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IB CHEM HL > Topic 4 + 14 > Flashcards

Topic 4 + 14 Flashcards

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1
Q

4 allotropes of carbon

A

graphene, graphite, diamond, C60

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2
Q

bonding of graphite

A
  • each carbon is bonded to 3 other carbons
  • all carbons are sp2 hybridized
  • layers are held together by London Dispersion Forces
  • weak intermolecular forces
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3
Q

bonding of diamond

A
  • each carbon is bonded to 4 other carbons
  • all carbons are sp3 hybridized
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4
Q

bonding of C60

A
  • each carbon is bonded to 3 other carbons
  • all carbons are sp2 hybridized
  • carbons form 60 member sphere
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5
Q

bonding of graphene

A
  • each carbon is bonded to 3 other carbons
  • all carbons are sp2 hybridized
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6
Q

physical properties of graphene (that make it useful)

A
  • good electrical conductor
  • good thermal conductor (best)
  • strong
  • high melting point
  • flexible
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7
Q

physical properties of graphite

A
  • good electrical conductor
  • low thermal conductivity
  • high melting point
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8
Q

physical properties of diamond

A
  • not electrical conductive
  • very high thermal conductivity
  • high melting point
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9
Q

physical properties of C60

A
  • semi electrical conductor
  • very low thermal conductivity
  • low melting point
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10
Q

elemental silicon

A
  • lot like diamond
  • each silicon atom is covalently bonded to 4 other silicon atoms
  • all silicon is sp3 hybridized
  • results in giant lattice structure
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11
Q

silicon dioxide (SiO2)

A
  • silica / quartz
  • giant covalent structure based on tetrahedral arrangement
  • each silicon atom is bonded to 4 oxygen atoms
  • each oxygen atom is bonded to 2 silicon atoms
  • strong
  • insoluble
  • high melting point
  • non-conductor of electricity
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12
Q

carbonate

A

C03 2-

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13
Q

sulfate

A

SO4 2-

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14
Q

nitrate

A

NO3 -

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15
Q

hydroxide

A

OH -

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16
Q

hydrogencarbonate

A

HCO3 -

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17
Q

ammonium

A

NH4 +

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18
Q

phosphate

A

PO4 3-

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19
Q

transitional metals

A
  • have electron configuration that allows them to lose different # of electrons from their d sub-shell
  • form stable ions with different charges -> these ions would have distinct properties such as colors
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20
Q

Silver ion charge

A
  • Ag+ always
  • never write oxidation number
21
Q

oxidation number

A

symbols come before numbers
e.g. +2 instead of 2+

22
Q

Tin

A

Sn

23
Q

Mercury

A

Hg

24
Q

formation of ionic bonds

A
  • electrostatic attraction between oppositely charged ions
  • ions form through the process of ionization: electrons are transferred between atoms
25
Q

ionic lattice

A
  • 3D crystalline structure formed by ionic compounds
  • always involves fixed arrangement of ions based on repeating units
26
Q

coordination number

A

number of ions that surround a given ion in a lattice

27
Q

lattice energy

A
  • measure of strength of attraction between ions in a lattice
  • great for ions that are small & highly charged (up, right on periodic table) bc they have larger charge density
28
Q

physical properties of ionic compounds

A
  • higher MP & BP: electrostatic attractions btwn ions in lattice are strong -> require large amount of energy to break
  • solid at room temp
  • conduct electricity when molten or in aqueous solution since ions are free to move
  • cannot conduct electricity when solid as ions are held in fixed positions & cannot move
29
Q

melting point & boiling point

A
  • higher when charge on ion is greater <- due to increased attraction btwn ions

e.g. MP of MgO > Na2O (Mg: 2+, Na: 1+)

30
Q

solubility

A
  • determined by the degree to which separated particles of solute are able to form bonds/attractive forces with solvent
  • ionic compounds: polar solvents
  • covalent compounds: polar compounds -> polar solvents, nonpolar compounds -> nonpolar solvents
  • metallic compounds: insoluble
31
Q

hydration

A
  • told by (aq)
  • substance now exists as individual ions surrounded by water molecules
32
Q

brittleness

A
  • brittle: shatter when large force is applied
  • ionic compounds: brittle bc movement of ions within lattice places ions of same charge next to each other -> repulsive forces cause the crystal to split
33
Q

electronegativity

A

≤ 0.4: non-polar
<1.8: covalent
≥ 1.8: ionic

34
Q

aluminum chloride (AlCl3)

A
  • solid: ionic, AlCl3
  • molten (liquified by heat): separates into Al2Cl6 molecules instead of its ions
  • gas: ionic, AlCl3
35
Q

allotropes

A

different forms of same chemical element in same physical state

36
Q

delocalized

A

when electrons are not restricted to one location

37
Q

giant molecular structure / network covalent structure

A
  • crystalline lattice in which atoms are linked by covalent bonds
38
Q

relative strength of intermolecular forces

A

hydrogen bonds > dipole-dipole forces > London dispersion forces

39
Q

London dispersion forces

A
  • temporary/instantaneous dipole: weak dipole formed when density of electrons at one point is greater over one region of molecule/atom
  • induced dipole: caused when temporary dipole affects the electron distribution of a neighbor atom/molecule
  • LDF: result of induced dipole
  • strength increases with molecular size bc greater # of electrons increase chance of temporary dipoles developing
  • only force that exists btwn non-polar molecules
40
Q

physical properties of non-polar molecules

A
  • gas at room temp
  • low MP & BP as relatively little E is required to break weak intermolecular forces
41
Q

dipole-dipole attraction

A
  • permanent dipole: permanent separation of charge within bonds due to electronegativity difference btwn bonded atoms (in polar molecules), one end is δ+ while the other end has δ-
  • dipole-dipole attraction: force of attraction caused when permanent dipoles result in opposite charges on neighboring molecules attracting each other
  • vary depending on distance & relative orientation of dipoles
  • cause MP & BP of polar substances to be higher than those of non-polar substances of comparable molar mass
  • lead to solubility of polar solutes in polar solvents
42
Q

Van der Waals’ forces

A
  • umbrella term to include LDF, dipole-dipole attractions & dipole-induced dipole forces
43
Q

hydrogen bond

A
  • molecule containing hydrogen bonds to very electronegative atom (F, O or N) -> molecules attracted to each other by a particularly strong type of intermolecular force
  • large EN difference results in electron pair being pulled away from H -> H has exposed proton & exerts strong attractive force on lone pair in electronegative atom of a neighboring molecule
44
Q

conductivity of covalent compounds

A
  • not able to conduct electricity in solid & liquid state since they don’t contain ions
45
Q

metalic bond

A
  • electrostatic attraction btwn lattice of positive ions & delocalized electrons
  • strength depends on # of delocalized ions, charge of cation & radius of cation
46
Q

metal alloy

A
  • substance that combines more than one metal or mixes a metal with other non-metallic elements
    e.g. brass: copper & zinc
47
Q

physical properties of metallic compounds

A
  • good electrical conductivity: delocalized electrons are highly mobile so they can move through metal structure under applied voltage
  • good thermal conductivity: delocalized electrons & close packed cations enable efficient transfer of heat energy
  • high MP & BP: lots of energy is required to break strong metallic bonds & separate atoms
  • ductile (can be drawn out into threads): movement of delocalized electrons are non-directional and random so metallic bonds remain intact while conformation changes under applied pressure
  • malleable (can be shaped under pressure)
48
Q

sigma bond

A
  • formed by direct head-on/end-to-end overlap of atomic orbitals resulting in electron density concentrated between the nuclei of the bonding atoms
  • hybridized
49
Q

pi bond

A
  • sideways overlap of atomic orbitals resulting in electron density above and below the plane of the nuclei of the bonding atoms
  • unhybridized, p bond
  • weaker than sigma bonds, can only form after one sigma bond has been formed

IB CHEM HL (5 decks)

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