Section 1
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VSEPR
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Last updated
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Date created
Mar 1, 2020
Cards (115)
Section 1
(50 cards)
VSEPR
Valance Electron Pair Repulsion model / Unshared electron pairs around the central atom
alpha decay
A nuclear reaction in which an atom emits a ________ particle consisting of two protons and two neutrons. This decreases the atomic number by 2 and the mass number by 4.
formula mass
the sum of the average atomic masses of all the atoms represented in the formula of any molecule, formula unit, or ion
core electrons
electrons in the inner shell
isotopes
same number of protons and electrons but different number of neutrons
Kinetic-Molecular Theory
a theory that explains that the behavior of physical systems depends on the combined actions of the molecules constituting the system
percentage composition
the percentage by mass of each element in a compound
reactants
a substance that takes part in and undergoes change during a reaction
mass number
number of neutrons and protons in nucleus
dipole-dipole attraction
attractive force resulting when polar molecules line up so that the positive and negative ends are close to each other
London dispersion forces
The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
standard pressure
1 atm or 101.3 kPa
products
The elements or compounds produced by a chemical reaction.
hybridization
Several atomic orbitals mix to form the same total number of equivalent hybrid orbitals
pi bond
when two p orbitals line up in parallel and electron clouds overlap. it exsits over a single bond.
ionic bond
Formed when one or more electrons are transferred from one atom to another
sigma bond
a bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Aufbau Principle
An electron occupies the lowest-energy orbital that can receive it
Charles's Law
V/T = k
atomic number
number of protons in nucleus
empirical formula
simplest whole # ration of atoms in a compound
binary compound
What ionic compounds are called when they are composed of only two different kinds of atoms.
Ideal Gas law
PV = n R T
metallic bond
a bond formed by the attraction between positively charged metal ions and the electrons around them
Pauli Exclusion Principle
An atomic orbital may describe at most two electrons, each with opposite spin direction
Dalton's Law of Partial Pressures
Total pressure of a gas is equal to the sum of the partial pressure of the component gases
beta decay
A nuclear reaction in which a neutron changes into a proton and into an electron, and the atoms emits a ______ particle, which is the electron. It increases the atomic number of the atom without changing the mass.
valence electrons
electrons in the outermost shell (can be easily shared, gained or lost)
atmospheric pressure
the pressure exerted by atoms and molecules in the atmosphere surrounding Earth, resulting from collisions of these particles with objects
electrostatic repulsion
Describes a force between particles with opposite electrical charges that causes them to push apart from one another
coefficient
A number in front of a chemical formula in an equation that indicates how many molecules or atoms of each reactant and product are involved in a reaction.
polyatomic ion
A covalently bonded group of atoms that has a positive or negative charge and acts as a unit
Combined Gas Law
P1V1/T1=P2V2/T2 (constant n)
lewis Structures
stable octet
the arrangement of eight electrons in the outermost shell of an atom
ionization energy
The amount of energy required to remove an electron from an atom
pascal
the SI unit of pressure equal to one newton per square meter
molecular mass
The sum of the masses of all the atoms in a molecule
transition elements
What are the elements in groups 3-12 called?
average atomic mass
weighted average of all of the isotope's mass numbers found in nature
net ionic equation
Includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution
covalent bond
A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Hund's Rule
electrons do not pair up until they have to
resonance structure
a structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
gamma radiation
electromagnetic radiation emitted during radioactive decay and having an extremely short wavelength
hydrogen bond
A relatively weak bond formed between any hydrogen atom (which is covalently bound to a nitrogen or oxygen atom) and a nitrogen or oxygen with an unshared electron pair
standard temperature
One atmosphere and 273 K.
Nobel Gas Notation
shortcut→ find the closest noble gas (column 18) with fewer electrons than the element then finish electron configuration
Boyle's Law
PV = k
electronegativity
A measure of the ability of an atom in a chemical compound to attract electrons
Section 2
(50 cards)
surface tension
An inward force that tends to minimize the surface area of a liquid; it causes the surface to behave as if it were a thin skin
hydrate
A compound that has a specific number of water molecules bound to its atoms
neutralization
A reaction of an acid with a base, yielding a solution that is not as acidic or basic as the starting solutions were.
enthalpy
The heat content of a system at constant pressure
pH
a numeric scale used to specify the acidity or basicity of an aqueous solution
Arrhenius Theory
acids are characterized by their sour taste, low Ph, and the fact that they turn litmus red. Bases are characterized by their bitter taste, slippery feel, high pH, and the fact that they turn litmus paper blue
factors affecting reaction rates
temperature, concentration ,particle size, and the use of a catalyst
activation energy
the minimum amount of energy required to start a chemical reaction
polarity
A lack of electrical symmetry in a molecule. Charge differences on opposite ends of a structure.
immiscible
Liquid solutes and solvents that are not soluble in each other
entropy
A quantitative measure of disorder or randomness, symbolized by S.
solubility product constant
an equilibrium constant applied to the solubility of electrolytes; it is equal to the product of the concentrations of the ions each raised to a power equal to the coefficient of the ion in the dissociation equation
boiling point
The temperature at which a liquid changes to a gas
Bronsted-Lowery Theory
Defines acids as proton donors and bases as proton acceptors; recognizes that acids and bases do not need to exist in aqueous (water) solutions; explains how acids and bases react to neutralize each other and produce water and salts when combined
Le Chatelier's Principle
States that if a stress is applied to a system at equilibrium, the system shifts in the direction that relieves the stress.
catalyst
a substance that initiates or accelerates a chemical reaction without itself being affected
exothermic
A chemical reaction that releases energy (heat)
buffer solution
A solution made from a weak acid and its conjugate base that neutralizes small amounts of acids or bases added to it
acid
A substance that increases the hydrogen ion concentration of a solution.
collision theory
atoms, ions, and molecules can react to form products when they collide, provided that the particles have enough kinetic energy
phase equilibrium
when the rates of evaporation and condensation equalize
base
A substance that decreases the hydrogen ion concentration in a solution.
alloy
A mixture of two or more metals
equilibrium constant
the ratio of product concentrations to reactant concentrations at equilibrium, with each concentration raised to a power equal to the number of moles of that substance in the balanced chemical equation
molarity
A common measure of solute concentration, referring to the number of moles of solute per liter of solution.
concentrated
Describes a solution that has a relatively large amount of dissolved solute
viscosity
A liquid's resistance to flowing
heat of vaporization
The amount of energy required for the liquid at its boiling point to become a gas
free energy
Measures the portion of a system's energy that can perform work when temperature and pressure are uniform throughout the system, as in a living cell.
saturated
unable to dissolve any more solute
equilibrium
A dynamic condition in which two opposing changes occur at equal rates in a closed system
acid ionization constant
the value of the equilibrium constant expression for the ionization of a weak acid
indicator
A compound that changes color in the presence of an acid or a base
end point
the point in a titration at which the indicator changes color
endothermic
A chemical reaction that absorbs energy (heat)
melting point
The temperature at which a solid becomes a liquid
crystal
An orderly, three-dimensional pattern of ions or atoms in a solid
colligative property
A property of a solution that depends on the number, not the identity, of the solute particles.
critical pressure
the lowest pressure at which the substance can exist as a liquid at the critical temperature
heat of fusion
Amount of energy required to change a substance from the solid phase to the liquid phase.
equivalence point
the point at which the two solutions used in a titration are present in chemically equivalent amounts
dilute
to lessen the concentration, force, or purity of by adding something
solute
A substance that is dissolved in a solution.
sublimation
A change directly from the solid to the gaseous state without becoming liquid
Gibbs free-energy equation
ΔG= ΔH(enthalpy)- TΔS(entropy)
conjugate base
particle that remains when an acid has donated a hydrogen ion
solvent
A liquid substance capable of dissolving other substances
conjugate acid
the particle formed when a base gains a hydrogen ion
critical temperature
the temperature above which the substance cannot exist in the liquid state
miscible
Describes two liquids that are soluble in each other
Section 3
(15 cards)