Welcome to the Quiz!
This quiz contains 12 questions from a mix of 1 subtopics.
What is the general formula for alkenes?
CnH2n
CnH2n-2
CnHn
CnH2n+2
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Which of the following statements about alkenes is true?
they contain only single carbon-carbon bonds
they are saturated hydrocarbons
they have at least one carbon-carbon double bond
they are less reactive than alkanes
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How many hydrogen atoms are present in a cyclic alkene with 6 carbon atoms?
8
10
12
14
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How is the electron density distributed in a pi (π) bond?
there is no electron density in a pi bond
directly between the nuclei
evenly around the bond
above and below the bond axis
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What is the approximate bond angle around each carbon atom in a carbon-carbon double bond?
109.5°
90°
180°
120°
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Which of the following describes the geometry of carbon atoms in a carbon-carbon double bond?
trigonal planar
tetrahedral
octahedral
linear
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Alkenes can readily participate in which type of reaction due to the presence of the pi (π) bond?
substitution reactions
addition reactions
redox reactions
elimination reactions
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Which of the following statements comparing alkenes and alkanes is true?
alkenes are more reactive than alkanes
alkenes and alkanes have similar reactivity
alkanes are more reactive than alkenes
reactivity cannot be compared between alkenes and alkanes
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Which of the following statements about sigma (σ) bonds is true?
they are only found in molecules with sp2 hybridised carbon atoms
they are formed by head-on overlap of atomic orbitals
they are weaker than pi (π) bonds
they involve sideways overlap of atomic orbitals
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Which of the following statements about pi (π) bonds is true?
they are formed by sideways overlap of atomic orbitals
they involve head-on overlap of atomic orbitals
they are only found in molecules with sp hybridised carbon atoms
they are stronger than sigma (σ) bonds
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Which of the following describes the shape of organic molecules containing carbon-carbon double bonds like ethene (H2C=CH2)?
trigonal planar
tetrahedral
linear
octahedral
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What makes the pi (π) bond electrons highly accessible for reactions?
low electron density
linear shape
high bond enthalpy
high electron density
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