Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
51 Cards in this Set
- Front
- Back
|
g --> mol
|
g x 1 mol / average atomic mass
|
|
|
mol --> grams
|
mol x avg atomic mass/mol
|
|
|
atoms --> mol
|
atoms x 1 mol/6.022x10^23
|
|
|
moles --> atoms
|
mol x 6.022x10^23 / 1 mol
|
|
|
atoms --> g
|
atoms x avg. atomic mass/6.022x10^23
|
|
|
g --> atoms
|
g x 6.022x10^23 / avg. atomic mas
|
|
|
Equation to get molecular formula
|
molar mass of compound / empirical formula mass
|
|
|
diatomics
|
HYDROGEN HON
-helium -oxygen -nitrogen |
|
|
precipitation reaction forms ...
|
solids!
|
|
|
Arrhenius acid
|
H+
|
|
|
Arrhenius Base
|
OH-
|
|
|
Nitrate
|
NO3-
|
|
|
Sulfate
|
SO4 -2
|
|
|
precipitation reaction
|
single replacement
- AB + CD --> AC + BD |
|
|
acid base reaction
|
acid + base --> salt + water
- example = HCL + NaOH -> NaCl H2O |
|
|
oxidation reduction reactions
|
transfer of electrons
- between a nonmental and a metal |
|
|
single replacement (type of oxidation reduction reaction)
|
A + BC -> B + AC
|
|
|
combustion (type of oxidation reduction reaction)
|
-prescense of 02
-C reactant -products are CO2 and H2O |
|
|
synthesis (type of oxidation reduction reaction)
|
two molecules coming together to make on big one
-- example: H2 + 02 -> H20 |
|
|
decomposition (type of oxidation reduction reaction)
|
one reactant broken down into two smaller molecules
|
|
|
g - mol - mol - g
THE STEPS |
1) balance
2) g -> mol: g x mol / mm 3) mol ratio: unknown/known coeficient 4)mol -> g: mol x mm/mol |
|
|
Bohr's model
|
-positive nucleus with electrons orbiting in quantized levels
|
|
|
s orbital
|
1
O -- what it looks like |
|
|
p orbital
|
3
00 -- what it looks like |
|
|
d orbital
|
4 lobes
5 |
|
|
metals ______ electrons
|
lose
|
|
|
nometals _______ electrons
|
gain
|
|
|
ionic bond
|
between opposite charged ions
|
|
|
covalent bond
|
electrons shared equally
|
|
|
polar covalent bond
|
electrons not shared equally
|
|
|
Electronegativity chart
|
0 = covalent
low - 1.9 = polar covalent greater than 2.0 = ionic |
|
|
the lowe the Electronegativity the more ________ it is
|
POSITIVE
|
|
|
dipole
|
+----->
+ is the positive end -> is the negative end |
|
|
when making lewis structures and you have a positive charge : :
|
need brakets with charge on outside of them
subtract charge |
|
|
when making lewis structures and you have a negative charge : :
|
need brakets with charge on outside of them
add charge |
|
|
resonance
|
molecule with more than one valid lewis structure
|
|
|
metals _____ electrons to become like ______ noble gas
|
lose
previous |
|
|
nonmetals ______ electrons to become like _____ noble gas
|
gain
next |
|
|
order of orbitals on periodic table
|
s
d - has one less than s and p p f - f has 2 less than s and p |
|
|
Pauli exclusion principle
|
only 2 e- are in an orbital and they have one of each spin
|
|
|
order of boxes
|
1s
2s 2p |
|
|
Carbonate
|
CO3 -2
|
|
|
sulfuric acid
|
H2SO4
|
|
|
Hydroxide
|
OH-
|
|
|
Nitric Acid
|
HNO3
|
|
|
resonance
|
molecule with more than one valid lewis structure
|
|
|
metals _____ electrons to become like ______ noble gas
|
lose
previous |
|
|
nonmetals ______ electrons to become like _____ noble gas
|
gain
next |
|
|
order of orbitals on periodic table
|
s
d - has one less than s and p p f - f has 2 less than s and p |
|
|
Pauli exclusion principle
|
only 2 e- are in an orbital and they have one of each spin
|
|
|
Ammonium
|
NH4+
|
