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CHEM 1211: Test 1
Number of Protons =
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Atomic Number
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Atomic Number
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Number of Electrons = Number of Protons =
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Number of Neutrons = Mass Number - Atomic Number
Isotope abundance
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Number of isotope atoms / number of all atoms
Has to equal 100% so average amount equals (first rate)(x)+(second rate)(1-x)
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coeeficient
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is a multiplicative factor in a term of an expression, so both numbers are coefficients in the math sense;
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subscript
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is used in chemistry to indicate the stoichiometric ratio within a chemical formula
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Anion
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Negative charged ion (there are two "n"s in the word)
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Cation
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Positively charged metallic ion
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Rules for naming Ionic Compounds
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----1. write the name of the POSITIVELY charged ion of the compound (often it's a metal)
----2. write the root word of the second element in the compound
----3. add -ide to the root name of the element if the negative ion is a single element
(ex. Chlorine becomes Chloride)
---4. or add -ate or -ite if the negative ion is polyatomic
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Group 1A
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Alkali Metals
1 electron in outer energy level
1
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Group 2A
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-alkaline earth metals
-harder, denser, higher melting point than alkali metals
-form 2+ cations
-less ractive
-heavier alkaline are more reactive than lighter
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Group 3A
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B, Al, Ga, In, Tl
Al, Ga, In, Tl metals
B is metalloid
All form compounds analogous formulas such as BCl_3_, AlCl_3_
+3 ions
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Group 4A
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consists of 2 non metals, the rest are metals, form cations and anions, ionic charge of +/-4.
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Group 5A
Ionic compounds
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oppositely charged ions that are held together by ionic bonds
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covalant (molecular)
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nonmetal and nonmetal
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molar mass
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grams/mole
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Avagadro's Number
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6.02x1023
Avagadros number is the amount of atoms per mole. 1 mole of Cl equals, avagadros number.
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the good King Henry Died Drinking Chocolate Milk
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Tara 12 T Pico -12 p
Giga 9 G Nano -9 n
Mega 6 M Micro -6 u
Kilo 3 K Milli -3 m
Hecta 2 H Centi -2 c
Deca 1 Da Deci -1 d
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Show exponents in webassign
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e2 or e-2
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significant figures
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1. Non-zero digits are always significant. 123
2. Any zeros between two significant digits are significant. 101
3. A final zero or trailing zeros in the decimal portion ONLY are significant. 0.100
4. Leading zeros are not sig 0.01
5. trailing ceroes in whole number not sig 1200
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density
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d=m/v
measured in mass per unit of volume
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mL to cm^3
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1mL = 1cm^3
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1 pound = kg
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0.45 kg
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1 kg= __ pound
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2.20 pound (av)
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pounds to grams
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1 pound = 454 g
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Conversion: Temperature: F C K
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c to f *9/5+32
f to c -32*5/9
c to k kelvin = 273.15 + Celsius
k to c °C = K − 273.15.
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Amonium
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Symbol = NH4
Charge = +1
Always soluble
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Cyanide ion
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CN
-1 charge
Anion neg 4A
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Acetate
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Acetate CH3CO2 or C2H3O2
-1 charge
Always soluble
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Carbonate
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CO3
-1 charge
Anion neg 4A
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Hydrogen Carbonate
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HCO3
Hydrogen Carbonate or bicarbonate
-1 charge
Anion neg 4A
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oxalate
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C12O4 -2
4A
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Hypochlorate Ion
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ClO-
-1
Anion neg 7A
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Chlorite
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Chlorite
ClO2
-1
Anion neg 7A
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Perchlorate
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Perchlorate
ClO4
-1
Always soluble
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Nitrite
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NO2 -1
Anion neg 5A
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Nitrate
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NO3
-1
Anion neg 5A
Always soluble
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Phosphate ion
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PO43-
Anion neg 5A
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Hydrogen phosphate ion
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HPO42-
Anion neg 5A
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Dihydrogen Phosphate ion
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H2PO4
-2
Anion neg 5A
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Chromate ion
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CrO4 2-
Anion neg transition metal
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Dichromate ion
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Cr2O7 2-
Anion neg transistion metal
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permanganate ion
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MnO4 -1
Anion neg transition metal
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Hydroxide IOn
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OH -1
Anion neg 6A
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Sulfite
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SO3 2-
Anion neg 6A
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Sulfate ion
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SO4 2-
Anion neg 6A
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Hydrogen sulfate ion
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HSO4 -1
Anion neg 6A
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What is the percent abundance of each isotope
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average=substance one *x+ substance 2*(1-x)
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subscript .coefficient .
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subscript . It indicates that each molecule of XeF6 contains 6 F atoms. The 6in 6 CsCl is a coefficient . It indicates that there are 6 formula units of CsClpresent.
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molicules to moles
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molicules * 1 mol/6.022e23=moles
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Molecular Formula
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exact formula of a molecule, gives type and number of atoms
emperical molar mass (add masses of all components) devided by Molar mass
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find empirical formula from percentages
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assume 100g of compound so that mass = %
make table -
percent, mass (g), moles, divide by smallest, multiply for whole #'s, round
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find percent mass
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1. multiply atomic weight by the number of atoms it contributes to the empirical formula
2. divide by weight of all atoms in molecular formula
3. multiply by 100
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Change in the internal energy of the system
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ΔE = q + w
energy = heat + work
Heat raising is positive
Energy going to system from surrounding positive, leaving system to environment negative
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Work is
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w = −PΔV
or -P (Volume 2-volume 1)
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To convert L·atm to joules (J),
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1 L·atm = 101.325 J
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State function
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Only interested in the relevent state (temp, pressure, volume), and not on the path it took to get to that state.
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Enthalpy change
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ΔH = qP = ΔE + PΔV
Heat change in system eqauls heal lost or gained at constant pressure equals change in internal energy + pressure (volume 2-volume 1)
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