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honors chem sem. 1 final
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matter
the stuff that makes the universe is composed of
elements
substances that only contain
ONE
type of atom
ex
: P
compounds
substances that are made by bonding (chemicaly)
DIFFERENT
atoms together in specific amounts
molocules
a collection of atoms bonded together as a unit
physical change
change that does not effect the composition of a substance
chemical change
a change in which a substance becomes a different substance
mixture
a substnace with variable composition
pure substances
always have the same composition
(cannot be physically separated into physical parts)
distilation
separation process that depends on the boiling point of substances
filtration
separation of a solid and a liquid by using filter paper
proton
+1 charge
located in nucleus
1 AMU
electron
-1 charge
in electron cloud
0 AMU
neutron
0 charge
located in nucleus
1 AMU
isotopes
atoms with the same # of protons but different # of neutrons
Radioactive decay
radioactive isotopes that have an unstable nuclei that emist particles means that the isotope is going through...
alpha particle reduction
a helium nucleus is produced in this type of radioctive decay
beta particle reduction
high speed electrons are produced from the nulceus
(add a proton)
gama ray relesase
a high enery pronton of light compostion id produces in this type of radioactive decay
fission
the process of slpitting a heavy nucleus into 2 or more stable nuclei with a smaller mass is produced in this tyoe of nuclear energy production
fusion
the process of combining 2 light nuclei to form a heavier more stable nucleus (nuclear energy production)
diatomic molocules
hydrogen
oxygen
nitrogen
flourine
chlorine
bromine
iodine
dmitri mendeleev
arranged elements in the periodic table based on similar properties
allotrope
different structural modification of an element
valence electrons
electrons located in the outermost shell of an element molocule or compound
cations
(positive) metals that tend to lose one or more electrons to form positive ions
anions
(negative) nonmetals that tend to gain 1 or more electrons
half life
the time required for 1/2 of the original sample of radiocative nuclides to decay
acid
a substance that produces hydrogen ions in solution
hydrolic acid
HCl
sulfuric acid
H
2
SO
4
nitric acid
HNO
3
phosphoric acid
H
3
PO
4
acetic acid
HC
2
H
3
O
2
formula unit
the formula unit shows the elements present in the smallest whole number ratios
molecular formula
formula unit that shows the acutal numbers of atoms in a molocule
formula mass
mass in atomic units (AMU) of an ionic compunds empirical formula
molecular mass
mass in atomic units (amu) of a molecular compound's molecular formula
molar mass
mass in grams of 1 mole
conversion poathway
mass<-->moles<-->particles
percent composition
percent of a compounds mass made up of its constituent elements
part over whole * 100
empirical formula
lowest whole # ratio of atoms in a formula unit (ionic)
3 steps to solve empirical formulas
1. the % becomes the mass amount
2. convert grams to moles for esch element
find the lowest whole # ratio by dividing by the smallest amound or #
hydrates
a molocule that contains some type of water
4 signs of a chemical reaction
emmision of gas
color change
frmation of precipitate
energy in form of light/heat
why chemical reactions occur
formations of a solid
formation of water
transfer of electrons
formation of gas
storng acid
an acid in which virtually every mollocule dissociates in water to create an H
+
ion and an anion
strong acid examples
HCl
HNO
3
H
2
NO
3
strong base
a metal hydroxide that is completely soluble in watergiving separate OH
-
ions and cations
examples of strong bases
NaOH
KOH
single displacment
a single atom reacts with a compound and replaves one of the elements in the compound
double displacment
2 ionic compounds exchange ions to form new compounds
combustion reactions
a chemical reaction involving oxygen as a reactant that produces enough heat that a flame results
synthesis
a chem reaction in which a compound is formed from simpler materials
decomposition
single reactent is broken down into 2 or more simple compounds or elements
stoichiometry
relative quantaties of reactants and products involved in the reaction
mole ratio
this is indicated by coefficients in a balanced equation
steps to solve a stoichiometry problem
1. write a balanced equation
2. identify knowns and unknowns
3. use fence and rail
4. check answer
limiting reactant
determines how much of each product can be made
excess reactant
this is added to ensure that the other reactant is completly used up
steps to solving a limiting reactant
1. recognize the limitiong reactant
2. perform a gram-to-gram stoichiometry problem on the first reactant
3. repeat on second reactant
4. look at which calculation gave you the least ammount of product formed
theoretical yiled
ammount of product that shoule be make with an equation
actual yield
the amount of a product actually produced
percent yield
percent for theoretical yiled actualy produced
cyanide
CN
-1
peroxide
O
2
-2
permanaganate
M
2
O
4
-1
hydroxide
OH
-1
ammonium
NH
4
+1
acetate
C
2
H
3
O
2
-1
hydrogen carbonate
HCO
3
-1
carbonate
CO
3
-2
perchlorate
ClO
4
-1
Hypochlorate
ClO
-1
chlorate
ClO
2
-1
dichromate
Cr
2
O
7
-2
chromate
CrO
7
-2
nitrate
NO
3
-1
nitrite
NO
2
-1
hydrogen phosphate
HPO
4
-2
dihydrogen phosphate
H
2
PO
4
-2
phosphate
PO
4
-3
sulfate
SO
4
-2
sulfite
SO
3
-2
Hydrogen sulfate (bisulfate)
HSO
4
-1
Author:
phreddie
ID:
122492
Card Set:
honors chem sem. 1 final
Updated:
2011-12-10 20:54:58
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