Chemistry - the Atom

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average atomic mass unit

amu

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molar mass unit

g/mol

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Erwin Schrodinger

quantum mechanical model of the atom, electrons don't always exist, it's impossible to know speed + location of electron

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James Chadwick

discovered the nuetron

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quantization

the concept that energy can occur only in discrete units called quanta

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Niels Bohr

determine energy is quantized, electrons exist at discreet energy levels (bohr model is useful but wrong)

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anion

a negatively charged ion with too many electrons

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cation

a positively charged ion with too few ions

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ion

atoms of the same type and have the same mass, BUT there is a difference in the number of protons or electrons

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isotope

atoms of the same type with different numbers of neutrons

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what does n stand for?

the charge (if the protons and electrons aren't the same number you put the net charge here)

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what does the Z stand for?

the atomic number (number of protons)

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what does the A stand for?

the mass number (protons AND neutrons)

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gold foil experiment

alpha particles that were shot at gold foil were deflected when they hit the positive center of gold atoms. The nucleus was discovered as a result of this experiment.

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Ernest Rutherford

using the gold foil experiment, he discovered protons and the nucleus

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plum pudding model

electrons were randomly distributed within a positively charged cloud

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cathode ray experiment

An experiment that showed that electrons had mass and a charge, electrons are ejected from the cathode and accelerated through a voltage

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JJ Thompson

used the cathode ray tube to discover electrons

plum pudding model

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used spherical model

John Dalton

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John Dalton atomic theory

  1. everything is composed of an atoms, they can not be created nor destroyed

  2. all atoms of 1 element are identical

  3. atoms of different elements are different masses and sizes

  4. compounds are comprised of whole number combinations of atoms

  5. a chemical reaction occurs is a rearrangement of atoms

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Democritus, stated that the atom is based on what two properties?

they are indivisible and atoms of a type are all the same

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Average atomic mass formula

(mass of A times percent A) + (mass of B times percent B) / 100

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speed

distance / time

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density

mass / volume

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rows (horizontal)

periods

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columns (vertical)

groups or families

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s block

first two groups

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p block

right six groups

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d block

teen groups (middle of periodic table)

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f block

bottom fourteen groups

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group 1

alkali metals

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group 2

alkaline earth metals

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groups 3 - 12

transition metals

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group 13

boron family

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group 14

carbon family

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group 15

pnictogen / nitrogen family

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group 16

chalcogen / oxygen family

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group 17

halogen family

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group 18

noble gases

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the s orbital shape

sphere

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the p orbital shape

dumbbell

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the d orbital shape

clover

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isoelectronic

the same electron

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why is chromium an electron configuration exception?

the electron can be spread out more evenly (memorize the configuration)

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why is copper an electron configuration exception?

the 1st set of electron must be paired up so 3d has more room than 4s (memorize the configuration)

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Aufbau Principle

electrons must fill the lowest energy level first

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Hund's Rule

electrons will spread out across all available energy levels before pairing up

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Pauli Exclusion Principle

that no two electrons can be the same (have the same quantum numbers)

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what does the n quantum number stand for

the principal quantum number (it is equivalent to the energy level of the electron)

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the electromagnetic spectrum from high energy to low energy

gamma ray - xray - ultraviolet - visible - infrared - microwave - radio

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photon

a particle that represent a quantum of light

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