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Chemistry 1b > Chapter 9 > Flashcards

Chapter 9 Flashcards

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1
Q

__________ __________ predict chemical bonding in nature.

A

Lewis structures

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2
Q

Step 1 for writing a Lewis structure for a molecular compound:

A
  1. Write the correct skeletal structure for the molecule
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3
Q

Step 2 for writing a Lewis structure for a molecular compound:

A
  1. Calculate the total # of electrons for the Lewis structure by summing the valence electrons of each atom in the molecule.
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4
Q

Step 3 for writing a Lewis structure for a molecular compound:

A

Distribute the electrons among the atoms, giving octets to as many atoms as possible.

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5
Q

Step 4 for writing a Lewis structure for a molecular compound:

A

If any atoms lack an octet, form double or triple bonds as necessary to give them octets.

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6
Q

“At the ends”.

A

Terminal

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7
Q

The only way to determine the skeletal structure of a molecule with absolute certainty is to __________ _____ _________ ________.

A

Examine it’s structure experimentally

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8
Q

__________ atoms are always terminal.

A

Hydrogen

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9
Q

__________ atoms must form at least two bonds.

A

Central

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10
Q

Put the more __________ __________ in terminal positions.

A

Electronegative elements

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11
Q

Put the __________ electronegative elements (other than hydrogen) in the central position.

A

Less

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12
Q

If you are writing a Lewis structure for a __________ _____, the charge of the ion must be considered when calculating the total # of electrons.

A

Polyatomic ion

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13
Q

_____ one electron for each negative charge.

A

Add

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14
Q

__________ one electron for each positive charge.

A

Subtract

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15
Q

The Lewis structure for a __________ _____ is usually written within brackets.

A

Polyatomic ion

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16
Q

For the polyatomic ion NH(subscript 4)^+ , there are 9 electrons. Would you add an electron to make the total 10, or subtract and make it 8?

A

Subtract and make it 8

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17
Q

This is used when two or more valid Lewis structures can be drawn for the same compound.

A

Resonance

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18
Q

An electron book-keeping system that allows us to discriminate between alternative Lewis structures.

A

Formal charge

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19
Q

Where there are two or more valid Lewis structures for the same molecule, we find that, in nature, the molecule exists as an _________ of the structures.

A

Average

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20
Q

Two or more valid Lewis structures that are shown with double-headed arrows between them to indicate that the actual structure of the molecule is intermediate between them:

A

Resonance structures

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21
Q

The actual structure of a molecule that is intermediate between two or more resonance structures:

A

Resonance hybrid

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22
Q

The only structure that actually exists is the __________ structure-the individual resonance structures do not exist and are merely a convenient way to describe the actual structure.

A

Hybrid

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23
Q

The concept of __________ is an adaptation of Lewis theory that helps account for the complexity of actual molecules.

A

Resonance

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24
Q

In Lewis theory, electrons are ________ either on one atom or between atoms.

A

Localized

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25
Q

The _________ of electrons lowers their energy; it stabilizes them.

A

Delocalization

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26
Q

__________ __________ is a fictitious charge assigned to each atom in a Lewis structure that helps us to distinguish among competing Lewis structures.

A

Formal charge

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27
Q

The charge that an atom would have if all bonding electrons were shared equally between the bonded atoms.

A

Formal charge

28
Q

The calculated charge for an atom if we completely ignore the effects of electronegativity.

A

Formal charge

29
Q

Formal charge =

A

(# of valence electrons) - [# of nonbonding electrons for element +1/2(number of bonding electrons)]

30
Q

The sum of all formal charges in a neutral molecule must be _____.

A

Zero

31
Q

The sum of all formal charges in an ion must equal _______.

A

The charge of the ion

32
Q

Small (or zero) formal charges on individual atoms are __________ than large ones.

A

Better

33
Q

When formal charge cannot be avoided, negative formal charge should reside on the __________ __________ atom.

A

Most electronegative

34
Q

A technique in which X-rays are scattered from crystals of the molecule of interest.

A

X-ray crystallography

35
Q

In 1989, researchers used X-ray crystallography to determine the structure of a molecule called what?

A

HIV-protease

36
Q

Without HIV-protease, HIV cannot spread in the human body because the virus cannot __________.

A

Replicate

37
Q

The working part of a molecule.

A

The active site

38
Q

Models that predict how atoms bond together to form molecules.

A

Bonding theories

39
Q

Many AIDS patients are still alive today because of:

A

Protease inhibitors

40
Q

Without chemical bonding, there would be only how many different kinds of substance?

A

91 (# of elements on the periodic table)

41
Q

Chemical bonds form because they lower the __________ __________ between the charged particles that compose atoms.

A

Potential energy

42
Q

If atomic/electron interactions result in an overall net reduction of energy between charged particles, what forms?

A

A chemical bond

43
Q

Metals tend to have low:

A

Ionization energies

44
Q

Nonmetals tend to have negative:

A

Electron affinities

45
Q

Nonmetals readily gain __________.

A

Electrons

46
Q

Nonmetals tend to have high:

A

Ionization energies

47
Q

Lowest potential energy = most __________.

A

Stable

48
Q

Since metals have low ionization energies, they tend to lose electrons __________.

A

Easily

49
Q

In the __________ __________ model, all of the atoms in a metallic lattice pool their valence electrons.

A

Electron sea model

50
Q

Lewis theory focuses on:

A

Valence electrons

51
Q

The easiest way to calculate lattice energy is with the:

A

Born-Haber cycle

52
Q

The magnitude of lattice energy __________ as we move down a column.

A

Decreases

53
Q

Lone pair electrons are also called:

A

Nonbonding electrons

54
Q

In general, double bonds are __________ and __________ than single bonds.

A

Shorter and stronger

55
Q

Triple bonds are even __________ and __________ than double bonds.

A

Shorter and stronger

56
Q

__________ bonds are directional.

A

Covalent

57
Q

The fundamental units of colvalently bonded compounds are __________ __________.

A

Individual molecules

58
Q

In covalently bonded molecular compounds, the interactions __________ molecules is much weaker than the bonding interactions __________ a molecule.

A

Between, within

59
Q

__________ compounds tend to have lower melting and boiling points than _________ compounds.

A

Molecular, ionic

60
Q

Intermediate in nature between a pure covalent bond and an ionic bond.

A

Polar covalent bond

61
Q

Having a positive pole and a negative pole.

A

Polar

62
Q

The ability of an atom to attract electrons to itself in a chemical bond (which results in polar and ionic bonds).

A

Electronegativity

63
Q

Elecgronegativity was quantified by American chemist:

A

Linus Pauling

64
Q

Energy required to break a bond.

A

Bond energy

65
Q

Electrons are shared equally and exactly.

A

Pure covalent bond

66
Q

Non-polar.

A

Purely covalent

Chemistry 1b (3 decks)

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