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bonding Flashcards

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1
Q

ionic bonding def

A

the electrostatic force of attraction between oppositely charged ions

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2
Q

when is ionic bonding stronger and the mp higher

A

when the ions are smaller and have higher charges

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3
Q

why are positive ions smaller

A

it has one less shell of electrons;
ratio of protons to electrons has increased so there is a stronger attraction to hold the remaining electrons

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4
Q

why are negative ions bigger

A

negative ions have more electrons than the element, but the same number of protons;
the attraction from the nucleus is shared over more electrons, making it weaker and the ions bigger

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5
Q

trend in ionic radii down a group

A

size of ionic radii increases;
as you go down the ions have more shells

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6
Q

covalent bond

A

the electrostatic force of attraction between the nuclei and bonding pair of electrons

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7
Q

dative/coordinate covalent bond

A

when the shared pair of electrons come from only one of the bonding atoms
e.g. NH4+, H3O+

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8
Q

metallic bonding

A

the electrostatic force of attraction between rhetorical positive metal ions and the delocalised electrons

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9
Q

factors that affect the strength of metallic bonds

A
  1. number of protons/strength of nuclear charge (more positive=stronger bond)
  2. number of delocalised electrons (more delocalised electrons=stronger bond)
  3. size (smaller ion=stronger bond)
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10
Q

why does Mg have stronger metallic bonding than Na

A

the metallic bonding gets stronger because Mg has more electrons that become delocalised;
Mg ion is smaller and has one more proton so a higher nuclear charge;
stronger electrostatic force of attraction between the positive metal ions and the delocalised and more energy is needed to break bonds

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11
Q

structure of compounds w ionic bonds

A

giant ionic lattice
e.g. sodium chloride (NaCl), magnesium oxide (MgO)

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12
Q

structure of compounds w weak covalent bonds

A

simple molecular;
vdw, permanent dipoles, H bonds between molecules
e.g. iodine, CO2, H2O, CH4

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13
Q

structure of compounds w strong covalent bonds

A

macromolecular;
e.g. diamond, graphite, silicon dioxide, silicon

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14
Q

structure of compounds w metallic bonds

A

giant metallic lattice
e.g. magnesium, sodium, all metals

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15
Q

melting and boiling points of ionic compounds/lattices

A

high;
because of giant lattice of ions with strong electrostatic forces between oppositely charged ions

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16
Q

solubility in water of ionic compounds

A

generally good

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17
Q

conductivity of ionic compounds when solid

A

poor; ions can’t move / fixed in place

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18
Q

conductivity of ionic compounds when molten

A

good; ions can move

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19
Q

melting and boiling points of simple molecular molecules

A

low; because of weak IM forces between molecules

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20
Q

solubility in water of simple molecular compounds

A

generally poor

21
Q

conductivity of simple molecular molecules when solid

A

poor; no ions to conduct and electrons are fixed in place

22
Q

conductivity of simple molecular molecules when molten

A

poor; no ions

23
Q

melting and boiling points of macromolecular substances

A

high;
because of many strong covalent bonds in macromolecular structure;
takes a lot of energy to break the strong bonds

24
Q

solubility in water of macromolecular substances

A

insoluble

25
Q

conductivity of macromolecular substances when solid

A

diamond and sand: poor;
because electrons can’t move (localised);
graphite: good;
as free delocalised electrons between layers

26
Q

conductivity of macromolecular substances when molten

A

poor

27
Q

melting and boiling points of metallic structures

A

high;
strong electrostatic forces between positive ions and delocalised sea of electrons

28
Q

solubility in water of metallic structures

A

insoluble

29
Q

conductivity of molten substances when solid

A

good;
delocalised electrons can move through structure

30
Q

conductivity of metallic structures of molten

A

good

31
Q

linear molecules

A

2 bonding pairs, no lone pairs, 180°
e.g. CO2, CS2, HCN, BeF2

32
Q

trigonal planar

A

3 bonding pairs, no lone pairs, 120°
e.g. BF3, AlCl3, SO3

33
Q

tetrahedral molecules

A

4 bonding pairs, no lone pairs, 109.5°
e.g. SiCl4, SO4^2-, ClO4^-, NH4^+

34
Q

trigonal pyramidal molecules

A

3 bonding pairs, 1 lone pair, 107°
e.g. NCl3, PF3, ClO3, H3O^+

35
Q

bent molecules

A

2 bonding pairs, 2 lone pairs, 104.5°
e.g. OCl2, H2S, OF2, SCl2

36
Q

trigonal bipyramidal

A

5 bonding pairs, no lone pairs, 120° and 90°
e.g. PCl5

37
Q

octahedral

A

6 bonding pairs, no lone pairs, 90°
e.g. SF6

38
Q

electronegativity

A

the ability for an element to attract a lone pair of electrons in a covalent bond

39
Q

factors affecting electronegativity

A

electronegativity increases as:
nuclear charge increases and atomic radii decreases because electrons are pulled in more so there’s a stronger attraction

40
Q

why does electronegativity decrease down the group

A

the distance between the nucleus and the outer electrons increases and the shielding of inner shell electrons increases

41
Q

formation of a permanent dipole

A

a polar covalent bond forms when the elements in the bond have different electronegativities;
when a bond is polar, it has an unequal distribution of electrons and produces a charge separation

42
Q

symmetric molecule

A

all bonds identical; no lone pairs;
not polar even if individual bonds within the molecule are polar
e.g. CO2

43
Q

van der waals

A

occurs between all molecular substances and noble gases;
not in ionic substances

44
Q

factor affecting size of vdw

A

the more electrons there are, the higher the chance that temporary dipoles will form,
this makes the vdw stronger between molecules so bp will be greater

45
Q

explain the reason for increasing boiling points down group 7

A

increasing number of electrons, causing an increase in the size in vdw;
iodine is solid and chlorine is a gas

46
Q

why do longer chain alkanes have stronger vdw

A

have a larger SA of contact between molecules for vdw to form than spherical shaped and branched alkanes, so stronger vdw

47
Q

permanent dipole

A

occurs between polar molecules;
stronger than vdw so have higher bp;
commonly compounds with C-Cl, C-F, C-Br, H-Cl, C=O;
asymmetrical and have a bond where there’s a significant difference in electronegativity

48
Q

hydrogen bonding

A

when H is attached to the 3 most electronegative elements; F, O, N
strongest IM force

chemistry (5 decks)

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