Prepare for NEET Chemistry Classification of Elements (Electron Affinity) with MCQs & PYQs on NEET.GUIDE. Access free practice, previous year questions, and expert solutions to understand an element’s tendency to gain electrons.
NEET Questions / Chemistry / Classification of Elements and Periodicity in Properties / Electron Affinity
Which of the following statements regarding the electron affinity trends across a period and down a group is INCORRECT?
Electron affinity generally becomes more negative across a period due to increasing effective nuclear charge.
Electron affinity always becomes more negative down a group due to increasing atomic size.
Noble gases have positive electron affinities.
Electron affinity values can be influenced by interelectronic repulsions.
Why is the electron affinity of nitrogen less negative than that of carbon, despite nitrogen having a higher effective nuclear charge?
Nitrogen has a smaller atomic radius than carbon.
Nitrogen has a half-filled p subshell, which provides extra stability.
Carbon has a higher electronegativity than nitrogen.
The electron added to nitrogen experiences greater shielding.
Which element among the following has the most negative electron affinity?
Fluorine (F)
Chlorine (Cl)
Bromine (Br)
Sodium (Na)
The electron affinities of beryllium and magnesium are both positive. The primary reason for this is:
Their large atomic radii.
Their low ionization energies.
Their filled s subshells lead to stable electronic configurations.
Their weak effective nuclear charge.
Which of the following factors LEAST influences the electron affinity of an element?
Effective nuclear charge
Atomic radius
Interelectronic repulsions
Number of neutrons in the nucleus
Explain the seemingly contradictory trend in electron affinity between sulfur and chlorine. Chlorine has a more negative electron affinity than sulfur, despite being larger. Why?
Sulfur's larger atomic radius makes it easier to add an electron.
Chlorine's higher effective nuclear charge outweighs the effect of its larger size, leading to a stronger attraction for the added electron.
Interelectronic repulsion is greater in chlorine than in sulfur.
Sulfur's half-filled p subshell makes it more stable.
Which of the following factors does NOT significantly influence the electron affinity of an element?
Number of neutrons in the nucleus
Effective nuclear charge
Atomic size
Electronic configuration
The electron affinity of chlorine is higher than that of fluorine. This is primarily due to:
Larger size of chlorine
Smaller size and increased electron-electron repulsion in fluorine
Higher electronegativity of fluorine
Lower ionization energy of chlorine
Which of the following generally has the most negative electron affinity?
Alkali metals
Alkaline earth metals
Noble gases
Halogens
