Atomic And Electronic Structure Flashcards
Energy, frequency and wavelength relationship
Energy and frequency are directly related. Wavelength is inversely related to energy and frequency. The HIGHER the frequency, the GREATER the energy and the SHORTER the wavelength
Electromagnetic radiation from lowest energy to highest energy:
Lowest energy (highest wavelength)
Roman
Men
Invented
Very
Unusual
X-ray
Guns
Highest energy (shortest wavelength)
(Roman Men Invented Very Unusual X-ray Guns)
Is N2 paramagnetic or diamagnetic?
Diamagnetic
Is O2 paramagnetic or diamagnetic
Paramagnetic
The strength of ionic bonds depend on:
The charge: the greater the charges of the ion the stronger the bond
The size: the smaller the size of the ion the stronger the bond
electron configuration of chromium (Cr):
[Ar] 4s1 3d5
electron configuration of copper (Cu):
[Ar] 4s1 3d10
electron configuration of silver (Ag):
[Kr] 5s1 4d10
electron configuration of gold (Au):
[Xe] 4f14 6s1 5d10
cations
- positively charged
- atoms that have lost one or more electrons
anions
- negatively charged
- atoms that have gained one or more electrons
what does Heisenberg uncertainty principle describe?
- it is impossible to perfectly find both, the momentum and the location, of an electron in an atom
- we can only figure out one or the other
bonds that have ____ lone pairs on their atoms will generally have lower bond strength. why?
- more
- due to the repulsion between the lone pairs weakening the covalent bond
what are the four aspects that bond strength depends on?
1) bond order
2) atomic radii
3) polarity
4) lone pairs
formula for calculating formal charge:
formal charge = (# of valence e-) - (# of nonbonding e-) - (# of bonds)
1 lone pair = 2 nonbonding e-, double bond = 2 bonds
what atoms cannot obtain a full octect?
Hydrogen, helium, lithium, berylium and boron
principle quantum number (n)
- represent main energy level occupied by electrons
- n = the row the atom is in
azimuthal quantum number (l)
- describes the shape of the subshells/ orbital shape within each principle energy level
- s, l = 0
- p, l = 1
- d, l =2
- f, l =3
magnetic quantum number (ml)
- describes the orientation of orbitals in space
- s, (ml) = 0
- p, (ml) = -1, 0, 1
- d, (ml) = -2, -1, 0, 1, 2
- f, (ml) = -3, -2, -1, 0, 1, 2, 3
spin quantum numeber (ms)
- describes the angular momentum of an electron
- either -1/2 or + 1/2
- electrons in the same orbital must have atiparallel spins
aufbau principle
- subshells get filled from lower energy to higher energy
what does electron configuration tell us?
- the number of electrons in each energy level and the organization of how the subshells are ffilled
characteristics of covalent bonds:
- formed between 2 different atoms in which electrons are shared
- atoms typically have similar electronegatvity
- usually involves 2 non-metals
covalent bonds are ____ than ionic bonds, so they have ____ melting and boiling points
much weaker
lower
what are covalent bonds characterized by?
- bond length: distance between the nuclei of each atom (triple bonds are the shortest, single bonds are longest)
- bond energy: energy needed to break the covalent bond (triple bonds have the highest bond energy, single bonds have the lowest)
- polarity: sharing of electrons (unequal sharing = polar due to dipoles, equal sharing = non-polar)
how many orbitals does the s subshell have?
one, spherical shape
how many orbitals does the p subshell have?
3, barbell shapped, lie on the x, y, and z axes
