In todays class we learned about Cyclo Alkanes and Aromatics.
Cyclo Alkanes
-Carbon compounds can form rings -Follow the same naming rules and add cyclo- in front of the parent chain
cyclobutane
Name:
1. cyclopentane 2. 1 ethyl 3 methyl cyclohexane
Draw the structural diagram for: 1. 1,3,5 trimethyl cyclo octane 2. 1 ethyl 3,4 dimethyl cyclohexane If a cyclic chain is a side chain use cyclo___yl 2 methyl 3 cyclopropyl pentane
Aromatics When a cyclic 6 carbon chain forms it can create a resonance structure *Benzene
There are more carbon compound than all ionic compounds combine
the study of carbon compounds is called organic chemistry
carbon can have multiple bonds and form many different shapes
Hydrocarbons:
Aliphatics
alkanes
alkenes
alkynes
Alycyclics
Aromatics
Hydrocarbons have 3 types of formulas:
Nomenclature of Hydrocarbons: - one molecular formula can have a number of different structures Isomers are compounds that can be drawn in more than 1 way
Naming Alkanes:(all single bonds)
name the longest chain by using the correct suffix and add -ane
locate any branches by numbering carbon atoms *use the lowest possible number system
name branches by using appropriate suffix and -yl ending (alkyl branches)
if there are more than one of the same alkyl group, number each one and add the multiplier number in front of the branch name. *use alphabetical naming system.
On thursday's class we learned about ions in solutions.
- The formation of a solution depends on the ability of the solute to dissolve in the solvent. - Solvation is the interacting between solutes and solvent. - Ionic solds are crystals made up of ions (salts) - Molecular solids are crystals made up of neutral molecules.
- Dissolving ionic solutions produces ions in a process called dissociation Ex. NaCl(s) --(H2O)--> Na+(aq) + Cl-(aq) - Ionization is the break up of a neutral molecule into charged particles Ex. CH3COOH ----> CH3COO(-) + H(+)
- Determining concentrations is relatively easy. Ex. What is the [Cl-] in a solution of 0.50M AgCl3 ----> Ag+(aq) + 3Cl-(aq)
What is the [NO3-] in a solution of 0.82M Fe(NO3)2? Fe(NO)3 ----> 2Fe 2+(aq) + 2NO3-(aq) 0.83M --(X2)--> 1.64M
What is the [Cr2O7 2-] and [K+] when 3.5g is dissolved in 40mL of water? K2Cr2O7 ----> 2K(+) + Cr2O7(2-) 294.2g/mol 3.5g divided by 294.2g/mol = 0.0119mol divided by 0.04L = 0.297M
What is the [NO3-] when 100mL of 0.6M AgNO3 is mixed with 200mL of 0.40M Mg(NO3)2?" AgNo3 ----> A3(+) + NO3(-) 0.600M 0.600M 0.600M
Intermolecular Bonds -Bonds between molecules -3 types
1. London Dispersion Force (L.D.F)
Results from temporary electron dipoles (2 poles)
Weakest intermolecular force
Increases as # e- incrase
occurs in any compound that has e- (ie: everything)
2. Dipole-Dipole Force (D.D.F)
Results from a permanent dipole in molecules
POLAR molecules experience this force
Polarity depends on how much elements want e-. (electronegativity)
Electronegativity increases right and up
The strength of a dipole-dipole bond depends on the difference in electronegativity between the 2 atoms
F-O -> lower boiling point because less electronegativity, strength of 0.5, weaker bonds F-N -> higher boiling point because more elecronegativity, strength 1.0, stronger bonds
3. Hydrogen Bonds (H-Bonds)
This is a special type of dipole-dipole bond between H and O, F, or N
Any molecule that has stronger bond with larger electronegativity difference
