Chapter 1- Atomic Structure Flashcards
(Z)
Atomic number. Different for each elements. Tells the amount of protons in an element
(A)
Atomic number. Tells the number of protons and neutrons in the nucleus of an elements.
Isotope, What subatomic particle differs between isotopes?
Atoms that share an atomic number (Z) but have different mass numbers (A)
Different number of neutrons.
Fundamental unit of charge
e= 1.6x10^-19
Proton + 1.6x10^-19
Electron - 1.6x10^-19
Between electrons and protons which is larger?
Protons.
Electrons are approximately 1/2000 the size of a proton
Electrons closer to the nucleus have higher low energy levels. Electrons further away from the nucleus have higher low energy levels
Electrons closest to the nucleus have low energy levels while electrons further away from the nucleus have high energy levels which is why they are the electrons that interact with other molecules.
Higher energy level equals less negative
Cation vs Anion
Cation: positively charged atom
Anion: negatively charged atom
Atomic weight vs Atomic mass
Atomic mass is nearly equal to an atoms mass number, the sum of protons and neutrons.
Atomic weights is the weighted average of all of an atoms different isotopes.
Avogadro’s number
6.02×10^23
A mole is equal to Avogadro’s number 
Planck’s equation
E=hf
E=energy of a quantum (Energy emitted from matter comes in discrete bundles called quanta) 
Planck’s constant (h) 6.26×10^-34 J x s
f= frequency of radiation
Planck’s constant
(h)
6.26×10^-34
E
E=energy of a quantum
Energy emitted from matter comes in discrete bundles called quanta
Speed of light
C is equal to 3×10^8m/s
What equation do you use to calculate the angular momentum of an electron orbiting a hydrogen nucleus?
L=nh/2pi
L=nh/2pi
Equation that tells the angular momentum of an electron orbiting the nucleus
L:angular momentum
n: principal quantum number
h: planck’s constant
How to calculate the energy of the electron?
E=-Rh/n^2
E: Energy of the electron
Rh: Rydberg unit of energy (experimentally determined) 2.18-10^-18 J/electron
n: distance from nucleas (bigger the n the greater the energy, less negative)
Ground state versus excited state
Ground state is the state of lowest energy (smaller in value) excited state is when one electron is moved to a sub shell of higher than normal energy.
From a lower energy level to a higher energy level they get…
AHED
A- Absorb light
H-Higher potential
E-Excited
D-distance (from the nucleus)

How do you determine the electromagnetic energy of a photon?
E=hc/lambda
Electromagnetic energy
H=planck’s constant
C=speed of light (3x10^8m/s)
Lambda=Wavelength of the radiation
When an electron returns back to ground state does is energy absorbed or omitted?
Energy is emitted through a photon
How do you calculate the energy of the emitted photon when it moves from a higher initial states to a lower initial state?
E=hc/lambda= -Rh[1/ni^2-1/nf^2]
Rh: Rydberg unit of energy (2.18×10^-18 J/electron)
Moving from high to low energy levels versus moving from low to high energy levels
Moving from high to low energy levels energy is emitted (emission). Moving from low to high energy levels energy is absorbed (absorption) 
n
Principal quantum number.
Gives you the shell an electron resides in.
Possible values include nonzero integers
l
Azimuthal (angular momentum) quantum number
Tells you the shape and number of subshells
Possible values include 0 to n-1 
ml
Magnetic quantum number
Tells you the particular orbital within a subshell where an electron is most likely to be found at a given moment of time.
Possible values between -l and +l
Maximum number of electrons per orbital
2
Which blocks of the periodic table do the following azimuthal numbers correlate with: I=0, I=1, I=2, l=3.
I=0 s
I=1 p
I=2 d
l=3 f
How do you figure out the maximum number of electrons within a sub shell?
4l +2
Shape of s orbital vs p orbital
Orbitals in the s subshell are spherical, the three orbitals of the p subshell are dumbbell shaped and aligned along the XY and Z axis
ms
Spin quantum number
Possible orientations include +1/2 and -1/2
n+1 rule
A rule that shows you which subshell should be filled first. The lower the sum of n+l the lower the energy of the subshell.
If two subshells possess the same n+1 value the subshell with the lower n value will fill first.
Or you can just read the periodic table 😜
How do you find the electron configuration of an ion?
For a cation electrons are removed from the highest sub shell
For an anion electrons are added to the highest subshell
Elements in which period and below accepts electrons into their d subshell which allows them to violate the octet rule
Period 3
Hunds rule
Within a given sub shell orbitals are filled such that there are a maximum number of half filled orbitals with parallel spins. Electrons would prefer to have their own are available for being forced to double up with another electron.
Half filled and fully filled orbitals have a lower energy than other states.
Which elements and their groups are the exceptions to electron configuration?
Chromium (4s1 3d5) and Copper (4s1 3d10)
One electron is moved from the 4s sub shell to the 3d sub shell to allow the 3d subshell to be half filled
Paramagnetic
Material composed of atoms with unpaired electrons orient their spins in alignment with the magnetic field. The material willl thus be weakly attracted to the magnetic field.
Paramagnetic means the magnetic field will cause parallels in unpaired electron therefore causing attraction. 
Diamagnetic
Materials with items that only have paired electrons will be slightly repelled by a magnetic field.
When drawing an orbital diagram how many orbitals are in the s,p,d subshells?
S=1
P=3
D=5
Heisenberg uncertainty principle
Position and velocity are related and cannot be simultaneously determined
Hunds Rule
Electrons in a subshell will only pair when the orbital is half filled
Aufbau’s principle
Electrons will fill lower energy orbitals before filling higher energy orbitals
Pauli’s exclusion principle
No two electrons in an atom can have the same exact quantum numbers
