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Human Anatomy & Physiology I Assessment Test Objectives.
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Human Anatomy & Physiology IAssessment Test Objectives
1. Atoms,Molecules<organelles,cells,tissues, organs,systems,organisms: -
Describe the levels of organization in multicellular organisms starting with atoms
and ending with organisms.
2. The maintenance of dynamic steady in the internal environment "strive for
stability": Define the term homeostasis.
3. +/- feedback: The general mechanisms of nervous or hormonal regulation.
- feedback: Provides stable, long term control.
+ feedback: Reinforces original deviation and causes rapid and temporary
changes in a variable.: Describe, in general terms, how negative and positive
feedback mechanisms are
used by organisms to maintain homeostasis.
4. BASE UNITS
Meter (m) - Length
Gram (g) - Mass/Weight
Liter (l) - Volume
Degree Celsius (ºC) - Temperature
Second (s) - Time: State the basic units of the metric system for length, mass, time
and volume.
5. Prefix symbol Prefix name Prefix value Fraction or Multiple Power
k kilo one thousand 1000 103
M mega one million 1,000,000 106
G giga one billion 1,000,000,000 109: Identify the fraction or multiple associated
with each of the following prefixes: kilo, deci, centi, milli, micro, and nano.
6. d deci 1/10
0.1 10-1
c centi 1/100 0.01 10-2
m milli 1/1000 0.001 10-3
µ micro 1/1000,000 0.000,001 10-6
n nano 1/1000,000,000 0.000,000,001 10-9: Combine the prefixes above with a
metric unit and know the correct abbreviation of the combined prefix and unit.
7. Basic build block of nature --- composed of one type of atom.: Define the
term element
8. O: Oxygen
C: Carbon
H: Hydrogen
N: Nitrogen
Ca: Calcium
K: Potassium
Na: Sodium
, Human Anatomy & Physiology I
Assessment Test Objectives
Cl: Chlorine
Fe: Iron
P: Phosphorous: Identify the common chemical symbols for: oxygen, carbon,
hydrogen, nitrogen, calcium, potassium, sodium, chlorine, iron, and phosphorus.
9. CO2: Carbon dioxide
CO: Carbon monoxide
H20: Water
HCI: Hydrochloric acid
NaCI: Sodium chloride
C6H12O6: Glucose
NaHCO3: Sodium bicarbonate: Identify the chemical formulas for carbon dioxide,
carbon monoxide, water, hydrochloric acid, sodium chloride, glucose, and sodium
bicarbonate.
10. Basic unit of matter: Define the term atom.
11. Atoms consist of three basic particles: *protons, electrons,* and *neu-
trons*.: Describe the basic structure of an atom.
12. The nucleus (center) of the atom contains the protons (positively charged)
and the neutrons (no charge). The outermost regions of the atom are called
electron shells and contain the electrons (negatively charged).: Identify the
charge and the location in an atom of protons, neutrons and electrons.
13. Isotopes are atoms which have the same number of protons but different
numbers of neutrons: Define the term isotope.
14. Radioisotopes (half-life)
Fluorine-18 is used in nuclear imaging
Erbium-169 is used for relieving arthritis pain in synovial joints.
Iodine-123 is used for diagnosis in thyroid function: Recognize that isotopes are
used in diagnosis and treatment in medicine.
15. Molecule: The fundamental components of chemical compounds and are
the smallest part of a compound that can participate in a chemical reaction
Ion: An atom or molecule with a net electric charge due to the loss or gain
of one or more. electrons transferred from one atom to another, electrical
attraction
Chemical bonding: Hold the nucleus in place. No electrons, no bonding. Two
bare nuclei would never stick together. Chemical bonding happens because
electrons in atoms are looking for ways to lower their energy. They can do this
by transferring to orbitals of lower energy (ionic bonding) or by spreading out
or delocalizing (covalent bonding): Define the terms molecule and ion. Explain
the role of electrons in chemical bonding.
, Human Anatomy & Physiology I
Assessment Test Objectives
16. Covalent: Also called a molecular bond, is a chemical bond that involves
the sharing of electron pairs between atoms.
Oxygen (6) and Oxygen (6) want to make up their own (8) atoms, they both
don't have enough so they share to pretend they have enough. (4) O (2)(2) O
(4)
Ionic: When one atom gives up one or more electrons to another atom.
Sodium- Na (1) >> wants to give up the (1) atom to Cholride- Cl (7) who wants
to take it>> Cl is now (7+1). Na is now Na+ and Cl forms Cl-, together they
make NaCl to create table salt: Compare how covalent and ionic bonds hold atoms
together and how each type of bond is shown in a diagram.
17. A covalent bond containing Hydrogen has a slight positive charge, the
hydrogen will be attracted to any neighboring negative charges, such as the
slight negative charge on the more electronegative atom of a nearby polar
covalent bond breaking up the bond.
Although an individual hydrogen bonds are weak and easily broken, numer-
ous hydrogen bonds in combination can be very strong.
Ionic Bond such as NaCl you could simply add water. For example, NaCl is
table salt. If you add water, the sodium and chlorine ions will separate thereby
breaking the ionic compound into two pieces.: Discuss the relative strengths of
covalent and ionic bonds (how easily the bonds can be broken).
18. Polar bond: Electrons are shared but not equally, resulting in a bond in
which one atom has a slightly negative charge and the other a slightly positive
charge. Can be broken by water- salt, sugar (one is positively charged, one
negative)
Nonpolar: Electrons are shared equally
Non polar bonds cannot be broken by water- a rock, piece of grass, oils, fats
* The greater the electronegativity difference, the more ionic the bond is.
Bonds that are partly ionic are called polar covalent bonds. Nonpolar covalent
bonds, with equal sharing of the bond electrons, arise when the electronega-
tivities of the two atoms are equal.: Compare polar and nonpolar bonds. Compare
and contrast the characteristics of polar and nonpolar molecules.
19. Carbon dioxide: Non polar covalent
Water: Polar covalent
Hydrochloric acid: Polar covalent
Sodium chloride: Ionic
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