Chemical Level of Organization Flashcards
Chemistry
the science of the structure and interactions of matter
Matter
Anything that occupies space and has mass; exists in three states : SOLID, LIQUID, & GAS
Mass
The amount of matter in any object; does NOT change
Weight
The force of gravity acting on matter(change)
Chemical Symbols
Given to elements for abbreviation
Major Elements
Oxygen(O), Carbon(C), Hydrogen(H), Nitrogen(N) ; Makes up 96% of body weight
Lesser Elements
Makes up 36% of body weight
- Calcium(Ca) -Sodium(Na)
- Phosphorus(P) -Chlorine(Cl)
- Potassium(K) -Sulfur(S)
- Magnesium(Mg) -Iron(Fe)
Trace Elements
Only present in tiny amounts; Makes up 0.4% of body weight
Aluminum(Al) Boron(B) Iron(I) Chromium(Cr) Manganese(Mn) Cobalt(Co) Fluorine(F) Molybdenum(Mo) Copper(Cu)
Atoms
Smallest units of matter that retain properties and characteristics of the element. Smallest atoms are: Hydrogen atoms (diameter less than 0.1 nanometer)
Subatomic Particles
compose individual atoms, there are 3 types:
a. Protons - (+) charged protons within the nucleus
b. Neutrons - uncharged or neutral; located within the nucleus
c. Electrons - tiny (-) charged electrons
Atoms consist of a nucleus that contains
protons, neutrons, and electrons that move about the nucleus
Electron Shells
Specific groups of electrons that move about within certain regions around the nucleus; electrons revolve around the nucleus . Each shell holds a specific number of electrons:
First shell - 2 (max)
Second shell - 8 (max)
Third Shell - 18 (max)
The number of electrons in an atom of a neutral element ALWAYS = the number of protons
Atomic Number
The number of protons in the nucleus of an atom. Since all atoms are electrically neutral the atomic number = the number of electrons in each atom
Mass Number
the sum of an atoms protons and neutrons
Isotopes
atoms of an element that have different numbers of neutrons, but same number of protons, and therefore different mass numbers
-stable isotopes do not change their nuclear structure overtime
Radioactive Isotopes
unstable; their nuclei decay (spontaneously change) in order to form a more simpler and stabler configuration
- They can be used to study the structure and function of particular tissues
Half-life
the time required for half of the radioactive atoms in a sample of that isotope to decay into a more stable form
Dalton or Atomic Mass Unit (amu)
the standard for measuring the mass of atoms and their subatomic particles:
- neutron: 1.008 daltons
- proton: 1.007 daltons
- electron: 0.0005 daltons
Atomic Mass or Atomic Weight
the average mass of an elements naturally occurring isotopes; atomic mass is typically close to the mass of the most abundant isotope
Ion
an atom that either gives up or gains electrons; a particle with a (+) or (-) charge because of unequal numbers of protons and electrons
ex. Ca^2+
Molecule
when 2 or more atoms sharing electrons
ex. H2O or O2
Ionization
the process of giving up or going electrons
Compound
a substance that contains atoms of 2 or more different elements
ex. water (H2O) or sodium chloride (NaCl)
Free Radical
an atom or group of atoms with an unaired electron in the outermost shell
- having a unpaired electron makes the free radical unstable, highly reactive, and destructive to nearby molecules
- they become stable by either giving up an electron or taking one from another molecule
Clinical Connection: Free Radicals and Antioxidants
Disorders and diseases linked to oxygen-derived free radicals are: cancer, atherosclerosis, Alzheimer’s disease, Emphysema, diabetes mellitus, cataracts, macular degeneration, rheumatoid arthritis, and deterioration associated with aging
