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Atom :
smallest unit of element (ie: hydrogen)
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Elment:
form as on periodic table: (ie: H, Na, Ar)
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Ions:
charged atoms or moleules
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Molecule:
Two or more atoms bonded together (ie: H2, or H2O)
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Compound:
Two or more atoms of different elements (ie: H2O)
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Diatomic elements and list
- 7 elements in their simplest form that cannot exist as monotomic
- Hydrogen
- Nitrogen
- Fluorine
- Oxygen
- Iodine
- Chlorine
- Bromine
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Polyatomic:
elements that can exist with various formulas (ie: S6, S8)
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Allotropes:
elemental molecules with different formulas (ie: S6, S8)
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Molecular compounds:
all nonmetal molecules that combine to form compound
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Covalent bonds:
bonds between two nonmetal molecules
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Ionic compounds:
metal + nonmetal, with the exception of NH4Cl, which is ionic
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Ionic bonds:
bonds between metal and nonmetal molecule
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Non-metal elements:
starting with carbon, then going stepwise down to Iodine and everything above, and hydrogen
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Metalloids:
stepwise down stargint at Boron to At
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Polyatomic ions:
- ions made up of 2 or more atoms ? REFER to Quizlet memorization chart (name, formula and charges)
- One adjustment to flashcard: Mercury 1 = Hg2 +2 (listed as Hg2 + on flashcards)
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3 steps in naming ionic compound:
- 1. Name the metal
- 2. Write oxidation state of metal as roman numeral (except for exceptions)
- 3. Name non-metal using ?ide?
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Metals that don?t need roman numerals
Column 1 (+1), column 2 (+2), Al (+3), Zn & Cd (+2) and Ag (+1)
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Oxidation number rules for metals:
- Column 1: +1
- Column 2: +2
- Column 5: -3
- Column 6: -2
- Column 7 (Halogens ie:F & Cl): -1
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Naming molecular compound rules
- 1. Give prefix to first element (ie: if C6H12, will be hexa) but do not use mono if it?s 1
- 2. Name first element by REGULAR name on periodic table
- 3. Give prefix to second element (ie: N2O ? dinitrogen MONoxide)
- 4. Name the second non-metal element using IDE (ie: N2O ? dinitrogen monoxIDE)
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Molecular compound Pre-fixes:
- Mono: 1
- Di: 2
- Tri: 3
- Tetra: 4
- Pent: 5
- Hexa: 6
- Hepta: 7
- Octa: 8
- Nona: 9
- Deca: 10
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Binary acid naming: H-other element
- Hydro + insert name of element 2, replacing ine with ic acid
- Ie: HCl: hydrochlorIC ACID
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Oxyacid naming: Hx-middle atomy-Oz
- 1. If Z 0-2, name is ?hypo + name of second element, replacing ine with OUS ACID?
- 2. If z is 3, becomes ous acid WITHOUT Hypo
- 3. If Z is 4, becomes ic acid WITHOUT Hypo
- 4. If Z is more than 4, becomes ?Per + name of second element, replacing ine with IC ACID
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Strong acids (7)
- Binary acids:
- HCl: hydrochloric acid
- HBr: Hydrobromic acid
- HI: Hydroiodic acid
- Oxyacids:
- HClO3: Chloric acid
- HClO4: Perchloric acid
- HNO3: Nitric acid
- H2SO4: Sulfuric acid
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Units
- +12(terra) ? +9(giga) ? +6(mega) ?+3(Kilo) ? g
- g ?-2(centi) ?-3(milli) ? -6(micro) ? -9(nano)
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Significant figure rules
- Zeros btw numbers are sig figs (ie: 1005 is 4 sig figs)
- Zeros to the left of numbers NEVER significant (ie: 0.02 is 1 sig fig, 0.0026 is 2 sig fig)
- Zeros to the right of the numbers are significant ONLY if AFTER the decimal point (ie: 0.0200 is 3 sig figs, 3.0 is 2 sig figs), 5000.0 is ONE sig fig)
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When multiplying or dividng sig figs
Need answer to have same number of SIG FIGS as the one with the Fewest sig figs
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When adding or subtracting sig figs
Need answer to round so it has same number of DECIMALS as the one with the FEWEST decimals
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Beer-Lambert Law
- Absorbance = ecl
- e= Molar extinction coefficient (brighter colors have higher e)
- C=sample concentration
- L=path length btw light and detector
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How does spectrophotometry measure things:
- Thru Absorption, which refers to amt of light passing through
- Transparent material has ZERO absorption and opaque has 100% absorption
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One mole = 6.022 x 1023 atoms
- Every carbon (12g, or one mole) contains 6.022 x 1023 atoms
- When dealing with grams, try to convert to moles if possible, can work with moles to moles
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Balancing
- Start with the element that is only in one compound on each side first
- ie: CO + O2 ? CO2, start with carbon
- Chem rxns
- Combination: 2 or more products on one side and 1 PRODUCT on other (ie 2 Na + Cl2 ? 2 NaCl)
- Decomposition: 1 product converted into 2 or more products (ie 2 NaCl ? 2 Na + Cl2)
- Combusion: rapid rxn where hydrocarbon (CxHx) or alcohol (CxHxOH) rx with oxygen: PRODUCTS are ALWAYS CO2 & H20
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Combustion rxn
Product + 02(in excess) ? CO2 + H2O
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Molecular formula: actual chem formula ie: C6 H12 O6 glucose
- Vs empirical formula: most reduced formula ie: C H2 O glucose
- To find MOLECULAR Weight of chem C6 H12 O6, use the ATOMIC MASS (ie: carbons?s is ~12)
- So 12(6) + 1(12) + 16(6) = 72 + 12 + 96 = 180
- glucose?s percent comp of carbon?s % is 72/180 = 40%
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If 17.3% H and 82.7% C
Assume 100% is 100g, so 17g H and 82g C, then divide this by atomic mass (17.3/1 = 17.3)
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Empirical to molecular
- 1st: Divide molecular weight by weight of the empirical formula
- 2nd: multiply the subscript in empirical formula by amt in step 1
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Limiting reaction rules
- BCC
- Balance the equation
- Convert to MOLES
- Use the Coefficients in equations to transform MOLES of things you know with things you don?t
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Limiting reactant
- Reactant that runs out first
- Remember BCPAA
- Balance Equation
- Convert to moles
- Pick 1 of the reactants
- Ask and then answer: How many moles of the other reactant are needed to react w one I picked
- Do I have enough moles of that OTHER reactant? If yes, the one you chose is the LIMITING reactant
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To calculate percent yield
- Calculate the limited reactant and calculate, from limiting reactant, amount of product you?d form ?this value is theoretical
- The amt of product you actually get divided by theoretical x 100 = percent yield
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Atomic symbols
- Lower left is Atomic Number = # of protons of element, NEVER Changes
- Upper left is Mass # = Protons + neutrons
- # of neutrons = Mass# - Atomic Number
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Different atoms of same element CAN change # of _____, but NOT ______
Neutrons, NOT Protons
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Isotopes
- Atoms of same element with DIFFERENT MASS NUMBERS
- All have same # of protons, just diff # of electrons or neutrons
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Quantized distances
Similar to distances Electrons distances from nuclei can only exist at specific distances
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How many electrons in a neutral atom
Equal to the number of PROTONS
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