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ap chem ap death > test 2 FUCK > Flashcards

test 2 FUCK Flashcards

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1
Q

ionic bond

A
  • held by electrostatic forces
  • strong lattice structure
  • usually solid at room temp, high melting and boiling points
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2
Q

factors that affect the melting points of ionic substances

A
  • Coulomb’s law: greater charge = greater bond (lattice energy
  • size of atoms: smaller atoms will have a greater Coulo,bic attraction (size inversely proportional to bond energy)
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3
Q

Ionic solids electrons are

A

localized, do not move around lattice, makes them poor conductors

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4
Q

ionic liquids

A

do conduct electricity, electrons are still localized but ions are free to move

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5
Q

metallic bonds often uses

A

sea of electrons

-positively charged core of metal is stationary, valence electrons move freely in a “sea”

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6
Q

mobile electrons in metallic bonds explain why

A

-metals are such good conductors of electricity
-makes them malleable and ductile (drawn into thin wire)
because deforming metal does not change environment surrounding the metal cores

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7
Q

metals bond w each other to form

A

alloys, (usually when two metals are melted into their liquid phases)

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8
Q

interstitial alloy

A

metal atoms with two vastly different radii combine (ex. steel)

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9
Q

substitutional alloy

A

forms between atoms of similar radii , some atoms are substituted

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10
Q

covalent bonds

A

shared electrons, each atom counts shared electrons as part of valence shell

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11
Q

all single bonds in covalent bonding are

A

sigma bonds

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12
Q

second bond in double bonds and second and third bond in triple bond

A

pi bonds, stronger and shorter

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13
Q

single covalent bond

A

one sigma

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14
Q

as you add the bonds they get

A

shorter and the bond energy increase

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15
Q

double covalent bond

A

one sigma and one pi

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16
Q

triple covalent bond

A

one sigma and two pi

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17
Q

internuclear distance

A
  • bonds form where the potential energy of the bond is at its lowest level
  • atoms very close together» potential energy is high
  • atoms very far apart»> potential energy close to zero
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18
Q

minimum potential energy in a bond occurs

A

when the repulsive and attractive forces are balanced

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19
Q

network covalent bonds

A

atoms are held together in a lattice of covalent bonds

  • like one big molecule, very hard, very high melting and boiling points
  • ex: (SiO2 quartz)
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20
Q

electrons in network covalent bonds

A

-localized, not free to move,&raquo_space;> moves them poor conductors

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21
Q

doping

A

process in which an impurity is added to an existing lattice

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22
Q

p-doping

A

adding an element w/ less valence electrons than needed, missing bond or hole in a lattice creates a positive charge attracting other electrons (conductivity)

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23
Q

n-doping

A

element with extra valence electrons i added to lattice, increases the negative charge and conductivity

24
Q

resonance forms

A

when you put a double bond, it has equal chance of falling on any of the same atoms on the central atom
- means that the strength and length of all three bonds in the carbonate ion are the same, between the strength and length of a single and double bond

25
Q

bond order calculation:

A
  • single bond: bond order 1, double bond: bond order 2, etc.
  • FIND by adding up the total bond order, so like 1 +1 +2 (if two single bonds and one double bond) divide by them number of resonance forms
26
Q

incomplete octets

A

some atoms are stable w/ less than eight electrons in outer shell: hydrogen only requires 2, Boron only requires six

27
Q

expanded octets

A

molecules with the d subshells can have expanded octets , central atom can have more than 8 electrons, but never more than twelve
SO n=3 or greater , NEVER n=2 (ex. NOT C, N, O)
explain why noble gases can form bonds

28
Q

formal charge

A
  • to determine most likely structure when multiple possible VSEPR available
  • should be 0 on a neutral atom
  • with a more actual formal charge … it is more likely
29
Q

calculate formal charge

A

formal Charge = [# of valence electrons on atom] – [non-bonded electrons + number of bonds] (not bonded electrons)

30
Q

molecule with more than two atoms

A

the shape is determined by the number of electron pairs on the central atom, which forms hybrid orbitals with a standard shape

31
Q

VSEPR

A
  • double and triple bonds are treated the same way as single bonds for predicting the overall geometry, but have more repulsive strength and may take up more space
  • lone electron pairs have more repulsive strength than bonding paires»» molecules w lone pairs will have a slightly reduced bond angle
32
Q

If the central atom has 2 electron pairs

A

sp hybridization, shape is linear

33
Q

If the central atom has 3 electron pairs with 0 lone pairs

A

sp2 hybridization, shape is trigonal planar

34
Q

If the central atom has 3 electron pairs with 1 lone pair

A

sp2 hybridization, shape is bent

35
Q

if the central atom has 4 electron pairs with 0 lone pairs

A

sp3 hybridization, shape is tetrahedral. bond angles about 109.5 degrees

36
Q

if the central atom has 4 electron pairs with 1 lone pairs

A

sp3 hybridization, shape is trigonal pyramidal

37
Q

If the central atom has 4 electron pairs with 2 lone pairs

A

sp3 hybridization, shape is bent

38
Q

if the central atom has 5 electron pairs with 0 lone pairs

A

the shape is trigonal bipyramidal

39
Q

if the central atom has 5 electron pairs with 1 lone pair

A

the shape is seesaw

40
Q

if the central atom has 5 electron pairs with 2 lone pairs

A

the shape is T-shaped

41
Q

if the central atom has 5 electron pairs with 3 lone pairs

A

the shape is linear

42
Q

if the central atom has 6 electron pairs with 0 lone pairs

A

the shape is octahedral

43
Q

if the central atom has 6 electron pairs with 1 lone pair `

A

the shape is square pyramidal

44
Q

if the central atom has 6 electron pairs with 2 lone pairs

A

the shape is square planar

45
Q

coulomb’s law

A

E=k (+q)(-q)
—————
r2

46
Q

what U know from Coulomb’s law

A
  • greater the charge of nucleus, the more energy an electron will have
  • explains binding energy
  • 3s electrons will have more PE than 1s electrons
47
Q

Energy and Electromagnetic radiation equation

A

E=hv
E. energy change (in Joules)n
h.. Planck’s constant (6.626 x 10 -34 Js)
v= frequency (in s-1)

48
Q

Frequency and Wavelength

A

c=wv
c= speed of light (2.998 x 10 8 ms-1)
v= frequency (in s -1)
w= wavelength (in m)

nm might need to be converted to m
1 nm = 1 x 10 -9 m

usually: use speed of light to convert wavelength to frequency… then use frequency and Planks constant to find energy

49
Q

in photoelectron spectroscopy

A

energy of incoming radiation must be conserved and any energy that does not go into breaking the electron free becomes kinetic energy :
incoming radiation energy = binding energy + kinetic energy

50
Q

aufbau principle

A

states when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, and shells in order of increasing energy

51
Q

pauli exclusion principle

A

states that two electrons which share an orbital cannot have the same spin , on electron must spin clockwise, the other counterclockwise

52
Q

hund’s rule

A

says that when an electron is added to a subshell, it will always occupy an empty orbital if one is available

53
Q

atomic radius

A

-decreases from left to right
-increases down
cations are smaller
anions are larger

54
Q

ionization energy

A

-opposite from atomic radius
-increases from left to right
-decreases down
second ionization energy is greater than the first

55
Q

what is electronegativity

A

how strongly the nucleus of an atom attracts the electrons of other atoms in a bond

  • smaller an atom is, the more effectively the nuclear charge will be felt past its outermost energy level, higher electronegativity
  • closer an element is to having a full energy level, the more likely to attract electrons to complete that
56
Q

electronegativity

A
  • increases from left to right

- decreases down

ap chem ap death (3 decks)

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