click below
click below
Normal Size Small Size show me how
Phases of Matter
vocab 5
Term | Definition |
---|---|
Solid | A form of matter that has a definite shape and volume. Particles are packed closely together. |
Liquid | A form of matter that has an indefinite shape, flows, yet has a fixed volume. Particles are close together. |
Gas | A form of matter that takes both the shape and volume of its container. Particles are far apart. |
Volume | The measure of space occupied by the object. Can change when there's a difference between internal and external pressure |
Non Polar Covalent Bond | When the atoms in the bond pull equally (as occurs when identical atoms are bonded), the bonding electrons are shared equally. Equal distribution of electrons between two atoms, no difference in electronegativity. |
Polar Covalent Bond | A covalent bond between atoms in which electrons are shared unequally. Unequal distribution of electrons between two atoms, there is a difference in electronegativity. |
Non Polar Covalent Molecule | Symmetrical in shape, all polar covalent bonds cancel out. |
Polar Covalent Molecule | Non symmetrical in shape, polar covalent bonds do not all cancel out. |
Dispersion Forces | The weakest of all molecular interactions are caused by the motion of electrons. They occur even between nonpolar molecules. |
Dipole Interactions | Occurs when polar molecules are attracted to one another. The slightly negative region of polar molecule is weakly attracted to the slightly positve region of another polar molecule. |
Hydrogen Bonds | An attraction between the hydrogen atom on one molecule to either F, O, or N on another molecule. |
Colanent Network Solids | Covalent molecules where the atoms are bonded in very rigid and structured arrangements. These are non- conducive, but are hard and have very high melting and boiling points. Happens in graphite and diamond (both carbon), and silicon dioxide (sand) |
Standard Temperature and Pressure | A temperature of 0 C and a pressure of 101.3 kPa or 1 atmosphere (atm). Can be found on table A. |
Absolute Zero | The temperature at which the motion of particles theoretically cease. |
Allotrope | Two or more different molecules form the same element in the same physical state. Carbon (coal, graphite, diamond) and oxygen (O2 and ozone O3). |
Melting | When a substance changes from a solid to a liquid, opposite of freezing. |
Freezing | When a substance changes from a liquid to a solid, opposite of melting. |
Evaporation | When a substance changes from a liquid into a gas, the opposite of condensing, also known as vaporization or boiling. |
Condensation | When a substance changes from a gas into a liquid, opposite of evaporation |
Sublimation | When a substance changes from a solid directly into gas with no liquid being formed at all, opposite of deposition. |
Deposition | When a substance changes from a gas directly into a solid with no liquid being formed at all, opposite of sublimation. |
Boiling Point | When a liquid is heated to temperature at which particles throughout the liquid have enough kinetic energy to vaporize , the liquid begins to bubble. Bubbles of vapor form throughout the liquid, rise to the surface, and escape into the air. The boiling po |
Melting Point | The temperature at which a solid changes into a liquid |
Gas Pressure | Results from the force exerted by gas per unit surface area of an object. |
Temperature | The Kelvin temperature of a substance is directly proportinal to the average kinetic energy of the particles of the substances. |
Diffusion | The tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout. |
Effusion | A gas escapes through a tiny hole in its container. |
Real and Ideal Gases | Real gases differ most from ideal gas at low temperature and high pressure |
Surface tension | The inward force, or pull, tends to minimize the surface area of a liquid. |