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Chem 130 > Exam 2 > Flashcards

Exam 2 Flashcards

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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
Q

Formula for Chlorite

A

ClO2 -

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26
Q

Formula for Chlorate

A

ClO3 -

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27
Q

Formula for Perchlorate

A

ClO4 -

28
Q

Formula for Permanganate

A

MnO4 -

29
Q

Formula for Sulfite

A

SO3 2-

30
Q

Formula for Hydrogen Sulfite (Bisulfite)

A

HSO3 -

31
Q

Formula for Sulfate

A

SO4 2-

32
Q

Formula for Hydrogen Sulfate (Bisulfate)

A

HSO4 -

33
Q

Formula for Cyanide

A

CN -

34
Q

Formula for Peroxide

A

O2 2-

35
Q

What are the excepciones to the octet rule?

A

Elements in the 3rd row and below can have expanded octets.

36
Q

What is the trend for first ionization energy?

A

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
Q

What is the trend for electron affinity?

A

Increases moving up and to the right. Because Zeff increases and pulls more strongly the incoming electron.

38
Q

What happens to the energy of the orbitals as n (the principal quantum #) increases?

A

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
Q

What is the difference between dismagnetism and paramagnetism?

A

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
Q

What is Pauli exlusion principle?

A

No 2 electrons in the same atom can have the same 4 quantum numbers.

41
Q

What are degenerate orbitals?

A

Orbitals that have the same energy (same value of n).

42
Q

How does l affect the energy level of the orbital?

A

Different l’s in the same n have different energy levels.
s<p<d<f

43
Q

What is Coulombs’s law?

A

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
Q

What is shielding?

A

The effect of the repulsion of one electron by another electron that shields it from the effective nuclear charge.

45
Q

How do you calculate Zeff?

A

Protons - #Core electrons

46
Q

What is penetration?

A

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
Q

What do the periodic trends mostly depend on?

A

of valence electrons. Elements in the same family (column) have similar properties.

48
Q

Metals tend to _____ electrons in chemical changes.

A

Loose (become cations)

49
Q

Non-metals tend to _____ electrons during chemical changes.

A

Gain (become anions)

50
Q

What are metalloids or semi-metals?

A

They exhibit mixed properties and are semi-conductors. B, Si, Ge, As, Sb Te, Po

51
Q

What ions do different groups form?

A

Alkali –> +1 cations
Alkali earth metals –> +2 cations
Halogens –> -1 anion

52
Q

How do you determine the length of a bond?

A

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
Q

What is the atomic radius?

A

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
Q

What is the trend for atomic size?

A

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
Q

What is the periodic trend for the metallic characters?

A

Increases as you move down and decreases as you move right. Because in both of these directions ionization energy increases.

56
Q

What is the difference between 1st and 2nd ionization energy?

A

Removing a valence electron (IE1) requires less energy than removing a core electron (IE2).

57
Q

What are the exceptions to the ionization energy trend?

A

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
Q

How do you name a simple ionic compound?

A

Name of cation + (name of anion + ide)

59
Q

What are hydrated ionic compounds?

A

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
Q

What is lattice energy?

A

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
Q

How do you name ionic compounds containing metals that form more than one ion?

A

Name one cation (Charge of cation in Roman numerals) + (name of anion + ide)

62
Q

How do you name covalent molecules?

A

(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
Q

Which elements can have multiple charges?

A

Cr, Fe, Co, Cu, Sn, Hg, Pb

64
Q

what is Hand’s Rule?

A

When filling degenerate orbitals electrons fill them singly first, with parallel spins.

65
Q

What is the Aufbau principle?

A

Electrons fill lower energy orbitals first.

Chem 130 (3 decks)

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