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Questions and Answers
The angle for methane (CH4) is exactly 109.5°.
True
In the VSEPR theory, bonding pairs of electrons repel more strongly than lone pairs.
False
The actual bond angle in the sulfite ion (SO32–) is 109.5°.
False
The ferrous hexaaqua ion is represented as Fe(H2O)62+.
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In VSEPR theory, a multiple bond is treated as if it were a single bond.
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The bond angle for water (H2O) is greater than that of ammonia (NH3).
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Energetically, it is more favorable for lone pairs to be as close to each other as possible.
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The ion FeSO4 contains ferrous ions (Fe2+).
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The bond angle in the sulfite ion is the same as that in methane.
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Lone pair repulsions have the least effect on molecular shape in VSEPR theory.
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Sulfur hexafluoride is used to enhance the echogenicity of blood in ultrasound imaging.
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EDTA is a metal ion that can form octahedral complexes.
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The molecular shape of a complex formed by a divalent transition metal ion with EDTA is tetrahedral.
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When FeSO4 dissolves in water, Fe2+ ions do not interact with the water molecules.
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Echogenicity refers to the ability of tissues to reflect ultrasound waves.
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The molecular shape of ammonia (NH3) is trigonal planar.
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EDTA can chelate both monovalent and divalent transition metal ions.
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The molecular shape of water (H2O) is linear.
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Cisplatin has a square planar molecular shape.
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The octahedral molecular shape denotes six identical groups surrounding a central atom.
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Sulfur hexafluoride (SF6) is an example of a tetrahedral molecule.
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The main application of sulfur hexafluoride is its use in dry eye lubricants.
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Disodium edetate is another name for ethylenediaminetetraacetic acid.
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In sulfur hexafluoride (SF6), the bond angle between the fluorine atoms is approximately 90 degrees.
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There are four bonding pairs and two lone pairs in the molecular shape of cisplatin.
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A higher signal to noise ratio in echocardiography can be achieved by reducing the echogenicity of the blood.
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Ammonia (NH3) contains a double bond between nitrogen and hydrogen.
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The molecular structure of water leads to its high boiling point compared to other similar-sized molecules.
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The density of sulfur hexafluoride (SF6) is lower than that of air.
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The presence of lone pairs of electrons affects the molecular shape of certain compounds.
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Study Notes
Molecular Shapes
- AB3E: Trigonal Pyramidal - Example: NH3 (ammonia)
- AB2E2: Bent, Angular, V-shaped - Example: H2O (water)
- AB4E2: Square Planar - Example: cis-PtCl2(NH3)2 (cisplatin)
- AB6: Octahedral - Example: SF6 (sulfur hexafluoride)
VSEPR Theory
- The central atom (A) is surrounded by valence electron pairs
- Bond pairs (B) and lone pairs (E) are calculated
- Lone/lone pair repulsions are greater than lone/bond pair repulsions, which are greater than bond/bond pair repulsions
- Lone pairs are positioned as far away from each other as possible
- Examples: SO32- (sulfite) = 106° angle, H2O = 104.5° angle, NH3 = 107° angle
Multiple Bonds
- Multiple bonds are treated as single bonds in VSEPR theory
- This simplifies calculations and avoids issues associated with resonance structures
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Description
Explore the fascinating world of molecular shapes through VSEPR theory. This quiz covers various molecular geometries such as trigonal pyramidal, bent, square planar, and octahedral forms. Test your understanding of electron pair repulsions and the impact of multiple bonds on molecular geometry.
