Chemistry Chapter 5: Ionic and Covalent Bonds
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Questions and Answers

What type of bond is formed between calcium and fluorine in calcium fluoride?

  • Hydrogen bonding
  • Covalent bonding
  • Metallic bonding
  • Ionic bonding (correct)

Which factor contributes to the greater strength of ionic bonding in sodium fluoride compared to potassium fluoride?

  • The greater electronegativity of potassium
  • The higher charge of sodium ions
  • The larger atomic radius of sodium
  • The smaller size of sodium ions (correct)

Why is the ionic bonding strength in calcium oxide approximately four times greater than that in potassium fluoride?

  • The molecular mass of potassium fluoride is greater than calcium oxide
  • Calcium ions have a smaller ionic radius than potassium ions
  • Calcium has a higher charge than potassium (correct)
  • Oxygen ions are larger than fluoride ions

What does the term 'polarisation of ions' refer to?

<p>The distortion of the electron cloud of an anion by a cation (D)</p> Signup and view all the answers

Which statement about ionic radii is NOT true?

<p>Ionic radii are always larger for cations than for anions. (B)</p> Signup and view all the answers

What is the electronic configuration of a chlorine atom?

<p>1s2 2s2 2p6 3s2 3px2 3py2 3pz1 (A)</p> Signup and view all the answers

What type of bond is primarily formed when two chlorine atoms bond together?

<p>σ bond (D)</p> Signup and view all the answers

In what circumstance can a π bond form after the creation of a σ bond?

<p>With sufficient orbital overlap (C)</p> Signup and view all the answers

What describes the bonding in a chlorine molecule according to one theory?

<p>The overlap of two sp3 hybrid orbitals (B)</p> Signup and view all the answers

What is a characteristic of a π bond formed between atoms?

<p>It creates regions of high electron density above and below the molecule (D)</p> Signup and view all the answers

What type of bond does oxygen (O2) exhibit in its dot-and-cross diagram?

<p>Double bond (B)</p> Signup and view all the answers

In the displayed formula of carbon dioxide (CO2), which represents the bonding structure?

<p>O=C=O (A)</p> Signup and view all the answers

What distinguishes a triple bond in the dot-and-cross diagram of nitrogen (N2)?

<p>It has three pairs of electrons shared. (D)</p> Signup and view all the answers

Which of the following correctly describes the displayed formula of ammonia (NH3)?

<p>H—N—H (B)</p> Signup and view all the answers

Which molecule's dot-and-cross diagram does NOT need to display lone pairs of electrons?

<p>Oxygen (O2) (B)</p> Signup and view all the answers

Which of the following molecules contains a double bond?

<p>Oxygen (O2) (D)</p> Signup and view all the answers

What is the correct number of hydrogen atoms in the displayed formula of ammonia (NH3)?

<p>3 (C)</p> Signup and view all the answers

Which option correctly matches the molecule with its bonding type based on the dot-and-cross diagram?

<p>Oxygen - Double bond (A)</p> Signup and view all the answers

What type of bond is formed between the chlorine atom of the second molecule and the aluminium atom of the first molecule?

<p>Dative covalent bond (B)</p> Signup and view all the answers

Which of the following best describes a dative covalent bond?

<p>A bond formed when an empty orbital overlaps with a lone pair of electrons from another atom (A)</p> Signup and view all the answers

In the formula for the aluminium dimer, which is the correct representation of the bonding?

<p>One dative bond and one single bond (C)</p> Signup and view all the answers

Which formula correctly represents the AlCl4− ion?

<p>AlCl3 + Cl− (A)</p> Signup and view all the answers

How many covalent and dative bonds are present in a carbon monoxide (CO) molecule?

<p>Two covalent bonds and one dative bond (D)</p> Signup and view all the answers

Which compound features a dative covalent bond in its Lewis structure?

<p>Ammonium ion (NH4+) (C)</p> Signup and view all the answers

What is the geometry of the molecule formed by aluminum dichloride (BeCl2) if each double bond is treated as an electron pair?

<p>Linear (A)</p> Signup and view all the answers

Flashcards

Ionic bonding

The electrostatic attraction between oppositely charged ions.

Ionic radius

Size of an ion, dependent on surrounding ions and measurement method.

Coordination number

Number of oppositely charged ions touching an ion.

Polarisation

Change in shape of ion due to surrounding ions.

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Strength of ionic bonding

Force of attraction between oppositely charged ions.

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Covalent Bonding in Chlorine

Two chlorine atoms share electrons to form a covalent bond, using their p orbitals.

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σ Bond Formation

A σ bond is formed when atomic orbitals overlap directly head-on.

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Ï€ Bond Formation

A π bond is formed when p orbitals overlap sideways, creating electron density both above and below the molecule.

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Orbital Overlap

The overlapping of atomic orbitals between atoms for sharing electrons, creating a covalent bond.

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Ethene Molecule and π Bond

Ethene molecule forms a π bond by sideways overlap of p orbitals, creating electron density above and below the molecule.

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Dot-and-cross diagram for O2

A diagram showing the arrangement of valence electrons in an oxygen molecule (O2).

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Dot-and-cross diagram for N2

A diagram illustrating the arrangement of valence electrons within a nitrogen molecule (N2).

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Dot-and-cross diagram for CO2

A representation of valence electrons in the carbon dioxide molecule (CO2).

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Displayed formula of H2O

The chemical formula showing the arrangement of atoms within a water molecule.

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Displayed formula of NH3

The chemical formula representing the structure of an ammonia molecule.

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Displayed formula of O2

The chemical formula illustrating the oxygen molecule structure.

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Displayed formula of N2

The chemical formula representing the nitrogen molecule structure.

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Displayed formula of CO2

The chemical formula representing the carbon dioxide molecule structure.

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Dative covalent bond

A type of covalent bond where one atom provides both electrons in the shared pair. This happens when one atom has a lone pair of electrons and the other has an empty orbital.

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What is a lone pair?

A pair of electrons that are not involved in bonding, but remain localized on an atom.

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What is an empty orbital?

An orbital that doesn't have any electrons in it, ready to accept electrons.

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How to identify a dative covalent bond in a dot-and-cross diagram?

Look for an atom with a lone pair sharing its electrons with an atom that has an empty orbital.

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Draw a dot-and-cross diagram for NH3

Nitrogen (N) has 5 valence electrons, Hydrogen (H) has 1 valence electron. Draw a dot-and-cross diagram illustrating the three covalent bonds in NH3 and the lone pair on the nitrogen.

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Draw a dot-and-cross diagram for BF3

Boron (B) has 3 valence electrons and Fluorine (F) has 7 valence electrons. Draw a dot-and-cross diagram showing the 3 single covalent bonds in BF3.

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Draw a dot-and-cross diagram for NH3 and BF3 interacting

Combine the diagrams for NH3 and BF3. Draw a dative covalent bond forming between the nitrogen of NH3 and the boron of BF3. Show the nitrogen atom donating the electrons to boron.

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Study Notes

Bonding and Structure

  • Atoms combine in various ways, forming different types of bonds, leading to diverse materials with unique properties
  • Understanding bonding and structure are key to developing new materials, such as electronics and outdoor clothing
  • Knowledge of molecular shapes is crucial for medicine design and understanding biological processes

Ionic Bonding

  • Formed by the loss and gain of electrons, creating oppositely charged ions
  • Ions are held together by strong electrostatic forces, resulting in a giant lattice structure
  • Ionic compounds generally have high melting points because significant energy is needed to overcome the strong attractions between ions

Covalent Bonding

  • Formed by the sharing of electron pairs between atoms
  • Strength of covalent bonds depends on the number of shared electron pairs (single, double, or triple bonds)
  • Bond lengths and strengths are linked: shorter bonds are generally stronger

Metallic Bonding

  • Metal ions are arranged in a regular lattice, surrounded by a 'sea' of delocalised electrons
  • Delocalised electrons allow for excellent electrical and thermal conductivity, high malleability, ductility
  • High melting temperatures are due to strong electrostatic attractions between fixed cations and the delocalised electrons.

Solid Lattices

  • Regular arrangements of atoms or ions (metals, ionic compounds, or covalent compounds) extending throughout a large structure
  • Properties of solids arise from strength and arrangement of forces between atoms/ions
  • Different types of solids (metallic, ionic, covalent, molecular) exhibit diverse characteristics, including conductivity, melting point, and hardness.

Maths Skills

  • Use angles and shapes in regular 2D and 3D structures
  • Visualise and represent 2D and 3D forms using 2D representations of 3D objects
  • Understand 2D and 3D symmetry

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Topic 3 Bonding Textbook PDF

Description

Test your understanding of bonding concepts in chemistry with this quiz focusing on ionic and covalent bonds, particularly those involving calcium, fluorine, and chlorine. Explore topics like ionic radii, bond strength, and electronic configurations. Challenge yourself to understand the nuances of atomic interactions!

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