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290 Cards in this Set
- Front
- Back
2.54 cm
|
1 inch
|
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1mL
|
1 cubic cm
|
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16 oz
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1 lb
|
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4 qts
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1 gal
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2.21 lbs
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1 kg
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.4536 kg
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1 lb
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|
.946 L
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1 qt
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1.0567 qt
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1 L
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megameters
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1 million meters
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kilometers
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1000 meters
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.1 m
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decimeter
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10 decimeters
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1 meter
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.01 m
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centimeter
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100 cm
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1 meter
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.001 m
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millimeter
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1000 mm
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1 m
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.000001 m
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micrometer
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.000000001 m
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nanometer
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10 meters cubed
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1 km
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10^-1
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decimeter
|
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10^-2
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centimeter
|
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10^-3
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millimeter
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10 exp -6
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micrometer
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10 exp -9
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nanometer
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milli
|
thousandth
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nano
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billionth
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|
micro
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millionth
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kilo
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1000
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mega
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1,000,000
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2.2046 lb
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1kg
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1 mile
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5280 ft
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.305 m
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1 foot
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.914 m
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1 yard
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.62 mi
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1 km
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1.609 km
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1 mi
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1 cubic decimeter
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1 L
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1 qt
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1/4 gal
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1 gal
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3.8 L
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1/1000 g
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1 milligram
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1/100 g
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1 centigram
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1/1000 kg
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1 gram
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1 metric ton
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1000 kg
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aluminum
|
Al
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antimony
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Sb
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argon
|
Ar
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arsenic
|
As
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barium
|
Ba
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bismuth
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Bi
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boron
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B
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bromine
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Br
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cadmium
|
Cd
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calcium
|
Ca
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carbon
|
C
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chlorine
|
Cl
|
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chromium
|
Cr
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|
cobalt
|
Co
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|
copper
|
Cu (cuprum)
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|
fluorine
|
F
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|
gold
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Au
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helium
|
He
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|
Hydrogen
|
H
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|
iodine
|
I
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|
iron
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Fe (ferrum)
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|
lead
|
Pb (plumbum)
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|
lithium
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Li
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magnesium
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Mg
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manganese
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Mn
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mercury
|
Hg
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neon
|
Ne
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nickel
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Ni
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|
nitrogen
|
N
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oxygen
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O
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phosphorus
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P
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platinum
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Pt
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potassium
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K
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radium
|
Ra
|
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silicon
|
Si
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silver
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Ag
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sodium
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Na
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strontium
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Sr
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sulfur
|
S
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tin
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Sn (stannum)
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titanium
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Ti
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tungsten
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W
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uranium
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U
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zinc
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Zn
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density
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mass divided by volume
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Ammonium
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NH4^+
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nitrite
|
NO2^-
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Sulfite
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SO3^2-
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Sulfate
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SO4^2-
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Hydrogen Sulfate/bisulfate
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HSO4^-
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Hydroxide
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OH^-
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Cyanide
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CN^-
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Phosphate
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PO4^3-
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Hydrogen phosphate
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HPO4^2-
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Dihydrogen phosphate
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H2PO4^-
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Carbonate
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CO3^2-
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Hydrogen carbonate/bicarbonate
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HCO3^-
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Hypochlorite
|
ClO^-
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Chlorite
|
ClO2^-
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Chlorate
|
ClO3^-
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Perchlorate
|
ClO4^-
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Acetate
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C2H3O2^-
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Permanganate
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MnO4^-
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Dichromate
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Cr2O7^2-
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Chromate
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CrO4^2-
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Peroxide
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O2^2-
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Polyatomic ions
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atoms which are bonded together through the sharing of electrons
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Polyatomic ions
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these unlike molecules, are charged.
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Polyatomic ions
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form ionic compounds with oppositely-charged species.
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Most polyatomic ions
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negatively charged
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ammonium is the only
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positively charged polyatomic ion
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Polyatomic ions are easy to recognize
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They will either be bonded to ammonium NH4^+ or a metal
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If you see NH4 or a metal in a compound,
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the rest of the compound is a negatively-charged polyatomic compound.
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Polyatomic nomenclature
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Cation is named first, followed by the anion
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Which two compounds have similar nomenclature?
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Polyatomic and Type I binary compounds
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What does the atomic number of a neutral atom equal to?
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its number of electrons
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How is the charge of an atom changed and what is it called after the change?
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Gain or loss of electrons
Ion |
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Ion
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The change in charge of an atom by loss or gain of electrons.
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A charged atom is called an ________
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ion
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Neutral atoms have what kind of charge?
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charge-balanced
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Neutral atoms have how many electrons compared to protons?
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Equal
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Anion
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an ion formed by gaining electrons
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What is the charge of an Anion?
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Negative
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Anions are formed by what?
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Nonmetals
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What is an ion called when it gains electrons?
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anion
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A negatively charged ion is called an ________
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anion
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nonmetals and some metalloids form_______
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anions
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What is the superscript for an anion
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-
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An atom that loses an electron
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Cation
|
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what is the charge of a cation?
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positive
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cations are formed by
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metals
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what kind of ion is formed by a metal
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cation
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what is the superscript for a cation
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+
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How many electrons in relation to protons does a cation have
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less electrons than protons
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Charges on representative metals can be predicted by their
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group numbers
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a group 2A metal will form a cation with what charge?
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2+
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How do you predict the charge of the anions for representative nonmetals?
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subtract 8 from group number
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What is the charge of the oxygen anion?
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2-
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What is the charge of the phosphorus anion?
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3-
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Cations and anions form __________.
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simultaneously
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The electron that is lost by the ______ is gained by the _______.
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metal
nonmetal |
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The result of an electron transfer is
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two oppositely-charged ions which are attracted to each other form an ionic bond.
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The electrostatic attractive force between two ions is called an ____________.
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ionic bond
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What is an ionic bond?
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the result of an electron transfer
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When an ionic bond forms between a cation and an anion
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ionic compound
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What is an ionic compound
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ionic bonds between cations and anions
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What compounds are always ionic
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metal-nonmetal
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metal-nonmetal compounds are always
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ionic
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How can ionic compounds be identified?
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by dissolving them in water
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What happens when an ionic compound is dissolved in water?
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The bonded ions dissociate from one another
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Separated ions _____________
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conduct electricity
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Why can ionic compounds be identified when dissolved in water?
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While solid the ions will not conduct electricity but when the ions separate, like all moving charges they conduct electricity
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Ionic compounds are always
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charge balanced
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charged species are energetically
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unstable
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The formula unit for an ionic compound can be predicted
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if the charges of the ions are known
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Why do ionic compounds form
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to lower the energy of the system
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Temperature
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measure of the average kinetic energy of the particles
faster particles - higher KE - higher temperature |
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Temperature reference points
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boiling and freezing points of water
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freezing point of water
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32 F
0 C 273 K |
|
boiling point of water
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212 F
100 C 373 K |
|
How many degrees between boiling and freezing
|
180 F
100 C 100 K |
|
Celsius to Kelvin conversion
|
Tk = Tc + 273.15
|
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Celsius to Fahrenheit conversion
|
Tf= 1.8 Tc + 32
|
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Fahrenheit to kelvin conversion
|
Tf-32/1.8= Tc + 273.15
|
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Density
|
mass/volume
|
|
Standard liquid units
|
g/mL
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standard solid units
|
g/cm^3
|
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standard units for gases
|
g/L
|
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Matter
|
anything that has mass and occupies space
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|
Three states of matter on earth
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solid, liquid, gas
|
|
fourth state of matter
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plasma
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solid
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fixed shape and volume
|
|
liquid
|
definite volume
takes the shape of its container |
|
gas
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no fixed shape or volume
takes the shape and volume of its container |
|
inter-particle forces
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hold particles together
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what holds particles together
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inter-particle forces
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solids have a high degree of
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order
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what state of matter has the highest degree of order
|
solids
|
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solids have _______ KE and PE
|
low
|
|
what is kinetic energy
|
energy of motion
|
|
low KE indicates a
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positive value with a small magnitude
|
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particles in fixed positions have
|
low kinetic energy
|
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What state of matter has low KE and PE
|
solids
|
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Low potential energy
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stable
|
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Why do solids form inter-particle attractive forces
|
lowers the PE
|
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what is one of the universal driving forces
|
an natural tendency to seek the lowest energy state available
|
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Particles in the liquid state
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Flow
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Particles in the liquid state have more __________ energy than solids.
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kinetic & potential
|
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In the _____ phase there are no inter-particle attractive forces.
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gas
|
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gas phase is characterized by a high degree of
|
disorder
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low KE, PE and order
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Solids
|
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More KE, PE and less order
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liquids
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high KE, PE and disorder
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Gas
|
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Formation of attractive forces lowers the ________ of a system
|
energy
|
|
____________________ lowers the energy of a system.
|
Formation of attractive forces
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Phase changes
|
physical changes
|
|
Physical changes are also called
|
Phase changes
|
|
The makeup of a substance is not changed
|
physical change
|
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Phase changes occur with an ____________ between the system and it's surroundings
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Energy exchange
|
|
What occurs with an energy exchange?
|
Phase changes
|
|
Ke and PE __________ between the solid to liquid to gas phase
|
increase
|
|
If KE and PE increases energy is being __________.
|
absorbed
|
|
energy absorbed increases
|
KE and PE
|
|
absorption of energy
|
endothermic
|
|
endothermic
|
absorption of energy
|
|
endothermic phase changes
|
solid to liquid to gas
|
|
Release heat
|
exothermic
|
|
ke and pe decrease in an
|
exothermic process
|
|
exothermic process phase changes
|
gas to liquid to solid
|
|
endothermic - name
|
melting, vaporizing, sublimation
|
|
exothermic - name
|
condensation, freezing, deposition
|
|
Endothermic processes occur
|
with the absorption of heat by the system from the surrounding
|
|
Exothermic processes occur
|
with the release of heat from the system to the surroundings
|
|
the formation of every kind of attractive force
|
lowers the energy of the system
|
|
formation of attractive forces is an__________ process
|
exothermic
|
|
reverse of exothermic
|
endothermic
|
|
disrupting attractive forces
|
endothermic
|
|
Chemical changes occur with an ______________.
|
energy exchange
|
|
Chemical changes ___________ the identity of a substance.
|
change
|
|
signs of a chemical change
|
color change
formation of a solid bubble odor flame production |
|
Chemical reactions are represented using
|
chemical equations
|
|
reactant
|
original substance
|
|
products
|
new substances
|
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Thermal equilibrium
|
heat flows from hot to cold
|
|
Chemical properties describe
|
how a substance interact with other substances
|
|
When chemical changes occur the products have ____________
|
very different properties
|
|
two types of substances in nature
|
elements
compounds |
|
compounds are made up of
|
two or more different elements
|
|
compounds can only be broken down to elements by
|
chemical processes
|
|
naturally occurring elements
|
gold (elemental)
oxygen iron carbon Neon (elemental) |
|
uncombined elements
|
generally unreactive
|
|
compound examples
|
water
table salt sugar carbon dioxide |
|
are properties of a compound related to the elements that compose it
|
no
|
|
Same chemical composition at all times
|
compounds
|
|
Law of constant composition
|
compounds have the same composition at all times
|
|
pure substances
|
elements and compounds
|
|
always have the same compostion
|
pure substances
|
|
mixtures
|
combination of pure substances
|
|
mixture phases
|
solid, liquid or gas
|
|
Air is a gas phased ___________ of __________.
|
mixture of pure substances
|
|
gold jewelry is an example of what
|
solid phase mixture containing pure substances
|
|
Homogeneous mixture
|
look the same throughout
|
|
homogenous mixture is also called
|
solution
|
|
another name for a solution
|
homogeneous mixture
|
|
Homogeneous quality is not limited to
|
appearance
|
|
heterogeneous mixture
|
mixtures which look different throughout
|
|
pure substances are seperated by
|
physical processes
|
|
Examples of physical processes
|
filtration
distillation |
|
Chemistry
|
the science that deals with the materials of the universe and the changes these materials undergo
|
|
Central science
|
Basic understanding of chemistry is necessary for other scientific disciplines
|
|
5 specialty areas
|
organic
inorganic physical Bio analytical |
|
Scientific method
|
observations
hypothesis test hypothesis adopt theory |
|
length
|
meter
|
|
volume
|
liter or cubic meter
|
|
mass
|
gram or kilogram
|
|
time
|
second
|
|
temperature
|
celsius or kelvin
|
|
precision is an indicator of
|
reliability of the measurement
|
|
Sig figs addition and subtraction
|
the least precise number
|
|
SIg figs multiplication and division
|
least number of sig figs
|
|
What are the first and second most abundant element in the universe?
|
Hydrogen and helium
|
|
Elements except for Hydrogen and helium are formed by
|
nuclear fusion
|
|
Nuclear fusion
|
fusion of small atoms to make larger ones
|
|
On earth, elements made by nuclear fusion are called _________, and are _____ abundant than hydrogen
|
heavy elements
more |
|
almost half of the atoms found on earth
|
oxygen
|
|
most common element in the human body
|
oxygen
|
|
protons and neutrons have roughly the same
|
mass
|
|
Neutrons have no
|
charge
|
|
protons and neutrons in the nucleus are called
|
nucleons
|
|
electrons have ________ masses
|
negligible
|
|
proton symbol
|
p or p^0
|
|
neutron symbol
|
n or n^0
|
|
electron symbol
|
e-
|
|
masses of three subatomic particles are compared to the mass of the ________ atom
|
carbon
|
|
nitrite
|
NO2^-
|
|
HI
|
hydroiodic acid
|
|
HCL
|
hydrochloric acid
|
|
HBr
|
hydrobromic acid
|
|
HNO3
|
nitric acid
|
|
HNO2
|
nutrous acid
|
|
H2SO4
|
sufuric acid
|
|
H2SO3
|
sulfurous acid
|
|
H2CO3
|
carbonic acid
|
|
H3PO4
|
phosphoric acid
|
|
HCLO3
|
chloric acid
|
|
HClO2
|
Chlorous acid
|
|
CH3COOH
|
Acetic acid
|
|
HClO4
|
perchloric acid
|