Chemistry
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| Chemistry | the study of matter and the change in undergoes. (usually energy changes)
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| Organic Chemistry | study of carbon containing compounds- now includes synthetics such as plastic
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| Biochemistry | matter and processes of living organisms- (fats, lipids, protein, enzymes)
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| Inorganic Chemistry | may contain short carbon chained molecules, but usually has no carbon.
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| Physical Chemistry | covers thermodynamics and kinetics as well as other topics (energy is a large factor)
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| Thermodynamics | change of heat
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| Kinetic | movement of particles
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| H | Hydrogen
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| Hydrogen | H
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| Lithium | Li
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| Li | Lithium
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| Na | Sodium
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| Sodium | Na
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| K | potassium
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| potassium | K
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| Rubidium | Rb
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| Rb | Rubidium
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| Cesium | Cs
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| Cs | Cesium
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| Francium | Fr
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| Fr | Francium
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| B | Boron
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| Boron | B
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| aluminum | Al
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| Al | Aluminum
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| gallium | Ga
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| Ga | Gallium
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| Indium | In
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| In | Indium
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| Thallium | Tl
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| Tl | Thallium
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| Carbon | C
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| C | Carbon
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| Silicon | Si
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| Si | Silicon
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| Germanium | Ge
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| Ge | Geranium
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| Tin | Sn
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| Sn | Tin
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| Pb | Lead
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| Lead | Pb
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| Why are Significant Figures important? | tells the reader how precise the measurements are.
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| T/F- all non-zero numbers are significant | True
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| T/F- zeros between non-zero numbers are significant figures | True
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| T/F- zeros at the beginning of a number are significant | False
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| T/F- Zeros at the end of a number with a decimal are not significant | False
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| T/F- All exact conversions and counting of a number have infinite numbers of significant figures | True
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| How many significant figures are in 11.8 units? | 3 sf
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| How many SF are in 0.024 mg? | 2 SF
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| How many SF are in 110 cars? | Infinite
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| When doing operations with SF what operation does this rule apply to? - the LEAST number of significant figures in any number of the problem determines the number of SF in the answer. | Multiplication and Division
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| When doing operations with SF what operation does this rule apply to? - count the number of place holders in the decimal portion of each number, the least number should be used in the answer of the problem. | Addition and Subtraction
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| What do we use to measure length? | meter
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| what do we use to measure volume? | liter
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| what do we use to measure mass | gram
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| what do we use to measure time? | seconds
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| what do we use to measure temperature? | kelvin
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| what do we use to measure amount? | mole
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| What do prefixes do to a base? | makes it larger or smaller
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| N | Nitrogen
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| Nitrogen | N
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| P | Phosphorus
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| Phosphorus | P
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| As | Arsenic
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| Arsenic | As
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| Antimony | Sb
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| Sb | Antimony
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| Bi | Bismuth
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| Bismuth | Bi
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| O | Oxygen
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| Oxygen | O
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| Sulfur | S
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| S | Sulfur
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| Se | Selenium
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| Selenium | Se
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| Tellurium | Te
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| Te | Tellurium
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| Polonium | Po
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| Po | Polonium
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| Analytical chemistry | Focuses on the composition of matter.
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| Heterogeneous mixture | You can see all parts and easily split them
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| Matter | Anything that has mass or takes up space
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| Mixture | Matter with variable composition made from 2 or more substances
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| Pure substance | Matter with a constant composition all particles have the same property
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| Element | A substance made of atoms with the same atomic number
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| Compound | A substance made of two or more elements that are chemically combined
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| Physical change | Does not change the chemical composition of the substance. â Bending polishing cutting boiling melting and freezing
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| Physical property | Describes physical appearance
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| Inertia | Resistance to change in motion
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| Kinetic Molecular Theory | All matter is made of particles in constant motion.
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| Kinetic Energy | Energy of motion
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| Heat | Energy that is transferred from one object to another. (You can't really measure heat, only change in temperature)
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| Intermolecular Forces | Forces between molecules and atoms that determine the physical state of a substance.
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| Intramolecular forces | All chemical bonds such as covalent, ionic, metallic
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| What type of force takes more energy to break? Intermolecular or Intramolecular? | Intramolecular
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| Solids | -Intermolecular forces are strong
-particles are closely packed and travel a fraction of their diameter
-have a definite shape and volume
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| Liquids | -particle motion is limited by intermolecular forces
-particles are in contact with each other
-travel in a straight line by slipping past each other
-have a definite volumes and takes shape of container
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| Gases | -particles are independent of each other (very weak intermolecular forces.)
-travel randomly in a straight line
-assume the shape and volume of container
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| Plasma | -matter is heated to extreme temperature (electrons are not away from matter)
-matter is composed of electrons and positive ions
-most of the universe is composed of plasma
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| Gas to a liquid | Condensation (exothermic)
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| Liquid to a gas | Vaporization (endothermic)
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| Gas to a solid | Deposition (exothermic)
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| Solid to a gas | Sublimation (endothermic)
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| Liquid to a solid | Freezing (exothermic)
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| Solid to a liquid | Melting (endothermic)
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| What did philosophers in the 1800s believe matter was made of? | Earth, fire, water, and air
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| What did Democritus do? | Propose tiny things called atmos â small individual indivisible particles. Said they move through empty space, different properties of matter where do two arrangements of atoms.
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| What did Dalton do? | Believed all matter is made up of small particles called atoms. All atoms of elements are identical by mass. Matter is neither created or destroyed. Adams combine and small hole number ratio's.
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| What did JJ Thompson discover? | Discovered electrons using the cathode ray tube. This was a pole that charge particles went up into.
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| What did Robert Millikan do? | Figured out the charge of electrons using a famous oil drop experiment. This experiment calculated using average is the mass of oil drops and the rate at which would move toward the positive plate.
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| What atom model did Thompson create? | The plum putting model- electrons embedded randomly and a mass of positive charge.
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| What atom model did Rutherford come up with? | Developed the first nuclear model as a result of the gold foil experiment. Make sure you understand the gold foil experiment.
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| Atomic Mass | The number of protons [e] in a neutral non- charged atom. Above the number on most periodic tables- always a whole number.
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| Mass number | Protons + neutrons.
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| Atomic Mass- | Usually blow symbol on periodic table. AMU x %
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| Isotopes | Atoms of an element that have a different number of neutrons â All atoms of an element therefore don't have the same atomic number
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| Nuclide Symbol | A symbol that notes the number of protons and neutrons of a specific isotope
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| Ions | Atoms of an element that have a different number of electrons
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| Cation | Ions that have lost all electrons(s) and are positively charged. Metals form cations
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| Anions | Ions that have lost electron(s) and are negatively charged. non-metals form anions.
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| 4 fundamental Forces | Gravity, Weak, Strong, electromagnetic
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| F | Fluorine
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| Fluorine | F
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| Chlorine | Cl
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| Cl | Chlorine
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| Br | Bromine
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| Bromine | Br
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| I | Iodine
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| Iodine | I
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| At | Astatine
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| Astatine | At
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| He | Helium
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| Helium | He
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| Ne | Neon
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| Neon | Ne
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| Argon | Ar
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| Argon | Ar
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| Krypton | Kr
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| Kr | Krypton
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| Xe | Xenon
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| Xenon | Xe
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| Rn | Radon
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| Radon | Rn
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Created by:
Kate_Spires
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