Exam 3 Flashcards
Electron
Subatomic particle with a negative charge and smallest of the main three subatomic particles.
Proton
Subatomic particle with positive electrical charge.
Neutron
Subatomic particle with no charge.
Nucleus
Small dense, positively charged center of atom containing all protons and neutrons.
Nucleon
Any subatomic particle found in nucleus of an atom.
Electron Configuration
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p⁶
Periodic Trends: Atomic Size
Top Right to Bottom Left: Increasing atomic size
Periodic Trends - Ionization Energy
Bottom Left to Top Right: Increasing ionization energy
Ionic Bond
Bond between metal and nonmetal
Covalent Bond
Chemical bond involving sharing of electrons between atoms in a molecule (nonmetals)
Bonding Electron
Pairs of valence electrons that are shared between atoms in a covalent bond.
Nonbonding electrons(lone pair electrons)
Pairs of valence electrons on an atom that are not involved in electron sharing.
HONC(Neutral molecules)
1234
Number of bonds
Electron Group Geometry: 2 Electron Groups
EG: Linear
Predicted Bond Angle: 180°
Electron Group Geometry: 3 Electron Groups
EG: Trigonal Planar
Predicted Bond Angle: 120°
Electron Group Geometry: 4 Electron Groups
EG: Tetrahedral
Predicted Bond Angle: 109.5°
Linear Electron Domain
MG: Linear
Trigonal Planar Electron Domain
All e- domains = Bonds: trigonal planar
One e- domain = Nonbonding: Bent/angular
Tetrahedral Electron Domain
All e- domains = BondingPair: Tetrahedral
One nonbonding pair e- domain: Trigonal Pyramidal
Two nonbonding pair e- domain: Bent/angular
Electronegativity
Measure of relative attraction that an atom has for the shared electron in a bond. Determined by nuclear charge and number of other electrons present in electron shell.
Bond Polarity
Measure of the degree of inequality in the sharing of electrons in a chemical bond.
Nonpolar Covalent Bond
Covalent bond in which there is equal sharing of electrons between two atoms.
Polar Covalent Bond
Covalent bond in which there is unequal sharing of electrons between two atoms.
Trait of Polar Covalent Bonds
The greater the difference in electronegativity, the more polar is the bond.
Nonpolar Covalent Bond (Electronegativity)
Difference of 0 - 0.4
Polar Covalent Bond (Electronegativity)
Difference of 0.5 - 2.0
Ionic Bond (Electronegativity)
Difference of > 2.0
Molecular Polarity
Measure of the degree of inequality in the attraction of bonding electrons to various locations within a molecule.
Polar Molecule
Asymmetrical distribution of electronic charge.
Nonpolar molecule
Symmetrical distribution of electronic charge.
Finding Polarity of Molecules
1: Is compound covalent?
2: Are the bonds polar?
3: Is the molecule asymmetrical.
Gas
State of matter with no fixed shape and no fixed volume.
Pressure
Pressure = Force/Area
mm Hg to torr
1 mm Hg = 1 torr
atm to mm Hg
1 atm = 760 mm Hg
atm to psi
1 atm = 14.7 psi = 101,325 Pa
Boyle’s Law (Pressure & Volume)
P₁V₁ = P₂V₂
Charles’s Law (Volume & Temperature)
V₁/T₁ = V₂/T₂
Gay-Lussac’s Law (Pressure & Temperature)
P₁/T₁ = P₂/T₂
Combined Gas Law (Pressure, Volume, Temperature)
P₁V₁/T₁ = P₂V₂/T₂
Avogadro’s Law (Volume, Number)
V₁/n₁ = V₂/n₂
Ideal Gas Law (All)
P₁V₁/n₁T₁ = P₂V₂/n₂T₂
Dalton’s Law of Partial Pressures
Total pressure exerted by mixture of gases is sum of partial pressure of individual gases present.
Standard Temperature and Pressure (STP)
1 atm and 273 K (0° C)
Molar Volume
Volume of one mole of gas at STP = 22.4L
Heats of Fusion
ΔHբᵤₛᵢₒₙ = kJ/mol
Heat of Vaporization
ΔHᵥₐₚ = kJ/mol
Intermolecular Force(IMF)
Attractive Force that acts between molecules influencing melting points, boiling points, viscosity and surface tension.
Dispersion Force
Weak temporary intermolecular force that occurs between an atom or molecule and another atom or molecule.
1) Number of e- in atom (more e-, more dispersion force)
2) Size of atom/molecule/molecular weight.
3) Shape of molecules with similar masses (more compact, less dispersion force)
Dipole-dipole interactions
IMF that occurs between polar molecules.
1) Greater the polarity, the greater the dipole-dipole interaction.
Hydrogen Bonding
Extra strong dipole-dipole interaction involving molecules with an H atom covalently bonded to small, very electronegative atom.
H-F
H-O
H-N
