Advertisements
Advertisements
प्रश्न
Assign the position of the element having an outer electronic configuration in the periodic table.
(n - 1)d2 ns2 for n = 4
उत्तर १
Since n = 4, the element belongs to the 4th period. It is a d–block element as d–orbitals are incompletely filled.
There are 2 electrons in the d–orbital.
Thus, the corresponding group of the element
= Number of s–block groups + number of d–block groups
= 2 + 2
= 4
Therefore, it is a 4th period and 4th group element. Hence, the element is Titanium.
उत्तर २
n = 4
Means element belongs to 4th period belongs to group 4 as in the valence shell (2 + 2) = 4 electrons.
Electronic configuration = 1s2 2s2 2p6 3s2 3p6 3d2 4s2, and the element name is Titanium (Ti).
APPEARS IN
संबंधित प्रश्न
Write the atomic number of the element present in the third period and a seventeenth group of the periodic table.
Use the periodic table to answer the following question.
Identify an element with five electrons in the outer subshell.
Use the periodic table to answer the following question.
Identify an element that would tend to lose two electrons.
Assign the position of the element having an outer electronic configuration in the periodic table.
ns2 np4 for n = 3
Write the outer electronic configuration of the following using the orbital notation method. Justify.
Ge (belongs to period 4 and group 14)
Answer the following question.
The electronic configuration of some element is given below:
1s2 2s2 2p6
In which group and period of the periodic table the element is placed?
Answer the following question.
For s-block and p-block elements show that the number of valence electrons is equal to its group number.
Consider the oxides Li2O, CO2, B2O3.
Which oxide would you expect to be the most basic?
The first ionisation enthalpies of \[\ce{Na, Mg, Al}\] and \[\ce{Si}\] are in the order:
In the modern periodic table, elements are arranged in order of increasing atomic numbers which is related to the electronic configuration. Depending upon the type of orbitals receiving the last electron, the elements in the periodic table have been divided into four blocks, viz, s, p, d and f. The modern periodic table consists of 7 periods and 18 groups. Each period begins with the filling of a new energy shell. In accordance with the Arfbau principle, the seven periods have 2, 8, 8, 18, 18, 32 and 32 elements respectively. The seventh period is still incomplete. To avoid the periodic table being too long, the two series of f-block elements, called lanthanoids and actinoids are placed at the bottom of the main body of the periodic table.
The electronic configuration of the element which is just above the element with atomic number 43 in the same group is ______.
An element belongs to 3rd period and group-13 of the periodic table. Which of the following properties will be shown by the element?
(i) Good conductor of electricity
(ii) Liquid, metallic
(iii) Solid, metallic
(iv) Solid, non metallic
Identify the group and valency of the element having atomic number 119. Also predict the outermost electronic configuration and write the general formula of its oxide.
How would you explain the fact that first ionisation enthalpy of sodium is lower than that of magnesium but its second ionisation enthalpy is higher than that of magnesium?
How does the metallic and non-metallic character vary on moving from left to right in a period?
Justify the given statement with suitable examples— “the Properties of the elements are a periodic function of their atomic numbers”.
The electronic configuration of Pt (atomic number 78) is ______.
E.N. of Si is ______. (Covalent radius of Si = 1.175 Å)
\[\ce{_92U^235}\] is a member of VI B group. The new element formed by the emission of α-particle will be a member of ______ group.
