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57 Cards in this Set
- Front
- Back
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Atom
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-smallest identifiable unit
-idea first pioneered by Greek philosophers Liucippus and Democritus -"Atomos" indivisible -1808 Dalton Atomic Theory |
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Dalton and his Atomic Theory
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1. Each element is composed of tiny indestructible particles called atoms
2. All atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements 3. Atoms combine in simple, whole-number ratios to form compounds summarized 1 tiny indestructible particles 2 atoms of the same element share common mass 3.atoms combine in whole number ratios/ compounds |
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Who is J.J. Thompson
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English physicist that proposed the plum pudding model of the atom to account for electrons and neutral charge atoms
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Electron
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- particle in atom with negative charge
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Ernest Rutherford
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-proved in gold foil experiment and proclaim the nuclear theory of the atom
- foundation for protons and neutrons |
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Gold Foil Experiemt
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-1909
-directed postively charged alpha particles through ultra thin gold foil - purpose to prove the THompson "plum pudding" model of the atom, by observing particles pass through with minimumdeflection -conclusion some particles were deflected and 1 in 20,000 bounced back -it gave the foundation for the nuclear atomic theory -small area of dense space -large regions of empty space |
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Nuclear Theory of the Atom
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1. Most of the atom's mass and all of its positive charge are contained in a small core called the nucleus
2. Most of the volume of the atomic empty space in which negatively charged electrons are dispersed |
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Protons vs Nuetrons
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Positive vs nuetral particles in an atom
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How much of the total atomic mass is found in the nucleus?
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-99.9% of the mass is located in the dense nucleus
-electron weighs about nothing |
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Perspective on atomic mass and nucleus
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-if a grain of sand was composed of nuclei 10 mllion pounds
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Atomic Mass Unit (amu)
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-1/12 of the mass of a carbon atom containging six protons and six nuetrons
-1.0073 amu = proton -1.0087 amu = neutron -.00055 amu = electron |
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Nature of Electrical Charge
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-electrical charge is a fundamental property of protons and electrons
- (-) and (+) cancel eachother out - (+) and (+) // (-) and (-) repulsion - electrical charge is a property of electrons and protons as in mass with matter |
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Atomic Number
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- Amount of protons in nucleus
- atomic number defines element |
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Chemical Symbol
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-one or two letter abbreviation appearing below atomic number on the periodic table
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Dmitri Mendeleev
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-(1834-1907)
-observed certain groups of elements had simliar properties - developed periodic law |
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Periodic Law
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"When the elements are organized in order of increasing relative mass certain sets of properties recur periodically."
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Modern Periodic Table
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-inspire by Mendeleev's conjecture of periodic law
- listing in order of actomic number |
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Metals
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-Occupy the left side of the periodic law table and have similiar properties
-good conductors of heat and electricity -malleable - dutcile -tend to lose electrons |
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Nonmetals
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-upper right side of teh periodic table
-some are solids some are gas at room temperature - tend to gain electrons - poor conductors of elect and heat |
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Metalloids
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-intermediate electrical conductivity which can be changed or controlled
-a Diagonal that seperates metals from nonmetals B-Boron ++> At- Astatine B = Boron Si = Silicon Ge = Germanium As = Arsenic Sb = Antimony Te = Tellerium Po = Polonium At = Astatine |
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Main-Group Elements
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Properties tend to be more predictable based on their position in thw periodic table
-Signified by (A) following group number |
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Transistion elements/ transition metals
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less easily predictable based on their position on the periodic table
Signified by (B) following group number |
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Family or Group
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-column within main group elements
- number printed directly above column - elements within group have similar properties |
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Group 8A
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-Far right column
- Nobel Gases -inert gases -chemically stable / won't combine with other elements to form compunds |
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Nobel Gases
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He - Helium
Ne - Neon Ar - Argon Kr - Krypton Xe - Xenon Rn - Radon |
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Group 1A
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- Alkali Metals
- very reactive metals - far left column |
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Alkali Metals
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Li = Lithium
Na = Sodium K = Potassium Rb = Rubidium Cs = Cesium Fr = Francium |
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Group 2A
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-Alkaline earth metals
- fairly reactive |
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Alkaline Earth Metals
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Be = Beryllium
Mg = Magnesium Ca = Calcium Sr = Strontium Ba = Barium Ra = Radium |
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Group 7A
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- Second from the right column
- Halogens -very reactive nonmetals |
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Halogens
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F = Flourine
Cl = Chlorine Br = Bromine I = Iodine At = Astatine |
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What happens in chemical reactions to atoms?
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-In chemical reactions, atoms often lose or gain electrons to form charged paticles called ions
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Ions
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-atoms that lose or gain electrons
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Two types of Ions
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Cations and Anions
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Cations
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positively charged particles
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Anions
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negatively charged particles
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Equation for an ion charge
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ion charge = number of protons - number of electrons
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Ion vs Isotope
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imbalance in electrons and protons vs imbalance in nuetrons and protons
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Isotopes
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same number of protons but different number of nuetrons
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Percent Natural Abundance
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- percentage of abundances of isotopes in nature
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Mass Number
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sum number of nuetrons and protons
a = Number of Protons + Number of nuetrons |
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Atomic Mass
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- The atomic mass of each element is listed in the perodic table directly beneath the elements's symbol; represents the average mass of atoms that compose the element
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Isotopes
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same number of protons but different number of nuetrons
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Percent Natural Abundance
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- percentage of abundances of isotopes in nature
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Mass Number
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sum number of nuetrons and protons
a = Number of Protons + Number of nuetrons |
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Atomic Mass
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- The atomic mass of each element is listed in the perodic table directly beneath the elements's symbol; represents the average mass of atoms that compose the element
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Atomic Mass Equations
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(Fraction of isotope x mass of isotope) /number or isotopes
First part done for each isotope ex (i1% x i1m) + (i2% x i2m) / 2 |
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52/24 Cr 3-
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52 = mass
24 = protons 28 = nuetrons 27 = electrons |
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Meter Conversions 1 meter
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= 10^-12 Terameters (Tm)
= 10^-9 Gigameters (Gm) = 10^-6 Megameters (Mm) = 10^-3 km = 10^2 cm (100) = 10^3 mm (1000) = 10^6 micrometers = 10^9 nanometers = 10^12 picometers |
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1 mile
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5280 ft
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Heat of Fusion
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-the amount of heat released when 1g of liquid freezes
-the amount of heat needed to melt 1g of a soild |
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Sublimation
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particles change directly from solid to gas
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Evaporation vs condensation
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liquid to gas vs gas to liquid
(gaining vs losing energy) |
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Heat of Vaporization
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-amount of heat absorbed to vaporize 1g of a liquid to gas at the boiling point
-amount of heat released when 1g of a gas condenses to liquid at the boiling point |
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Heating Curve
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-changes that occur when heating a solid
-slopes increase in temperature (melting, boiling vaporizing) -plateaus flat lines indicate a change of state (melting point, boiling point) |
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A flat line on a heating curve represents
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- constant temperature
-change of state |
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Sloped line on a heating curve
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-terperature change
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