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bonding Flashcards

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1
Q

ionic compounds contain..

A

a metal and non metal

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2
Q

what happens when ionic compounds form

A

electron transfer

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3
Q

what us a single covalent bond

A

a shared pair of electrons

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4
Q

what does the number of unpaired electrons indicate?

A

the number of covalent bonds that can be made

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5
Q

how many covalent bonds can carbon make

A

4

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6
Q

what is an ion?

A

a charged particle

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7
Q

what are cations?

A

positive ions

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8
Q

what are anions?

A

negative ions

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9
Q

what is an ionic bond?

A

the elctrostatic attraction between oppositely charged ions

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10
Q

what do elements lose/gain electrons to achieve?

A

nobel gas configuration

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11
Q

what is different about transition metals?

A

do not always achieve nobel gas configuration

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12
Q

what is an ionic lattice?

A

regular, repeated 3D framework of ions

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13
Q

what is each:

1) Na+ ion sureounded by in NaCl

2) Cl- ion sureounded by in NaCl

A

1) 6 Cl- ions

2) 6 Na+ ions

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14
Q

what tyoe of crystal structure is NaCl?

A

cubic

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15
Q

what is decrepitation?

A

cracking sounds made when an ionic crystalline structure breaks up upon heating

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16
Q

why does ionic solids have high melting points?

A

strong electrostatic attractions between oppositely charged ions require alot of energy to break

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17
Q

what increases the strength of ionic bonds?

A

smaller ions and higher charge

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18
Q

why are positive ions smaller than their atoms

A

losing an electron from an outer shell inscreases the effective nuclear charge pulling electrons closer to the nucleus

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19
Q

why are negative ions larger than their atoms?

A

effective nuclear charge decreases and increases electron repulsion

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20
Q

wht are ionic compounds usually soluble in water?

A

water is a polar solvent

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21
Q

why are some ionic compounds not soluble in water

A

the electrostatic attraction is so strong, water cannot break the lattice apart

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22
Q

why can ionic compounds conduct electrocity when molten or dissolved?

A

charges are free to move and transport a current

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23
Q

how is a single covalent bond represented

A

a line

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24
Q

how is a double covalent bond represented

A

a double line

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25
Q

what is a lone pair

A

a pair of electrons not involved in bonding

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26
Q

whoch orbitals are used if bonding results in more than 8 calence electrons?

A

d orbitals

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27
Q

what is another name for a dative covalent bond

A

coordinate bond

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28
Q

what is a dative covalent bond?

A

a lone pair is donated into an empty orbital on another atom

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29
Q

what is different about a dative covalent bond?

A

both electrons come from one atom

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30
Q

how do you represent a dative covalent bond?

A

an arrow

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31
Q

what is different about the properties of a dative covalent bond and a standard covalent bond?

A

nothing

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32
Q

define metallic bonding

A

electrostatic forces between delocalised electrons and positive metal ions in a lattice

33
Q

why can metals conduct electricity?

A

delocalised electrons can transport a current

34
Q

why can metals conduct heat?

A

delocalised electrons can transfer energy

35
Q

why are metals malleable/ductile?

A

laters of metal ions can slide over eachother without distrupting the bonding

36
Q

why do metals have high boiling points?

A

requires a lot of energy to break strong electrostatic atteaction between delocalised electrons and positive metal ions

37
Q

why do transition metals have higher boiling points?

A

large number of d subshell, electrons delocalise forming stronger bonds

38
Q

what is another name for a giant covalent structure?

A

macromolecular

39
Q

what are crystal structures of simple covalent compounds called?

A

molecular covalent crystals

40
Q

give an example of a molecular covalent crystal

A

ice

41
Q

name three properties of molecular covalent crystals:

A

low melting point
brittle
do not conduct electricity

42
Q

what is an allotrope?

A

different forms of the same element in the same physicao state

43
Q

give two allotropes of carbon

A

diamond
graphite (graphene)

44
Q

give three properties of diamond

A

hard
high melting point
does not conduct electricity

45
Q

give three properties of graphite

A

lubricant
high melting point
does conduct electricity

46
Q

what is sublimination?

A

change of state from solid to gas

47
Q

why do lone pairs cause more repulsion?

A

held closer to the nucleus

48
Q

2 bonding pairs
0 lone pairs:

name
angle

A

linear
180•

49
Q

3 bonding pairs
0 lone pairs:

name
angle

A

trigonal planar
120•

50
Q

4 bonding pairs
0 lone pairs:

name
angle

A

tetrahederal
109.5•

51
Q

3 bonding pairs
1 lone pair:

name
angle

A

pyramidal
107•

52
Q

2 bonding pairs
2 lone pairs:

name
angle

A

bent
104.5•

53
Q

5 bonding pairs
0 lone pairs:

name
angles

A

trigonal bypyramid
90• and 120•

54
Q

3 bonding pairs
2 lone pairs:

name
angle

A

T shaped
86•

55
Q

2 bonding pairs
3 lone pairs:

name

A

linear

56
Q

6 bonding pairs
0 lone pairs:

name
angle

A

octahederal
90•

57
Q

4 bonding pairs
2 lone pairs:

name
angle

A

square planar
90•

58
Q

4 bonding pairs
1 lone pair:

name
angles

A

sawhorse
86• and 117•

59
Q

what is electronegativity?

A

the power of an atom to attract electron density towards itself

60
Q

wht is the most electronegative element?

A

fluorine

61
Q

what does electronegativity depend on?

A

atomic radius- smaller=stronger attraction

nuclear charge- more protons=stronger attraction

shielding- more e-=more shielding=less attraction

62
Q

what is the trend in electronegativity?

A

increases across a period and up a group

/^

63
Q

what dies a delta +ve charge represent?

A

electron efficient

64
Q

what does a delta -ve charge represent?

A

electron rich

65
Q

why is BF3 non-polar

A

it is symmetrical

66
Q

what is another word for polar?

A

permenant dipole moment

67
Q

what is an intermolecular force?

A

a force between molecules

68
Q

what is an intramolecular force?

A

a force within molecules

69
Q

name theee types if intermolecular force

A

Van dee Waal
dipole-dipole
Hydrogen bond

70
Q

how do VDW forces occur?

A

random movement of electrons causes a temporary dipole which induces a dipole in a neighbouring atom, the resulting opposite delta charges attract

71
Q

what are teo other names for VDW forces?

A

induced dipole-dipole
london forces

72
Q

what happens to VDW attraction as atomic radius increases

A

gets stronger

73
Q

what is a permenant dipole-dipole force?

A

interaction between teo permenant dipoles due to the attraction of opposite delta charges

74
Q

which theee bonds can form hydrogen bonds?

A

N-H
O-H
F-H

75
Q

which intermolecular force is the strongest?

A

hydrogen bonds

76
Q

why is ice less dense than water?

A

hudrogen bonds form an open crystalline structure

77
Q

what sort of molecules dissolve in polar solvents?

A

polar molecules

78
Q

what sort if molecules dissolve in non-polar solvents?

A

non-polar molecules

chemistry (6 decks)

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