Section 1
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electrong
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Cards (140)
Section 1
(50 cards)
electrong
one of the parts of an atom having a negative charge. Indivisible particle with a charge of -1
energy
ability to do work
electrolysis
changing the chemical structure of a compound using electrical energy
effusion
movement of gas molecules through a small opening
cathode
electrode where electrons have gained (reduction) in redox reactions
buffer solutions
solutions that resist change in their pH, even when small amounts of acid or base are added
equilibrium
when the reactants and products are in a constant ratio. The forward reaction and the reverse reactions occur at the same rate when a system is in this state
base
substance which gives off hydroxide ions (OH-) in solution
charge
describes an object's ability to repel or attract other objects. Protons have a positive ...while electrons have a negative... Like ...repel each other, while opposites attract.
electromagnetic spectrum
complete range of wavelengths which light can have. These include infrared, ultraviolet and all other types of radiation as well as visible light
endothermic
process that absorbs heat from its surroundings as the reaction proceeds
atom
the smallest object that retains properties of an element. Composed of electrons and a nucleus (containing protons and neutrons)
cations
ion with positive charge
conjugate acid
a substance which can lose H+ ion to form a base
acid
compound that gives off H+ ions in solution
equilibrium constant
value that expresses how far the reaction proceeds before reaching equilibrium. A small number means that equilibrium is towards the reactants side while a large number means that the equilibrium is towards the product side
compound
two or more atoms joined together chemically, with covalent or ionic bonds
equilibrium expression
the expression giving the ratio between the products and reactants. It is equal to the concentration of each product raised to its coefficient in a balanced chemical equation and multiplied together, divided by the concentration of the product of reactants to the power of their coefficients
catalyst
substances that speed up a chemical process without actually changing the products of reactions
covalent bonds
when two atoms share at least one pair of electrons
conjugate base
a substance which can gain H+ ion to form an acid
chemical changes
processes or events that have altered the fundamental structure of something
electrodes
device that moves electrons into or out of a solution by conduction
entropy
measure of the disorder of a system
dipole-dipole forces
intermolecular forces that exist between polar molecules. Active only when the molecules are close together. The strengths of intermolecular attractions increase when polarity increases
acidic
describes a solution with a high concentration of H+ ions
central atom
in a Lewis structure, usually the atom that is the least electronegative
anion
ions with a negative charge
enthalpy
change in heat at constant pressure
element
substance consisting of only one type of atom
combustion
when substances combine with oxygen and release energy
atmospheres
common units for measuring pressure
Avogadro's number
number representing the number of molecules in (1) mole: 6.022 * 10 to the 23 power
concentration
the amount of a substance in a specified space
electronegativity
measure of a substance's ability to attract electrons
basic
having the characteristics of a base
atomic number
number of protons in an element
dissociation
breaking down of a compound into its components to form ions from an ionic substance
Bohr's atom
He made significant contributions to the atom. He understood the line spectra--the reason why only certain wavelengths are emitted when atoms jump down levels
dispersion forces (London dispersion forces)
dispersion is an intermolecular attraction force that exists between all molecules. These forces are the result of the movement of electrons which cause slight polar moments. Generally very weak, when their molecular mass increases, so does their strength
electrostatic forces
forces between charged objects
electrochemical cell
gives an electric current with a steady voltage as a result of an electron transfer reaction
equivalence point
occurs when the moles of acid equal the moles of base in a solution
empirical formula
formula showing the simplest ratio of elements in a compound
decay
change of an element into a different element, usually with some other particle(s) of energy emitted
colligative properties
properties of a solution that depend only on the number of particles dissolved in it, not the properties of the particles themselves. The main ones are boiling point elevation and freezing point depression.
anode
the electrode where electrons are lost (oxidized) in redox reactions
density
mass per unit volume of a substance
chemical equation
an expression of a fundamental change in the chemical substance
double bond
when an atom is bonded to another atom by two sets of electron pairs
Section 2
(50 cards)
hydrogen bonding
strong type of intermolecular dipole-dipole attraction. Occurs between hydrogen and F, O or N
mass number
the number of protons and neutrons in an atom
isotopes
elements with the same number of protons but have different numbers of neutrons, and thus different masses
mole fraction
the number of moles of a particular substance expressed as a fraction of the total number of moles
ionic bond
when two oppositely charged atoms share at least one pair of electrons but the electrons spend more time near one of the atoms than the other
parent isotopes
an element that undergoes nuclear decay
Planck
He contributed to the understanding of the
Planck
What is h?
intermolecular forces
forces between molecules
orbitals
an energy state in the atomic model which describes where an element will likely be
frequency
number of events in a given unit of time. When describing a moving wave, means the number of peaks which would pass a stationary point in a given amount of time
octet
In Lewis structures, the goal is to make almost all atoms have this structure. This means they will have access to (8) electrons regularly, even if they do have to share some of them
Graham's law
the rate of diffusion of a gas is inversely proportional to the square root of its molar mass
Le Chatlier's Principle
states that a system at equilibrium will oppose any change in the equilibrium conditions
half life
the amount of time it takes for half an initial amount to disintegrate
oxidation-reduction-reaction
a reactions involving the transfer of electrons
physical property
a property that can be measured without changing the chemical composition of a substance
molecular formula
shows the number of atoms of each element present in a molecule
percent composition
expresses the mass ratio between different elements in a compound
ionization energy
energy required to remove an electron from a specific atom
Gibb's free energy
the energy of a system that is available to do work at a constant temperature and pressure
exothermic
process that gives off heat to the environment
periodic table
grouping of the known elements by their number of protons. There are many other trends such as size of elements and electronegativity that are easily expressed in terms of the periodic table
mole
a collection of 6.022 * 10 to the 23 power number of objects. Usually used to mean molecules
molecular mass
the combined mass (as given on the periodic table) of all the elements in a compound
Kelvin
The SI unit of temperature. It is temperature in degrees Celsius plus 273.15
kinetic energy
energy an object has because of its mass and velocity. Objects that are not moving do not have this.
hydrolysis
the reactions of cations with water to produce a weak base or of anions to produce a weak acid
partial pressure
the pressure exerted by a certain gas in a mixture
mixture
composed of two or more substances, but each keeps its original properties
nm
abbreviation for nanometers. A nanometer is equal to 10 to the -9 power meters
molality
the number of moles of solute (the material dissolved) per kilogram of solvent (what the solute is dissolved in)
ideal gas law
ion
removing or adding electrons to an atom creates an ... (a charged object very similar to an attom)
photon
massless packet of energy, which behaves like both a wave and a particle
Lewis structures
a way of representing molecular structures based on valence electrons
oxidation number
a number assigned to each atom to help keep track of the electrons during a redox-reaction
molecule
two or more atoms chemically combined
particle
small portion of matter
molar
a term expressing molarity, the number of moles of solute per liters of solution
limiting reagent
the reactant that will be exhausted first
nucleus
the central part of an atom that contains the protons and neutrons. Plural=nuclei
pH
measures the acidity of a solution. It is the negative log of the concentration of the hydrogen ions in a substance
neutral
an object that does not have a positive or negative charge
intramolecular forces
forces within molecules. Forces caused by the attraction and repulsion of charged particles
molarity
the number of moles of solute (the material dissolved) per liter of solution. used to express the concentration of a solution
Geiger counter
instrument that measures radiation output
Heisenberg uncertainty principle
the principle states that it is not possible to know a particle's location and momentum precisely at any time
neutron
a particle found in the nucleus of an atom. It is almost identical in mass to a proton, but carries no electrical charge
molecular geometry (VSEPR)
shape of a molecule, based on the relative position of the atoms
Section 3
(40 cards)