Periodic table and its properties

Periodic table and its properties – II

Periodic properties and their variations in groups and periods, definition and trends in atomic size, metallic character, non-metallic character, ionisation potential electron affinity and electronegativity

1 / 10

Electron affinity generally becomes less negative as you move down a group because:

Atomic size increases, reducing the nuclear attraction for the added electron

Ionization energy decreases, making it harder to add electrons

Electronegativity decreases, lowering electron affinity

Metallic character increases

2 / 10

Which element is expected to show the least variation in electronegativity down its group in the periodic table?

Fluorine (F)

Nitrogen (N)

Carbon (C)

Phosphorus (P)

3 / 10

Valency of elements generally increases across a period until Group 14 and then decreases. This trend is due to:

Increasing atomic number

Variation in electron affinity

Filling of s and p orbitals

Increasing ionization energy

4 / 10

Which of the following trends in electronegativity is correct as you move from left to right across a period?

Decreases due to increasing atomic size

Increases due to increasing nuclear charge

Remains constant across the period

Decreases due to increasing metallic character

5 / 10

Which of the following elements has the highest electron affinity in the periodic table?

Oxygen (O)

Chlorine (Cl)

Fluorine (F)

Sulfur (S)

6 / 10

Which group in the periodic table contains elements with the highest ionization energies?

Group 1 (Alkali metals)

Group 18 (Noble gases)

Group 17 (Halogens)

Group 2 (Alkaline earth metals)

7 / 10

Which of the following best explains the decrease in metallic character as you move across a period from left to right?

Increase in ionization energy and electron affinity

Decrease in atomic size

Decrease in electron-electron repulsion

Increase in atomic size

8 / 10

What is the trend in atomic size as you move across a period from left to right?

Atomic size decreases due to increasing nuclear charge

Atomic size increases due to electron-electron repulsion

Atomic size increases due to decreasing electronegativity

Atomic size remains constant

9 / 10

Which of the following elements is expected to have the highest metallic character?

Sulfur (S)

Aluminum (Al)

Lithium (Li)

Francium (Fr)

10 / 10

As you move from top to bottom in Group 1 (alkali metals), which trend is observed in the reactivity of the elements?

Reactivity decreases due to increasing ionization energy

Reactivity increases due to decreasing ionization energy

Reactivity remains the same throughout the group

Reactivity decreases due to increasing electronegativity

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