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chemistry - Welch > atomic structure and bonding > Flashcards

atomic structure and bonding Flashcards

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 l 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
2 factors that affect covalent bonds strength
number of bonds and size of atoms
25
why do bigger atoms form weaker covalent bonds
bigger atoms longer bonds further from nucleus attraction is weaker bonds is weaker
26
define structure of metals
giant metallic lattice
27
define bonding in metals
electrostatic attraction between positive metal cations and a negatively charged sea of delocalised electrons
28
what does the strength of metallic bonding depend on 3
cation charge cation radius (smaller means stronger) number of delocalised electrons
29
why can metals conduct
delocalised electrons are free to move throughout the structure
30
why are metals malleable
layers of metal ions cam slide over each other without disruption the bonding
31
what is VSEPR
valence (shell) electron - pair repulsion
32
what shape has minimum pair repulsion
2-6 pair shapes
33
what would 2 pairs look like be called angle sizes
linear
34
what would 3 pairs look like be called angle sizes
trigonal planar
35
what would 4 pairs look like be called angle sizes
tetrahedral
36
what would 5 pairs look like be called angle sizes
trigonal bipyramidal
37
what would 6 pairs look like be called angle sizes
octahedral
38
why do lone pairs cause a change in shape
lone pairs attract more than bonding pairs
39
what do 3 bonding pairs and 1 lone pair look like are called and angle sizes
trigonal pyramidal
40
what do 2 bonding pairs and 1 lone pair look like are called and angle sizes
bent
40
what happens to the shape of the molecule if there are double bonds
double bonds repel a lot more so bonding electrons move doen
41
for bigger molecules, how do you draw them
alanine - apply VSPER to each individual atom in the larger molecule
42
how to calculate number of lone pairs
add middle element and number of bonds divide by 2
43
define electronegativity
the tendency of an atom (of an element) to attract bonding electrons
44
what elements have the lowest electronegativity
metals
45
what elements have the highest electronegativity
non metals
45
what bonding has a low electronegativity difference and a low mean electronegativity
metallic
46
what bonding has the highest electronegativity difference
ionic
47
what bonding has low electronegativity difference and high mean electronegativity
covalent
48
mps why electronegativity increases up a group 3
atomic radius decreases less electron shielding stronger attraction to nucleus
49
mps on why electronegativity increases across a period
similar radius and shielding nuclear charge increases stronger attraction to the nucleus
49
on a graph of mean electronegativity and electronegativity difference, where does each bonding go
ionic top metal bottom left covalent bottom right
50
diamond structure electron arrangement
2,4
50
diamond number of c bonds for each atom
4 (max number)
51
what temp does diamond sublime
4000 degrees Celsius strong c-c bonds need to be broken
52
diamond conductivity
doesn't conduct all electrons held between atoms in structure
52
diamond hardness
covalent bonds operating in 3 dimensions
53
diamond solubility
insoluble in water and organic solvents no attraction that could outweigh carbon covalent bonds
54
graphite number of c bonds for each atoms
3 4th electron becomes delocalised
54
how do graphite sheets stay together
atom within sheets held together by strong covalent bonds delocalised electrons add extra attraction
54
what are van der waals dispersion forces in graphite
dipoles induced in sheets above and below
54
graphite melting point
high strong covalent bonding
54
graphite solubility
insoluble in water and organic solvents no attraction that could outwigh carbon covalent bonds
54
graphite density compared to diamond
less dense large space between sheets
54
graphite feel
soft and slippery layers slide over each other
55
graphite conductivity
conducts electricity deleocalisede-s free to move throughout the sheets
56
silicon dioxde melting point
1700 degrees Celsius strong silicon-oxygen covalent bonds
57
silicon dioxide hardness
hard strong silicon-oxygen covalent bonds
58
silicon dioxide conductivity
doesnt conduct all electrons trapped in structure
59
silicon dioxide solubility
insoluble in water and organic solvents no attraction that could outweigh covalent bonds
60
define polar bonds
covalent bonds are polar if there is a significant electronegativity difference
61
define polar molecules
a molecule with asymmetrically arranged polar bonds
62
how to test if a liquid contains polar molecules
jet of liquid bends away from a charged rod
63
what IM forces have 0-30 kJmol
london forces
64
what IM forces have 30-50kJmol
dipol-dipol bonding
65
what IM forces are 50-150 kJmol
hydrogen bonding
65
define london forces
attraction between induced dipoles
65
What IM forces are more than 151 kJmol
covalent bonds
66
wat does the strength of london forces depend on
no of electrons per molecule consider the shape of the molecule
67
what shape of molecule has stronger london forces and why
longer thinner molecules can pack closer together slightly stronger attracton
68
what moleular substances have london forces
all
69
how are dipoles induces in solids
electrons move randomly more move on way at one point inducing a dipole
70
explain how a dipole appears
as son as more elctrons go one way than the other, an instantaneous dipole appears - inducing the other dipole
71
what are permanent dipoles called
dipole-dipole forces
72
whats the difference between dipole-dipole forces and london forces 2
dipole-dipole forces are stronger because dipoles are already there molecules are polar for dipole-dipole forces
72
why does polarity increasing increase hydrogen bond strength
weaker atom is exposed to the outside of the electron cloud
73
conditions for there to be a hydrogen bond
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
define a Hydrogen bond
n/Fattraction between a H (alpha+) in O-H/N-F/F-H and a lone pair on o/

chemistry - Welch (7 decks)

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