Advertisements
Advertisements
प्रश्न
Write the outer electronic configuration of the following using the orbital notation method. Justify.
Ge (belongs to period 4 and group 14)
उत्तर
- Ge belongs to period 4. Therefore, n = 4.
- Group 14 indicates that the element belongs to the p-block of the modern periodic table.
- The general outer electronic configuration of group 14 elements is ns2np2.
- Thus, the outer electronic configuration of Ge is 4s24p2.
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 that would tend to lose two electrons.
Use the periodic table to answer the following question.
Identify an element that would tend to gain two electrons.
Use the periodic table to answer the following question.
Identify the group having metal, non-metal, liquid as well as gas at room temperature.
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.
Po (belongs to period 6 and group 16)
Write the outer electronic configuration of the following using the orbital notation method. Justify.
Cu (belongs to period 4 and group 11)
Answer the following.
La belongs to group 3 while Hg belongs to group 12 and both belong to period 6 of the periodic table. Write down the general outer electronic configuration of the ten elements from La to Hg together using the orbital notation method.
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:
The period number in the long form of the periodic table is equal to ______.
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 ______.
Which of the following sets contain only isoelectronic ions?
(i) \[\ce{Zn^{2+}, Ca^{2+}, Ga^{3+}, Al^{3+}}\]
(ii) \[\ce{K+ , Ca^{2+}, Sc^{3+}, Cl-}\]
(iii) \[\ce{P^{3-}, S^{2-}, Cl- , K+}\]
(iv) \[\ce{Ti^{4+}, Ar, Cr^{3+}, V^{5+}}\]
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?
Write down the outermost electronic configuration of alkali metals. How will you justify their placement in group 1 of the periodic table?
The electronic configuration of Pt (atomic number 78) is ______.
E.N. of Si is ______. (Covalent radius of Si = 1.175 Å)
The IUPAC nomenclature of an element with electronic configuration [Rn] 5f146d17s2 is ______.
