Bonding Flashcards
Molecule
Covalent (Non Metal)
Formula Unit
Ionic Bond
Stable Octet Rule
atoms tend to either gain or lose electrons in their highest energy level to form ions
Ionic Crystal Lattice
repeating arrays of positive and negative ions
Characteristics of Ionic Bonds
- Crystalline at Room Temperature
- Higher Mp and Bp than covalent compounds
- Conduct electrical current in molten or solution state but nit in solid state
- complete polar bonds
- more soluble in polar solvent such as water
Polarity
depends on relative electronegativity of one atom in the molecule
Polar Covalent molecule
an unven distribution of charge due to an unequal sharing of bonding electrons
Non Polar if
Equal polar bonds that balance each other around the central atom then it is non polar even though the actual bonds may be polar
Network Solids
have repeating networks of covalent bonds that extends throughout the solid forming equivalent of one molecule
- hard and rigid
- high melting points
ex: diamond
Allotropes
very different chemical structures of the same element
- ex: carbon with grpahite and a diamond
Nanotubes
constructed with length to diameter ratio of up to 132,000,000 to 1
- hexagonally shaped
- tiny straw like cylindars of pure carbon
- stiffest and strongest fibers known
- useful electrical properties
Metallic bonding
bonding only in metals and consists of positive ions surrounded by a sea of electrons
Metallic binding characteritics
- Conductors of heat and electricity
- strong
- malleable
- ductile
- luster
- high density
- easy to form alloys because any similar sized sphere can fit into the spaces of the sea of electrons
Close packaging strcutures
metallic?
- Offset: positioning the 3rd layer over the second
2. directly above: positioning the third layer above the second
Ionic bond forms
with a metal and non metal either losing or gaining an electron then becoming a cation or anion. Then the electrons are transferred
