Advertisements
Advertisements
Question
Explain the following:
Metallic character of elements decreases from left to right in a period while it increases in moving down a group.
Solution
On moving across a period, nuclear pull increases because of the increase in atomic number, and thus, the atomic size decreases. Hence, elements cannot lose electrons easily. Hence, Group 17 elements are strong non-metals, while Group 1 elements are strong metals. Down a group, the atomic size increases and the nuclear charge also increases. The effect of an increased atomic size is greater as compared to the increased nuclear charge. Therefore, metallic nature increases as one moves down a group, i.e. they can lose electrons easily.
RELATED QUESTIONS
Arrange the following as per the instructions given in the brackets:
Cl, F, Br, I (increasing order of electron affinity)
In Period 3 of the Periodic Table, element B is placed to the left of element A. On the basis of this information, choose the correct word from the option to complete the following statement:
The element B would have ______ metallic character than A.
Metallic character and non-metallic character are periodic properties discuss ?
An element barium has atomic number 56. Look up its position in the periodic table and answer the following question.
Is it a metal or a non-metal?
State whether the following statement is true or false
All members of zero group are non metals.
If an element is in group 7 is it likely to be metallic or non metallic in character?
Arrange the following elements in order of their decreasing metallic character.
Na, Si, Cl, Mg, Al
The tendency of an element to form anion is the ______ character of that element.
Write the name.
Two elements having two orbits.
Write scientific reason.
The metallic character of elements increases while going down the groups.
