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Definition
two or more atoms sharing electrons joined by a chemical bond
*can be two atoms of the same element
*can be atoms of different elements |
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Definition
Molecule that contains atoms of different elements
Examples: H2O, NaCl, CaCl2 |
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Definition
| A substance which cannot be split into smaller substances without losing its chemical properties |
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Definition
| The smallest unit of matter which retain the properties and characteristics of the element |
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Term
| Major elements in the body |
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Definition
Oxygen
Carbon
Nitrogen
Hydrogen |
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Definition
| bones, small amounts in blood, makse muscles contract, allows nerve communication, allows blood coagulation, releases some hormones |
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Definition
RNA, DNA
Main component of ATP (energy)
Found in bones and teeth |
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Definition
All protiens
Nucleic Acids (RNA, DNA) |
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Definition
Component of water
Ion that makes us acidic |
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Definition
Fats (good and bad)
Carbs, Protien
Forms backbone chains and rings of all organic molecules |
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Definition
Component of water
Used when metabolizing food into engery |
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Definition
Balance water in cells
Needed for nerve activity
Potasium: Inside cells
Sodium: Extracellular fluid |
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Definition
Ionized forms are part of:
Hemoglobin - oxygen carrying protein in red blood cells
Some enzymes |
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Definition
| Neede for many enzymes; aid in the increase rate of chemical reactions |
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Definition
Follows sodium around
Found in extracellular fluid
Maintains water balance |
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Definition
| Component of some vitamins and many protiens |
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Definition
Particles are tightly associated with each other
Definite shape and definite volume
Not very compressable |
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Term
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Definition
Indefinite shape, definite volume
Not very compressible |
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Term
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Definition
Widely spaced particles that fly around, and bang off eachother
Indefinite shape, indefinite volume
Very compressable |
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Term
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Definition
Energy cannot be created or destroyed,
the total energy of a closed system is constant |
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Term
Potential energy
vs
Kinetic energy |
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Definition
Potential energy is stored energy, and not yet able to do work.
Kinetic energy is the energy of movement. |
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Term
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Definition
Reaction that stores, and requires energy
*also refered to as an anabolic reaction |
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Term
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Definition
Reactions that release energy
*also refrred to as a catabolic reaction |
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Term
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Definition
Energy stored in chemical bonds
*reaction is also reffered to as endergonic |
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Term
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Definition
Energy released from chemical bonds, this energy can be turned into work
*reaction is also reffered to as exergonic |
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Definition
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Term
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Definition
the amount of energy it requires to raise one gram of substance 1*C
Specific heat of water = 1.000 |
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Term
| Specific Heat Calories Food Calories |
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Definition
| 1000 specific heat calories (cal) = 1 food calorie (Cal) *1 food calorie = 4.2 kJ |
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Definition
Oxygen
*Major element in body |
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Definition
Hydrogen
*Major element in body |
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Definition
Calcium
*Lesser element in body |
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Term
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Definition
Phosphorus
*Lesser element in body |
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Definition
Potassium
*Lesser element in body |
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Term
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Definition
Sulfur
*Lesser element in body |
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Definition
Clorine
*Lesser element in body |
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Definition
Magnesium
*Lesser element in body |
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Definition
Iron
*Lesser element in body |
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Definition
Aluminum
*Trace element in the body |
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Term
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Definition
Boron
*Trace element in the body |
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Term
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Definition
Chromium
*Trace element in the body |
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Term
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Definition
| Cobalt *Trace element in the body |
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Definition
Copper
*Trace element in the body |
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Definition
Flourine
*Trace element in the body |
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Definition
Iodine
*Trace element in the body |
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Definition
Manganese
*Trace element in the body |
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Definition
Molybdenum
*Trace element in the body |
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Term
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Definition
Selenium
*Trace element in the body |
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Term
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Definition
Silicon
*Trace element in the body |
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Term
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Definition
Tin
*Trace element in the body |
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Term
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Definition
Vanadium
*Trace element in the body |
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Term
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Definition
Zinc
*Trace element in the body |
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Term
| What defines a noble gas? |
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Definition
| Atoms that do not combine with other atoms, are not present in the human body |
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Term
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Definition
| Elements that share metal and non-metal properties |
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Term
| Where are metals located on the periodic table? |
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Definition
| Left 2/3 of the periodic table |
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Term
| Where are the non-metals located on the periodic table? |
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Definition
| Far right side of the periodic table |
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Term
| What are the three elementary particles that make up an atom? |
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Definition
Electrons
Neutrons
Protons |
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Term
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Definition
Smallest of the elementary particles
Negatively charged
Responisble for the atom's chemical properties (ability to bond, etc)
Surround the nucleus of the atom |
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Term
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Definition
Found in the nucleus
Positively charged
Cannot participate in chemical reactions
Break apart in nuclear fission
Mass = 1 dalton |
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Term
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Definition
Found in the nucleus
Have no charge
break apart in nuclear fission
Mass = 1 dalton |
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Term
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Definition
| Number of protons in an element |
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Term
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Definition
| Average sum of protons and neutrons |
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Term
| Atomic mass (atomic weight) |
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Definition
| Average mass of all naturally-occuring isotopes of an element |
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Term
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Definition
Can't touch the inner electron shells
The outer shell determines the chemical properties of the element
Shells like to be "full"
Inner shell holds 2 electons, the remaining shells hold 8 |
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Term
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Definition
| Atoms that vary in the number of neutrons |
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Term
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Definition
Hydrogen-2, hydrogen with an added neutron (making it one neutron, one proton, and one electron)
Represented as either D or 2H |
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Term
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Definition
Hydrogen-3, hydrogen with two added neutrons (making it two neutrons, one proton, and one electron)
Represented as 3H |
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Term
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Definition
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Term
| What is the correct order of energy wavelengs in the electromagnetic spectrum? |
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Definition
Gamma
X-Rays
UV light
Visible light
Infared
Radiowaves |
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Term
| How are wavelengths related to energy? |
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Definition
long wavelengths = low energy
short wavelengths = high energy |
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Term
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Definition
| Molecule that breaks into two charged atoms, can be either a cation or anion ion. |
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Term
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Definition
| Positive charge - excess protons |
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Term
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Definition
| Negative charge - excess electrons |
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Term
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Definition
Ions that are dissolved in the tissues and fluids of the body
They can and do conduct electricity
Examples: Na+, Cl- |
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Term
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Definition
A molecule with an unpaired electron
Extremely damaging to biological systems
Likely the cause of diseases such as cancer
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Term
| What are some examples of the free radical scavengers? |
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Definition
Lycopenes, omega-3 fatty acids, vitamins C and E
They reduce the amount of free radicals in cells and prevent disease |
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Term
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Definition
| combinations of ions that travel together, also reffered to as ionic compounds |
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Term
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Definition
| Generally the same as the number of electrons that will be taken to form anions (expressed as a negative number) or cations (expressed as a positive number). These electrons are taken from the outer shell, which is why it's referred to as the valence shell. |
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Term
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Definition
| when elements fill their shells by sharing electrons |
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Term
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Definition
| a bond that shares characteristics of a polar bond (a partial charge, one end has a + charge, and one end has a - charge) , as well as sharing electrons |
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Term
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Definition
Atoms hang out together because they have opposite charges
Do NOT share electrons
Example: Na+ and Cl-
NaCl
Typically formed by elements that are on opposite ends of the periodic table |
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Term
Hydrogen bonds
(strength and example in a biological system) |
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Definition
Weakest type of bond - partial charge
Broken down by water
Creates surface tension
Holding protien structures, and strands of DNA together |
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Term
Covalent bond
(strength and example in a biological system) |
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Definition
Covalent bonds are the strongest because the two molecules share electrons.
Single strands of DNA, RNA
Gases dissolved in blood O2, N2, CO2
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Term
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Definition
Steal/give electrons
Second strongest of the three bonds
Teeth and Bones |
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Term
Define surface tension:
What releases surface tension? |
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Definition
strong attraction between water molecules create hydrogen bonds, which then creates a dome
Surfactant (soap) relase the hydrogen bonds
*surfactants in lung prevent lungs from collapsing
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Term
| Solution, Solvent, Solute |
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Definition
In a solution, a substance called the solvent dissolved another substance called the solute.
More solvent than solute.
Solvent is almost always water. |
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