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AP Chemistry: IMF

AP Chemistry: IMF

memorize.aimemorize.ai (lvl 286)
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26 cards
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Section 1

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Body-Centered Unit Cell

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Last updated

5 years ago

Date created

Mar 1, 2020

Cards (26)

Section 1

(26 cards)

Body-Centered Unit Cell

Front

Has particles located at the corners and in the center of the cube

Back

Liquid State

Front

Liquid particles are in constant flux. Clumps of particles may form and then break apart. Liquids have a fixed volume and no fixed shape. At the surface of the liquid, molecules are being pulled into the body of the liquid from the sides and below, not above. The effect of this unequal attraction is because liquids try to minimize their surface area by forming a sphere. It requires force to break the attractive forces at the surface. 3 Properties: Surface Area, Viscosity, Capillary Action

Back

Ionic Solids

Front

Lattices composed of ions are held together by the attraction of the opposite charges of the ions. These crystalline solids tend to be strong, with high melting points because of the strength of the IMF. Ex: NaCl

Back

Atomic Solids

Front

Individual atoms are held in place by London forces. Ex: noble gases

Back

Simple Unit Cell

Front

Has particles located at the corners of a simple cube

Back

Viscosity

Front

Resistance of liquids to flow. It's affected by intermolecular forces, temperature, and molecular shape. Liquids with strong intermolecular forces tend to have a higher____ than those with weaker molecular forces. As temperature increases, kinetic energy increases overcoming attractive forces, which lowers____ The longer and more complex the molecule, the more contact the particle will have as they slip past each other increasing the_____

Back

Ion-Dipole IMF

Front

These forces are due to the attraction of an ion and one end of a polar molecule (dipole). This type of attraction is important in aqueous salt solutions, where the ion attracts water molecules and may form a hydrated ion, such as Al(H2O)6. One of the strongest IMF.

Back

London (Dispersion) IMF

Front

Occurs in all forces, specifically those when other types of IMF are absent. Arises from a momentary distortion of the electron cloud, with the creation of a very weak dipole.

Back

Molecular Solids

Front

Lattices composed of molecules are held in place by London forces, dipole-dipole forces, and hydrogen bonding. Ex: solid methane and water

Back

Capillary Action

Front

The spontaneous rising of a liquid through a narrow tube, against the force of gravity. It is caused by competition between the liquid and the tube wall. Stronger the attraction between the tube and the liquid, the higher the level will be. Ex: Hg would have a low___ H2O would have a high_____

Back

Metallic Bonding

Front

Bonding situation between metals in which the valence e- are donated to a vast electron pool ("sea of e-"), so that the valence e- are free to move through the entire metal solid.

Back

Water's Unusual Properties

Front

Due to its H-bonding -will dissolve both ionic and polar covalent because of its polarity to form H-bonds. -Universal Solvent -High heat capacity (heat absorbed to increase T) -High heat vaporization(heat needed for liquid to gas) -High Surface Area

Back

Intermolecular Forces (IMF)

Front

Attractive or repulsive forces between molecules, caused by partial charges. 1. Ion-Dipole 2. Dipole-Dipole 3. Hydrogen Bond 4. Ion-Induced Dipole and Dipole-Induced Dipole 5. London (Dispersion)

Back

Covalent Bonding

Front

Nonmetal + nonmetal. Sharing of one or more pairs of e-. Nonpolar covalent = equal sharing. Polar covalent = greater attraction.

Back

Face-centered Unit Cell

Front

Has particles at the corners and one in the center of each face of the cube, but not in the canter of the cube itself

Back

Hydrogen Bond IMF

Front

Special type of dipole-dipole attraction in which a H-atom is polar-covalently bonded to one of the extremely electronegative elements (N, O, or F). Extremely polar bonds with a great degree of charge separation within the molecule.

Back

Dipole-Dipole IMF

Front

Result from the attraction of the positive end of one dipole to the negative end of another dipole. These attractions are important in polar liquids. Ex: gaseous hydrogen chloride, HCl

Back

Ion-Induced Dipole and Dipole-Induced Dipole IMF

Front

Occur when the charge on an ion or a dipole distorts the e- cloud of a non polar molecule and induces a temporary dipole in the non polar molecule. Fairly weak attractions.

Back

Ionic Bonds

Front

Metals + nonmentals. Transfer of electrons from a metal to a nonmetal.

Back

Covalent Network Solids

Front

Covalent bonds join atoms together in the crystal lattice, which is large. Ex: graphite, diamond, and SiO2

Back

Solid State

Front

Has both a definite shape and volume 2 Types: Amorphous- lack extensive ordering of particles. These types of ___ have no distinct melting point and get softer as T rises decreasing viscosity. (Ex: Glass + Rubber) Crystalline- Regular ordering of particles in a 3D structure called crystal lattice

Back

Phase Diagram: Represents relationship between substance's state of matter to temperature and pressure. AC: solid's change in VP with changing T, for sublimation. AD: varying melting point with varying P. AB: variation in liquids VP with varying P. B: critical point, gas at equilibrium with liquid. A: triple point, 3 states of matter coexist.

Front

Back

Relationship of IMF to Phase Changes

Front

Strong IMF in liquid means more KE is required to convert it into a gas. Conversely, strong IMF in a gas makes it easier to condense it into a liquid.

Back

Relationship Between Average Kinetic Energy and Temperature

Front

Substance state of matter depends on KE + IMF. KE moves particles away from each other. Temperature (T) is a measure of average KE of the molecules. As T increases so does its average KE moving particles farther away.

Back

Metallic Solids

Front

Metal atoms occupying the crystal lattice are held together by the metallic bonding. In metallic bonding, e- of the atoms are delocalized and are free to move throughout the entire solid. This explains the electrical and thermal conductivity, as well as many other properties of metals.

Back

Surface Tension

Front

The amount of force required to break through the molecular layer of a liquid at the surface. Polar liquids, especially those that undergo hydrogen bonding, have a much higher surface tension than non polar liquids.

Back