structure 2 test hl chem | Quizlet

why don't transition metal ions need to reach NGC

they have electrons in the d sublevel making the atoms and ions more stable

nitrate

NO3-

hydroxide

OH-

hydrogencarbonate

HCO3 -

carbonate

CO3 2-

sulfate

SO4 2-

phosphate

PO4 3-

ammonium

NH4 +

intramolecular force

within molecules

intermolecular force

between different molecules

non-directional force

an ion will attract all the oppositely charged ions around it equally - stronger force

lattice enthalpy

energy required to break apart the ionic lattice convert the ions into their gaseous state and spread them infinitely apart

what affects the size of lattice enthalpy?

ionic radius and ionic charge (greater charge density = greater lattice enthalpy)

High Melting (Properties of Ionic Bonds)

greater lattice enthalpy = higher melting point

Solubility (Properties of Ionic Bonds)

solvent molecules surround solute molecules and pull them apart from the ionic lattice (LIKE DISSOLVES LIKE; polar solvents dissolve polar solutes)

Volatility (Properties of Ionic Bonds)

measure of how easily a substance will turn into gas - ionic compounds are non volatile due to strength of ionic bonds and forces

Electrical Conductivity (Properties of Ionic Bonds)

solid ionic compounds don't conduct electricity unless molten

Brittleness (Properties of Ionic Bonds)

measure of how easily solids will shatter into small pieces when force is applied - ionic compounds are brittle since positive ions will repel other positive ions where slid together

covalent bond

formed by electrostatic attractions between shared pair of electrons and the positively charged nucleus

exceptions of the octet rule

B, Be, H, He, Al

bond length

distance between the nuclei of two atoms in a bond (stronger intramolecular electrostatic attraction = shorter bond length)

two types of covalent bonds

pure covalent (nonpolar) and polar covalent bond

electronegativity difference in a nonpolar covalent bond

0-0.4

electronegativity difference in a polar covalent bond

0.5 - 1.7

only IMF in non-polar molecules

london dispersion forces

hydrogen bonds form between hydrogen and...

N, O, F

hydrogen bonding is what type of force

intermolecular (between molecules)

Volatility (Properties of covalent compounds)

nonpolar molecules are very volatile due to only IMF being LDF's, polar molecules are less volatile

Electrical Conductivity (Properties of covalent compounds)

covalent compounds dont conduct electricity as solids or molten due to having no delocalized electrons

allotropes of carbon

diamond, graphite, fullerene

diamond shape

tetrahedral

graphene shape

trigonal planar

graphite shape

trigonal planar

fullerene shape

spherical structure - trigonal planar

silicon dioxide structure shape

tetrahedral

resonance structures

structures that occur when it is possible to draw two or more lewis structures that have the same number of electron pairs for a molecule or ion

no

no

metallic bond is caused by

an electrostatic attraction between a lattice of cations and delocalized electrons

factors determining size of the metallic bond

number of delocalized electrons (more de = bigger charge difference), charge of teh cation (greater pos. charge = greater force of attraction), and radius of the cation (smaller cations exert greater electrostatic force)

electrical conductivity: properties of metals

metals are good electrical conductors due to having delocalized electrons

thermal conductivity: properties of metals

metals are good thermal conductors due to having delocalized electrons and the cations being closely packed together

malleability: properties of metals

metals can be beaten into different shapes since metallic bonding is non-directional (delocalized electrons are attracted to all the cations in all directions)

alloys

mixture of a metal and other metals or non-metals, which have enhanced properties

alloys are what type of mixture

homogenous

polymers

large molecules made from repeating subunits called monomers

polymerisation

process of joining monomers together to make a polymer

properties of polymers

do not conduct electricity (no delocalized electrons) and poor thermal conductors (covalent compound)

addition polymerisation

occurs when a monomer contains a double bond, and has only one product - the monomer

condensation reactions

polymers formed by a reaction between functional groups in each monomer with the release of a small molecule, usually H2O, molecules with two or more functional groups can carry out condensation reactions

ester bond

bond between hydroxyl and carboxylic group (in PET molecules)

amino bond

bond between carboxyl and amino group to make a protein out of amino acid monomers

hydrolisis

opposite of condensation - addition of water to break the bond between monomer units