. The same applies for the group 2 metals. Generally speaking, Alkali metals will react with hydrochloric acid: X + HCl -----------> XCl + H2 Where X is the alkali metal and will react to form a chloride
There's no reason for it.It was built on the basis of increasing atomic number and then the similarities were observed. However you can say this is because of the presence of the metalloids present b/w them which form the zig-zag line.
Alkali metals have increasing reactivity going down the group. Francium may not be considered as it is not a stable atom: it is radioactive. The next four are Cesium, Rubidium, Potassium and Sodium in decreasing reactivity order.
The reactivity is increasing goinng down in the group.
In the alkali metals column (Group 1), atomic radius increases down the group and reactivity increases. There are more shells preventing the attraction between the positive nucleus and negatively charged outer electron. (All Group 1 elements have 1 electron in their outer shell). Also, because they contain more shells down the group, the distance between the nucleus and electrons is increased. Therefore the electrostatic force is lessened between them. Both of these allow the outer electron to be lost easier to other elements, thus increasing reactivity.
Chemical properties. The classic example is the Group (I) Alkali metals, they all react with water., to produce the hydroxide, and liberate hydrogen gas. Here is the general equation 2M + 2H2O = 2MOH + H2 However in going down this Group , their reactivity with water becomes more violent, from genetle fizzing (Lithium) to explosive (Francium). Francium is not found in a lab. because it is also radio-active. Group (II) Alkaline Earth metals also have a similar property, but their reactivity is more genetle. M + 2H2O = M(OH)2 + H2
Caesium belong to Group (1) The Alkali metals. Since it is the lowest in the Group , except for 'Francium', its reactivity with water and oxygen is 'explosive'. Going down the Group (1) the elements are , with increasing reactivity , Lithium, Sodium, Potassium, Rubidium, Caesium, and Francium. You will not find francium in the open lab. as it is radio-active.
A family is a vertical column in the periodic table. Elements in a family all share similar characteristics, whether they be physical or chemical. There are 18 family (or group) columns in the periodic table.
In the Periodic table of Elements There are 118 Elements 96 are metals The rest are non-metals Group 7= Halogens Group 8/0= Noble gases Going down group 1 and 2, elements become more reactive
The Group 1 and Group 17 elements are the most reactive. Group 1 is the Alkali metals, and their reactivity increases going down the column. Group 17 is the Halogens, and their reactivity increases going up the column.this is not answering the question. The question asks which ORGANIC Functional group (amine, ketone, etc.) is the most reactive, not which group on the periodic table.
Yes they do, with metaloids in between.
AnswerAlkali metals are the most reactive metalsFrancium is the most reactive metal. This is as it has many layers, the last layer having only one electron, far away from the positive pull of the proton.
The Alkali Earth metals are found in group 1 and 2 of the periodic table. When reacted with hydrochloric acid, the vigour of the reactions increases going down the groups. So Lithium will react gently with hydrochloric acid whilst Caesium will react explosively. The same applies for the group 2 metals. Generally speaking, Alkali metals will react with hydrochloric acid: X + HCl -----------> XCl + H2 Where X is the alkali metal and will react to form a chloride
The rows on the Periodic table are called "periods" and the increasing atomic number across a period represents additions to the electron orbitals, which cause the properties manifested by individual elements (elements of the same group, or column, have similar properties).