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AP Chem > Unit 1 + 2 > Flashcards

Unit 1 + 2 Flashcards

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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
Q

Formal charge must equal…

A

Valence electrons in a single atom and the charge on an entire molecule (shifting of bonds)

26
Q

Resonance structures

A

All ways to draw lewis dot structures

27
Q

Bond Order

A

of bonds/ # of bond sites (decimal)

28
Q

the larger the bond order…

A

The shorter the bond length and stronger bond (high bond energy)

29
Q

Metallic bonds

A

Good conductors, malleable, shiny, high melting points (higher melting point, the stronger the metallic bond)

30
Q

Metal Alloys

A

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
Q

Ionic bond

A

metal and non metal, do not conduct electrcity when solid because there are no mobile ions, soluble, brittle, high melting point stronger bond

32
Q

Covalent Bonds

A

High melting points, very hard, poor conducters,

33
Q

Required covalent bonds

A

C (diamond), SiO2, SiC, C(graphite)

34
Q

When are molecules polar

A

when outside atoms are different

35
Q

VESPR theory

A

pairs of electrons will repel eachother

36
Q

dimagnetic

A

All electrons are paired (less attraction)

37
Q

paramagnetic

A

Unpaired electrons causing magnetic attraction

38
Q

Does a shorter bond length create less or more bond energy?

A

Creates more due to more attraction

39
Q

first ionization energy

A

First electron removed

40
Q

Are ionic compound less or more electronegative?

A

Larger electronegativity

41
Q

when can you see an atom went up in energy levels?

A

The ionization jumps

42
Q

what shape is the S? P?

A

Sphere, dumbell

43
Q

wavelength conversion

A

_ ._ _ to the -7

44
Q

Electron- electron replusion

A

electrons are both negative, decreases ionization energy, easier to remove

45
Q

Empirical formula

A

Lowest formula possible- divide by molar mass (each compound) divide by lowest mols , round to whole number

46
Q

Molecular formula

A

Formula of values given, divide empirical formula molar mass, by actual molar mass, then multiply by that value

47
Q

Mass spectrometery

A

How much of a compound, estimate using graph

48
Q

PES

A
  • 1s starts at the higher value, then go in order
49
Q

Coloumbs Law

A

-Greater the charge the greater the force of attraction
-Greater the distance the weaker the force of attraction

50
Q

Zeff

A

-effective nuclear charge

51
Q

Higher Zeff in regards to ionization engery, electronegative, and atomic radius

A

The higher the Zeff the higher the ionization energy and electronegative and smaller radius

52
Q

If atoms have valence electrons in…

A

the same energy level (n=) then compare zeff (amount of protons)
different energy levels then compare distance from the nucleus

53
Q

Atomic Radius

A

-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
Q

Electronegativity

A

-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
Q

Ionization energy

A

-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
Q

Ionization exceptions

A

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
Q

Reactivity of metals

A

Become more reactive further down due to the increased # of energy levels increases the distance from the nucleus thus, looser electrons to react

58
Q

Reactivity of non-metals

A

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
Q

ion radius cations

A

As the ratio of protons to electrons increases as electrons are lost therefore they are held tighter together with a smaller radius

60
Q

ion radius anions

A

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
Q

What factor causes bond angle to compress?

A

greater repulsion, multiple bonds

AP Chem (9 decks)

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