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chemistry - Welch > atomic structure and bonding > Flashcards

atomic structure and bonding Flashcards

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1
Q

what is a mass spectrometer

A

machine that measures the mass + abundance of particles

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2
Q

what does the hydrogen emission spectrum show

A

shows there are specific energy levels that have patterns

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3
Q

what are the 2 evidences for ions

A

migration of ions
x-ray diffraction

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4
Q

what is migration of ions

A

wet filter paper with coloured ions in has a charge flowing through it
if colours move, they must be charged ions, not neutral atoms

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5
Q

what is x-ray diffraction

A

x ray tube shoots a beam through a crystal and shield
this displays where the ions are
gaps show repulsion and therefore charge

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5
Q

what does an s orbital look like

A

spherical
centred on the nucleus
come on their own

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6
Q

what are the 4 orbitals in order

A

S
P
D
F

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7
Q

what does a p orbital look like

A

at right angles
come in sets of 3

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8
Q

what do d orbitals look like

A

come in sets of 5

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9
Q

what do f orbitals look like

A

come in sets of 7

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10
Q

what orbitals do al atoms have

A

all

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11
Q

what is Aufbaus’s rule

A

fill orbitals from lowest energy

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12
Q

what is Pauli’s rule

A

two electrons sharing an orbital have opposite spin while orbiting

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13
Q

what is the acception for filling orbitals

A

fill 4s orbital before the 3d orbitals
also lose 4s before 3d if +ion

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14
Q

what is Hund’s rule

A

degenerate orbitals fill singly, before pairing up

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15
Q

where do the orbitals goon the periodic table

A
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16
Q

ionic structure -ions in the lattice

A

+ions and -ions alternate
in a giant ionic lattice

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17
Q

ion conductivity needs

A

high conductivity in liquid or aqueous states
no conductivity in solid states

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18
Q

ionic bonding definitions

A

electrostatic attraction between oppositely charged ions

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19
Q

what does ionic charge depend on 2

A
  • charges of each ion
    -radii of each ion
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20
Q

properties of simple molecules

A

low MP
don’t conduct
some soluble in water

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21
Q

define dative covalent bond

A

electrostatic attraction between positively charged nuclei of bonding atoms and shared pair of electrons where both electrons come from the same atom

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22
Q

when expanding octets, why are 2 extra bonds made

A

energy needed to promote 3d-3s is less than the energy released when 2 extra bonds form

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23
Q

order of bonds energy in carbon

A

as number of bonds increase, bond energy increases

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24
Q

2 factors that affect covalent bonds strength

A

number of bonds and size of atoms

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25
Q

why do bigger atoms form weaker covalent bonds

A

bigger atoms
longer bonds
further from nucleus
attraction is weaker
bonds is weaker

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26
Q

define structure of metals

A

giant metallic lattice

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27
Q

define bonding in metals

A

electrostatic attraction between positive metal cations and a negatively charged sea of delocalised electrons

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28
Q

what does the strength of metallic bonding depend on 3

A

cation charge
cation radius (smaller means stronger)
number of delocalised electrons

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29
Q

why can metals conduct

A

delocalised electrons are free to move throughout the structure

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30
Q

why are metals malleable

A

layers of metal ions cam slide over each other without disruption the bonding

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31
Q

what is VSEPR

A

valence (shell) electron - pair repulsion

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32
Q

what shape has minimum pair repulsion

A

2-6 pair shapes

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33
Q

what would 2 pairs
look like
be called
angle sizes

A

linear

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34
Q

what would 3 pairs
look like
be called
angle sizes

A

trigonal planar

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35
Q

what would 4 pairs
look like
be called
angle sizes

A

tetrahedral

36
Q

what would 5 pairs
look like
be called
angle sizes

A

trigonal bipyramidal

37
Q

what would 6 pairs
look like
be called
angle sizes

A

octahedral

38
Q

why do lone pairs cause a change in shape

A

lone pairs attract more than bonding pairs

39
Q

what do 3 bonding pairs and 1 lone pair
look like
are called
and angle sizes

A

trigonal pyramidal

40
Q

what do 2 bonding pairs and 1 lone pair
look like
are called
and angle sizes

A

bent

40
Q

what happens to the shape of the molecule if there are double bonds

A

double bonds repel a lot more
so bonding electrons move doen

41
Q

for bigger molecules, how do you draw them

A

alanine - apply VSPER to each individual atom in the larger molecule

42
Q

how to calculate number of lone pairs

A

add middle element and number of bonds
divide by 2

43
Q

define electronegativity

A

the tendency of an atom (of an element) to attract bonding electrons

44
Q

what elements have the lowest electronegativity

A

metals

45
Q

what elements have the highest electronegativity

A

non metals

45
Q

what bonding has a low electronegativity difference and a low mean electronegativity

A

metallic

46
Q

what bonding has the highest electronegativity difference

A

ionic

47
Q

what bonding has low electronegativity difference and high mean electronegativity

A

covalent

48
Q

mps why electronegativity increases up a group 3

A

atomic radius decreases
less electron shielding
stronger attraction to nucleus

49
Q

mps on why electronegativity increases across a period

A

similar radius and shielding
nuclear charge increases
stronger attraction to the nucleus

49
Q

on a graph of mean electronegativity and electronegativity difference, where does each bonding go

A

ionic top
metal bottom left
covalent bottom right

50
Q

diamond structure electron arrangement

A

2,4

50
Q

diamond number of c bonds for each atom

A

4 (max number)

51
Q

what temp does diamond sublime

A

4000 degrees Celsius
strong c-c bonds need to be broken

52
Q

diamond conductivity

A

doesn’t conduct
all electrons held between atoms in structure

52
Q

diamond hardness

A

covalent bonds operating in 3 dimensions

53
Q

diamond solubility

A

insoluble in water and organic solvents
no attraction that could outweigh carbon covalent bonds

54
Q

graphite number of c bonds for each atoms

A

3
4th electron becomes delocalised

54
Q

how do graphite sheets stay together

A

atom within sheets held together by strong covalent bonds
delocalised electrons add extra attraction

54
Q

what are van der waals dispersion forces in graphite

A

dipoles induced in sheets above and below

54
Q

graphite melting point

A

high
strong covalent bonding

54
Q

graphite solubility

A

insoluble in water and organic solvents
no attraction that could outwigh carbon covalent bonds

54
Q

graphite density compared to diamond

A

less dense
large space between sheets

54
Q

graphite feel

A

soft and slippery
layers slide over each other

55
Q

graphite conductivity

A

conducts electricity
deleocalisede-s free to move throughout the sheets

56
Q

silicon dioxde melting point

A

1700 degrees Celsius
strong silicon-oxygen covalent bonds

57
Q

silicon dioxide hardness

A

hard
strong silicon-oxygen covalent bonds

58
Q

silicon dioxide conductivity

A

doesnt conduct
all electrons trapped in structure

59
Q

silicon dioxide solubility

A

insoluble in water and organic solvents
no attraction that could outweigh covalent bonds

60
Q

define polar bonds

A

covalent bonds are polar if there is a significant electronegativity difference

61
Q

define polar molecules

A

a molecule with asymmetrically arranged polar bonds

62
Q

how to test if a liquid contains polar molecules

A

jet of liquid bends away from a charged rod

63
Q

what IM forces have 0-30 kJmol

A

london forces

64
Q

what IM forces have 30-50kJmol

A

dipol-dipol bonding

65
Q

what IM forces are 50-150 kJmol

A

hydrogen bonding

65
Q

define london forces

A

attraction between induced dipoles

65
Q

What IM forces are more than 151 kJmol

A

covalent bonds

66
Q

wat does the strength of london forces depend on

A

no of electrons per molecule
consider the shape of the molecule

67
Q

what shape of molecule has stronger london forces and why

A

longer thinner molecules
can pack closer together
slightly stronger attracton

68
Q

what moleular substances have london forces

A

all

69
Q

how are dipoles induces in solids

A

electrons move randomly
more move on way at one point
inducing a dipole

70
Q

explain how a dipole appears

A

as son as more elctrons go one way than the other, an instantaneous dipole appears - inducing the other dipole

71
Q

what are permanent dipoles called

A

dipole-dipole forces

72
Q

whats the difference between dipole-dipole forces and london forces 2

A

dipole-dipole forces are stronger because dipoles are already there
molecules are polar for dipole-dipole forces

72
Q

why does polarity increasing increase hydrogen bond strength

A

weaker atom is exposed to the outside of the electron cloud

73
Q

conditions for there to be a hydrogen bond

A

a N/O/F atom bonded to a hydrogen atom
hydrogen atom can form a hydrogen bond with another N/O/F atom with a spare electron pair

74
Q

define a Hydrogen bond

A

n/Fattraction between a H (alpha+) in O-H/N-F/F-H and a lone pair on o/

chemistry - Welch (2 decks)

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