Bonding

Question 1

Coulomb’s Law

Answer 1

(+q)(-q)/r^2

• Bigger charges mean bigger bonds, smaller charges mean smaller bonds
• Charges closer together mean stronger bonds

Question 2

Ionic Bonds

Answer 2

• One atom takes away valence electrons from the other electron
• Usually between metals and non-metals
• Electrons held in a lattice structure-poor conductor of electrons as a solid, but good conductor as a liquid

Question 3

Covalent Bonds

Answer 3

-Electrons are shared
- First covalent bond is a sigma bonds (σ), and all the following are pi bonds (π)
-Double and Triple Bonds are stronger than single bonds
- Sometimes electrons shared equally, but when one electronegativity is stronger than the other, electrons pulled to one side creating positive/negative side =dipole moment
Greater Charge, Larger Distance >Larger Dipole Moment> More polar

Question 4

Lewis Diagram Exceptions

Answer 4

BeH2-> Beryllium can be stable with 4 valence elections
BF3-> can be stable with only six valence electrons
PCl5, SF4, SF6, Elements with a d-subshell can accept more than 8 valence electrons
NO and NO2 have an odd number of electrons

Question 5

Network Solids

Answer 5

Lattice of Covalent Bonds
Hard, have a high melting point
Electrons held in a lattice, poor heat conductors
EX. compounds of carbon(diamond), SiO2

Question 6

Metallic Bonds

Answer 6

• Sea of freely moving electrons
• Malleable and Ductile
• High boiling and melting points
• Good conductors of heat and electricity

Question 7

Dipole-Dipole

Answer 7

• Weak bonds, low melting and boiling points

- Happens only in polar molecules

Question 8

London Dispersion

Answer 8

• Non-polar Molecules
• Weak, low boiling and melting points
• More electrons =stronger london dispersion

Question 9

Hydrogen Bonding

Answer 9

• When a hydrogen is bonded to N, O or F
• Stronger than di-pole di-pole
• reason why water is less dense as a solid than a liquid