Ionic and Metallic Bonding Quiz
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Questions and Answers

What is the definition of ionic bonding?

Electrostatic force of attraction between oppositely charged ions formed by electron transfer.

What factors affect the strength of ionic bonding?

The size of the ions and the magnitude of their charges.

Ionic compounds have high melting points.

True

Ionic compounds are generally good conductors of electricity in solid state.

<p>False</p> Signup and view all the answers

Explain why positive ions are smaller than their corresponding neutral atoms.

<p>Positive ions have one less electron shell than their parent atoms, resulting in a smaller ionic radius. This is because the electrostatic attraction between the nucleus and the remaining electrons is stronger in the absence of an outer electron shell.</p> Signup and view all the answers

Explain why negative ions are larger than their corresponding neutral atoms.

<p>Negative ions have more electrons than their corresponding atoms, resulting in a larger ionic radius. This is because the electrostatic attraction between the nucleus and the increased number of electrons is weaker, leading to a larger ionic radius.</p> Signup and view all the answers

What is the effect of the size of the ionic radii on the strength of ionic bonding?

<p>Smaller ions have stronger ionic bonds because the electrostatic forces between them are more concentrated.</p> Signup and view all the answers

What is metallic bonding?

<p>Electrostatic force of attraction between positive metal ions and delocalized electrons.</p> Signup and view all the answers

What are the three main factors that affect the strength of metallic bonding?

<p>Number of protons, number of delocalised electrons per atom, and size of the ion.</p> Signup and view all the answers

Metals are good conductors of electricity.

<p>True</p> Signup and view all the answers

Metals are malleable and ductile.

<p>True</p> Signup and view all the answers

What is covalent bonding?

<p>Strong electrostatic attraction between the negative shared pair of electrons and the positive nuclei of the bonded atoms.</p> Signup and view all the answers

What are the two types of covalent bonding?

<p>Simple covalent bonding and dative covalent bonding.</p> Signup and view all the answers

What type of forces hold simple molecules together in a solid or liquid state?

<p>Intermolecular forces, such as van der Waals forces, permanent dipoles, and hydrogen bonds.</p> Signup and view all the answers

Covalent compounds generally have low boiling and melting points.

<p>True</p> Signup and view all the answers

What is a dative covalent bond?

<p>A covalent bond in which one atom provides both electrons to the shared pair.</p> Signup and view all the answers

What is the difference between a simple covalent bond and a dative covalent bond?

<p>In a simple covalent bond, each atom contributes one electron to the shared pair, while in a dative covalent bond, one atom contributes both electrons to the shared pair.</p> Signup and view all the answers

What is the shape of a carbon atom in a diamond?

<p>Tetrahedral.</p> Signup and view all the answers

Diamond is a very hard substance.

<p>True</p> Signup and view all the answers

What is the structure of graphite?

<p>Planar arrangement of carbon atoms in layers.</p> Signup and view all the answers

Graphite can conduct electricity.

<p>True</p> Signup and view all the answers

What is activation energy?

<p>The minimum energy which particles need to collide to start a reaction.</p> Signup and view all the answers

What is the Maxwell Boltzmann distribution?

<p>A statistical distribution that describes the distribution of energies among the particles in a system.</p> Signup and view all the answers

The Maxwell Boltzmann distribution shows that the total area under the curve should remain constant because the total number of particles is constant.

<p>True</p> Signup and view all the answers

What is rate of reaction?

<p>Change in concentration of a substance in unit time.</p> Signup and view all the answers

Rate of reaction is an approximation for the rate of reaction as it does not include concentration.

<p>True</p> Signup and view all the answers

What are van der Waals forces?

<p>Transient, induced dipole-dipole interactions between molecules caused by temporary fluctuations in electron density.</p> Signup and view all the answers

What is the main factor affecting the size of van der Waals forces?

<p>The number of electrons in the molecule.</p> Signup and view all the answers

Van der Waals forces occur between all molecular substances and noble gases.

<p>True</p> Signup and view all the answers

What is hydrogen bonding?

<p>A type of intermolecular force that occurs between molecules containing hydrogen atoms bonded to highly electronegative atoms like oxygen, fluorine, or nitrogen.</p> Signup and view all the answers

Hydrogen bonding is a type of dipole-dipole interaction.

<p>True</p> Signup and view all the answers

What are permanent dipole-dipole forces?

<p>Electrostatic attractions between molecules with permanent dipoles, arising from unequal sharing of electrons in polar covalent bonds.</p> Signup and view all the answers

Permanent dipoles can occur in molecules with only non-polar covalent bonds.

<p>False</p> Signup and view all the answers

What does electronegativity refer to?

<p>The relative tendency of an atom in a covalent bond to attract electrons to itself.</p> Signup and view all the answers

Electronegativity generally increases down a group in the periodic table.

<p>False</p> Signup and view all the answers

What is a non-polar molecule?

<p>A molecule with no net dipole moment, typically due to symmetrical shape and/or non-polar covalent bonds.</p> Signup and view all the answers

Non-polar molecules generally have low boiling and melting points.

<p>True</p> Signup and view all the answers

Study Notes

Ionic Bonding

  • Formed by electrostatic attraction between oppositely charged ions formed by electron transfer.
  • Giant lattices of ions have stronger structures and higher melting points when the ions are smaller and/or have higher charges.
  • Positive ions are smaller than the corresponding neutral atom because they have lost an electron shell, leading to a greater ratio of protons to electrons, hence a stronger force on remaining electrons.
  • Negative ions are larger than the corresponding neutral atom because they have gained more electrons than protons.
  • Ions do not conduct electricity in the solid state but do so when molten.

Metallic Bonding

  • Electrostatic force of attraction between positive metal ions and delocalised electrons.
  • Metals are shiny and malleable because positive ions in a lattice are identical and layers of ions can slide easily.
  • Delocalised electrons can move, preventing fragmentation and allowing good conductivity.
  • The strength of metallic bonding depends on the number of protons, the number of delocalised electrons, and the size of the ions.

Covalent Bonding

  • Strong electrostatic attraction between the negative shared pair of electrons and the positive nuclei of the bonded atoms.
  • Covalent compounds can form molecules.
  • Low boiling and melting points due to similar electronegativity of the constituent elements.
  • Generally poorly soluble in water as a gas or liquid.
  • Dative covalent bonds are a type of covalent bond where both electrons in the shared pair originate from the same atom.

Giant Covalent Structures

  • High boiling and melting points due to strong covalent bonds.
  • Macromolecular structure.
  • Localisation of electrons in the bonds prevents electrical conductivity.
  • Generally insoluble in water, solids.
  • Examples: Diamond (tetrahedral arrangement, 4 covalent bonds per atom) and graphite (planar arrangement, 3 covalent bonds per atom, with delocalised electrons, which allows conductivity).

Maxwell-Boltzmann Distribution

  • The distribution of energies among particles in a sample of matter.
  • The mean energy of the particles is not at the peak of the curve.
  • The area under the curve represents the total number of particles.
  • Most molecules have energies between the two extremes but the distribution is not symmetrical.
  • Energy (Eₐ) is required for particles to successfully collide and start a reaction.

Rate of Reaction

  • Change in concentration of a substance in unit time.
  • An approximation of the rate of reaction as it doesn't include concentration.

Van der Waals' Forces

  • Transient, induced dipole-dipole interactions caused by fluctuating electron density in molecules.
  • The number of electrons in a molecule affects the strength of Van der Waals' forces.
  • Long chain alkanes have a higher surface area for intermolecular contact which lead to stronger Van der Waals' than branched alkanes.
  • Occur between all molecular substances and noble gases.
  • Not in ionic substances.

Hydrogen Bonding

  • Compounds with hydrogen atoms attached to highly electronegative atoms (N, O, F) with lone pairs of electrons.
  • Large electronegativity differences create a strong dipole between the hydrogen atom and the more electronegative atom.
  • Hydrogen bonding is stronger than other intermolecular forces, impacting boiling and melting points.

Permanent Dipole-Dipole Forces

  • Covalent bonds with elements of different electronegativity creating a charge separation in the bond resulting in permanent dipoles.
  • The molecules interact because the positive end of one molecule and the negative end of the other molecule attract.
  • Dipoles in symmetrical shapes cancel making the molecule non-polar, while asymmetrical ones are polar.

Electronegativity

  • Relative tendency of an atom in a covalent bond to attract electrons towards itself.
  • Electronegativity Trends: Increases across a period, decreases down a group.
  • F, O, N, and Cl are the most electronegative elements.
  • Affected by the distance between the nucleus and the outer electrons, the shielding of inner electron shells and the number of protons in the nucleus. Atomic radius also influences electronegativity.

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Description

Test your understanding of ionic and metallic bonding concepts. This quiz covers the properties, formation, and characteristics of ionic and metallic bonds. Perfect for chemistry students looking to reinforce their knowledge on these fundamental topics.

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