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bonding Flashcards

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1
Q

ionic bonding

A

oppositely charged ions attract through electrostatic forces to form a giant ionic lattice

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2
Q

sulfate formula

A

SO4 2-

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3
Q

hydroxide formula

A

OH-

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4
Q

nitrate formula

A

NO3 -

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5
Q

carbonate formula

A

CO3 2-

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6
Q

ammonium formula

A

NH4 +

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7
Q

single covalent bond

A

shared pair of electrons between two outer shells in order to achieve full outer shell

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8
Q

multiple covalent bond

A

multiple pairs of electrons shared

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9
Q

co-ordinate (dative covalent) bond

A

shared pair of electrons with both electrons supplied by one atom

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10
Q

how to represent covalent or coordinate bond

A

covelant using a line
coordinate using an arrow from the lone electron pair

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11
Q

metallic bonding

A

strong electrostatic force of attraction between delocalised electrons and positive ions arranged in a lattice

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12
Q

four types of crystal structure

A

ionic
metallic
macromolecular
simple molecular

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13
Q

crystal structure of diamond

A

macromoleular

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14
Q

crystal structure of graphite

A

macromolecular

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15
Q

crystal structure of ice

A

simple molecular

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16
Q

crystal structure of iodine

A

simple molecular

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17
Q

crystal structure of magnesium

A

metallic

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18
Q

crystal structure of sodium chloride

A

ionic

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19
Q

MP of macromolecular structures

A

very high mp as multiple covalent bonds to overcome which are very strong

20
Q

MP and conductivity of simple molecular

A

usually low mp due to IDD but depends if PDD or hydrogen bonding
very poor conductors as no charged particles

21
Q

MP and conductivity of ionic strucutres

A

high MP as strong electrostatic forces
conducs electricity in molten or solution as ions seperate so free to move and carry a flow of charge

22
Q

MP and conductivity of metallic substances

A

high mp due to strong electrostatic forces of attraction
high melting poins nealry alwasys solid at room temp

23
Q

explain the energy changes associated with changes of state

A

as temp rises kinetic energy of the particle increases

24
Q

bonding pairs and lone pairs of electrons are

A

charge clouds that repel each other

25
Q

arrangement of pairs of electrons in outershell of atom

A

arrange themselves as far apart as possible to minimise repulsion

26
Q

lone pair, bond pair replusion comparison

A

lone pair-lone pair repulsion> lone pair- bond pair> bond pair-bond pair

27
Q

effects of electron pair replusion on bond angles

A

lone pair- lone pair replusion reduced the bond angle

28
Q

bonding pairs , lone pairs , bond angle of linear

A

2
0
180

29
Q

bonding pairs , lone pairs , bond angle of trigonal planar

A

3
0
120

30
Q

bonding pairs , lone pairs , bond angle of tetrahedral

A

4
0
109.5

31
Q

bonding pairs , lone pairs , bond angle of trigonal biprymidal

A

5
0
120 and 90

32
Q

bonding pairs , lone pairs , bond angle of octahedral

A

6
0
90

33
Q

bonding pairs , lone pairs , bond angle of v-shape

A

2
1
117.5
and
2
2
104.5

34
Q

bonding pairs , lone pairs , bond angle of see-saw

A

4
1
119 and 89

35
Q

bonding pairs , lone pairs , bond angle of square pyramidal

A

5
1
89

36
Q

bonding pairs , lone pairs , bond angle of triangular pyramid

A

3
1
107

37
Q

bonding pairs , lone pairs , bond angle of t-shape

A

3
2
89

38
Q

bonding pairs , lone pairs , bond angle of square planar

A

4
2
90

39
Q

electronegativity

A

the power of an atom to attract the pair of electrons in a covalent bond

40
Q

trend in electronegativity down a group and across a period

A

decreases down a group as shielding increases
increases across a period as atomic radius decreases

41
Q

causes of permentant dipole

A

electron distribution in a covalent bond between elements with different electronegativities will be unsymmetrical which produces a polar covalent bond and may cause molecule to have permentant diploe

42
Q

explain why some molecules with polar bonds do not hvae a permentant dipole

A

non-polar molecule may still contain polar bonds and the presence of symmetrical bonds in a molecules means that the delta charges cancel each other out so no permentant diople formed

43
Q

3 main types of intermoleuclar forces

A

induced dipole dipole
permeant diploe dipoles
hydrogen bonding

44
Q

how are melting and boiling points of simple molecular substances influenced by the strenth of these intermolecular forces

A

IDD- weakest type of intermolecular force, larger the mr the stronger the intermolecular force higher the melting point (generally lower mp though)
PDD- stronger intermolecular forces than IDD weaker than hydrogen bonding of similar sized molecules, mid melting and boiling point
Hydrogen bonding- much higher melting and boiling points compared to similar sized molecules without hydrogen bonding

45
Q

how does hydrogen bonding arise

A

forms between hydrogen and the 3 most electronegative atoms(nitrogen, oxegon and flourine). the lone pair on NOF attracted to the delta positive on hydrogen (shown with a dotted line)

46
Q

importance of hydrogen bonding in the low density of ice and anomalous boiling points of compounds

A

low densisty of ice- water molecules become arranged into 3D networks where each water molecule is connected to 4 other water molecules by hydrogen bonds so the water molecules in solid ice are further apart than the molecules in liquid water
anomalous boiling point- requires more energy to break its hydrogen bonds before it can begin to boil

Chem (33 decks)

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