CHEM 121 FINAL EXAM | UPDATED QUESTIONS AND ANSWERS UPDATED .Buy Quality Materials!
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Course
CHEM 121
Institution
CHEM 121
CHEM 121 FINAL EXAM | UPDATED QUESTIONS AND ANSWERS UPDATED .Buy Quality Materials!
describe photoelectric effect
light shining on certain materials cause it to emit electrons
define a collapse in terms of quantum theory
collapse of probability
once something happens, there is no more pr...
CHEM 121 FINAL EXAM | UPDATED QUESTIONS AND
ANSWERS UPDATED .Buy Quality Materials!
describe photoelectric effect
light shining on certain materials cause it to emit electrons
define a collapse in terms of quantum theory
collapse of probability
once something happens, there is no more probability for what it could be. it is what it is.
describe the stationary state hypothesis
as per Bohr, electrons dont emit radiation unless theres a reason for the energy level of
the electron to change
in the equation
λ = h/(mv) = h/p
what does each variable represent
λ = wavelength
h = plancks constant
m = mass
v = velocity
p = momentum
what does schrodingers wavelength equation give
describes he behaviour of a quantum states possible state
define the aufbau principle
electrons fill lower energy orbitals first
define hunds rule
electrons must fill all available orbitals in the shell before doubling
what are the 4 quantum numbers and what do they describe
1. principle quantum number (n)
- tells the energy level and size
2. angular momentum quantum number (l)
- determines orbital shape
- values: 0 to (n-1)
- different values correspond with diff. orbital shapes
3. magnetic quantum number (m)
- specifies orbital orientation
- values: [-l, l]
- gives the number of possible orbital orientations
4. spin quantum number (s)
, - describes the behaviour of the electron in a pair
- values: [-1/2, 1/2]
define the pauli-exclusion principle
no two electrons in an atom can have the same four quantum numbers
define ionization energy
energy required to remove an electron from an atom
describe trend of ionization on a periodic table
increases left to right
increases bottom to top
define electronegativity
the tendency for an atom to attract an electron
describe the trend of electronegativity on a periodic table
increases left to right
increases bottom to top
describe the trend of atomic radii on a period table
increases right to left
increases top to bottom
define electron affinity
amount of energy absorbed or released when an atom accepts an electron
name the 3 bond types
1. covalent - sharing of e
2. ionic - transferring of e
3. metallic - sea of e - e are free to move throughout the structure
name the types of reactions
1. combination
2. decomposition
3. single replacement
4. double replacement
5. combustion
6. acid-base
7. red-ox
in a redox reaction, what is what
reduction: the one gaining an e / decrease in O-state
oxidation: the one losing an e / increase in O-state
define allotropes
elements that occur in different forms
ex. carbon - diamond and graphite
define liquid elements
elements that are liquid at STP
(Hg, Br, Fr)
define half reactions
reactions wherein the e are tracked separately from atoms
give description of acids
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