Atomic Bonding and Periodic Table Review

Mr. Janick

Johan Dobereiner

Firts grouped elements into units of 3 called triads based on properties

John Newlands

developed the law of octaves in that every 8th elemt repeats similar properties.

Lothar Myer and Dmitri Mendeleev

arranged the elements by atomic mass. they also independently developed the first periodic law which states that element’s properties repeat themselves when the element are arranged by atomic mass.

Mendeleev’s Periodic Table

was chosen over meyer’s because he left gaps for undiscovered elements and predicted the propeties ofthose elements.

Henry Mosley

Later revised the periodic table by using the atomic number in an element rather than the atomic mass because the electron structure is what determines the properties of elements.
Revised the periodic table law to state that the chemical; and physical properties of the elements are periodic functions of their atomic numbers instead of mass.

The Octet Rule

states that the main group elements bond in such a way that the valance electrons with have 8 electrons in the outermost S and P levels. If atoms have less than 8 electrons they will try and bond with other atoms to form more stable compounds.

periods

horozontal rows on the periodic table which stand for the same energy level from 1 to 7.

Families

vertical columns on the periodic table that represnts similar properties due to having the same number of valence eletrons.

Valance electrons

outermost S and P electrons

Coulomic attraction

the force of attraction between oppositely charged particles that are stationary. The farther the protons are to the electrons, the weaker the attraction.

shielding

the repulsion of negative electrons pushing away other negative electrons

electromagnetic force

the broader interaction between electric and magnetic firces of particles that are both moving and stationary so it would include coulombic attraction and more.

Atomic radius

the distance from the nucleus to the outermost electron energy level (low, left, large)

ionization energy

the energy required to remove an electron from an atom (low, left, low)

electronegativity

the tendency of an atom to attract electrons twords itself. (low, left, low)

Metals

left of the jagged line separating metals and non metals.

metalloids

the metals on or next to the jagged line on both sides, 7 of them

ionic bonds

the elctrons are completely transfered from one atom to another, also called formula units.

covalent bonds

the elctrons are shared between the bonded atoms

non polar covalent bonds

share electrons equally

polar covalent bonds

share electrons unequally with one side of the molecule becoming negative becasue it is holding electrons closer to its negative side while the other side becomes positive because the elctrons are partially pulled away.

metallic

metals or alloys of the same type being bonded together, positive metal ions allow electrons to shift between them

ionic bond

metal with a non metal, transfers electrons from positive cation to negative anion causing the oppositely charged ions to attract.

covalent bond

one metal and one non metal.

single bond

shares two electrons equally

double bond

shares four electrons between the two covalent bonded atoms

triple bond

shares 6 electrons between the two covalent bonded atoms

Dipole-Dipole interaction

the positve side of one molecule attracts the negative side of another molecule.

Hydrogen Bonding

the positive sideis usually the hydrogen side which attracts the negative side of another molecule

linear molecule

forms a staright line

bent molecule

forms and angle

trigonal planar molecule

flat triangle shape

trigonal pyramidal molecule

forms a pyramid shape

Tetrahedral molecule

when a central atom is bomded to four other atoms

Polarity

is the molecule is equally balanced, it will be non polar. if the molecule is unbalanced, it will be polar

Low, Left, Large

The further down the periods, the kore energy levels, thus the larger the atomic radius. the further left on the famile’s, the less protons and electrons and once again the large the atomic radius.

Low, Left, Low

The further down the periods, the more enegry levels, thus the larger atomic radius and the lower the energy is to remove an electron from an atom.