Bonding

bonding

can involve transfer, sahring, or super-sharing of e- between two atoms

ionic bond

bond that forms when atoms transfer one or more e- and becomes ions

• difference in EN is greater than 1.67

covalent bond

bond that forms when atms share one or more pairs of e-

• difference in EN is less than or equal to 1.67 but greather than or equal to 0.00

• three subtypes

  • polar covalent bonds

  • nonpolar covalent bond

  • coordinate covalent bond

polar covalent bond

unequal sharing of e- pair

• difference in EN is less than or equal to 1.67 but greather than 0.00

nonpolar covalent bond

equal sharign of e- pair

• difference in EN is equal to 0.00

cordinate covalent bond

one atom shares a pair of e- (2e-) with another atom or ion

metalic bonding

• occurs between metalic atoms

• ‘super-shaaring” or all e- within a metalic sample

sigma bond

when two atoms form a single covalent bond

Pi bond

when two atoms form a duble covalent bond another bond forms around the first sigma bond

hybrid orbitals

when e- form different orbitals ina given atom form sigma bonds the different orbitals will hybridize

• Pi bonds DO NOT hybridize they require normal orbitals to stretch around the sigma bonds

metalic

most metalic elements have either one or two valence e-

• have low EN so they cant take valence e- from other atoms, nor can they share enough e- between two atoms to make an Octet

• instead all of the mtalic nuclei in a given sample share all of their valence e- equally

ionic compounds

(salts): composed of ionic bonds

• crystal lacttice: repetitie 3 diemnsional pattern of cations and anions

• verry high melting and vaporizaiton temps

• hard but brittle solid at room temp

  • hard to break but will crack with enough force

  • can seperate ions or groups of ions

• conduct electricity in a liquid state or dissolved in water (electrolyte)

covalent compounds

(molecules): composed of covalent bonds

• each molecule is a stable set of atoms

  • moelcules can be separated from eachother, but individual atoms of a moelcute stay tigherth

• low melting and vaporization temp

• usually gases or liquid but can be solids at room temp

  • brittle in solid state

• bad conductor of heat and electricity

• solubility

  • polar molecules disolve in polar substances

  • nonpolar molecules dissolve in nonpolar substances

metal compounds

(alloys): ie elements composed of metalic bonds

• alloys examples:

  • brass: copper + Zinc

  • bronze: copper + tin

  • steel: iron, carbon, + other elements

• typiclay hihg melting and vaporization tiemp

• solids at room temp (except murcury)

• flexible

  • malleable: hammered or rolled in thin sheets

  • scuttle: drawn into wires

• verry good conductior of electricity and heat

• hard and durable