Nature of molecules, Chapter 2 Flashcards
Anatomic number
Determine by the number of protons in the nucleus
Anatomic Mass
- Sum of protons and neutrons
- measured in Daltons 6.02x1023 daltons/1 gram
Cation
Positive charge
Anion
Negative charge
Isotopes
- Atoms of a single element with a different number of neutrons
- Named based on their atomic mass
Radioactive Isotope
- unstable meaning their nucleus has a tendency to break apart= Radioactive decay
Half-life
- the time it takes the atoms to decay
- half of whatever isotopes has decay
Carbon 14
- Use for living tissue bond
- Carbon isotopes exist natural in known ratios
Bohr Model
Way to view anatomic structure, with electrons in discrete orbitals
Orbitals
Around a nucleus where electrons are most like
Oxidation
loss of electrons
Reduction
Gain of electrons
Rule of 8
Atoms establish completely full of outer energy levels (8 electrons)
Elements found in the 96.3% weight of your body
Carbon, hydrogen, Oxygen, Nitrogen
Ionic Bond
- Attraction of opposite charges, strong
- Form crystals
Covalent bonds
Sharing Electrons pairs, very strong
Hydrogen bonds
Sharing of hydrogen atom- has 1 electron
Hydrophobic Interaction
Forcing of the hydrophobic portion of molecules together in the presence of polar substances, weak
- Double convents bonds
- Triple covalent bonds
- Share 2 pairs of electrons
- Strongest covalent bonds
Polarity- Nonpolar
- Bonds between identical atoms
- The affinity for electrons is the same and electrons are shared equally
Polar bonds
- Charge is not uniform
Chemical reactions
formation of making and breaking chemical bonds
Reactions
Molecules before a reaction starts
Products
The molecule resulting from a chemical reaction
Chemical reactions impacted by?
1) Temperature
2) Concentration of reactants and products
3) Catalysts- substances
Water molecules is a?
Polar covalent bond
Most important chemical property of water is ?
Hydrogen bonds
Cohesion
- Polarity of water allows water molecules to be attracted to one another
- Responsible for being a liquid (not gas)
adhesion
Water adheres to any substance with which it can form hydrogen bonds
Capillary action
water is attracted to polar molecules- this is responsible for capillary action
Emergent properties
- Water has a high specific heat
- water has a high heat of vaporization
- Solid water is less dense than liquid water
- Water is good solvent
- Water organizes non polar molecules
Hydratation shell
Prevents them from associating with other crystal lattice
Hydrophobic exclusion
Nonpolar molecules aggregate in water
Nonpolar molecules are?
Hydrophobic- not form H-bonds with water
Spontaneous ion formation
ionization
pH measures?
Concentration
Substance that disassociates in water to increase the H+ concentration?
Acid
Any substance that combines with H+ when dissolved in water(lowering H+ concentration
Base
- Resist changes in pH
Buffer
In human blood is an acid-base pair consisting of carbonic acid (acid) and bicarbonate (base)
The key buffer
