Periodic Properties (10)

Periodic properties and their variations in groups and periods

Periodicity on the basis of atomic number for elements

The energy required to remove an electron
Match the atomic number 2, 4, 8, 15, and 19
He, Ar, Ne (Increasing order of the number of electron shells)
Na, Li, K (Increasing Ionisation Energy)
F, Cl, Br (Increasing electronegativity)
Na, K, Li (Increasing atomic size)
The tendency of an atom to attract electrons
The electrons present in the outermost shell of an atom
If an element has a low ionization energy then it is likely to be
If an element has seven electrons in its outermost shell
Use the letters only written in the Periodic Table
The following table shows the electronic configuration of the elements W, X, Y, Z:
The most electronegative element from the following elements is
In Period 3, the most metallic element is
The tendency of an atom to attract electrons towards itself
Arrange in decreasing order of ionization potential: Li, K, Na, H
Arrange in increasing order of electron affinity: F, B, N, O
The element with highest ionization potential is
The tendency of an atom to attract electrons to itself
The following table represent the elements and the atomic number
Name the following elements
Ionisation potential increases across a period, from left to right
In Period 3 of the Periodic Table, element B is placed to the left of element A