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Chemistry - Unit 2

Chemistry Unit 2 Learning Statements

TermDefinition
Mendeleev arranged the periodic table by atomic mass & identified characteristics of elements that had not yet been discovered
Mosely arranged the periodic table by their number of protons (atomic number)
Thomson used cathode ray tubes to discover the electron
Rutherford experimented with alpha particles and gold foil to discover the nucleus is located in the center of the atom and the rest is mostly empty space
Bohr studied light and electron movement to discover that electrons are in fixed orbits (energy shells)
neutral atom has equal number of protons and electrons
valence electrons electrons located in the outermost shell of an atom
group number tells how many valence electrons are in atoms of those elements
groups vertical columns on periodic table; elements in the same one have similar chemical properties or reactivity
periods horizontal rows on periodic table; elements in the same one have the same number of energy shells
group 18 most stable group; has 8 valence electrons; does not want to form compounds
group 1 highly reactive group; has 1 valence electron; wants to bond to form compounds
group 17 highly reactive group; has 7 valence electron; wants to bond to form compounds
atomic number number of protons; determines the identity of an element
wavelength the distance between two identical points on a wave; crest to crest; trough to trough
wave frequency the number of times a wave passes a fixed point in a given amount of time
electromagnetic spectrum consists of different types of waves; radio > micro > infrared > visible light > ultraviolet > x-rays > gamma rays
wavelength and frequency inversely proportional; when wavelength increases = frequency decreases
energy and frequency directly proportional; when frequency increases = energy increases
short wavelengths high energy waves
long wavelengths low energy waves
violet color of light with highest amount of energy
red color of light with lowest amount of energy
atomic mass number of protons + number of neutrons
isotopes atoms with the same number of protons, but different numbers of neutrons
number of neutrons atomic mass minus atomic number
average atomic mass weighted average of all the isotopes of an element; will be closer to the isotope with the highest percent abundance
atomic radius size of the atom; distance from the nucleus to the valence electrons
atomic radius trend decreases across a period (from left to right); increases down a group (top to bottom)
ionization energy the amount of energy needed to remove an electron
ionization energy trend increases across a period (left to right); decreases down a group (top to bottom)
ionization energy trend reason as you go across a period, electrons feel stronger attraction from the nucleus (protons); as you go down a group, energy decreases because valence electrons are further away from the nucleus
electronegativity the tendency for an atom to attract electrons; excludes noble gases
electronegativity trend increases across a period (left to right); decreases down a group (top to bottom)
electronegativity trend reason as you go across a period, electrons reel more attraction from the nucleus to pull in more electrons; as you go down a group, the size of the atoms increases and valence electrons are not influenced as much by the nucleus
nonmetals tend to have a higher electronegativity than metals
metals tend to have a lower electronegativity than nonmetals
Created by: teafair
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