Lesson 1 - Glossary Terms
precision
the ability of a measuring instrument to
give the same measurement repeatedly
accuracy
the closeness of a measurement to its
accepted value
chemistry
the study of the composition and
properties of substances and the changes they undergo
research
the investigation of new ideas or applying
ideas in new ways
analysis
can refer to the measurement of the physical
properties of a substance using an instrument
significant figures
all of the numbers
in a measurement that are known to be accurate, plus one digit that is an
estimate
Lesson 2 - Glossary Terms
density
the ratio of mass to volume for a
substance
unit multiplier
unit ratios used to convert a
substance from one unit to another
graphing
a technique used to represent data in a
visual manner
Lesson 3 - Glossary Terms
potential energy
stored energy or energy of
position
chemical potential energy
energy
stored in a chemical bond
kinetic energy
energy of motion
electromagnetic energy
form of energy
consisting of waves made up of oscillating electric and magnetic fields at right
angles to each other, also known as light energy
ultraviolet energy
form of electromagnetic
energy which comes from UV waves (waves with a shorter wavelength than that of
the visible electromagnetic spectrum)
infrared energy
form of electromagnetic energy
which comes from infrared waves (waves with a longer wavelength than that of the
visible electromagnetic spectrum)
Second Law of
Thermodynamics
states that energy can neither be created nor destroyed,
only converted into different forms
heat
the amount of energy in a system
temperature
a measure of the average kinetic
energy of a compound
photosynthesis
process in which green plants
use energy from the sun to produce glucose from carbon dioxide and water
fossil fuels
fuels consisting of compressed,
decomposed remains of ancient plants and animals; typically made of
hydrocarbons
greenhouse gas
a substance containing two or
more elements, which absorbs infrared energy inside the earth’s atmosphere and
radiates that energy back to earth
Kelvin Scale
SI temperature scale with a zero
point of absolute zero
absolute zero
theoretically lowest temperature
that can be reached, -273.15 degrees C or 0 K
matter
anything that has mass and volume
element
a substance that cannot be separated into
simpler substances by a chemical change; simplest type of pure substance
physical property
character of a substance
that can be observed without altering the identity of that substance
chemical property
characteristic of a
substance that cannot be observed without altering the identity of a
substance
reactivity
a chemical property that refers to how
quickly and easily a substance can undergo a chemical change
states of matter
the physical arrangement of
a substance (can be solid, liquid, gas, or plasma)
plasma
a high-energy state that is not composed of one
specific substance
solid
state in which matter holds a definitely shape and
volume
liquid
state in which matter does not hold a definite
shape but occupies a definite volume
gas
state in which matter has no definite shape or
volume
periodic law
states that the physical and
chemical properties of the elements are consequences of their atomic numbers
group
vertical column of the periodic table that
contains elements with similar electron configurations, also known as a
family
family
vertical column of the periodic table that
contains elements with similar electron configurations, also known as a
group
molecule
a group of two or more atoms, which are
chemically combined
compound
a substance that contains two or more
elements in fixed proportions
law of definite proportions
states
that molecules contain elements combined in specific ratios
Lesson 4 - Glossary Terms
anion
an atom that has taken on a negative charge
through gaining an electron
atom
smallest particle of an element that retains the
chemical identity of the element; made up of negatively charged electrons,
positively charged protons, and uncharged electrons
cation
an atom that has taken on a positive charge
through losing an electron
ion
an atom that has taken on a positive or negative
charge through the gain or loss of an electron
nucleus
concentrated core of an atom, which contains
protons and neutrons
proton
positively charged particle within the nucleus
of an atom, has a mass of 1.00720 amu
neutron
neutral particle within the nucleus of an
atom; has a mass of 1.00867 amu
electron
negatively charged particle within the atom;
has a mass at rest of 0.000555 amu
mass number
sum of the number of protons and
neutrons in the nucleus of a given atom
isotopes
atom that has the same number of protons as
another atom, but has a different number of neutrons
average atomic mass
weighted average of
the masses of the existing isotopes of an element
Lesson 5 - Glossary Terms
electric force
the force holds together two
oppositely charged species
ionic compound
a compound of positive and
negative ions combined such that the charges are neutralized; generally formed
from a metal and a nonmetal
covalent bond
a chemical bond resulting from the
sharing of electrons between two bonding atoms
macroscopic sample
a large bulk sample of a
given compound
mole
a quantity of a substance that has a mass in grams
numerically equal to its formula mass; 6.022 x 10^23 particles
Avogadro's number
number of representative
particles in one mole; equal to 6.022 x 10^23 particles
valance electrons
electrons in the outermost
energy level of an atom; for most atoms, it is available to be gained, lost, or
shared in the formation of chemical bonds
octet rule
the rule that states that atoms tend to
gain, lose, or share electrons so that each atom has a full outermost energy
level, which is typically 8 electrons
single bond
a covalent bond resulting from the
sharing of a pair of electrons between two atoms
double bond
a covalent bond resulting from the
sharing of a pair of electrons between two atoms
triple bond
a covalent bond resulting from the
sharing of three pairs of electrons between two atoms
Lesson 6 - Glossary Terms
covalent bond
a chemical bond resulting from
the sharing of electrons between two bonding atoms
nonpolar
description of a bond that has an even
distribution of charge due to an equal sharing of bonding electrons
polar
description of a bond that has an uneven
distribution of charge due to an unequal sharing of bonding electrons
electronegativity
property of an element
that indicates how strongly an atom of that element attracts electrons in a
chemical bond
ionic bond
a chemical bond resulting from the
transfer of electrons from one bonding atom to another
acid
a substance that increases the amount of hydrogen
ion concentration in a solution
base
a substance that increases the amount of hydroxide
ion concentration in a solution
neutralization reaction
a chemical
reaction between an acid and a base that destroys the distinctive properties of
both; produces a salt
salt
an ionic compound formed form the anion of an acid
and cation of a base; typically a crystalline compound with a high melting
point
Lesson 7 - Glossary Terms
chemical reaction
process in which one or
more substances are converted into new substances with different physical and
chemical properties
isotopic abundance
the amount of each
isotope of an element found in a natural sample
percent by mass
the relative mass of each
component within a compound
Law of Concentration of
Matter
states that matter is neither created nor destroyed, it just
changes form
diatomic molecule
molecules which, in their
natural form, exist as two atoms bonded together (i.e. oxygen and chlorine)
Lesson 8 - Glossary Terms
combination reaction
a reaction in which
two substances ( elements or compounds ) combine to form one compound
decomposition reaction
a chemical
reaction in which a single complex compound is broken down into two or more
products
combustion reaction
a reaction in which a
substance reacts with oxygen to form products that contain oxygen
single displacement reaction
a
reaction in which one element takes the place of another element as part of a
chemical compound
double displacement reaction
a
reaction in which the elements of the reactants break up and reform new
products
Lesson 9 - Glossary Terms
percent composition
refers to how much of
each element is in a compound as a percent by mass
empirical formula
the simplest possible
whole number ratio of moles of each elements in a compound
molecular formula
the actual molar ratio of
elements in a compound, as expressed by the subscripts in a formula
Lesson 10 - Glossary Terms
stoichiometry
(stoi-kee-ahm-uh-tree) the study
of quantitative relationships that can be derived from chemical formulas and
equations
limiting reactant
reactant that is
completely used up in a chemical reaction and that therefore determines the
maximum amount of product that can be formed
molar mass
also known as formula mass; mass in
grams of one mole of a substance
STP
standard temperature and pressure; designated as 0
degrees C/273 K and one atm
Lesson 11 - Glossary Terms
theoretical yield
the expected amount of
product of a chemical reaction given the known amount of reactants
actual yield
the measured amount of product of a
chemical reaction
percent yield
the ratio of actual yield to
theoretical yield (multiplied by 100 to give a percentage)
Lesson 12 - Glossary Terms
combustion
class of exothermic reactions in which a
substance combines with gaseous oxygen (O2) to produce an oxide
endothermic
describes a reaction that absorbs
heat
exothermic
describes a reaction that emits heat
heat
a measure of the total energy of a substance
joule
the SI unit of energy
thermochemistry
the study of changes in heat
in chemical reactions
enthalpy
the heat content of a specific amount of a
substance
standard enthalpy change
the change
in enthalpy in a reaction that takes place at 25 degrees C and 1 atm
pressure
calorimeter
a well-insulated container used to
measure temperature changes
calorimetry
the study of heat and heat
measurement
carbohydrates
a category of molecules that are
used as food, supplying 17 kJ/g (4 Cal/g) of energy
heat capacity
the amount of heat needed to raise
the temperature of an object a certain amount
specific heat
characteristic property of a
substance; the amount of heat necessary to raise the temperature of 1 gram of a
substance by 1 degree Celsius
temperature
a measure of the average kinetic
energy of a compound
Lesson 13 - Glossary Terms
amplitude
the distance from a wave's origin to its
peak
frequency
the number of times a wave cycles up and
down per unit of time
wavelength
the distance a wave travels during one
full cycle
electromagnetic wave
light waves;
composed of oscillating electric and magnetic waves that are perpendicular to
each other
speed of light
constant rate at which an
electromagnetic wave travels; 3.0 x 10^8 m/s
quantum
discrete bit of energy; smallest unit of
radiant energy that can be absorbed or emitted
photoelectric effect
a phenomenon in
which electrons are ejected from the surface of a metal when that metal is
exposed to light
photons
quantum of electromagnetic energy
quantum number
number assigned to each orbit of
an electron in an atom
ground state
the lowest energy level of electrons
in an atom
excited state
energy level attained by an
electron that absorbs additional energy and jumps from its normal level to a
higher energy level
Bohr Model
the model of an atom in which electrons
orbit the nucleus in quantized orbitals
Heisenberg Uncertainty
Principle
proposes that the momentum (mass x velocity) of a moving object
cannot be determined at the same time as its position
Lesson 14 - Glossary Terms
quantum-mechanical model
a model that
explains the properties of atoms by treating the electron as a wave and by
quantizing its energy
electron cloud
the graphical representation of
the probability of finding an electron around the nucleus of an atom
electron density
the concentration of
electrons in an electron cloud of an atom
atomic orbitals
a graphical representation of
the area inside which there is a 90% probability of finding an electron around
the nucleus
principal energy level
one of a limited
number of energy levels in an atom
principal quantum number
denotes the
principal energy levels of an atom; noted as n
sublevel
division of a principal energy level in an
atom
spin
direction in which an electron turns
Pauli Exclusion Principle
states
that each orbital can only hold two electrons and that the electrons have
opposite spins
electron configuration
outlines the
distribution of electrons among its orbitals
Aufbau Principle
states that electrons fill
the lowest energy level first and work their way up
Hund's Rule
states that electrons occupy
equal-energy orbitals such that the maximum number of electrons remain
unpaired
Lesson 15 - Glossary Terms
periodic trend
property of the elements that
can be predicted from the arrangement of the periodic table
period
horizontal row of elements in the periodic
table
group
vertical column of elements in the periodic
table
atomic radius
distance between the center of the
nucleus of an atom and its outermost electron
ionic radius
distance between the center of the
nucleus of an ion and its outermost electron
ionization energy
energy required to remove
one electron from an atom
successive ionization
energy
refers to the energy required to remove multiple electrons from an
atom (second ionization energy, third ionization energy, etc.)
electronegativity
property of an element
that indicates how strongly an atom of that element attracts electrons in a
chemical bond
polar
description of a bond that has an uneven
distribution of charge due to an unequal sharing of bonding electrons
alkali metals
the elements in group 1A of the
periodic table
malleability
the ability of a substance to be
molded into thin sheets without breaking
ductility
the ability of a substance to be stretched
into thin wire without breaking
electrical conductivity
the ability of
a substance to transfer electrical energy
alkaline earth metals
the elements in
group 2A of the periodic table
Lesson 16 - Glossary Terms
hypothesis
an educated guess about the results of
an experiment prior to conducting the experiment
independent variable
the item that will
be changed by the researcher in each trial of an experiment
dependent variable
the item that is
affected by the independent variable in an experiment
control
the standard against which you compare the
trails of an experiment
inner transition metal
the metals
located in the center block or "B" groups of the periodic table
corrosion
gradual wearing away of a metal through a
reaction at the surface of the metal with water, oxygen, and/or an acid
alloy
a solid solution of metals
Lesson 17 - Glossary Terms
periodic table
arrangement of the elements in
order of their atomic numbers so that the elements with similar electron
configurations are located in the same column
atomic number
number of protons in the nucleus
of an atom
atomic mass
weighted average of the masses of the
existing isotopes of an element
proton
positively charged particle within the
nucleus of an atom
neutron
neutral particle within the nucleus of an
atom
electron
negatively charged particle that orbits
the nucleus of an atom
metal
element that typically has a high melting point,
is ductile, malleable, shiny, and is a good conductor of heat and electricity;
found on the left side of the periodic table
nonmetal
an element that has a low melting point,
dull surface, breaks easily, is a poor conductor of heat and electricity, and
tends to gain electrons in a chemical reaction
lanthanide series
elements 58-71 of the
periodic table
actinide series
elements 89-102 of the
periodic table
rare earth metals
another name for the
actinide series; elements 89-102 of the periodic table
p-block elements
elements located to the
right of the inner transition metals of the periodic table
ozone
a rare form of elemental oxygen (O3); acts as a
shield in the atmosphere to protect the earth from harmful solar radiation
halogens
elements in group 7A of the periodic
table
noble gases
elements in group 8A of the periodic
table; well known because they are unreactive
Lesson 18 - Glossary Terms
elastic collision
a collision in which
neither party loses energy
inelastic collision
a collision in which
one or both party loses energy
velocity
distance divided by time
pressure
force per unit area
atmospheric pressure
pressure exerted by
the weight of the air in the atmosphere
barometer
instrument used to measure atmospheric
pressure
manometer
instrument used to measure the pressure
inside a closed container
Lesson 19 - Glossary Terms
Boyle's Law
gas law stating the relationship
between pressure and volume (P1V1 = P2V2)
Charles' Law
gas law stating the relationship
between temperature and volume (T1V2) = T2V1)
absolute zero
theoretically lowest
temperature that can be reached, -273.15 degrees C or 0 K
Avogadro's Law
gas law that states that equal
volumes of gas at an equal pressure contain an equal amount (number of
particles)
Dalton's Law of Partial
Pressures
each component gas of a mixture exerts pressure as if it were
in the container alone at the same temperature
The Combined Gas Law
describes the
relationship between temperature, pressure, and volume; P1V1/T1 = P2T2/V2
The Ideal Gas Law
gas law stating the
relationship among pressure, volume, temperature and amount for an ideal gas; PV
= nRT
ideal gas
theoretical gas described perfectly by
the kinetic-molecular theory of gases
kinetic-molecular theory
model that
explains the physical properties of gases based on the submicroscopic behavior
of gas particles; in mathematical form, it yields the ideal gas law
Lesson 20 - Glossary Terms
condensed states of matter
the
solid and liquid states; name refers to the fact that in the solid or liquid
phases, molecules of a substance are packed together much more tightly
metallic bond
a bond that occurs between two
metals; consequence of the attractive force between metallic elements that share
valence electrons
kinetic-molecular-theory_20
model
that explains the physical properties of gases based on the submicroscopic
behavior of gas particles; in mathematical form, it yields the ideal gas law
intermolecular forces
forces between
molecules
intramolecular forces
forces within a
molecule
induced dipole
dipole created by the presence
of a neighboring dipole
dipole
molecule in which the centers of positive and
negative charge are not the same
London dispersion
forces
intermolecular force that is the result of the attractive force
among induced dipoles
dipole-dipole forces
intermolecular force
that is the result of the attractive forces among molecules with permanent
dipoles
hydrogen bond
strong intermolecular force
between the hydrogen atom of one molecule and a highly electronegative atom of
another molecule, such has fluorine, oxygen, or nitrogen
viscosity
the friction among molecules of a liquid
as they move past each other
surface tension
a measure of the amount of
energy required to increase the surface area of a liquid by a specified
amount
Lesson 21 - Glossary Terms
crystalline solids
solids with particles
arranged in a repeated orderly manner
unit cell
the smallest component of a regular
repeating three-dimensional pattern of a solid
crystal lattice
term used to describe the
three-dimensional pattern of atoms or ions in a crystal
hydrated
term used to describe an ionic solid that is
dissolved in water
anhydrous
term used to describe an ionic solution
that is heated such that the water evaporates leaving behind the solid
amorphous solid
a substance that shares the
rigid property of a crystalline solid, but does not have the same regular
repeating molecular pattern of a crystalline solid
supercooled liquid
another name for
amorphous solids; this name is used because, at the molecular level amorphous
solids appear to be liquids that have such a low energy that their particles do
not slide past one another
metallic solid
solid that consists entirely of
metal atoms; intermolecular forces are metallic bonds
molecular solid
a solid that is held together
by any of the following intermolecular forces: London dispersion, dipole-dipole,
or hydrogen bonds
ionic solids
solid composed of ions that are
electrically attracted to each other
covalent network solid
solid held
together by covalent bonds throughout the compound (i.e. graphite and
diamond)
phase change
process of a substance changing from
one of the three states of matter to another
vaporization
the phase change from liquid to
gas
evaporation
vaporization at the surface of a
liquid
condensation
the phase change from the gaseous to
the liquid phase
liquid-vapor equilibrium
state in
which the rate of evaporation and condensation are equal
dynamic equilibrium
refers to the fact
that when a substance is in equilibrium, changes are still occurring at the
molecular level, but no net change in concentration occurs
equilibrium vapor pressure
the
pressure of the vapor above the liquid at liquid-vapor equilibrium
boiling point
the temperature at which the vapor
pressure of the liquid is equal to the atmospheric pressure
heat of vaporization
the energy required
to heat one mole of a specific substance in the liquid phase to one mole of that
substance in the gaseous phase at 1 atm of pressure
freezing point
the point where the liquid phase
of a substance is in equilibrium with the solid phase of a substance
sublimation
the process of a substance passing
directly from the solid phase to the gaseous phase
deposition
the process of a substance passing
directly from the gaseous phase to the solid phase
heating curve
a plot of temperature versus time
that can show the melting/freezing and vaporization/sublimation points
phase diagram
a graphical representation of
temperature and pressure for a substance; gives conditions necessary for
freezing/melting, vaporization/condensation, and sublimation/deposition
triple point
temperature and pressure at which a
substance is in equilibrium with the solid, liquid and gas phases
critical point
the temperature above which a
gas cannot be liquefied, regardless of the pressure
Lesson 22 - Glossary Terms
solution
a homogenous mixture of two substances at
the same phase
homogenous
property of a substance such that its
composition is the same throughout; in a solution refers to the fact that the
individual components cannot be distinguished from one another
heterogeneous
property of a substance such that
its composition is not uniform throughout
solute
the substance that is dissolved in a
solution
solvent
the substance that dissolves the solute in a
solution
soluble
property referring to the fact that a
substance can be dissolved in another substance
insoluble
property referring to the fact that a
substance cannot be dissolved in another substance
miscible
the ability of two liquids to be able to mix
together
immiscible
the inability of two liquids to mix
together
aqueous solution
a solution with water as the
solvent
electrolyte
substance that yields ions in
solution; named for its ability to conduct electricity
Lesson 23 - Glossary Terms
concentration
the amount of solute in a solution
with a given amount of solvent
dilution
the process by which the concentration of a
solution is reduced by adding more solvent
molarity
moles of solute per liter of solution
molality
moles of solute per kilogram of solvent
mole fraction
moles of component (either solute
or solution) over total number of moles of solution
saturation
the maximum amount of solute that can be
dissolved in a given amount of solvent
supersaturation
a solution that holds more
solute than can be dissolved in it
solvation
the process of dissolution at a molecular
level when water is the solvent; each solute particle is surrounded by water
solubility
the amount of solute that can be
dissolved in a give amount of solvent
Henry's Law
states that the solubility of a gas is
proportional to the partial pressure of the vapor above the liquid
Lesson 24 - Glossary Terms
nonvolatile
a substance that is not necessarily
prone to entering the gaseous phase easily
volatile
a substance that is prone to entering the
gaseous phase
boiling point elevation
an increase in
the vapor pressure of a solution as compared to that of the pure solvent
freezing point depression
the
ability of a dissolved solute to lower the freezing point of a pure solvent
osmosis
the flow of solvent particles from a solution
of lower concentration to a solution of high concentration
osmotic pressure
pressure required to prevent
osmosis; arises when there is a flow of solvent across a semipermeable
membrane
isotonic solution
a solution that has the
same osmotic pressure as another solution
hypotonic
a solution that has a lower osmotic
pressure than another solution
hypertonic
a solution that has a higher osmotic
pressure than another solution
concentration gradient
results when a
two solutions of differing concentrations are placed on either side of a
semipermeable membrane; solvent flows down a concentration gradient from a
solution with a high concentration (and a high osmotic pressure) to a solution
with a low concentration (low osmotic pressure)
Lesson 25 - Glossary Terms
equilibrium
refers to a general state in which the
forward is happening at the same rate as the reverse
static equilibrium
equilibrium state in
which all activity has ceased (as opposed to dynamic equilibrium in which
changes are occurring but no net change results because the forward is occurring
at the same rate as the reverse)
forward reaction
the reaction as read from
left to right
reverse reaction
the reaction as read from
right to left
chemical equilibrium
state in which the
forward reaction is happening at the same rate as the reverse
law of mass action
expresses the
product/reactant concentration ratio as an equilibrium constant
equilibrium constant
the ratio of product
to reactant concentration at equilibrium
law of chemical equilibrium
states
that every reversible reaction has a specific equilibrium constant that remains
the same regardless of starting concentrations
heterogeneous equilibrium
an
equilibrium in which one or more of the components is in a different physical
state
Lesson 26 - Glossary Terms
LeChatlier's Principle
states that if a
system at equilibrium is subjected to changes in conditions, the system will
shift in direction such that the change imposed is minimized
Haber Process
chemical process that utilizes Le
Chatelier's principle to produce ammonia commercially from nitrogen and hydrogen
gas
Lesson 27 - Glossary Terms
dissolution
process in which an ionic solid
dissolves in a polar liquid
precipitation
the process of solute leaving a
solution and becoming solid
solubility equilibrium
state in which
the rate of dissolution and precipitation are equal
solubility product
the equilibrium constant
for solubility equilibria
precipitation reaction
reaction in
which a precipitate is formed
Lesson 28 - Glossary Terms
Arrhenius acid/base
states that acids
produce hydrogen ions while bases produce hydroxide ions
Bronsted-Lowry acid/base
states that
acids are hydrogen ion donors and bases are hydrogen ion acceptors
dissociation
the process of an acid separating
into ions and water
monoprotic acid
dissociates into one proton
and its conjugate base
diprotic acid
dissociates into two protons and
two conjugate bases
triprotic acid
dissociates into three protons
and three conjugate bases
conjugate base
the resulting anion present when
an acid loses a proton
hydronium ion
ion formed by the addition of a
proton to a water molecule; accounts for the properties of acids
amphoteric
describes a substance that can act as
both an acid and a base
conjugate acid
the resulting compound present
when a base accepts a proton
acid dissociation
constant
quantitative measure of the strength of an acid; measures the
extent to which an acid dissociates
base dissociation
constant
quantitative measure of the strength of a base; measures the
extent to which a base dissociates
salt hydrolysis reaction
reaction in
which a salt forms a hydronium ion or hydroxide ion
Lesson 29 - Glossary Terms
self-ionization of water
the reaction
of water with itself to form a hydronium and hydroxide ion
ion-product constant of
water
the product of the concentration of hydroxide and hydronium ion
concentrations in water; always constant
pH scale
logarithmic scale that measures the
hydronium ion concentration of a solution
indicator
a chemical that changes color when it
picks up or loses protons; tells the acidity/basicity of a solution
pH meter
instrument that can detect the hydronium ion
concentration of a solution using an electrode
Lesson 30 - Glossary Terms
oxidation
the process by which a substance loses
electrons
reduction
the process by which a substance gains
electrons
redox reaction
a reaction in which oxidation
and reduction take place
oxidation number
the apparent charge assigned
to an atom based on the assumption of a complete transfer of electrons
oxidizing agent
a substance that results in
the oxidation of another compound; the oxidizing agent gets reduced
reducing agent
a substance that results in the
reduction of another compound; the reducing agent gets oxidized
direct combination reaction
a
chemical reaction in which two or more simple reactants join to form a single,
more complex product; also known as a synthesis reaction
synthesis reaction
a chemical reaction in
which two or more simple reactants join to form a single, more complex product;
also known as a direct combination reaction
decomposition reaction
chemical
reaction in which a single complex compound is broken down into two or more
products
single replacement
reaction
chemical reaction in which an uncombined element replaces an
element that is part of a compound
activity series
list of elements organized
according to the ease with which they undergo certain chemical reactions
Lesson 31 - Glossary Terms
organic chemistry
the study of compounds
containing carbon
allotropes
forms of the same element with different
bonding structure; carbon has different allotropes like charcoal, graphite, and
diamond
fossil fuels
fuels consisting of compressed,
decomposed remains of ancient plants and animals; typically made of
hydrocarbons
saturated hydrocarbon
hydrocarbon
containing only single bonds
unsaturated hydrocarbon
hydrocarbon
containing one or more double bond
alkenes
hydrocarbons with at least one double bond and
no triple bonds
alkynes
hydrocarbons with at least one triple bond
structural isomer
a compound that has the
same molecular formula of another compound, but its atoms are bonded in a
different way
parent chain
longest continuous chain of carbon
atoms in an organic molecule
monomer
small molecule that joins with other similar
molecules to make a polymer; repeating unit of a polymer
polymer
large organic molecule consisting of small
repeating units called monomers
Lesson 32 - Glossary Terms
halocarbon
organic molecule in which one or more of
the hydrogen atoms in a hydrocarbon is replaced with a halogen
alcohol
one or more hydrogen atoms of a hydrocarbon is
replaced with a hydroxyl group (-OH)
ether
a molecule in which an oxygen atom is bonded
between two carbon atoms (R-O-R)
aldehyde
hydrocarbon derivative in which a carbonyl
group is located on the end of a hydrocarbon chain (R-CHO)
ketone
hydrocarbon derivative in which a carbonyl group
is located within a hydrocarbon chain (R-COR')
carbonyl group
carbon atom double bonded to an
oxygen atom (-CO)
carboxyl group
combination of a carbonyl group
and a hydroxyl group (-COOH)
carboxylic acid
hydrocarbon derivative
containing a carboxyl group
ester
hydrocarbon derivative containing a carboxyl group
in which the hydrogen atom is replaced by a hydrocarbon group (R-COOR')
amine
hydrocarbon derivative in which an amino group is
attached to a hydrocarbon chain (R-NH2)
amide
hydrocarbon derivative containing an amino group
attached to the carbon atom of a carbonyl group (R-CONH-R')
Lesson 33 - Glossary Terms
biochemistry
study of the chemistry of living
organisms
biomolecules
molecules necessary to sustain
life
photosynthesis
the process by which plants
convert solar energy to chemical energy
cellular respiration
the chemical process
by which all organisms use glucose for energy
metabolism
collective term for all the chemical
reactions that occur in an organisms
carbohydrates
the class of biomolecules that
store energy
glucose
molecule that living organisms use for
energy
monosaccharide
monomer of a carbohydrate,
simple sugar
disaccharide
compound composed of two
monosaccharides; double sugar
polysaccharide
compound composed of several
monosaccharides; complex sugar
lipid
organic compound with oily or waxy properties;
includes fats, waxes, phospholipids, and steroids
hydrophobic
insoluble in water; "water
fearing"
triglyceride
ester of glycerol and three fatty
acids; general term for fats and oils
hydrogenation
process by which hydrogen atoms
are added across the double bonds of unsaturated fats, synthesizing a saturated
fat
essential fatty acids
fatty acids needed
to sustain life; can't be produced by the body
phospholipid
lipid made up of an alcohol, fatty
acids and a phosphate group
cholesterol
important biomolecule; precursor to
all sex hormones; member of steroid class
steroids
class of biologically important molecules
with characteristic ring structure; necessary to sustain life
protein
most diverse class of biomolecules; serve a
variety of functions including in muscles, hair, and as enzymes
enzyme
biological catalyst
catalyst
substance that increases the rate of a
reaction
amino acids
building blocks of proteins
primary structure of a
protein
sequence of amino acids in a protein
secondary structure of a
protein
describes how the chain of amino acids folds upon itself
tertiary structure of a
protein
describes how the entire protein molecule folds upon itself
quaternary structure of a
protein
describes how subunits of a protein join together
subunit
has its own primary, secondary, and tertiary
structure but joins with another subunit(s) to make a complete protein
denatruation
the process of the tertiary and/or
quaternary structure of a protein being altered by extraneous factors
substrate
substance on which an enzyme acts
nucleic acids
the molecular code for genetic
information that can be passed onto the next generation of an organism
nucleotide
monomer of a nucleic acid
