HONORS CHEM Electron Configuration

shell 2

2 subshells s and p orbitals 1 orbital in s subshell, 3 orbital in p subshell 4 orbitals in n2 energy level 8 electrons in 2n2 energy level

energy level 3

3 sublevels, 5 orbitals, 18 electrons

energy equation

E = h(v) where v is frequency

speed of light

c= 2.998 x 10^8 m/s

shapes of orbitals

s: sphere, 1 orbital p: dumbbell/infinity sign, 3 orbitals d: flower/clover, 5 orbitals f: cluster, 7 orbitals

neutrons

1 amu mass, located in nucleus, neutral charge

protons

1 amu mass, located in nucleus, positive charge

energy level 1

1 sublevel, 1 orbital, 2 max electrons

shell 1

1 subshell s orbital 1 orbital in subshell 1 orbital in n2 energy level 2 electrons In 2n2 energy level

energy level 1

1 subshell s sphere orbital 1 orbital in sublevel 1 orbital in n2 energy level 2 electrons in 2n2 energy level

things electron configuration shows

1. principle quantum number (energy level) or shell (n) - distance from the nucleus 2. energy subshell or sublevel: (orbital/angular quantum number) tells type/shape of orbital - shows electron cloud shape - s, p, d, f 3. number of electrons

electrons

1/2000 amu mass, negative charge, located in electron cloud outside nucleus

1s2 - representation

1: quantum number/energy level/shell s: energy subshell 2: # of electrons found in each subshell

energy level 2

2 sublevels, 3 orbitals, 8 electrons

energy level 2

2 subshells s sphere and p dumbbell orbitals 1 and 3 orbitals in sublevels 4 orbitals in n2 energy level 8 electrons in 2n2 energy level

energy level 3

3 subshells s sphere, p dumbbell and d flower orbitals 1, 3 and 5 orbitals in sublevels 9 orbitals in n2 energy level 18 electrons in 2n2 energy level

shell 3

3 subshells s, p, d orbitals 1, 3 and 5 orbitals in subshells 9 orbitals in n2 energy level 18 electrons in 2n2 energy level

3p5 - what does it represent?

3: quantum number/energy level/shell p: energy subshell 5: superscript - # of electrons in each subshell

energy level 4

4 sublevels, 7 orbitals, 32 electrons

energy level 4

4 subshells s sphere, p dumbbell, d flower and f orbitals 1, 3, 5 and 7 orbitals in sublevels 16 orbitals in n2 energy level 32 electrons in 2n2 energy level

shell 4

4 subshells s, p, d and f orbitals 1, 3, 5 and 7 orbitals in subshells 16 orbitals in n2 energy level 32 electrons in 2n2 energy level

possible levels and shapes

7 possible energy levels, 4 possible shapes

frequency wave equation

C = V//\

size of radius of negative ion to neutral atom

Cl o Cl - O as an ion gains electrons, its atomic radii increases

size of radius of positive ion to neutral atom

Li O Li+ o as an ion loses electrons, its atomic radii decreases

properties of light relationship

V = c//\ E = hv E= hc over v c = v/\ 1 nm = 1.0 x 10^-9 m convert wavelength from nm to m v = frequency, /\ = wavelength, c = speed of light

frequency

V, H^2, or s-1 rate at which vibration occurs that constitutes a wave, measured per second in a material: sound waves, electromagnetic field - radio waves, light c = V/\

quantum

a quantum of energy is the amount of energy required to move an electron from one energy level to another

flame test lab

absorbing energy excites atoms, but then they move back to their normal level/ground state going from a higher to lower level = photons energy of photon determines color

quantum

amount of energy required to move an electron from 1 energy level to another

Pauli Exclusion Principle

an atomic orbital may describe at most 2 electrons, and to occupy the same orbital, electrons must have opposite spins

ion

atom w/electric charge due to loss or gain of electrons, ability of neutral atom to gain or lose electrons

ions

atoms that have gained or lost electrons to try to be like a noble gas

diff of cations/anions

cations - lose electrons, become positive anions - gain electrons, become negative

group

column/family

orbital

contains 2 electrons

isotope

diff # of neutrons, same atomic and proton

wavelength

distance between crests of a wave

orbital notation

electrons are drawn in on blanks representing the orbitals

understanding electrons using the Bohr Model

electrons can be found in different shells around the nucleus and correspond to regions in space that electrons can occupy - like rungs of a ladder, electrons can't be located between shells - each shell can only hold a certain number of electrons, and when full, electrons must go to a new shell

Aufbau Principle and order of sublevels

electrons enter orbitals of lowest energy first - orbitals represented by boxes, each orbital holds 2 electrons, within a principle energy level (n) the s is always the lowest energy sublevel, as the principal energy number increases, sublevels can overlap - 4s is lower than 3d, 4f is lower than 5d

orbitals

electrons exist at energy levels in these defined areas known as orbitals - orbitals are regions of probability in which the electron can be found, and these regions have very specific shapes based on the energy of the electrons that will be occupying them

core electrons

electrons located in all of the inner shells, total electrons minus valence electrons = # of core electrons

valence electrons

electrons occupying the outermost shell

quarks

elementary particles, forms hadrons (protons/neutrons)

Planck's Constant

energy of each photon in terms of frequency

atomic radius trends

gains: increases size, loses: decreases size - period: increases right to left <---- (highest at left) - group: increases top to bottom | (highest at bottom) - large radii very bottom left of table, small at very right top

Planck's Constant and its use

h= 6.625 x 10^-34 J/s - using this, we can calculate the energy (E) needed to excite that electron to the next energy level

metal

hard, opaque, shiny, good conductor of electricity/heat

anions

have negative charge, gained electrons

cations

have positive charge, lost electrons

how electrons move levels

heat, electricity and light can move the electron up to diff energy levels, the electron is now said to be excited and as it falls back to the ground state, it gives the energy back as light

core electron

inner shells

periodic law

law that properties of chemical elements are periodic functions of their atomic number

S Orbital

lowest-energy style orbital, sphere-shaped and is always first orbital filled in any energy level, first 2 columns of periodic table are S block elements - electrons can move anywhere within the S orbital sphere

electronegativity and trends

measure of the tendency of an atom to attract a bonding pair of electrons - Francium lowest, Fluorine highest - periodic table: increase up left to right / - metals lowest, nonmetals highest - group: increase bottom to top - period: increase left to right

how electron configuration works

n = principal quantum number, shell, energy level energy sublevel - s, p, d, f - each sublevel has orbitals - each orbital holds 2 electrons each

anion

negatively charged ion that gained electrons

P Orbitals

once the s orbital has been filled for any energy level, the electrons start filling this orbital - the p orbitals are shaped like propeller blades, with one set lined up along the x axis (horizontally), 2nd set along the y axis (vertically) and 3rd set along z axis (from front to back through atom)

what do outermost electrons determine?

outermost electrons determine the chemical properties of the element

valence electron

outermost shell

transition metal

partially filled d-subshell, can rise to cations

photon

particle representing quantum of light/electromagnetic radiation

cation

positively charged ion that lost electrons

electron configuration representation

principle energy level - assigned values 1, 2, 3 or 4 atomic orbital - region in space where there is high probability of finding an electron: s, d, p, f sublevel: combined principle energy level and orbital - 3s, 3p, 3d

energy level or quantum level

principle level 1, 2, 3, 4

ionization energy and trends

process by which an atom or molecule acquires negative or positive charge, increases upward left to right, gain or lose electrons - group: increase bottom to top - period: increase left to right - periodic table: increase up left to right /

Pauli Exclusion Rule

responsible for idea for spin or shape orientation of electron in the orbital

Aufbau Rule

responsible for orbitals filling from lowest to highest energy level

Hund's Rule

responsible for orbitals filling one electron per orbital until all orbitals of subshell are filled

period

row

subshell or shape

set of electrons w/same quantum number

electron shells

shells are represented by the letter n (the quantum number) and each shell can hold 2n^2 electrons

Aufbau Principle

the Aufbau Principle starts at the lowest energy level and build up to the higher energy levels only after the lowest are filled

Hund's Rule

the Hund's Rule states that each p orbital must receive one electron before any p orbital can receive a 2nd filling electron: each of the 2p orbitals will receive one electron (up-facing) before any will get a second electron (down-facing)

Bohr Model

the energy level of an electron is analogous to the rungs of a ladder: the electron cannot exist between energy levels, just like you can't stand between rungs on a ladder

what do energy levels show?

the energy levels of the atoms correspond to the rows of the periodic table, and the energy levels are built up from the level closest to the nucleus outward

what does electron configuration show you?

the total of the superscripts will always be equal to the atomic number

D Orbital

there are 5 making 10 electrons in all, filled by the elements in the dropped central section of the table with d block elements/transition metals

F Orbital

there are 7 making 14 electrons in all, the 2 rows separated at the bottom of the table are F Block elements

color as light

this light as energy is color, and we see this at a specific wavelength in the visible spectrum: from the wavelength, we can use the equation C=/\V to calculate the frequency (V) at which this occurs)

Hund's Rule

when electrons occupy orbitals of equal energy, they don't pair up until they have to

explanation of atomic spectra

when we write electron configurations, we are writing the lowest energy or the ground state: the lowest energy level and where the electron starts from