Chemical Level of Organization Flashcards

1
Q

Chemistry

A

the science of the structure and interactions of matter

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2
Q

Matter

A

Anything that occupies space and has mass; exists in three states : SOLID, LIQUID, & GAS

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3
Q

Mass

A

The amount of matter in any object; does NOT change

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4
Q

Weight

A

The force of gravity acting on matter(change)

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5
Q

Chemical Symbols

A

Given to elements for abbreviation

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6
Q

Major Elements

A

Oxygen(O), Carbon(C), Hydrogen(H), Nitrogen(N) ; Makes up 96% of body weight

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7
Q

Lesser Elements

A

Makes up 36% of body weight

  • Calcium(Ca) -Sodium(Na)
  • Phosphorus(P) -Chlorine(Cl)
  • Potassium(K) -Sulfur(S)
  • Magnesium(Mg) -Iron(Fe)
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8
Q

Trace Elements

A

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)

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9
Q

Atoms

A

Smallest units of matter that retain properties and characteristics of the element. Smallest atoms are: Hydrogen atoms (diameter less than 0.1 nanometer)

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10
Q

Subatomic Particles

A

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

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11
Q

Atoms consist of a nucleus that contains

A

protons, neutrons, and electrons that move about the nucleus

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12
Q

Electron Shells

A

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

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13
Q

Atomic Number

A

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

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14
Q

Mass Number

A

the sum of an atoms protons and neutrons

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15
Q

Isotopes

A

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

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16
Q

Radioactive Isotopes

A

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

17
Q

Half-life

A

the time required for half of the radioactive atoms in a sample of that isotope to decay into a more stable form

18
Q

Dalton or Atomic Mass Unit (amu)

A

the standard for measuring the mass of atoms and their subatomic particles:

  • neutron: 1.008 daltons
  • proton: 1.007 daltons
  • electron: 0.0005 daltons
19
Q

Atomic Mass or Atomic Weight

A

the average mass of an elements naturally occurring isotopes; atomic mass is typically close to the mass of the most abundant isotope

20
Q

Ion

A

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+

21
Q

Molecule

A

when 2 or more atoms sharing electrons

ex. H2O or O2

22
Q

Ionization

A

the process of giving up or going electrons

23
Q

Compound

A

a substance that contains atoms of 2 or more different elements

ex. water (H2O) or sodium chloride (NaCl)

24
Q

Free Radical

A

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
25
Q

Clinical Connection: Free Radicals and Antioxidants

A

Disorders and diseases linked to oxygen-derived free radicals are: cancer, atherosclerosis, Alzheimerโ€™s disease, Emphysema, diabetes mellitus, cataracts, macular degeneration, rheumatoid arthritis, and deterioration associated with aging