Periodic Table Archives - Flash Education

Arrange the following elements as per the guidelines in brackets.
(a) Na, Cl, Mg, P [in decreasing order of atomic size]
(b) C, Li, F, N [in increasing order of electronegativity]
(c) Cl, Al, Na, S [in increasing order of ionization potential]
(d) Li, F, C, O [in increasing order of electron affinity]
(e) Ar, He, Ne [in increasing order of number of electron shells]

(a) Na > Mg > P > Cl (b) Li < C < N < F (c) Na < Al < S < Cl (d) Li < C < O…

Give reasons for the following:
If combining atoms have nearly similar electronegativities the bond between them is covalent.

If two combining atoms have almost similar electronegativities then transference of electrons cannot take place and the atoms share their valence electron equally with each other hence covalent bond is…

Give reasons for the following:
Down a group electronegativity should increase with increase in nuclear charge but it is seen that the electronegativity decreases.

On moving down a group both atomic size and nuclear charge increases but the increase in atomic size dominates over increase in nuclear charge hence Electronegativity decreases on moving down…

Give reasons for the following:
Atomic size of an element depends on the nuclear charge of that element.

Nuclear charge is the positive charge present in the nucleus of an atom and when there is an increase in nuclear charge then the atomic size decreases because the electrons…

Give reasons for the following:
Properties of elements are periodic functions of their atomic numbers and not atomic weights.

Atomic number of an element is equal to the number of protons (or electrons in case of a neutral atom). Physical and chemical properties of elements depend on the number…

Give reasons for the following:
Occurrence of characteristic properties of elements takes place at definite intervals in the modern periodic table.

Characteristic properties recur at definite intervals in the modern periodic table because elements with similar valence shell configurations (and thus similar properties) appear periodically as you move through increasing atomic…

Match the elements in column ‘X’ with the correct group they belong from column ‘Y’
X Y
1: Element with atomic number 19 A: Group 18 [0 group]
2: Element with electronic configuration 2 B: Group 16 [VI A]
3: Element with a valency of -2 C: Group 1 [IA]
4: Element ‘P’ which loses 3 electrons to form a cation D: Group 17 [VII A]
5: Element ‘Q’ in period-3 which has the highest electron affinity E: Group 13 [III A]

X	Y
1: Element with atomic number 19	A: Group 18 [0 group]
2: Element with electronic configuration 2	B: Group 16 [VI A]
3: Element with a valency of -2	C: Group 1 [IA]
4: Element ‘P’ which loses 3 electrons to form a cation	D: Group 17 [VII A]
5: Element ‘Q’ in period-3 which has the highest electron affinity	E: Group 13 [III A]

X Y 1: Element with atomic number 19 A: Group 1 [IA] 2: Element with electronic configuration 2 B: Group 18 [0 group] 3: Element with a valency of -2…

With reference to group 1 [IA] of the periodic table – fill in the blanks with the correct word:
The elements are …………… [light/heavy] …………… [metals/non metals] since their atomic size is …………… [large/small]. The energy binding the atoms is …………… [high/low] and hence the elements have …………… [high/low] melting points. The melting points of the elements …………… [increases/decreases] down the subgroup. The electropositive character …………… [increases/decreases] down the subgroup and the elements are strong …………… [reducing/oxidizing] agents. The element with electronic configuration 2, 8, 1 will have …………… [higher/lower] electron affinity and …………… [smaller/larger] atomic size than the element with electronic configuration 2, 1.

The elements are light metals since their atomic size is large. The energy binding the atoms is low and hence the elements have low melting points. The melting points of the elements decreases down the subgroup. The electropositive character increases down…

With reference to period 3 of the periodic table — State :
(a) The type of bonding of the element with electronic configuration 2, 8, 7.
(b) The formula of the chloride of the element with electronic configuration 2, 8, 4.
(c) The nature of the oxide of the alkaline earth metal in the period.
(d) The number of electrons in the penultimate shell of the element with valency -1.
(e) The electronic configuration of the element whose hydroxide is a weak base.

(a) The element with electronic configuration 2, 8, 7 will form ionic bonds with metals and with non-metal it will form covalent bond. (b) The element with electronic configuration is 2, 8,…

In period 2, element ‘A’ is to the right of element ‘B’
(a) The element ‘A’ would probably have a …………… [smaller/larger] atomic size than ‘B’.
(b) The element ‘B’ would probably have …………… [lower/higher] ionization potential than ‘A’.
(c) The element ‘A’ would have …………… [lesser/higher] electron affinity than ‘B’.
(d) Nuclear charge of element ‘B’ would be …………… [less/more] than element ‘A’.
(e) If an element ‘C’ had a low electronegativity and ionization potential it would have more tendency to …………… [gain/lose] electrons.

(a) The element 'A' would probably have a smaller atomic size than 'B' (b) The element 'B' would probably have lower ionization potential than 'A'. (c) The element 'A' would have higher electron…