2 ATOMIC THEORY Flashcards by Unknown Unknown

what are the quantum numbers?

principle, orbital, magnetic, spin

How well did you know this?

Not at all

Perfectly

what does principle number represent?

n; wave function type; number of nodes (n-1)

How well did you know this?

Not at all

Perfectly

what does orbital number represent?

l; which orbital its in; s0 p1 d2 f3

How well did you know this?

Not at all

Perfectly

what does magnetic number represent?

ml; xyz; orientation of orbital; depends on l

How well did you know this?

Not at all

Perfectly

what does spin number represent?

ms; identifies the two electrons in orbital; each electron has a diff spin; +1/2 or -1/2

How well did you know this?

Not at all

Perfectly

what is an orbital node?

point in a wave that is never displaced; where wave function and wavefunction^2 change phase; at a node - the electron density is 0

How well did you know this?

Not at all

Perfectly

what is electron density?

possibility of finding electron

How well did you know this?

Not at all

Perfectly

what are the rules to consider when placing electrons in orbitals?

aufbau: electrons added to lowest level - pauli: no two electron can have the same set of quantum numbers - hund: same spin maximized, half fill subshells first

How well did you know this?

Not at all

Perfectly

what does a longer wavelength indicate?

lower frequency

How well did you know this?

Not at all

Perfectly

what does changing amplitudes do?

affects intensity (e.g. brightness, volume, etc)

How well did you know this?

Not at all

Perfectly

what is the range of the visible spectrum? and which colour is lowest?

approx 400nm-750nm; violet - red

How well did you know this?

Not at all

Perfectly

what are the colours in the visible hydrogen emission spectrum?

violet, blue, blue-green, red

How well did you know this?

Not at all

Perfectly

what is the order in the electromagnetic spectrum from smallest wavelength to highest? (or highest frequency to smallest)

gamma rays, x rays, uv, visible, infrared, microwaves, radio

How well did you know this?

Not at all

Perfectly

what is the rydberg formula used for?

used to determine wavelength of electron moving between energy levels

How well did you know this?

Not at all

Perfectly

what is diffraction?

the bending of light

How well did you know this?

Not at all

Perfectly

when does constructive interference occur and what is the result?

when two wavelengths are in phase; wavelengths added

How well did you know this?

Not at all

Perfectly

when does destructive interference occur and what is the result?

when wavelength’s maxima is aligned with the others minima; wavelengths cancel out to zero

what occurs when a beam of light is used in the double slit experiment?

an interference pattern is produced

what occurs when a stream of particles is used in the double slit experiment?

two bright bands are produced but no interference pattern

what can the double slit experiment be used for?

to distinguish between waves and particles

what is bregolis equation used for what did he propose?

relating mass and velocity; proposed that electrons exhibit wavelike behavior in addition to particle-like properties

what is a standing wave?

a wave thats bound and only oscillates at certain frequencies

how do electrons travel if they cant be at the node?

they cross thru quantum tunneling

why do orbitals in the same shell differ in energy?

this is due to electron repulsion

what does isoelectronic mean?

atoms with the same charge; includes anions and cations

what is effective nuclear charge?

the net positive charge experienced by the valence electrons, accounting for screening from the core electrons

patterns in the periodic table: bond length and size of atoms/ions

increase in size as you go down pt. decrease in size as you go right pt.

patterns in the periodic table: ionization energy

decrease in size as you go down pt. increase in size as you go right pt.

patterns in the periodic table: electron affinity

decrease in size as you go down pt. increase in size as you go right pt.

patterns in the periodic table: electronegativity

decrease in size as you go down pt. increase in size as you go right pt.

what is ionization energy?

energy needed to remove electron from gaseous atom; with each successive ionization the energy needed to remove electrons increase (enthalpy H = +)

what is electron affinity?

energy change when gaseous atom gains electron; with each successive addition, energy required decreases (enthalpy more favourable H = -)

what is electronegativity?

ability of atom in molecule to draw electron density of a bond (pairs of electrons) to itself

what conclusion can be drawn from the double slit experiment?

electrons possess the properties of waves

according to bohr's model of hydrogen, why is the jump from 5to4 smaller than 2to1?

the energy gap decreases as n increases, which is also | why orbitals such as 5s and 4d are so close in energy)

although there is a trend in electron affinity on the pt, it is important to note that...?

more energy is required when adding electrons to a new orbital!

what do charges indicate about the size of an atom?

more electron charge means bigger size. anion>cation

how are the energy, wavelength, and frequency of electromagnetic radiation related?

energy of electromagnetic radiation inversely proportional to its wavelength. short wavelength = higher energy. frequency is how many times the wave repeats itself. shorter wavelength = higher frequency. energy and frequency are directly proportional. higher energy = higher frequency.

explain the bohr model

electron in hydrogen occupies lowest energy level (ground state). if electron absorbs energy, it promotes, reaching excited state. because excited state isnt stable electron will return to original state emitting energy as light. this energy difference corresponds to light of certain wavelength.

explain the origin of balmer, lyman, paschen series using the bohr model. list the energy levels and the spectrum it falls into

refers to the wavelength emitted when electron falls from a higher energy level to (BALMER) n=2 visible light, (LYMAN) n=1 UV, (PASCHEN) n=3 infrared.

explain in the context of quantum mechanics, what a node is.

area where the value of Ψ(x) is 0. it occurs at the point where wave changes phase (other than the fixed ends of the wave). it is where there is 0 probability of finding an electron

in quantum mechanics, what is the definition of an orbital?

area of space around the nucleus where an electron is most likely to be found within 90% probability