Gen Chem Review Vocab

solid

defined shape + volume, not compressible; atoms are relatively immobile

liquid

definite volume, indefinite shape, not compressible; atoms have greater degree of motion than solids

gas

indefinite shape + volume, easily compressible; assume the shape and volume of the container they occupy; atoms are relatively far from each other

temperature

a measure of the kinetic energy of motion of the particles of a substance

Dalton's Atomic Theory

1. elements are composed of atoms. 2) atoms of same element are identical, but differ from other elements. 3) elements can mix together 4) atoms only change when mixed with other elements

1 mole of any element

6.02 x 10^23 atoms

molar mass

the mass of one mole of a pure substance

binary ionic compounds (w/o transition metal)

metal, nonmetal-ide

binary ionic compound (w/ transition metal)

metal (charge) nonmetal-ide

binary compound (w/ polyatomic ions)

metalpolyatomic ion or metal(charge) polyatomic ion

Ionic compounds w/ waters of hydration

ionic compound prefix-hydrate

Binary covalent compound

prefix-first element prefix-second element-ide

Binary Acid Naming Rules

hydro-anion-ic acid

oxoacids

polyatomic ion-ous acid or polyatomic ion-ic acid

linear alkane

prefix-ane

alkali metals

elements found in group 1a of the periodic table that are reactive metals with a tendency to form +1 cations

alkaline earth metals

elements found in group 2a of the periodic table that are reactive metals with a tendency to form +2 cations

anhydrous

an ionic compound that has had its waters of hydration removed

binary acid

a type of molecule in which hydrogen is bound to a second nonmetallic element; the molecule dissociates when dissolved in water

diatomic molecule

a molecule consisting of two atoms

metals

elements that are often characterized by their high thermal and electrical conductivity, and high ductility and malleability

nonmetals

elements that are often characterized by their low thermal and electrical conductivity, and low ductility and malleability

organic compounds

a compound that contains carbon and hydrogen

oxoacid

a molecule in which hydrogen is bound to an oxygen-containing anion that dissociates when dissolved in water

polyatomic ion

an ion in which two or more atoms are held together through covalent bonding, but with an overall charge

transmutation reactions

reactions in which elements are transformed into different elements

waters of hydration

water molecules that are bound in definite quantities within the crystalline structure of ionic compounds

Rydberg Equation

gives the frequencies of all photoemission lines of the hydrogen atom

quanta

a discrete, small packet of energy proportional to its frequency of the electromagnetic radiation

wavefunction

mathematical representation of a quantum particle (like an electron) in Schrödinger's equation

the square of the wavefunction

determines the probability of finding an electron within a certain region of space

principal quantum number (n)

quantizes the energy of an electron in the hydrogen atom

orbital angular momentum quantum number (l)

quantizes the angular momentum of an electron and produces s, p, d, and f orbitals

magnetic quantum number (m sub l)

spatially quantizes an orbital in certain orientations and determines how many s, p, d, and f orbitals exist

spin quantum number (m sub s)

describes the intrinsic magnetic field orientations of an electron (spin up or spin down)

spdf notation

used to construct electron configurations for the elements using Aufbau principle, Pauli exclusion principle, and Hund's rule

Aufbau principle

electrons are filled into lowest energy orbitals first

Pauli exclusion principle

the electrons within one atom must have a completely unique set of quantum numbers

Hund's rule

electrons are filled into orbitals such that the total spin of the atom is maximized

valence electrons

outer electrons that participate in chemical bonding

core electrons

electrons closest to the nucleus that do not participate in chemical bonding

atomic size trend

increases from top to bottom within a group and decreases from left to right across a period

ionization energy

the amount of energy required to remove an electron bound to an atomic nucleus in the gas phase

ionization energy trend

decreases from top to bottom in a group; increases from left to right in a period

electron affinity

the energy change associated with attaching an electron to an atomic nucleus in the gas phase

metallic character (of an atom)

defined by its ability (or tendency) to readily lose an electron

angular node

a node in an angular wave function that results in planar regions within atomic orbitals at which the probability density is zero

angular wave function

a wave function that depends only on polar and azimuthal angles around an atomic nucleus

atomic orbital

the space around a nucleus that has a high probability density as a result of certain combinations of quantum numbers

blackbody

an idealized body capable of absorbing and emitting radiation of all frequencies

blackbody radiation

the light emitted from an idealized body in which the distribution of wavelengths emitted is solely a result of its temperature

blackbody spectrum

range of wavelengths and frequencies of electromagnetic radiation emitted by a blackbody

Bohr frequency condition

equation derived from the Bohr model of the atom to explain the absorption and emission lines observed from atomic hydrogen

Bohr radius

the most probable distance between an electron and the nucleus of a hydrogen atom; a constant with a value of 5.29 × 10^-11 m

complementarity

the concept that quantum particles have certain sets of properties that cannot all be measured simultaneously

condensed electron configuration

a shorthand spdf notation in which a noble gas electron configuration is used in place of spdf-notated electrons

constructive interference

the net effect of the interaction between two or more waves, resulting in an increase in the amplitude

degeneracy

equivalent in energy

destructive interference

the net effect of the interaction between two or more waves, resulting in a decrease in the amplitude

diffraction

the spreading out of a wave once it passes through a narrow slit

electromagnetic radiation

an oscillating electric and magnetic field consisting of broad regions called radio waves, microwaves, infrared (IR), visible, UV rays, X-rays, and gamma rays

excited state

an electron configuration of an atom that is higher in energy than the ground state

frequency

the rate at which crests (or troughs) of a wave pass through a point

gamma rays

the highest frequency on the electromagnetic spectrum

ground state

an electron configuration of an atom that is of the lowest possible energy

hamiltonian operator

a mathematical function that, when applied to a wave function, returns the total energy of a system

Heisenberg's uncertainty principle

a tenet of quantum mechanics that states it is impossible to simultaneously know both the momentum and position of a particle with absolute certainty

incandescence

the emission of electromagnetic radiation as a result of an object being heated

infrared (IR)

third lowest frequency on the electromagnetic spectrum after microwaves

isoelectronic

having the same number of electrons and having the same electron configuration

magnetic quantum number (ml)

an integer associated with the orientation of a wave function

microwaves

the second lowest frequency on the electromagnetic spectrum, just above radio waves

nodes

the points on a standing wave that have zero amplitude

paramagnetic

a property in which an atom (or molecule) is attracted to a magnetic field as a result of having unpaired electrons

photoelectric effect

the phenomenon in which electromagnetic radiation is able to eject electrons from the surface of an object

photoemission spectrum

the light emitted from excited atoms at characteristics wavelengths

photon

a particle representing one quantum of electromagnetic radiation

Planck's constant (h)

a fundamental physical constant with a value of 6.626 x 10^-34 J•s

probability density

a quantitative measure of the likelihood of finding an electron in 3D space around an atomic nucleus

quantum numbers

a set of numbers predicted by Schrödinger's equation related to quantized properties of an electron

radial node

a node in a radial wave function that results in spherical regions within atomic orbitals for which the probability density is zero

radial probability density

the probability density for an electron to be at a point located the distance r from the nucleus

radial wave function (R)

a wavefunction that depends only on the distance from the atomic nucleus

radio waves

the lowest frequency on the electromagnetic spectrum

Schrödinger's equation

an equation that describes the wave motion of particles

shell

the name given to all electrons that possess the same principal quantum number

speed of light in a vacuum

the speed at which electromagnetic radiation travels through a vacuum; equal to 2.998 x 10^8 m/s

spin

intrinsic magnetic moment possessed by an electron (or other subatomic particle)

subshell

a grouping of electrons within a shell with common orbital angular momentum quantum numbers

threshold frequency

the minimum frequency (or energy) of electromagnetic radiation required to eject an electron in the photoelectric effect

ultraviolet (UV) light

borders violet light on the electromagnetic spectrum

visible region

the part of the electromagnetic spectrum that humans can detect with our eyes

wave function

a mathematical description of a wave in a wave equation

wavelength

the distance between successive crests (or troughs) of a wave

wave-particle duality

the concept that light and matter can be treated as both a wave and a particle

X-rays

second highest frequency on the electromagnetic spectrum

lewis structure

A model that uses electron-dot structures to show how electrons are arranged in molecules. Pairs of dots or lines represent bonding pairs.

bond order

the number of electron pairs shared between two atoms

delocalized

the phenomenon in which an electron pair is spread out over two or more covalent bonds

dipole moment

the magnitude of the charge separation between the electron poor and electron rich regions within a compound or within an individual chemical bond; often represented with a special arrow and typically measured in units of debye