Finals
REVIEW CHAPTERS 1 through 16
Finals in Room T123 at 9:30 am
Dec 19th (Monday)
Bring a scantron
Calculation of
Final grade
SCCC GRADING
60-64 “D”; 65-69 “D+”;
70-74 “C”; 75-79 “C+”;
80-85 “B”; 85-89 “B+”;
Above 90 “A”
Item
Scores Weighta
ge
Exam 4X100 =
400 *1.25
500
50%
Finals
150
15%
Hws (drop 1
lowest grade)
80
8%
Lab (drop 1
lowest grade)
250
25%
Attendance/impr
ession/quiz
20
2%
Total
1000
100%
Chapter 1 and 3
 Concept of Experiment Hypothesis and Theory
 Classification of matter
 Physical change? Chemical change?
 Pure substance? Mixture?
Chapter 2
Significant figure –how many in 0.0050 ?
Scientific notation in form of exponent of 10
Conversion eg. cm-> meter->kilometer, liters-> ml etc., ºF to ºC
2.3 The Basic Units of Measurement (memorize power of 10 table)
A. English, metric, SI
B. SI Units (Mass – kg; Length – m; Time – sec, volume L)
C. Prefix Multipliers
milli (m) 0.001
centi (c) 0.01
kilo (k) 1000
Mega (M) 1,000,000
1.8  C  32  F
2.8
Density (D= Mass/Volume)

F - 32
C 
K  C  273
Density calculations-check density lab calculations (Lab#2, 3)
1.8
Chapter 4
Symbols for elements (from periodic table)
No. protons, no. neutrons, no. electrons, charge problem
• Atomic Number = Number of protons
Mass #
• Mass Number = # of Protons + # of neutrons
• Isotopes, writing in the 14C convention
At. #
•Periodic Table (section 4.8)
35
Cl
17
1. Group 1 – alkali metals
+1 ion only
2. Group 2 – alkali earth metals +2 ion only
3. Group 7 – halogens usually –1 ion
4. Group 8 – noble gases Elements
Chapter 11
electronic configuration of atoms and ions
valence electrons
orbital, how many electrons can sub-shells have? S-2, p-6, d? etc
Filling order 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s-MEMORIZE
A. Atomic size
1. Decreases as you move to the right along a row (period)
2. Increases as you go down a column (group)
Ionization energy has trends opposite to Atomic Size
Chapter 12 Bonding and shapes- MODELS LAB #7
Correct Lewis structure
Molecular geometry –important-2 questions!
Type of bonding? Ionic, Polar covalent, non polar covalent etc.
Polar- non polar??,
Chapter 5 (check review 3)
How many atoms in some chemical formula Al (NO3)3 Ans:13
Correct formulas for chemicals, polyatomics
Names of compounds molecular, ionic compounds and Acids
Chapter 6 and 7 –Check single/Double lab (#9 and 10)
Types of reaction? Displacement, dissociation etc
Balancing equation- write the coefficients?
Solubility chart
(check review 3)
Chapter 8 (check review 3)
How many moles, number of atoms/molecules ?
Empirical formula- easy one
Molecular formulas- Ratio
Mass %- hey this is easy!!!
Chapter 9
Balance equations First!!!
Calculations in chemical reaction how much reactant will
produce how much product, moles to moles, grams to grams
etc- STOICHIOMETRY
Chapter 13 – Gases –
Boyle’s law relation of P and V
Charles law relation of V and T
Avogadro's law relation of V and N
combined gas law PV=nRT relationship
• P ∞T, P ∞n and P ∞1/V
Chapter 14
Polar dissolves polar and non polar dissolves non polar
Intermolecular forces are strong will result in high boiling point
H-bonding INTER molecular bond between H and O or F or N
Electrolytes and metallic bonding; London dispersion forces,
dipole-dipole forces
Chapter 15 Check review 4 in website
Mass percentage
Molarity and number of moles in solution
Titration
Chapter 16
Weak and strong electrolytes (refer to lab): NEED IONS!!
Acids produce H+and Bases produce OH-concepts
pH<7 : Acid; pH>7 bases, pH=7 neutral Strong acid or strong base
Buffers: Weak acid + salt containing anion of weak Acid
Basic Buffers: Weak Base + Salt containing cation of weak base
• 6.023x1023 ATOMS = 1 mole OF ATOMS
weighs At. Mass in g
• 6.023x1023 MOLECULES = 1 mole OF MOLECULES
weighs Molar mass in g
• Suppose the molecule has formula A2B
then
• 1 mole of A2B consists of 6.023x1023 MOLECULES of A2B
and
• 2 X 6.023x1023 ATOMS of A
weighs 2 X At. Mass of A in g
• 1 X 6.023x1023 ATOMS of B
weighs 1 X At. Mass of B in g
Important Formulas to memorize
•
•
•
•
•
•
•
•
•
•
Chapter 2 – Density, temperature conversion, powers of 10
Chapter 10– At .#, mass#, protons, neutrons, e-, isotopes, ions
Chapter 11 – Valence electrons, electron config.
Chapter 5 – Formulas of compounds, Lewis structure rules
Chapter 12 – VSEPR shapes of molecules, polarity, dipole
Chapter 6, 7 – Balancing chemical equations, Single-double displacement
reactions
Chapter 8,9 – Moles? Avogadro number? Molar mass, Stoichiometry Start
from balanced equation, moles of A to moles of B? grams of A to grams
of B? etc
Chapter 14 –, Concept of inter-molecular bonding, H-bond
Chapter 13 – Gas laws, relation of P vs V, T & n Temp in Kelvin!!
Chapter 15 – Molarity = moles/L of solution,
% composition = mass solute x 100%
Titrations 1:1 M V = M V
mass solution
a a
b
• Chapter 16 – pH = -log([H+]), [OH-] = Kw/[H+], pH calculations
b