This document provides information on various chemistry concepts including:
1) The scientific method process of observation, hypothesis, experiment, and conclusion.
2) Differences between physical and chemical changes and examples of each.
3) Density concepts including the density formula and how density relates to floating and sinking.
4) Classification of matter including elements, compounds, mixtures, and various types of mixtures.
5. Density
Density =
πππ π ππ π π’ππ π‘ππππ
π£πππ’ππ ππ π π’ππ π‘ππππ
Small density Float
Heavy density Sink
m
D V
7. Chemistry Calculation SkillsSignificant Figures
Decimal ABSENT to the
Right
Decimal PRESENT to the
Left
Multiplication & Division
Lowest Sig Fig
Addition & Subtraction
Lowest Decimal
Scientific Notation
Calculator Results in Scientific Notation:
2nd Drg SCI FLO
Plug in Scientific Notation 2nd E
8. Metric Units & SI unitsMetric Units
Meter (m)
Liter 9L)
Gram (g)
Degree (ΒΊC)
Seconds (s)
SI units
Meter (m)
Cubic meter (M3)
Kilogram (Kg)
Kelvin (K)
Second (s)
Metric & SI prefixes & suffixes
Tera T 1012
Giga G 109
Mega M 106
Kilo K 103
Deci d 10-1
Centi c 10-2
Milli m 10-3
Micro 10-6
Nano n 10-9
Pico p 10-12
9. Energy
Q=mCspβ²T
Q: Energy (joules)
M: mass (grams)
Csp: Specific Heat (J/gΒΊC)
β²T: Change in Temperature (ΒΊC)
Energy
1cal =4.184J
1kcal=100J
1KJ=1000J
1Cal=1Kal =1000cal
1Cal =4.184J=4184J
Carbohydrates 4calories
kcal/g
Proteins 4calories Kcal/g
Fats 9calories Kcal/g
10. Heat of Fusion
Heat = Mass * Heat of fusion
80cal/g or 334J/g
Heat of Vaporization
Heat= Mass * Heat of vaporization
540cal/g or 2260J/g
15. Atom
Protons: + [1amu]
Electrons: - [0amu]
Neutrons: neutral [1amu]
Atomic mass: P +N
Atomic Weight: Weighted
average of isotopes
Isotopes: elements vary in neutrons
Ions: elements vary in electrons
16.
17. Periodic Table: How to Read
Column: Group
Row: Period
Alkali Metals [group 1]
Alkaline Earth Metals [group 2]
Transition Metals [group 3-12]
Halogens [Group 17]
Noble gases [Group 18]
Metals shiny, good conductors, ductile
Nonmetals NOT
Metalloids Semiconductors
18. Periodic Table Trends
Ionization &
Electronegativity
Atomic Size
& metallic
Increase: Left to Right
Increase: Bottom to Top
Increase: Right to Left
Increase: Top to Bottom
21. Energy
KE=1/2mv2
PE=mgh
Kinetic EnergyMotion
(Example Running)
Potential Energy
Stored Energy
(Example chemical bonds as in ATP)
Electrical Electrons along a conductor
(Example a electrons moving across a neuron)
Chemical Energy released when bonds are broken
(Example breaking the bonds of glucose or ATP)
Thermal internal energy resulting from the
movement of atoms and molecules within it
(Example: Thyroid not working cold, burning building..)
Mechanical
Summation of PE &KE
(Example the heart contraction or
windmill)
1st law of Thermodynamics:
Energy cannot be created
nor destroyed, just
transferred from one form
to another
22. Bonding &
Nomenclature
Ionic (Type I Binary
compounds)
Transfer of Electrons:
Metal transfers electrons
to nonmetal
BIG difference in
Electronegativity
Example: NaCl (sodium
Chloride), KI (Potassium
Iodide)
Ionic (Type II Binary
Compounds)
Transition metals vary in
oxidation number and
roman numerals indicate
the oxidation number
used
Example Iron (III) Oxide
(Fe2O3)
Ionic Compounds with
polyatomic ions
Ammonium NH4+
Acetate CH3COO-
Cyanide CN-
Hypochlorite ClO-
Clhorite ClO2-
Chlorate ClO3-
Perchlorate ClO4-
Nitrate NO3-
Hydroxide OH-
Phosphate PO43-
Sulfate SO42-
Example: Ammonium
Sulfate (NH4SO4)
Covalent
Polar (Binary Type III)
Uneven Sharing of
Electrons
Moderate Difference in
Electronegativity
Example: H2O
(dihydrogen monoxide)
Polar dissolves polar &
universal solvent
Covalent nonpolar (Binary
Type III)
Even sharing of electrons
Low or no difference in
electronegativity
Ex. CO2, (Carbon
dioxide), O2
Fats, oils, lipids, gasoline,
carbon monoxide
Insoluble in water &
other solvents
Hydrogen Bond
Extra-molecular
(intermolecular) Between
2 or more molecules
Hydrogen can bond to
FON
Water properties: H2O,
High BP, High surface
tension, High specific
HEAT
Inter- molecular
(between the two)2Nonmetals
1 metal +
1nonmetal
Mono: 1
Di; 2
Tri: 3
Tetra: 4
Penta : 5
Hexa: 6
Hepta: 7
Octo: 8
23. Classifying Type of Attractions
Ionic Bonding
Metal + Nonmetal [Greater than 1.8]
Hydrogen Bonding
FON
Dipole- Dipole
Polar [0.5-1.8]
Dispersian
Temporary Dipole Nonpolar [0-0.4]
1. Increase in melting point (ΒΊC)
2. Increase in force of attraction
26. VSEPR: Geometry
Linear 180ΒΊ
Trigonal Planar 120ΒΊ
Bent 120ΒΊ
Tetrahedral 109ΒΊ
Trigonal Pyramid 109ΒΊ
Bent 109ΒΊ
2 3 4
nonpolar
nonpolar nonpolar
polar
polar
polar
27. Oxidation States
Group 1: 1+
Group 2: 2+
Group 13: 3+
Group 3: 3+
Group 4: 2+ 3+ 4+ 5+
Group 5: 2+ 3+ 4+ 5+
Group 6: 2+ 3+ 4+ 5+ 6+
Group 7: 2+ 3+ 4+ 5+ 6+ 7+
Group 8: 2+ 3+ 4+ 5+ 6+
Group 9: 2+ 3+ 4+ 5+
Group 10: 2+ 3+ 4+
Group 11: 2+ 3+
Group 12: 2+
Group 14: 4-
Group 15: 3-
Group 16: 2-
Group 17: 1-
Group 18: Noble gases
29. Atmospheric Pressure
Atmospheric pressure increase at lower
altitudes
[Less air inside chip bag]
Pressure in Bag < Atmospheric pressure
Atmospheric pressure decrease at higher
altitudes
[more air inside chip bag]
Pressure in Bag > Atmospheric pressure
31. Reaction Types
A + B ο AB
Combination
AB ο A + B
Decomposition
A + BC ο AC + B
Single Replacement
AB + CD ο AD + CB
Double Replacement
CxHy + ZO2(g) ο XCO2 + YH2O + Energy
Combustion
33. Kinetic Molecular Theory of Gases
1. A gas consist of small particles (atoms or
molecules that move randomly with high
velocities)
2. The attractive forces between the particles of a
gas are usually very small
3. The actual volume occupied by gas molecules is
extremely small compacted with the volume gas
occupies
4. Gas particles are in constant motion moving
rapidly in straight paths
5. The average kinetic energy of gas molecules is
proportional to the kelvin temperature
34. Gases Laws
Gay Lussacβs:
π·π
π»π
=
π·π
π»π
Charles:
π½π
π»π
=
π½π
π»π
Boyles:P1V1=P2V2
Combined Gas Laws:
π·ππ½π
π»π
=
π·ππ½π
π»π
Avagadros Law:
π½π
ππ
=
π½π
ππ
Dalton Law: Ptotal = P1 + P2 + P3
Measurement of Gas
Pressure (P) =
πππππ
π¨πππ
Conversian Factors
1atm=760mmHg=760torr
1mmHg=1torr
1atm = 1.01325*10^5Pa=101.325kPa
1atm=14.7lb/in2
Property Description Units
Pressure (P) The force exerted by a
gas against the walls of
the container
(atm)
(mmHg)(Pa)
Volume(V) The space occupied by
a gas
(L) (ml)
Temperature(T) The determining factor
of the kinetic energy
and rate of motion of
gas particles
(ΒΊC) (K)
Amount (n) The quantity of gas
present in a container
(g) (n)
Properties that describe gas
37. Osmosis movement of Water
Hypotonic Solution
Lower solute
concentration ,water
flows in to the cell
Hypertonic Solution
Higher solute
concentration, water
flows out of the cell
Isotonic = Equilibrium
.9% NaCl & 5% Glucose
47. Acids & Bases
Acid + metal ο H2+ salt
Acid + carbonates/bicarbonateο Co2 +H2O + Salt
Acids + Base (Hydroxides) ο Acid + Base ο Water + Salt
βNeutralizationβ
48. [H3O+] > [OH-] Acidic
[H3O+] = [OH-] neutral
[H3O+] < [OH-] Basic
How to define pH
49. 7 More [Basic]Less [Acidic]
Calculation:
[H3O+]=10-ph
1) Whole number Plug in as pH
2) NOT whole number & switch to negative 10(-ph)
pH=-log[H3O+]
1) Plug in H3O+ number
2) -log (#)
3) Make sure setting scientific notation
51. Radioactive
spontaneously emits small particles of energy called radiation to become more stable
Alpha Decay
Mass # decrease by 4
Atomic # decrease by 2
2 protons & 2 neutrons
emitted as alpha
particles
Beta Decay
Neutrons decreased by 1
Protons increase by 1
Transmutation mass SAME!!
Gamma Decay
Mass number same
Atomic # same
Stable nucleus of same element
Energy is lost to stabilize nucleus
Travel: 2-4cm
Tisssue depth: .05mm
Shielding: paper clothing
Typical source: Radium 226
Travel: 200-300cm
Tisssue depth: 4-5mm
Shielding: heavy clothing, Lab coats
& gloves
Typical source: carbon-14
Travel: 200-300cm
Tisssue depth: 50cm< or more
Shielding: lead thick concrete
Typical source: Technetium -99