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AP Chem > Unit 1 + 2 > Flashcards

Unit 1 + 2 Flashcards

(61 cards)

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1
Q

Hybrid SP bond angle

A

180

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2
Q

Hybrid SP2 bond angle

A

120

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3
Q

Hybrid SP3 bond angle

A

109.5

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4
Q

When does an atom have no net dipole?

A

When it is non-polar, molecule is symmetric

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5
Q

Sigma bonds

A

The first bond between atoms

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6
Q

Pi bonds

A

The second or third bond between atoms

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7
Q

Can hydrogen hybridize?

A

No because it does not have a P orbital

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8
Q

How do you determine the hybridization of an atom?

A

How many bonding sites there are
2 bonding sites = sp
3 bonding sites = sp2
4 bonding sites = sp3

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9
Q

tetrahedral

A

4 atoms bonded, no lone pairs on central atom, bond angle is 109.5

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10
Q

trigonal planar

A

3 atoms bonded, no lone pairs on central atom, bond angle is 120

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11
Q

Bent

A

2 atoms bonded, 1 lone pair on central atom, bond angle is <120 - if two lone pairs bond angle is 104

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12
Q

trigonal pyramidal

A

3 atoms bonded, 1 lone pair on central atom, bond angle is 107

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13
Q

trigonal bipyramidal

A

5 atoms bonded, no lone pairs, bond angle is eq. 120 ax. 90

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14
Q

Seesaw

A

4 atoms bonded, lone pair, bond angle is eq. 120 ax. 90

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15
Q

T shape

A

3 atoms bonded, 2 lone pairs, bond angle 90

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16
Q

Linear

A

1 or 2 atoms bonded, could be lone pairs, bond angle 180

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17
Q

octahedral

A

6 atoms bonded, no lone pairs, bond angle is 90

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18
Q

square based pyramid

A

5 atoms bonded, 1 lone pair, bond angle is 90

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19
Q

square planar

A

4 atoms bonded, 2 lone pairs, bond angle is 90

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20
Q

formal charge

A

formal charge should be as low as possible- ex. Oxygen has 6 valence electrons therefore wants 6 electrons in dot structure

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21
Q

Electron deficient molecules

A

Are stable when central atom has less than 8 electrons ( Boron or Beryllium) they do not have enough electrons to have 8

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22
Q

Odd number of valence electron molecules

A

NO, NO2, ClO2

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23
Q

what group has no electronegativity?

A

noble gases

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24
Q

What atoms can expand their octets?

A

3rd period and lower, often when P, S or Xe are the central atom

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25
Formal charge must equal...
Valence electrons in a single atom and the charge on an entire molecule (shifting of bonds)
26
Resonance structures
All ways to draw lewis dot structures
27
Bond Order
of bonds/ # of bond sites (decimal)
28
the larger the bond order...
The shorter the bond length and stronger bond (high bond energy)
29
Metallic bonds
Good conductors, malleable, shiny, high melting points (higher melting point, the stronger the metallic bond)
30
Metal Alloys
Substitutional alloy- metallic atoms of similar sizes in a lattice form (might be weaker only difference) Interstitial Alloys- Atoms of different sizes fitting into gaps, causes it to be harder
31
Ionic bond
metal and non metal, do not conduct electrcity when solid because there are no mobile ions, soluble, brittle, high melting point stronger bond
32
Covalent Bonds
High melting points, very hard, poor conducters,
33
Required covalent bonds
C (diamond), SiO2, SiC, C(graphite)
34
When are molecules polar
when outside atoms are different
35
VESPR theory
pairs of electrons will repel eachother
36
dimagnetic
All electrons are paired (less attraction)
37
paramagnetic
Unpaired electrons causing magnetic attraction
38
Does a shorter bond length create less or more bond energy?
Creates more due to more attraction
39
first ionization energy
First electron removed
40
Are ionic compound less or more electronegative?
Larger electronegativity
41
when can you see an atom went up in energy levels?
The ionization jumps
42
what shape is the S? P?
Sphere, dumbell
43
wavelength conversion
_ ._ _ to the -7
44
Electron- electron replusion
electrons are both negative, decreases ionization energy, easier to remove
45
Empirical formula
Lowest formula possible- divide by molar mass (each compound) divide by lowest mols , round to whole number
46
Molecular formula
Formula of values given, divide empirical formula molar mass, by actual molar mass, then multiply by that value
47
Mass spectrometery
How much of a compound, estimate using graph
48
PES
- 1s starts at the higher value, then go in order
49
Coloumbs Law
-Greater the charge the greater the force of attraction -Greater the distance the weaker the force of attraction
50
Zeff
-effective nuclear charge
51
Higher Zeff in regards to ionization engery, electronegative, and atomic radius
The higher the Zeff the higher the ionization energy and electronegative and smaller radius
52
If atoms have valence electrons in...
the same energy level (n=) then compare zeff (amount of protons) different energy levels then compare distance from the nucleus
53
Atomic Radius
-increases down to the left Higher Zeff =smaller radius because it pulls attraction to the nucleus Higher energy increases distance over which the nucleus must pull therefore, reducing attraction
54
Electronegativity
-Zeff increases attraction of the nucleus therefore strengthens attraction of electrons -Increased energy levels increases distance from the nucleus therefore reduces attraction of electrons
55
Ionization energy
-Zeff increases attraction of the nucleus therefore holds electrons tighter to the nucleus -Increased energy levels increases distance from the nucleus therefor reduces attraction
56
Ionization exceptions
Groups II, III - between groups 2 and 3 there is a drop in IE due to group 3 having electrons in the p orbital which is further from the nucleus therefore group II is more tightly held Groups V, VI - Sense group 5 has more unpaired electrons therefore due to the electron-electron repulsion of the unpaired electrons group 6 requires less energy to remove
57
Reactivity of metals
Become more reactive further down due to the increased # of energy levels increases the distance from the nucleus thus, looser electrons to react
58
Reactivity of non-metals
non-metals become more reactive further up because non metals tend to gain electrons therefore there is a higher Zeff which means the attraction to the nucleus is larger creating a stronger pull which makes it more reactive
59
ion radius cations
As the ratio of protons to electrons increases as electrons are lost therefore they are held tighter together with a smaller radius
60
ion radius anions
Added electrons reduces the proton to electron ratio, therefore the electrons are not as tightly held, along with increased electron-electron repulsion thus, a larger radius
61
What factor causes bond angle to compress?
greater repulsion, multiple bonds

AP Chem (9 decks)

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