A level Chem 1.3 Bonding

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Which species has a square planar shape? (1) 

A NH₄⁺

B SF₄

C XeF₄

D PCl₄⁺

C XeF₄ (1) 

What formula can you use to quickly determine the number of lone pairs on the central atom? (1)

Number of lone pairs on central atom=0.5x​[Valence electrons on central atom-(Number of bonded atoms)+Charge] (1)

In which molecule are all the atoms in the same plane? (1)

A CH₃CHO

B CH₃NH₂

C C₆H₅Cl

D C₆H₅CH₃

C C₆H₅Cl (1)

Sodium fluoride contains sodium ions (Na⁺ ) and fluoride ions (F^– ). Na⁺ and F^– have the same electron configuration. Explain why a fluoride ion is larger than a sodium ion (2) 

Fluoride ion has (two) fewer protons/lower nuclear charge (1) 

Weaker attraction between nucleus and (outer) electrons (1) 

The ion H₂F⁺ is formed when hydrogen fluoride gains a proton as shown in the equation HF⁺ H⁺ → H₂F⁺

Name the type of bond formed when HF reacts with H⁺

Explain how this bond is formed. (2)

Type of Bond: Coordinate bond / dative (covalent) bond (1)

Explanation: A (lone) pair of electrons is donated from F (1)

hydrogen ion (H⁺) has no electrons