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CHM 115 Blechle > E.4_ch.8.9_ > Flashcards

E.4_ch.8.9_ Flashcards

1
Q

What is a ionic bond?

A

electron transfer between metals and nonmetals

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2
Q

What is a covalent bond?

A

electron sharing between nonmetals

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3
Q

What is a metallic bond?

A

electron pooling between metals

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4
Q

What do Lewis Symbols help predict?
What does the symbol represent?
What does the dots represent?

A

bonding

nucleus and core electrons

valence electrons

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5
Q

What is the number of valence electrons on the periodic table?

A

the A group number

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6
Q

What do lewis symbols number of dots tell us?

A

for main group metals, they equal the number of electrons the atom loses to form a cation

for nonmetals, they equal the number of electrons the atom gains to form a anion

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7
Q

Who created the octet rule?

A

Gilbert Lewis (1916)

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8
Q

What is the octet rule?

A

bonded atoms either gain, lose, or share electrons to attain a filled outer layer of 8 e-

atoms like to achieve noble gas configurations

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9
Q

What does the octet rule apply to?

A

almost all compounds made of the period 2 elements and some others

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10
Q

Why do ionic bonds cause attraction between 2 atoms?

A

transfer of electrons = opposing charges

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11
Q

What is ionization energy?

A

The energy absorbed by 1 mole of an atom when it loses 1 mole of electrons

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12
Q

What is electron affinity?

A

The energy released by 1 mole of an atom when it gains 1 mole of electrons

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13
Q

What is a lattice?

A

The structure of a crystalline solid formed from the attraction of multiple ions

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14
Q

What is lattice energy?

A

The energy to separate 1 mole of a solid to form 1 mole of gaseous ions

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15
Q

What kind of energy to atoms want?

A

Energy kept to a minimum

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16
Q

What happens to the overall energy when ionic bonds form?

A

Energy is released

Overall energy lowers

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17
Q

What are the physical behavior of an ionic solid?

A

Ionic solid is hard, rigid, and brittle

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18
Q

What are the electrical conductivity of an ionic solid?

A

Ionic solid does not conduct electricity, but it does once melted or dissolved

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19
Q

What are the thermal conductivity of an ionic solid?

A

In the normal state, there is no such thing as an individual ionic molecules, just interconnected solids or arrays

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20
Q

What must we understand to understand why and how covalent bonds are formed?

A

Electro negativity

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21
Q

What is electronegativity not the same as ?

A

Electron affinity

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22
Q

Who discovered electronegativity?

A

Linus Pauling (1932)

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23
Q

What is electronegativity?

A

The relative ability of a bonded atom to attract shared electrons

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24
Q

What are electronegativity values relative to?

A

The greatest value of 4.0 which is fluorine

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25
Q

How is electronegativity related to size?

A

EN is inversely related to size

Smaller the atom … the closer the shared pair can get to the nucleus

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26
Q

Do electrons share equally when a covalent bond is formed?

A

No

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27
Q

What is a unequal sharing of electrons?

A

Polar covalent bond

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28
Q

What is an equal sharing of electrons?

A

No polar covalent bond

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29
Q

What is used to determine bond polarity ?

A

Electronegativity

30
Q

What sharing does two atoms of the same element form when bonded?

A

Equal sharing of electron

Non polar covalent bond

31
Q

What sharing does two atoms of different elements form when bonded?

A

Unequal sharing of electrons

Polar covalent bond

32
Q

What charge does the most electronegative element get? The least electronegative?

A

Most EN = partial negative charge

Least EN = partial positive charge

33
Q

What helps is determine bond polarity?

A

The difference in electronegativity between two bonded species

34
Q

Names the name— EN difference — bond type — example …

What’s the biggest difference in EN

A

Zero — (0-0.4) — polar covalent — Cl2

Intermediate — (0.4-2.0) — polar covalent — HF

Large — (2.0+) — ionic — NaCl

3.3

35
Q

What is the difference between bond polarity and molecular polarity?

A

Bond polarity: if bond is polar or not

Molecular polarity: if molecule is polar or not

36
Q

What do Lewis structures and Lewis symbols describe?

A

Lewis symbols : single atom

Lewis structures : molecules

37
Q

What is a Lewis structure an outline for?

A

Bonding and arrangement of atoms in a molecule

38
Q

What is a resonance structure?

A

The different Lewis model structures that can be made

39
Q

What are equivalent resonance structures and what are no equivalent resonance structures?

A

Equivalent resonance structures: mirrored

No equivalent resonance structures: not the same/mirrored

40
Q

What structure is the real molecule when choosing a where the double bond goes?

A

Hybrid

41
Q

How is the bonding order calculated?

A

Bond Order = Bonding pairs / Atom pairs

42
Q

How do we represent ions in a Lewis structure?

A

Braquets and charge outside top right corner

43
Q

When do we want to limit formal charges on Lewis structures?

A

When we have non equivalent resonance forms

44
Q

How do you calculate the formal charge?

A

FC= # valence e - # unshared e - (1/2)(# shared e)

45
Q

What do the FC added together equal?

A

The charge of the ion molecule

46
Q

What is the best resonance form ?

A

Limits formal charge
Places negative charge on the most EN atom
(Places positive charge on lease EN atom)

47
Q

What happens to the d(distance form nucleuses) and lattice energy as the size of ions increase?

A

d increases

LE decreases

48
Q

What two things can coulombs law predict?

A

strength of ionic bond

lattice energy

49
Q

What kinds of ions and charges do we want?

A

small ions
large charges

= high LE

50
Q

What is the equation for coulombs law?

A

E ∝ (q1q2)/d ∝ LE

51
Q

Do lewis structures tell us anything about the shape of the molecule?

A

no

52
Q

What are the five rules of lewis structures?

A

hydrogen can only form one bond and can never be a central atom no matter what EN

halogens generally form 1 bond and are generally surrounding atoms

carbon forms 4 bonds

nitrogen forms 3 bonds

oxygen forms 2 bonds

53
Q

What are the three ways an octet rule can disobey the octet rule ?

A

electron deficient atom

odd electron atom

atoms with expanded valence shells

54
Q

What are electron deficient atoms and what are examples?

A

these atoms often have fewer than 8 electrons around them when they are the central atom

Be and B

when not central is willing to follow octet rule after bond

55
Q

What are odd electron atoms and what is an example?

A

electrons don’t always come in pairs
leaves one electron by itself

NO2

56
Q

What is it called when one electron is left by itself on a lewis dot structure?

A

free radicals

57
Q

What are expanded valence atoms and what is an example?

A

atoms that expand their valance shells to beyond 8 electrons
period 3 or higher

sulfur

58
Q

Why can atoms in period 3 or higher bond more than 8 valance electrons?

A

it has 3d orbitals available to it

has 3s and 3p to place electrons

59
Q

Do lewis structures tell us anything about the arrangement of molecules in space?

A

no

60
Q

What do lewis structures tell us?

A

used to determine geometry

61
Q

What does molecular shape determine?

A

functionality

62
Q

What is electron group arrangement?`

A

the distribution of electrons (shared and unshared) around a central atom

63
Q

What is molecular geometry?

A

the distribution of the atoms in 3D space

64
Q

What do the following represent for drawing in three dimensions?

single lines
bold lines
dashed lines

A

bonds in the plane

bonds that are angled forward

bonds that are angled backward

65
Q

What does VSEPR stand for?

A

valence-shell electron-pair repulsion

66
Q

What is VSEPR?

A

the primary theory behind determining molecular geometry, based on 2 principles

67
Q

What are the two principles of the theory of VSEPR?

A

e pairs repel each other … occupy space farthest away from each other as possible

a bond is sharing electrons … unpaired electrons are more localized on a single atom

68
Q

How do we use VSEPR?

A
  1. determine the # of e- groups around central atom
  2. determine e- group arrangement
    ( identify optimal bond angles )
  3. consider lone pair repulsion impact on a bond angle
  4. determine molecular geometry
69
Q

True or False: double and triple bonds are considered a single e- group?

A

true

70
Q

In electron group arrangements, the total # of electron groups around a central atom can range from what?

Each e- group arrangement will provide us with various possible _______?

A

2-6

molecular geometries

71
Q

What electron group arrangement is when there are only two electron groups around a central atom?
What are the other possible geometries?

A

linear electrons group arrangement

linear is the only one possible

CHM 115 Blechle (8 decks)

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