- discovered the mass and charge of an electron - the electric field must be a multiple of the charge of an electron to suspend particles

Exam 1 Flashcards by Sydney Johnson

first controlled reaction

fire

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Aristotle believed in…

unlimited divisions of matter, not true

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Democritus believed in…

limited divisions, true = atom as smallest fundamental unit

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law

describes an observation, answers “what”?

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theory

explains an observation, answers “how” and “why”? (think conspiracy theories)

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Law of Conservation of Mass

matter is neither created or destroyed

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Law of Definite Proportions

a substance is always made of the same proportion of elements

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Law of Multiple Proportions/Constant Composition

elements combine in small whole number ratios (multiples)

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Dalton’s Atomic Theory (5 parts, 2 proven wrong)

Matter composed of small, indivisible particles (=atoms)
Atoms of a particular element are identical*
Atoms combine in small, whole number ratios
Atoms are neither created or destroyed*
Atoms of different elements are different

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J.J. Thomson findings

discovered the electron (cathode rays are negatively charged particles), creating the plum pudding model in response
discovered applying force caused acceleration

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Millikan findings

discovered the mass and charge of an electron

- the electric field must be a multiple of the charge of an electron to suspend particles

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Rutherford findings in gold foil experiment

positive charge located in one dense area: nucleus
neutral particles with mass also here: neutrons
atom is mostly empty space
created the nuclear model of the atom: nucleus as very tiny and atom as huge and largely open space

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Mass defect

difference between the predicted mass and the actual mass of an atom’s nucleus

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atomic number, number of protons (and electrons in neutral atom), written on bottom

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atomic mass, # of protons and neutrons, written on top

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to determine number of neutrons…

mass # - protons

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isotopes

atoms of the same element with different number of neutrons (as evident through mass number)

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ions

atoms that are not neutral due to different numbers of protons and electrons

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atomic mass

weighted average between atomic mass of natural abundance of isotopes of an element

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Avogadro’s number

6.02 x 10^23 (just a number, no units)

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how are E, frequency, wavelength related?

as E and frequency increase, wavelength decreases

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on color spectrum of light, which colors are high E/low E?

Reds are low E, blues are high E

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photoelectric effect

the emission of electrons when light hits a material

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photon

particle of light

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Planck's constant relates to...

light /E of photon

work function

E of a photon necessary to remove an electron from metal via the photoelectric effect

What does Rydberg's equation measure?

predicts the transitions between quantized energy levels (n) based off of wavelength (and vice versa)

Bohr

made first model of the atom with quantized electrons; problems: only works for 1 electron atoms and treats electrons classically

de Broglie equation

how to find wavelength

de Broglie equation

how to find wavelength, mass must be in kg and velocity in meters/second

microscopic particles are best considered to be

waves

uncertainty principle

it's impossible to know simultaneously and exactly the position and momentum of a microscopic particle

wave function

electrons described as standing waves

standing waves

waves that don't travel

(wave function)^squared

describes the likelihood of finding an electron at a particular point in space (a sort of probability density map)

quantum numbers

describe where a particular electron is within an atom

atomic orbital

where electrons are likely to be found for each possible quantum state

principle quantum number = n

- shells, distance from nucleus - coordinates to periods - higher n = higher E

angular momentum quantum number = l

- subshells - describes an orbital's shape - s,p,d,f

circle node and how to find

radial/spherical, what's leftover

line node and how to find

planar/angular; l

how to find total nodes

n-1

magnetic quantum number = m sub l | *helpful for remembering what l corresponds to n if you look at picture/energy table

- number of orbitals in each subshell - for l=0, 1 orbital - for l=1, 3 orbitals - for l-2, 5 orbitals - for l=3, 7 orbitals * to help remember, look at electron config

pauli exclusion principle

no 2 electrons in one atom can have same set of quantum numbers, caused spin quantum number to be created

spin quantum number = M sub s

+1/2, -1/2 | spin direction of electron

aufbau principle

electrons in ground state atom (low E) occupy the lowest energy orbitals available to them first then move up

shielding

attraction between an electron and the nucleus in an atom with multiple electrons

Z effective

nuclear charge that electrons feel

relationship between Z actual and Z effective in multi electron atom

Z effective < Z actual | if there is more than one electron, don't feel full pull of nucleus = farther away

closed shell

full outermost shell

how to find an elements inner and valence electrons

- inner: look at Z of last noble gas | - valence: what's left

hund's rule

equal E orbitals are singly filled before they are fully filled

d-block anomaly #1

it is particularly stable for d-orbitals to be half-filled or fully-filled. 1 s-orbital electron is moved to d-orbital to satisfy this

isoelectronic

atoms/ions with identical electron configurations

d-block anomaly #2

when losing electrons, d-orbital elements lose both valence shell s-orbital electrons before losing d-orbital electrons (applies to ions)

periodic trends: to go up/down table use

periodic trends: to go left/right table use

why use Slater's Rules

to approximate Z effective

periodic trends: Z effective

up/down table (as n goes up), Z eff goes up | as z goes up (move left to right), Z eff goes up

periodic trends: atomic radius

as n goes up (move down table), radius goes up | as z goes up (move left to right), radius goes down

periodic trends: ionization energy

- as n goes up (move up to down), IE goes down | - as z goes up (move L to R), IE goes up

periodic trend: ion radius

- as ions lose electrons, radius decreases ( = less pull) | - as ions gain electrons, radius increases

electron affinity (EA)

the E released when an electron is added to an atom - very general - EA increases as you move across and up the periodic table

Exam 1 Flashcards

(63 cards)