The second period elements (Li to F), highlight that these elements exhibit unique chemical behaviors compared to their heavier counterparts in the same groups, due to these factors EXCEPT

• strong π-bond formation

• smaller size

• lack of readily available d-orbitals

• smaller electronegativity

These are elements in the second period of the periodic table EXCEPT

• Lithium

• Nitrogen

• Calcium

• Carbon

Lithium chloride (LiCl), despite being an ionic compound, exhibits a greater solubility in polar organic solvents compared to water. Why this occurs?

This occurs due to the ​SMALL size of the element, which results in a​ ........................... charge density of its cation. Consequently, the cation exhibits​ polarizing power, leading to a significant great covalent character in its compound.

• similar

• low

• decrease

• high

When two oppositely charged ions approach each other, the attraction between the positive charge of cation and the negative charge of anion and also the simultaneous repulsion between both of their nuclei and between their electrons results in the ____________ of the electron charge cloud of the anion.

• attraction

• polarization

• repulsion

• bonding

Why fluorine has a lower electron affinity than chlorine?

Fluorine is significantly ​ SMALLER than chlorine, meaning its electrons are .......................... ​ to the nucleus. When an electron is added to fluorine, it must enter the already crowded 2p orbitals, leading to .............................. ​ electron-electron repulsion. Therefore, the energy released when an electron is added is WEAKER​ than in chlorine. 

• far, weaker

• closer, greater

• far, greater

• close, weaker

Why fluorine has lower bond energy compared to chlorine?

Fluorine atom are significantly​ SMALLER than chlorine atom, meaning their electrons are more concentrated in a smaller space. This high electron density within the small fluorine atoms leads to ​............................. repulsions between the non-bonding (lone pair) electrons on adjacent fluorine atoms. The strong interelectronic repulsions WEAKEN the F-F bond, making it easier to break (lower bond energy) compared to the Cl-Cl bond.

• no

• strong

• weak

• enough

Diagonal relationships occur due to similarities in size and charge between elements that are diagonally adjacent in the periodic table. The following diagonal relationship pairs are correct EXCEPT

• Li and Mg

• Be and Al

• B and Si

• Na and Mg

Inert pair effect is the tendency of the two outermost s-electrons in heavier ................................. elements to remain unshared in their compounds, leading to a preference for lower oxidation states than predicted by their group number

• f-block

• d-block

• s-block

• p-block

Which ionic compound is stable due to the inert pair effect?

• GeO

• PbO₂

• PbCl₂

• SnCl₄

Be and Al have a diagonal relationship because of the following EXCEPT

• 1. Both metals have a high electropositive potential

• • Both elements have nearly comparable electronegativity (Be = 1.5, Al = 1.5)

• Both elements have the same covalent radius

• Be²⁺ (0.033) and Al³⁺ (0.044) ions have about the same cationic charge-to-size ratio