Exam 1 (chapters 1-4) Flashcards
10^6
mega- (M)
10^-6
micro- (µ)
10^-9
nano- (n)
Aufbau Principle
e- fills the lowest energy level first
3*10^8 m/s
Speed of light
Hund’s Rule
-e filled in the same energy level in 1 orbital at a time and is oriented in the same direction
no two e- in an orbital can have the same spin
Pauli Exclusion Principle
the ion with the most protons is the smallest b/c there are more protons in the nucleus to pull fewer e- in the shells
for ions of an isoelectric series:
How can you tell if an element is in an excited state from the electron configuration?
subshells that are not the last sub shell are not filled
ℓ =0
Sub-shell s
-spherical
ℓ=1
sub-shell p
3 orbitals
dumbbell shape
ℓ=2
Sub-shell d
5 orbitals
cloverleaf shaped
ℓ=3
Sub-shell f
7 orbitals
Cr electron configuration
[Ar]4s^1 3d^5
(2 *ℓ)+1
number of orbital or _ in a configuration
Cu electron configuration
[Ar] 4s^1 3d^10
Electron affinity (EA)
The energy change associated with the addition of an electron to a gaseous atom
energy absorbed during the gain of an e-
EA is endothermic
energy is released during the gain of an e-
EA is exothermic
an atom is ionized when
an e- is leaving an atom; n(final)=∞
attractive interactions are
negative
repulsive interactions are
positive
atoms of the same element with different neutrons
isotopes
mechanical kinetic energy
-moving mass
-mechanical pot. energy
-stored mass in a place where a force acts
electrical kinetic energy
-moving charge
-electrostatic pot. energy b/c or the interaction of charged particles
light kinetic energy
-moving photons
-chemical pot. energy
-stored in bonds
heat enters a system
+q
heat leaves a system
-q
work is done on a system
+w
work is done by the system
-w
state function
a function that depends only on the initial and final states of a system, not the path in between.
-represented by uppercase letters, P, V, H, T
electrostatic energy
proportional to the magnitude of the charges
inverse to the distance between particles
enthalpy
heat transferred at a constant pressure
exothermic process
when energy (often as heat) leaves a system into the surroundings
endothermic process
energy (as heat) is added to a system
hc/λ
E(photon)=
Gamma ray wavelength range
<10^-8
UV and visible wavelength range
10^-8 to 10^-6
infrared wavelength range
10^-6 to 10^-4
microwave wavelength range
10^-4 to 10^-1
radio wavelength range
10^0 to 10^4
black body radiaiton
radiation emitted by an object
when light is reflected or transmitted…
the complementary color is absorbed
transmitted light
is not absorbed, passes through
when interacting with matter, gamma rays, x rays, UV rays…
-ionize atoms and molecules
-break chemical bonds
when visible spectrum rays interact with matter (electronic transitions)
e- is promoted to higher energy
when infrared rays interact w matter
increased amplitude of vibrations (KE goes up)
microwave interactions with matter
rotations increase
radio waves…
flip nuclear spin
lowest energy is when
closest to p+ (ground state)
electron transition causes
e- moves from one allowed energy state to another
e- changes energy levels emitting/absorbing photons
principle quantum number (n)
-info on orbital size
-defines what shell e- is in
info on orbital energy
quantum number ℓ
determines shape
magnetic quantum number (mℓ)
-describes orientation of orbital in 3D space
- ranges from -ℓ to ℓ
node
no electrons
n-1=nodes
core shielding
- inner e- shield valence e- from nucleus
- outer e- experience less Ze and have a weak attraction
- outer e- have less energy
atomic radius
increases down a group
decreases across a period
ionization energy
energy needed to remove e- in gaseous state
always positive
increases across a period
decreases down a group
Zeff for valence e-
increases down a group and across a period
EA is more negitive
across a period
size of ion relative to parent atom
anion>parent>cation
isoelectic series
group of atoms or ions that have the same number of e- (same ground state configuration)
effective nuclear charge (Zeff)
net positive charge experienced by valence e-
when valence e- are further from the nucleus
more reactive
metallic character and reactivity increase
as ionization energy decreases
IE=
energy needed to form a positive ion
E(g) –> (E+) + (e-)
ionization energy representation
electron affinity representation
E(g) + (e-) –> E(g)-
p block elements, nonmetals
elements that have ionization energies > 1000
metals s,d,f block elements
elements that IE<1000
potential energy
-stored energy
- not a state function (path matters)
1000J
1KJ
Planck’s Constant
6.63*10^-34 m^2kg/s
Avogadro’s Number
6.02*10^23
Moles to grams conversion
of moles * molar mass
