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OCHEM > Chapter 1 > Flashcards

Chapter 1 Flashcards

1
Q

Atoms are made up of _______, _______, _______

A

protons, neutrons, and electrons

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2
Q

each element is distnguished by the number of _______ in the nucleus = _______

A

protons, atomic number

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3
Q

electrons are found in _______, which are grouped into different _______ found at different distances from the nucleus

A

orbitals, shells

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4
Q

the most common _______ elements are found in the first __ rows of the period table: electrons are found in just the first __ electron shells

A

organic, 2, 2

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5
Q

The first shell (n=1) consists of just the 1s orbital and can hold ___ electrons

A

2

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6
Q

the second shell (n=2) consists of the 2s, 2px, 2py, 2pz orbitals and can hold __ electrons

A

8

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7
Q

What principle states that an electron will fill the lowest energy orbital first

A

Aufbau’s principle

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8
Q

In ionic bonding, electrons are _______ from one atom to another in an attempt to fulfill their _______. The resulting Ions have _______ charges, which _______ each other

A

transferred, octet, opposite, attract

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9
Q

in covalent bonding, electrons are _______ between atoms in an attempt to fulfill their octet

A

shared

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10
Q

Octet rule: atoms desire to have a filled shell of electrons. A _______ shell means 8 valence elections. (exception H and He want __)

A

full, 2

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11
Q

What are the common bonding patterns of H, C, N, O, and Cl (halogens)

A

H: one bond
C: 4 bonds
N: 3 bonds, 1 lone pair
O: 2 bonds, 2 lone pairs
Cl (halogens): 1 bond, 3 lone pairs

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12
Q

A bonding pair of e- is symbolized by a pair of _______ or _______

A

dots, dash

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13
Q

lone pairs are _______ e- that are not shared between 2 atoms

A

nonbonding

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14
Q

Nonpolar covalent bonds have electrons which are shared _______ between the 2 atoms

A

equally

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15
Q

Polar covalent bonds have bonding electron which are shared _______ between two atoms

A

unequally

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16
Q

Formal charge =

A

group # - (nonbonding e-) - (1/2 shared e-)
group # - bats - balls

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17
Q

Some organic compounds contain _______ bonds

A

ionic

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18
Q

Some organic compounds can be drawn either _______ or _______

A

covalently or ionically

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19
Q

resonance = movement of _______ only! _______ cannot be moved

A

electrons
atoms

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20
Q

The negative charge is _______ (spread out) over both O1 and O2 atoms. Spreading the negative charge over two atoms makes the ion ______ stable than it would be if localized in only one atom. This is known as _______

A

localized
more
resonance stabilization

21
Q

When can you draw resonance?

A

When an atom with a lone pair, positive charge, or negative charge is adjacent to a double or triple bond

*special: when atom with lone pair is next to atom with positive charge

22
Q

Resonance rules:
1) resonance forms must be valid _______ for the compound and follow the _______ rule
2) move only ______, never move atoms
3) all _______ must remain the same
4) single bonds are very _______ and are rarely involved in resonance
5) the major resonance contributor is the one with the _______ energy and follow most important to least important
a) _____ satisfied
b) _____ charges
c) negative charges prefer _____ atoms
6) EN atoms can hold a _______ charge only if they have octets
7) more resonance structures = _______ energy

A

1) lewis structures, octet
2) electrons
3) bond angles
4) stable
5) lower
a) octets
b) minimize
c) EN
6) positive
7) lower

23
Q

Condensed structural formula does not show all the individual _______

A

bonds

24
Q

in structural formula, _______, _______, _______ are shown and H is invisible unless bonded to an atoms that is shown.

A

N
O
halogens

25
Q

Atomic Orbitals can be described by its _______ which is the _______ description of the shape of the wave as it vibrates

A

wave function
mathematical

26
Q

the square of the wave function tells us where the _______ is the highest

A

electron density

27
Q

where is electron density highest for the s orbital

A

at the nucleus

28
Q

2p atomic orbitals have __ lobes which are _______ and are seperated by a _______

A

2
out of phase (- and +)
node

29
Q

the more nodes an orbital contains the _______ the energy

A

higher

30
Q

atomic orbitals can combine to generate new, more complex, orbitals in a process called _______

A

linear combination of atomic orbitals

31
Q

orbitals on _______ atoms interact to produce _______ that lead to bonding or antibonding interactions

A

different
molecular orbitals

32
Q

orbitals on the _______ atom interact to produce ______ orbitals that define the geometry of the bonds

A

same
hybrid atomic orbitals

33
Q

The stability of a covalent bond results from a large amount of electron density in the _______ region

A

bonding

34
Q

in the bonding region, electrons are shared between the atoms and are close to both nuclei’s creating _______

A

molecular orbital

35
Q

as 2 H’s with the same sign approach each other, their 1s orbital can add _______ to form a ______ bond

A

constructively
sigma

36
Q

all single bonds are sigma bonds, and every double or triple bond contains __ sigma bond

A

1

37
Q

all double bonds are pi bonds, and every triple bond contains __ pi bond

A

2

38
Q

as 2 H’s with opposing signs approach each other, their 1s orbital can add _______ to form a ______ bond. The result is a _______ separating the 2 atoms

A

destructively
anti-bonding
node

39
Q

Bonding MO have _______ energy compared to anti-bonding

A

lower

40
Q

if electrons are found in the _______ MO the molecule likely won’t exist

A

anti-bonding

41
Q

a pi bond result from the overlap between two p orbitals that are ________ to the line connecting the nuclei. This overlap is _______, not linear like a sigma bond

A

perpendicular
parallel

42
Q

Hybrid atomic orbitals: mixing of orbitals on the _______ atom. Their geometry accounts for the actual structures and _______ angles observed in organic compounds

A

same
bond

43
Q

electron pairs ______ each other and will adopt an arrangement that _______ repulsion

A

repel
minimizes

44
Q

When resonance is possible, the _______ hybridization option will be the truth

A

lower

45
Q

rotation about the _______ bond is allowed, but a _______ is rigid and cannot be twisted under normal conditions

A

single
double

46
Q

Rotation of a _______ bond usually represents the same compound. This is an example of _______ isomerism.

A

single
conformational

47
Q

Double bonds tend to be rigid, therefor the placement of the groups attached to the double bond matters and can result in_______ different compounds. what is an example?

A

two
cis and trans

48
Q

Constitutional (structural) isomers: _______ molecular formula, _______ connectivity. The number of isomers _______ rapidly as the number of carbon atoms increase

A

same
different
increases

49
Q

Stereoisomerisms: _______ molecular formula, ______ connectivity, _______ spatial orientation

A

same
same
different

OCHEM (12 decks)

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