Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
127 Cards in this Set
- Front
- Back
|
Specific heat of water
|
1.00 ca/g *C
|
|
|
Specific heat of Aluminum (Al)
|
0.21 cal/g *C
|
|
|
Specific heat of Copper (Cu)
|
0.092 cal/g *C
|
|
|
Specific heat copacity is measured in what units
|
cal/g *C
|
|
|
Molar heat of fusion formula
|
Heat= (mass)(Cp)(delta T)
Calories= g x cal/g*C x *C |
|
|
specific heat formula
|
Cp= heat/(mass x delta T)
|
|
|
Percent error formula
|
theoretical value - experimental value/ theoretical value x 100
|
|
|
Cs
|
q/m x delta T
|
|
|
specific heat of water in Joules
|
4.18 J/g-K
|
|
|
q=
|
Cs x m x delta T
|
|
|
the measure of heat flow
|
calorimetry
|
|
|
device used to measure heat flow
|
calorimeter
|
|
|
Enthalpy formula is delta H=
|
Hproducts - Hreactants
|
|
|
enthalpy
|
thermodynamic function
|
|
|
pressure-volume work
|
w= -P delta V
|
|
|
state function
|
property of a system that is determined by specifying the system's condition, or state (in terms of temperature & pressure)
|
|
|
state function depends on only what?
|
the pressent state of the system, not on the path the system took to reach that state
|
|
|
delta E =
|
q + w
q=heat positive=gains negatives=loss w= positive=work done on system negative=work done by system delta E= positive= net gain energy negative=net loss of energy |
|
|
exothermic
|
a process which a system losses heat
|
|
|
endothermic
|
a process which a system absorbs heat
|
|
|
change in internal energy
|
delta E= Efinal - Einitial
|
|
|
internal energy
|
sum of all the kinetic and potential energies
|
|
|
first law of thermodynamics
|
energy is conserved
|
|
|
kenetic energy
|
energy of motion
|
|
|
Ek=
|
1/2 mv^2
|
|
|
potential energy
|
energy that can be produced by force
|
|
|
force
|
a push or pull exerted on an object
|
|
|
Molarity=
|
moles solute/volume of solution in liters
|
|
|
Mconc x Vconc=
|
Mdil x Vdil
|
|
|
M1 x V1=
|
M2 x V2
|
|
|
an aton in its elemental form has what oxidation number?
|
zero
|
|
|
a monatomic ion oxidation number equals what?
|
the charge on the ion
K+ has oxidation number of +1 |
|
|
nonmetals have what oxidation numbers
|
negative
|
|
|
sum of oxidation numbers in a neutral compound is?
|
zero
|
|
|
loss of electrons by a substance is called?
|
oxidation
|
|
|
oxidation-reduction is also known as what?
|
redox reactions
|
|
|
base
|
substance that accepts (reacts with) H+ ions
|
|
|
bases produce what?
|
hydroxide ions (OH-) when dissolve in water
|
|
|
acid
|
substance that ionizes in aqueous solutions
|
|
|
acids produce what?
|
hydrogen H+ ions
|
|
|
spectator ions
|
ions that are the same on both sides of an equation
|
|
|
precipitant
|
insoluble solid formed by a reaction
|
|
|
strong electrolyte
|
solutes that exist in solution completely as ions
|
|
|
weak electrolyte
|
solutes that exist in solution mostly in the form of molecules w/only a small fraction in the form of ions
|
|
|
NaCl is what type of electrolyte?
|
strong electrolyte
|
|
|
CH3COOH is what type of electrolyte?
|
weak electrolyte
|
|
|
solvent
|
substance with greatest quantity
|
|
|
solute
|
substances that are not the greatest quantity
|
|
|
aqueous solution
|
a solution in which water is the dissolving medium
|
|
|
% element =
|
(number of atoms)(atomic weight)/formula weight of compound x 100%
|
|
|
% yield =
|
(actual yield)/(theoretical yield) x 100%
|
|
|
limiting reactant
|
complete consumption of this stops the reaction, because it's all used up
|
|
|
theoretical yield
|
product calculated when all the limiting reagent reacts
|
|
|
percent yield compares what?
|
actual & theoretical yield
|
|
|
stoichiometry
|
quantitive relationships between chemical formulas and chemical equations
|
|
|
combination reaction
|
two reactants combine to form one product
A + B = AB |
|
|
decomposition reaction
|
a single reactant forms two or more products
AB= A + B |
|
|
compustion reaction in oxygen
|
compound reacts with O2 to form CO2 and H2O
|
|
|
Avogadro's number
|
(6.02 x 10^23)
|
|
|
molar mass
|
formula weigh (g) of the material
|
|
|
formula weight
|
sum of atomic weights of the atoms in its formula
|
|
|
molecular weight
|
another name for formula weight
|
|
|
converting grams to moles
|
(g)(1 mole/molecular weight)
|
|
|
converting moles to grams
|
(moles)(g/1 mole)
|
|
|
calculating molar mass
|
sum of all atomic weights in compound
|
|
|
converting moles to atoms
|
moles(6.02 x 10^23/1 mole)(atoms/1 mole)
|
|
|
% composition
|
% by mass, of each element in compound
|
|
|
calculating % composition
|
%element= molar weight/formula weight x 100%
|
|
|
reactants
|
compounds left of the equation
|
|
|
products
|
compounds right of the equation
|
|
|
alkanes have what at the end?
|
-ane
|
|
|
alkanes are also know as what?
|
hydrocarbons
|
|
|
mono-
|
1
|
|
|
Di-
|
2
|
|
|
Tri-
|
three
|
|
|
Tetra-
|
4
|
|
|
Penta-
|
5
|
|
|
Hexa-
|
6
|
|
|
Hepta-
|
7
|
|
|
Octa-
|
8
|
|
|
Nona-
|
9
|
|
|
Deca-
|
10
|
|
|
acids containing anions are named by doing what?
|
changing the -ide to -ic and adding prefix hydro-
|
|
|
ionic compounds consist of
|
cation name followed by the anion name
|
|
|
polyatomic anions containing oxygen have names ending in what?
|
-ate
-ite |
|
|
oxyanions
|
polyatomic anions ending in -ate or -ite
|
|
|
ionic compound
|
contains positively and negatively charged ions
|
|
|
polyatomic ions consist of what?
|
ions of atoms joined as a molecule, but have a net positive or negative charge
|
|
|
ion
|
a charged particle
|
|
|
cation
|
positive charged ion
|
|
|
anion
|
negatively charged ion
|
|
|
alkali metals group
|
1A
|
|
|
Alkaline earth metals group
|
2A
|
|
|
Chalcogens group
|
6A
|
|
|
Halogens group
|
7A
|
|
|
Noble gases group
|
8A
|
|
|
atoms are made of
|
protons, electrons, and neutrons
|
|
|
most mass in atom is located where?
|
nucleous
|
|
|
protons are equal to what
|
neutrons
|
|
|
neutrons are equal to what
|
protons
|
|
|
Dalton atomic theory claimed what
|
atoms are the smallest particles of an element that retain the chemical identity of the element
|
|
|
law of conservation
|
matter is neither created nor distroyed-----what was present before must be present after
|
|
|
K=
Kalvin |
*C + 273.15
|
|
|
*C=
Celcius |
5/9(*F - 32)
|
|
|
*F=
Fahrenheit |
9/5(*C+32)
|
|
|
Density=
|
mass/volume
|
|
|
mass =
|
density x volume
|
|
|
volume =
|
density/mass
|
|
|
D= m/V
|
formula for density
|
|
|
20.42 has how many sig figs
|
2
|
|
|
1.322 has how many sig figs
|
3
|
|
|
83.1 has how many sig figs
|
1
|
|
|
1.03 x 10^ 4 has how many sig figs
|
3
|
|
|
1.030 x 10^ 4 has how many sig figs
|
4
|
|
|
1.0300 x 10^ 4 has how many sig figs
|
5
|
|
|
zeros at beginning of number
|
are never significant
|
|
|
elements cannot be
|
decomposed into simpler substances
|
|
|
compounds
|
substances composed of 2 or more elements
|
|
|
gas
|
has no fixed volume or shape
|
|
|
liquid
|
has distinct volume, and takes shape of what holds it
|
|
|
solid
|
has definite shape and volume
|
|
|
matter comes in how many states?
|
3
|
|
|
chemisty is the study of
|
properties and behavior of matter
|
|
|
physical property
|
color, odor, density, melting point, boiling point, and hardness
|
|
|
chemical property
|
the way a substance may change/react to form another substance.
example= flammability |
|
|
temperature, melting point, and density are known as what properties?
|
intensive properties
|
|
|
extensive properties
|
mass and volume
=how much |
