Term
|
Definition
the study of
1) composition
2) structure
3) properties and
4) changes
of matter |
|
|
Term
|
Definition
| that with finite shape and volume (ie, occupies space) |
|
|
Term
| What is Mass, what is Weight? |
|
Definition
Mass: a quantity of matter
Weight: is dependent on the potential field |
|
|
Term
| Law of conservation of mass/ matter |
|
Definition
"the total mass remains concstant during a chemical change/ reaction"
stated another way:
"Matter is neither created nor destroyed in a chemical reaction; it is just moved around" |
|
|
Term
|
Definition
rigid, incompressible (can't manipulate volume), fixed shape and volume
ex: ice |
|
|
Term
|
Definition
relatively incompressible fluid (fluid: no fixed shape, flows), fixed volume, no fixed shape
ex: water |
|
|
Term
|
Definition
easily compressible (compressible: volume can be manipulated) fluid (fluid: no fixed shape, flows), sample will fit into container of any size or shape; no fixed volume or shape
ex: steam |
|
|
Term
| physical change/ change of state |
|
Definition
change in the form of matter but not in the chemical identity
ex: change of state (melt ice, boil water)
dissolution (dissolving kool aid powder in water)
distillation (moon shine; boil mixture, it vaporizes, encounters a condensor, condenses back to liquid, is collected in a receiver) |
|
|
Term
|
Definition
change in which one or more kinds or matter are transformed into a new kind of matter or several new kinds of matter
ex: 2Na+ Cl --> 2NaCl |
|
|
Term
| test for chemical versus physical change |
|
Definition
original components cannot be reclaimed by physical means (chemical reaction; ex: bake a cake, if you freeze it, it wont turn back into the chocolate, flour, ect. you put in)
original components can be reclaimed by physical means
(physical change; ex: had ice, melted it, can freeze it to restore it to original state) |
|
|
Term
|
Definition
cannot use physical means to separate into other kinds of matter
possesses definitie intensive (independent of amount) physical and chemical properties
ex: color |
|
|
Term
|
Definition
cannot be decomposed by any chemical means into simpler substances; building blocks of matter
ex: K, Cl, Na, O, ect. |
|
|
Term
| Who receives credit for the periodic table? |
|
Definition
|
|
Term
| how did Mendeleev arrange the periodic table |
|
Definition
|
|
Term
| how is the periodic table arranged today? |
|
Definition
|
|
Term
|
Definition
number of protons in nucleus;
chemical identity is linked to the number of protons
ex: add a proton to Na and it becomes Mg |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
substance or mixture characterized by luster (shine) and generally a good conductor of heat and electricity
most solid at room temp, except for Hg
malleable ( hammered into a shape; changable) and ductile (drawn into wire; not brittle) |
|
|
Term
|
Definition
element that doesn't exhibit characteristics of a metal
most are gases (ex: N, O) or solids (ex: P, S)
solids are hard and brittle (shatter when hit)
only liquid nonmetal at room temperature is Br) |
|
|
Term
|
Definition
elements possessing both metallic and nonmetallic properties; properties depend on what they react with (react w/ metal, acts as nonmetal, vice versa)
ex: Si and Ge (semiconductors)
when pure, poor conductors of electricity; when doped (impure), or at high temps, become good conductors of electricity |
|
|
Term
|
Definition
| physical, extensive, intensive, chemical |
|
|
Term
|
Definition
| characteristic of material that can be observed without altering its chemical identity (ex: color, mass, density, state) |
|
|
Term
|
Definition
dependent on amount
ex: mass |
|
|
Term
|
Definition
independent of amount
ex: color |
|
|
Term
|
Definition
characteristic of material involving its chemical change
reactivity (how much it reacts) |
|
|
Term
| le systeme international d'unites |
|
Definition
SI units
common/ standard units |
|
|
Term
SI base units:
quantity: Length
unit? symbol? |
|
Definition
|
|
Term
|
Definition
kilogram (often use gram)
kg (g) |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
SI Prefixes:
Multiple: 10^6
prefix?
symbol? |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
how do you use SI prefixes?
what do they indicate? |
|
Definition
augment base units with prefixes
prefixes indicate the power of 10 that you multiply the base unti by
ex: kg= 10^3g= 1,000g |
|
|
Term
celsius scale:
bp of water?
fp of water? |
|
Definition
|
|
Term
Kelvin scale:
lowest theoretical temp?
h2O fp?
h2O bp? |
|
Definition
lowest: 0 K
fp: 273 K
bp: 373 K |
|
|
Term
fahrenheit scale
h2O fp?
h2o bp? |
|
Definition
|
|
Term
temp conversions
celsius to Kelvin |
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
volume units
length x length x length |
|
Definition
m^3 = 1,000 L
1L = dm^3 = 10^3 cm^3
1 cm^3 = cc= 1 mL |
|
|
Term
|
Definition
|
|
Term
density formula?
density formula units? |
|
Definition
d= m/V
units: g/cm^3
ex: H2O d=1g/cm^3 |
|
|
Term
relative densities:
density generally ______ as you change from solid to liquid to gas
exception? |
|
Definition
density generally DECREASES as you change from solid to liquid to gas
exception: H2O; ice (0.92 g/cm^3), water (1 g/cm^3), gas (6x10^-4 g/cm^3) |
|
|
Term
|
Definition
| "the potential or capacity to do work or heat transfer" |
|
|
Term
|
Definition
w=F x d
work = force x distance |
|
|
Term
units of energy?
(unit of energy, work, heat) |
|
Definition
| the Joule: 1J = (1kg*m^2)/s^2 |
|
|
Term
|
Definition
the energy required to raise the temperature of 1g of H2O by 1 degree C
1 cal = 4.184 J |
|
|
Term
|
Definition
Kinetic energy = 1/2 mass * velocity squared
KE = 1/2 mv^2
energy of an object by virtue of its motion |
|
|
Term
|
Definition
potential energy of an object by virtue of its position in a field of force
ex: gravity --> PE=mgh |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
| all types of energy (KE,PE,U,E total) are relative values based on______ |
|
Definition
a reference point
ex: the floor for PE; 0 velocity for KE |
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
