Chemistry Unit 3

periodic

a regular repeating pattern

periodic table

arrangement of elements so that their physical and chemical properties follow a regular repeating pattern

periodic

a regular repeating pattern

periodic table

arrangement of elements so that their physical and chemical properties follow a regular repeating pattern

groups or families

columns(vertical), all have similar properties, same number of valence electrons(these electrons affect physical and chemical properties)

period

rows(horiziontal)

Dmitri Mendeleev

-Element 101 was named in his honor
-first to come up with a periodic table
-(1870) Organized the 63 known elements of the time in order of their atomic mass
-Saw a pattern with the number of elements that can be bonded to that element- has to do with valence electrons
-Left spaces in periodic table where it appeared an element wasn't discovered yet
-Predicted properties of unknown elements and was correct

issue with Mendeleev's table

arranged his table by atomic mass instead of atomic number

Henry Moseley(1910)

-Discovered atomic number(number of protons in an atom)
-Rearranged periodic table by this number and it fell into perfect order

periodic law

Physical and chemical properties of the elements are periodic functions of their atomic numbers-when elements are arranged by atomic number you should see chemical and physical properties repeating themselves

Alkali Metals

Group 1 excluding H, all have 1+ charge, extremely reactive

Alkaline Earth Metals

Group 2, all have 2+ charge

Transition metals

groups 3-12, slightly reactive

halogens

Group 17, extremely reactive

noble gases

Group 18, extremely inactive or inert because of full valence shell

lanthanide series

top row on the bottom two

actinide series

bottom row on the bottom two

Elements on the steps

all metalloids or semiconductors(except Al- it is a metal)

Physical properties(metals)

luster, conductive, malleable, ductile, high density, high melting point(All are solid at room temperature except for Hg)

Chemical properties(metals)

most metal will react with O2 or H2O to form an oxide(metal+oxygen), this is rusting or tarnishing

Metals give up_to get to a full valence shell

e-(electron)

Physical properties(nonmetals)

dull, don't conduct, brittle, low density, low melting points(can be solid, liquid, or gas at room temperature)

Nonmetals take____to get full valence shell

e-

Physical properties(metalloids)

shiny or dull, conduct ok, ductile and malleable, or brittle(Al is light metal not metalloid)

Avogadro's Law

The number of particles of a gas of equal volumes as equal pressures and temperatures was a constant regardless of the gas

amu =

g/mol

Most reactive metals(trend)

down and to the left, in a square- N-shape

Most reactive nonmetal

up and right(excluding noble gases), in a square- Z-shape

atomic radius(trend)

down and to the left, backwards Z-shape

Ionization energy

energy required to remove an electron from an atom

Ionization energy(trend)

up and to the right, backward z-shape

electron affinity(trend)

up and to the right, backward z-shape

oxyanions

Negative ions containing oxygen

metal and nonmetal bond

ionic bond

nonmetal and nonmetal bond

covalent bond

nonmetal and metalloid bond

covalent bond

Polyatomic and anything bond

ionic bond