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S215 > Block 1 - The Periodic Table > Flashcards

Block 1 - The Periodic Table Flashcards

1
Q

What are the alkali metals

A

group 1 metals

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2
Q

What is a primary use of the alkali metals

A

As cations for OH- and CO32- ions because these ions are important in many reactions but do not dissolve in water readily apart from when bonded to the alkali metals

The alkali metals also won’t react with the intended reactants for the OH- and CO32- ions

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3
Q

describe the appearance of alkali metal halides

A

white crystalline solid

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4
Q

what are the characteristics of alkali metal halides

A

high melting temperature
melts are electrically conductive
dissolve in water to form colourless solutions which conduct electricity

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5
Q

what oxide does lithium form

A

Li2O

lithium burns with a lilac flame

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6
Q

what oxide does sodium form

A

Na2O2

O22- peroxide ion

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7
Q

what oxide do potassium rubidium and caesium form

A

MO2

O2- ion (small 2 at the bottom, single -ve charge)
superoxide ion

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8
Q

what happens when alkali metals are heated gently with H2

A

colourless crystal hydride MH formed

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9
Q

what is the appearance of fluorine

A

yellow gas

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10
Q

what is the appearance of chlorine

A

green-yellow gas

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11
Q

what is the appearance of bromine

A

deep red liquid

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12
Q

what is the appearance of iodine

A

shiny black solid

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13
Q

what happens when hydrogen halides dissolve in water

A

acid is formed

HF forms a weak acid (because H3O+ and F- ions form hydrogen bonds), the rest form strong acids

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14
Q

what are the possible valencies of the halogens

A

1,3,5,7

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15
Q

how do the halogens react with aluminium

A

AlX3 formed

AlF3 is ionic
AlCl3 is layered
AlBr3 and AlI3 are covalent dimers Al2X6

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16
Q

why are the noble gasses unreactive

A

they all have a full outer shell of electrons

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17
Q

what is unique about radon

A

it is alpha active so can cause damage if inhaled

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18
Q

how does metallic character vary down a group

A

increases

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19
Q

how does metallic character vary across a period

A

decreases

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20
Q

how does the maximum valency vary down a group

A

no change

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21
Q

how does the maximum valency vary across a period

A

increases

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22
Q

how does the melting temperature of group 1 and 2 metals vary down a group

A

decreases apart from Ca

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23
Q

how does the melting temperature of group 1 and 2 metals vary across a period

A

increases

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24
Q

how does the density of group 1 and 2 metals vary down a group

A

decreases apart from Li

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25
Q

how does the density of group 1 and 2 metals vary across a period

A

increases

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26
Q

how does the reactivity of group 1 and 2 metals vary down a group

A

increases

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27
Q

how does the reactivity of group 1 and 2 metals vary across a period

A

decreases

28
Q

what is Hund’s rule

A

in any sub shell there will be the maximum number of electrons with spins of the same sense

this leads to ground-state arrangements

(think monopoly)

29
Q

what is valency

A

the combining power of an element

however valence electrons refers to the number of electrons in the outer shell

30
Q

what are the 4 ways to define oxidation

A

addition of oxygen
removal of hydrogen
loss of electrons
increase in oxidation number

31
Q

what are the 4 ways to define reduction

A

removal of oxygen
addition of hydrogen
gain of electrons
decrease in oxidation number

32
Q

what is the rule for F when calculating oxidation number

A

always -1

33
Q

what is the rule for O when calculating oxidation number

A

-2 apart from in F2O

34
Q

what is the rule for H when calculating oxidation number

A

+1 apart from hydrides of elements with lower electronegativity (group 1)

35
Q

what is the rule for Cl, Br and I when calculating oxidation number

A

-1 apart from when with O or other halogens

36
Q

what is the lewis definition of an acid

A

a lone pair acceptor

37
Q

what is the lewis definition of a base

A

a lone pair donor

38
Q

what is the Arrhenius definition of an acid

A

a substance which contains hydrogen and releases H+ ions when dissolved in water

39
Q

what is the Arrhenius definition of a base

A

a substance which releases OH- ions when dissolved in water

40
Q

what is the Brønsted–Lowry definition of an acid

A

a proton donor

41
Q

what is the Brønsted–Lowry definition of a base

A

a proton acceptor

42
Q

what is the steric effect

A

when the shape of a molecule blocks bonding/reaction

43
Q

define repulsion axis

A

each pair of electrons (bonded or non bonded)

they define the shape of a molecule

44
Q

what are the rules regarding the strength of different inter-axis repulsion

A

lone pair-lone pair > lone pair-bond pair > bond pair-bond pair

triple bond > double bond > single bond

interactions at 90 degrees are stronger than those at 120 degrees

45
Q

what is special about lone pair positioning in trigonal bypyramidal shapes

A

they occupy equatorial positions (to limit interactions at 90 degrees)

leads to a T-shaped molecule

46
Q

what shape and bond angle does a molecule with 3 atoms take

A

linear

180

47
Q

what shape and bond angle does a water molecule take

A

V-shaped

104.5

48
Q

what shape and bond angle does a molecule with 4 atoms take

A

trigonal planar

120

49
Q

what shape and bond angle does a molecule with 5 atoms and a lone pair take

A

pyramidal

107.8

50
Q

what shape and bond angle does a molecule with 5 atoms take

A

tetrahedral

109.5

51
Q

what shape and bond angle does a molecule with 6 atoms take

A

trigonal bipyramidal

90 and 120

52
Q

what shape and bond angle does a molecule with 7 atoms take

A

octahedral

90

53
Q

what shape and bond angle does a molecule with 8 atoms take

A

pentagonal bipyramidal

90 and ?

54
Q

what shape and bond angle does a molecule with 4 atoms and 2 lone pairs take

A

square planar

55
Q

what is the bond angle in an alkene

A

122 from the carbon double bond to the hydrogen

117 between the hydrogens

56
Q

what shape does a molecule with 6 atoms and a lone pair take

A

square pyramidal

57
Q

define electronegativity

A

the power of an atom to attract electrons

58
Q

what are the trends in electronegativity in the periodic table

A

increases up and across the table

therefore metals have lower electronegativity than non-metals

59
Q

how is electronegativity measured

A

on the Pauling scale

60
Q

what electronegativity difference is the threshold for ionic bonding

A

one element >2 and the other <1.9

61
Q

what is the dipole moment and how is it calculated

A

it is the extent of charge separation (μ)

μ = qr

q = charge at the positive end (C)
r = distance between charges (m)
62
Q

what is 2 debye (D) equal to

A

3.336x10^-30Cm

63
Q

what are dipole moments affected by

A

electronegativity difference

position of non-bonded electron pairs

64
Q

what are London dispersion forces and what is their trend down a group

A

forces between instantaneous dipole and induced dipole

they increase down a group

65
Q

what is a resonance hybrid

A

each bond is a mix of dative and normal covalent bond so the bond length is somewhere between

66
Q

when does hydrogen bonding occur and how does its strength change down a group

A

when a H is bonded to the lone pair of electrons on N, O or F

strength decreases down a group

67
Q

how are the electrons described in metallic bonding

A

electron gas

group 1 and 2 and aluminium all bond this was
Al is the bet electrical conductor since it has 3 electrons free to move

S215 (3 decks)

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