Intermolecular Forces Test Questions – Flashcards

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Three types of intermolecular forces
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London Dispersion

Dipole-Dipole

Ionic

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What is an ion dipole?
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Force between an ion and the partial charge on the end of a polar molecule
NOT REALLY IMPORTANT
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Dipole-Dipole
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Polar molecules attracted to each other
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With molecules of equal mass and size what happens with increasing polarity?
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Dipole-Dipole Strength increases
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London Dispersion
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Everything has London Dispersion
Attraction between all molecules
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As molecular weight increases so does what?
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Strength of London Dispersion
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Hydrogen bonding occurs when Hydrogen bonds to?
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F, O, or N
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Hydrogen bonding Definition
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Very strong Dipole-Dipole
H-F is most polar, so strongest
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Which is more dense. Ice or Water? Why?
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Water
Molecules assume an ordered, open arrangement
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Ions are involved
Polar molecules and ions are present
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Ion-Dipole Forces
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Ions are involved
Only ions are present
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Ionic Bonding
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Ions aren't involved
Polar molecules aren't involved
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London Dispersion Forces
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Ions aren't involved
Polar molecules are involved
Hydrogen not bonded O, N, or F
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Dipole-Dipole Forces
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Ions aren't involved
Polar molecules are involved
Hydrogen bonded O, N, or F
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Hydrogen Bonding
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Organize these in terms of 1. being Weakest
Dipole-Dipole
H-Bonding
Ionic Bonding
London Dispersion
Ion-Dipole
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First is weakest remember
1. London Dispersion
2. Dipole-Dipole
3. H-Bonding
4. Ion-Dipole
5. Ionic Bonding
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Viscosity
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Resistance of liquid to flow
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Viscosity ______ as molecular weight increases
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Increases
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Viscosity _____ with increasing temperature
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Decreases
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Why do liquids bead up on surfaces
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Surface Tension
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Surface Tension
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Energy required to increase the surface area of a liquid
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Heat of fusion
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Energy required to melt a solid
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Heat of vaporization
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Energy required to make a liquid a gas
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Critical temperature
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Highest temperature at which a liquid phase can form
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Critical Pressure
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Pressure required at the critical tiemperature
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Nonpolar, low weight substances have _____ critical temperatures and pressures
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Lower
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Vapor Pressure
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Pressure exerted by a gas on its space
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Volatile liquids Definition
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Liquids that evaporate readily/quick
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Volatile liquids have __ vapor pressures
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High
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Triple Point
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All 3 phases at equilibrium
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Orderring of atoms in Crystalline solid
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Well defined
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Properties of molecular bonds in crystalline solids
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Fairly soft
Low melting point
Dont conduct electricity
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Forces between molecular bonds in crystalline solids
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LD
Dipole-Dipole
H-Bonds
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Form of unit particles of molecular bonds in crystalline solids
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Atoms or molecules
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Properties of Covalent-network bonds in crystalline solids
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Very Hard
Very high melting point
Dont conduct electricity
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Properties of Ionic bonds in crystalline solids
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Hard and brittle
High melting point
Dont conduct electricity
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Properties of Metallic bonds in crystalline solids
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Soft to very hard
Low to very High melting point
Conduct electricity
Malleable and Ductle
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Forces between Covalent-network bonds in crystalline solids
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Covalent Bonds
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Forces between Ionic bonds in crystalline solids
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Electrostatic attractions?
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Forces between Metallic bonds in crystalline solids
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Metallic Bonds
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Form of unit particles of Covalent-network bonds in crystalline solids
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Atoms connected in a network of covalent bonds
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Form of unit particles of Ionic bonds in crystalline solids
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Positive and negative ions
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Form of unit particles of Metallic bonds in crystalline solids
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Atoms
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What are Diamond and SiO2 and Graphite
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Covalent Network
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Most substances that are gas or liquid at room temperature are usually ______ solids
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Molecular
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What is the only type of bond not due to LD
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The bonds in metallic solids
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Stronger the IMF the ____ the viscosity
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Greater
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What are held together by a "sea" of electrons
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Metallic Solids
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volatility= what in relation to imf
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Lowest
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Odor
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High vapor pressure and volatility
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What conducts electricity only when melted or dissolved
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Ionic
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What is usually water soluble
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Ionic
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Insoluble in water
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LD nonpolar with covalent bonds
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Insoluble in common solvents
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Covalent
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