Chapter 2 Flashcards
Matter
Anything that occupies space and has mass
Mass
Amount of matter
Weight
Force exerted upon matter by gravity
What is matter composed of
Elements that are composed of atoms
Atoms
The smallest part of the element which retains the properties of that particular element. Each element is composed of only one kind of element
Charges of atomic structures
Protons carry a positive charge, neutrons carry no charge, electrons carry a negative charge
What particles make up the nucleus
Protons and neutrons
Atomic number
Equal to the number of protons in the nucleus. Each element is defined by the number of protons it possesses.
Noncharged atom
Protons equals number of neutrons
What an atom becomes once it gains or loses an electron
An Ion thag always carries a charge
Mass of particles
Protons and neutrons have the same mass, electrons have very little mass
Mass number
Protons + number of neutrons in an atom
Atomic mass
Almost identical to the mass number, varying only slightly due to isotopes. It is the average mass of the element. Refers to the number of atoms of an element.
Isotopes
Naturally occurring variations of an element that has slightly different numbers of neutrons.
Use of isotopes in clinical settings
Treating cancer
Tracking hormone uptake
Sterilization of surgical materials
Which number is used on the periodic table over the other
Atomic mass is used instead of mass number for completely accurate measuring considering isotopes.
Mole
Atomic mass measured out in grams
Avogadros number
6.02 x 10^23
The number of atoms needed to make up a mole of a substance
Cation
Positive charge from losing an electron
Anion
Negative charge from gaining an electron
What form do atoms exist in in the body
Ionic bc they are dissolved in water
When are atoms happiest
With 8 electrons in their outer shell
The chemical behavior of an atoms is determined by
The electrons in its outermost shell
Ionic bond
Electrons are transferred
Easily dissolved in water
Covalent bond
Atoms share electrons
Sharing one pair is a single bond
Sharing two pairs is a double bond
Strongest of chemical bonds
Polar covalent bond
Electrons are shared by unequally
Helps make water the universal solvent
Hydrogen bond
Between hydrogen and either octagon, nitrogen, or fluorine
Often occur between molecules that are polar covalently bonded
Hydrogen is attracted to the negative side of the molecule and forms the week hydrogen bond
Solubility
Ability of one substance to dissolve in another
Dissociation
Breaking up of sonically bonded compounds into their ions, each becomes surrounded by water molecules
Electrolytes
The cations and anions that result from dissociation
Anabolic reaction
Two or more compounds join to form one
Anabolism
Catabolic or decomposition
Tearing down reactions
Synthesis dehydration
Synthesis reaction where water is a product
Decomposition hydrolysis
Adding water to break down
Example of a synthesis dehydration
Glucose + glucose -> maltose + H2O
Example of decomposition hydrolysis
Maltose + H2O -> glucose + glucose
Exchange reaction
Molecules change dance partners
Reversible reactions
When the rate of one reaction equals the rate of the second reaction, the reaction is at equilibrium.
Which way a reversible reaction goes depends on
The concentration of the reactants
High reactants goes right
Low reactants goes left
Reaction that helps carry co2 to lungs
CO2 + H2O <-> H+ + HCO3-
High hydrogen ions in the body
High acidity and low alkalinity
Energy
The capacity to do work
Potential energy
Stored energy not activity doing work
Kinetic energy
The energy of motion - doing the work
Chemical energy
Potential energy in the bonds of elements due to the attraction between electrons and protons
What reactions require energy and which release
The formation of chemical bonds requires energy
The breaking down of chemical bonds releases energy
Always takes a bit of energy to get the reaction started
Energy molecule of the body
Adenosine tripgosphad
When is more energy required with ATP
If energy is stored in product than reactant
Activation energy
Minimum energy required to start a chemical reaction
Catalysts
Increases the rate of reaction by decreasing the activation energy required for the reaction to occur
Factors affecting the rate of chemical reactions
Activation energy
Catalysts
Concentration of the reactants
Temperature
Exceptions to inorganic chemistry rule
Co, co2, H2O, HCO3-
Most important inorganic molecule
H2O
Required in the final step in the series of reactions used ti extract energy from food
O2
Metabolic waste product
Carbon dioxide
How much water is in the human body
50-60%
Plasma is 92% water
Properties of water
High specific heat - stabilizes body temperature
Protection (lubricant, cushion)
Participates in chemical reactions - many reactions take place in water (hydrolysis, dehydration)
Mixing medium
Solutions
Contains totally dissolved particles
Ex. Electrolytes in plasma
Suspension
Contain in dissolved particles that will settle out of the solution
Ex. RBC in plasma
Colloids
Contains indisposed particles that will not settle out of the solution
Ex. Proteins in blood plasma
Solvent
Dissolves solute
Solute
Dissolves in the solvent
Percentage method of concentration
Weight in grams of a substance/100 mls of solution
Osmole method of concentration
A mole of a substance/1 kg of H2O
Osmolality
Number of particles dissolved in one kilogram
Human body uses what measurement of concentration
Millismoles
300 in avg human body
Proton
H+ ion
An acid is a
Proton donor (released H+ into solution)
Strong acids almost completely dissociate in water
A base is a
Proton acceptor
Ex. NaOH, KOH (OH portion binds to hydrogen)
pH is the measure of
H+ in a solution
High H+ = low pH = high acidity
Alkaline solutions have
More OH than H in the solution
Salts
Have a cation other than H+ and an anion other than OH-
Mixing an acid and base makes
Salt and water
In water, salt..
Dissolves into Na+ and Cl-
Buffers
Solutions or compounds that keep pH balanced by resisting drastic change in pH.
Biological buffers
Bicarbonate
Phosphates
Proteins
Renal/respiration1-
Incorporate hydrogen or hydroxyl group into otwn makeup to keep out of the solution
Four classes of organic molecules
Carbohydrates
Lipids
Proteins
Nucleic acids
Carbohydrates
Composed of carbon, hydrogen, and oxygen in ring formations
Building block of a car
Five or six carbon ring sugar. C6H12O6
Monosaccharide
One sugar ring. Building block of carbs.
Six and five rung sugar examples
Glucose, fructose and galactose
5 ring- atp dna and rna
Disaccharides
Two sugar rings hooked together, joined by synthesis dehydration. Ex- sucrose, lactose
Polysaccharides
Multiple sugar rings hooked together. Storage form for glucose.
Complex carbs benefit his
Break down slower to provide a more sustained release of energy
Glycogen
Animal glucose storage form
Starch and cellulose
Glucose storage used by plants
Lipids
Also composed of CHO but may also contain phosphorus and nitrogen.
Cannot be dissolved in water but can in acetone or alcohol
Subtypes of lipids
Fats
Phospholipids
Eicosanoids
Steroids
Fat soluble vitamins
Fats
Ingested from food or energy.
Triglyceride
Majority of fats. Fatty acid chains attached to glycerol molecule
Triglyceride
Majority of fats. Fatty acid chains attached to glycerol molecule
Saturated fats
Only single bonds with a more rigid structure
Unsaturated fats
One or more double binds in carbon chain that results in more relaxed structure
Trans fats
Unsaturated fats that have been artificially altered to be more saturated
Phospholipids
Fatty acid chains with a phosphate groups at one end. Results in one hydrophilic head and. Hydrophobic tail. Seen in the cell membrane.
Eicosanoids
Prostaglandins, leukotruenes, thromboxines.
Have many regulatory functions- like blood clotting, reproduction, hormone secretion
Fat soluble vitamins
Non polar molecules stored in the liver and perform vital functions. A, E, D, K
Steroids
Cholesterol and its derivatives.
Structure of four carbon rings.
Function as a component of the cell membrane and physiological regulation
Building blocks of protein
Amino acids
Peptide bond
Bind between amino acids
How many amino acids are there
20
Nonessential are those we can make
Essential are those that come from our diet
Types of proteins
Dipeptide - 2 acids
Tripeptide- 3 acids
Polypeptide - multiple acids
Types of proteins
Dipeptide - 2 acids
Tripeptide- 3 acids
Polypeptide - multiple acids
Primary structure of protein
Sequence of amino acids
Primary structure of protein
Sequence of amino acids
Secondary structure of proteins
Primary structure coils into alpha helix or pleated sheet with hydrogen bonds
Tertiary structure
Folding inward if secondary structure, spontaneous, requires no energy. Structure determines the shape of a domain in the protein, where the functions occur.
Desaturation
When hydrogen bonds in protein break and cause protein to fall apart
Quaternary structure
When two or more proteins associate to form a functional unit.
Like the hemoglobin molecule
Quaternary structure
When two or more proteins associate to form a functional unit.
Like the hemoglobin molecule
Enzymes
Lower activation energy and increase rate of reaction.
Active site
Where reactants (substrates) attach to an enzyme
Lock and key method
Things fit
Induced fit model
Compound binds to enzyme and changes shape
Cofactor
A no protein portion that might activate an enzyme
Building block of a nucleic acid
Nucleotide, composed of sugar, a nitrogenous base, and a phosphorous groups
DNA nitrogenous bases
Adenine, thymine, guanine, and cytosine in a double helix
RNA nitrogenous bases
Adenine, uracil, guanine, and cytosine in a single strand
Structure of dna
Double stranded model where bases pair in the middle through a hydrogen bonds
Long long chain of dna in nucleus
Chromatin
ATP is
A nucleotide with adenosine as a phosphate base, attached to a ribose sugar, and with three phosphate groups
