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Chem 130 > Exam 2 > Flashcards

Exam 2 Flashcards

(65 cards)

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1
Q

What are the names of the electron geometries?

A
  • Linear
  • Trigonal Planar
  • Tetrahedral
  • Trigonal Bipyramidal
  • Octahedral
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2
Q

What are the molecular geometries within Linear? State: #bonds, #lone pairs, and angles.

A

Linear –> 2 bonds –> 0LP –> 180 deg

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3
Q

What are the molecular geometries within Trigonal Planar? State: #bonds, #lone pairs, and angles.

A

Trigonal Planar –> 3 bonds –> 0LP –> 120 deg

Bent –> 2 bonds –> 1LP –> <120 deg

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4
Q

What are the molecular geometries within Tetrahedral? State: #bonds, #lone pairs, and angles.

A

Tetrahedral –> 4 bonds –> 0LP –> 109.5 deg

Trigonal Pyramidal –> 3 bonds –> 1LP –> <109.5 deg

Bent –> 2 bonds –> 2LP –> <109.5 deg

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5
Q

What are the molecular geometries within Trigonal Bipyramidal? State: #bonds, #lone pairs, and angles.

A

Trigonal Bipyramidal –> 5 bonds –> 0LP –> 120 deg (equatorial), 90 deg (axial)

Seesaw –> 4 bonds –> 1 LP –> <120 deg (equatorial), <90 deg (axial)

T-Shaped –> 3 bonds –> 2LP –> <90 deg

Linear –> 2 bonds –> 3LP –> 180 deg

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6
Q

What are the molecular geometries within Octahedral? State: #bonds, #lone pairs, and angles.

A

Octahedral –> 6 bonds –> 0LP –> 90 deg

Square Pyramidal –> 5 bonds –> 1LP –> <90 deg

Square Planar –> 4 bonds –> 2LP –> 90 deg

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7
Q

What are the hybrid orbitals and their associated geometries?

A

sp –> linear
sp^2 –> trigonal planar
sp^3 –> tetrahedral
sp^3d –> trigonal bipyramidal
sp^3d^2 –> octahedral

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8
Q

Pi bonds form from the overlap between _____

A

2 P orbitals that overlap adjacent to each other.

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9
Q

Sigma bonds form between ____

A
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10
Q

How many sigma bonds can you have?

A

1

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11
Q

How many pi bonds can you have?

A

Two maximum. There is 1 in double bonds and 2 in triple bonds.

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12
Q

What is the chemical formula of acetate?

A

(C2H3O2)^-

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13
Q

What is the chemical formula for carbonate?

A

(CO3)^2-

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14
Q

Formula for Hydrogen Carbonate (Bicarbonate)

A

HCO3 -

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15
Q

Formula for Hydroxide

A

OH -

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16
Q

Formula for Nitrite

A

NO2 -

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17
Q

Formula for Nitrate

A

NO3 -

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18
Q

Formula for Chromate

A

CrO4 2-

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19
Q

Formula for Dichromate

A

Cr2O7 2-

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20
Q

Formula for Phosphate

A

PO4 3-

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21
Q

Formula for Hydrogen Phosphate

A

HPO4 2-

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22
Q

Formula for Dihydrogen Phosphate

A

H2PO4 -

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23
Q

Formula for Ammonium

A

NH4 +

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24
Q

Formula for Hypochlorite

A

ClO -

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25
Formula for Chlorite
ClO2 -
26
Formula for Chlorate
ClO3 -
27
Formula for Perchlorate
ClO4 -
28
Formula for Permanganate
MnO4 -
29
Formula for Sulfite
SO3 2-
30
Formula for Hydrogen Sulfite (Bisulfite)
HSO3 -
31
Formula for Sulfate
SO4 2-
32
Formula for Hydrogen Sulfate (Bisulfate)
HSO4 -
33
Formula for Cyanide
CN -
34
Formula for Peroxide
O2 2-
35
What are the excepciones to the octet rule?
Elements in the 3rd row and below can have expanded octets.
36
What is the trend for first ionization energy?
Decreases as you move down and increases as you move to the right. Down --> outermost electrons are further from the nucleus, so they are easier to lose. Right --> Zeff increases, so it's harder to remove e.
37
What is the trend for electron affinity?
Increases moving up and to the right. Because Zeff increases and pulls more strongly the incoming electron.
38
What happens to the energy of the orbitals as n (the principal quantum #) increases?
As n increases so deos the energy of the orbitals, which makes them less stable as there is les Zeff acting no the electrons that are further appart.
39
What is the difference between dismagnetism and paramagnetism?
Diamagnetism—> Paired electrons, not attracted to external magnetic field. Paramagnetic—> Unpaired electrons, attracted to external magnetic field. Ferronagnetic —> no need to apply magnetic field bc spins are already aligned.
40
What is Pauli exlusion principle?
No 2 electrons in the same atom can have the same 4 quantum numbers.
41
What are degenerate orbitals?
Orbitals that have the same energy (same value of n).
42
How does l affect the energy level of the orbital?
Different l's in the same n have different energy levels. s
43
What is Coulombs's law?
The potential energy of two charged particles depends on their charges and their separation. - Like charges --> positive interaction. The potential energy decreases as the particles get farther apart. - Unlike charges --> negative interaction. Potential energy becomes more negative as particles move closer. - The magnitude of the interaction increases as the charge of the particles increases
44
What is shielding?
The effect of the repulsion of one electron by another electron that shields it from the effective nuclear charge.
45
How do you calculate Zeff?
#Protons - #Core electrons
46
What is penetration?
Some higher orbitals have significant amounts of probability within the space occupied by lower orbitals. AS electrons penetrate they experience higher Zeff and lower energy.
47
What do the periodic trends mostly depend on?
of valence electrons. Elements in the same family (column) have similar properties.
48
Metals tend to _____ electrons in chemical changes.
Loose (become cations)
49
Non-metals tend to _____ electrons during chemical changes.
Gain (become anions)
50
What are metalloids or semi-metals?
They exhibit mixed properties and are semi-conductors. B, Si, Ge, As, Sb Te, Po
51
What ions do different groups form?
Alkali --> +1 cations Alkali earth metals --> +2 cations Halogens --> -1 anion
52
How do you determine the length of a bond?
Van der Waals radius --> for atoms that form crystals (not bonded together). r=1/2*d Covalent radius= 1/2 * distance between 2 atoms next to each other.
53
What is the atomic radius?
Set of the average bonding radii determined from measurements on a large # of elements and compounds. --> smaller than Van der Waals radius because atoms are bonded together.
54
What is the trend for atomic size?
Atoms get bigger as you move down and left in the periodic table. Down --> bc size of outermost occupied orbital increases. Left --> bc Zeff increases as you move to the right so there is more pull of electrons towards the nucleus.
55
What is the periodic trend for the metallic characters?
Increases as you move down and decreases as you move right. Because in both of these directions ionization energy increases.
56
What is the difference between 1st and 2nd ionization energy?
Removing a valence electron (IE1) requires less energy than removing a core electron (IE2).
57
What are the exceptions to the ionization energy trend?
Boron has a lower ionization energy than beryllium. Because of the change from s to p block. 1s electrons shield 2p electrons more than the 2s, resulting in 2p being higher in energy and easier to remove. Oxygen has a lower 1st ionization energy than nitrogen. Due to electron repulsion, there is one paired electron in oxygen and zero in nitrogen.
58
How do you name a simple ionic compound?
Name of cation + (name of anion + ide)
59
What are hydrated ionic compounds?
Hydrate --> contains a specific number of water molecules associated with the unit. Water usually removed by heating the compounds. To name hydrate compounds add the prefix + hydrate to the name of the ionic compound. eg., barium chloride hexahydrate. Anhydrous --> not associated with water.
60
What is lattice energy?
The energy is associated with the formation of a crystalline lattice with alternating anions and cations. Energy is emitted as heat when lattice forms. Higher lattice energy when the difference between charges is bigger.
61
How do you name ionic compounds containing metals that form more than one ion?
Name one cation (Charge of cation in Roman numerals) + (name of anion + ide)
62
How do you name covalent molecules?
(prefix + name of 1st element) + (prefix + name of 2nd element) The first element is the more metalike element --> more towards left of p table
63
Which elements can have multiple charges?
Cr, Fe, Co, Cu, Sn, Hg, Pb
64
what is Hand's Rule?
When filling degenerate orbitals electrons fill them singly first, with parallel spins.
65
What is the Aufbau principle?
Electrons fill lower energy orbitals first.

Chem 130 (3 decks)

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