Trends in the Periodic Table
Chemistry ⇒ Atomic Structure and the Periodic Table
Trends in the Periodic Table starts at 9 and continues till grade 12.
QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Trends 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 10
Arrange the following elements in order of increasing ionization energy: K, Na, Li.
As you move down a group in the periodic table, what happens to the atomic radius?
Context: Consider the elements magnesium (Mg), aluminum (Al), and silicon (Si) in period 3. Which has the highest electronegativity?
Describe the trend in electron affinity across a period from left to right.
Describe the trend in reactivity of alkali metals as you move down the group.
Explain why fluorine is more reactive than chlorine among the halogens.
Explain why noble gases have very low reactivity.
Explain why the atomic radius of noble gases is larger than that of halogens in the same period.
Which element in period 2 has the highest ionization energy?
Which element is more likely to gain an electron: sodium or chlorine? Explain your answer.
Which group in the periodic table contains the most reactive metals?
Which property increases both across a period (left to right) and up a group (bottom to top) in the periodic table?
Context: Consider the elements calcium (Ca), strontium (Sr), and barium (Ba) in Group 2. Which of these elements would react most vigorously with water, and why?
Describe how the trend in metallic character across a period is related to the trend in ionization energy.
Explain why the first ionization energy of oxygen is lower than that of nitrogen, even though oxygen is to the right of nitrogen in the same period.
