Chapter 2 PPT Flashcards
Matter
Anything that takes up space and has mass. Matter is composed of elements. Solids, liquids, and gases are matter.
Elements
Simplest types of matter with certain chemical properties. There are 98 naturally occurring elements.
Atoms
Smallest particles of an element that have properties of that element.
Bulk Elements
required by the body in large amounts (C, O, H, N, S, P)
Trace Elements
required by the body in small amounts (F e, I)
Ultratrace Elements
Required by the body in very minute amounts (As)
Atoms
Composed of subatomic particles
Proton
Carries a single positive charge
Neurton
Carries no electrical charge
Electron
Carries a single negative charge
nucleus
Central part of atom. Composed of protons and neutrons. Electrons move around the nucleus
Atom Characteristic
Smallest particle of an element that has the properties of that element
Electron Characteristic
Extremely small particle within an atom; almost no weight; carries a negative electrical charge and is in constant motion around an atomic nucleus
Proton Characteristic
Relatively large particle within an atom; carries a positive electrical charge and is found within an atomic nucleus
Neutron Characteristic
Relatively large particle within an atom; about the same weight as a proton; uncharged and thus electrically neutral; found within an atomic nucleus
Ion Characteristic
Particle, formed from an atom, that is electrically charged because it has gained or lost one or more electrons
Molecule Characteristic
Particle formed by the chemical union of two or more atoms
Atomic Number
Number of protons in the nucleus of an atom of a specific element. Each element has a unique atomic number.
Atomic Weight
Number of protons plus the number of neutrons in one atom. Electrons do not contribute to the weight of the atom because they are so light
Isotops
Atoms with the same atomic numbers but with different atomic weights. Contain different number of neutrons.
Radioactive Isotopes
Are unstable, releasing energy or atomic fragments (atomic radiation) until they gain stability, some are used to detect and treat disease
Radioactive Iodine-131
Can be used to destroy cancerous thyroid gland tissue. Only part of the body that transports and metabolizes iodine.
Radioactive Isotope Medical Uses
Detecting coronary blood vessel disorders, evalualting kidney function, measuring hormone concentration in body fluids and assessing changes in bone density.
Ionizing Radiation
Radiation (Alpha, Beta, Gamma) called this because energy can remove electrons from atoms, resulting in the formation of ions. The free electrons can damage nearby atoms.
Molecule
Particle formed when two or more atoms chemically combine
Compound
Particle formed when two or more atoms of different elements chemically combine
Molecular Formulas
Depict the elements present and the number of each atom present in the molecule
For atoms with atomic number 18 or less
the first shell can hold 2 electrons and the second and third shell can hold up to 8 electrons
Ion
An atom that gains or loses electrons to become stable. An electrically charged atom
Cation
A positively charged ion. Formed when an atom loses electrons
Anion
A negatively charged ion. Formed when an atom gains electrons
Ionic Bonds
Formed when electrons are transferred from one atom to another atom. Attraction between a cation and an anion forms a very strong bond between the ions, called an ionic bond
Covalent Bond
Strong chemical bonds, formed between atoms that share electrons.
Polar Molecules
Molecules with a slightly negative end and a slightly positive end. REsults from unequal sharing of electrons in covalent bonds. WAter is the most important one
Hydrogen Bond
A weak attraction ebtween a slightly positive H end of one polar molecule and a slightly negative (N or O) end of another polar molecule. Formed between adjacent water molecules. Important for protein and nucleic acid structure
Chemical Reactions occur
when chemical bonds form or break between atoms, ions, or molecules
Reactants are
the starting material of a chemical reaction: the atoms ions, or molecules
PRoducts are
substances formed at the end of the chemical reaction
Synthesis REaction
More complex chemical structure is formed
A + B –> AB
Decomposition Reaction
Chemical bonds are broken to form a simpler chemical structure
AB –> A + B
Exchange Reaction
Chemical bonds are broken and new bonds are formed
AB + CD –> AD + CB
Reversible REaction
The products can change back to the reactants
A + B AB
Electrolytes
Susbtances that release ions in water. The solution can conduct an electric current, so its called an electroylte
NaCl –> Na + Cl
Acids
Electroyltes that dissociate to release hydrogen ions in water
HCl –> Na + OH
Bases
Substances that relase ions that can combine with hydrogen ions
NaOH –> Na + OH
Salts
Electrolytes formed by the reaction between an acid and a base
HCl + NaOH –> H2O + NaCl
When an ionically bonded substance is put into water,
the charged ions are attracted to the slightly charged ends of the polar water molecules. Substance dissociates, and the ions become surrounded by water molecules.
The pH scale is used as shorthand for
H+ ion concentration, it is based on the number of decimal places in the concentration.
The higher the H+ concentration,
the lower the pH, and the higher the acidity
The lower the H+ concentration,
the higher the pH and the lower the acidity
pH Scale
indicates teh concentration of hydrogen ions in a solution
Neutral pH
A pH of 7 indicates equal concentrations of H+ and OH-. pH of water,
Acidic pH
A pH of <7 indicates a greater concentration H+ than OH-
Basic (Alkaline) pH
A pH >& indicates a higher concentration of OH- than H+
Normal range of blood pH?
7.35 - 7.45
Acidosis occures when
blood pH drops to 7.0-7.3
Person feels disoriented, fatigued. Caused by vomiting of alkaline intestinal contents
Alkalosis occurs when
blood pH rises to 7.5 - 7.8
Makes person feel dizzy and agitated. Caused by high altitude breathing
What mechanisms help regulate pH?
Homeeostatic
Buffers are
chemicals which act to resist pH changes, bind and release H+ ions to regulate pH
ORganic Molecules contain
C and H
Orgain Molecules can
dissolve in either water or organic liquids
Water-soluble organic compounds do not
release ions, and are non-electrolytes
Organic Molecules include
Carbohydrates, Proteins, Lipids, and Nucleic Acids
Inorganic Molecules generally do not
contain C and H
Inorganic molecules usually
dissolve inw ater and dissociate, forming ions and are electroytes
Inorganic molecules include
water, oxygen, CO2 and inorganic salts
Water has an important role in
transporting chemicals in the body
CO2 ; waste product released during
metabolic reactions
Inorganic salts help control
H2O concentration, pH, blood clotting, nerve and muscle processes
Carbohydrates are a main
source of cellular energy.
Supply materials to build cell structures
Carbohydrates solubility
Water-soluble
Carbohydrates contain
C, H, and O
Ratio of H to O for Carbohydrates
2:1
Size classification of carbohydrates
Monosaccharides(Single Sugars)
Disaccharides (Double Sugars)
Polysaccharides (Complex Carbohydrates)
Monosaccharides include
glucose and fructose
Disaccharides include
sucrose and lactose
Polysaccharides include
starch, glycogen, and cellulose
Lipid solubility
insoluble in water, but soluble in organic solvents
Lipids include
triglycerides (fats), phospholipids, steroids
Lipids important component of
cell membranes, and have several functions in cells
Most abundant lipids are
triglycerides (Fats)
TRiglycerides used for
Cellular energy
Contain more energy per gram than carbohydrates
Contain C, H , but less O than Carbs
Triglycerides consist of
1 molecule of glycerol and 3 fatty acids
Saturated Fatty Acids have
only single carbon-carbon bonds. Most are solid at room temperature, and of animal origin
Unsaturated fatty acids have
one or more carbon-carbon double bond. Most are liquid at room temperature, and are of plant origin
Phospholipids consist of
1 glycerol, 2 faty acids, and 1 phosphate
Phospholipids have
hydrophillic glycerol portion, and hydrophobic fatty acid ends
Phospholipids major component of
cell membranes
Steroids are
4 connected rings of carbon and widely distributed in the body, various functions
Steroids are a component of
cell membranes
steroids used to synthesize
adrenal and sex hormones
Main steroid in the body?
Cholesterol
Proteins are used as
structual materials, energy source, hormones, receptors, enzymes, and antibodies
Proteins consist of
building blocks called amino acids
Amino Acid contains
an amino group
carboxyl group
and a unique r (side chain) group
Amino acids are bound to each other by
peptide bonds
Peptide bonds form between
the amino group of one amino acid, and the carboxyl group of the adjacent amino acid
Primary Structure
Amio acid sequene
Secondary structure
Pleated or twisted structure form by hydrogen bonding between nonadjacent amino acids
Tertiary Structure
Unique 3D folded shape of the protein
Quaternary Structure
Structure formed by some proteins, when 2 or more polypepetide chains are conencted to become 1 protein
Nucleic cids can
carry genetic code (DNA) or aid in protein synthesis (RNA)
Nuclueic acids encode
amino acid sequences of proteins
Building blocks are called
nucleotides, which consist of a sugar (S), a phosphate group (P) and an organic base (B)
DNA structure
Double chain of nucleotides
RNA structure
single chain of nucleotides
DNA function?
Store the geneteic code
DNA contains
the sugar deoxyribose
DNA structure
Double helix
DNA composed of
nucleotides
RNA function?
interacts with DNA to conduct protein synthesis
RNA contains
the sugar ribose
RNA structure
single strand
RNA composed of
nucleotides
CT Imaging
Used to visualize internal antaomy. Used xray imitting decide to create 3D image
Differentiates tissuese with slightly different densities, tumors
PET Imaging
Uses radioactive isotopes that emit positrons (unusual positively charge electrons) to detect biochemical activity
PET used to
detect various brain disroders, blood flow, normal brain physiology
