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143 Cards in this Set
- Front
- Back
quantitative observation
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involves numbers
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qualitative observation
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involves descriptions
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celsius to kelvin
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k=c+273
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celsius to fahrenheit
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f=1.8c+32
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density
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density=mass/volume
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accuracy
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how close a measured value is to an accepted or true value
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precision
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how close a series of measurements are to one another
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percent error
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accepted value-experimental
percent error--------------------- accepted value |
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gases
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indefinite shape indefinite volume
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liquids
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definite volume indefinite shape
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solids
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definite shape definite volume
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physical properties
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describe the appearance of matter
state, color, volume, odor, taste, hardness, density, solubility, melting/boiling point. |
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extensive properties
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dependent upon the amount of substance present
mass, length and volume |
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intensive properties
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independent of the amount of substance present.
density, color, temperature, hardness, melting point, boiling point, pressure, and molecular weight |
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physical changes
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the form but not the identity of matter changes
bend, crumple, split, crush, boil, freeze, condense, vaporize, or melt **if after the substance undergoes the change and can still be identified as the original substance it is a physical change** |
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solid--> liquid
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melting
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gas--> liquid
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condensing
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solid-->gas
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sublimation
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liquid--> solid
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freezing
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gas--> solid
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reverse sublimation
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liquid--> gas
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evaporation
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chemical property
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the ability of a substance to combine with or change into one or more other substances. describes how matter behaves when it changes into another kind of matter
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chemical change
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process that involves one or more substances changing into new substances. also called chemical reaction
explode, rust, cook, oxidize, corrode, tarnish, ferment, burn, or rot. |
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element
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pure substance that cannot be broken down into other substances by chemical means
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compound
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when two or more elements combine in a fixed composition by weight. can be broken down into simpler substances by chemical means
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law of definite proportions
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regardless of amount, a compound is always composed of the same elements in the same proportion by mass.
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percent by mass
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mass of element
% by mass=--------------- x 100 mass of compound |
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mixture
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something that has variable composition and is made of a number of pure substances and each pure substance retains its individual properties
wood, wine, coffee, air |
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pure substance
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always has the same composition like
elements and compounds purified water |
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homogeneous mixture
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the same throughout.
salt water |
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solid--> liquid
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melting
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gas--> liquid
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condensing
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solid-->gas
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sublimation
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liquid--> solid
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freezing
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gas--> solid
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reverse sublimation
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liquid--> gas
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evaporation
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chemical property
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the ability of a substance to combine with or change into one or more other substances. describes how matter behaves when it changes into another kind of matter
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chemical change
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process that involves one or more substances changing into new substances. also called chemical reaction
explode, rust, cook, oxidize, corrode, tarnish, ferment, burn, or rot. |
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element
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pure substance that cannot be broken down into other substances by chemical means
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compound
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when two or more elements combine in a fixed composition by weight. can be broken down into simpler substances by chemical means
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law of definite proportions
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regardless of amount, a compound is always composed of the same elements in the same proportion by mass.
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percent by mass
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mass of element
% by mass=--------------- x 100 mass of compound |
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mixture
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something that has variable composition and is made of a number of pure substances and each pure substance retains its individual properties
wood, wine, coffee, air |
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pure substance
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always has the same composition like
elements and compounds purified water |
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homogeneous mixture
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the same throughout. also called a solution
salt water, cough syrup, lemonade, air, brass (made of copper and zinc) |
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heterogeneous mixture
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contains regions that have different properties from those of other regions
sand water |
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filtration
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used to separate an insoluble solid from a liquid
pour mixture onto a mesh or filter paper which allows the liquid to pass through and leaves the solid behind |
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distillation
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used to separate either a liquid from a soluble solid or two liquids with different boiling points
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distillation of liquid from soluble solid
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mixture is heated to boiling state so liquid will evaporate and rise into the condenser where it returns back to liquid state leaving the solid behind
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distillation of two liquids
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mixture is heated to one of the liquid's boiling points so that liquid evaporates leaving the liquid with the higher boiling point behind.
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energy
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the ability to do work or produce heat
measured in joules (J) or calories **1 calorie= 4.184 J** |
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potential energy
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energy due to composition or position of an object
also known as death from physics las year |
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kinetic energy
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the energy of motion
or potential energy's partner in crime |
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law of conservation of energy
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in any chemical reaction or physical process, energy can be converted from one for to another but it is neither created nor destroyed
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calorie
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amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius
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specific heat capacity
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the amount of energy required to change the temperature of one gram of that substance by one degree Celsius
Energy (heat) required= SHC x mass x change in temp. ºC or Q = s x m x change in temp ºC unit: J/gºC |
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exothermic process
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when heat is transferred from the system to the surroundings
freezing, wood that is burning |
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endothermic process
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when heat is transferred to the system from the surroundings
melting, |
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Dalton's Atomic Theory
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1. All matter is composed of tiny particles called atoms
2. All atoms of a given element are identical 3. The atoms of a specific element are different to those of any other element 4. atoms of different elements combine to form compounds. compounds have a fixed composition known as the law of definite proportion 5. atoms cannot be created, divided in small particles, or destroyed. in a chemical reaction they are simply rearranged to form new compounds. |
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JJ Thompson
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discovered the electron and it's mass using negative cathode rays
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heterogeneous mixture
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contains regions that have different properties from those of other regions
sand water |
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filtration
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used to separate an insoluble solid from a liquid
pour mixture onto a mesh or filter paper which allows the liquid to pass through and leaves the solid behind |
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distillation
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used to separate either a liquid from a soluble solid or two liquids with different boiling points
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distillation of liquid from soluble solid
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mixture is heated to boiling state so liquid will evaporate and rise into the condenser where it returns back to liquid state leaving the solid behind
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distillation of two liquids
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mixture is heated to one of the liquid's boiling points so that liquid evaporates leaving the liquid with the higher boiling point behind.
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energy
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the ability to do work or produce heat
measured in joules (J) or calories **1 calorie= 4.184 J** |
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potential energy
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energy due to composition or position of an object
also known as death from physics las year |
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kinetic energy
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the energy of motion
or potential energy's partner in crime |
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law of conservation of energy
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in any chemical reaction or physical process, energy can be converted from one for to another but it is neither created nor destroyed
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calorie
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amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius
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specific heat capacity
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the amount of energy required to change the temperature of one gram of that substance by one degree Celsius
Energy (heat) required= SHC x mass x change in temp. ºC or Q = s x m x change in temp ºC unit: J/gºC |
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exothermic process
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when heat is transferred from the system to the surroundings
freezing, wood that is burning |
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endothermic process
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when heat is transferred to the system from the surroundings
melting, |
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Dalton's Atomic Theory
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1. All matter is composed of tiny particles called atoms
2. All atoms of a given element are identical 3. The atoms of a specific element are different to those of any other element 4. atoms of different elements combine to form compounds. compounds have a fixed composition known as the law of definite proportion 5. atoms cannot be created, divided in small particles, or destroyed. in a chemical reaction they are simply rearranged to form new compounds. |
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JJ Thompson
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discovered the electron using negative cathode rays
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heterogeneous mixture
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contains regions that have different properties from those of other regions
sand water |
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filtration
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used to separate an insoluble solid from a liquid
pour mixture onto a mesh or filter paper which allows the liquid to pass through and leaves the solid behind |
|
distillation
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used to separate either a liquid from a soluble solid or two liquids with different boiling points
|
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distillation of liquid from soluble solid
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mixture is heated to boiling state so liquid will evaporate and rise into the condenser where it returns back to liquid state leaving the solid behind
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distillation of two liquids
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mixture is heated to one of the liquid's boiling points so that liquid evaporates leaving the liquid with the higher boiling point behind.
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energy
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the ability to do work or produce heat
measured in joules (J) or calories **1 calorie= 4.184 J** |
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potential energy
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energy due to composition or position of an object
also known as death from physics las year |
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kinetic energy
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the energy of motion
or potential energy's partner in crime |
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law of conservation of energy
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in any chemical reaction or physical process, energy can be converted from one for to another but it is neither created nor destroyed
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calorie
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amount of energy (heat) required to raise the temperature of one gram of water by one degree Celsius
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specific heat capacity
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the amount of energy required to change the temperature of one gram of that substance by one degree Celsius
Energy (heat) required= SHC x mass x change in temp. ºC or Q = s x m x change in temp ºC unit: J/gºC |
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exothermic process
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when heat is transferred from the system to the surroundings
freezing, wood that is burning |
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endothermic process
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when heat is transferred to the system from the surroundings
melting, |
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Dalton's Atomic Theory
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1. All matter is composed of tiny particles called atoms
2. All atoms of a given element are identical 3. The atoms of a specific element are different to those of any other element 4. atoms of different elements combine to form compounds. compounds have a fixed composition known as the law of definite proportion 5. atoms cannot be created, divided in small particles, or destroyed. in a chemical reaction they are simply rearranged to form new compounds. |
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JJ Thompson
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discovered the electron using negative cathode rays
also constructed plum pudding model |
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Robert Millikan
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determined exact mass and charge or the electron
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Ernest Rutherford
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designed experiment involving directing alpha (+) particles towards a thin metal foil. surrounding the foil was a detector coated with a substance that produced tiny flashes wherever it was hit by an alpha particle. he discovered that some particles were deflected at angles and some straight back and some passed through concluding that atoms had a small positively charged center called a nucleus containing protons
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James Chadwick
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discovered the nucleus also contained neutral particle called the neutron with the same mass as a proton
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atomic number
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the number of protons in the nucleus of the atom
also tells us the number of electrons |
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mass number
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number of protons + neutrons
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Isotope
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an atom with the same number of protons and electrons but different number of neutrons
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metals
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good conductors of heat and electricity, usually shiny in appearance, and most are solid at room temp.
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Diatomic molecules
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molecules mad up of 2 atoms of the same element
***HOFBrINCl*** |
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ion
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an atom that has lost or gained an electron
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cations
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atoms that have lost electrons and are positively charged
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anions
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atoms that have gained an electron and are negatively charged
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ionic compounds
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compounds that contain a metal and a nonmetal
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molecular compounds
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compounds that contain two nonmetals
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type II binary compound prefixes
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mono...1
di...2 tri...3 tetra...4 penta...5 hexa...6 hepta...7 octa...8 |
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acid
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a compound that produces hydrogen ions when dissolved in water
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aqueous solutions
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a substance dissolved in water.
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strong electrolyte
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when a large number of ions are present in a solution, the solution will be an excellent conductor of electricity.
any aqueous ionic compound |
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weak electrolyte
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does not conduct electricity well
molecular compound |
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Precipitation Reactions
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formation of a solid
double displacement reaction ***memorize solubility rules*** |
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spectator ions
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ions that do not participate in the reaction.
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acid-base reactions
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formation of water
double displacement reaction acid+base-->salt+water |
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strong acids
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HCl, HBr, HI, HClO4, HNO3, H2SO4
**all numbers are subscript** |
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strong bases
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group 1 and Ca, Sr, Ba with hydroxide
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Oxidation Reduction (REDOX) reactions
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transfer of electrons
element losing electrons become oxidized, element gaining electrons becomes reduced, element being oxidized is reducing agent, element being reduced is oxidizing agent |
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single displacement reaction
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reactions that form gases
where only a single type of ion has been exchanged between positive ions |
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combustion
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reactions where oxygen is used to burn fuels to produce energy. products are always CO2 and H2O
C & H +O2--> CO2 + H2O |
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synthesis
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when two elements combine to form a compound
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decomposition
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a reaction where a compound is broken down into simpler substances. opposite of synthesis.
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Atomic Mass Unit
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amu
unit for mass of atoms. **unit of mass of element on periodic table** |
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average atomic mass
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(m # of 1st x % abundance)+(m # of 2nd...)/100
when writing % abundance keep number in % form. so for 75% use the number 75 rather than .75 |
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mole
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the number equal to the number of atoms in 1g of an element.
6.02x10^23 |
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molar mass
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g of substance/ 1 mole of substance
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percent composition
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tot. m of element in 1 mole of compound
-------------------------------- total mass of 1 mole of the compound |
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empirical formula
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simplest whole number ratio of the atoms of each element in that compound.
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molecular formula
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tells us exactly how many atoms of each element are present in the compound rather than just the simplest whole number ratio like in the empirical formula
molar mass of molecular formula n=-------------------------- molar mass of empirical formula **molar mass of molecular formula is always given |
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stiochiometry
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the study of quantitative relationships between amounts of reactants used and the products formed y a chemical reaction
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percent yield
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actual yield of product
% Yield=---------------------- theoretical yield of product |
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Electromagnetic radiation
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one of the ways light travels through space.
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speed of light
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c=3x10^8
c=wavelength x frequency wavelength and frequency are inversely related |
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Electromagnetic spectrum
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ROYGBIV
red has large wavelength and small frequency violet has small wavelength and large frequency |
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quantum concept
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Max Planck concluded that matter can gain or lose energy only in small specific amounts called quanta
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quantum
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minimum amount of energy that can be gained or lost by an atom
Equantum = hv h=6.62x10^-34 Js (joule seconds) E= energy v= frequency |
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atomic emission spectra
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the set of frequencies of the electromagnetic waves emitted by atoms of an element
each element emits a color unique to that element |
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Bohr model of the atom
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all atoms have a ground state (lowest allowable energy) and an excited state (highest allowable energy)
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quantum mechanical model of the atom
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each orbital can be thought of as a fuzzy cloud where an electron may be found
it may not be possible to pin point the exact position of the electron at any one time, but it is possible to say that the electron will be within a certain area called an orbital |
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major difference between the Bohr model and wave mechanical model of the atom
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in the bohr model, the energy of the electron is described in terms of a definite orbit or pathway. in the wave mechanical model the energy is described in terms of the probability of locating the electron in a region of space outside the nucleus. energy levels are thought of as clouds of electrical charge surrounding the nucleus.... POOP!!!! hahaah : )
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aufbau principle
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electrons enter orbitals of lowest energy first
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pauli exclusion principle
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2 electrons per orbital with opposite "spins" represented by up and down arrows
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hund's rule
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fill orbitals of a given energy one at a time before pairing electrons up.
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valence electrons
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the electrons in the outermost principle energy level of an atom.
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core electrons
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electrons not involved in bonding
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CHEMISTRY
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DEATH!!!!
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cameron
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most amazing person ever for making all these flashcards and being wiling to share with everyone!!!
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