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Chemistry 1A > Week Five > Flashcards

Week Five Flashcards

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1
Q

How electrons arrange

A

arrange themselves as far away as possible

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2
Q

Lewis model - deficiencies

A

H2 and F2 are treated equivalently by lewis dot model

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3
Q

Valence bond theory

A

assumes electrons in a molecule occupy atomic orbitals

presumes electron density is equally shared

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4
Q

sigma bond

A

a single bond that is formed by the overlap of the 2 1s shells

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5
Q

overlap of a s and p orbital

A

sigma bond

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6
Q

every first bond

A

sigma bond

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7
Q

Hybridisation

A

when covalent bonds are formed atomic orbitals mix or hybridise to form new sets of orbitals

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8
Q

how many orbitals in hybridisation

A

must have the same amount as started with

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9
Q

pi bonds

A

formed by the sideways overlap of 2p orbitals

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10
Q

electron density - pi bonds

A

above and below the axis joining the two atoms

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11
Q

sigma bond strength

A

stronger than pi bonds because sideways overlap is not as effective as the end on bond

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12
Q

single bond

A

sigma

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13
Q

double bond

A

one sigma one pi

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14
Q

triple bond

A

one sigma and 2 pi

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15
Q

sp

A

linear

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16
Q

sp2

A

trigonal

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17
Q

sp3

A

tetrahedral

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18
Q

sp3d

A

trigonal byprimidal

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19
Q

sp3d2

A

octahedral

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20
Q

Molecular orbital theory - predictions

A

accurate structures
dissociation energies
line positions
paramagnetism and diamagnetism

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21
Q

molecular orbital theory - molecular bonds

A

treat them as a sharing of electrons between 2 nuclei

treats as delocalised, spread out

22
Q

bonding orbital

A

has lower energy so more stable

fills first

23
Q

anti bonding orbital

A

has higher energy less stable

will fill last

24
Q

sigma orbital

A

bonding molecular orbital with cylindral symmetry about an inter nuclear axis

25
Q

bond order

A

stability of molecule

1/2 ( electrons in bonding orbital - number in anti bonding orbitals)

26
Q

net bond order of 0

A

wont form bond

27
Q

diamagnetic

A

no unpaired spins, cant interact in a magnetic field

28
Q

paramagnetic

A

has unpaired spins

29
Q

Heteronuclear diatomics

A

if they have same electronegativity they have similar diagram to homonuclear

30
Q

Acids

A

sour taste
corrosive
conduct electricity

31
Q

bases

A

bitter
soapy
corrosive
conduct electricity

32
Q

strong

A

dissociates fully in water

33
Q

weak

A

partially dissociates

34
Q

Arrenhius acids and bases

A

form solvated hydrogen cations written as H+ or H3O+

Arrenhius bases form hydroxide OH-

35
Q

Bronsted Lowry acids bases

A

acids are protons donors

bases proton acceptors

36
Q

Lewis acid and bases

A

acids act as electron pair acceptors

bases act as electron pair donors

37
Q

Monoprotic acids

A

acids ionise to form one H+ ion for every acid molecule

38
Q

Diprotic acids

A

produces 2H+ ions for every acid molecule

39
Q

Kw

A

equilibrium constant

[H3O+][OH-]

40
Q

ph

A

-log[substance]

41
Q

strong bases

A

fully dissociate in water to give metal cation and hydroxide ions `

42
Q

neutralisation reactions

A

when acids and bases are mixed

43
Q

pOH

A

-log[OH-]

44
Q

pH + pOH

A

14.00 at 25 degrees

45
Q

acidity constant

A 
       [HA]
46
Q

Acid constant equation

A

HA +H2O => H3O+ + A-

47
Q

Basicity constant

A 
     [B]
48
Q

Basicity constant equation

A

B + H2O => BH+ + OH-

49
Q

Ka + Kb

A

Kw

50
Q

tha larger the Ka value

A

stronger the acid

51
Q

the smaller the pKa value

A

stronger the acid

Chemistry 1A (12 decks)

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