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physical chem > bonding > Flashcards

bonding Flashcards

1
Q

substances

A

made of single repeating unit at atomic level

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2
Q

mixture

A

made of several repeating units at atomic level

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3
Q

2 properties of particles

A

always have kinetic energy
always hold onto each other

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4
Q

3 properties of metals

A

malleable
ductile
conductive

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5
Q

electron sea model

A

electrons in a metal can move freely around in the structure

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6
Q

what keeps electrons together in electron sea model

A

positive ions form structure and balance charge of delocalized electrons

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7
Q

whats a lattice

A

regular repeating structure of ions

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8
Q

what holds lattice together

A

electrostatic force between cation and electron

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9
Q

stronger attraction in cations and electrons

A

stronger metallic bonding

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10
Q

why are metals malleable

A

lattice shape changed but cations can slide over each other keeping shape and metallic bonding

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11
Q

what happens when metal turns to liquid

A

regular lattice structure broken and cations can slide over each other

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12
Q

properties of liquid metal

A

not malleable or ductile
shiny and conductive

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13
Q

bonding in a liquid metal

A

does have delocalized electrons
weaker metallic bonding

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14
Q

higher melting point of metals

A

stronger metallic bonding

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15
Q

properties of gas

A

no metallic bonding and higher boiling point

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16
Q

do metals in liquid state have lattice

A

no lattice of cations

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17
Q

what happens when a metal boils

A

overall attractive forces overcome repulsive forces so no balance of forces

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18
Q

why do metals have higher melting and boiling points

A

because there is a strong attraction between cations and delocalized electrons

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19
Q

properties of metal gases

A

only have metal atoms

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20
Q

trend of metallic bonding

A

increases across period

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21
Q

why do metallic bonding increase across period

A

ions in lattice become more charges and number of electrons increases so higher electrostatic force between cation and electrons

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22
Q

why cant metals delocalize electrons all the time

A

only delocalize outer shells electrons

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23
Q

why can metals only delocalize outer shell electrons

A

only largest orbital overlap
small orbitals dont overlap so cant delocalize

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24
Q

trend of metallic bonding down group

A

decreases

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25
Q

why does metallic bonding decrease down group

A

size increases so more distance between cations nucleus and electrons so weaker forces

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26
Q

2 features of cations that effect metallic bonding

A

charge and size

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27
Q

state and explain general properties of metals exam question

A

melting point across period 3 eg

charge of cation increases so stronger attraction between cations and electrons
stronger attraction means stronger metallic bonding

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28
Q

compare melting point of 2 metals

A

eg mg ions more charges than potassium ions so stronger attraction of cations and electrons
stronger bonding so more energy to break forces

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29
Q

explain general melting point down group

A

size increases so more distance between cation and electrons so less energy required

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30
Q

what are alloys

A

metals with 2 or more elements

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31
Q

properties of all salts

A

high melting and boiling points
brittle
soluble
only conductive soluble

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32
Q

whats the perfect ionic model

A

all salts are made of positive and negative ions arranged in 3D lattice and ions perfect spheres

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33
Q

what keeps lattice together in ionic bonding

A

negative and positive electrostatic force/ attraction

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34
Q

what is ionic bonding

A

attraction between all cations and anions in lattice

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35
Q

charge of silver

A

+

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36
Q

charge of zinc

A

2+

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37
Q

charge of iron

A

2+ or 3+

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38
Q

charge of copper

A

1+ or 2+

39
Q

charge of lead

A

2+ or 4+

40
Q

group 7 6 5 anions

A

7= -
6=2-
5=3-

41
Q

how to name anions

A

add ide to element name

42
Q

hydrogencarbonate ion

A

HCO3-

43
Q

sulfate ion

A

SO42-

44
Q

phosphate ions

A

PO43-

45
Q

maganate ions

A

MnO42-

46
Q

hydroxide ions

A

OH-

47
Q

how do cations and anions combine

A

1 to 1 ratio to keep compound neutral

48
Q

how to present ionic compounds

A

use empirical formula

49
Q

how ionic compounds are formed in terms of electrons

A

how many electrons transferred from one element to other

50
Q

what happens when ionic compound melts

A

lattice breaks down and flow over each other
weaker ionic bonding

51
Q

liquid ionic compound into gas

A

seperates into individual compounds
no ionic bonding

52
Q

properties of solid ionic compounds

A

cant carry charge
dont conduct electricity

53
Q

properties of liquid ionic compound

A

can carry charge
can conduct electricity

54
Q

properties of gas ionic compiund

A

cant carry charge or conductive

55
Q

why are ionic bonds so strong

A

attraction of negative and positive
repulsion between both same

56
Q

why do ionic compounds have high melting and boiling points

A

strong electrostatic attraction between anions and cations

57
Q

whats is the electrostatic attraction effected by

A

charge and distance between particles

58
Q

what happens as you move down group for ionic bonding

A

elements get larger

59
Q

ioselectronic

A

equal number of electrons

60
Q

property of isoelectronic ions

A

larger nuclear charge smaller ion

61
Q

how do predict melting points

A

look at cations and anions and compare charge and then size

62
Q

why are ionic compounds brittle

A

when hit opposite charges together and lots of repulsion breaks layers apart

63
Q

how does a covalent bond form between two atoms

A

shared pare of electrons between atoms

64
Q

how much covalent bonds to atoms form

A

until they have full outer shell

65
Q

problems with circle and dot diagrams

A

cant see which electron came from where
messy

66
Q

bonding pairs

A

pairs of electrons bonding in covalent bonds

67
Q

lone pairs

A

outside unbonded electrons

68
Q

double bonds

A

2 pairs of electrons shared between 2 atoms

69
Q

triple bonds

A

3 electrons shared between 2 atoms

70
Q

how to predict which covalent bond will be longer

A

compare size of atoms forming bonds
bigger atoms is longer bonds

71
Q

how to predict melting and boiling point of bonds

A

compare bond lengths
shorter lengths stronger

72
Q

dative covalent bonds

A

one atom contributes both electrons to the shared pair

73
Q

how to represent dative bond

A

arrow from which one have it to where its going or two of same dot or cross

74
Q

2 elements to form electrons

A

dative bond donors and acceptors

75
Q

valence bond theory

A

if two atoms have orbitals which have unpaired electrons then orbitals will overlap with each other forming a covalent bond

76
Q

how do orbitals overlap

A

one pair of orbitals overlap head on to form one bond and other bond side on

77
Q

sigma bonds

A

when orbitals overlap head on lower case sigma

78
Q

pi bonds

A

orbitals overlap side on

79
Q

why does carbon form 4 bonds instead of 2

A

ground state = lowest energy orbital
in ground state can have 4 unpaired electrons

80
Q

electronegativity

A

ability to attract electron in covalent bond

81
Q

electronegativity across period

A

increases as more protons

82
Q

electronegativity down group

A

decreases down group
shell increases so nucleur radius bigger so less atraction

83
Q

electronegativity

A

ability to attract electron pair in a covalent bond

84
Q

factors that affect electronegativity of bonded pair

A

-nuclear charge
-distance from nucleus
-shielding

85
Q

exceptions of trends of electronegativity

A

-hydrogen similar to C as no electron shielding
-dont apply to group 8
-rare bonds

86
Q

dipole

A

one part of molecule slightly negative and the other slightly positive

87
Q

polar

A

slightly negative and positive parts of molecule

88
Q

comparing polarity

A

look at pauling scale values and compare difference

89
Q

ionic compounds formed when electronegativity high

A

when difference between to atoms so high the electrons almost belong to that atom
-atom able to conduct electricity and metal and brittle
-electrons sent to other atom

90
Q

metals formed in electronegavitity

A

when difference lower than 1.5 or greater

91
Q

what holds polyatomic ionic bonds together

A

covalent bonds

92
Q

ionic compounds with polyatomic ions

A

covalent and ionic bonds

93
Q

accounting for charge when drawing polyatomic ions

A

if compound has negative charge add electrons to most electronegative compound
-if molecule positive add electron to least electronegative molecule

94
Q
A

physical chem (8 decks)

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