Class 10SciencePeriodic Classification of ElementsMix Examples - Periodic Classification of Elements
MediumName the element which has:
$(a)$ the electronic configuration $2, 8, 1$.
$(b)$ a total of two shells,with $4$ electrons in the valence shell.
$(c)$ a total of three shells,with $3$ electrons in the valence shell.
$(d)$ one shell which is completely filled with electrons.
$(e)$ twice as many electrons in the second shell as in the first shell.
$(a)$ the electronic configuration $2, 8, 1$.
$(b)$ a total of two shells,with $4$ electrons in the valence shell.
$(c)$ a total of three shells,with $3$ electrons in the valence shell.
$(d)$ one shell which is completely filled with electrons.
$(e)$ twice as many electrons in the second shell as in the first shell.
(N/A) Sodium $(Na)$ has the electronic configuration $2, 8, 1$.
$(b)$ Carbon $(C)$ has atomic number $6$. Its electronic configuration is $2, 4$. It has a total of two shells ($K$ and $L$),with $4$ electrons in the valence shell.
$(c)$ Aluminium $(Al)$ has atomic number $13$. Its electronic configuration is $2, 8, 3$. It has a total of three shells ($K, L,$ and $M$),with $3$ electrons in the valence shell.
$(d)$ Helium $(He)$ has atomic number $2$. Its electronic configuration is $2$. It has one shell $(K)$ which is completely filled with $2$ electrons.
$(e)$ Carbon $(C)$ has atomic number $6$. Its electronic configuration is $2, 4$. The first shell $(K)$ has $2$ electrons and the second shell $(L)$ has $4$ electrons. Thus,it has twice as many electrons in the second shell as in the first shell.
$(b)$ Carbon $(C)$ has atomic number $6$. Its electronic configuration is $2, 4$. It has a total of two shells ($K$ and $L$),with $4$ electrons in the valence shell.
$(c)$ Aluminium $(Al)$ has atomic number $13$. Its electronic configuration is $2, 8, 3$. It has a total of three shells ($K, L,$ and $M$),with $3$ electrons in the valence shell.
$(d)$ Helium $(He)$ has atomic number $2$. Its electronic configuration is $2$. It has one shell $(K)$ which is completely filled with $2$ electrons.
$(e)$ Carbon $(C)$ has atomic number $6$. Its electronic configuration is $2, 4$. The first shell $(K)$ has $2$ electrons and the second shell $(L)$ has $4$ electrons. Thus,it has twice as many electrons in the second shell as in the first shell.
Explore More
Similar Questions
Up to which element was the Law of Octaves found to be applicable?
Easy
View SolutionThree elements $A$, $B$, and $C$ have $3$, $4$, and $2$ electrons respectively in their outermost shell. Determine the group number to which they belong in the Modern Periodic Table and state their valencies.
Medium
View Solution$(a)$ Electropositive nature of the element$(s)$ increases down the group and decreases across the period.
$(b)$ Electronegativity of the element decreases down the group and increases across the period.
$(c)$ Atomic size increases down the group and decreases across a period (left to right).
$(d)$ Metallic character increases down the group and decreases across a period.
On the basis of the above trends of the Periodic Table,answer the following about the elements with atomic numbers $3$ to $9$:
$(a)$ Name the most electropositive element among them.
$(b)$ Name the most electronegative element.
$(c)$ Name the element with the smallest atomic size.
$(d)$ Name the element which is a metalloid.
$(e)$ Name the element which shows maximum valency.
$(b)$ Electronegativity of the element decreases down the group and increases across the period.
$(c)$ Atomic size increases down the group and decreases across a period (left to right).
$(d)$ Metallic character increases down the group and decreases across a period.
On the basis of the above trends of the Periodic Table,answer the following about the elements with atomic numbers $3$ to $9$:
$(a)$ Name the most electropositive element among them.
$(b)$ Name the most electronegative element.
$(c)$ Name the element with the smallest atomic size.
$(d)$ Name the element which is a metalloid.
$(e)$ Name the element which shows maximum valency.
Difficult
View SolutionMendeleev predicted the existence of certain elements not known at that time and named two of them as Eka-silicon and Eka-aluminium.
$(a)$ Name the elements which have taken the place of these elements.
$(b)$ Mention the group and the period of these elements in the Modern Periodic Table.
$(a)$ Name the elements which have taken the place of these elements.
$(b)$ Mention the group and the period of these elements in the Modern Periodic Table.
Medium
View SolutionArrange the following elements in the order of their increasing non-metallic character: $Li, O, C, Be, F$.
Medium
View SolutionVedclass Products
For Students
Vedclass Test Series
Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.
Start Free TrialFor Teachers
Exam Paper Generator
Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.
Try FreeFor Institutes
Online Exam Module
Live online exams with unlimited students, 360° analytics & white-label branding.
See Demo