Ionic Bonding Concepts
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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 elements form cations?

All metals.

What is endothermic?

<p>Energy is absorbed.</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

Is the formation of ionic compounds endo or exothermic?

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

What are the characteristics of ionic compounds?

<p>Strongest bonds</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, ______.

<p>The stronger bond formed</p> Signup and view all the answers

The higher the total oxidation charge is for an atom...

<p>The stronger bond formed</p> Signup and view all the answers

The stronger the bond, ______.

<p>The more negative lattice energy is for a compound.</p> Signup and view all the answers

What is oxidation charge?

<p>The charge of a monatomic (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

What elements have pseudo noble gas configurations?

<p>Elements like Copper, silver, zinc.</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

What are the diatomic elements?

<p>H2, N2, O2, F2, Cl2, Br2, I2</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

Match the following numbers with their corresponding molecular geometries, bond angles, and hybridization.

<p>2,0 = Linear, 180, sp 2,1 = Bent, 120, sp2 3,0 = Trigonal planar, 120, sp2 3,1 = Trigonal pyramidal, 109.5, sp3 4,0 = Tetrahedral, 109.5, sp3 2,2 = Bent, 109.5, sp3 5,0 = Trigonal bipyramidal 6,0 = Octahedral</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

What are the exceptions to the octet rule?

<p>BH3</p> Signup and view all the answers

What elements can have expanded octets?

<p>Elements in the third period or lower.</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 shorter the bond length, ______.

<p>The stronger the bond</p> Signup and view all the answers

As the number of bonds increase, ______.

<p>The bond length decreases</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

Match the bond types with their length, strength, and dissociation energy characteristics.

<p>Single bond = Longest length, weakest strength, least dissociation energy Double bond = Short length, strong strength, great dissociation energy Triple bond = Shortest length, strongest strength, greatest ionization 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 bonds are forces holding charged particles together in compounds.

Valence Electrons

  • Valence electrons are outermost shell electrons.

Cations

  • Metals form cations.

Anions

  • Nonmetals form anions.

Endothermic

  • Energy is absorbed during endothermic reactions.

Exothermic

  • Energy is released during exothermic reactions.

Ionic Compound Alias

  • An ionic compound is also called a salt.

Crystal Lattice Structure

  • Ionic compounds have a crystalline structure called a crystal lattice.

Lattice Energy

  • Lattice energy is the energy needed to separate the ions in an ionic compound.

Ionic Compound Formation

  • Ionic compound formation is exothermic; stable, low-energy systems.

Ionic Compound Characteristics

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

Anion Reaction Equation

  • ELEMENT + e- -> ELEMENT-1 + electron affinity

Electron Affinity

  • Electron affinity is energy released when an electron joins a gaseous atom.

Cation Reaction Equation

  • ELEMENT + ionization energy -> ELEMENT+1 + e-

Ionization Energy

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

Atomic Radii and Bonding

  • Smaller atomic radii lead to stronger bonds.
  • Higher total oxidation charges lead to stronger bonds.
  • Stronger bonds have more negative lattice energy

Oxidation Charge

  • Oxidation charge is the charge of a monatomic ion (one-atom ion).

Ionic Solid Brittleness

  • Ionic solids break due to the alignment of ions.

Pseudo Noble Gas Configuration

  • Relatively stable electron arrangements, similar to noble gases.

Elements with Pseudo Noble Gas Configurations

  • Copper, Silver, Zinc

Stable Bonding Configuration

  • Atoms achieve a noble gas configuration when they bond.

Covalent Bonding

  • Covalent bonds form through electron sharing.

Diatomic Elements

  • H2, N2, O2, F2, Cl2, Br2, I2

Bonds and Shared Atoms

  • Single bond: 2 shared atoms
  • Double bond: 4 shared atoms
  • Triple bond: 6 shared atoms

Sigma Bond Position

  • Sigma bonds are located directly between two bonding atoms.

Sigma Bond Formation Explanation

  • Electron orbitals overlap, centering the shared electrons.

Pi Bond Location

  • Pi bonds are positioned above and below the bonding axis.

Pi Bond Pre-Conditions

  • Occur when there's one sigma bond plus one or two pi bonds.

Molecular Geometry - 2,0

  • Linear (180°) sp hybridised

Molecular Geometry - 2,1

  • Bent (120°) sp2 hybridised

Molecular Geometry - 3,0

  • Trigonal planar (120°) sp2 hybridised

Molecular Geometry - 3,1

  • Trigonal pyramidal (109.5°) sp3 hybridised

Molecular Geometry - 4,0

  • Tetrahedral (109.5°) sp3 hybridised

Molecular Geometry - 2,2

  • Bent (109.5°) sp3 hybridised

Molecular Geometry - 5,0

  • Trigonal bipyramidal

Molecular Geometry - 6,0

  • Octahedral

Dissociation Energy

  • Dissociation energy represents the energy needed to break a bond.

Lewis Structures

  • Lewis structures illustrate molecular structure using symbols and dots to show bonds and lone pairs.

Resonance

  • Resonance occurs when multiple Lewis structures represent a molecule, especially with multiple double and single bonds to the same atom.

Hybridization

  • Hybridization is the mixing of atomic orbitals to form new, identical hybrid orbitals.

Electronegativity

  • Electronegativity is the ability of an element to attract electrons in a chemical bond.

Electron Affinity (diff.)

  • Electron affinity is the tendency of an atom to accept electrons.

Electronegativity vs. Electron Affinity

  • Electronegativity's about attracting electrons; electron affinity's about accepting them.

Exceptions to Octet Rule

  • BH3, NO2, ClO2, PCl5, XeF3+

Expanded Octets

  • Elements in Period 3 or lower can have expanded octets (more than 8 valence electrons).

Van der Waals Forces

  • Includes dispersion, dipole-dipole, and hydrogen bonding intermolecular forces.

Dispersion Forces

  • Weak intermolecular forces between nonpolar molecules (London Dispersion Forces).

Dipole-Dipole Forces

  • Stronger intermolecular forces between polar molecules.

Dispersion Force Scope

  • Exist between all molecules, but only present in nonpolar ones.

Hydrogen Bonding

  • Hydrogen bonding involves hydrogen atoms in one dipole and fluorine, oxygen, or nitrogen from another.

Atomic Charged Regions

  • Atomic charged regions referred to as poles or dipoles.

Bond Charge Indication

  • Used to show opposing charges, delta negative (δ-) and delta positive (δ+).

Electronegativity Placement

  • Lower electronegative element receives positive delta and higher the negative delta.

Bond Length and Strength Relationship

  • Shorter bonds are generally stronger.

Bond Number and Length Relationship

  • Increasing bond numbers decrease bond length.

Electronegativity Difference - 0

  • Zero electronegativity difference indicates nonpolar covalent bonds.

Electronegativity Difference (0-1.7)

  • Electronegativity difference between 0 and 1.7 indicates polar covalent bonds.

Electronegativity Difference - 1.7

  • Electronegativity difference of 1.7 or greater suggests ionic bonds.

Single Bond Characteristics

  • Longest length, weakest strength, least dissociation energy

Double Bond Characteristics

  • Shorter length, stronger strength, greater dissociation energy

Triple Bond Characteristics

  • Shortest length, strongest strength, greatest dissociation energy

Ionic vs. Covalent Physical Properties

  • Ionic: High melting/boiling points, good conductors in aqueous solutions, hard/brittle.
  • Covalent: Low melting/boiling points, easily molded (malleable/ductile), poor conductors.

Malleable/Ductile

  • Malleable: Can be hammered into sheets.
  • Ductile: Can be drawn into wires.

Property Differences Explanation

  • Property differences result from different attractive forces.

Elements with Variable Charges/Roman Numerals

  • 10 elements may need a charge/roman numeral indicating oxidation.

Non-Metal Elements Needing Roman Numerals

  • 5 nonmetals require Roman numerals indicating oxidation.

Specific Non-Metal Elements Needing Roman Numerals

  • Gallium, Indium, Thallium, Lead, Tin

Metal Elements with Specific Charges

  • Zinc (+2); Silver (+1); Cadmium (+2)

Elements Requiring Prefix System

  • Antimony and Bismuth always use the prefix system to show charge.

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Description

Test your knowledge on ionic bonding, including the formation of cations and anions, the properties of ionic compounds, and the significance of lattice energy. This quiz covers fundamental concepts in chemistry regarding ionic interactions and energy changes in reactions.

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