Koofers

TESTBANK•PROF RATINGS•GPA HISTORIES•FLASHCARDS•SCHEDULES•TEXTBOOKS•DEALS
Universities » Georgia Tech (GT) » CHEM - Chemistry » 1310 - General Chemistry » Flash Cards

Bonding Chapters - Flashcards

Flashcard Deck Information

Class:CHEM 1310 - General Chemistry
Subject:Chemistry
University:Georgia Institute of Technology-Main Campus
Term:Fall 2009
- of -
INCORRECT CORRECT
- INCORRECT     - CORRECT     - SKIPPED
Shuffle Remaining Cards Show Definitions First Take Quiz (NEW)
Hide Keyboard shortcuts
Next card
Previous card
Mark correct
Mark incorrect
Flip card
Start Over
Shuffle
      Mode:   CARDS LIST       ? pages   PRINT EXIT
Ionic Bonding Bonding between a metal and nonmetal through electrostatic interactions
Bond Length The distance at which the energy of the ion pair system is the lowest
Covalent Bonding The bonding in which electrons are shared by the nuclei
Pure Covalent Bond Electrons are shared equally
Generated by Koofers.com
Polar Covalent Bond Electrons are shared unequally
Electronegativity The ability of an atom to ATTRACT the shared electrons to itself
Electron Affinity The measure of the energy required to DETACH an electron from
Isoelectronic Series Atoms with the same noble gas configuration prefix
Generated by Koofers.com
Periodic Law 1) Size of the atoms INCREASES DOWN the group 2) For isoelectronic series, the size DECREASES WITH INCREASING ATOMIC NUMBER 3) Electronegativity INCREASES ACROSS a period and DECREASES DOWN a group
Lattice Energy A measure of the strength of bonds in that ionic compound; The change in energy that takes place when separated gaseous ions are packed together to form an ionic compound.
Percent Ionic Character of a Bond (measured dipole moment of X-Y) ----------------------------- * 100% (calculated dipole moment of XY)
Bond Enthalpy (ΔH) The enthalpy change in a reaction in which a chemical bond is broken in the gas phase. ΔH = (energy required to break bonds) - (energy released when bonds form)
Generated by Koofers.com
Bond Energy (ΔE) The energy needed to break a chemical bond.
Lewis Structures Lewis structures, also called Lewis-dot diagrams, Electron-dot diagrams or Electron-dot structures, are diagrams that show the bonding between atoms of a molecule, and the lone pairs of electrons that may exist in the molecule.
Formal Charge C = (group no.) − (no. of lone pair electrons) − ½ (no. of electrons in bonding pairs)
Resonance The case where more than one Lewis structure can be drawn for a molecule.
Generated by Koofers.com
Steric Number The steric number of a molecule is the number of atoms bonded to the central atom of a molecule plus the number of lone pairs on the central atom.
VSEPR Theory Valence shell electron pair repulsion (VSEPR) theory is a model in chemistry used to predict the shape of individual molecules based upon the extent of electron-pair electrostatic repulsion.
Intramolecular Forces (Chemical Bonds) An intramolecular force is any force that holds together the atoms making up a molecule or compound. Characteristics: Strong Directional Short Range (relative)
Intermolecular Forces Forces that act between stable molecules or between functional groups of macromolecules. Characteristics: Weaker than chemical bonds, usually much weaker Less directional than covalent bonds, more directional than ionic bonds Longer range than covalent bonds but at shorter range than ionic bonds
Generated by Koofers.com
Dipole-Dipole Attraction A type of polar bond where molecules have dipole moments. Characteristics: Very weak compared to covalent or ionic bonds Becomes weaker as distance between the dipoles increases
Hydrogen Bonding A hydrogen bond is a particularly strong dipole-dipole interaction of a hydrogen atom with an electronegative atom, like nitrogen, oxygen or fluorine. The strength of the interaction results from the great polarity of the bond and the closer than normal approach of the dipoles.
London Dispersion Forces London dispersion forces are weak intermolecular forces that arise from the interactive forces between temporary multipoles in molecules without permanent multipole moments. They exist among NOBLE GAS atoms and NONPOLAR molecules. The more electrons that are present in the molecule, the stronger the dispersion forces will be, so the higher the melting and boiling points will be. As the mass of the molecules increases, so does the strength of the dispersion force acting between the molecules.
List of molecules with Hydrogen Bonding Water, Ammonia (NH3), Hydrofluoric Acid (HF), Hydrogen Peroxide (H2O2), Methanol (CH3OH) and all alcohols, Acetic Acid (CH3COOH) and all carboxylic acids, Methyl Amine (CH3NH2) and all amines
Generated by Koofers.com
Order of Hydrogen Bonding Strength in Alcohols 1 degree (1 hydrocarbon attached to the carbon atom to which OH is attached) > 2 degree (2 hydrocarbons) > 3 degree (3 hydrocarbons)
Polarizability Polarizability is the relative tendency of a charge distribution, like the electron cloud of an atom or molecule, to be distorted from its normal shape by an external electric field, which may be caused by the presence of a nearby ion or dipole. Polarizability is more in larger atoms, and thus greater london dispersion forces.
Molecules with LD forces Noble Gases, H2, CH4, CCl4, I2, CO2, Teflon, Polyethylene, BF3, All Hydrocarbons These contain LD to some extent: HF, HCl, CO, CHCl3, NH3, NO,
Molecules with Dipole-Dipole Forces HBr, HCl, CO, CHCl3, NO, H2S, CH3Cl
Generated by Koofers.com
Force of Attraction in KBr Ion-Dipole
Order of Strength of Forces Dispersion < Dipole-Dipole < Hydrogen Bonding < Ion-Dipole < Ionic Bonding
Generated by Koofers.com

List View: Terms & Definitions

  Hide All 30 Print
 
Front
Back
 Ionic BondingBonding between a metal and nonmetal through electrostatic interactions
 Bond LengthThe distance at which the energy of the ion pair system is the lowest
 Covalent BondingThe bonding in which electrons are shared by the nuclei
 Pure Covalent BondElectrons are shared equally
 Polar Covalent BondElectrons are shared unequally
 ElectronegativityThe ability of an atom to ATTRACT the shared electrons to itself
 Electron AffinityThe measure of the energy required to DETACH an electron from
 Isoelectronic SeriesAtoms with the same noble gas configuration prefix
 Periodic Law1) Size of the atoms INCREASES DOWN the group
2) For isoelectronic series, the size DECREASES WITH INCREASING ATOMIC NUMBER
3) Electronegativity INCREASES ACROSS a period and DECREASES DOWN a group
 Lattice EnergyA measure of the strength of bonds in that ionic compound; The change in energy that takes place when separated gaseous ions are packed together to form an ionic compound.
 Percent Ionic Character of a Bond(measured dipole moment of X-Y)
----------------------------- * 100%
(calculated dipole moment of XY)
 Bond Enthalpy (ΔH)The enthalpy change in a reaction in which a chemical bond is broken in the gas phase.
ΔH = (energy required to break bonds) - (energy released when bonds form)
 Bond Energy (ΔE)The energy needed to break a chemical bond.
 Lewis StructuresLewis structures, also called Lewis-dot diagrams, Electron-dot diagrams or Electron-dot structures, are diagrams that show the bonding between atoms of a molecule, and the lone pairs of electrons that may exist in the molecule.
 Formal ChargeC = (group no.) − (no. of lone pair electrons) − ½ (no. of electrons in bonding pairs)
 ResonanceThe case where more than one Lewis structure can be
drawn for a molecule.
 Steric NumberThe steric number of a molecule is the number of atoms bonded to the central atom of a molecule plus the number of lone pairs on the central atom.
 VSEPR TheoryValence shell electron pair repulsion (VSEPR) theory is a model in chemistry used to predict the shape of individual molecules based upon the extent of electron-pair electrostatic repulsion.
 Intramolecular Forces (Chemical Bonds)An intramolecular force is any force that holds together the atoms making up a molecule or compound.
Characteristics:
Strong
Directional
Short Range (relative)
 Intermolecular ForcesForces that act between stable molecules or between functional groups of macromolecules.
Characteristics:
Weaker than chemical bonds, usually much weaker
Less directional than covalent bonds, more directional than ionic bonds
Longer range than covalent bonds but at shorter range than ionic bonds
 Dipole-Dipole AttractionA type of polar bond where molecules have dipole moments.
Characteristics:
Very weak compared to covalent or ionic bonds
Becomes weaker as distance between the dipoles increases
 Hydrogen BondingA hydrogen bond is a particularly strong dipole-dipole interaction of a hydrogen atom with an electronegative atom, like nitrogen, oxygen or fluorine. The strength of the interaction results from the great polarity of the bond and the closer than normal approach of the dipoles.
 London Dispersion ForcesLondon dispersion forces are weak intermolecular forces that arise from the interactive forces between temporary multipoles in molecules without permanent multipole moments. They exist among NOBLE GAS atoms and NONPOLAR molecules. The more electrons that are present in the molecule, the stronger the dispersion forces will be, so the higher the melting and boiling points will be.
As the mass of the molecules increases, so does the strength of the dispersion force acting between the molecules.
 List of molecules with Hydrogen BondingWater, Ammonia (NH3), Hydrofluoric Acid (HF), Hydrogen Peroxide (H2O2), Methanol (CH3OH) and all alcohols, Acetic Acid (CH3COOH) and all carboxylic acids, Methyl Amine (CH3NH2) and all amines
 Order of Hydrogen Bonding Strength in Alcohols1 degree (1 hydrocarbon attached to the carbon atom to which OH is attached) > 2 degree (2 hydrocarbons) > 3 degree (3 hydrocarbons)
 PolarizabilityPolarizability is the relative tendency of a charge distribution, like the electron cloud of an atom or molecule, to be distorted from its normal shape by an external electric field, which may be caused by the presence of a nearby ion or dipole. Polarizability is more in larger atoms, and thus greater london dispersion forces.
 Molecules with LD forcesNoble Gases, H2, CH4, CCl4, I2, CO2, Teflon, Polyethylene, BF3, All Hydrocarbons
These contain LD to some extent:
HF, HCl, CO, CHCl3, NH3, NO,
 Molecules with Dipole-Dipole ForcesHBr, HCl, CO, CHCl3, NO, H2S, CH3Cl
 Force of Attraction in KBrIon-Dipole
 Order of Strength of ForcesDispersion < Dipole-Dipole < Hydrogen Bonding < Ion-Dipole < Ionic Bonding
+0
Karma