Module 2: Chemistry And Biochemistry Flashcards
3 types of mixtures
Solutions, colloid, suspensions
Solutions
Solute particles are very tiny, do not settle out or scatter light. Tends to not have any color to it.
e.g., mineral water
Colloid
Solute particles are larger than in a solution and scatter light; do not settle out (proteins). Do have color to it.
e.g., jello-o
Suspension
Solute particles are very large, settle out, and may scatter light e.g. Blood
What are the ways we can note the concentrations of a solution?
% (D5 = 5% dextrose solution) *IV fluid
mg/dL or mg/L
molarity (mmol/L)
1 mol =
of grams of an element/compound equal to atomic weight of that substance
– this gives equal number of particles in the solution
avogadro’s number
Molarity
1 mole dissolved in enough solvent to give IL volume
Molarity (M) of a solution is expressed in
Moles of solute/liters of solution
Molality (m) is expressed in
Moles of solute I mass of solvent (kg)
Molality
I mole dissolved in IL of solvent
Biological solutions are - solutions
Molal
Bonding occurs between
Electrons in the valence shell
How many electrons do most elements want
8
How many elections does hydrogen want
2
How can we make a complete shell
In order to make a complete shell, we can either lose extra electrons to go down to the next shell, or we can add electrons to the outer shell to make it complete
Types of chemical bonds
Ionic
–Anion vs cation
–Salts
Covalent
–Nonpolar
–Polar
–Hydrogen bonds
What happens in ionic bonding
Electrons are transferred from one element to another
Causes them to have a charge (either +/-) depending if they lost or gained an electron
What happens in covalent bonding
Electrons are shared
What happens in covalent bonding
Electrons are shared
Example of ionic bond
Sodium Chloride (NaCl)
Sodium has 1 extra electron in its outer shell, so it loses it and drops it down to a full outer shell at the next level
Chlorine has 7 shell electrons in its outer shell, it wants to gain another electron to make its outer shell 8 and complete
Sodium becomes + chlorine -
Example of ionic bond
Sodium Chloride (NaCl)
Sodium has 1 extra electron in its outer shell, so it loses it and drops it down to a full outer shell at the next level
Chlorine has 7 shell electrons in its outer shell, it wants to gain another electron to make its outer shell 8 and complete
Sodium becomes + chlorine -
Example of a covalent bond
Methane CH4
Nonpolar covalent bonds have_______sharing
Equal e.g. Co2
Polar covalent bonds have______ sharing
Unequal
Nonpolar vs. Polar examples
Nonpolar: CO2, methane
Polar: water, ammonia
Polar things like to group together, non polar things like to group together… Why does this cause issues?
Causes issues when it comes to things in the bloodstream
This is because polar molecules tend to form slight bonds between each other
What does hydrogen bonding do in H20?
It helps give water its surface tension, it also helps form grouping.
Polar vs nonpolar molecules in blood
Nonpolar molecules e.g., fats have to find themselves in a polar environment with water.
***hydrophobic
How to more non polar molecules inthe bloodstream
Carrier proteins
or
Fat soluble (sequester the non polar things away from the water)
Think of oil and vinegar salad dressing
Types of chemical reactions
Synthesis/combination
(anabolic)
endergonic (uses energy)
Decomposition (catabolic)
Exergonic (releases energy)
Exchange/displacement
(combined)
Example of synthesis (anabolic) reaction
Dehydration synthesis
Ex ample of decomposition (catabolic) reaction
Hydrolysis
Example of exchange/displacement reaction
Oxidation-reduction (electron-donor acceptor)
Synthesis (combination) reaction
A reaction in which two or more substances combine to form a new compound
Decomposition reaction
A reaction in which a single compound breaks down to form two or more simpler substances
Exchange (displacement) reaction
Bonds are both made and broken
Rate of reactions is affected by
Body temperature
Concentration
Reactant size
Catalysts (ex: enzymes)
Acids
Acids release H+
e.g., HCl (stomach acid), H2CO3 (found in bloodstream)
Bases
Bases absorb H+
e.g.,HCO3 , NH3 (ammonia)
pH scale
Measurement of H+
concentration in a solution (how acidic or basic a solution is)
Solutions with lower concentrations of hydrogen ions have ______ pHs and are considered _______
Higher, basic
Solutions with higher concentrations of hydrogen ions have ______ pHs and are considered _______
Lower, acidic
Solutions with higher concentrations of hydrogen ions have ______ pHs and are considered _______
Lower, acidic
Negative logarithmic scale
Negative = lower numbers = higher
concentration
Logarithmic = each unit =10-fold change
(pH 6 is 10X higher concentration than pH
7)
Arterial pH
7.35- 7.45
Denaturation
Changes in pH can cause
disruption in protein
structure by disrupting
hydrogen bonding
What happens W denaturation
Denature hydrogen bonding, so it can denature our proteins and render them nonfunctional. Causing our enzymes, hormones, etc to stop working.
Eventually will die if too basic or too acidic.
Buffers
prevent significant/rapid pH changes
a buffer will absorb the extra acid and neutralize it. if you do not have enough acid, that same compound can dissociate and form acid.
What serves as buffers intracellularly?
phosphates, hemoglobins, other proteins. resist pH changes inside the cells.
What serves as buffers extracellularly
HCO3, plasma
What server as a buffer for both Intra/extracellular
Amino acids
What server as a buffer for both Intra/extracellular
Amino acids
Carbohydrates function
Energy source (it’s all about those hydrogens) ***the hydrogen are used by the mitochondria to flow through ATP synthase enzyme and form ATP. All about getting the hydrogens off of the carbohydrates and moving them over to the mitochondria.
Cell-cell interactions, on surface of cell membrane
-Glycosylated (proteins with sugars attached) molecules on cell surfaces
-form signaling molecules that help signal to other cells
Structure of carbohydrates
C,H,O in a 1:2:1 ratio