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CM133-1 Organic Chemistry 1 > Chemical Bonding and Molecular Structure > Flashcards

Chemical Bonding and Molecular Structure Flashcards

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1
Q

What are the physical properties used to replace damaged tissue?

A

strength, durability, polarity

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2
Q

this is the nature of electrical charges on surfaces

A

polarity

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3
Q

this is the ability of material to interact biologically without triggering an immune response

A

biocompatibility

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4
Q

the greater the difference in metallic/nonmetallic properties, the more likely it is a compound will be ___

A

ionic

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4
Q

this is formed by the electrostatic attraction of oppositely charged ions

A

ionic bond

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5
Q

Ionic compounds form __ and __.

A

metals and nonmetals

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6
Q

In the formation of cations with np6 electronic configuration, metals in the s and p blocks have __ ionization energies.

A

low

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7
Q

large jumps in ionization energy occur when ____ an electron from an np6 electronic configuration

A

removing

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8
Q

these are smaller than their corresponding neutral atoms

A

cations

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9
Q

___ electrons reduces electron electron repulsion

A

losing

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10
Q

remaining electrons are ____ bound to the nucleus

A

more tightly

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11
Q

these can form cations with more than one possible charge

A

transition metals

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12
Q

they first lose electrons from the s subshell

A

transition metals

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13
Q

common example of ions that are stable

A

Fe^2+ and Fe^3+

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14
Q

in the formation of anions with an np6 electronic configuration, ___ have negative electron affinities

A

nonmetals

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15
Q

these are larger than their corresponding neutral atoms

A

anions

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16
Q

___ electrons increases electron electron repulsion

A

gaining

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17
Q

valence electrons are _____ bound to the nucleus

A

less tightly

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18
Q

________ increases from left to right across a period

A

number of protons

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19
Q

____ decrease in size from left to right across the periodic table

A

cations and anions

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20
Q

____ are held more tightly from left to right across a period, resulting in smaller ions

A

electrons

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21
Q

energy input to form the cation is _____ by energy released by forming the anion.

A

not offset

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21
Q

electron affinites for nonmetals are _____

A

negative

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21
Q

forming an ionic bond between a ___ and ___ usually required energy

A

metal and nonmetal

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22
Q

ionization energies are _____

A

positive

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23
Q

once an ion pair is formed, _________ between the ions significantly lowers overall energy

A

electrostatic force of attraction

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24
Q

in formation of ions, what is the formula for Force? (coulomb’s law)

A

F=q1*q2/r^2

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25
Q

using potential energy (V), the ion pair can be calculated with what formula?

A

V = k(q1q2/r)

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26
Q

what is the value or k in V = k(q1q2/r)

A

1.389x10^5 kJ pm/mol

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27
Q

in ionic solids, the ions are arranged in a ____

A

crystal lattice

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28
Q

strength of interaction ____ with distances

A

decreases

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28
Q

Ions experience attractive and repulsive interactions in _______

A

three dimensions

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28
Q

is the overall result of the attractive and repulsive forces a crystal contains

A

lattice energy

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29
Q

form ionic compounds with
small lattice energies.

A

Large ions with small charges

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29
Q

is based on the sharing of pairs of electrons between two atoms.

A

covalent bond

29
Q

form ionic compounds with
large lattice energies.

A

Small ions with large charges

30
Q

what is the Driving force behind bond formation?

A

lowering of overall energy.

31
Q

_______ lowers energy by transferring electrons between a metal and a nonmetal.

A

Ionic bonding

32
Q

Electrons on each atom are ______ to the nucleus of the other atom

A

attracted

32
Q

lowers energy by sharing electrons
between two nonmetals.

A

Covalent bonding

33
Q

forms where the attractive and repulsive forces balance each other and energy is at a minimum.

A

covalent bond

33
Q

Nuclei of the bonding atoms _____ each other, as do the bonding
electrons.

A

repel

34
Q

energy released when isolated atoms form a covalent bond.

A

Bond energy

35
Q

vary depending on the bonding atoms involved.

A

bond energies

35
Q

an atom will form covalent bonds to achieve a complement of eight valence electrons

A

octet rule

35
Q

the distance between the nuclei of the bonding atoms where the potential energy is a minimum.

A

Bond length

35
Q

Formation of bonds always releases _______

A

energy

36
Q

Once a bond is formed, the same amount of energy. what is this energy?

A

bond energy

37
Q

are u happy

A

no

38
Q

The valence shell electronic configuration is ______ for a
total of eight electrons.

A

ns2np6

39
Q

these keep track of valence electrons, especially for main group elements, allowing prediction of
bonding in molecules

A

lewis dot symbols

40
Q

it shows how electrons are shared in a molecule

A

Lewis dot Structures

41
Q

lagi

A

lagi

42
Q

pairs of electrons associated with one atom are called ______

A

nonbonding or lone pair electrons

43
Q

A pair of shared electrons between two atoms is called

A

bonding pair

44
Q

this bond results when two bonding pairs are shared

A

double bond

45
Q

this bond results when three bonding pairs are shared

A

triple bond

46
Q

Strength of the covalent bond increases as the ____ increases

A

number of bonding pairs

47
Q

the attraction of an atom for the shared electrons in a covalent bond

A

electronegativity

48
Q

Electronegativities increase from _____ across a period
and from ______ for a group

A

left to right, bottom to top

48
Q

this element is the most electronegative element, with how much electronegativity?

A

Fluorine, 4.0

48
Q

is not shared equally when elements with
different electronegativities bond

A

Electron density

49
Q

The more electronegative element experiences an increase in electron density and attains a ________

A

partial negative charge

50
Q

The less electronegative element experiences a decrease in electron density and attains a ________

A

partial positive charge

51
Q

The two points of positive and negative charge constitute
a _____

A

dipole

52
Q

A bond along which a dipole exists

A

polar bond

53
Q

polar bond is also called

A

polar covalent bond

54
Q

The greater the electronegativity difference, the ____ polar bond

A

more

55
Q

When the electronegativity difference is zero, the bond is
classified as

A

nonpolar covalent

56
Q

When the electronegativity difference exceeds 2.0, the bond
is classified as

A

ionic

57
Q

indicate how many bonds are formed and between which elements in a compound

A

lewis structures

58
Q

this structures can be drawn when the choice of multiple bond location is arbitrary.

A

resonance structures

59
Q

in resonance structures, position of all atoms are _____; only the positions of the electrons are different

A

identical

60
Q

this indicates the structures are resonance structures.

A

double arrow

61
Q

is the result of constructive interference for end-to-end overlap, where electron density lies along a line between the bonding atoms.

A

sigma bond

62
Q

is the result of constructive interference for side- to-side overlap, where electron density lies above and below, or in front and in back of a line between the bonding atoms

A

pi bond

63
Q

reconciles the notion of orbital overlap with observations of molecular shapes and structures

A

Orbital Hybridization

64
Q

is the way bonded atoms arrange themselves in three dimensions

A

molecular shape

65
Q

in this theory, molecules assume a shape that allows them to minimize the repulsions between electron pairs in the valence shell of the
central atom

A

valence shell electron pair repulsion (VSEPR)

66
Q

what is the angle of linear and number of electron pairs?

A

180, 2 electron pairs

67
Q

what is the angle of trigonal planar and number of electron pairs?

A

120, 3 electron pairs

68
Q

what is the angle of tetrahedral and number of electron pairs?

A

109.5, 4 electrons pairs

69
Q

what is the angle of trigonal bipyramidal and number of electron pairs?

A

120 or 90, 5 electron pairs

70
Q

what is the angle of octahedral and number of electron pairs?

A

90 or 180, 6 electron pairs

71
Q

these may offer a promising route for drug delivery, since they can deliver drugs to a targeted location and thus avoid side effects from affecting non-targeted organs.

A

Mesoporous silica nanoparticles

CM133-1 Organic Chemistry 1 (6 decks)

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