Lecture 2 Flashcards
(43 cards)
Types of bonds
- Covalent Bonds
- Noncovalent Bonds
Covalent bonds are formed by ________
Sharing of electrons
Types of Covlent bonds
Polar
Non polar
Difference between ethane and ethene
Ethane is free rotating
Ethene is more rigid, stronger, shorter and planar
Electronegativity
Tendency to attract electrons
Polar covalent bond
Electrons shared unequally
Non polar covalent bond
electrons shared equally
Increased Polarity increases
reactivity: less energy needed to break the bond
Covalent bonds are ________
Strong
What is bond length
Amount of energy requires to break a bond
Thermal energy
Average energis of impacts molecules undergo
Relationship between bond length and thermal energy of the cell
Bond length»_space;»» thermal energy of the cell
Ionic Bonds
- Non covalent bonds
- Attraction between charged atoms
- NaCl (table salt)
- Equal electron sharing
Ionic bonds in crystal form are ______
Stronger
In solution ions are surrounded by H2O hence
easily disruptable
Hydrogen Bonds
- Non covalent bond
- H,O,N
hydrophobic interactions
Polar molecules: Hydrophilic
Non Polar molecules: Hydrophobic (Driving force for forming vesicular structure)
Van der Waals forces
- Weak Force
- Hold together neutral molecules
- Operate at optimum distances
- Maximized by complimentary surfaces
Properties of Water
- Highly asymmetric
- Polarized covalent bonds
- All 3 atoms can H - Bond
Life Supporting properties of water
- Dissolving power
- H- Bonding
- Temperature regulation
- Versatility in physical states
Acids
Release H
Bases
Accept H
Macromoleucles
- Huge Polymers
- Formed by building monomers
Polymerization
Process of linking monomers