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Chem > 3..., 13... > Flashcards

3..., 13... Flashcards

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1
Q

period

A
  • row of elements (horizontal)
  • number of shells
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2
Q

group

A
  • column of elements (vertical)
  • number of valance electrons
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3
Q

s,d,p,f blocks on periodic table

A
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4
Q

what do all s-block elements have?

A
  • only s electrons in the outer shell
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5
Q

what do all p-block elements have?

A
  • atleast one p-electron in the outer shell
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6
Q

what do all d-block elements have?

A
  • atleast one d-electron and one s-electron but no f or p electrons in thr outer shell
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7
Q

what do all f-block elements have?

A
  • atleast one f-electron and atleast one s-electron, but no d or p electrons in the outer shell
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8
Q

what is the pattern seen in chemical and physical properties on the periodic table

A
  • physical and chemical properties of elements in the periodic table show clear patterns related to the position of each element in the table
  • elements in the same group show similar properties
  • properties change gradually as you go across a period
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9
Q

what is atomic radius?

A
  • size of an atom
  • ## distance between the nucleus of an atom and the outermost electron shell
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10
Q

atomic radius across a period?

A

decreases

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11
Q

atomic radius down the group?

A

increases

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12
Q

ionic radius

A
  • measure of the size of an ion
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13
Q

ionic radius down the group?

A

increases

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14
Q

ionic radius across a period

A
  • ionic radius increases with increasing negativ charge
  • ionic radius decreases with increasing positive charge
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15
Q

first ionisation energy

A
  • ## amount od energy required to remove one mole of electrons from one mole of atoms of an elemts in gaseous state to form one mole of gaseous ions
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16
Q

first ionisation energy across a period?

A

increases

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17
Q

first ionisation energy down the group

A

decreases

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18
Q

Why does ionisation energy increases across a period?

A
  • nuclear charge increases
  • distance between the nucleus and outer electron remains reasonably constant
  • shielding by inner electrons remains the same
  • rapid decrease in ionisation energy between the last element in one period and the first element in the next period
  • increased distance between the nucleus and outer electrons
  • increased shielding by inner electron
  • these outweigh nuclear charge
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19
Q

why does ionisation energy decrease down the group?

A
  • distance between the nucleus and outer electron increases
  • shielding by inner shell electrons increases
  • effective nuclear charge is decreasing as shielding increases
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20
Q

why does successive ionisation energie of an element increases?

A
  • ## removing an electron from a positive ion is more difficult than from a neutral atom
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21
Q

electron affinity

A
  • ## amount of energy released when one mole of electrons is gained by one mole of atoms of an element in the gaseous state to form one mole of gaseous ions
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22
Q

electron affinity down the group?

A

decreases

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23
Q

electron affinity across a period?

A

increases

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24
Q

Electronegativity

A
  • ## ability of an atom to attract a pair of electrons towards itself in a covalent bond
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25
Q

electronegativity down the group?

A

decreases

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26
Q

electronegativit across a period

A

increases

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27
Q

how does nuclear charge affect electronegativity?

A
  • attractions exist between protons and electrons
  • increase in the number of protons leads to an increase in nuclear attraction
  • ## increased nuclear charge/protons = increased electronegativity
28
Q

how does atomic radius affect electronegativity?

A
  • electrons closer tot he nucleus are more strongly attracted towards it’s positive nucleus
  • increased atomic radius = decreased electronegativity
29
Q

bonding of metals and non-metals

A

metals: metallic due to loss of outer shell electrons
non-metals: covalent by sharing outer shell electrons

30
Q

electron conductivity of metals vs non-metals

A

metals: good conductors of electricity
non-metals: poor conductors fo electricity

31
Q

type of oxides metals vs non-metals

A

metals: basic oxides (few amphoteric)
non-metals: acidic oxides (some neutral_

32
Q

reactions with acids metals vs non-metals

A

metals: many reaction with acids
non-metals: do not react with acids

33
Q

physical characteristics metals vs non-metals

A

metals: malleable, can be bent and shaped
non-metals: flaky and brittle

34
Q

melting and boiling point metals vs non-metals

A

metals: high melting and boiling point
non-metals: low melting and boiling point

35
Q

pH of oxides across a period

A

basic –> amphoteric –> acidic
Al: amphoteric

36
Q

melting point in period three oxides

A

Na2O: high
MgO: High
Al2O3: very high
SiO2: very high
P4O10: low
SO2: low

37
Q

chemical bonding of oxides across period 3

A

Na2O: ionic
MgO: ionic
Al2O3: ionic
SiO2: covalent
P4O10: covalent
SO2: covalent

38
Q

Na2O reaction with water and the pH

A

Na2O+H2O –> 2NaOH
pH:14

39
Q

MgO reaction with water

A

MgO + H2O –> Mg(OH)2
pH:10

40
Q

P4O10 reaction with water

A

P4O10 + 6H2O –> 4H3PO4
pH:2

41
Q

NO2 reaction with water

A

2NO2 + H2O –> HNO3 + HNO2
pH:1

42
Q

SO2/SO3 reaction with water

A

SO2 + H2O –> H2SO3
SO3 + H2O –> H2SO4
pH:1

43
Q

patter of oxides reacting with water

A
  • metallic oxides form hydroxides when reacted with water
  • non-metallic oxides form oxoacids when they react with water
44
Q

how to predict oxides reacting with water

A
  • position of an element in the periodic table can be used to predict and explian its metallic and non-metallic behavior
  • metal and non-metal elements generarly form ionic compounds
  • oxides become more ionic as you go down the group
  • ## oxides become less ionic across a period
45
Q

physical properties of the group 1 metals

A
  • soft eady to cut, softer and denser as you go down the group
  • shiny silvery surfaces
  • conducct heat and electricity
  • low melting and densities
  • melting point decreases down the group
46
Q

chemical properties of grp 1 metals

A
  • react readily with oxygen and water vapour in air, so they are usually kept in oil
  • react readily with water to produce alkaline metal hydroxide and hydrogen gas
47
Q

grp 1 reacting with grp 17

A
  • react vigorously
  • reaction rate increases down group 1
  • as atoms get larger
  • electron further away from nucleus
48
Q

physical properties of grp 17

A
  • density and metling point increases down the group
49
Q

reactivity of grp 17

A
  • decreases down the group
  • electron affinity decreases
  • ## atomic radius increases
50
Q

halogen displacement reactions with halide ions

A
  • occurs when a more reactive halogen displaces a less reactive halogen
  • reactivity of grp 17 increases as you move up the group
  • when halide ion is above the halogen in compound, it is replaced
  • ## when Cl- replaces Br - solution becomes orange
51
Q

Transition elements

A

-incomplete d-subshells or that can form atleast one stable cation with incomplete d-subshells

52
Q

what d-block elements arent transition metals

A

Sc, Zn

53
Q

what do transition elements have that other metals don’t

A
  • variable oxidation states
54
Q

why transition elements form complex ions

A
  • due to their variable oxidation states
55
Q

what is a complex ion

A

molecule or ion, consisting of a central metal atom or ion, with anumber. ofmolecules or ions surrounding it

56
Q

what is a ligand

A
  • molecule or ion surrounding the central metal atom or ion
  • due to different oxidation states of central metal ion, a different number and wide variety of ligands can form bonds with the transition elements
57
Q

transition elements are able to form ____ compounds

A

colored

58
Q

why do transition elements act as catalysts?

A
  • since they have variable oxidation states
  • during catalysis, the transition element can change to various oxidation states by gaining electron from or donating electrons to reagents withing the reaction
59
Q

magnetic properties of transition elements

A
  • diamagnetic, paramagnetic or ferromagnetic
  • transition metals exhibit properties depending on their electronic configurations
  • result of unpaired electron in the trainsition metal atom or ion
60
Q

common ligands

A

H2O
NH3
Cl-
CN-
OH-

61
Q

co-ordinate number

A
  • number of coordinate bonds to the metal ions
62
Q

naming complexes

A

prefix for number of ligands / ligand name/ element / oxidation number

63
Q

transition metals as catalysts

A
  • heterogeneous catalyst as they can provide a surface for reaction
  • use 3d and 4s electrons to form weak bonds to reactant molecules
64
Q

why do transition metals exhibit colors?

A
  • d-orbital have the same energy in an isolated atom, but split into two sub-levels in a complex ion.
  • electrical field of ligands cause the d orbital in complex ions to split so that the energy of an electron transition between them corresponds to a photon of visible light
65
Q

what does the color exhibited by complex ion depend on?

A
  • color observed is complementary to the color absorbed
  • color depends on the identity of the metal ion, oxidation state of metal, and identity of the ligand
  • ions with higher charge and ligands with greater charge density produce a greater split in the d-orbital
  • spechtochemical series arranges ligans according to the energy seperation between the two sets of d orbitals.

Chem (13 decks)

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