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Gen Chem 1 > Theory and Problem Solving > Flashcards

Theory and Problem Solving Flashcards

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1
Q

Expanded octets are only for

A

elements in period 3 and beyond because they have empty d orbitals

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2
Q

Bond energies
- which one is positive and negative, and what is the equation

A

delta H of bonds broken-formed

formation: - (hence why the equation is a minus)
breaking: +

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3
Q

polarity

A

-np EN difference is less than or equal to 0.4

-p EN difference is btwn 0.4-2.0

-EN diff greater than 2.0 is ionic

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4
Q

T/F: flip the equation in bond enthalpy

A

F

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5
Q

Linear molecular geometry is also w/

A

2 0

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6
Q

Electron groups for geometry

A
  • single and double bonds are counted as 1 group
  • lone pairs count as 1 group
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7
Q

T/F: flip the equation for bond enthalpies

A

F

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8
Q

Forming H bonds

A
  • When H atoms that are far apart approach each other, PE=0
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9
Q

electron domain/charge cloud
refers to what

A

electron geometry

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10
Q

By definition polar bonds have a

A

En not equal to 0
- assume this if EN aren’t given
(for instance if given a few molecules and asked to assume polarity, label diatomic as np and that’s it)

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11
Q

Determining the number of degenerate orbitals needed

A

Use trial and error:

For example: Cl: ? degenerate orbitals for 7 electrons with 5 unpaired

= you would need 6

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12
Q

For elements n=3 and above (hybridization)

A

switch to d

  • sp^3 is fine
  • sp^4 is not it should be sp^3d
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13
Q

Bond order is

A

number of bonds (double and single aren’t tx equal) /bond position (surrounding atoms)

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14
Q

p-p make up

A

pi bond

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15
Q

LOW IMF refers to

A
  • low viscosity
  • low surface tension
  • high vapour pressure
  • low BP
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16
Q

HIGH IMF refers to

A
  • high viscosity
  • high surface tension
  • low vapour pressure
  • high BP
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17
Q

Difference in BP between Octane and Isooctane

A

iso: 5 C-H with 3 methyl

oct: straight C-H (stronger IMF)

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18
Q

Sublimination

A

solid to gas

= ENDOTHERMIC

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19
Q

deposition

A

gas to solid

= EXOTHERMIC

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20
Q

melting

A
  • also called fusion

solid to liquid

= ENDOTHERMIC

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21
Q

freezing

A
  • liquid to solid

= EXOTHERMIC

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22
Q

vaporization

A
  • also called evaporation
  • liquid to gas

= ENDOTHERMIC

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23
Q

condensation

A
  • gas to liquid

= EXOTHERMIC

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24
Q

TRIPLE POINT

A
  • all 3 phases touch
  • all 3 equilibriums meet
    = T + P for all reactions is good to occur simultaneously
    so you get gas, solid, liquid particles
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25
Q

CRITICAL POINT

A

point where liquid and gas are indistinguishable
- merge as a single phase

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26
Q

Determining states on curve

A

the one flowing along x axis= GAS
the one by y axis= SOLID
the one between = LIQUID

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27
Q

solving curve questions

A
  • break temperature change down into steps
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28
Q

free radicals

A
  • exception to octet, O will get the electrons if there’s an odd number
  • identify: any O atom with unpaired electrons
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29
Q

T/F: flip average bond enthalpies

A

F

30
Q

T/F: flip the enthalpies of formation

A

T

31
Q

Energy is directly proportional to

A

q1q2/r

= use this relationship to determine the energy released between two ions

32
Q

Bond energy, order, and length relationship

A
  • Higher bond order means stronger bonds (higher bond energy) and shorter bond lengths
    -while lower bond order means weaker bonds (lower bond energy) and longer bond lengths.

a higher bond order indicates more shared electrons between atoms, increasing the attractive force and pulling the nuclei closer together, shortening the bond.

33
Q

For curve q: Use R

A

with only J/mol/K

none of pv=nRT

34
Q

room temperature

A

25 degrees celsius

35
Q

Pressure at room temperature

A

1.01 bar

36
Q

MO: pi orbitals only start

A

at p orbitals

37
Q

Which elements use which MO diagram

A

O-Ne: sigma, pi, pi, sigma

Li-N: pi, sigma, pi, sigma

(for 2p)

38
Q

electrolytes

A

substance that conducts electricity in solution

STRONG: dissociating completely (e.g., strong acids, bases, salts)

WEAK: partially dissociating (e.g., weak acids and bases).

39
Q

percent yield

A

actual/theoretical (100%)

40
Q

Electrical conductivity

A

High electrical conductivity comes from ionic compounds that fully dissociate in water, such as salts, strong acids, and strong bases.

= ability to transfer electrons

41
Q

q, H, U chart

A

Exothermic: Enthalpy (ΔH), heat (q), and internal energy (ΔU) are negative.

Endothermic: Enthalpy (ΔH), heat (q), and internal energy (ΔU) are positive.

42
Q

HUNDS, AUFBAU, AND PAULI EXCEPTIONS

A

Hund’s Rule: Electrons fill degenerate orbitals singly before pairing.

Aufbau Principle: Electrons fill orbitals from lowest to highest energy.
Exception: Transition metals and lanthanides often have electron configurations that differ (e.g., Cr, Cu + elements after period 3)
typically involve transition metals in periods 4-6 (like Cr, Cu, Mo, Ag) and involve d-orbital stability

Pauli Exclusion Principle: No two electrons in an atom can have the same set of quantum numbers.
Exception: None.

43
Q

ER wavelength

A

Radio waves: longest wavelength

Microwaves: shorter than radio waves

Infrared: just below visible light

Visible light: ranges from red
(longest) to violet (shortest)

Ultraviolet: just above visible light

X-rays: shorter than ultraviolet

Gamma rays: shortest wavelength

“Raging Martians Invaded Venus Using X-ray Guns”

44
Q

shielding

A

reduction of the effective nuclear charge on an electron due to repulsion from other electrons.

45
Q

lattice energy

A

energy required to separate one mole of an ionic compound into its gaseous ions.

  • charge based too ions with greater charges will have higher lattice energies
46
Q

covalent radius

A

covalent radius is the distance between two bonded atoms, while the atomic radius is the size of an isolated atom

47
Q

work function of an element

A

work function is the minimum energy needed to remove an electron from the surface of an element

ϕ=hνthreshold

48
Q

determining oxidation states of elements

A

Assign known oxidation states (e.g., O = -2, H = +1).

Sum of oxidation states in a neutral compound = 0, in a polyatomic ion = charge of ion.

Solve for unknown oxidation states based on these rules.

49
Q

kinetic molecular theory

A

gas particles are in constant, random motion, colliding with each other and the container walls. These collisions are elastic, and the average kinetic energy is proportional to the temperature.

50
Q

photoelectric effect

A

phenomenon where electrons are ejected from a material’s surface when it absorbs light of sufficient energy.

51
Q

effective nuclear charge

A

Zeff= Z - S

Z = atomic number

S (based on electron config): 0.85(1s electrons) + 0.35 (2s+p)

52
Q

pressure-volume work theorem

A

-PV

53
Q

STP

A

0° Celsius (273.15 K)
Pressure: 100 kPa (1 bar)
Molar volume: 22.4 L

54
Q

trends

A

ATOMIC RADIUS: increases down and left
IE: increases up and right
ELECTRONEGATIVITY: increases up and right
ELECTRON AFFINITY: increases up and right
METALLIC CHARACTER: increases down and left

ATOMIC RADIUS
METALLIC CHARACTER

ELECTRON AFFINITY
ELECTRONEGATIVITY
IONIZATION ENERGY

55
Q

nodes

A
  • region where there are no electrons

Radial nodes: Spherical regions where the probability of finding an electron is zero.
Equation: n-l-1

Angular nodes: Planar or conical regions where the probability is zero.
Equation: l

TOTAL: n-1

56
Q

standard enthalpy; do you flip the equations

A

yes

57
Q

What will be the case if an electron is emitted?

A

hv must be greater than work function

58
Q

H2CO3

A

break down into H2O + CO2

59
Q

doing work on a system

A

endothermic
relates to W

60
Q

loosing or gaining heat

A

loosing: - q
gaining: +q

61
Q

E comb

A

delta Hr

62
Q

What is Erxn
What is Hrxn

A
  • a measure of change of energy (same as delta U)
  • a measure of reaction
63
Q

Delta U is

A

H-W

64
Q

why are atoms roughly spherical

A

because when the different shaped orbitals are overlapped, they take on a spherical shape

65
Q

determining transitions of n values

A
  • lower the number the greater the energy level
66
Q

exothermic reactions

A
  • weak bonds break and strong bonds form
67
Q

VSEPER

A

theory predicts molecular geometry by minimizing repulsion between electron pairs (bonding and nonbonding) around a central atom to achieve the most stable arrangement.

68
Q

born haber order

A

Sublimation of metal (solid to gas) → up

Bond dissociation of nonmetal (if diatomic, break into atoms) → up

Ionization energy of metal (remove electron) → up

Electron affinity of nonmetal (add electron) → down

Lattice energy (formation of ionic solid) → down

69
Q

MO

A

describes the electronic structure of molecules by combining atomic orbitals to form molecular orbitals, which are spread over the entire molecule and can be bonding, antibonding, or nonbonding, explaining properties like bond order, magnetism, and stability.

70
Q

normal boiling point
boiling point

A

a) the temp when vapour pressure of liquid is around 1 bar
b) temp when vapour pressure of liquid = external pressure

Gen Chem 1 (2 decks)

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