Second Semester College Prep Chem Final Review
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Democritus
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Greek philosopher, thought that matter was made of tiny indivisible spheres, all matter made up of same spheres
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John Dalton
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tiny indivisible spheres, formed theory with 5 postulates: 1. Matter is made of atoms 2. Atoms of same element are identical. 3. Atoms of different elements have different chemical and physical properties. 4. Two or more different elements can join to form compounds. 5. Atoms can be separated, rearranged, and combined, but cannot be destroyed or split.
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JJ Thomson
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Conducted cathode ray tube experiment and discovered the ELECTRON. "Plum Pudding Model" of the atom where the electrons were the plums and the pudding was a field of positive charge.
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Ernest Rutherford
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Conducted gold foil experiment. He shot alpha particles at gold foil. Most of the time, they went straight through. Sometimes they bounced back. Told him 2 things: 1. Most of atom is empty space 2. There was a small, dense, positive nucleus
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Niels Bohr
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Proposed that electrons orbited the nucleus like planets around the sun ("planentary model"). He also found that the electrons could "jump" between orbits ("energy levels"). To jump to a higher level, electrons absorb photons. To jump to a lower level, electrons release photons.
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Erwin Schrodinger
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Electron Cloud Model- electrons did not move in defined orbits, they exist in orbitals and you can't identify their exact location- based on probability
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atomic mass
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Number of neutrons plus protons, the larger number for each element on the periodic table
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average atomic mass
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Since there are isotopes for each element, the decimal Number on the periodic table represents a weighted average of all isotopes. For instance, Carbon can be Carbon-12, Carbon-13, or Carbon-14, but its average atomic mass is 12.0107.
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isotope
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Atoms of the same element with different masses. For instance Carbon-12, Carbon-13, and Carbon-14 are isotopes. All the same element, but different number of neutrons leading to different masses.
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How many protons, neutrons, and electrons in Silicon-30?
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14 protons, 16 neutrons, 14 electrons
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atomic number
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number of protons (and the number of electrons if the atom is neutral)
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Location/Charge of nucleus
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center of atom, charge is positive (because its made up of protons which are positive and neutrons which are neutral)
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Location/Charge/Mass of protons
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in nucleus, positive, 1 amu
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Location/Charge/Mass of electrons
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in electron cloud, negative, almost no mass
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Location/Charge/Mass of neutrons
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in nucleus, neutral, 1 amu
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Electromagnetic Spectrum (low E/low frequency/long wavelength to high E/high frequency/short wavelength)
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radiowaves, microwaves, infrared, visible, UV, Xray, Gamma
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Relationship Between Frequency and Energy
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DIRECTLY PROPORTIONAL. High E, High Freq. Low E, Low Freq.
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Relationship Between Frequency and Wavelength
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INVERSELY PROPORTIONAL. High Freq, Short Wavelenght. Low Freq, Long Wavelength.
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Group Number and Valence Electrons
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Group Number = Number of Valence Electrons in that Column. For example, Group 1 all have 1 valence (outer) electron.
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Atomic Size Trend
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LEFT TO RIGHT, get SMALLER because they have the same period (number of energy levels and number of protons increases, pulling electrons close) DOWN A COLUMN, atoms get bigger because you're adding energy levels.
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Ionic Size Trend (Neutral versus Positive Ion)
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Neutral is BIGGER. Positive Ion lost electrons (lost an energy level) and nucleus pulls remaining electrons closer.
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Ionic Size Trend (Neutral versus Negative Ion)
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Negative Ion is Bigger. Negative ion gained electrons and the nucleus has less of a pull because there are more electrons.
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Electronegativity
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An atom's "hunger for electrons". Higher electronegativity means the atom "wants" to pick up electrons to fill its valence shell. Low electronegativity means the atom "wants" to give up electrons. Metals typically have low electronegativity. Nonmetals have high electronegativity.
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Electronegativity Trend
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Fr has lowest electronegativty. F has highest electronegativty. As you left to right and up, electronegativity increases
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Location of Metals on Table
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Left side of "stairway"
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Location of Nonmetals on Table
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Right side of "stairway"
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Location of Metalloids on Table
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Located one box to either side of "stairway"
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Reactivity of Metals
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Most reactive is near Fr. Going down and to the left on table. Lowest electronegativity = highest reactivity for metals.
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Reactivity of Nonmetals
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Most reactive is near F. Going up and to the right on table. Highest electronegativity = highest reactivity for nonmetals.
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Group 1 Name
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Alkali Metals
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Group 2 Name
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Alkaline Earth Metals
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Group 7 Name
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Halogens
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Group 8 Name
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Noble Gases
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radioactivity
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