unit one study guide key words and terms Flashcards
paired electron
means all two spin states of the orbital specified by three quantum numbers n, l and m are fully occupied by two electrons
alkaline earth metals
group 2a metals, fairly reactive metals
electron affinity
energy released when adding an electron
Dalton
created Dalton’s law of partial pressure. A law stating that the sum of the partial pressures of each component in gas mixture equals the total pressure
unpaired electron
electron that occupies an orbital of an atom singly, rather than as part of an electron pair
J.J. Thomson
J.J. Thomson was born on December 18, 1856, in Cheetham Hill, England, and went on to attend Trinity College at Cambridge, where he would come to head the Cavendish Laboratory. His research in cathode rays led to the discovery of the electron, and he pursued further innovations in atomic structure exploration.
electron density
measure of the probability of an electron being present at a specific location.
what family of elements is mostly unreactive
nobel gases, all their valence electrons are full
metalloids
aka semiconductors zig zag line intermediate electrical conductivity which can be changed and controlled usefull for manufacturing
effective nuclear charge equation
Zeff= Z - S
excited state
unstable state for an atom/molecule in which energy has been absorbed but not re-emitted, raising an electron from ground state into a higher energy orbital
what is angular momentum QN aka, and what does it affect, what are the possible values
aka: subshell
affects: orbital shape
possible values: 0,1,2,3 or n-1
what does ml stand for, and what does it affect, possible values
magnetic quantum number, affects spatial orientation
possible values: -L,…-1,0,1,…L
metals
left side/periodic table. good conductors/heat and electricity. malleable, can be drawn to wires (ductility) often shiny
alkali metals
grop 1a elemetnys, highly reactive metals
angular momentum quantum #
The angular momentum quantum number, l, (subshell) describes the shape of the orbital. l = 0, 1, 2, … , n – 1 The higher the value of l the higher the energy.
energy level
light is a particle that moves like a wave. (everything moves like a wave) Only certain energy levels can exist. energy is quantized.
transition metals
less easily predictable properties based on their position in the periodic table
what does Zeff mean
charge “felt” by a valence electron
order of electromagnetic spectrum
radio waves, microwaves, infrared waves, visible light, ultraviolet radiation, X-rays, and gamma rays
principal quantum #
The atomic orbitals are first described by the principal quantum number (n), which describes how far the electron is from the nucleus. n = 0, 1, 2, 3 The higher the value of n, the larger the orbital. The higher the value of n, the higher the potential energy.
quantum mechanics
Scientists studied hydrogen’s spectrum and found a pattern that enabled them to develop a model to predict the probability of finding an electron at any location: can be expressed graphically by atomic orbitals
ionization energy
energy required to move an electron from an atom in a gaseous state
non-metal
upper right side/periodic. diving line b/w metals and nonmetals. solid @ room temp. other are gaseous. tned to be poor conductors of heat and electricity, tend to GAIN electrons in chemical changes
orbital
- can contain up to two electrons and has a particular shape and orientation. e.g. is the z-aligned orbital in the p subshell in the second shell.
what does Z equal in the Zeff equation
Z = the nuclear charge = the number of protons
pauli exclusion principle
Atoms other than Hydrogen have more than one electron in them. Just like bowling balls on a hill, electrons all want to go to the lowest energy level (n=1, s subshell). However, just as people need space, electrons need their own space too! It turns out that at most two electrons can occupy one atomic orbital. Furthermore, the two electrons must have opposite electron spins (spin up ↑ and spin down ↓).
how do you find the number of angular nodes?. Define each variable
l
l= angular momentum QN
what 2 factors does the atomic radius depend on
The valence orbital, The larger the value of n, the larger the atom Zeff, The larger Zeff, the smaller the atom
halogens
group 7. most familiar is chlorine, very reactive nonmetals
how do you find the total number of nodes? explain each variable
n-1 n= principle quantum number
noble gases
group 8. chemically inert, full valence electrons
ionic radius
For a specific element, the radius decreases with increasing positive charge As you go down the periodic table, the ionic radius increases
magnetic quantum #
The magnetic quantum number, ml, describes the spatial orientation. ml = -l, … , -1, 0, 1, … , l
isoelectronic
radius decreases with increasing protons,(atomic number)/ positive charge
emission spectrum
Spectrum assosiated with emission of electromagnetic radiation by elements or compunds
alkaline earth metals
fairly reactive, not as reactive as alkali
whats the principal QN symbol possible value, other name, and effects
symbol: n
possible values: 0,1,2,3,…
AKA: shell
Effects: orbital
in effective nuclear charge, the properties of an atom are determiend by
The charge of the nucleus 2) The repulsion between electrons 3) The wave nature of the atomic orbitals
ground state
state of atom/molecule in which electrons occupy the lowest possible energy orbitals available
subshell
Subshell - a group of orbitals with particular properties like shape and angular momentum. Labelled s, p, d, f, g etc.
hunds rule
energy orbital in a subshell is singly occupied w/ one electron any one orbital is doubly occupied. All electrons in singly occupied orbitals have same spin
bonding atomic radius
The bonding atomic radius is defined as one-half of the distance between covalently bonded nuclei
how do you find the number of radial nodes
n-1-L
