Chemia TEST

enthalpy

energy required to break the bond

Intermolecular forces

- permanent dipole-dipole interaction - induced dipole - dipole forces - London forces

Dipole-dipole forces

- different or same molecules. - permanent

Hydrogen bonds

very strong, NOT Van der Waals, 2 conditions (the electonegative element must have at least one lone pair, hydrogen atom must be attached to a highly electronegative atom)

London forces

- weak and only for a second - 17 and 18 group mostly

covalent bond

electrostatic force of attraction between the shared pairs and the positively charged nuclei

ligands

te atomy z boku

lattice enthalpy

energy required to break one mole of a solid compound into ions in the gas phase

Ions

not volatile (nie lotne), in solid state they don't conduct electricity, in liquid yes, soluble mostly

the lower the ia

the weaker the compound

Formal charge

=n wal - 1/2 bond - wolne electr

hybridization

sp3 - sigma bonds, sp2 - pi bond, trigonal planar, sp3 - two pi bonds, linear

Metalic bond

force of electrostatic attraction between the lattice of cations and demoralized electrons

the smaller and more positive the ion

the stronger the bond

high melting point

strong metal

bonding triangle

average and delta

alloys might have different properties

different packaging of the cations in the lattice

alloys are

stronger more resistant to corrosion

steel

iron and carbon

bronze medal

copper and sn (tin)

brass

copper zinc