Unit 9- Chemical Bonds Flashcards
chem bonds
forces that hold the atoms together in substance
- ionic bonding: cation + anion (ionic cpd)(transfer of e-)
- covalent bonding: nonmetal eles (molec cpd)
Lewis Electron-Dot Symbol
Symbol of ele surrounded by dots which represent their ve-
- cations: most have no ve- shown
- anions: most hve 8 ve-
lattice energy
energy required to sep 1 mol of ionic solid into its gaseous ions
LE= (k|Q1Q2|)/r
Q1 and Q2 = ionic charges
r = distance between ions in the solid
- use Q1Q2 for LE but when all the same, use r
covalent bonding
results from atoms sharing an e- pair
bond length
the distance between the nuclei of 2 bonded atoms
Lewis Structures
show how the ve- are arranged in a molec or polyatomic ion
bonding pairs
e- shared between 2 atoms and are rep by lines
lone pairs
entirely on one atom and are rep by 2 dots
octet rule
atoms share e- until each atom is surrounded by 8 e-
- single bond: share 1 pair e-
- double bond: share 2 pair e-
- triple bond: share e pair e-
bond order
the # of e- pairs shared between 2 atoms
- as bond order incs, length of bond decs and strength of bond incs
skeleton structure
shows which atoms are bonded to each other
central atom
bonded to 2 or more other atoms
- usually farthest left and down on periodic table
terminal atom
bonded to 1 other atom
* H and F are always terminal
writing Lewis Structure
- start with the skele structure
- sum the ve-
- substract 2e- for each bond in skele structure
- count the # of e- needed to satisfy octet rule (if # needed > # remain, add 1 bond for each additional 2e- needed )
- place remaining e- as lone pairs to satisfy octet rule
bond polarity
- UNEQUAL sharing leads to a POLAR covalent bond
- EQUAL sharing leads to a NONPOLAR covalent bond