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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