Download V. Chemical reactions

I. Atomic structure
A) Subatomic particles
a. What are the atomic mass units for protons, neutrons, and electrons?
1 amu- protons & neutrons 0 amu- electrons
b. What does the atomic number represent? number of protons
c. What does the mass number represent? number of protons & neutrons
d. What particles are in equal numbers in a neutral atom? protons & electrons
e. How is the number of protons determined? by atomic number
f. How is the number of neutrons determined? subtract atomic number from mass number
g. How is the number of electrons determined in a neutral atom?
Equal to the number of protons
B) The nucleus
a. What subatomic particles are located in the nucleus? protons & neutrons
C) The electron cloud
a. What determines the location of an electron in the electron cloud?
amount of energy the electron has
b. How many electrons can be found in the first energy level of an atom? 2
c. How many electrons can be found in the second energy level of an atom? 8
d. How can the electron arrangement/configuration be determined for a neutral atom?
Determine the number of electrons then arrange from level closest to nucleus to farthest
away- 2 maximum in the first level and 8 maximum in the 2nd (& 3rd for what we are doing in
this class)
D) Isotopes
a. How are isotopes different from other forms of the same element? Different number of neutrons;
different mass number
II. Periodic Table
A) Identifying elements by atomic number
B) Identifying elements with the same number of valence electrons
a. Which elements have one valence electron? Column 1
b. Which elements have two valence electrons? Column 2
c. Which elements have three valence electrons? Column 13
d. Which elements have four valence electrons? Column 14
e. Which elements have five valence electrons? Column 15
f. Which elements have six valence electrons? Column 16
g. Which elements have seven valence electrons? Column 17
h. Which elements have eight valence electrons? Column 18
C) Identifying elements by family
a. Which elements are alkali metals? Column 1
b. Which elements are alkaline earth metals? Column 2
c. Which elements are halogens? Column 17
d. Which elements are noble gases? Column 18
D) Identifying elements by period
a. Which elements have one electron shell? Row 1
b. Which elements have two electron shells? Row 2
c. Which elements have three electron shells? Row 3
d. Which elements have four electron shells? Row 4
e. Which elements have five electron shells? Row 5
f. Which elements have six electron shells? Row 6
g. Which elements have seven electron shells? Row 7
E) Identifying elements by area of the periodic table
a. Which elements are metals? Left of the zigzag line
b. Which elements are nonmetals? Right of the zigzag line
c. Which elements are metalloids? As, B, Ge, Sb, Si, Te
Which elements are transition metals? the ones located between columns 2 & 13
III. Ionic bonding
A) Electrons are transferred between atoms
B) Valence electrons- outer shell electrons
C) Metals
a. Lend valence electrons
b. 1 – 4 valence electrons
c. Form positive ions ( more protons than electrons)
D) Nonmetals
a. Borrow valence electrons
b. 4 - 8 valence electrons
c. Form negative ions (more electrons than protons)
D) Metals lend and non-metals borrow to become stable.
a. Stable- having only full outer electron shells
E) Oxidation number
a. The number of electrons an atom can lend, borrow, or share
b. Metals have positive oxidation numbers
1. Calcium has two outer shell electrons
2. Calcium lends two electrons
3. Calcium has an oxidation number of 2+
c. Nonmetals have negative oxidation numbers
1. Oxygen has six outer shell electrons
2. Oxygen gains two electrons to have a full outer shell of 8
3. Oxygen has an oxidation number of 2d. There are no oxidation numbers above 4.
F) Electrolytes
a. Ionic compounds dissolved in water will conduct electricity
IV. Rules for formula writing
A) Metals are listed first
B) Nonmetals are listed second
C) The total number of electrons shown as being lost by the metal must equal the total number of
electrons shown being gained by the nonmetal.
D) The number 1 is NOT used as a subscript.
E) When the subscripts would be the same for both the metal and nonmetal they are not used.
F) Examples
a. Calcium and Chlorine- CaCl2
b. Magnesium and oxygen- MgO
c. Magnesium and phosphorus- Mg3P2
V. Chemical reactions
A)
Types of chemical reactions
a. Synthesis
A +B
b. Decomposition
c. Single Replacement
d. Double Replacement
e. Combustion
Ch4 + O2 → H20 + CO2
e. Identify types of reactions based on chemical equations
B)
Components of a chemical reaction
a. Identify products in a chemical equation
b. Identify reactants in a chemical equation
d. Energy
i. Endothermic reactions
a) Less energy is released than is needed to
continue the reaction
b) The products have more energy than the
reactants have
c) Energy is absorbed from the surroundings
d) Would feel cold
ii. Exothermic reactions
a) More energy is released than is needed to
continue the reaction
b) The reactants have more energy than the
products have
c) Energy is released to the surroundings
d) Would feel warm
C)
Law of Conservation of Mass
a. In a chemical reaction mass is neither lost nor gained.
i. Atoms are rearranged
b. Equations are balanced to show Conservation of Mass
D)
Reaction rate
a. Substances must collide to react.
b. The more collisions the faster the reaction
c. Four factors that affect reaction rate
i.Surface area- amount of exposed surface
ii.Temperature- affects how fast particles move
iii.Catalysts- affect reactions without being part of
the reaction
iv. Concentration- how much of a material is in a given
area
E)
Flame tests- results
a. Oxygen- Splints re-light
b. Carbon dioxide- Splints go out
c. Oxygen and hydrogen- Violent reaction
VI. Covalent bonding
A. chemical bonding between nonmetals
B. electrons are shared
1. single covalent bond- one pair of shared electrons
2. double covalent bond- two pair of shared electrons
3. triple covalent bond- three pair of shared electrons
C. attraction of nuclei to the shared electrons keeps the atoms close to each other
D. molecules are formed
VII. Organic compounds
A. All organic compounds contain carbon
B. Organic compounds have covalent bonding
VIII. Hydrocarbons
A. Made up of only carbon and hydrogen
B. Chain hydrocarbons
1. Saturated hydrocarbons
a. Alkanes
1. All single bonds between carbons
2. Compound names end in ane (EX: ethane)
2. Unsaturated hydrocarbons
a. Alkenes
1. One double bond between carbons in chain
2. Compound names end in ene (EX: ethene)
b. Alkynes
1. One triple bond between carbons in the chain
2. Compound names end in yne (EX: ethyne)
IX. Alcohols
A. Carbon chain with an –OH group
B. Compound names end in anol (EX: ethanol)
X. Organic acids
A. Carbon chain with an –COOH group
B. Compound names end in anoic (EX: ethanoic acid)
XI. Naming organic compounds
A. Prefixes1. Based on number of carbons
2. Know the first five prefixes. (meth, eth, prop, but, pent)
B. Suffixes
1. alkanes -ane
2. alkenes -ene
3. alkynes - yne
4. alcohols -anol
5. organic acids -anoic
XII. Molecular formulas
A. Show the type of atoms in a compound and the number of each
B. EX: C2H6
XIII. Structural formulas
a. Show the arrangement of atoms in a compound.
b. EX:
XIV. Isomers
A. Compounds with the same molecular formula but different
structural formula
B. EX:
XV. Acids
A) Molecules- covalent bonding
B) Contain more [H+]ion than plain water therefore more Hydronium ions H3OC) Taste sour
D) Neutralize bases
E) React with metals to form a salt and hydrogen
F) Results of color indicators
1. Red litmus- red
2. Blue litmus- red
3. Phenolphthalein- clear
G) pH below 7
XVI. Bases
A) Ionic bonding
B) Contain more Hydroxide [OH-] ion than plain water
C) Taste bitter
D) Neutralize acids
E) Formed when metals react with water
F) Results of color indicators
1. Red litmus- blue
2. Blue litmus- blue
3. Phenolphthalein- pink
G) pH above 7
XVII. Neutralization
A) Acid + base
B) Double replacement reaction
C) Determining relative concentrations of H+ and OH- using titration (adding drops)
XVII. pH Scale
A) Measure of acidity or alkalinity (baseness) of a solution
B) Measurement of the concentration of H+- ions in a solution
C)
Acid ---------- Neutral ----------Base