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239 Cards in this Set
- Front
- Back
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HYDROGEN
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H
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HELIUM
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He
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LITHIUM
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Li
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BERYLLIUM
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Be
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BORON
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B
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CARBON
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C
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OXYGEN
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O
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NITROGEN
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N
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FLUORINE
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F
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NEON
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Ne
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SODIUM
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NA
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MAGNESIUM
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Mg
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ALUMINIUM
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AL
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SILICON
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Si
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PHOSPHOROUS
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P
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CHLORINE
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Cl
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SULFUR
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S
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ARGON
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Ar
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POTASSIUM
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K
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CALCIUM
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Ca
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CHROMIUM
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Cr
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MANGANESE
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Mn
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IRON
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Fe
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NICKEL
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Ni
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COPPER
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Cu
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ZINC
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Zn
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BROMINE
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Br
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RUBIDIUM
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Rb
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STRONTIUM
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Sr
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SILVER
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Ag
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TIN
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Sn
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IODINE
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I
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MERCURY
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Hg
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BARIUM
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Ba
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LEAD
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Pb
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COVALENT BONDS
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SHARING ELECTRONS. IT MAKES A MOLECULE.
NONMETAL AND NONMETAL |
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IONIC BONDS
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COMPLETE TRANSFER OF ELECTRON
METAL TO NON METAL TABLE SALT |
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ATOMIC NUMBER
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NUMBER OF PROTONS
BOTTOM NUMBER-IT NEVER CHANGES |
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IN A NEUTRAL ATOM THE
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PROTONS AND ELECTRONS HAVE EQUAL OPPOSITE CHARGES.
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ISOTOPES HAVE SAME____AND MORE OR LESS_______
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SAME PROTONS AND ELECTRONS THE NEUTRONS CHANGE IN AN ISOTOPE.
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MASS_______ATOMIC NUMBER IS NEUTRONS
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MINUS
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LAW OF MULTIPLE
PROPORTIONS |
TWO OR MORE ELEMENTS MUST BE SAME ELEMENTS IN DIFF PROPORTIONS
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LAW OF MULTIPLE PROPORTIONS
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NH4 AND NH4CL
ZNO2 AND ZN CL2 NO AND NO2 ******* CH4 AND CO 2 |
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LAW OF MULTIPLE PROPORTIONS
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SO AND SO2 *******
H2O AND C12H2O11 H2SO4 AND H2S KCL AND PCLO2 |
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DALTON'S THEORY
KNOW BY HEART |
EACH ELEMENT MADE UP OF TINY PARTICLES
THE ATOMS OF A GIVEN PARTICLE ARE IDENTICAL |
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DALTONS THEORY CONT.
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CHEMICAL COMPOUNDS ARE FORMED WHEN ATOMS COMBINE WITH EACHOTHER
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DALTONS THEORY C
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CHEMCIAL REACTION INVOLVE REORGANIZATION OF THE ATOMS.
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Which one of the following is not one of the postulates of Dalton’s atomic theory?
Each element is composed of tiny, indivisible particles called atoms All atoms of a given element are identical to each other and different from those of other elements During a chemical reaction, atoms are changed into atoms of different elements Compounds are formed when atoms of different elements combine Atoms of an element are not changed into different types of atoms by chemical reactions |
DURING A CHEMICAL REACTION ATOMS ARE CHANGED INTO ATOMS OF DIFFERENT ELEMENTS
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Which one of the following is not one of the postulates of Dalton’s atomic theory?
Atoms are composed of protons, neutrons and electrons All atoms of a given element are identical; the atoms of different elements are different and have different properties Atoms of an elements are not changed into different types of atoms by chemical reactions: atoms are neither created nor destroyed in chemical reactions Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms Each element is composed of extremely small particles called atoms |
ATOMS ARE COMPOSED OF PROTONS,NEUTRONS, AND ELECTRONS
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WHAT DID JJ THOMSON DO
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POSTULATED THE EXSISTENCE OF ELECRONS(USING THE CATHODE RAY TUBE) AND SAID THEY WERE - CHARGED AND HE DETERMINED CHARGE TO MASS RATIO.
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JJ THOMSON
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KNEW ELECTRONS WERE NEGATIVELY CHARGED AND THAT THERE WAS A CHARGE TO MASS RATIO
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ROBERT MILLIKEN DETERMINED
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THE ACTUAL CHARGE TO MASS RATION AND THE MASS OF AN ELECTRON
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RUTHERFORD WANTED PROVE THE PLUM PUDDING THEORY
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PROVED INSTEAD IT WASN'T RIGHT BECAUSE THE BEAM DIDN'T GO DIRECTLY THROUGH, AND SO DISCOVERED THE NUCLEUS
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RUTHERFORD IS RESPONSIBLE FOR THE
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MODERN VIEW OF THE ATOM
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. The first scientist to show that atoms emit any negative particles was
a) J. J. Thomson. b) Lord Kelvin. c) Ernest Rutherford. d) William Thomson. e) John Dalton |
J J THOMSON
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The scientist whose alpha-particle scattering experiment led him to conclude that the nucleus of an atom contains a dense center of positive charge is
a) J. J. Thomson. b) Lord Kelvin. c) Ernest Rutherford. d) William Thomson. e) John Dalton |
RUTHERFORD
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. Rutherford’s experiment was important because it showed that:
a) radioactive elements give off alpha particles. b) gold foil can be made to be only a few atoms thick. c) a zinc sulfide screen scintillates when struck by a charged particle. d) the mass of the atom is uniformly distributed throughout the atom. e) an atom is mostly empty space |
THE ATOM IS MOSTLY EMPTY SPACE
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PERIODIC TABLE TO THE LEFT OF THE STAIR STEP IS _____ AND THE RIGHT IS
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TO THE LEFT IS METALS AND THE RIGHT IS NON-METALS
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THE RIGHT OF THE STAIR STEP HAD _______BONDING
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COVALENT IS METAL TO METAL WHICH IS ALSO MOLECULES
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THE LEFT OF THE STAIR STEP HAS _______BONDING
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IONIC BONDING IS NONMETAL TO METAL
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IN THE PERIODIC TABLE WHICH COLUMNS ARE THE MAIN GROUP ELEMENTS
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1ST TWO AND LAST 6
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THE MIDDLE BLUE PORTIONS OF THE TABLE IS CALLED WHAT
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TRANSITION METALS
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WHAT ARE THE BOTTOM TWO ROWS OF THE PERIODIC TABLE CALLED
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RARE EARTH MINERALS
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CATION
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POSITIVE ION
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ANION
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NEGATIVE ION
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IONIC BONDING
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FORCE OF ATTRACTION BETWEEN OPPOSITLY CHARGED IONS.
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ELEMENTS ARE CLASSIFIED BY
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PROPERTIES AND ATOMIC NUMBER
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GROUPS ARE VERTICAL OR HORIZONTAL
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VERTICAL
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1A
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ALKALI METALS
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2A
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ALKALI EARTH METALS
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7A
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HALOGENS
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8A
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NOBLE GASSES
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PERIODS ARE HORIZONTAL OR VERITCAL
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HORIZONTAL
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THE NUCLEUS IS VERY SMALL AND CONTAINS
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ALMOST ALL OF THE MASS OF THE ATOM
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THECHEMISTRY FROM THE ATOM RESULTS FROM ITS
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ELECTRONS
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ELECTRON MAKE UP MOST OF THE ____________ OF AN ATOM
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VOLUME
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THE ______AND __________ OF THE ELECTRON IS WHAT GIVES VARIATION TO AN ATOM
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NUMBER AND ARRANGEMENT
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HALOGENS NEED TO GAIN OR LOSE AN ELECTRON TO BE LIKE A NOBEL GASS
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HALOGENS NEED TO GAIN, THAT MEANS LOSE 1 ELECTRON
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THE CHARGE FOR THE ENTIRE HALOGEN COLUMN IS
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-1 THAT MEANS THAT GAIN 1 ELECTRON
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THE OXYGEN COLUMN NEEDS TO GAIN OR LOSE
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OXYGEN NEEDS TO GAIN 2 ELECTRONS SO THEY ARE
-2 |
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NITROGEN NEEDS TO GAIN OR LOSE HOW MANY ELECTRONS TO BE PURE
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NITROGEN NEEDS TO GAIN 3, WHICH IS -3
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CARBON NEEDS TO GAIN OR LOSE HOW MANY ELECTRONS
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CARBON NEEDS TO GAIN 4
WHICH IS -4 |
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DO THE METALS NEED TO GAIN OR LOSE ELECTRONS TO BE MORE LIKE THE NOBLE GASSES?
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THE METALS NEED TO LOSE ELECTRONS WHICH MEANS +1,+2,+3
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BINARY COMPOUNDS
USE ELEMENTAL NAME FOR THE 1ST ELEMENT AND 2ND ELEMENT END "IDE" |
COMPOSED OF ATOMS OF 2 DIFFERENT ELEMENTS-TWO METALS FAR RIGHT OF TABLE
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1, 2, 3, 4, 5, 6, 7
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MONO,DI,TRI,TETRA,PENTA,HEXA,HEPTA
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BINARY COMPOUND METAL AND A NONMETAL
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NAMED METAL FIRST AND THEN NONMETAL "IDE" ON THE END OF NONMETAL
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NH4+
POLYATOMIC IONS |
AMMONIUM
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CN-
POLYATOMIC IONS |
CYANIDE
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OH-
POLYATOMIC IONS |
HYDROXIDE
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H*
CATIONS |
HYDROGEN
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Li+
CATIONS |
LITHIUM
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NA+
CATIONS |
SODIUM
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K+
CATIONS |
POTASSIUM
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Rb*
CATIONS |
RUBIDIUM
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Mg2+
CATIONS |
MAGNESIUM
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Ca2+
CATIONS |
CALCIUM
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Sr2+
CATIONS |
STRONTIUM
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Ba2+
CATIONS |
BARIUM
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Al3+
CATIONS |
ALUMINUM
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Ni2+
CATIONS |
NICKEL
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ZN2+
CATIONS |
ZINC
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FE3+
CATIONS |
IRON III OR FERRIC
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FE2+
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IRON II OR FERROUS
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Cu2+
CATIONS |
COPPER II OR CUPRIC
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Cu1+
CATIONS |
COPPER I OR CUPROUS
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Pb4+
CATIONS |
LEAD (IV) OR PLUMBIC
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Pb2+
CATIONS |
LEAD II OR PLUMBOUS
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Sn4+
CATIONS |
TIN IV OR STANNIC
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Sn2+
CATIONS |
TIN II OR STANNOUS
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Hg2+
CATIONS |
MERCURY II OR MERCURIC
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ZN2+
CATIONS |
ZINC
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FE3+
CATIONS |
IRON III OR FERRIC
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FE2+
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IRON II OR FERROUS
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Cu2+
CATIONS |
COPPER II OR CUPRIC
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Cu1+
CATIONS |
COPPER I OR CUPROUS
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Pb4+
CATIONS |
LEAD (IV) OR PLUMBIC
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Pb2+
CATIONS |
LEAD II OR PLUMBOUS
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Sn4+
CATIONS |
TIN IV OR STANNIC
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Sn2+
CATIONS |
TIN II OR STANNOUS
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Hg2+
CATIONS |
MERCURY II OR MERCURIC
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F-
ANIONS |
FLUORIDE
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Cl-
ANIONS |
CHLORIDE
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Br-
ANIONS |
BROMIDE
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I-
ANIONS |
IODIDE
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H-
ANIONS |
HYDRIDE
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O2-
ANIONS |
OXIDE
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S2-
ANIONS |
SULFIDE
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N3-
ANIONS |
NITRIDE
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P3-
ANIONS |
PHOSPHIDE
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C4-
ANIONS |
CARBIDE
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TERNARY COMPOUNDS
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COMPOSED OF 3 OR MORE COMPOUNDS-USUALLY NEGATIVE IONS CALLED POLYATOMIC IONS
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MnO4-
POLYATOMIC IONS |
PERMANGANATE
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C2H3O2-
POLYATOMIC IONS |
ACETATE
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NO3-
POLYATOMIC IONS |
NITRATE
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NO2-
POLYATOMIC IONS |
NITRITE
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2-
CO3 POLYATOMIC IONS |
CARBONATE
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2-
SO4 POLYATOMIC IONS |
SULFATE
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2-
SO3 POLYATOMIC IONS |
SULFITE
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2-
S2O3 POLYATOMIC IONS |
THIOSULFATE
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3-
PO4 POLYATOMIC IONS |
PHOSPHATE
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3-
CrO4 POLYATOMIC IONS |
PHOSPHATE
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2-
CrO4 POLYATOMIC IONS |
CHROMATE
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2-
Cr2O7 POLYATOMIC IONS |
DICHROMATE
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ClO-
POLYATOMIC IONS |
HYPOCHLORITE
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ClO2-
POLYATOMIC IONS |
CHLORITE
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ClO3-
POLYATOMIC IONS |
CHLORATE
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ClO4-
POLYATOMIC IONS |
PERCHLORATE
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BrO-
POLYATOMIC IONS |
HYPOBROMITE
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BrO2-
POLYATOMIC IONS |
BROMITE
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BrO3-
POLYATOMIC IONS |
BROMATE
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BrO4-
POLYATOMIC IONS |
PERBROMATE
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IO-
POLYATOMIC IONS |
HYPOIODITE
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IO2-
POLYATOMIC IONS |
IODITE
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IO3-
POLYATOMIC IONS |
IODATE
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IO4-
POLYATOMIC IONS |
PERIODATE
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BINARY ACIDS-WATER SOULUTIONS OF COMPOUNDS COMPOSED OF _______ AND _____
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WATER SOULUTIONS OF COMPOUNDS COMPOSED OF HYDROGEN AND A NONMETAL
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HF
BINARY ACIDS |
HYDROFLUORIC ACID
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HCl
BINARY ACIDS |
HYDROCHLORIC ACID
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HBr
BINARY ACIDS |
HYDROBROMIC ACID
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HI
BINARY ACIDS |
HYDROIODIC ACID
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H2S
BINARY ACIDS |
HYDROSULFURIC ACID
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2.54 cm
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1 inch
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453.6 g
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1 pound
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1 L
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1.06 qt
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A digit that must be estimated is called ------. A measurement always has some degree of uncertainty
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A digit that must be estimated is called UNCERTAIN. A measurement always has some degree of uncertainty
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Accuracy refers to
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Accuracy refers to the agreement of a particular value with the true value
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A measurement always has some degree of
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uncertainty
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Precision refersto the.
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degree of agreement among several elements of the same quantity.
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5. A titration was performed to find the concentration of hydrchloric acid with the following results:
Trial Molarity 1 1.25 +/- 0.01 2 1.24 +/- 0.01 3 1.26 +/- 0.01 The actual concentration of HCl was determined to be 1.000 M; the results of the titration are : Both accurate and precise Accurate but imprecise Precise but inaccurate Both inaccurate and imprecise Accuracy and precision are impossible to determine with the available information |
Precise but inaccurate. All are in the same area but not in the right area
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Accurate
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To the true value
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Precise
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able to reproduce.
IF you can reproduce it you have precision. |
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Rules for Counting Significant Figures - Overview
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1. Nonzero integers
2. Zeros leading zeros (0.0025) captive zeros (1.008) trailing zeros (100 has one sig fig while 1.00 x 102 has three sig figs or 100. has three sig figs) 3. Exact numbers |
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Nonzero integers always count as significant figures.
3456 has |
4 SIG FIGS
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Leading zeros do not count as
significant figures. 0.0486 has |
3 SIG FIGS
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Captive zeros always count as
significant figures. 16.07 has |
4 SIG FIGS
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Trailing zeros are significant only
if the number contains a decimal point. 9.300 has |
4 SIG FIGS
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Exact numbers have an infinite number of significant figures.
1 inch = |
2.54 cm EXACTLY
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Express 0.000543 in exponential notation
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5.43 x 10-4********
5.43 x 10-6 54.3 x 10-5 54.3 x 10-3 543 x 10-3 |
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Express 784000000 in exponential notation
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7.84 x 106
7.84 x 108******** 78.4 x 107 784 x 106 784 x 107 |
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Multiplication and Division: # sig figs in the result equals the number in the least precise measurement used in the calculation.
6.38 2.0 |
12.76 13 (2 sig figs)
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Addition and Subtraction: # sig figs in the result equals the number of decimal places in the least precise measurement.
6.8 + 11.934 = here it is one place passed the deciam |
18.734=18.7
3.SIG FIGS For addition, answer is one past the decimal like equation |
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Using the rules of significant figures, calculate the following:
6.167 + 83/ 5.10 |
so add 6.167+83=89.167 so no places past zero because 83 has none past zero so it is 89/5.10=17.450 89 has 2 and 5.10 has three, so 2 is less than 3 so answer is expressed in 2 so answer is 17
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Using the rules of significant figures, calculate the following:
4.0021 – 0.004 |
3.998*** same number past the decimal
4 3.9981 4.00 4.0 |
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1 kilo
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is 1000 liter
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1 gram
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is 1000 miligram or kilogram
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1 meter
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1000mm or 100 cm
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MIXTURES HAVE
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VARIABLE COMPOSITION
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homogeneous mixture
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IS A SOLUTION LIKE VINEGAR
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heterogeneous mixture
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NOT UNIFORM TO THE NAKED EYE LIKE RANCH DRESSING
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COMPOUND
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A substance with a constant composition that can be broken down into elements by chemical processes.
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ELEMENT
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: A substance that cannot be decomposed into simpler substances by chemical means
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PURE SUBSTANCES
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CAN BE BROKEN DOWN INTO OR ELEMENTS BYCHEMICAL METHODS.
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1 m
1 meter |
1.094 yards
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2.54 centimeters
2.54 cm |
1 inch
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1 kg
1 kilogram |
2.205 pounds
2.205 lbs. |
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453.6 g
453.6 grams |
1 pound
|
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1 L
1 liter |
1.06 quarts
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3
1 ft one foot cubed |
28.32 liters
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miles to centimeters
160934.4 cm |
1 mile
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1 mile
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160934.4 cm-centimeters
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one meter
1 m |
3.2808399 ft
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one mL
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equals 1cm cubed
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one mile
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1.61 km
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Total kelvins
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Tk=total Celsius + 273.15
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Total Farenheit
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TF=Total celsius times 9/5+32
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Total Celsius
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TC= Total Farenheit -32 times 5/9
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mega M 1,000,000
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mega is a million 10 to the 6th
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kilo is k 1000
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kilo is 1000, 10 to the 3
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hecto is h it is 100
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hecto is 100 10 to the 2nd
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deka is da 10
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deka is 10 to the 1st, da
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one is 1
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ten to zero
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deci is d it is 0.1
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deci is 0.1 or 10-1
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centi is c it is0.01
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centi 0.01 or 10-2
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mili is m it is 0.001
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mili is 0.001 or 10-3
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micro is u it is 0.000001
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micro is 10-6
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nano is n it is 0.000000001
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nano is 10-9
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How many yards in 1 meter?
|
1.094 yards = 1 meter
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How many feet in 1 meter?
|
3.2808399 feet = 1 meter
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1 meter=100 centimeters=1000 milliters
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1000 mililiters=1 meter
100 centimeters =1 meter |
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how many cm in an inch?
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2.54 cm in an inch
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WHat does 1 ft cubed equal in liters
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1 foot cubed = 28.32 L
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What does one quart = in mililiters?
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one quart = .946 mililiters
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1 mile in kilometers?
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1.61 km = 1 mile
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1 mile in in centimeters?
|
160934.4 centimeters in a mile
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1 mile in yards?
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1760 yards in a mile
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how many kilograms in a pound
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2.205 kilograms in a pound
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how many grams in a pound
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453.6 grams in a pound
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how many yards in a meter
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1.094 yards in a meter
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how many yards in a mile
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1760 yards in a mile
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density is mass over volume
|
D=m/v
grams per liter is density |
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Carbon atomic mass = 12.01 amu
|
1 mole of anything = 6.022 10 to the 23 units of
substance |
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Avogadro’s number equals 6.022 10 top the 23 units
|
A substance’s molar mass (molecular weight) is the mass in grams of one mole of the compound
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Percent Composition
|
Mass percent of an element:
mass % = mass of element in compound over mass of compound times 100% |
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molecular formula = (empirical formula)n
[n = integer] molecular formula = C6H6 = (CH)6 empirical formula = CH |
molecular formula = (empirical formula)n
[n = integer] molecular formula = C6H6 = (CH)6 empirical formula = CH |
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Empirical Formula Determination
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1. Base calculation on 100 grams of compound.
2. Determine moles of each element in 100 grams of compound. 3. Divide each value of moles by the smallest of the values. 4. Multiply each number by an integer to obtain all whole numbers. |
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A representation of a chemical reaction:
C2H5OH + 3O2 2CO2 + 3H2O reactants products |
A representation of a chemical reaction:
C2H5OH + 3O2 2CO2 + 3H2O reactants products |
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C2H5OH + 3O2 2CO2 + 3H2O
The equation is balanced. 1 mole of ethanol reacts with 3 moles of oxygen to produce 2 moles of carbon dioxide and 3 moles of water |
C2H5OH + 3O2 2CO2 + 3H2O
The equation is balanced. 1 mole of ethanol reacts with 3 moles of oxygen to produce 2 moles of carbon dioxide and 3 moles of water |
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Calculating Masses of Reactants and Products
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1. Balance the equation.
2. Convert mass to moles. 3. Set up mole ratios. 4. Use mole ratios to calculate moles of desired substituent. 5. Convert moles to grams, if necessary. |
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Solving a Stoichiometry Problem
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1. Balance the equation.
2. Convert masses to moles. 3. Determine which reactant is limiting. 4. Use moles of limiting reactant and mole ratios to find moles of desired product. 5. Convert from moles to grams |
