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AP Chem > Unit 2 > Flashcards

Unit 2 Flashcards

(47 cards)

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1
Q

Bonds

A

Atoms bond in order to reach a stable 8 valence state

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2
Q

Ionic Bond

A

Electrostatic forces held together ions.

Generally between metals and nonmetals

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3
Q

Metallic Bond

A

Bons between metals that are neither covalent or ionic: the e- is delocalized so they are free to roam - like a soup

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4
Q

Covalent Bond

A

Sharing electrons and forming a molecule

generally non-metal and non-metal

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5
Q

Lattice

A

structure of a molecule

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6
Q

Network covalent bonds

A

Lattice of covalent bonds making a 3D structure

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7
Q

What are some characteristics of Ionic Bonds (3)

A
  1. Strong lattice structure
  2. Solid at room temp
  3. High melting and boiling points
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8
Q

What are some factors for melting points? (2)

A
  1. Greater charge = greater melting point
  2. Smaller size = greater melting point
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9
Q

What are some factors for bond energies? (3)

A
  1. Greater charge = greater bond energy
  2. Smaller size = greater bond energy
  3. More bonds = higher energy
    (Greater bond order)
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10
Q

What are some characteristics of metallic bonds? (2)

A
  1. malleable and ductile
  2. they can form alloys
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11
Q

Alloy

A

combination of elements where at least one is a metal

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12
Q

What are the two types of Alloys and explain

A
  1. Interstitial alloy - different radii sizes
  2. subsitual alloy - similar radii sizes
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13
Q

What are some characteristics of Network Covalent structures? (2)

A
  1. Hard
  2. High melting and boiling points
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14
Q

Aqueous

A

a substance put in H2O

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15
Q

Bond Order:

A

(total # of bonds)/(# of atoms)

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16
Q

What are the three rules to keep in mind when you draw Lewis Dot Structures?

A
  1. Least Electronegative = central atom
  2. Add extra e- till valence shells are finished
  3. Add extra e- to central atom
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17
Q

What is the maximum amount of e- the central atom can have?

A

No more than 12

They can take up to 12 due to the d-block

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18
Q

Resonance Forms

A

A bond can go anywhere - in reality, the e- is at all of those locations the equal amount of time

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19
Q

Incomplete Octets (2)

Study These Flashcards
A
  1. B and Al - stable with 6 e-
  2. H - stable with 2 e-
20
Q

Expanded octets

Study These Flashcards
A

there can be up to 12 e- ONLY AND ONLY IF
n = 3

NEVER
n = 2
n = 1

21
Q

Formal Charge

Study These Flashcards
A

(# of valence e-) - (# of valence e- assigned)

PER ATOM

22
Q

How do I know if an atom is stable?

Study These Flashcards
A

If the formal charge per atom is 0 or close to 0

23
Q

VSEPR

Study These Flashcards
A

Valence electron model that predicts the three dimensional geometry of the molecule

24
Q

For formal charge, a lone pair stands for

25
For formal charge, a covalent bond stands for
1 e-
26
Repulsion Model for bonds and e-
single < double < triple < lone
27
Metal characteristics (3)
1. Malleable 2. Great conductors 3. Solid at room temp
28
Non metals Characteristics
1. Bad conductors 2. gases at room temp
29
What are two components of bond energy?
1. Higher number of bonds - higher energy 2. smaller atoms - higher energy
30
Smaller atoms mean...
Smaller distance between atoms
31
According to the Coulomb's law, what type of atoms are harder to pull apart?
1. Smaller 2. More charge
32
What are the two types of covalent bonds?
1. pi 2. sigma
33
The first bond in a covalent is ALWAYS...
sigma everything else is pi
34
The more bonds, the higher the...
energy
35
If there are more than two structures having a -1 charge on either atom, how do you determine which is correct?
The more electronegative atom takes the -1 example obvi
36
In a VSEPR model, how do you determine the geometry of the atom as a whole?
1. determine the geometry of the central atom 2. Determine the molecular geometry of the molecule by ignoring any lone pairs on the central atom.
37
Dipole moment
measurement of polarity of two atoms
38
What is the equation for Dipole moment?
u = QD Q = magnitude of a charge in Coulombs D = magnitude of distance in Meters divide by 1 Debye
39
What is one Debye equal to?
3.34 X 10^-30 C . m
40
What is one electron equal to in Couloumbs
1.60 x 10^-19
41
Hybirdization
Since s and p (etc.) are in different energy states, we hybridize them
42
S character, P character is depended on...
the % of each of them
43
The more S character, the.....
smaller and tighter the bond
44
Steric Number calculation
(# of sigma bonds) + (# lone pairs) calculated on central atom
45
Steric Number calculates what?
the number of hybridized orbitals
46
What kind of bonds are not hybridized?
Pi bonds
47
Higher bond order means...
shorter bonds

AP Chem (11 decks)

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