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129
Biology
Undergraduate 1
06/10/2008
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Term
The matter in all living things are made up of
 Definition
separate chemicals.
Term
These chemicals could be
 Definition
compounds or elements.
Term
The elements are the basic chemical units that cannot be broken down by
 Definition
chemical processes.
Term
There are 92
 Definition
naturally occurring elements
Term
How many elements does Life require?
 Definition
25 of these elements
Term
96.3% of human body is made up of
 Definition
oxygen, carbon, hydrogen and nitrogen.
Term
Other important elements include:
 Definition
Phosphorus Sulfur Sodium Chlorine Potassium Iron
Term
Means water generator
 Definition
Hydrogen (H)
Term
Much lighter than air
 Definition
Hydrogen (H)
Term
Hydrogen (H) is Used in
 Definition
Hydrogenating vegetable oils As rocket fuel along with oxygen
Term
Reacts explosively with water to make hydrogen gas
 Definition
Potassium (K)
Term
Potassium hydroxide is
 Definition
a corrosive basic compound known as lye (used as drain cleaner)
Term
Soap is made by
 Definition
mixing fats and oils with potassium hydroxide.
Term
Important in function of nerve cells
 Definition
Potassium (K)
Term
Potassium nitrate
 Definition
is saltpeter (gunpowder)
Term
What is the formula for Potassium Chloride
 Definition
KcL
Term
^(they inject people with this to make the heart stop working)^
 Definition
Potassium Chloride
Term
Light grey metal
 Definition
Calcium (Ca)
Term
80% of bones and teeth are
 Definition
calcium.
Term
Lime stone and chalk are compounds of
 Definition
calcium.
Term
Calcium hydroxide is used as..(&Give the formula)
 Definition
lime water. Ca(oH)2
Term
Cement has compounds of
 Definition
calcium.
Term
Common metal
 Definition
Iron (Fe)
Term
Mixed with carbon to make steel
 Definition
Iron (Fe)
Term
Rust is
 Definition
Iron Oxide.
Term
Important part of hemoglobin of the red blood cells
 Definition
Iron (Fe)
Term
A brown solid used as a disinfectant before surgery
 Definition
Iodine (I)
Term
Human thyroid gland needs __________ to secrete a hormone called thyroxin
 Definition
Iodine (I)
Term
Body obtains _________ from seafood and iodized salt.
 Definition
Iodine (I)
Term
Hydroiodic acid is a
 Definition
very strong acid.
Term
VN is the formula for
 Definition
Zinc
Term
Cu is the formula for
 Definition
Copper
Term
CO is the formula for
 Definition
Cobalt
Term
Elements contain one kind of
 Definition
atom.
Term
Compounds are made up of
 Definition
two or more kinds of atoms bonded to each other.
Term
Different combinations of atoms determine
 Definition
the unique properties of each compound.
Term
Atoms are the smallest unit of
 Definition
matter
Term
Atoms are made up of
 Definition
nucleus and electrons
Term
Nucleus is made up
 Definition
of protons & neutrons
Term
Electrons move at high speeds around the
 Definition
nucleus.
Term
__________ = Number of electrons = ________
 Definition
Number of protons = Number of electrons = atomic number
Term
__________ + number of neutrons = __________
 Definition
Number of protons + number of neutrons = atomic mass (weight)
Term
Atoms that have the same number of ___________ but differ in number of _______ are called isotopes
 Definition
protons and electrons; neutrons
Term
Give 2 examples of Isotopes:
 Definition
Carbon-12 & Carbon 14
Term
If the numbers of neutrons are much higher than the number of protons
 Definition
the nucleus becomes unstable.
Term
Unstable nucleus becomes
 Definition
radioactive.
Term
Carbon-14 is
 Definition
radioactive.
Term
Isotopes of the same element behave
 Definition
the same way chemically.
Term
This fact can be used for good (one can follow the chemicals in the body and find out where they end up).
 Definition
This fact can also be bad, because body incorporates radioactive element into the body that might cause cancer.
Term
During a nuclear reactor accident
 Definition
radioactive iodine entered the bodies of many people in Ukraine and caused cancer.
Term
Properties of elements depend on the number of
 Definition
electrons that occupy the outer-most area of the atom (called outer-most shell)
Term
Atoms react to form
 Definition
molecules.
Term
Atoms either
 Definition
lose, gain or share electrons.
Term
Ionic bond is between
 Definition
two ions.
Term
Ions are
 Definition
elements or substances that have either gained or lost electrons.
Term
Gain of electrons gives a substance a
 Definition
negative (-) charge.
Term
Loss of electrons gives a substance a
 Definition
positive (+) charge.
Term
In an ionic bond,
 Definition
one substance gives electrons to another substance.
Term
There is attraction between
 Definition
positive (+) & negative (-)
Term
Attractions between + & - bonds
 Definition
keeps molecule together (forming ionic bond)
Term
Sodium chloride (table salt) is an example of
 Definition
an ionic compound.
Term
Covalent compounds form when atoms
 Definition
share electrons.
Term
Each atom shares one to
 Definition
six electrons in its outer shell. During the sharing, electrons go around both atoms.
Term
For each bond, each element contributes
 Definition
one electron.
Term
Most of the compounds found in living organisms are____; they mostly contain
 Definition
covalent compounds.They mostly contain carbon.
Term
Carbon can form up to _________ with other carbons and other elements such as ________
 Definition
four covalent bonds ; (such as hydrogen, oxygen, nitrogen).
Term
Single Bond:
 Definition
Sharing of a single pair of electrons.
Term
Double bond:
 Definition
Sharing of two pairs of electrons.
Term
Give two examples of triple bonds
 Definition
Example: H: C ::: C:H (acetylene) Used in Welding Torches H: C ::: N (hydrogen cyanide)
Term
Compounds containing double or triple bonds are called_______; give an example
 Definition
unsaturated. Example: Olive oil
Term
In a non-polar covalent compound… ;Give an example
 Definition
electrons are shared equally between atoms. Example: CH 4 Methane
Term
In a polar covalent compound, ;Give an example
 Definition
electrons spend more time around one atom than the other. Example: Water (H2O)
Term
In water, electrons spend more time around
 Definition
oxygen than hydrogen.
Term
Oxygen becomes slightly ________ and hydrogen becomes slightly __________
 Definition
negative (-) ; positive (+).
Term
Slightly negative charge of one molecule is attracted to a
 Definition
slightly + charge of another molecule.
Term
This attraction is called a
 Definition
hydrogen bond
Term
Hydrogen bonds are
 Definition
weak bonds.
Term
Hydrogen bonding occurs in other biologically important compounds including:
 Definition
Proteins & Nucleic Acids (DNA and RNA)
Term
Cohesion is:
 Definition
The tendency of the water molecules to stick together.
Term
This cohesion allows what to form?
 Definition
water droplets
Term
Surface Tension is
 Definition
the resistance of the water molecules at the surface to be broken.
Term
Water can support _______ ______ on its surface such as _________
 Definition
small weight; an insect.
Term
Hydrogen bonding causes the water to have a
 Definition
Much higher than expected freezing temp, & a Higher than expected boiling temp.
Term
Water heats up slowly because
 Definition
hydrogen bonds must be broken.
Term
This causes the water to evaporate
 Definition
less quickly.
Term
Water also cools down
 Definition
slowly.
Term
So hydrogen bonding moderates
 Definition
temperature change in water.
Term
Ice floats on top of
 Definition
liquid water.
Term
Hydrogen bonding helps formation of
 Definition
ice crystals.
Term
Ice has fewer _______ than ________ ________ so it floats
 Definition
water molecules; liquid water
Term
Water freezes from the
 Definition
top down to the bottom
Term
Aquatic life can live underneath
 Definition
the ice.
Term
Water is the
 Definition
universal solvent
Term
Water dissolves many thing
 Definition
in itself.
Term
A solution is made up of
 Definition
solvent (liquid) and solute (solid).
Term
Major part is _______, minor part is the ______
 Definition
solvent; solute.
Term
A solute can be either a
 Definition
solid, liquid or gas.
Term
Water readily dissolves ______; Give an example
 Definition
other polar compounds. Example: Urea (Nacl) dissolves in water and excreted in urine.
Term
Acids have what kind of a taste?
 Definition
sour taste
Term
Acids are Corrosive at
 Definition
high concentrations.
Term
Give an example of an acid
 Definition
Example: Hydrochloric acid (HCl) (Vinegar)
Term
What kind of taste do bases have?
 Definition
Have a bitter taste
Term
Bases are corrosive at
 Definition
high concentrations.
Term
Give an example of a base
 Definition
(Halopenos)
Term
pH means
 Definition
Potential of hydrogen
Term
ph is a measure of
 Definition
acidity and basicity
Term
a pH of 7 is
 Definition
neuteral
Term
a pH of 1-6.9 is
 Definition
acidic
Term
a pH of 7.1-14 is
 Definition
basic.
Term
Strong acids have a
 Definition
low pH
Term
Strong bases have a
 Definition
high pH
Term
Stomach acid has a pH of
 Definition
1.
Term
Seawater has a pH of
 Definition
9.
Term
Buffers are substances that
 Definition
resist change in pH.
Term
pH of blood is buffered by
 Definition
Carbonic Acid (H2CO3).
Term
pH of blood is about
 Definition
7.4.
Term
How does Acid Rain form?
 Definition
Compounds of sulfur & nitrogen (part of air pollutants released into the air).
Term
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' The Chemical Basis of Life Title
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