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chemistry A1 physical > Bonding > Flashcards

Bonding Flashcards

(67 cards)

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1
Q

Explain the structure present in Ionic bonding

A

giant ionic lattice

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2
Q

describe the bonding present in ionic bonding

A

strong electrostatic forces of attraction between oppositely charged ions

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3
Q

what is the formula for sulphate ions

A

SO₄²-

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4
Q

what is the formula for a hydroxide

A

OH-

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5
Q

what is the formula for nitrate

A

NO3-

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6
Q

what is the formula for carbonate

A

CO₃²⁻

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7
Q

what is the formula for ammonium

A

NH4+

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8
Q

how can you represent a co-ordinate bond

A

an arrow

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9
Q

what is a co-ordinate/ dative bond

A

shared pair of electrons with both electrons being supplied by one atom

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10
Q

what does metallic bonding involve

A

electrostatic forces of attraction between positvely charged ions and the delocalised electrons

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11
Q

how are the positive ions arranged in metallic bonding

A

in a giant metallic lattice

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12
Q

what are the 4 types of crystal stuctures

A

-ionic
-metallic
-macromolecular
-simple molecular

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13
Q

what shape has 2BP 0LP

A

Linear

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14
Q

what shape has 3BP 0LP

A

trigonal planar

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15
Q

what shape has 2BP 1LP

A

Bent/ Angular

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16
Q

what shape has 4BP 0LP

A

tetrahaedral

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17
Q

what shape has 3BP and 1LP

A

trigonal pyramidal

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18
Q

what shape has 2BP 2LP

A

Bent/ Angular

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19
Q

what shape has 5BP and 0 LP

A

trigonal bipyramid

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20
Q

what shape has 4BP 1LP

A

Seesaw

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21
Q

what shape has 3BP 2LP

A

T-Shape

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22
Q

what shape has 2BP 3LP

A

Linear

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23
Q

what shape has 6BP and 0LP

A

Octaehaedral

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24
Q

what shape has 5BP 1LP

A

sqaure pyramid

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25
what shape has 4BP 2LP
square planar
26
what shape has 3 BP 3LP
T-shape
27
what shape has 4BP 2LP
Linear
28
what s the bond angle in a linear shape
180 degrees
29
what is the bond angle in a trigonal planar
120 degrees
30
what is the bond angle in a tetrahaedral
109.5
31
what is the bond angle in a trigonal bipyramidal
90 degrees
32
what is the bond angle in a seasaw
90 120 degrees
33
what is the bond angle in an octahedral
90 degrees
34
what is the bond angle in a square planar
90 degrees
35
why do lone pairs of repulsion reduce the bond angle by 2.5 degreees
they arrange themselves as far apart as possible to minimise repulsion
36
which type of repulsion is greaterr
lone-pair lone-pair
37
what is the second highest repulsion
lone-pair bond-pair
38
what is the least type of repulsion
bond-pair bond-pair
39
what is meant by the term electronegativity
the power to attract electrons in a covalent bond
40
what may cause a polar covalent bond
when the electronegativites are unsymmetrrical
41
what are the different types of intermolecular forces
permanent dipole-dipole hydrogen Van-Der Waal forcces
42
what is the strongest intermolecular force
hydrogen bondng
43
what is the least strongest type of intermolecular forces
Van-Der Waal forces
44
describe Van Deer Waal forces
-uneven distrubition of electrons in a molecule which induces a dipole in a neighbouring molecule -
45
Sodium fluoride contains (Na+) and (F-) and they both have the same electron configuration Explain why fluoride ions are larger than sodium ions
-fluoride ions have fewer protons -therefore nuclear charge decreases -weaker attraction between the nucleus and outermost electrons
46
describe how permanent dipole-dipole forces arise
-differences in electronegativity -the dipoles dont cancel out -attraction between delta positive and negative molecules
47
what can you conclude when there are no lone pairs
the electrons repel equally
48
explain why the electronegativity increases as you go across a period
-number of protons increases -atomic radius decreases -cause electrons are pulled more
49
explain why the electronegativity decreases as you go down the group
-distance between nucleus and outermost electrons increases -shielding also increases
50
what is a factor that affects the size of Van deer waal forces
the Mr -more electrons
51
what happens to the boiling point/ melting point when the van der waal forces incresease
it increseas
52
where do van der waal forces occur
in ALL molecules
53
what is the shape of polar molecules
asymmetrical
54
why do polar molecules occur
due to a differnece in the eelctronegativity
55
when are polar molecules fromed
when thee dipoles dont cancel out
56
give examples of a macromolecualr structure
-graphite -diamond
57
explain hydrogen bonding
when hydrogen is attached to nitrogen oxygen fluorine
58
what do nitrogen fluorine oxygen have in common
they are the most electronegative elements
59
what happens when theres a difference in the electronegativity
theres a permanent dipole
60
why do some molecules have a polar bond but they dont have a dipole
-dependant on the shape of the molecule - the dipoles cancel out
61
what happens when the arrows face opposite directons
no dipole non-polar
62
what happens when the arrows face opposite ddirectiosn
they cancel out and theres no dipole
63
what happens wwhen the arrows face the same direction
theres a dipole and the bond polarities dont cancel makes a polar molecule
64
where do permanent dipole-dipole forces occurs
molecules with a permanenet dipole
65
what is a single bond known as
sigma bond
66
what is a double bond known as?
pi bond
67
what is polar bond
a charge imbalance due to a difference in electronegativites

chemistry A1 physical (5 decks)

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