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M.Sc Chemistry Alkenes — practice questions — page 2

Explore 57 free Alkenes questions in M.Sc Chemistry Chemistry. Open each question or exercise to read its content, reference answers and available explanation.

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Alkenes questions and exercises with answers

Showing questions 31–57 of 57.

Assertion and reason: filling orbitalsRead the answer and worked solution →True or false: shells and subshellsRead the answer and worked solution →Complete the two filling rulesRead the answer and worked solution →Match each scientist to their contributionRead the answer and worked solution →Ionic or covalent?Read the answer and worked solution →Complete the driver of bond formationRead the answer and worked solution →Single, double and triple bondsRead the answer and worked solution →True or false: Lewis structuresRead the answer and worked solution →Complete the definition of resonanceRead the answer and worked solution →Tap every bond parameter the chapter namesRead the answer and worked solution →True or false: ionic solidsRead the answer and worked solution →Assertion and reasonRead the answer and worked solution →Two are true, one is notRead the answer and worked solution →Three of these are wrong. Find the one that holds.Read the answer and worked solution →Bonded pair or lone pair?Read the answer and worked solution →Flip and pair: term with meaningRead the answer and worked solution →Spot the one that does not belongRead the answer and worked solution →Order the reasoning: why resonance is neededRead the answer and worked solution →Reading the definitions backRead the answer and worked solution →True or false: what bond parameters affectRead the answer and worked solution →Bond parameters in useRead the answer and worked solution →Which parameter answers this?Read the answer and worked solution →True or false: resonanceRead the answer and worked solution →Order the steps: draw a Lewis structureRead the answer and worked solution →Spot the one that does not belongRead the answer and worked solution →Assertion and reason: structureRead the answer and worked solution →Flip and pair: parameter with what it measuresRead the answer and worked solution →

Worked practice questions

Assertion and reason: filling orbitals

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Questions
  1. Reason
    Pauli forbids two electrons in an atom sharing all four quantum numbers.
    Verdict
    Both are true; the reason explains the assertion.
    Assertion
    An orbital holds at most two electrons.
  2. Reason
    Hund's rule of maximum multiplicity requires single occupancy first.
    Verdict
    Both are true; the reason explains the assertion.
    Assertion
    Electrons spread out before pairing up in a subshell.
  3. Reason
    Rutherford discovered the nucleus by alpha-particle scattering.
    Verdict
    Both are true; the reason does not explain the assertion.
    Assertion
    Orbitals fill in order of increasing energy.
The last round pairs two true halves that do not explain one another. Source: syllabus Chemistry Part I, Ch 2 Structure of Atom.

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True or false: shells and subshells

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Questions
  1. Statement is true
    Yes
    Statement
    Electron distribution is divided into shells.
  2. Statement is true
    Yes
    Statement
    Shells consist of one or more subshells.
  3. Statement is true
    Yes
    Statement
    Subshells are composed of one or more orbitals.
  4. Statement is true
    No
    Statement
    Orbitals are composed of shells.
  5. Statement is true
    Yes
    Statement
    Electrons occupy orbitals.
How the quantum mechanical model organises the electrons. Source: syllabus Chemistry Part I, Ch 2 Structure of Atom.

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Complete the two filling rules

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Missing parts
  1. Answer
    Pauli exclusion
    Choices
    1. Pauli exclusion
    2. Heisenberg
    3. Aufbau
  2. Answer
    Hund's
    Choices
    1. Hund's
    2. Bohr's
    3. Dalton's
  3. Answer
    singly
    Choices
    1. singly
    2. doubly
    3. never
Complete the statement
The {0} principle says no two electrons in an atom may share the same set of four quantum numbers. {1} rule says pairing does not begin until every orbital of the subshell is {2} occupied.
Both rules together produce the electronic structure of the atom. Source: syllabus Chemistry Part I, Ch 2 Structure of Atom.

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