Exam Review Flashcards
Three regions of space
trigonal planar, 120
Three regions of space, 1 LP
bent, <120
Four regions of space
tetrahedral, 109.5
Four regions of space, 1 LP
trigonal pyramidal, < 109.5
Four regions of space, 2 LP
bent, «109.5
Five regions of space
trigonal bipyramidal, 90 & 120
Five regions of space, 1 LP
seesaw, 90 & 120
Five regions of space, 2 LP
t shape, 90
Five regions of space, 3 LP
linear
Six regions of space
octahedral, 90
Six regions of space, 1 LP
square pyramidal, 90
Six regions of space, 2 LP
square planar, 90
Intermolecular forces & Types
- Btwn atoms
- Dipole-dipole
- H bonding
- LD forces
Intramolecular force
Btwn subatomic particles
Ionic Solids
- More e- given = stronger
- High pnts
- Brittle
- Unconductive as solid, conductive as liquid
Molecular/atomic Solids
- Neutral molecules w/weak intermolecular forces
- Noble gases
- Low pnts
- Poor conductors
- Variety
Network/covalent Solids
- Atoms w/covalent bonds
- Hard
- High pnts
- Nonconductors
Metallic Solids
- Malleable
- High pnts
- Conductors
Thermal Energy
KE + PE
Types of KE
- Translation
- Rotational
- Vibrational
Enthalpy (H)
Total internal nrg of a substance (even w/o change in T)
Exo and Endothermic Enthalpy
- Exo = -ive
- Endo = +ive
BDE
Nrg needed to break bonds (H = react - prod)
Strong bonds have
Low PE, high BDE
Weak bonds have
High PE, low BDE
As bond strength increases
- Needs more nrg (like 2/3 bonds)
- d btwn atoms decreases
Standard Enthalpy of Formation
- Uses standard form of element as 0KJ
- Hf = change in H for 1 mol (H = prod - react)
Ways of Measuring Rates
- Gas
- Colour
- Mass
- pH
- Conductivity
Collision Theory
Rxns only happens when entities collide at right orientation & KE
Factors that affect Rate of Reaction
- Ea
- Temp
- Bond type/strength (covalent needs more)
- C
- SA
- Catalysts
Rate law
= K [A]^m [B]^n
Reaction Mechanisms Requirements
- Steps must added to eqn
- Rate determ step = rate eqn
Characteristics of EQ
- Only macroscopi properties change
- System is closed, temp constant
- Rate F/B =
K Properties
- K always same regardless of C, except temp
- If EQ eqn reversed, K = 1/k
- When rxns +, xK
Changes in Pressure
EQ shifts to side that has less molecules
Endothermic Reactions
- Cooled = shift L
- Heated = shift R
Exothermic Reactions
- Cooled = shift R
- Heated = shift R
Changing EQ Sys without Changing Position
- Catalysts
- Inert gases
- Diff states
Solubility
Amount of solute that dissolves in a solvent at a temp
Molar Solubility is used to calculate
Ksp
Salt Ratios
- 1:1 = s^2
- 1:2 = 4s^3
- 1:3 = 27s^4
Trial Ion Product
Uses Q to find if precip will form
Common Ion Effect
Decrease in solubility when same ion present
Bronsted-Lowry Theory
Acid are donors, bases are acceptors
Strong acid/base
Very weak conjugate
Weak acid/base
Weak conjugate
Very weak acid/base
Strong conjugate
Weak A/B Ksp Value
-4 to -10
Salt is neutral if
- Cation from grp 1 or 2
- Anion is from a SA
Salt is basic if
Anion is a Cb to WA
Salt is acidic if
Cation is Ca to WB
Metallic Oxides
Basic
Non-metallic
Acidic
Orbitals
Cloud of probability for e
Principal Quantum Number
Size & nrg for atomic orbital
Secondary Quantum Number
Nrg sublvls (l = n-1)
Magnetic Quantum Number
Orientation of orbital (-l to +l)
Spin Quantum Number
Spin up or down (+/- 0.5)
Pauli Exclusion Principle
No same quantum #s
Aufbau Principle
lowest orbitals first
Hund’s Rule
No pairing first
Hybrid Orbital
Orbital formed from combination of diff orbitals
Sigma Bonds
Orbitals overlap head to head
Pi Bonds
Orbitals overlap side to side
Covalent Bonds with Sigma and Pi Bonds
- Single = sigma
- Double = pi
- Triple = sigma, pi, pi
Oxidation Number Rules
- F always -1
- O2 usually -2, except peroxides = -1
Oxidizing Agent
Gains e-, is reduced
Reducing Agent
Loses e-, is oxidized
Reactions happens if
OA is above RA
Anode and Cathode Redox Reactions
- Anode = oxidized
- Cathode = reduced
Ethers
- Has O in the middle
- +oxy
Aldehyde
- Has O2 at the end
- +al
Ketones
- Has O2 in the middle
- +one
Carboxylic Acid
- COOH
- +oic acid
Ester
- COOH + OH
- +oate for COOH chain
Amine
- N
- +amine
Amides
- COOH + NH
- +amide for O2 + N chain
Types of Addition Reactions
- Hydrogenation
- Halogenation
- Hydrohalogenation
- Hydration
Alcohols Reactions
- Dehydrate into akenes
- Oxidize into aldehyde/ketone
Aldehydes and Ketones Reactions
Hydrogenation into 1 or 2nd alcohol
Estertification
COOH + OH = ester
Amine Condensation
Alkyl Halide + amine
Amides Condensation
COOH + amine
Organic Compound Hierarchy
- COOH
- Amides
- Alcohol
- Amines
- Ketones
- Aldehyde
- Ester
- Ether
- Benzene
- Alkynes
- Alkenes
- Alkanes
Electron Configuration Exceptions
- Cr: [Ar] 4s13d5
- Cu: [Ar] 4s13d10
- Ag: [Kr] 5s14d10
- Au: [Xe] 6s14f145d10