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WorksheetsPERIODIC TABLE
Total questions: 15
Worksheet time: 8mins
Periodicity of the elements in the Periodic Table refers to
The arrangement of elements in increasing order of proton numbers
The arrangement of elements in increasing order of neutron numbers
The electronegativity of elements across a period
The classification of elements based on increasing proton numbers and similar valence electronic configuration
*The first three successive ionisation energies for the element N increase gradually but the fourth ionisation energy increases sharply.
*Element N is a third period element.
*N form an amphoteric oxide.
Which of the following s electronic configuration matches the statements above?
1s2 2s2 2p6 3s2 3p1
1s2 2s2 2p6 3s2 3p3
1s2 2s2 2p6 3s2 3p6 3d1 4s2
1s2 2s2 2p6 3s2 3p6 3d3 4s2
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
decreases, increases
increases, increases
increases, decreases
stays the same, increases
Which of the following elements has the smallest atomic radius?
Sulfur [Z=16]
Chlorine[Z=17]
Aluminum[Z=13]
Sodium[Z=11]
Atomic radius generally increases as we move __________.
down a group and from right to left across a period
up a group and from left to right across a period
down a group and from left to right across a period
up a group and from right to left across a period
Which block is letter C
s - block
p - block
d - block
f - block
Based on the successive ionisation energies below,how many valence electrons does the element M have?
IE1 = 943
IE2 = 1,950
IE3 = 3,852
IE4 = 5,492
IE5 = 23,085
IE6 = 26,791
IE7 = 30,024
2
3
4
5
What will be formed when Al2O3 reacts with NaOH?
NaAlO + H2O
NaAlO2 + H2O
NaAlO3 + H2O
Na3Al + H2O
Element Q has the following electronic configuration:
1s2 2s2 2p6 3s2 3p6 3d5 4s1
Which of the following is true about the position of element Q in periodic table?
Period 3, Group 1, Block s
Period 4, Group 16, Block d
Period 4, Group 6, Block d
Period 4, Group 1, Block s
What is the tendency of an atom to attract electrons towards itself?
atomic radius
ionization energy
shielding
Electronegativity
Why does ionization energy decrease going down a group?
Adding more energy levels makes the valence electron further from the nucleus
There are more valence electrons in the outer shell
There are more protons in the nucleus
There are less protons in the nucleus
Which is smaller... Mg or Mg2+ ?
Mg because it gains an energy level
Mg due to extra electron repulsion
Mg2+ because of extra electron repulsion
Mg2+ because it loses an energy level
Why the electronegativity of Cl is the highest in Period 3?
Cl is the largest and has the greatest effective nuclear charge
Cl is the smallest and has the lowest effective nuclear charge
Cl is the largest and has the lowest effective nuclear charge
Cl is the smallest and has the greatest effective nuclear charge
