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70 Cards in this Set
- Front
- Back
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Matter
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-It has mass
-It takes up space |
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Solid
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o Definite shape
oDefinite volume oVibrations oClosely packed |
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Liquid
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o Takes shape of it’s container
oDefinite volume oSlight movement oMore loosely packed than a solid |
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Gas
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o Takes shape of it’s container
o Indefinite volume o Move freely o Very spread out |
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atoms
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Atoms are the smallest unit of matter
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Elements
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substances made from only 1 type of atom.
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Compounds
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substances made by combing 2 or more types of atoms.
- A compound is made up of different elements, but it always has the same composition. |
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Molecules
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substances made from combined atoms
- Molecules are bonded together. |
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Physical property
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: a characteristic that can be sense. They can be determined without changing the composition of the element.
- Color - Odor - Volume - State - Melting and boiling points |
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Chemical property
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ability of a substance to change into other substances.
- Flammability and reactions with other acids - Example: The copper sheets that form the “skin” of the Statue of Liberty have acquired and greenish coating over the years. |
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Physical change
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a change of physical properties without changing the substance; a change of state.
- Example: a rock is broken into small pieces. |
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Chemical change
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a change in which the substance changes.
- Example: Iron combines with oxygen to form rust. |
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Homogeneous mixture
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a mixture that is the same throughout.
o Ex: salt and water |
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Solution
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another name for a homogeneous mixture
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Heterogeneous mixture
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- a mixture that contains regions that have different properties from those of other regions
o Ex: mixture of sand and water |
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Distillation
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a separation process that involves boiling water and leaving behind other minerals as solids
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Filtration
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- a physical method of separating minerals. Involves pouring a liquid through a mesh, such as filter paper, to separate the liquid from any solids.
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Robert Boyle
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first scientist to realize measuring was important
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J.J Thompson
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discovered electrons
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Lord Kelvin
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pudding model (Big positively charged pudding, with little raisins with a negative charge)
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Rutherford
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1911 – performed his Gold foil experiment
discovered proton and nucleus |
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Chadwick
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1932 - discovered the neutron, which has no charge
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Mendeleev
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figured out the periodic table
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Dalton’s Atomic Theory
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‘Law of Constant Composition’
1. all elements are made of tiny particles; atoms 2. all atoms of a given element are identical (this is not true today) 3. atoms of a given element are different from all others 4. atoms of different element can combine to form compounds in a given form. 5. atoms not created or destroyed in a chemical process. They change the way they group together. |
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Groups
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vertical columns on periodic table with similar properties.
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Names of the columns of elements?
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a) Alkali metals: 1A
b) Alkaline earth Metals: 2A c) Halogens: 7A d) Noble Gases: 8A- don’t bound with anything e) In the middle of 2A and 7A are transition metals. |
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Metals
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- solid at Room Temp.( 25 degress celicus)- expect Mercury
- shiny - Malleable: able to be flattened into sheets - Conduct heat and electricity - Ductile: ability to be stretched into wires |
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Non- metals
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- solid, liquid, or gas at room temperature
- not shiny - non malleable - not a conductor of heat or electricity - non ductile |
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Metalloids
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- touching the stair step expect for Aluminum which is a metal and Boron is a non metal
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Alltrope
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different forms of pure element
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Diatomics
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oxygen, nitrogen, hydrogen, fluorine, chlorine, iodine, bromine
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Diatomic molecules
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molecules made up of two atoms
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isotopes
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atoms of the same element with different # of neutrons
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Ions
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are produced by adding or removing one or more electrons.
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Cation
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positive ion
One or more electrons are lost from a neutral atom |
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Anion
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negative ion
One or more electrons are gained from a neutral atom |
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Ionic compounds
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when a compound forms between a metal and a nonmetal, it can be expected to contain these
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If a compound contains ions, it must:
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1. there must be both positive ions (cations) and negative ions (anions) present.
2. the numbers of cations and anions must be such that the net charge is zero. |
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Type 1 Compounds
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2 elements
~ Metal ~ Nonmetal * Not transition metals* (I- D- E) How to name type 1 compounds: KCl – Potassium chloride |
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Type 2 Compounds
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Ionic compounds
2 elements ~ Metal ~ Nonmetal * Transition metals* (Roman Numeral) How to name type 2 compounds: Fe3O2- Iron (III) oxide |
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Type 3 Compounds
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Non ionic compound
2 non metals (Use prefixes) Note- do not use the prefix mono on the first element Mono Di Tri Trenta Penta Hexa Hepta Octa |
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Polyatomic
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If a polyatomic ends in I-T-E use Hypo
If a polyatomic ends in A-T-E use Per How to name a polyatomic I-T-E- Sulfite- Hyposulfite A-T-E- Sulfate- Persulfate |
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Acids
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Acids always named with H+ and an anion
If an acid does not have oxygen: Name by: Hydro- element name- ic acid Example: Iodine- Hydroiodic acid If an acid does have oxygen: Name by: changing the ending of the anion A-T-E-: ic acid I-T-E: ous acid Example: HNO3- nitric acid HNO2- nitrous acid |
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Scientific Notation
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a number between 1 & 10 multiplied by a power of ten
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Qualitative
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describing based on looks
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Quantitative
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based on a measurement (needs a number and a unit)
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Adding and Subtracting exponents...
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exponents must be equal
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Multiplying exponents...
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multiply numbers, and add exponents
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Dividing exponents...
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divide numbers and subtract exponents
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Units/ Measurement
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o Length – Meter (m)
o Mass – Kilograms (kg) o Time – seconds (s) o Temperature – Kelvin (K) |
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Significant Digits
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o All non zero # are significant
o Leading zeros are not sig. o Captive zeros are sig. o Trailing zeros: If there is a decimal point then they are sig. Not decimal point means they are not sig. |
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Celsius to Kelvin
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C + 273
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Kelvin to Celsius
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K – 273
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Fahrenheit to Celsius
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F – 32/ 180
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Celsius to Fahrenheit
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180 (C) + 32
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Density of water
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1.00 g/mL
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Density =
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mass/volume
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Mole
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the number equal to the number of atoms that has a mass of grams
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Atomic mass
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1 mole of atoms in grams
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Avogadro’s number
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6.022 x 1023
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Moles to grams
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multiply by mass
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Grams to moles
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divide by mass
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Moles to atoms
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multiply by Avogadro’s number
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Atoms to moles
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divide by Avogadro’s number
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Molar mass
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the mass in grams of 1 mol of the substance
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Mass Percent
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The percent by mass of a component of a mixture or of a given element in a compound
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Percent Composition
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1. Find the molar mass of a compound
2. Divide each individual elements mass by the molar mass of the compound 3. Multiply the quotient by 100 |
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Molecular Formula
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The exact formula of a molecule giving the types of atoms and the number of each type
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Empirical Formula
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- The simplest whole number ratio of atoms in a compound.
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Calculating Empirical Formulas
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1. Step 1-Find the mass of each element
2. Step 2-Divide the given mass of an element by the its atomic mass (Convert into moles) 3. Step 3- Divide all moles by the smallest number of moles 4. Multiply the molar amounts to get whole numbers |
