Ionic Bonding and Compounds Quiz
55 Questions
0 Views

Choose a study mode

Play Quiz
Study Flashcards
Spaced Repetition
Chat to lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

What is ionic bonding?

The force that holds appropriately charged particles together within a compound.

What are valence electrons?

Electrons in the outermost shell

Which of these elements forms cations?

  • Carbon
  • Sodium (correct)
  • Oxygen
  • Chlorine

    • An endothermic process releases energy.

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

    An exothermic process absorbs energy.

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

    What is another name for an ionic compound?

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

    What does crystal lattice refer to?

    <p>The crystalline structure of ionic compounds.</p> Signup and view all the answers

    What is lattice energy?

    <p>The energy required to separate the ions which compose an ionic compound.</p> Signup and view all the answers

    The formation of ionic compounds is an endothermic process.

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

    Which of the following are characteristics of ionic compounds? (Select all that apply)

    <p>Nonconductors as solids</p> Signup and view all the answers

    How do you write an anion reaction equation?

    <p>ELEMENT + e- -&gt; ELEMENT-1 + electron affinity</p> Signup and view all the answers

    What is electron affinity?

    <p>The energy released when an electron attaches to an atom in a gaseous state.</p> Signup and view all the answers

    What is ionization energy?

    <p>The energy required to remove an electron from an atom.</p> Signup and view all the answers

    The smaller an atomic radii, the weaker the bond formed.

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

    The higher the total oxidation charge is for an atom, the weaker the bond formed.

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

    The stronger the bond, the more positive the lattice energy is for a compound.

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

    What is oxidation charge?

    <p>The charge of a monatomic ion (one atom ion).</p> Signup and view all the answers

    Why do brittle ionic solids break apart?

    <p>Their ions line up.</p> Signup and view all the answers

    What is a pseudo noble gas configuration?

    <p>Relatively stable electron arrangements</p> Signup and view all the answers

    Which of these elements have pseudo noble gas configurations?

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

    What configuration do atoms achieve when they bond?

    <p>Noble Gas</p> Signup and view all the answers

    How do covalent bonds form?

    <p>Sharing of electrons</p> Signup and view all the answers

    Which of the following are diatomic elements?

    <p>F2</p> Signup and view all the answers

    How many atoms are shared between a single bond? Double? Triple?

    <p>2, 4, 6</p> Signup and view all the answers

    Where is a sigma bond positioned in a bond between two atoms?

    <p>Directly between the two atoms</p> Signup and view all the answers

    Why is a sigma bond in the middle of a bond?

    <p>The electron orbitals of the two elements overlap, so electrons are completely centred.</p> Signup and view all the answers

    Where is a pi bond located?

    <p>Above and below a bond</p> Signup and view all the answers

    When can pi bonds occur?

    <p>When there is either 1 sigma bond and two pi bonds or one sigma bond and one pi bond.</p> Signup and view all the answers

    What is a Lewis structure?

    <p>A way of showing the structural formula for molecules.</p> Signup and view all the answers

    What is resonance?

    <p>When a Lewis Structure can be written multiple ways. It occurs when a molecule has one double bond and one or more single bonds of oxygen.</p> Signup and view all the answers

    What is hybridization?

    <p>When atomic orbitals are mixed to form new, identical hybrid orbitals.</p> Signup and view all the answers

    What is the difference between electronegativity and electron affinity?

    <p>Electronegativity indicates the ability to attract electrons while electron affinity is the tendency of an atom to accept an electron.</p> Signup and view all the answers

    Which of the following are exceptions to the octet rule?

    <p>ClO2</p> Signup and view all the answers

    Only elements in the second and third periods can have expanded octets.

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

    What are Van der Waals forces?

    <p>Intermolecular forces. (Dispersion, dipole-dipole, and hydrogen bonding.)</p> Signup and view all the answers

    What is dispersion within van der Waals forces?

    <p>The weak intermolecular force between nonpolar molecules. (Sometimes called London Dispersion Force)</p> Signup and view all the answers

    What is dipole-dipole within van der Waals forces?

    <p>The stronger intermolecular force between polar molecules.</p> Signup and view all the answers

    Where does the dispersion force occur?

    <p>Between all molecules, but is the only one available for nonpolar molecules.</p> Signup and view all the answers

    What is hydrogen bonding within van der Waals forces?

    <p>The hydrogen of one dipole (polar bond) and a fluorine, oxygen, or nitrogen of another dipole.</p> Signup and view all the answers

    What are the charged regions of an atom called?

    <p>Poles and dipoles.</p> Signup and view all the answers

    What symbols are used to show the charges on each side of a bond?

    <p>The delta symbol, δ, which can be δ- (negative) and δ+ (positive).</p> Signup and view all the answers

    Where does each electronegative symbol (weird s) go?

    <p>The positive one goes on the less electronegative atom and the negative one goes on the more electronegative atom.</p> Signup and view all the answers

    The longer the bond length, the stronger the bond.

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

    As the number of bonds increase, the bond length decreases.

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

    What does an electronegative difference of 0 mean?

    <p>Nonpolar covalent</p> Signup and view all the answers

    What does an electronegative difference between 0 and 1.70 mean?

    <p>Polar covalent</p> Signup and view all the answers

    Which of the following characteristics are true for single bonds?

    <p>Least dissociation energy</p> Signup and view all the answers

    What are the differences between physical properties of ionic and covalent compounds?

    <p>Ionic compounds have high melting and boiling points, are good conductors within aqueous solutions, and are hard/brittle. Covalent compounds have low melting and boiling points, can be molded easily (malleable and ductile) and don't conduct well.</p> Signup and view all the answers

    What is malleable? Ductile?

    <p>Malleable is when metals can be pressed into flat sheets. Ductile is when metals can be pulled into wires.</p> Signup and view all the answers

    Why are there differences between properties of covalent and ionic compounds?

    <p>Differences in attractive forces.</p> Signup and view all the answers

    How many elements have either a weird charge or need roman numerals even though they're not metals?

    <p>10</p> Signup and view all the answers

    How many nonmetals need roman numerals?

    <p>5</p> Signup and view all the answers

    What five elements need roman numerals even though they're nonmetals?

    <p>Gallium, Indium, Thallium, Lead, Tin</p> Signup and view all the answers

    What three elements have a specific charge even though they're in the metal group? List charge with a dash - Separate with a semicolon

    <p>Zinc-+2; Silver-+1; Cadmium-+2</p> Signup and view all the answers

    What two elements use the prefix system no matter WHAT?

    <p>Antimony and Bismuth</p> Signup and view all the answers

    Study Notes

    Ionic Bonding

    • Ionic bonding is the attractive force between oppositely charged particles in a compound.
    • Metals form cations, nonmetals form anions.

    Valence Electrons

    • Valence electrons are electrons in the outermost shell of an atom.

    Cations and Anions

    • Metals form cations (positive ions).
    • Nonmetals form anions (negative ions).

    Endothermic and Exothermic Reactions

    • Endothermic reactions absorb energy.
    • Exothermic reactions release energy.

    Ionic Compounds (Salts)

    • Ionic compounds are also called salts.
    • They have a crystal lattice structure.

    Lattice Energy

    • Lattice energy is the energy needed to separate the ions in an ionic compound.
    • Formation of ionic compounds is exothermic because they form stable, low-energy systems.

    Properties of Ionic Compounds

    • High melting and boiling points.
    • Strongest bonds.
    • Nonconductors as solids.
    • Good conductors when melted or dissolved in water (aqueous solutions).

    Formation of Anions

    • Anion formation: ELEMENT + e⁻ → ELEMENT⁻¹ + Electron Affinity

    Electron Affinity

    • Electron affinity is the energy released when an electron attaches to a gaseous atom.

    Formation of Cations

    • Cation formation: ELEMENT + Ionization Energy → ELEMENT⁺¹ + e⁻

    Ionization Energy

    • Ionization energy is the energy needed to remove an electron from an atom.

    Bond Strength and Atomic Radii

    • Smaller atomic radii lead to stronger bonds.
    • Higher oxidation charges result in stronger bonds.
    • Stronger bonds correspond to more negative lattice energy.

    Oxidation Charge

    • Oxidation charge is the charge on a monatomic ion.

    Ionic Solid Brittleness

    • Ionic solids break when ions line up during stress.

    Pseudo Noble Gas Configuration

    • Pseudo noble gas configurations are relatively stable electron arrangements.
    • Elements like copper, silver, and zinc have pseudo noble gas configurations.

    Stable Configurations in Bonding

    • Atoms achieve a noble gas configuration during bonding.

    Covalent Bonding

    • Covalent bonds form by sharing electrons.

    Diatomic Elements

    • Diatomic elements include H₂, N₂, O₂, F₂, Cl₂, Br₂, and I₂.

    Bond Types and Number of Shared Electrons

    • Single bonds share 2 electrons.
    • Double bonds share 4 electrons.
    • Triple bonds share 6 electrons.

    Sigma and Pi Bonds

    • Sigma bonds are located directly between two bonded atoms.
    • Pi bonds are located above and below the bond axis.
    • Pi bonds only form when there is both a sigma bond and at least one pi bond.

    Molecular Geometry and Hybridization

    • Various molecular geometries (linear, bent, trigonal planar, trigonal pyramidal, tetrahedral, trigonal bipyramidal, octahedral) relate to the number of bonding and nonbonding electron pairs. These correlate with specific hybridization (sp, sp², sp³).

    • Key examples are shown in relation to the bonding (e.g., 2,0 is linear, 2,1 is bent).

    Dissociation Energy

    • Dissociation energy quantifies the energy required to break a bond.

    Lewis Structures

    • Lewis structures are diagrams representing molecular structures.

    Resonance Structures

    • Resonance occurs where multiple Lewis structures adequately represent a molecule.

    Hybridization

    • Hybrid orbitals form from mixing atomic orbitals.

    Electronegativity

    • Electronegativity measures an atom's ability to attract electrons in a bond.

    Electron Affinity

    • Electron affinity is the attraction an atom has for an electron.

    Exceptions to Octet Rule

    • Some molecules (e.g., BH₃, NO₂, ClO₂) do not follow the octet rule, accommodating expanded octets.

    Expanded Octets

    • Elements in the third period and lower can have expanded octets.

    Intermolecular Forces (Van der Waals Forces)

    • Intermolecular forces include dispersion, dipole-dipole, and hydrogen bonding.

    Dispersion Forces

    • Dispersion forces (London Dispersion Forces) are weak intermolecular forces between nonpolar molecules.
    • Present in all molecules.

    Dipole-Dipole Forces

    • Dipole-dipole forces are stronger intermolecular forces between polar molecules.

    Hydrogen Bonds

    • Hydrogen bonds are strong intermolecular forces between a hydrogen atom of one dipole and a fluorine, oxygen, or nitrogen atom of another dipole.

    Polarity and Charges in Bonds

    • Polar bonds have partial positive and negative charges (δ+ and δ-).
    • Electronegativity differences determine bond polarity.

    Bond Length and Strength

    • Shorter bonds are generally stronger.
    • Increased bond number leads to shorter bond length.

    Electronegativity Differences and Bond Types

    • Electronegativity differences determine bond types:
      • Zero difference: Nonpolar covalent
      • 0–1.7: Polar covalent
      • 1.7 or greater: Ionic

    Bond Length, Strength, and Dissociation Energy (Summary)

    • Single bonds: Longest length, weakest strength, least dissociation energy.
    • Double bonds: Shorter length, stronger strength, greater dissociation energy.
    • Triple bonds: Shortest length, strongest strength, greatest dissociation energy.

    Physical Properties of Ionic vs. Covalent Compounds

    • Ionic: High melting/boiling points, good aqueous conductors, hard/brittle.
    • Covalent: Low melting/boiling points, diverse physical forms, poor conductors.

    Malleability and Ductility

    • Malleability is the ability to be shaped into sheets.
    • Ductility is the ability to be drawn into wires.

    Differences in Covalent and Ionic Properties

    • Differences stem from the types of attractive forces.

    Elements with Variable Charges/Roman Numerals

    • Transition metals often have multiple oxidation states.
    • Certain nonmetals (e.g., gallium, tin, lead) also require Roman numerals in their compounds' names.

    Specific Charges for Some Transition Metals

    • Zinc (+2), silver (+1), and cadmium (+2) have consistent charges.

    Prefix System Exception Elements

    • Antimony and bismuth require the prefix system for representing their specific charges.

    Studying That Suits You

    Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

    Quiz Team

    Description

    Test your knowledge on ionic bonding, the formation of cations and anions, and the properties of ionic compounds. This quiz covers the basics of ionic interactions, including endothermic and exothermic reactions, and lattice energy concepts.

    More Like This

    Mastering Ionic Bonding
    10 questions

    Mastering Ionic Bonding

    EruditeConsciousness avatar
    EruditeConsciousness
    Ionic Bonding and Valence Electrons
    5 questions

    Ionic Bonding and Valence Electrons

    GlisteningRadon avatar
    GlisteningRadon
    Ionic Bonds in Chemistry
    39 questions

    Ionic Bonds in Chemistry

    PeacefulYellow avatar
    PeacefulYellow
    Ionic Bonding Concepts
    24 questions

    Ionic Bonding Concepts

    WellReceivedSerenity avatar
    WellReceivedSerenity
    Use Quizgecko on...
    Browser
    Open
    Browser
    Browser