Chem 108A, Chapter 01., Structure & Bonding

Front 1

What's the name for Viagra?

Back 1

sildenafil

Front 2

Draw cholesterol

Back 2

Front 3

When did organic chemistry originate?

Back 3

Mid-1700s

Front 4

Who was the first chemist to distinguish between organic and inorganic?

Back 4

Torbern Bergman in 1770

Front 5

vitalistic theory

Back 5

An incorrect idea that organic substances contained a "vital force" that resulted from their living origins. It was thus believed that organic compounds could not be synthesized

Front 6

Draw the structure for urea:

Back 6

Front 7

What is the distinguishing feature of organic chemistry?

Back 7

That organic chemicals all contain carbon.

Front 8

Of the ~ 30 million known compounds, how many of them contain carbon?

Back 8

~99%

Front 9

picometer (pm)

Back 9

1×10^−12 m

Front 10

angstrom (Å)

Back 10

Often used in expressions of atomic distance; internationally recognized unit of length equal to 0.1 nanometre or 1×10^−10 metres

Front 11

atomic number

Back 11

number of protons in an atom

Front 12

mass number

Back 12

protons + neutrons

Front 13

isotope

Back 13

atoms with the same atomic number but a differing mass number

Front 14

amu

Back 14

atomic mass units; used to express atomic and molecular masses.

Front 15

atomic mass/weight

Back 15

the weighted average mass in amu of an element's naturally occurring isotopes

Front 16

What's the atomic mass of hydrogen?

Back 16

1.008

Front 17

What's the atomic mass of carbon?

Back 17

12.011

Front 18

What's the atomic mass of phosphorous?

Back 18

30.974

Front 19

ψ

Back 19

psi

Front 20

Draw an s orbital

Back 20

Front 21

Draw a p orbital

Back 21

Front 22

Draw a d orbital

Back 22

Front 23

electron shells

Back 23

orbital layers of successively larger size and energy

Front 24

What's the capacity of the first electron shell?

Back 24

2 electrons

1s

Front 25

What's the capacity of the second electron shell?

Back 25

8 electrons

1s2s2p

Front 26

What's the capacity of the third electron shell?

Back 26

18 electrons

1s2s2p3s3p3d

Front 27

How are the electrons of each orbital represented?

Back 27

Up and down arrows

Front 28

How are the three different p orbitals written?

Back 28

Front 29

node

Back 29

the area between orbitals containing zero electron density

Front 30

Draw a 2px orbital

Back 30

Front 31

Draw a 2py orbital

Back 31

Front 32

Draw a 2pz orbital

Back 32

Front 33

ground-state electron configuration

Back 33

the lowest energy arrangement of an atom

Front 34

aufbau principle

Back 34

lowest energy orbitals fill up first

1s --> 2s --> 2p --> 3s --> 3p --> 4s --> 3d

Front 35

Pauli exclusion principle

Back 35

Only two electrons can occupy an orbital

Front 36

Hund's rule

Back 36

If two or more empty orbitals of equal energy are available, one electron occupies each with spins parallel until all orbitals are half-full

Front 37

What is carbon's ground state configuration?

Back 37

Front 38

Draw out the ground state configuration of phosphorous

Back 38

Front 39

tetravalent

Back 39

forms four bonds (e.g., carbon)

Front 40

Does making bonds release or absorb energy?

Back 40

release

Front 41

Does breaking bonds release or absorb energy?

Back 41

absorbs

Front 42

valence shell

Back 42

the outermost shell

Front 43

ionic bonds are caused by?

Back 43

electrostatic attraction

Front 44

molecule

Back 44

the neutral collection of atoms held together by covalent bonds

Front 45

Lewis structure

Back 45

electron-dot structure

Front 46

Kekule structures

Back 46

line-bond structure

Front 47

What's the formula for ammonia?

Back 47

NH3

Front 48

What's the formula for methanol?

Back 48

CH3OH

Front 49

lone pair electrons

Back 49

valence electrons not used for bonding

Front 50

What's the formula for chloroform?

Back 50

CHCl3

Front 51

valence bond theory

Back 51

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

Front 52

σ

Back 52

sigma

Front 53

sigma (σ) bond

Back 53

bond formed by the head-on overlap of two atomic orbitals

Front 54

bond length

Back 54

the optimum distance between nuclei, where atoms are neither repelled due to proximity or are too far apart to bond

Front 55

Draw four sp^3 orbitals

Back 55

Front 56

Draw an sp^3-sp^3 alpha bond

Back 56

Front 57

What's the formula for ethylene?

Back 57

C2H4

Front 58

pi bond

Back 58

covalent chemical bonds where two lobes of one involved electron orbital overlap two lobes of the other involved electron orbital.

Front 59

What's the formula for formaldehyde?

Back 59

CH2O

Front 60

organophosphate

Back 60

compound that contains a phosphorous atom bonded to four oxygens, with one of the oxygens also bonded to a carbon

Front 61

sulfide

Back 61

compounds which have a sulfur atom bonded to two carbons

Front 62

thiol

Back 62

sulfur atom bonded to one hydrogen and one carbon

Front 63

condensed structures

Back 63

structures drawn where the bonds aren't shown.
e.g. CH3CH2CH3

Front 64

skeletal structures

Back 64

where carbon and hydrogen symbols are omitted and bonds are drawn as lines

Front 65

hyponatremia

Back 65

an electrolyte disturbance in which the sodium concentration in the serum is lower than normal

can be lethal

Front 66

sp^3 is caused by ______ bonds

Back 66

single

Front 67

sp^2 is caused by ______ bonds

Back 67

double

Front 68

sp is caused by ______ bonds

Back 68

triple

Front 69

Vitamin C is also called:

Back 69

ascorbic acid

Front 70

Are vitamin C and citric acid the same thing?

Back 70

No@

Front 71

NutraSweet is?

Back 71

aspartame

Front 72

How many valence electrons in iron?

Back 72

2 (in 4s subshell), 6 (in 3d subshell)

Front 73

At what angles are the bonded carbons of a benzene ring?

Back 73

120 degree

Front 74

Advil is made from?

Back 74

ibuprofen

Front 75

Tylenol is made from?

Back 75

acetaminophen

Front 76

Aleve is made from?

Back 76

naproxen

Front 77

In a solid line structure, a dashed bond represents:

Back 77

The bond pointing towards the viewer.

Front 78

In a solid line structure, a wedged bond represents:

Back 78

The bond pointing away toward the viewer.

Front 79

What's the bond angle?

Back 79

Front 80

How will a carbon structure with a triple bond orient itself?

Back 80

In a straight line

-C:::C-

Front 81

carbocation

Back 81

an ion with a positively-charged carbon atom

Front 82

A positively charged carbon is ____ hybridized

Back 82

sp2

Front 83

carbanion

Back 83

an anion in which carbon has an unshared pair of electrons and bears a negative charge usually with three substituents for a total of eight valence electrons

Front 84

isoelectric

Back 84

having the same number of electrons

Front 85

carbene

Back 85

a molecule containing a neutral carbon atom with a valence of two and two unshared valence electrons. The general formula is RR'C:

Front 86

A carbanion is _______ hybridized

Back 86

sp3

Front 87

Draw a single and a triple methylene.

Back 87