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76 Cards in this Set
- Front
- Back
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solid to liquid |
melting |
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liquid to solid |
freezing |
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solid to gas |
sublimation |
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gas to solid |
deposition |
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liquid to gas |
vaporization/boiling |
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gas to liquid |
condensation |
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solid state |
definite volume and definite shape |
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what happens to a solid each passing minute? what does this cause? |
energy is added to the substance - this causes molecules of substance to move more rapidly which we detect by a temp rise in substance |
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liquid state |
definite volume and indefinite shape |
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gas state |
indefinite volume and indefinite shape
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solids |
-high density -incompressible -low rate of diffusion |
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liquid |
- takes shape of container - high density - relatively incompressible - medium rate of diffusion |
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gas |
- takes shape and volume of container - low density - compressible - fast rate of diffusion |
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kinetic molecular theory |
- based on idea that particles of matter are always in motion - can be used to explain properties of solids, liquids and gases in terms of the energy of particles and the forces that act between them |
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melting |
- temp at which solid becomes liquid is the melting point - kinetic energies of particles overcome attractive forces holding them together |
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what is the freezing point |
temp at which solid and liquid are in equilibrium at 1 atm |
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molar enthalpy of fusion |
amount of energy as heat required to melt one mole of solid at the solid's melting point |
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boiling |
energy must be added continuously in order to keep a liquid boiling |
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what does the added energy do to boiling? |
overcomes attractive forces between molecules of the liquid during the liquid-to-gas change and is stored in the vapor as potential energy |
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normal boiling point |
boiling point at normal atmospheric pressure |
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molar enthalpy of vaporization |
amount of energy as heat that is needed to vaporize on mole of liquid at the liquid's boiling point at constant pressure |
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two types of solids |
cyrstalline and amorphous solids |
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which of the two types of solids are most solids in the world? |
cyrstalline solids (consist of crystals) |
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crystal |
substance in which the particles are arranged in an orderly, geometric, repeating pattern |
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amorphous solid |
one in which particles are arranged randomly; sometimes classified as supercooled liquids |
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super cooled liquids |
substances that retain certain liquid properties even at temps at which they appear solid |
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crystal solids melting point order |
CM |
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ionic |
- melt at high temps - good insulators |
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covalent network |
- melt at high temps - nonconductors or semiconductors |
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metallic |
- melt at high temps - good conductors |
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covalent molecular |
- melt at low temps - good insulators |
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capillary action |
attraction of the surface of a liquid to the surface of a solid |
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what is capillary action responsible for? |
concave liquid surface, called a meniscus |
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surface tension |
force that tends to pull adjacent parts of a liquid's surface together, thereby decreasing surface area to the smallest possible size |
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what do vapor molecules do in equilibrium with a liquid in a closes system? |
exert a pressure proportional to the concentration of molecules in the vapor phase |
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equilibrium vapor pressure |
pressure exerted by a vapor in equilibrium with its corresponding liquid at a given temperature |
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boiling point |
temp at which equilibrium vapor pressure of the liquid equals the atmospheric pressure ex. Denver |
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volatile liquids |
liquids that evaporate readily ex. rubbing alcohol - have relatively weak forces of attraction between particles |
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nonvolatile liquids |
don't evaporate quickly - have relatively strong attractive forces between their particles |
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how many sig figs are in this number: 3.0800 |
5 |
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how many sig figs are in this number 0.00418 |
3 |
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how many sig figs are in this number: 7.09x10^5 |
3 |
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how many sig figs are in this number: 0.0101 |
3 |
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how many sig figs are in this number: 0.0035 |
4 |
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what does an econo-balance round to? |
rounded to the nearest 100g |
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what does a balance pro round to? |
round to nearest 1g |
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what does a good balance do? |
round to nearest 10g |
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what does an exacto balance round to? |
nearest 0.1g |
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density equation |
d=m/v density is in g/mL m is in g v is in mL |
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what is a chemical change |
change in color, formation of precipitate (new solid substance that settles out of solution), the production and release of gas or change in temp |
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what is a physical change |
change in shape, size, density or state but chemical composition stays the same PHYSICAL IS WHEN SOMETHING CHANGES FROM SOLID TO LIQUID TO GAS |
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chem or phys: burning wood |
chem |
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chem or phys: dry ice turning into gas |
phys |
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chem or phys: freezing water |
physical |
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chem or phys: sugar dissolving in water |
phys |
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1 km = how many m? |
1000 m |
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1m = how many cm? |
100 cm |
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1m = how many mm? |
1000mm |
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1m = how many um? |
1,000,000,000 um |
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1m = how many nm? |
1,000,000,000 nm |
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what is a heterogenous mixture? |
when 2 substances are mixed and you can see the two different mixtures |
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what is a homogenous mixture? |
when 2 substances are mixed and you can't see the two different mixtures (see all together as one) |
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what is a compound? |
multiple elements compounded together |
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what is an element? |
something part of the periodic table and isn't compound with any other element |
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what is gatorade? |
homogenous mixture |
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what is copper wire? |
element |
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what is beach sand? |
compound |
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identify what is the metals, non-metals & metalloids |
blue - metals gold - non-metals green - metalloids |
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expansion |
when something expands |
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diffusion |
spontaneous mixing of particles of 2 substances caused by their random motion |
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ionic crystals |
+ & - ions arranged in regular pattern |
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covalent network crystals |
each atom is covalently bonded to it's nearest neighboring atoms. bonds extend through a network including large number of atoms |
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metallic crystals |
made of metal cations surrounded by sea of aelocalized valence electrons |
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covalent molecular crystals |
consists of covalently bonded molecules held together by intermolecular forces - forces holding polar/nonpolar molecules together are much weaker than covalent chemical bonds between the atoms in a molecule |
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intensive |
independent; doesn't change when you take part of it away from the sample |
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extensive |
changes when the size of the sample changes; mass, volume, length or total charge change |
