Chemistry Final Exam Review Guide ~ 2012 Name ______
Periodic Table
Complete the following periodic table by labeling and knowing the locations of the following:
· Rows (periods)
· Families (Alkali Metals, Alkaline Earth Metals, Halogens, Noble Gases, Transition Metals, Lanthanide, Actinide)
· Valence electrons
· Oxidation numbers
· Groups 1-18
· s, p, d, f blocks
Who created the first periodic table? Mendeleev
How was it arranged? Atomic mass
Who created the modern periodic table? Mosley
How is it arranged? Atomic number
What is a group? Family; vertical columns; same number of valence electrons
All elements in a group have the same number of: valence electrons
What is a period? Horizontal row
All elements in a period have the same number of energy levels
Know where the following are located on the periodic table: metals, nonmetals, metalloids
The most active metals are located where? Left side
The most active nonmetals are located where? Right side
List the 4 properties of metals: List the 4 properties of nonmetals:
Malleable / Brittle/dullLuster / Not malleable/ductile
Ductile / Gases – not solids
Conductor of heat & electricity / Take e- in order to form chemical bonds
Define:
· Valence electrons: e- in atom’s outermost orbital and included in bonding
· Ionization energy: energy required to remove atom from gaseous atom
· Periodic law: elements are arranged by increasing atomic number & showing a repeating pattern
· Octet rule: atoms lose, gain, or share electrons in order to acquire full set of 8 valence e-
· Ion: atom or bonded group of atoms with + or - charge
· Cation: ion with positive charge; forms when valence e- removed
· Anion: ion with negative charge; forms when valence e- added
· Electronegativity: indicates relative ability of atom to attract e- in a chemical bond
· Oxidation number: + or – charge of monatomic ion
What is the periodic trend for What is the periodic trend for
atomic radius? ionization energy?
Atomic Mass and Isotope Structure:
A=P=E (atomic # - whole number; atomic mass # - has decimal in it (round up or down)
mass – atomic # = no Isotope form = mass Symbol
atomic #
NAME / SYMBOL / MASS / ATOMIC # / p+ / no / e-Yitrium / Y / 89 / 39 / 39 / 50 / 39
Scandium / Sc / 45 / 21 / 21 / 24 / 21
Chlorine - 33 / Cl / 33 / 17 / 17 / 16 / 17
Iron - 59 / Fe / 59 / 26 / 26 / 33 / 26
Electromagnetic Spectrum: Label and know the correct locations with associated colors
Frequency / Wavelength / Gamma rays / x-raysHigh frequency / Low frequency / Long wavelength / Short wavelength
Microwaves / Radio waves / Ultraviolet / Infrared
Electron Configuration
1s2
Complete the chart:
Name / Mass # / Atomic # / P+ / N° / E- / Valence / BohrSodium
Na / 23 / 11 / 11 / 12 / 11 / 1 /
Aluminum
Al / 27 / 13 / 13 / 14 / 13 / 3 /
Sulfur
S / 32 / 16 / 16 / 16 / 16 / 6 /
Fluorine
F / 19 / 9 / 9 / 10 / 9 / 7 /
Draw Lewis dot diagrams for the following atoms:
Calcium Carbon Argon Oxygen
Ions formed: cation (+2) either none anion (-2)
Ca+2 C+4/-4 Ar° O-2
What are the 7 diatomic elements? N2, O2, F2, Cl2, Br2, I2, H2
Bonding
Write the chemical formula for the following ions and then name the item.
Na+ and Cl - NaCl
Al3+ and OH- Al(OH)3
K+ and PO4 3- K3(PO4)
Mg 2+ and CO3 2- MgCO3
Name the following or write the formula
KOH: Potassium hydroxide Magnesium IV chloride: MgCl4
Ca3N2: Calcium nitride Lithium oxide: Li2O
Mg3(PO4)2: Magnesium phosphate Beryllium fluoride: BeF2
LiCl: Lithium chloride Carbon tetrachloride: CCl4
SnCl2: Tin II chloride Sodium hypochlorite: Na(ClO)
SO3: Sulfur trioxide Calcium nitrate: Ca(NO3)2
Chemical Equations
Balance and give the type of reaction in each of the following.
2HgO à 2Hg + 1O2 decomposition
2H3PO4 + 3Ba(OH)2 à 6H2O + 1Ba3(PO4)2 double displacement
1Li + 1H2SO4à 1LiSO4 + 1H2 single displacement
1CH4 + 2O2 à 1CO2 + 2H2O combustion
1Ba(OH)2 + 2HCl à 1BaCl2 + 2H2O double displacement
Label the parts of the equation:
Fe(s) + CuSO4(aq) → Fe2(SO4)3(aq) + Cu(s)
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