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Periods and Groups in the Periodic Table

Chemistry ⇒ Atomic Structure and the Periodic Table

Periods and Groups in the Periodic Table starts at 8 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Periods and Groups in the Periodic Table. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.
See sample questions for grade 12
Describe the trend in electronegativity as you move across a period from left to right.
Describe the trend in metallic character as you move across a period from left to right.
Describe the trend in reactivity of halogens as you move down group 17.
Explain the difference between a group and a period in the periodic table.
Explain why elements in the same group have similar chemical properties.
Explain why the atomic radius increases as you move down a group.
Explain why the noble gases are chemically inert.
Explain why the reactivity of alkali metals increases as you move down the group.
State the group and period of the element with the electron configuration [Ar] 4s2 3d10 4p5.
State the group number and period number for the element with the electron configuration 1s2 2s2 2p6 3s2 3p5.
State the period and group of the element with the electron configuration [Ne] 3s2 3p1.
State the total number of periods in the modern periodic table.
The alkali metals are found in which group of the periodic table?
The d-block elements are found in which periods of the periodic table?
The lanthanides and actinides are placed separately at the bottom of the periodic table. State the period numbers to which they belong.
What is the general trend in atomic radius as you move from left to right across a period?
Which period contains the element with the highest electronegativity?
An element has the electron configuration [Kr] 5s2 4d10 5p2. State its group and period in the periodic table.
Describe how the shielding effect influences the trends in atomic radius and ionization energy as you move down a group in the periodic table.
Explain why the first ionization energy of elements generally increases across a period, but there are exceptions such as between group 2 and group 13 elements.