Questions and Answers
What is the polarity of CO2?
What is the shape of SO2?
What type of bond polarity exists in NH3?
Polar
What is the polarity of NOBr?
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Is NOCl polar or non-polar?
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What is the polarity of CH4?
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What is the shape of H2O?
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What is the polarity of POCl3?
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Is CCl4 a polar or non-polar molecule?
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What is the shape of SO3?
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What is the polarity of BF3?
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What is the polarity of COCl2?
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Is SiH4 polar or non-polar?
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What is the shape of H2S?
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Is CH2Cl2 a polar or non-polar molecule?
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Is CH3Br polar or non-polar?
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Study Notes
Carbon Dioxide (CO2)
- CO2 has polar C-O bonds due to differing electronegativities but is overall non-polar.
- The linear molecular shape allows bond dipoles to cancel each other out.
Sulfur Dioxide (SO2)
- SO2 has polar S-O bonds; the molecule is overall polar due to its bent shape.
- There are 3 electron repulsions, with a lone pair on sulfur affecting the bond arrangement.
Ammonia (NH3)
- NH3 has a trigonal pyramidal shape due to one lone pair, despite being tetrahedral initially.
- Contains polar N-H bonds resulting in an overall polar molecule due to asymmetrical charge distribution.
Nitrosyl Bromide (NOBr)
- NOBr adopts a bent shape with one lone pair, leading to asymmetrical charge distribution.
- The molecule is overall polar, as dipoles do not cancel.
Nitrosyl Chloride (NOCl)
- NOCl also has a bent shape due to a lone pair, resulting in a polar molecule.
- Asymmetrical charge distribution causes the cancellation of dipole effects.
Methane (CH4)
- CH4 displays a tetrahedral shape and symmetric charge distribution; therefore, it is non-polar.
- The bond dipoles cancel out due to symmetrical arrangement.
Water (H2O)
- H2O has a bent shape with two lone pairs, leading to overall polarity.
- The asymmetrical charge distribution results in a slightly negative end and a slightly positive end.
Phosphoryl Chloride (POCl3)
- POCl3 features a tetrahedral geometry, exhibiting an overall polar nature.
- The molecular structure has asymmetrical charge distribution.
Carbon Tetrachloride (CCl4)
- CCl4 is tetrahedral with symmetric charge distribution, making it a non-polar molecule.
- Dipoles from C-Cl bonds cancel out due to symmetrical arrangement.
Sulfur Trioxide (SO3)
- SO3 has a trigonal planar shape with symmetrical charge distribution, resulting in non-polarity.
- The uniform arrangement allows for dipole cancellation.
Boron Trifluoride (BF3)
- BF3 features a trigonal planar shape and symmetric charge distribution, making it non-polar.
- The arrangement results in cancellation of dipole moments.
Carbonyl Dichloride (COCl2)
- COCl2 has a trigonal planar shape with asymmetrical charge distribution leading to it being polar.
- Polar bonds arise from differences in electronegativity between C, Cl, and O.
Silane (SiH4)
- SiH4 has a tetrahedral shape with polar Si-H bonds, which are symmetrically arranged, rendering the molecule non-polar.
- The symmetry allows the dipoles to cancel out.
Hydrogen Sulfide (H2S)
- H2S exhibits a bent shape due to two lone pairs, resulting in overall polarity.
- Polar S-H bonds lead to an asymmetrical charge distribution within the molecule.
Dichloromethane (CH2Cl2)
- CH2Cl2 has a tetrahedral shape with polar C-Cl bonds; however, the charge distribution is asymmetric and gives a polar character to the molecule.
- The different polarities of C-H and C-Cl bonds result in cancellation issues.
Bromoform (CH3Br)
- CH3Br is tetrahedral and features polar bonds where C-Br is more polar than C-H.
- As dipoles do not cancel out, the molecule is overall polar due to its asymmetrical arrangement.
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Description
This quiz focuses on the concepts of atomic bonding and molecular polarity as part of the NCEA Level 2 curriculum. It covers key molecules like CO2 and SO2, explaining their bond characteristics and overall polarity. Ideal for students preparing for their exams in chemistry.
