Orgo Unit 1

What are isotopes?

two atoms of the same element with different number of neutrons

What orbitals are core versus valence?

orbitals 1 and 2 are core, 3 are valence

Ionic ____ not bonding

association

Why do ions gain or lose electrons?

because they want to be a noble gas, gaining or losing electrons will make them more stable

How many bonds does H want?

1 bond

How many bonds does C want?

4 bonds

How many bonds does O want?

2 bonds

How many bonds does N want?

3 bonds

How many bonds (halides) F, Cl, Br, I want?

1 bond

What is formal charge?

when an atom deviates from normal behavior, the number of electrons different from their valence electrons ([total # of valence] - 1/2bonding + nonbonding)

What is a covalent bond?

when electrons are shared between two atoms

What is isomerism?

2 molecules that share 1 common trait but differ in other ways

What is a constitutional isomer?

molecules with the same molecular formula but different arrangments of atoms (C2H7N can be written different ways)

What is a resonance isomer?

molecules with the same constitution and arrangments of atoms, but different arrangements of electrons

What are the resonance rules?

all atoms except H follow octet rule, negatives prefer more electronegative atoms, positives prefer less electronegative atoms, electrons go from bond to atom or atom to bond not atom to atom

Organic structure follows VSEPR theory, what does this mean?

valence shell electron repulsion theory, it minimizes repulsions between atoms on the same molecule

What are areas of e density?

lone pair, single bond, double bond, triple bond, each of these are one area of e density

When a molecule has 2 areas of e density…

it is linear, at 180 degrees

When a molecule has 3 areas of e density…

it is trigonal planar, at 120 degrees

When a molecule has 4 areas of e density…

it is tetrahedral 109.5, 2 straight lines, 1 dotted line 1 thick line for going towards or away from you

How many different consitituional isomers does C9H12 have and how do you know?

it has a benzene ring so 3, bc 3 double and 3 single bonds that can change places

What kind of bonds are in a single, double, and triple?

A single bond has one sigma, a double bond has one sigma and one pi, a triple bond has one sigma and two pi

When are sigma bonds formed?

when orbitals overlap, and hybridized orbitals

When are pi bonds formed?

when there are unaccounted orbitals that need bonding, unhybridized orbitals

What do orbitals tell you?

the most probable location you can find electrons

How do you find hybridization of atoms?

look at electron configuration and see where valence electrons are, if 2 in s and 2 in p, s1p2 (since the orbital of s is full and there are 2 orbitals in p not full), this one will have an energy level in between s and p closer to p than s

What shape are s, p, and d orbitals?

sphere, dumbell, and tetrahedral dumbell

How to find n number?

this is the energy level (2p would be 2)

How to find l number?

s = 0, p = 1, d = 2, f = 3

How to find ml number?

this is the orbital number, s is 0, p can be -1,0,1, d can be -2,-1,0,1,2,

How do find ms number?

this is the spin of electron either +1/2 or -1/2

What does bond length and number have to do with bond strength?

Single bonds are often longest making them weakest, double bonds are in the middle making them second weakest, triple bonds are the shortest, making them strongest, triple bonds also have pi bonds making them reactive

What is a Bronsted-lowry acid?

a hydrogen or proton donor, has to have a hydrogen to give up

What is a Bronsted-lowry base?

a hydrogen or proton acceptor (taker)

What is a conjugate acid?

became an acid after reaction (has an H to give or e to accept)

What is a conjugate base?

became a base after reaction (has electron to give or H to accept)

Arrows always move from ___ to ____

negative to positive, a hydrogen will not take from a base

What is the most electronegative atom?

F

What is K?

equilibrium constant

What is ka and pka?

Ka shows [products/reactants] how good an acid is if ka is big the acid is big bc lots of products, pKa used to compare acids, close to 0 is strong acids, 5 is weak acids

Acids get weaker as molecules include atoms that get closer to ___

left

In an acid base reaction, equilibrium will favor side of reaction ___

with higher pKa (weaker acid), bigger arrow will point towards higher pKA because side with lower pka is better acid and will produce more products

How does the periodic table impact acid strength?

across a row left to right is increasing acidity because you are increasing electronegativity, in a column going up to down increases acidity because size of nuclei is bigger (lower electronegativity) and can give away H easier

How can hybridization impact acid strength?

most acidic hydrogen comes from the hybrid with the most s character (sp is more acidic than sp2)

How does the inductive effect impact acid strength?

through bond influence on hydrogen in molecule, more e negative has greater acidity influence (if the molecule has a very electronegative molecule its pulling electrons away from bond holding H, closer the electronegative molecule is to the H, the stronger the acid is)

How does the resonance effect impact acid strength?

a weaker conjugate base (more stable) corresponds to a stronger acid

What is a lewis acid?

an electron acceptor

What is a lewis base?

an electron doner

What is a nucleofile?

it donates a pair of electrons to form a new bond to a non-hydrogen atom in a reaction, a lewis base which must have a lone pair to donate

What is a functional group?

an atom or group of atoms with some type of characteristic or physical properties (reactive sites)

What is a heteroatoms?

anything that is not C or H, usually N, O, S, P, Cl, Br,, they are more electronegative than carbon which create partial positive charges on carbon (polarity)

What is an alkane?

a structure that only has C-C bonds

What is an alkene?

a structure that has one pi bond

What is an alykne?

a structure that has 1 triple bond

What is an aromatic?

it has a benzene ring, 6 carbons 3 single bonds 3 double bonds

What is a primary carbon?

a carbon that is only attached to one other carbon, symbol is circle and 1^0

What is a secondary carbon?

a carbon attached two 2 carbons, symbol is triangle

What is tertiary carbon?

a carbon attached to three carbons, symbol is square

What is a quaternary carbon?

a carbon attached to 4 carbons, has no hydrogens

When c-z and z is a halide what is it called?

an alkyl halide

When c-z and z is OH what is it called?

an alcohol

What number does Z typically take on?

usually the identity of the carbon it is attached too

When z-c and z = OR (r=carbon group), what is it called?

an ether

When z-c and z = n, what is it called?

an amine

When there is a c double bond o what is it called?

a carbonyl

When a C is attached to an H, double bond O, and R, what is it called?

aldehyde

When C is attached to double bond O and two R’s what is it called?

a ketone

When C is attached to an R, a double bond O, and an OH what is it called?

a carboxylic acid

When C is attached to double bond O, R, and NR what is it called?

an amide

When C is attached to R, double bond O, and OR what is it called?

an ester

When C is attached to double bond O, an R, and Cl what is it called?

an acid chlorine

When do van der walls/london dispursion forces occur?

in momentary electron distributions since electrons are always moving, if the molecule is bigger, this force will be greater since more surface area means more interactions

What is the weakest IMF?

van der walls/london dispursion forces, but it exists in every molecule

Between a molecule containing 10 carbons and one containing 3 carbons, which would have the higher boiling point when thinking about VDW/LDF?

10 carbon would have higher boiling/melting point, it would be harder to pull those molecules apart than the 3 carbon molecules because there are more interactions happening with the 10 carbon molecule

When do dipole dipole IMFs occur?

When you add N, O, halides to a molecule, this happens when partial charges are created in one molecule, other molecules near it will align themselves with the molecule so they’re oppisite charges will be near each other so things can be neutral

When does hydrogen bonding IMFs occur?

dipole dipole but when H is bonded to O or N, so in alcohols, carboxylic acids, amines, and amides

When people say “like dissolves like” what are they talking about?

When considering if something is soluble in something else, look at their IMFs. If they have the same IMFs it is likely that solubility will occur.