Advertisements
Advertisements
प्रश्न
How does the metallic and non-metallic character vary on moving from left to right in a period?
Advertisements
उत्तर
As we move from left to right in a period, the number of valence electrons increases by one at each succeeding element but number of shells remains same. Due to this, effective nuclear charge increases. More is the effective nuclear charge, more is the attraction between the nucleus and electron.
Hence, the tendency of the element to lose electrons decreases. This results in decrease in metallic character. Furthermore, the tendency of an element to gain electrons increases with increase in effective nuclear charge, so non-metallic character increases on moving from left to right in a period.
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 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.
Ge (belongs to period 4 and group 14)
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?
Consider the oxides Li2O, CO2, B2O3.
Give the formula of an amphoteric oxide.
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 ______.
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?
The electronic configuration of Pt (atomic number 78) is ______.
\[\ce{_92U^235}\] is a member of VI B group. The new element formed by the emission of α-particle will be a member of ______ group.
The IUPAC nomenclature of an element with electronic configuration [Rn] 5f146d17s2 is ______.
