Orgo chem 1:1

What is the significance of carbon in organic compounds?

Organic compounds contain carbon, which is essential for life.

Organic compounds

from living organisms (with a vital force)

inorganic compounds (without a vital force)

from minerals

what do organic compounds contain?

carbon

How to tell a compound is organic?

it’s covalent and has a carbon as the center bond

How to tell a compound is inorganic?

it’s ionic

what does carbon do in covalent bonds?

share electrons

What type of bond is formed when carbon shares electrons?

Covalent bond

What is the difference between organic and inorganic compounds?

Organic compounds contain carbon and are derived from living organisms, while inorganic compounds do not contain carbon and are derived from minerals.

isotope

elements with different molecular mass based off of different neutron numbers

what is called a proton even though it technically isn’t?

H^+

First shell contains:

s

Second shell contains:

s,p

third shell contains:

s,p,d

fourth shell contains:

s,p,d,f

which shell is closest to nucleus?

first: s

The closer the atomic orbital is to the nucleus______

the lower its energy

does s or p have a greater energy

p

difference between d and s block

d is 1 behind s

difference between f and s block

f is 2 behind s

aufbau principle

an electron goes into the atomic orbital with the lowest energy

put in order of lowest to greatest amount of energy: 2s,2p,1s,3s

1s<2s<2p<3s

electron configuration

up and down arrows for atomic orbitals

pauli exclusion principle

no more than two electrons can be in an atomic orbital

hund’s rule

an electron goes into an empty degenerate orbital rather than pairing up

what makes an atom stable?

outer shell is filled or has 6 electrons

electronegativity difference for nonpolar covalent bonds

<0.5

electronegativity difference for polar covalent bonds

0.5-1.9

electronegativity difference for ionic bonds

1.9<

dipole moment

size of charge x distance between charges

what does red electrostatic mean?

attracts positive charge/ it’s negative

what does blue electrostatic mean?

attracts negative charge/ it’s positive

formal charge

number of valence electrons - (number of lone-pair +number of bonds)

what happens if carbon doesn’t form 4 bonds?

has a charge or is a radical

radical

the atom has at least one unpaired valence electron in its outer shell

carbocation

positive charge carbon

carbanion

negative charge carbon

kekule’s structure

like lewis structure but without the lone pairs included

condensed structure

looks like the chemical formula

skeletal structures

show carbon-carbon bonds as lines [doesn’t show the carbons or hydrogens bonded to carbon}

atomic orbital

region of space around nucleus where electron is most likely to be found

smaller electron density is proportional_______

to a smaller orbital

electrons behave____

like a standing wave

lobes of p atomic orbitals have____

opposite phases

overlapping s bonds form:

sigma bond

waves can:

reinforce or cancel each other

atomic orbitals combine to form:

molecular orbitals

orbitals are

conserved

number of molecular orbitals is equal to

number of atomic orbitals combined

side to side overlap in In-plane p orbitals form a

pi bond

carbon has to promote _______ to form 4 bonds

electron

where does that one promoted electron go?

p orbital, removed from 2s

promotion of carbon causes:

4 orbitals to be hybridized

sp3 orbital has a

large and small lobe

cation usually indicates

acid

anion usually indicated

base

single bond

1 sigma

double bond

1 sigma, 1 pi

triple bond

1 sigma, 2 pi

electron geometry

tells you what type of hybridization it is

2 electron domains

sp

3 electron domains

sp2

4 electron domains

sp3

1 electron domain

s

What is hybridization in the context of atomic orbitals?

Hybridization is the promotion of an electron to form new hybrid orbitals for bonding.

What is the maximum number of electrons in the first shell of an atom?

2 electrons

What principle states that electrons occupy the lowest energy orbitals first?

Aufbau principle

What is the Pauli exclusion principle?

No more than two electrons can occupy the same atomic orbital, and they must have opposite spins.

What is a dipole moment?

A dipole moment is the measure of the separation of positive and negative charges in a molecule.

How does bond strength relate to bond length?

The more bonds holding two atoms together, the stronger and shorter the bond.

What is the relationship between electron density and bond strength?

The greater the electron density in the region of overlap, the stronger and shorter the bond.

What does sp3 hybridization indicate about bond angles?

Sp3 hybridization results in bond angles of approximately 109.5 degrees.

What is the significance of sigma (σ) and pi (π) bonds in double and triple bonds?

A double bond consists of one σ bond and one π bond, while a triple bond consists of one σ bond and two π bonds.

What is the effect of increasing s character in hybrid orbitals?

The more s character, the shorter and stronger the bond, and the larger the bond angle.

What is the definition of a cation?

A cation is a positively charged ion.

What is the definition of an anion?

An anion is a negatively charged ion.

What is the role of valence electrons in bonding?

Valence electrons are involved in forming bonds between atoms.

What is the significance of bond strength in molecular structures?

Stronger bonds contribute to the stability and structure of molecules.

What is the relationship between bond length and bond strength?

Bond strength decreases as bond length increases.

What does it mean for a molecule to be polar?

A polar molecule has an uneven distribution of charge, resulting in a dipole moment.

What is the definition of electronegativity?

Electronegativity is the ability of an atom to attract electrons in a bond.

How does the presence of lone pairs affect bond angles?

Lone pairs can reduce bond angles due to their repulsion on bonding pairs.

What is the significance of Kekulé structures?

Kekulé structures represent the arrangement of atoms in a molecule, often used for organic compounds.

What is the concept of resonance in chemistry?

Resonance describes the delocalization of electrons in molecules that can be represented by multiple structures.

What is the role of molecular orbitals in bonding?

Molecular orbitals are formed by the combination of atomic orbitals and determine the bonding characteristics of molecules.

The more bonds holding 2 atoms together

the stronger and shorter it is

The greater the electron density in the region of overlap

the stronger and shorter the bond

The more s character in the orbital

the stronger and shorter is the bond

bond strength___ as bond length____

increase, decrease

bond angle_____ as s character in the orbital ____

increase, increase

the ____ the bond, the _____ it is

shorter, stronger

The ______ the electron density in the region of orbital overlap, the _____ the bond

greater, stronger

The more s character, the ____ and _____ the bond

shorter, stronger

The more s character, the ___ the bond angle

larger

is a pi or sigma bond weaker?

pi

pi bond strength

strength of double bond- sigma bond

true or false: structure of molecule help determine if it’s dipole or not (same chemical formula)

true

the more bonds holding two atoms together, the ____ and ____ it is

stronger, shorter

the greater the electron density in the region of overlap, the ____ and ____ the bond

stronger, shorter

sp3 and no lone pair:

109.5