Bonding test Chem

bonding

all about valence electrons

what do you need for bonding

energy + orientation

BARF

Break absorb, Release form

Break absorb

endothermic- absorbing heat

release form

exothermic-release energy

Ionic

A metal and non metal

Electrons Transferd

electronegativity 1.7 or higher

Properties of Ionic compounds

High melting/boiling point, hard and brittle. can only conduct electricity as a LIQUID AND AQUEOUS

TICS

Transfer Ionic, Covelent shared

Covelent

non metals only

Electrons are shared TICS

Electronegitivity difference is less than 1.7

can be polar or non polar

covelent Non polar =

0 —> 0.4

electrons are equally shared

covelent polar

0.4 —→ 1.7

electrons are unequally shared

Properties are molecular or covelent solids

low melting and boiling point = weak and soft

Network solids

strong

example: diamond and quartz

NaNO3

has both ionic and covelent bonds

Polyatomic

metallic

metals only, sea of mobile electrons

properties: strong, high melting and boiling point, and good conductors

Ionic drawing

Brackets

positive=no dots

Negative=8 dots

covelent drawing

octet rule NOT H

ex. H-H

SNAP

Symmetrical non polar

Asymmetrical polar = dots in the middle

Mole ion attraction

Strongest, highest boiling point and melting point

A METAL

ex. NaCl in water

Hydrogen bonding

strong

Hydrogen with F, O, or N

Ex. HF, NH3, H2O

Dipole-Dipole

polar molecules

asymetrical

Ex. H-Cl

Van Der Waals

non polar

symmetrical

lowest melting/ boiling point

Ex. H-H