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Chemistry > Periodicity > Flashcards

Periodicity Flashcards

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1
Q

definition of periodic

A

repeating pattern; in properties of the elements

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2
Q

similarties of elements in the same group

A

have a similar outer electron configuration

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3
Q

similarities of elemens in a period

A

have outer electrons in the same principal energy level ( a new row atrts when an electron enters a new shell)

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4
Q

similartities of elements in the same block

A

within a given block , the final electron is added to an orbital of that type

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5
Q

atomic radius variation across period

A

-decreases across a period–> across a period electrons enter the same shell, but there is an increase in nuclear charge (shielding remains approx constant). thus the elctrostatic force of attraction of the nucleus on outer electrons increases, resulting in a decrease in radius

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6
Q

atomic radius down a group

A

down a group, e- enter a new shell. shielding increases, there is a smaller attraction of the nucleus on the outer e-. the increase in proton number down a group does not compensae for hte increase in shielding effect.

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7
Q

IE across a period

A

increases along a period (few exceptions)
-e- enter the same shell across a period therefore shielding remains apprx constant. the proton number increases, the radius deceases–> increase of attraction between nucleus and outer e-. more energy is required

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8
Q

IE down a group

A

decreases down a group
e- enter a new shell, shielding and atomic radii increase. decrease in electrostatic froce of the nucleus on the outer e-. less energy needed.

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9
Q

melting point of period2

A

Li and Be have metallic bonding
B and C are macromolecular (C has a smaller radius than B and C-C bonds are shorter and therefore stronger than B-B bonds)
N O F Ne are almost all the same
remember to put gases below 0 on graph

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10
Q

melting point of period 3

A

Na and Mg and Al just have metalli cbonding
Si is macromolecular
P4, S8 and Cl2 are all simple molecular. S8 hsa the highest and Cl2 has the lowest.
Ar is atomic and so the lowest

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11
Q

polarising power

A

the ability of a positive ion to distort the electron cloud of a neighbouring ion. a high positive charge density leads to high polarising power

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12
Q

bonding in AlCl3 and BeCl2

A

both metallic covalent chlorides
both have high polarising power leading to an electron pair sharing, giving rise to covalent character.
AlCl3 forms dimers and BeCl3 is polymeric

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13
Q

PCl3

A

liquid at room temp
trigonal pyramidal
covalent cimple molecular

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14
Q

PCl5

A

solid at room temp —>ionic lattice
when in the gas state–> trigonal bipyramidal
ionic made of [PCl4]+ [PCl6]-
PCl5 is an empirical formula

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15
Q

why is PCl3 a liquid but PCl5 a solid?

A

ionic interactions are stronger than the pd-pd in PCl3, more energy needed

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16
Q

ionic chlorides with water

A

they do not undergo hydrolysis, just dissolve and form ions

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17
Q

MgCl2

A

Mg2+ has a high enough charge density that gives MgCl2 some covalent character. this allows for partial hydrolyss of MgCl2 ONLY WITH HEATING.
MgCl2 + H2O —> Mg(OH)Cl(s) + HCl

18
Q

why cant solid MgCl2 be prepared by heating a solution of MgCl2?

A

it will undergo partial hydrolysis, therefore cannot be heated until crystallisation

19
Q

reactions of chlorides of Li, Be,B ,C and N with water

A

LiCl Li+ and Cl-
BeCl2 + H2O —. Be(OH)2 + HCl
BCl3 + H2O —> H3BO3(s) + HCl boric acid
CCl4 no hydrolysis
NCl3 + H2O —-> NH3 + HClO chloric I acid

20
Q

reactions of chlorides of Na,Mg,Al,Si,PCl3 and PCl5 with wtaer

A

NaCl–> Na+ and Cl-
MgCl2+ H2O —> Mg(OH)2 + HCl or just ions
AlCl3 + H2O —-> Al(OH)3 + HCl
SiCl4 + H2O —-> SiO2 + HCl
PCl3 + H2O —> HCl + H3PO3
PCl5 + H2O –> HCl + POCl3 phosphorus trichloride oxide

21
Q

which is the chloride that does not produce HCl upon the reaction with water?

A

NCl3

22
Q

examples of basic oxides

A

Na2O, MgO

23
Q

acidic oxides examples

A

SiO2, CO2, P4O10, SO3, Cl2O

24
Q

SiO2 in water

A

insoluble white solid (in water)

macromeluclar structure would require oo much energy to break covalent bonds.

25
Q

acidic oxides reactions with alkalis

A

–SiO2 + NaOH—> Na2SiO3 + H2O silicate ion= siO3 2-

–P4O10 + NaOH —-> Na3PO4 +H2O
SO2 + NaOH—-> Na2SO3 + H2O
SO3 + NaOH—> Na2SO4 + H”O
Cl2O + NaOH —-> NaClO + H2O

26
Q

acidic oxides with water (P4O10, SO2,SO3,Cl2O)

A

H3PO4
H2SO3
H2SO4
HClO

27
Q

amphoteric oxides, give 2 examples and a hydroxide

A

react both with acids and bases

Al2O3 and BeO, Al(OH)3

28
Q

show Al2O3 acting as both an acid and base

A

as a base
Al2O3 + HNO3 —> Al(NO3)3 + H2O

as an acid
Al2O3 + NaOH + H2O —> Na[Al(OH)4]

29
Q

examples of neutral oxides

A

Co and NO

30
Q

Mg(OH)2 in qualitative analysis

A

Mg(OH)2 is a white solid. on addition to a few drops of OH- to MG2+, a white pp of Mg(OH)2 is produced. this is insoluble in excess OH- sinc eit is a basic hydroxide.

31
Q

show Al(OH)3 being amphoteric

A

Al(OH)3 + HNO3 —–> Al(NO3)3 + H2O
dissolvs to make a colourless solution

Al(OH)3 + OH- —-> [Al(OH)4]-

32
Q

Al3+ and Al(OH)3 in qualitative analysis

A

-few drops of OH- to Al3+ to give Al(OH)3 white pp
this white pp dissolves in excess NaOH to from a colourless solution containing the tetrahydroxoaluminate ion. this is because Al(OH)3 is amphoteric

33
Q

Na reaction with EXCESS O2

A

produces Na2O2 sodium peroxide

34
Q

reaction of Li and Na with water

A

LiOH and H2

NaOH and H2

35
Q

carbon with water (conditions)

A

C+ H2O —> CO+ H2

at high temp

36
Q

F with water vs Cl with water

A

F + H2O —> HF+ O2
only one product since F can only have oxidation state of -1 in compounds

Cl2+ H2O HClO + HCl
disproportionation reaction. produces chloric I acid and HCl

37
Q

Mg with water and steam

A

room temp: Mg(OH)2 and H2

steam: MgO + H2 white powder

38
Q

reaction of B with Cl requires ___

A

heat

39
Q

reaction of F2 with Cl2

A

F2+ Cl2 –> ClF
F2+ Cl2 —> ClF3
both interhalogen compounds

40
Q

why are dry conditions needed when heating Al and Cl2

A

the AlCl3 formed would react with water to form Al(OH)3 and HCl

41
Q

reaction of S and Cl2

A

S+ Cl2 –> S2Cl2

yellow liquid with a bad smell

Chemistry (11 decks)

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