Term
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Definition
--New properties are observed
--Change is reversable |
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Term
|
Definition
--New substances are formed
--Change is irriversable |
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Term
| Evidence of a Chemical Change |
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Definition
--Cooling/heating
--Reactants are consumed
--Change in color
--Gas formed
--Precipitate formed
(CHewing RoCks is Gross, People!) |
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Term
| Physical Properties mnemonic |
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Definition
Hear
Master
Daniel
Maximoff
Bellow
Cry
Scream.
Very
Difficult.
Can
Another? |
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Term
|
Definition
| Hardness, Malleability, Ductility, Melting, Boiling, Crystal shape, Solubility, Viscosity, Density, Conductivity, Appearance |
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Term
|
Definition
| combinations of more than one substance |
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Term
|
Definition
| - alloy, solution, colloid, suspension |
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Term
|
Definition
| homogeneous and heterogeneous |
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Term
| Define: homogeneous & heterogeneous |
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Definition
Homogenous: a mixture with one visible phase (ex: alloy & solution)
Heterogeneous: a mixture with more than one visible phase (ex: colloid & suspension) |
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Term
|
Definition
| homogeneous mixture including at least one fluid |
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Term
|
Definition
| a homogeneous mixture of solid metals |
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Term
|
Definition
| heterogeneous mixture that seperates by gravity |
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Term
|
Definition
| heterogenous mixture that does not seperate by gravity |
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Term
| Particle Theory of Matter (6 parts) |
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Definition
(1) particles are always moving except at absolute zero (-273 degrees)
(2) particles attract each other up to a certain distance and then repel each other
(3) particles at a higher temperature are moving faster than particles at a lower temp.
(4) particles can rotate, translate and vibrate
(5) everything is made up of particles
(6) each pure substance has its own type of particle that is different than the particles of other pure substances |
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Term
|
Definition
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Term
|
Definition
|
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Term
| Define: condensation point |
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Definition
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Term
|
Definition
|
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Term
|
Definition
|
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Term
| Define: sublimation point |
|
Definition
| solid to gas or gas to solid |
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Term
|
Definition
--new substances are formed
--change is not reversible |
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Term
|
Definition
--new properties are observed
--change is reversible |
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Term
| Evidence of chemical changes (not nessecarily in order; not all have to happen) (5) |
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Definition
| heat is absorbed or produced; reactants are consumed; change in color; gas formed; precipitate formed |
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Term
| List of chemical properties (3) |
|
Definition
(1) combustibility
(2) reactivity
(3) toxicity |
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Term
|
Definition
| always homogeneous; contains only one type of material; all properties uniform |
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Term
| Law of definite proportions |
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Definition
| Compounds are pure substances that contain two or more elements chemically combined together in fixed proportions (ex: H^2O always has 2 hydrogen atoms and one oxygen atom) |
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Term
| Dalton's atomic theory (5) |
|
Definition
(1) all matter is made of small particles called atoms
(2) an atom cannot be created, destroyed, or divided
(3) each atom for each element is identical in mass and size but different in mass and size from atoms of other elements
(4) compounds are created when atoms of different elements link together in definite proportions
(5) the atomic mass of hydrogen is defined as one |
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Term
|
Definition
| - a solid formed from two fluids |
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Term
| Why can't you see the particles in a solid move? |
|
Definition
| Particles usually translate, rotate, and vibrate, but in a solid they do not translate. They just move slightly in place. |
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Term
| Evidence of a chemical change (5): |
|
Definition
--heat is absorbed or produced
--reactants are consumed
--change in color
--gas formed
--precipitate formed |
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Term
|
Definition
| effect on living organisms |
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Term
|
Definition
| ability to be involved in a chemical reaction with other substances |
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Term
|
Definition
| the ability to burst into flames |
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|
Term
| Why does a candle need a wick to burn? |
|
Definition
| Because the flame needs something to support it, even though the actual fuel for the fire is the gas from the wax. |
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Term
| How would you tell if something is pure (metal) or not? |
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Definition
| First you measure the density (mass over volume) of the pure metal, then you measure the density of the object, and see if they are the same. |
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|
Term
| How can you figure out the volume of an irregularly shaped object? |
|
Definition
| You put the object in water and figure out how much it displaces. This figure is the volume. |
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Term
| What was the original elemental theory? |
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Definition
| Everything in the world was composed of mixtures of 4 elements: earth, wind, fire, and water. For example, alcohol is a liquid that burns, therefore it would be both fire and water. |
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Term
| What scientific law did Lavoisier state? |
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Definition
| The law of definite proportions |
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Term
| What did Francis Bacon contribute to the scientific world? |
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Definition
| proposed the original scientific method (or the lab report) which helped scientists share their information with other scientists |
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Term
| What contributions did Robert Boyle give to the scientific world? |
|
Definition
| Rejected four elements theory; proposed that pure substances can come together to form compounds |
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Term
| What did Antoine Lavoisier demostrate? |
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Definition
| That pure substances could not be decomposed physically |
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Term
| What did Humphrey Davy do? |
|
Definition
| he was a chemist who isolated (discovered and stated that they were an individual element) a few elements including sodium, potassium, magnesium, calcium, stronium, and barium |
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Term
| What did Jons Jacob Berzelius do? |
|
Definition
| He proposed a system for naming all the elements (giving them symbols), and the symbols would be the same everywhere |
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Term
|
Definition
| a pure substance that contains only one type of atom and cannot be broken down (chemically or physically) |
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|
Term
|
Definition
| A pure substance that contains more than one type of atom (is a combination of different elements) and can be broken down chemically but not physically |
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|
Term
| What did Dmitri Ivanovich Mendeleev do? |
|
Definition
| He proposed a system that would organize the elements so we could understand how they were classified in every way |
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|
Term
| Definition: Periodic Table |
|
Definition
| A chart thst organized the elements according to their atomic number |
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|
Term
| Definition: Chemical formulae |
|
Definition
| A formula for compunds involving letters and numbers (ex: H^2O) |
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|
Term
|
Definition
| The smallest unit of an element or compound, a cluster of 2 or more atoms |
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|
Term
| Definition: molecular elements |
|
Definition
| the smallest unit of an element, or a cluster of atoms containing only one type of atom |
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|
Term
| Definition: molecular compound |
|
Definition
| The smallest unit of a compound, or a cluster of atoms with more than one type of atom (ex: H^2O) |
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Term
|
Definition
| a horizontal row of elements in the periodic table |
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Term
|
Definition
| a vertical row of elements in the periodic table |
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|
Term
| What were the contributions of Antoine Lavoisier to the scientific community? |
|
Definition
| demonstreated that pure substances can't be decomposed by physical means |
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|
Term
| What were the contributions of Antoine Lavoisier to the scientific community? |
|
Definition
| demonstreated that pure substances can't be decomposed by physical means |
|
|
Term
| What were the contributions of Humphrey Davy to the scientific world? |
|
Definition
| isolated K, Na, Mg, Ca, Sr, Ba |
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Term
| What were the contributions of Dmitri Ivanocich Mendeleev to the scientific world? |
|
Definition
| examined all known elements and arranged them based on common properties |
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Term
|
Definition
| elements arranged by atomic number |
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Term
|
Definition
| row in the periodic table |
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Term
|
Definition
| column in the periodic table |
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Term
|
Definition
| substance containing one type of atom. Has distinct properties and cannot be broken down by chemical on physical means |
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Term
|
Definition
| substance made up of a combination of two or more diffrent elements; can be broken down chemically but not physically |
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Term
|
Definition
| the smallest, independent unit of a pure substance, is generally a cluster of atoms bound together. |
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Term
| Define: molecular elements |
|
Definition
| molecules that contain only one type of element |
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Term
|
Definition
| nearly not-reactive gases |
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Term
|
Definition
| gases, liquids, and solids, very reactive |
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Term
|
Definition
| soft, hightly reactive metals |
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|
Term
| Define: alkaline earth metals |
|
Definition
| less reactive thatn alkali metals |
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|
Term
| What is the formula for density? |
|
Definition
|
|
Term
| Describe the experiments of Rutherford |
|
Definition
|
|
Term
| Describe the experiments of Heinrich Geissler |
|
Definition
| invented the gas discharge tube |
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|
Term
| Describe the experiments of William Crooks |
|
Definition
| Discovered streams of negatively charged particles leaving a chathode and traveling towards an anode |
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|
Term
| Describe the experiments of Goldstein |
|
Definition
| detected positive particles (protons) traveling from the anode of a hydrogen tube |
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|
Term
| Describe the experiments of J.J. Thomson |
|
Definition
| Discoved that the stream of negatively charged paticles were attracted to a negatively charged plate; theorized the presence of positively charged particles; proposed the muffin model of the atom |
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