Electron configuration
Coulomb’s Law: allows us to quantify the force between the atomic nucleus (atoomkern) and the
electrons
- It comes down to the charges and the distance between the charges
𝑄 𝑄
𝐹=𝑘
𝑟
Ionization Energy: the amount of energy needed to pull the electron away
𝑄 𝑄
𝐸=𝑘
𝑟
Energy level of electrons
Electrons that you can put inside
2 6 10 14 Energy level
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d 6f
Octet rule: you have to have 8 electrons in the outermost shell by interacting with other atoms
Addition of electron increase radius
Dictate strength / melting point
Removal of electron decreases radius
Radius anion (negative) > ration cation (positive) (compared to a neutral atom)
Types of intermolecular bonds
1. Hydrogen bonds
2. Dipole-dipole
3. London dispersion forces
Polarity: the condition where electrons of the molecule spend more time near the atom with higher
electronegativity
Covalent bonds
- Electron sharing
Metallic bonds
- Electron dispersion
- The electrons can move freely in a configuration knows as sea of electrons
Ionic bonds
- Electron transfer
- It has an electron donor and one electron acceptor atom
, Bonding energy curve
- Deeper energy well higher melting temperature
higher stiffness (higher E modulus when stiffer)
- Asymmetry curve thermal expansion
Interatomic bonds
- Occur between individual atoms within a molecule
Intermolecular bonds
- Occur between two individual molecules
Coulomb’s Law: allows us to quantify the force between the atomic nucleus (atoomkern) and the
electrons
- It comes down to the charges and the distance between the charges
𝑄 𝑄
𝐹=𝑘
𝑟
Ionization Energy: the amount of energy needed to pull the electron away
𝑄 𝑄
𝐸=𝑘
𝑟
Energy level of electrons
Electrons that you can put inside
2 6 10 14 Energy level
1s
2s 2p
3s 3p 3d
4s 4p 4d 4f
5s 5p 5d 5f
6s 6p 6d 6f
Octet rule: you have to have 8 electrons in the outermost shell by interacting with other atoms
Addition of electron increase radius
Dictate strength / melting point
Removal of electron decreases radius
Radius anion (negative) > ration cation (positive) (compared to a neutral atom)
Types of intermolecular bonds
1. Hydrogen bonds
2. Dipole-dipole
3. London dispersion forces
Polarity: the condition where electrons of the molecule spend more time near the atom with higher
electronegativity
Covalent bonds
- Electron sharing
Metallic bonds
- Electron dispersion
- The electrons can move freely in a configuration knows as sea of electrons
Ionic bonds
- Electron transfer
- It has an electron donor and one electron acceptor atom
, Bonding energy curve
- Deeper energy well higher melting temperature
higher stiffness (higher E modulus when stiffer)
- Asymmetry curve thermal expansion
Interatomic bonds
- Occur between individual atoms within a molecule
Intermolecular bonds
- Occur between two individual molecules
