Unit 3 Flashcards
1
Q
How are groups arranged on the P.T.?
A
They go down
2
Q
Group 1
A
Alkali Metals
3
Q
Group 2
A
Alkali Earth Metals
4
Q
Groups 3-12
A
Transition Metals
5
Q
Group 17
A
Halogens
6
Q
Group 18
A
Noble Gases
7
Q
How are periods arranged on the P.T?
A
They go across left to right
8
Q
What do periods correspond with?
A
The number of Principle Energy Levels where valence electrons are located
9
Q
Where are Metals located?
A
Left of Staircase
10
Q
What do Metals form?
A
Cations
11
Q
Description of metals
A
Malleable, ductile, good conductors
12
Q
Where are nonmetals located?
A
Right of the staircase
13
Q
What do nonmetals form?
A
Anions
14
Q
Description of nonmetals
A
Brittle, dull, non-conductors
15
Q
Locations of metalloids
A
Touch the staircase
16
Q
What are the metalloids?
A
B, Si, Ge, As, Sb, Te
17
Q
Nuclear Charge
A
Represented by atomic number and increases by one through each successive element
18
Q
The outer electrons determine what?
A
Many physical and chemical properties of an element
19
Q
What prevents the valence electrons from experiencing the full nuclear charge?
A
Repulsion and Shielding due to the inner electrons
20
Q
As you go across period…
A
- Same amount of shielding
- Greater nuclear charge
More effective nuclear charge
21
Q
As you go down group…
A
- Same effective nuclear charge
- Charge increases by 8
- Shielding increases by 8
22
Q
Atomic Radius
A
Half the distance between neighboring atoms
23
Q
Why does atomic radius increase down a group?
A
Greater numbers of P.E.L.’s as seen by period number
24
Q
Why does atomic radius decrease across a period?
A
Same number of P.E.L.’s, greater nuclear charge
25
Cations are ___ than its atom
Smaller
26
Anions are ___ than its atom
Larger
27
Isoelectronic
The same electronic configuration
28
Cations have a...
Same nuclear charge with less electrons, which pulls electrons closer, have a smaller radius
29
Anions have a...
Same nuclear charge, more electrons, cannot pull electrons as close, larger radius
30
Electron Affinity
A measure in the charge in energy when one mole of its electrons are added to one mole of gaseous atoms to form gaseous ions; exothermic process
Becomes endothermic when adding a second electron
31
Electronegativity
A measure of an element's attraction for one electron in a covalent bond
32
Electronegativity increases...
Across a period
33
Electronegativity decreases...
Down a group
34
The melting point of metals...
Increases as the number of valence electrons increases
35
Metalloids have...
Very high melting points and strong bonds due to being covalent structures
36
The melting point of nonmetals...
Are low due to weak intermolecular forces
37
The melting point of Noble Gases...
Are very low due to very weak intermolecular forces and being monatomic
38
Chemical properties of metals
-More reactive as you go down groups
-React by losing electrons
-Bigger, easier to lose electrons
39
Metal Oxides with Acids
Form a salt and water
Neutralization reaction, the metal cation bonds with the acidic anion to form a salt, the leftover H and O form water
40
Nonmetal Oxides with Bases (Alkali)
Form a salt and water
Neutralization reaction, shows that nonmetal Oxides are acidic in nature
41
Group 17 Reactivity
Most reactive at the top (F)
42
Properties of Fluorine
Yellow gas
43
Properties of Chlorine
Yellow/green gas
44
Properties of Bromine
Dark Red liquid
45
Properties of Iodine
Purple Solid
46
Displacement reaction
A more reactive halogen will be in compound form, less reactive alone
47
Nonmetal Oxides in water
Bonds together, forms an acid
48
Amphoteric Oxide (Al2O3)
Can act as both an acid and base (Lewis)
49
What two Nonmetal Oxides do not react with water?
SiO2 and CO
50
Properties of Transition Metals
1. Variable oxidation states
2. Incomplete d sublevel as atom or as positive ion
3. Catalytic and magnetic properties
4. Form complex ions with ligands
5. Colored compounds
51
How is Zinc not a Transition Metal
It always has a complete d sublevel, is always colorless and only has one oxidation state
52
All Transition Metals can form what two oxidation states?
+2 and +3
53
From Sc to Cr, what oxidation state is the most common?
+3
54
The +2 oxidation state is most common where?
After Mn due to a greater nuclear charge making it harder to lose more than two electrons
55
Where and what is the maximum oxidation state?
At Mn, highest is +7
56
Trend for oxidation states across transition metals
Oxidation states increase by one up to Mn, where they decrease by one after
57
What two metals have the highest oxidation states and are the best reducing agents?
Mn +7 and Cr +6
58
What do Transition Metals do as catalysts?
Increase the rate of reaction and provide an alternate pathway
59
Homogeneous catalyst
A catalyst in the same phase as the reactant(s)
60
Medical uses of Transition Metals
1. Fe +2 heme in blood to transport oxygen
2. Co +3 in vitamin B12
61
Heterogeneous Catalyst
A catalyst in a different phase than the reactant(s)
62
Catalyst Converter
(Pd/Pt catalysts) Converts CO and NO into CO2 and N2
2CO + 2NO = 2CO2 and N2
63
Haber Process
(Fe catalyst) The production of ammonia from its elements
N2 + 3H2 = 2NH3
64
Contact Process
(V2O5 Vanadium V Oxide Catalyst) Production of sulfuric acid
2SO2 + O2 = 2SO3
65
Hydrogenation
(Ni catalyst) Converting unsaturated hydrocarbons into saturated hydrocarbons
C2H4 + H2 = C2H6
66
Decomposition of Hydrogen Peroxide
(MnO2 catalyst) 2H2O2 = 2H2O + O2
67
Magnetic properties of Transition metals
How they behave when introduced to a magnetic field
68
Paramagnetic
Contains unpaired electrons
-Will be pulled into a magnetic field
-Do not retain magnetic properties
-More unpaired electrons, more attraction
69
Diamagnetic
Contains paired electrons
-Weakly repelled by magnetic properties after field is removed
70
Ferromagnetic
Contain unpaired electrons that align parallel to each other in domains
-Retain magnetic properties when magnetic field is removed (Iron, Cobalt, Nickel)
71
Complex Ion
Because of their small size, d block ions attract species that are electron rich (ligands)
72
Ligands
Species with lone pair(s) of electrons that form coordinate covalent bonds with a central metal ion. Ligands are Lewis bases
73
Spectrochemical series
I - < Br - < S -2 < Cl - < H2O < OH - < SCN- < NH3 < CO = CN -
Weakest -> strongest
Stronger = more splitting
74
Monodetant ligands
Form one coordinate covalent bond using one lone pair of electrons
*If the ligand is neutral, the charge of the central ion is the same as the complex ion
*The number of coordinate covalent bonds from the ligand to the central ion is the coordination number
75
Polydentant Ligands
Contain more than one pair of lone electrons and can form two or more coordinate covalent bonds to the central ion
76
Bidentant Ligands
Can form two coordinate covalent bonds (Oxalate ion C2O4 -2)
77
Ethylenediamine
H2NCH2CH2NH2
78
Hexadentate ligand
Has six atoms with lone pairs of electrons (EDTA -4)
79
Chelate
Two or more separate coordinate covalent bonds between ligand and central atom
80
Oxidization rules
1. Compounds sum to zero
2. Ions sum out to their charge (NO3-)
3. Lone elements = 0
4. Group 1 metals = +1
5. Group 2 metals = +2
6. Oxygen is almost always -2, unless peroxide or with F-2
7. Hydrogen is +1 unless with metal -1
8. Fluorine is always -1
81
Oxidation states vs oxidation numbers
Oxidation states: (+) or (-) in front
Oxidation numbers: Roman numerals
82
Color of Transition Metals
-Related to presence of partially filled d orbitals
-The color is determined by the color of light it absorbs and which color it transmits or reflects (Opposite color on the color wheel)
83
Degenerate
A free ion, the d orbitals are all of equal energy
84
Location of the 5 d orbitals
3 between the axis
2 along the axis
85
Splitting
When a ligand comes in, its lone electrons repell the 2 orbitals along the axis, causing them to split, anything that changes the splitting changes the color
86
Identity of central metal ion
-Larger metals provide greater splitting
-A greater nuclear charge will cause a greater electrostatic attraction to the ligand and result in more splitting
More energy = more splitting
87
Oxidation state of metal ion
As oxidation state increases for the same metal, the splitting of the d orbitals also increases
88
Geometry of Complex ion
Octahedrall (6) > Tetrahedral (4) > Linear (2)
89
Identity of ligand
Stronger ligand = greater splitting
90
(Cu(H2O)6) vs [Cu(NH3)4(H2O)2]
When some of the water ligands are replaced by ammonia the splitting of the d orbital increases. The new complex Ion will absorb more energy and light with decreasing wavelength.
