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chemistry: physical chemistry 1 > bonding > Flashcards

bonding Flashcards

(60 cards)

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1
Q

what is ionic bonding? (3)

A

● strong electrostatic forces of attraction between oppositely charged ions

● electrons are transferred

● between metal and non metal

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2
Q

what is the structure of ionic compounds?

A

giant ionic lattice

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3
Q

what are the properties of giant ionic lattices? (3)

A

● electrical conductivity

● shatters easily / brittle

● high melting point and boiling point

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4
Q

why do ionically bonded substances have high boiling points?

A

takes a lot of energy to overcome strong electrostatic forces of attraction between oppositely charged ions

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5
Q

describe why ionic compounds can conduct electricity

A

when molten or aqueous, ions are free to move and can carry the charge (can’t when solid)

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6
Q

describe the strength of ionic compounds (2)

A

● shatters easily / brittle

● any disruption to structure that makes positive ions or negative ions align will cause them to repel and shatter

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7
Q

what does the strength of an ionic bond depend on? (2)

A

● charge (larger the charge of ion, the stronger the attraction)

● size (smaller the ion, the stronger the attraction)

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8
Q

what is covalent bonding?

A

shared pair of electrons

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9
Q

what are the properties of simple covalent molecules? (3)

A

● low melting point

● low boiling point

● can’t conduct electricity

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10
Q

why can’t simple covalent molecules conduct electricity?

A

all electrons are used in bonding and aren’t free to move

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11
Q

why do simple covalent molecules have low melting and boiling points?

A

weak van der waals forces of attraction which dont take much energy to overcome

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12
Q

what is macromolecular covalent bonding?

A

lattice of many atoms held together by strong covalent bonds

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13
Q

do substances with macromolecular covalent bonds have high or low melting and boiling points? (2)

A

● high

● as it takes lots of energy to overcome many strong covalent bonds

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14
Q

do substances with macromolecular covalent bonds conduct electricity?

A

most don’t as all electrons are used in bonding

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15
Q

draw and describe the structure of diamond

A

3D tetrahedral structure of carbon atoms, with each c atom bonded to 4 others

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16
Q

draw and describe the structure of graphite (4)

A

● macromolecular covalent

● each atom bonded to 3 others - so in layers

● weak vdw’s forces of attractions mean they can slide over each other - soft, slippery

● one electron from each carbon is delocalised and can carry the charge - conducts electricity

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17
Q

describe and draw metallic bonding

A

lattice of positive metal ions strongly attracted to sea of delocalised electrons

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18
Q

what are the properties of metals? (6)

A

● can conduct electricity

● good conductor of heat

● malleable

● ductile

● strong

● high mp and bp

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19
Q

what does malleable mean?

A

can be beaten into shape

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20
Q

what does ductile mean?

A

can be pulled into thin wires

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21
Q

do metallic compounds have high or low melting and boiling points? (2)

A

● high

● strong forces of attraction between positive metal ions and negatively charged sea of delocalised electrons which takes a lot of energy to overcome

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22
Q

do metallic compounds conduct electricity? why? (2)

A

● yes

● delocalised electrons can move throughout the structure to carry the charge

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23
Q

what does the strength of a metallic bond depend on? (2)

A

● charge (larger the charge of ion, the stronger the attraction)

● size (smaller the ion, the stronger the attraction)

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24
Q

how does the strength of metallic bonds change across the periodic table? why? (4)

A

● increases

● larger charge on metal ions

● more delocalised electrons per ion

● so, stronger forces of attraction between them

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25
smaller ions will attract electrons...
more strongly as they are closer to nucleus
26
if nuclear charge is bigger...
stronger attraction
27
if there are more delocalised electrons...
more forces of attraction
28
what is orbital theory?
covalent bonds are formed when orbitals, each containing 1 electron, overlap
29
what is the octet rule? (3)
● tendency to prefer 8 electrons in outer shell ● we do not consider p and f electrons ● only s and d are involved
30
what is coordinate bonding? (2)
● shared pair of electrons but both electrons come from same atom ● have exactly same strength and length as ordinary covalent bonds once they are formed
31
when is a coordinate bond formed?
when an electron deficient atom / ion accepts a lone pair of electrons from an atom / ion (not used in bonding)
32
what are coordinate bonds represented by?
→ (points towards atom accepting bond)
33
draw the formation of a dative covalent bond in ammonium
‎
34
define electronegativity
the power of an atom to attract the electron density in a covalent bond towards itself it
35
what are the factors which affect electronegativity? (3)
● nuclear charge ● atomic radius ● shielding
36
how does nuclear charge affect electronegativity? (2)
● more protons ● stronger attraction between nucleus and bonding pair of electrons
37
how does atomic radius affect electronegativity? (2)
● electrons closer to the nucleus ● stronger attraction between nucleus and bonding pairs of electrons
38
how does shielding affect electronegativity? (3)
● less shells of electrons between nucleus and electrons ● so, less shielding (less repulsion) ● stronger attraction between nucleus and bonding pair of electrons
39
what is the trend of electronegativity down a group? why? (3)
● decreases ● nuclear charge increases, but atomic radius increases and more shielding ● therefore, less attraction between nucleus and bonding pair of electrons
40
what is the trend of electronegativity across a period? (3)
● increases ● nuclear charge increases, but atomic radius decreases and shielding stays the same ● therefore, stronger attraction between nucleus and bonding pair of electrons
41
explain electronegativity in bonds between identical atoms (3)
● electrons are shared equally ● so, no difference in electronegativity ● so, non polar
42
explain electronegativity in bonds between different atoms (6)
● different electronegativity ● so, one will pull the electrons closer to its end ● it will have a slight negative charge (δ⁻) ● other will have slight positive charge (δ⁺) ● leads to a charge difference called a dipole ● greater the difference in electronegativity, the greater the polarity of the bond
43
can dipoles be permanent?
yes
44
what are some elements with high electronegativity? (4)
● O ● F ● N ● Cl
45
what is polarity?
about the unequal sharing of electrons between atoms that are bonded covalently
46
how is bond polarity represented?
an arrow with a line at the end pointing to more electronegative atom
47
what do non polar molecules take into account? (2)
● all of the dipoles across the bonds of molecule ● for molecules that are symmetrical, dipoles of any bond within the molecule can cancel out
48
are all molecules containing polar bonds polar overall? (3)
● no ● if bond dipoles cancel each other the molecule isn't polar ● if there is a 'net dipole' the molecule will be polar
49
what are the types of intermolecular forces? (3)
● van der waals ● dipole-dipole ● hydrogen bonding
50
what is the weakest intermolecular force?
van der waals
51
describe van der waal's forces (4)
● as electrons are constantly moving, an instantaneous dipole can occur in molecule / atoms that arent polar ● instantaneous dipole induces a new dipole in a neighbouring molecule ● now also polar, the two molecules are attracted to each other ● act between all atoms and molecules
52
what is an instantaneous dipole?
where electron density shifts to one end of the molecule
53
what affects the strength of van der waal's forces? (2)
● number of electrons ● more electrons means the stronger the instantaneous dipole will be
54
does melting point and boiling point increase with more van der waal's forces? (4)
● yes ● as number of electrons increases ● van der waal forces increases ● so, melting and boiling point increases (takes more energy to overcome)
55
describe dipole-dipole forces (3)
● polar molecules have permanent dipoles (negatively and positively charged end) ● δ+ end of the dipole in one molecule and the δ- end of the dipole in a neighbouring molecule are attracted towards each other ● act only between certain types of molecules
56
why do you get a higher boiling and melting point than expected for a given mass in molecules with dipole-dipole forces between them?
extra attraction between dipoles means more energy must be put in to separate molecules
57
what are the conditions needed for hydrogen bonding to occur? why? (3)
● only occurs when hydrogen is bonded covalently to fluorine, nitrogen or oxygen ● hydrogen has large charge density (small) and F, N and O are highly electronegative ● often attracted to lone pairs on O and N
58
what are the characteristics of molecules with hydrogen bonding?
● same as covalent and dipole dipole forces ● but 1/10 strength of regular covalent bond
59
what is the strongest intermolecular force?
hydrogen bonding
60
draw a diagram of hydrogen bonding
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chemistry: physical chemistry 1 (7 decks)

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