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Chem-109 > Test 4 > Flashcards

Test 4 Flashcards

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1
Q

VSEPR stands for

A

Valence shell electron pair repulsion

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2
Q

When it comes to repulsion list the 3 pair groupings from most repulsive to least

A

(lone pair, lone pair) > (lone pair, bond pair) > (bond pair, bond pair)

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3
Q

2 electron groups

A

linear, 180

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4
Q

3 electron groups

A

trigonal planer, 120

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5
Q

3 electron groups - 1 lone pair

A

bent, <120

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6
Q

4 electron groups

A

tetrahetral, 109.5

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7
Q

4 electron groups - 1 lone pair

A

trigonal pyramidal, <109.5

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8
Q

4 electron groups - 2 lone pair

A

bent, <109.5

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9
Q

5 electron groups

A

trigonal bypyramidal, 90,120

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10
Q

5 electron groups - 1 lone pair

A

seesaw, <120

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11
Q

5 electron groups - 2 lone pair

A

t-shaped, <90

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12
Q

5 electron groups - 3 lone pair

A

linear, 180

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13
Q

6 electron groups

A

octahedral, 90

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14
Q

6 electron groups - 1 lone pair

A

square pyramidal, <90

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15
Q

6 electron groups - 2 lone pair

A

square planar

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16
Q

Trend in atomic radius

A

Increases from top right to bottom left

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17
Q

nonbonding atomic radius is the same as this

A

van der Waals radius

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18
Q

bonding atomic radius is the same as this

A

covalent radius

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19
Q

How is the atomic radius measured in metals and nonmetals

A

Metals- 1/2 the distance between two of the atoms next to each other in a crystal of metal
nonmetals- 1/2 the distance between two of the atoms bonded togeather

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20
Q

The atomic radius is determined by this

A

a set of average bonding radii

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21
Q

Which is larger atomic radius or van der Waals radius

A

Atomic radius < van der Waals radius

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22
Q

Atomic radius is found by doing this

A

adding each atomic radius of a molecule to find the molecules atomic radius

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23
Q

Formula for finding effective nuclear charge

A

effective nuclear charge = actual nuclear charge - charge screened by the other electrons

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24
Q

Which group of elements atomic radius stays relatively consistant

A

transition metals

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25
Q

What is the exception to the rule when removing electrons to form a cation

A

In transition metals you remove the greatest N value shell first, even if it is not the reverse order

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26
Q

Paramagnetic, what is it, and how does it react in a magnetic field

A

an atom or ion that contains unpaired electrons, attracted to an external magnetic field

27
Q

diamagnetic, what is it, and how does it react in a magnetic field

A

an atom or ion that contains no unpaired electrons, repelled by an external magnetic field

28
Q

Trends in cations, and anions

A

Cations are much smaller than their respective atom, and anions are much larger than their respective atom

29
Q

What is ionization energy

A

energy required to remove an electron from an atom or ion in its gasous state

30
Q

What is the sign of ionization energy and why

A

positive, because it always takes energy to remove an electron

31
Q

Trend in ionization energy

A

Increases from bottom left to top right

32
Q

Are there any exceptions to the ionization energy trend, and if so what are they

A

Yes, half filled shells have lower then expected ionization energy

33
Q

Where do jumps in ionization energy occur

A

when removing electrons past a stable electron core

34
Q

What is electron affinity

A

energy change associated with the gaining of an electron by the atom in the gaseus state

35
Q

What is the sign of electron affinity and why

A

usually, but not always negative. because an atom or ion usually release energy when it gains and electron

36
Q

trend in electron affinity

A

become more negative as you move from the left to right

37
Q

Are there any exceptions to the electron affinity trend, and if so what is it

A

yes, half filled shells are lower then the trend, and almost half filled shells are higher then the trend

38
Q

trend in metalic character

A

Increases from top right to bottom left

39
Q

What is the best reason to discribe why chemical bonds form

A

because they lower the potential energy between the charged particals that compose atoms

40
Q

Three types of bonds

A

Ionic, covalent, metallic

41
Q

metal to nonmetal form

A

ionic

42
Q

nonmetal to nonmetal

A

covalent

43
Q

metal to metal

A

metallic

44
Q

Born-haber cycle formula is used for these types of bonds

A

ionic

45
Q

Born-Haber cycle formula is

A

dH_f = sub + IE + BE + EA + lat

46
Q

Trends in lattice energy

A

as the ionic radii increase as we move down the column, the ions cannot get as close to eachother and therefore do not release as much energy when the lattice forms

47
Q

This happens to lattice energies as atomic radii increase and decrease

A

as ionic radii increase lattice energy becomes less exothermic(less negative),
as ionic radii decrease lattice energy becomes more exothermic ( more negative)

48
Q

T/F: Electrons are always equally shared

A

F, the more electronegative atom uneually shares the electrons

49
Q

This type of bond is between pure covalent and ionic

A

polar covalent

50
Q

trend in electronegativty

A

increases from bottom left to top right

51
Q

covalent bonds are classified by an electronegativity difference of this range, and do this with their electrons

A

0 - .4 , equally share

52
Q

polar covalent bonds are classified by and electronegativity difference of this range, and do this with their electrons

A

.4 - 2, unequally share

53
Q

Ionic bonds are classigied by an electronegativity difference of this range, and do this with their electrons

A

2+ , transfer

54
Q

(4) Steps for writing Lewis structure for molecular compounds

A
  1. Write the correct skeletal structure for the molecule\
  2. calculate the total number of electrons
  3. distribute the electrons among the atoms, giving octets to as many atoms as possible
  4. If any atoms lack octets, form double/triple bonds as necessary to give them octets
55
Q

For polyatomic ions do this in your lewis structures

A
  1. put it in brackets

2. add/subtract the proper amount of electrons for the given ionic charge

56
Q

How to find the formal charge

A

formal charge = number of valence electrons originally for the atom - (total lone pair electrons + 1/2 bonded pair electrons)

57
Q

Odd electron species include

A

free radicals, incomplete octets, expanded octets

58
Q

Free radicals have this

A

and odd number of electrons and are generally unstable

59
Q

Some atoms that form incomplete octets include

A

Boron {B}, Beryllium {Be}

60
Q

Atoms that may form expanded octets

A

Atoms that are at N>=3 may have expanded octets

61
Q

Bond energy formula

A

dH_rxn = sum(d)H_bonds broken + sum(d)H_bonds formed

62
Q

The sign of broken bonds, and the sign of formed bonds

A

broken bonds are positive, and formed bonds are negative

63
Q

Exothermic reactions occur when

A

weak bonds break and strong bonds form

64
Q

Endothermic reactions occur when

A

weak bonds form and strong bonds break

Chem-109 (12 decks)

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