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chemical bonding Flashcards

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1
Q

ionic bonding

A

transfer of electrons and subsequent electrostatic attraction (between oppositely charged ions)

metals lose
non-metals gain

ions pack into ionic crystal lattice

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2
Q

covalent bonding

A

sharing of at least 1 pair of electrons by 2 non metal atoms

forming molecule

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3
Q

mono

A

1

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4
Q

di

A

2

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5
Q

tri

A

3

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6
Q

tetra

A

4

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7
Q

penta

A

5

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8
Q

ionic naming

A

metal first

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9
Q

valancy method writing formula

A

swap+drop charges
simplify with highest common factor

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10
Q

naming transition metal

A

stock notation

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11
Q

covalent bond

A

a sharing of at least one pair of electrons by two non-metal atoms

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12
Q

electronegativity

A

a measure of the tendency of an atom to attract a bonding pair of electrons
0- non polar covalent bond
greater EN, more polar the bond is
<0,5 - very weak polar covalent bond
1- polar bond
1,4- highly polar covalent bond
2.0- polar covalent

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13
Q

metallic bonding

A

being between a positive kernel and a sea of delocalised electrons

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14
Q

intramolecular bond

A

a bond which occurs between atoms within molecules

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15
Q

intermolecular force

A

a weak force of attraction between molecules or atoms of noble gases

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16
Q

viscosity

A

a measure of how easily a liquid flows

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17
Q

london (dispersion) forces (3)

A

experienced by all molecular substances
only van der waals force that exists between non polar molecules
due to attraction of 1 molecule to the nucleus of another

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18
Q

origin of london forces (4)

A

-as a result of random movement of electrons, a temporary, instantaneous dipole is set up in one molecule
-this causes the electrons of the neighbouring molecule to disperse when molecules come close to one another
-this results in an induced dipole forming
-the 2 temporary dipoles are then able to electrostatically attract each other

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19
Q

forces w noble gases

A

do not participate in bonding as have full set of valance electrons (stable)
BUT noble gas atoms interact w london forces between their atoms

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20
Q

dipole dipole forces (3)

A

occurs between permanently polar molecules
slightly positive side of molecule attracts slightly negative of another
electron pair lives closer to the atom

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21
Q

origin of dipole dipole forces

A

-as a result of polar bonds (an unequal sharing of an electron pair as a result of END) and permanent asymmetrical distribution, these molecules are permanently polar
- and experience an attractive electrostatic force between the slightly positive side of one molecule and the slightly negative side of another molecule

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22
Q

hydrogen bond forces (2)

A

special case of dipole dipole forces
involves highly polar molecules

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23
Q

origin of hydrogen bond forces (3)

A

-within a molecule, a hydrogen atom must be covalently bonded to a small highly electronegative (N,O,F) atom (producing a greater END difference than in other polar bonds) with at least one pair of electrons
-within a molecule, a small highly electronegative atom attracts the bonded pair of electrons away from the covalently bonded hydrogen atom
-therefore, a naked proton is exposed and is attracted to a lone pair of electrons on another small highly electronegative atom of a neighbouring molecule , hence the forces exist between molecules

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24
Q

why are hydrogen bonds stronger than dipole dipole forces

A

-large END in bonds of molecule, making highly polar molecules with high charge density on exposed H atom
- the small atoms form molecules that can get close together and thus the forces act over shorter distances

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25
Q

substances that experience hydrogen bonding between their molecules

A

-water
-ammonia
-hydrogen fluoride
-alcohols
-carboxylic acids

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26
Q

hydrogen bonds in water

A

on average, each H20 molecule forms 4 hydrogen bonds with another H20 molecule at sites:
the 2 slightly hydrogen atoms
the 2 lone pairs on each atom oxygen atom

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27
Q

hydrogen bonds in ammonia

A

on average, each NH3 molecule forms 2 hydrogen bonds w other NH3 molecules at sites:
single lone pair on N atom
one of the slightly hydrogens (other 2 are wasted as there are insufficient lone pairs )

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28
Q

hydrogen bonds in hydrogen fluoride

A

on average, each HF molecule forms 2 hydrogen bonds w other HF molecules at sites:
-the single slightly positive hydrogen
-one of the lone pairs on the fluoride atom (other 2 lone pairs are wasted as there are insufficient slightly positive atoms on molecules)

29
Q

properties of diamond

A

(C)-4
giant covalent structure
extremely strong, high MP+BP—many strong covalent bonds between atoms—more energy required to break bonds
poor electrical conductor-no charges in lattice to move + carry charge

30
Q

properties of graphite

A

(C) -3 therefore unpaired e-

giant covalent structure
high MP+BP—many strong covalent bonds between atoms—more energy required to break bonds
sheets of carbon atoms held together by weak electrostatic forces (London)
good conductor of electricity- delocalised e-

31
Q

why does diamond have higher MP+BP than graphite

A

more energy required to break larger no of covalently bonds in diamond (4>3)

32
Q

silicon dioxide

A

SiO2

giant covalent structure
high MP+BP—many strong covalent bonds between atoms—more energy required to break bonds
poor electrical conductor-no charges in lattice to move + carry charge

33
Q

atomic/covalent bonds

A

many strong covalent bonds between atoms

34
Q

ionic structures properties

A

ionic bonding
structure made up by many,strong electrostatic forces of attraction between cations and anions -melting point determined by strength of these forces
brittle- shift in arrangement of ions brings like charges alongside each other which results in force of repulsion which causes solid to fracture
can’t conduct in solid state (cations +anions not free to move to carry charge)
- molten+ aqueous

35
Q

metallics structures

A

metallic bonding
structure made up by many strong electrostatic forces of attraction between positive kernels + delocalised valence electrons
good electrical conductors - delocalised e-‘s can move over positive kernels
malleable-sheets of cations can slide past over each other but remains held together by electrostatic forces of attraction between delocalised electrons and cations

36
Q

malleability

A

sheets of cations can slide over e-‘s but remiannheld tiegther by forces

37
Q

interactions in non metal atoms (excl noble gases)

A

intramolecular bond, specifically covalent bonding

38
Q

interactions in noble gas atoms

A

intermolecular forces , specifically london forces only

39
Q

interactions in molecules

A

intermolecular forces, specifically london, dipole-dipole + hydrogen bond forces

40
Q

interactions in metal atoms

A

electrostatic force of attraction in a metallic bond

41
Q

interactions in ions

A

electrostatic forces of attraction in an ionic bond

42
Q

what do MP+BP indicate

A

indicators of collective strength of forces holding substances together (increased strength - more energy to overcome forces - higher MP/BP)

43
Q

intramolecular bond

A

bond between atoms w/in molecules

44
Q

heating in molecular substances

A

as substance is heated-temp +average Ek of molecules increases- more energy provided to overcome come/break forces of attraction between molecules-changing physical properties of substances
( intramolecular/covalent bonds not broken by heating , only IMF forces broken or electrostatic forces of attraction overcome)

45
Q

factors that influence strength of IMFs

A

-the type of IMF force (predom. and add. london force)
-no. of electrons in molecule (indicated by molar mass) which affects size of temporary dipoles formed which influences strength of london forces
-no of IMF forces which influences strength of hydrogen bond forces
-interacting surface area of molecules which affects london forces in organic substances

46
Q

mp + bp questions

A

-identity types of IMFs present in both molecules
-compare relative strengths of IMF influenced by diff factors
-“more energy is required to overcome the collective stronger IMFs”
-conclude which substance has higher or lower BP/MP

47
Q

what does phase of substance depend on

A

strength of IMF forces that hold it together

48
Q

phases:liquids and SOLIDS

A

IMFs so strong- movement of molecules is limited

49
Q

phases:gases

A

no or very weak IMFs between molecules

50
Q

what happens when a PD is applied

A

charged particles move resulting in a current

51
Q

what determines density

A

mass/volume (constant for substance at any temp) (molar mass indicator of density)
IMFs between molecules (greater attractive force= greater density, relative strength of IMFs in substance =greater density)
greater mass=greater density (at constant volumes)

52
Q

solubility in ionic compounds

A

ions are attracted by polar water molecules of solvent
IMFs in each substance must be similar in nature and magnitude

53
Q

solubility of covalent compounds

A

dependent on polarity of solute + solvent (like)
nature+ magnitude of forces between molecules of each substance ( like)
predominant IMF of solute important

54
Q

how to collect non polar gases

A

downward displacement of water
gas bubbled through up turned cylinder filled w water
gas rises through H20 and is collected, H2O pushed down

55
Q

collect polar gases

A

upward + downward displacement of air
(diff gases have diff densities relative to air which is mostly nitrogen)
higher density than air -air pushed up, gas sinks
lower density than air- air pushed down,gas rises

56
Q

electronegativity

A

measure of tendency of atom to attract a bonding pair of e-‘s

57
Q

END=0

A

equal sharing of bonding pair of electrons as both atoms have same tendency
therefore non polar (pure) covalent

58
Q

non polar covalent molecule

A

an equal sharing of electrons

59
Q

END>0

A

unequal sharing of bonding pair of electrons as both atoms have diff tendencies hence polar covalent bond

60
Q

polar covalent bond

A

unequal sharing of electrons leading to a dipole forming (as a result of END)

61
Q

molecule w END=0

A

non-polar covalent bond
non polar molecule
experiences london forces

62
Q

molecule w END>0 and e- symmetry

A

polar covalent bond
non polar molecule
london forces only

63
Q

END >0 w no e- symmetry

A

polar covalent bond
polar molecule (hydrogen bond force +LF OR dipole-dipole force + LF)

64
Q

molecular substances mp+bp

A

affected by strength and relative no per molecule of IMF forces

65
Q

polar covalent

A

unequal sharing of electrons leading to a dipole forming
the greater the END, the more polar the bond

66
Q

shapes

A

Linear (HCl, CO2)
Trigonal planar (BF3)
Tetrahedral (CH4)
Pyramidal (NH3, sides under side)
bent/angular (H20, ^)

67
Q

molecular polarity

A

if bonds non polar covalent - non polar molecule
if bonds are polar covalent :
- if symmetry in molecules electron cloud - non polar
else polar

68
Q

non polar molecule

A

electron symmetry or END= 0
london forces only

69
Q

polar molecule

A

polar covalent bonding (END> 0)
no electron symmetry
dipole dipole + london or
hydrogen bond + london

physics (36 decks)

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