Organic Chemistry Chapter 1

Front 1

What is organic chemistry

Back 1

The chemistry of compounds that contain the element carbon

Front 2

What is a compound?

Back 2

It is made up of elements combined in different proportions.

Front 3

Elements are made up of

Back 3

Atoms

Front 4

Atoms are made up of

Back 4

a dense, positively charged nucleus containing protons and neutrons and are surrounded by a cloud of electrons.

Front 5

The mass of an atom is made up by what

Back 5

Neutrons and Protons which have nearly the same mass of 1 atomic mass unit each. They are 1800 times as heavy as an electron

Front 6

What makes up most of the volume of an atom?

Back 6

The volume occupied by the electrons is 10,000 times larger than that of the nucleus.

Front 7

The atomic number (Z) above the element is

Back 7

equal to the number of protons in its nucleus and number of electons surrounding it's nucles.

Front 8

What are isotopes

Back 8

Atoms of the same element that have different masses because they have different number of neutrons.

Front 9

How many electrons does an atom have in its valence shell?

Back 9

We look at the periodic table, the number of electons in the valence shell is equal to the group number of the atom.

Front 10

What are isomers?

Back 10

Different compounds that have the same molecular formula

Front 11

What kind of bonds can the following atoms make what type of fixed number of bonds:
Carbon
Oxygen
Hydrogen and halogen atoms

Back 11

Carbon is tetravalent, 4 bonds
Oxygen is divalent, 2 bonds
Hydrogen and Halogen atoms are monovalent and can make 1 bond.

Front 12

What are constitutional isomers, how doe they differ

Back 12

different compounds with the same molecular formula but differ in the sequence in which their atoms are bonded, that is in their connectivity. ( They differ in their melting point, boiling point and density) and they have different chemical properties (reactivity).

Front 13

What are the two major types of chemical bonds? define them.

Back 13

Ionic (or electrovalent) bonds are formed by the transfer of one or more electrons from one atom to another to create ions.
Covalent bonds result when atoms share electrons.

Front 14

Atoms that gain or lose electrons and form charged particles are called

Back 14

Ions

Front 15

An ionic bond is:

Back 15

an attractive force between oppositely charged ions, one source of such ions is a reaction between atoms of widely differing electronegativety.

Front 16

what is electronegativity?

Back 16

a measure of the ability of an atom to attract electrons. It increases as we go across a horizontal row of the PT from left to right and as we go up a verticle column

Front 17

How to salts form?

Back 17

Salts form only when atoms of very different electronegativities transfer electrons to become ions

Front 18

how do covalent bonds form, what happens to the atoms?

Back 18

Covalent bonds form by sharing of electrons between atoms of similar electronegativities to achieve the configuration of a noble gas.

Front 19

What is composed of atoms joined exclusevely or predominantly be covalent bonds?

Back 19

Molecules.

Front 20

How do you calculate "Formal Charge"

Back 20

F = Z - (1/2)S - U
Valence - a (1/2) shared - unshared

Front 21

Resonance theory states that:

Back 21

whenever a molecule or ion can be represented by two or more lewis structures, none of these structures is a realistic representation of the molecule or ion. Instead, the actual molecule or ion will be better represented by a hybrid (average) of these structures.

Front 22

What is the difference between resonance and equilibrium?

Back 22

Resonance is represented by a two arrows, resonance by a two sided arrow indicating that it only exists on paper while equilibrium is different structures moving ( or fluctuating) atoms. Resonance atoms do not move.

Front 23

Wave Function corresponds to

Back 23

a different energy state for an electron

Front 24

How can the energy associated with an electron be calculated?

Back 24

by its wavefunction

Front 25

the probability of finding an electron in a given region can be calculated by

Back 25

the wave function

Front 26

Occurs when wave functions with the same phase sign interact. There is a reinforcing effect and the amplitude of the wave function increases

Back 26

Constructive Interference

Front 27

Occurs when wave functions with opposite phase signs interact. There is a subtractive effect and the amplitude of the wave function goes to zero or changes sign

Back 27

What is Destructive interference

Front 28

Is a region of space where the probability of finding an electron is high

Back 28

What is the orbital

Front 29

are plots of (wavefunction square) in three demensions

Back 29

what are atomic orbitals

Front 30

which principle state that orbitals of lowest energy are filled first?

Back 30

Aufbau principle (german for "building up")

Front 31

Principle that states that a maximum of 2 electrons may be placed in each orbital but only when spins of the electrons are paired

Back 31

What is the Pauli exclusion principle

Front 32

Orbitals of equal energy such as the three 2p orbitals are called

Back 32

degenerate orbitals

Front 33

Rule that states that first you add electrons to degenerate orbitals with spins unpaired so that they have maximum separation, then you begin to add the second electron so the spins are paired

Back 33

What is Hund's rule

Front 34

principle that states that we cannot simultaneously know the position and momentum of an electron

Back 34

The Heisenberg uncertainty principle

Front 35

Represents the region of space where one or two electrons of an isolated atom are likely to be found

Back 35

atomic orbital

Front 36

Represents the region of space where one or two electrons of a molecule are likely to be found

Back 36

molecular orbital (MO)

Front 37

results when two orbitals of the same phase overlap

Back 37

what is a bonding molecular orbital

Front 38

results when two orbitals of opposite phase overlap

Back 38

what is antibonding molecular orbital

Front 39

All purely single bonds are

Back 39

sigma bonds

Front 40

All purely single bonds are

Back 40

sigma bonds

Front 41

Hydrocarbons whose molecules contain a carbon-carbon double bond are called

Back 41

alkenes. Ethene (C2H4) and propene (C3H6) are both alkenes.

Front 42

What is the region of space about the nucleus of a single atom with the high probability of finding an atom

Back 42

Atomic Orbital (AO)

Front 43

when Atomic Orbitals Overlap, they combine to form ...

Back 43

Molecular Orbitals

Front 44

Is the Energy of Electrons in the bonding molecular orbital has more or less energy than the energy of the electrons in their separate atomic orbitals

Back 44

less

Front 45

Is the Energy of Electrons in the anti-bonding molecular orbital has more or less energy than the energy of the electrons in their separate atomic orbitals

Back 45

more

Front 46

The number of molecular orbitals is equal to

Back 46

the number of atomic orbitals from which they are formed. Combining two atomic orbitals will always yield two molecular orbitals, one bonding and one anti-bonding

Front 47

Hybrid atomic orbitals are obtained by

Back 47

mixing (hybridizing) the wave functions for orbitals of different types (s & p orbitals) from the same atom

Front 48

True or False
Atoms joined by single bonds can rotate relatively freely with respect to one another

Back 48

True