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IB chemistry HL > chapter 4 > Flashcards

chapter 4 Flashcards

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1
Q

between what elements does ionic bonding occur?

A

metal and non-metal

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2
Q

between what elements does covalent bonding occur?

A

non-metals

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3
Q

what does isoelectronic mean

A

species with the same number of electrons

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4
Q

what happens in ionic bonding ?

A

electrons are transferred from one atom to another to form positive and negative ions

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5
Q

how are cations formed?

A

metals loosing an electron

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6
Q

how are anions formed?

A

non- metals gaining electrons

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7
Q

what determines the number of electrons lost or gained?

A

electron configuration

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8
Q

why does ionic bonding occur?

A

electrostatic attraction between oppositely charged ions

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9
Q

what is a giant structure?

A

no individual molecules

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10
Q

physical properties of ionic compounds?

A

high boiling points, low volatility, dont conduct electricity (when solid), soluble in water

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11
Q

what is volatility

A

how readily a substance evaporates

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12
Q

why do ionic compounds have low volatility?

A

strong electrostatic forces

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13
Q

how is a covalent bond formed?

A

electrostatic attraction between a shared pair of electrons and the positively charged nuclei

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14
Q

what happens when you add more bonds (double, triple)

A

bond strength increases

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15
Q

what is longer single bond or double bond

A

single bond

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16
Q

what is electronegativity

A

measure of the attraction of an atom in a molecule for the electron pair in the covalent bond

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17
Q

how does bonding polarity occur

A

difference in electronegativities of the bonded atoms

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18
Q

why do noble gases not have electronegativity values

A

because they do not form compounds

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19
Q

what bonds will atoms with highly different electronegativities form

A

ionic

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20
Q

what does a lewis structure show?

A

all the valence electrons in a covalently bonded species

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21
Q

what is the octet rule

A

atoms in a covalence bond have a tendency to have a shell of 8 electrons

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22
Q

what is a coordinate bond

A

a coordinate covalent bond is a type of covalent bond in which both electrons come from the same atom

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23
Q

how is a covalent bond shown?

A

an arrow

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24
Q

what are some exceptions to the octet rule?

A

Be and B

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25
Q

when do resonance structures form?

A

when there is more than one possible position for a double bond in a molecule

26
Q

what determines the shape of a molecule?

A

VSEPR theory (valence shell electron pair repulsion)

27
Q

what is the VSEPR theory?

A

paris of electrons in the valence shell of an atom repel each other and will therefore take up positions in space to minimise the repulsions

28
Q

what is the shape and bond angle of a molecule with 2 electron domains?

A

linear, 180

29
Q

what is the shape and bond angle of a molecule with 3 electron domains?

A

trigonal planar, 120

30
Q

what is the shape and bond angle of a molecule with 4 electron domains?

A

tetrahedral, 109.5

31
Q

what is an electron domain?

A

a pair of electrons

32
Q

what is the order of repulsion strength for pairs of electrons?

A

lp-lp>lp-bp>bp-bp

33
Q

what is the basic shape

A

arrangement of the electrons around the central atom

34
Q

what is a polar bond

A

one end is slightly less positive than the other (difference in electronegativity)

35
Q

if individual bonds are polar does that make the molecule polar

A

no, the symmetry of the molecule may cause the dipole moment of individual molecules to cancel out

36
Q

what are allotropes

A

different forms of the same element

37
Q

what is the structure of diamond

A

giant covalent, no individual molecules, four carbon bonds, tetrahedral array

38
Q

properties of diamond?

A

high melting and boiling point (covalent bonds), doesn’t conduct electricity, not soluble in water (forces between atoms are too strong)

39
Q

what is the structure of graphite ?

A

giant covalent structure, each carbon is linked to 3 others in trigonal planar, single layers connected with london forces

40
Q

what are properties of graphite?

A

conducts electricity, not soluble in water

41
Q

what is graphene?

A

a single layer of graphite

42
Q

what is the structure of C60 fullerene?

A

molecule, covalent bonds and london forces

43
Q

properties of fullerene?

A

insoluble in water, soluble in some organic substances, doesnt conduct electricity, forms 3 bonds

44
Q

give examples of intermolecular forces (van der waal)?

A

London dispersion forces, dipole-dipole forces and hydrogen bonding

45
Q

what are intermolecular forces?

A

forces between molecules

46
Q

what are intramolecular forces?

A

forces within a molecule

47
Q

how are london forces made?

A

temporary dipole-induced interactions

48
Q

what makes london forces become stronger?

A

as relative molecular mass increases

49
Q

what are hydrogen bonds?

A

interaction between an electronegative atom and a hydrogen atom

50
Q

what are the requirements for hydrogen bonding?

A

H atom is attached to a very electronegative atom: N, O or F

51
Q

what forces are broken down when covalent molecular substances are melted or boiled?

A

intermolecular forces, covalent bonds are NOT

52
Q

what are the van der waal forces from weakest to strongest?

A

london < permanent dipol-dipole < hydrogen

53
Q

what is solubility in intermolecular forces?

A

a substance will dissolve in a solvent if the intermolecular forces in the solute and solvent are similar

54
Q

what are the requirements for a substance to have hydrogen bonding?

A

soluble in water, because they are able to hydrogen bond to the water

55
Q

what is metallic bonding?

A

electrostatic attraction between the positive ions in the lattice and the delocalised electrons

56
Q

what is the structure of metals?

A

a regular lattice arrangement of positive ions surrounded by a ‘sea’ of delocalised electrons

57
Q

why are metals ductile?

A

non-directionality of the bonding

58
Q

what are alloys?

A

alloys are homogenous mixtures of two or more metals, or of a metal with a non-metal

59
Q

why are alloys stronger than pure metals?

A

because the atom sizes are different

60
Q

what determines the strength of a metallic bond?

A

charge of the ion and radius of the metal ion

IB chemistry HL (7 decks)

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