Organic Chemistry - Structure And Bonding

Front 1

orbitals

Back 1

describe the volume of space around the nucleus that an electron is most likely to occupy

Front 2

shells

Back 2

the different layers of orbitals, each orbital ina shell can be occupied by two electrons

Front 3

ground state electron configuration

Back 3

listing of the orbitals occupied by its electrons

Front 4

statin

Back 4

drugs that reduce the risk for coronary heart disease by stopping the biosynthesis of cholesterol in the blood (Lipitor is an example, among the most widely prescribed drugs in the world)

Front 5

What distinguishes organic chemistry from inorganic chemistry?

Back 5

The presence of carbon

Front 6

Why is carbon in 99% of chemical compounds?

Back 6

1. Because it can form four bonds

2. Because it has a strong bond with other elements

3. Carbon has the ability to form longs chains and rings

Front 7

covalent bonds

Back 7

bonds with shared electron pairs between elements

Front 8

an atom consists of ___ surrounded by ___

Back 8

a dense positively charged nucleus, negatively charged electrons

Front 9

the nucleus consists of ___ and ____

Back 9

neutrons (electrically neutral) and protons (positively charged)

Front 10

the number of ___ and ___ in an atom are the same, making the atom ___

Back 10

protons and electrons, neutral

Front 11

The nucleus contains all of the ____ of the atom

Back 11

mass

Front 12

an atom is described by its ____ and its ___

Back 12

atomic number (number of protons), mass number (total number of protons plus neutrons in the nucleus)

Front 13

all atoms of a given element have the same ___, but can have different ___

Back 13

atomic number, mass number (protons are always the same, but neutrons can vary)

Front 14

atoms with the same atomic number but different mass numbers?

Back 14

isotopes

Front 15

how are the behavior of electrons in an atom described?

Back 15

wave equation

Front 16

what is the solution to a wave equation?

Back 16

wave function (orbital)

Front 17

the orbital describes the ___

Back 17

volume of space around the nucleus that the electrons occupy

Front 18

what are the four orbital types and the most common two used in organic and biological chemistry

Back 18

s,p,d,f

s and p

Front 19

An s orbital is ____ with the nucleus at the ___

Back 19

spherical, center

Front 20

A p orbital is ___ shaped

Back 20

dumbbell

Front 21

The orbitals in an atom are organize into layers or ____

Back 21

electron shells

Front 22

1st shell

Back 22

1s (2 electrons)

Front 23

2nd shell

Back 23

1 2s, 3 2p (8 electrons)

Front 24

3rd shell

Back 24

1 3s, 3 3p, 5 3d (18 electrons)

Front 25

What are the 3 rules for predicting the ground state electron configuration?

Back 25

1. The lowest energy orbitals fill up first (1s ->2s -> 2p -> 3s -> 3p -> 4s -> 3d)

2. Only two electrons can occupy and orbital and they must be of opposite spin (denoted as up and down)

3. If two or more empty orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half-full (1s ^ 2, 2s ^ 2, 2px ^1, 2py ^1)

Front 26

tetravalent

Back 26

it always forms four bonds when it joins to other elements to form stable compounds (carbon)

Front 27

carbon can form ___, ____ and ___ bonds

Back 27

single double and triple

Front 28

what shape does carbon and the four atoms to which they are bonded take?

Back 28

tetrahedron

Front 29

why do atoms bond together to form compounds?

Back 29

the compound is more stable and lower in energy than the separate atoms, energy generally is released and flows out a chemical system when a chemical bond forms.

Front 30

Making bonds ____ energy, breaking bonds ___ energy

Back 30

releases, absorbs energy

Front 31

valence shell

Back 31

the atoms outermost shell

Front 32

noble gas

Back 32

group 18 or the rightmost column of the periodic table (odorless, colorless, and have very low chemical re-activity)

Front 33

ionic vs. covalent bond

Back 33

covalent bonds are pairs of electrons shared by two atoms and take a lot of energy to break (between two non-metals, liquid or gaseous at room temperature), ionic bonds occur when atoms differ in electronegativity and one of the atoms loses an electron to the other causing one to become a cation and one to become an anion (between a metal and a non-metal, solid at room temperature)

Front 34

cation

Back 34

positively charged ion

Front 35

anion

Back 35

negatively charged ion

Front 36

carbon molecules form ___ bonds

Back 36

covalent

Front 37

what are lewis structures or electron dot structures?

Back 37

a way to represent the covalent bonds between atoms in a molecule

Front 38

what is a kekule or line-bond structure?

Back 38

Covalent are represented as a single line (instead of two dots like lewis structure)

Front 39

lone pair electrons or non-bonding electrons

Back 39

electrons that are not available for bonding (they already are in a pair)

Front 40

valence bond theory

Back 40

a covalent bond forms when two atoms approach each other closely and a singly occupied orbital on one atom overlaps a singly occupied orbital on the other atom. The electrons are paired in the overlapping orbitals and are attracted to the nuclei of both atoms, thus bonding them together

Front 41

bond strength

Back 41

the amount of energy it would take to break the bond

Front 42

bond length

Back 42

the optimal distance between nuclei that leads to maximum stability

Front 43

What does the superscript in sp3 stand for?

Back 43

How many of each type of atomic orbital combine to form the hybrid.

Front 44

What is hybridization?

Back 44

The process of different types of orbitals (for example s and p) combining to create a new type of orbital and allow bonds like carbon with hydrogen to form. (sp3 bonds with each s orbital in hydrogen to create four identical bonds)

Front 45

bond angle

Back 45

what angle is formed between each bond

Front 46

sigma bond

Back 46

bonds that are formed by the head on overlap of two atomic orbitals, making them cylindrically symetrical

Front 47

sp2 hybrid orbitals

Back 47

2s orbital combines with two of the 2p oribtals to create three sp2 hybrid orbitals an done 2p orbital remains unchanged. The three hybrid orbitals are in a plane with 120 degrees between them, and the 2p orbital is perpendicular to that.

Front 48

What happens when two sp2-hybridized carbon atoms approach eachother?

Back 48

They form a sigma bond by sp2-sp2 overlap, at the same time the two 2p unhybridized orbitals come in for a sideways overlap, resulting in a pi bond. The combination of these two bonds forms a carbon double bond.

Front 49

is a single or double carbon bond stronger and why?

Back 49

double, because it has four electrons bonding to the nuclei instead of two

Front 50

single carbon bonds are ____ hybridized

Back 50

sp3

Front 51

double carbon bonds are ___ hybridized

Back 51

sp2

Front 52

what is the angle between the four carbon hydrogen single bonds in ethane? Why?

Back 52

109.5, because each of the bonds has an electron and this allows them each to be as far apart as possible from eachother since they will repel eachother

Front 53

Bond angle in a carbon-carbon double bond?

Back 53

120

Front 54

the triple carbon-carbon bond is the ___ and ___ of all of the bonds

Back 54

shortest and strongest

Front 55

single carbon bonds form ___ shaped molecules, double carbon bonds form ____ molecules, triple carbon bonds form ___ molecules

Back 55

tetrahedral, planar, linear

Front 56

what is stronger, a sigma or a pi bond

Back 56

sigma bond - head on, not sideways

Front 57

what other atoms can form sp3 hybrid orbitals?

Back 57

nitrogen, oxygen, phosphorus, sulfur

Front 58

molecular orbital theory

Back 58

covalent bonds formation that belongs to the entire molecule instead of each individual atom

Front 59

pi bonds combined with sigma bonds make the bond ___ and unable to ___

Back 59

stronger, rotate

Front 60

In the symmetrical covalent bond neither of the atoms involved in the bond will have any type of ____ because the electrons are shared ____

Back 60

partial charge, equally

Front 61

difference between a molecule and a compound

Back 61

a molecule is when two atoms bond together, a compound is a molecule that contains at least two different elements (H2) is a molecule, but not a compound